Polarity of Covalent Bonds
In a polar covalent bond,
the more electronegative atom gains a greater fraction of the shared electrons and acquires a partial negative charge; indicated by δ- or the head of a crossed arrow
the less electronegative atom has a lesser fraction of the shared electrons and acquires a partial positive charge; indicated by δ+ or the tail of a crossed arrow
Polarity of Molecules
Water, H2O, has two polar bonds and, because of its geometry, is a polar molecule.
Polarity of Covalent Bonds
Although all covalent bonds involve sharing of electron pairs, they differ in the degree of sharing:
nonpolar covalent bond: electrons are shared equally
polar covalent bond: electron sharing is not equal
the degree of sharing depends on the relative electronegativities of the bonded atoms.
(chemistry) the tendency of an atom or radical to attract electrons in the formation of an ionic bond
Polarity of Covalent Bonds
Although all covalent bonds involve sharing of electron pairs, they differ in the degree of sharing:
nonpolar covalent bond: electrons are shared equally
polar covalent bond: electron sharing is not equal
the degree of sharing depends on the relative electronegativities of the bonded atoms.
a chemical bond that involves sharing a pair of electrons between atoms in a molecule
Polarity of Covalent Bonds
Although all covalent bonds involve sharing of electron pairs, they differ in the degree of sharing:
nonpolar covalent bond: electrons are shared equally
polar covalent bond: electron sharing is not equal
the degree of sharing depends on the relative electronegativities of the bonded atoms.
Polarity of Covalent Bonds
Although all covalent bonds involve sharing of electron pairs, they differ in the degree of sharing:
nonpolar covalent bond: electrons are shared equally
polar covalent bond: electron sharing is not equal
the degree of sharing depends on the relative electronegativities of the bonded atoms.
breed animals or plants using parents of different races and varieties
The Nature of Chemical Bonds: Valence Bond Theory
Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals
Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
H-H bond is cylindrically symmetrical
Bonds formed by head-on overlap of two atomic orbitals along a line drawn between the ...
(genetics) the act of mixing different species or varieties of animals or plants and thus to produce hybrids
The Nature of Chemical Bonds: Valence Bond Theory
Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals
Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
H-H bond is cylindrically symmetrical
Bonds formed by head-on overlap of two atomic orbitals along a line drawn between the ...
an electron in the outer shell of an atom which can combine with other atoms to form molecules
Bonding In Methane CH4
The formation of molecular orbitals in ethane
The formation of molecular orbitals in ethane
The Nature of Chemical Bonds: Valence Bond Theory
Bond length
The distance between nuclei at the minimum energy point
Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
The Nature of Chemical Bonds: Valence Bond Theory
Bond stre...
The Nature of Chemical Bonds: Valence Bond Theory
Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals
Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
H-H bond is cylindrically symmetrical
Bonds formed by head-on overlap of two atomic orbitals along a line drawn betwe...
a covalent bond in which two pairs of electrons are shared between two atoms
VSEPR Model
Predict the shape of formaldehyde, CH2O
The Lewis structure shows carbon surrounded by three regions of electron density; two regions contain single pairs of electrons and the third contains two pairs of electrons forming the double bond to oxygen.
Polarity of Covalent Bonds
Although all covalent bonds involve sharing of electron pairs, they differ in the degree of sharing:
nonpolar covalent bond: electrons are shared equally
polar covalent bond: electron sharing is not equal
the degree of sharing depends on the relative electronegativities of the bonded atoms.
The Nature of Chemical Bonds: Valence Bond Theory
Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals
Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
H-H bond is cylindrically symmetrical
Bonds formed by head-on overlap of two atomic orbitals along a line drawn between the ...
ExamplePredicting the Structures of Simple Molecules
Solution
There is only one way that two hydrogens, one carbon, and one oxygen can combine
Like the carbon atoms in ethylene, the carbon atom in formaldehyde is sp2-hybridized
The Nature of Chemical Bonds: Molecular Orbital Theory
Molecular Orbital Theory (MO)
A description of covalent bond formation as resulting from a mathematical combination of atomic orbitals (wave functions) to form molecular orbitals
Additive combination of tw...
Bonding In Methane CH4
The formation of molecular orbitals in ethane
The formation of molecular orbitals in ethane
The Nature of Chemical Bonds: Valence Bond Theory
Bond length
The distance between nuclei at the minimum energy point
Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
The Nature of Chemical Bonds: Valence Bond Theory
Bond stre...
The Nature of Chemical Bonds: Valence Bond Theory
Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals
Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
H-H bond is cylindrically symmetrical
Bonds formed by head-on overlap of two atomic orbitals along a line drawn betwe...
a planet seen just before sunrise in the eastern sky
Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
Oxygen
Methanol CH3OH
Methyl alcohol
Bonds are close to the109.5º tetrahedral angle
Two of the four sp3 hybrid orbitals on oxygen are occupied by nonbonding electron lone pairs
Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
Covalent bonds formed by other elements can also be described using hybrid orbitals
Nitrogen
Methylamine CH3NH2
Organic derivative of ammonia and the substance responsible for the odor of ro...
an insecticide that interferes with an insect's nervous system
Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
Oxygen
Methanol CH3OH
Methyl alcohol
Bonds are close to the109.5º tetrahedral angle
Two of the four sp3 hybrid orbitals on oxygen are occupied by nonbonding electron lone pairs
Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
Covalent bonds formed by other elements can also be described using hybrid orbitals
Nitrogen
Methylamine CH3NH2
Organic derivative of ammonia and the substance responsible for the odor of rotting f...
VSEPR Model
Predict the shape of ethylene, C2H4
The Lewis structure shows carbon surrounded by three regions of electron density; two regions contain single pairs of electrons and the third contains two pairs of electrons forming the double bond to the other carbon.
a compound of sulphur and some other element that is more electropositive
Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
Oxygen
Methanol CH3OH
Methyl alcohol
Bonds are close to the109.5º tetrahedral angle
Two of the four sp3 hybrid orbitals on oxygen are occupied by nonbonding electron lone pairs
Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
Covalent bonds formed by other elements can also be described using hybrid orbitals
Nitrogen
Methylamine CH3NH2
Organic derivative of ammonia and the substance responsible for the odor of rotting f...
Bonding In Methane CH4
The formation of molecular orbitals in ethane
The formation of molecular orbitals in ethane
The Nature of Chemical Bonds: Valence Bond Theory
Bond length
The distance between nuclei at the minimum energy point
Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
The Nature of Chemical Bonds: Valence Bond Theory
Bo...
Polarity of Covalent Bonds
Although all covalent bonds involve sharing of electron pairs, they differ in the degree of sharing:
nonpolar covalent bond: electrons are shared equally
polar covalent bond: electron sharing is not equal
the degree of sharing depends on the relative electronegativities of the bonded atoms.
the simplest structural unit of an element or compound
Polarity of Covalent Bonds
In a polar covalent bond,
the more electronegative atom gains a greater fraction of the shared electrons and acquires a partial negative charge; indicated by δ- or the head of a crossed arrow
the less electronegative atom has a lesser fraction of the shared electrons and acquires a partial positive charge; indicated by δ+ or the tail of a crossed arrow
Polarity of Molecules
Water, H2O, has two polar bonds and, because of its geometry, is a polar molecule.
the molecular weight of a substance expressed in grams
Bonding In Methane CH4
The formation of molecular orbitals in ethane
The formation of molecular orbitals in ethane
The Nature of Chemical Bonds: Valence Bond Theory
Bond length
The distance between nuclei at the minimum energy point
Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
The Nature of Chemical Bonds: Valence Bond Theory
Bond stre...
the offspring of genetically dissimilar parents or stock
The Nature of Chemical Bonds: Valence Bond Theory
Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals
Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
H-H bond is cylindrically symmetrical
Bonds formed by head-on overlap of two atomic orbitals along a line drawn between the ...
an abundant tasteless odorless multivalent nonmetallic element; best known in yellow crystals; occurs in many sulphide and sulphate minerals and even in native form (especially in volcanic regions)
Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
Oxygen
Methanol CH3OH
Methyl alcohol
Bonds are close to the109.5º tetrahedral angle
Two of the four sp3 hybrid orbitals on oxygen are occupied by nonbonding electron lone pairs
Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
Covalent bonds formed by other elements can also be described using hybrid orbitals
Nitrogen
Methylamine CH3NH2
Organic derivative of ammonia and the substance responsible for the odor of ro...
The Nature of Chemical Bonds: Valence Bond Theory
Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals
Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
H-H bond is cylindrically symmetrical
Bonds formed by head-on overlap of two atomic orbitals along a line drawn between the ...
Polarity of Covalent Bonds
In a polar covalent bond,
the more electronegative atom gains a greater fraction of the shared electrons and acquires a partial negative charge; indicated by δ- or the head of a crossed arrow
the less electronegative atom has a lesser fraction of the shared electrons and acquires a partial positive charge; indicated by δ+ or the tail of a crossed arrow
Polarity of Molecules
Water, H2O, has two polar bonds and, because of its geometry, is a polar molecule.
a relation between two opposite attributes or tendencies
Polarity of Covalent Bonds
Although all covalent bonds involve sharing of electron pairs, they differ in the degree of sharing:
nonpolar covalent bond: electrons are shared equally
polar covalent bond: electron sharing is not equal
the degree of sharing depends on the relative electronegativities of the bonded atoms.
a colorless poisonous gas; made by the oxidation of methanol
VSEPR Model
Predict the shape of formaldehyde, CH2O
The Lewis structure shows carbon surrounded by three regions of electron density; two regions contain single pairs of electrons and the third contains two pairs of electrons forming the double bond to oxygen.
the capacity of something or someone to react with or affect others
The Nature of Chemical Bonds: Valence Bond Theory
Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals
Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
H-H bond is cylindrically symmetrical
Bonds formed by head-on overlap of two atomic orbitals along a line drawn betwe...
binary compound that occurs at room temperature as a clear colorless odorless tasteless liquid; freezes into ice below 0 degrees centigrade and boils above 100 degrees centigrade; widely used as a solvent
Polarity of Covalent Bonds
In a polar covalent bond,
the more electronegative atom gains a greater fraction of the shared electrons and acquires a partial negative charge; indicated by δ- or the head of a crossed arrow
the less electronegative atom has a lesser fraction of the shared electrons and acquires a partial positive charge; indicated by δ+ or the tail of a crossed arrow
Polarity of Molecules
Water, H2O, has two polar bonds and, because of its geometry, is a polar molecule.
a rounded projection that is part of a larger structure
The Nature of Chemical Bonds: Valence Bond Theory
Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals
Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
H-H bond is cylindrically symmetrical
Bonds formed by head-on overlap of two atomic orbitals along a line drawn between the ...
Polarity of Covalent Bonds
Although all covalent bonds involve sharing of electron pairs, they differ in the degree of sharing:
nonpolar covalent bond: electrons are shared equally
polar covalent bond: electron sharing is not equal
the degree of sharing depends on the relative electronegativities of the bonded atoms.
a light volatile flammable poisonous liquid alcohol
Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
Oxygen
Methanol CH3OH
Methyl alcohol
Bonds are close to the109.5º tetrahedral angle
Two of the four sp3 hybrid orbitals on oxygen are occupied by nonbonding electron lone pairs
Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
Covalent bonds formed by other elements can also be described using hybrid orbitals
Nitrogen
Methylamine CH3NH2
Organic derivative of ammonia and the substance responsible for the odor of ro...
Bonding In Methane CH4
The formation of molecular orbitals in ethane
The formation of molecular orbitals in ethane
The Nature of Chemical Bonds: Valence Bond Theory
Bond length
The distance between nuclei at the minimum energy point
Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
The Nature of Chemical Bonds: Valence Bond Theory
Bond stre...
a colorless flammable gas used chiefly in welding and in organic synthesis
VSEPR Model
Predict the shape of acetylene, C2H2
The Lewis structure shows carbon surrounded by two regions of electron density; one region contains a single pair of electron, and the second contains three pairs of electrons forming the triple bond to carbon.
The Nature of Chemical Bonds: Valence Bond Theory
Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals
Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
H-H bond is cylindrically symmetrical
Bonds formed by head-on overlap of two atomic orbitals along a line drawn betwe...
a colorless, odorless gas that is essential for respiration
VSEPR Model
Predict the shape of water, H2O
The Lewis structure shows oxygen surrounded by four regions of electron density; two regions contain single pairs of electrons, and the third and fourth contain unshared pairs of electrons.
relating to the simplest units of an element or compound
Bonding In Methane CH4
The formation of molecular orbitals in ethane
The formation of molecular orbitals in ethane
The Nature of Chemical Bonds: Valence Bond Theory
Bond length
The distance between nuclei at the minimum energy point
Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
The Nature of Chemical Bonds: Valence Bond Theory
Bo...
a light volatile flammable poisonous liquid alcohol
Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
Oxygen
Methanol CH3OH
Methyl alcohol
Bonds are close to the109.5º tetrahedral angle
Two of the four sp3 hybrid orbitals on oxygen are occupied by nonbonding electron lone pairs
Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
Covalent bonds formed by other elements can also be described using hybrid orbitals
Nitrogen
Methylamine CH3NH2
Organic derivative of ammonia and the substance responsible for the odor of ro...
of or existing within the Arctic or Antarctic Circles
Polarity of Covalent Bonds
Although all covalent bonds involve sharing of electron pairs, they differ in the degree of sharing:
nonpolar covalent bond: electrons are shared equally
polar covalent bond: electron sharing is not equal
the degree of sharing depends on the relative electronegativities of the bonded atoms.
Bonding In Methane CH4
The formation of molecular orbitals in ethane
The formation of molecular orbitals in ethane
The Nature of Chemical Bonds: Valence Bond Theory
Bond length
The distance between nuclei at the minimum energy point
Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
The Nature of Chemical Bonds: Valence Bond Theory
Bond stre...
a substance that is altered during a chemical process
Bonding In Methane CH4
The formation of molecular orbitals in ethane
The formation of molecular orbitals in ethane
The Nature of Chemical Bonds: Valence Bond Theory
Bond length
The distance between nuclei at the minimum energy point
Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
The Nature of Chemical Bonds: Valence Bond Theory
Bond stre...
ExamplePredicting the Structures of Simple Molecules
Solution
There is only one way that two hydrogens, one carbon, and one oxygen can combine
Like the carbon atoms in ethylene, the carbon atom in formaldehyde is sp2-hybridized
The Nature of Chemical Bonds: Molecular Orbital Theory
Molecular Orbital Theory (MO)
A description of covalent bond formation as resulting from a mathematical combination of atomic orbitals (wave functions) to form molecular orbitals
Additive combination of tw...
a common nonmetallic element that is normally a colorless odorless tasteless inert diatomic gas; constitutes 78 percent of the atmosphere by volume; a constituent of all living tissues
VSEPR Model
Predict the shape of ammonia, NH3
The Lewis structure shows nitrogen surrounded by four regions of electron density; three regions contain single pairs of electrons, and the fourth contains an unshared pair of electrons.
Polarity of Covalent Bonds
In a polar covalent bond,
the more electronegative atom gains a greater fraction of the shared electrons and acquires a partial negative charge; indicated by δ- or the head of a crossed arrow
the less electronegative atom has a lesser fraction of the shared electrons and acquires a partial positive charge; indicated by δ+ or the tail of a crossed arrow
Polarity of Molecules
Water, H2O, has two polar bonds and, because of its geometry, is a polar molecule.
Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
Oxygen
Methanol CH3OH
Methyl alcohol
Bonds are close to the109.5º tetrahedral angle
Two of the four sp3 hybrid orbitals on oxygen are occupied by nonbonding electron lone pairs
Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
Covalent bonds formed by other elements can also be described using hybrid orbitals
Nitrogen
Methylamine CH3NH2
Organic derivative of ammonia and the substance responsible for the odor of ro...
United States chemist who studied the nature of chemical bonding (1901-1994)
The Nature of Chemical Bonds: Valence Bond Theory
Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals
Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
H-H bond is cylindrically symmetrical
Bonds formed by head-on overlap of two atomic orbitals along a line drawn between the ...
a part of the cell responsible for growth and reproduction
The Nature of Chemical Bonds: Valence Bond Theory
Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals
Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
H-H bond is cylindrically symmetrical
Bonds formed by head-on overlap of two atomic orbitals along a line drawn betwe...
ExamplePredicting the Structures of Simple Molecules
Solution
There is only one way that two hydrogens, one carbon, and one oxygen can combine
Like the carbon atoms in ethylene, the carbon atom in formaldehyde is sp2-hybridized
The Nature of Chemical Bonds: Molecular Orbital Theory
Molecular Orbital Theory (MO)
A description of covalent bond formation as resulting from a mathematical combination of atomic orbitals (wave functions) to form molecular orbitals
Additive combinatio...
ExamplePredicting the Structures of Simple Molecules
Solution
There is only one way that two hydrogens, one carbon, and one oxygen can combine
Like the carbon atoms in ethylene, the carbon atom in formaldehyde is sp2-hybridized
The Nature of Chemical Bonds: Molecular Orbital Theory
Molecular Orbital Theory (MO)
A description of covalent bond formation as resulting from a mathematical combination of atomic orbitals (wave functions) to form molecular orbitals
Additive combination of tw...
United States civil rights leader who was elected to the legislature in Georgia but was barred from taking his seat because he opposed the Vietnam War (born 1940)
The Nature of Chemical Bonds: Valence Bond Theory
Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals
Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
H-H bond is cylindrically symmetrical
Bonds formed by head-on overlap of two atomic orbitals along a line drawn betwe...
characterized by an imbalance in spatial arrangement
The Nature of Chemical Bonds: Valence Bond Theory
Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals
Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
H-H bond is cylindrically symmetrical
Bonds formed by head-on overlap of two atomic orbitals along a line drawn between the ...
ExamplePredicting the Structures of Simple Molecules
Solution
There is only one way that two hydrogens, one carbon, and one oxygen can combine
Like the carbon atoms in ethylene, the carbon atom in formaldehyde is sp2-hybridized
The Nature of Chemical Bonds: Molecular Orbital Theory
Molecular Orbital Theory (MO)
A description of covalent bond formation as resulting from a mathematical combination of atomic orbitals (wave functions) to form molecular orbitals
Additive combination of tw...
The Nature of Chemical Bonds: Valence Bond Theory
Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals
Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
H-H bond is cylindrically symmetrical
Bonds formed by head-on overlap of two atomic orbitals along a line drawn betwe...
a representation of something, often on a smaller scale
Bonding In Methane CH4
The formation of molecular orbitals in ethane
The formation of molecular orbitals in ethane
The Nature of Chemical Bonds: Valence Bond Theory
Bond length
The distance between nuclei at the minimum energy point
Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
The Nature of Chemical Bonds: Valence Bond Theory
Bond stre...
Bonding In Methane CH4
The formation of molecular orbitals in ethane
The formation of molecular orbitals in ethane
The Nature of Chemical Bonds: Valence Bond Theory
Bond length
The distance between nuclei at the minimum energy point
Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
The Nature of Chemical Bonds: Valence Bond Theory
Bond stre...
The Nature of Chemical Bonds: Valence Bond Theory
Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals
Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
H-H bond is cylindrically symmetrical
Bonds formed by head-on overlap of two atomic orbitals along a line drawn betwe...
The Nature of Chemical Bonds: Valence Bond Theory
Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals
Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
H-H bond is cylindrically symmetrical
Bonds formed by head-on overlap of two atomic orbitals along a line drawn between the ...
United States chemist who studied the nature of chemical bonding (1901-1994)
The Nature of Chemical Bonds: Valence Bond Theory
Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals
Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
H-H bond is cylindrically symmetrical
Bonds formed by head-on overlap of two atomic orbitals along a line drawn between the ...
Polarity of Covalent Bonds
Although all covalent bonds involve sharing of electron pairs, they differ in the degree of sharing:
nonpolar covalent bond: electrons are shared equally
polar covalent bond: electron sharing is not equal
the degree of sharing depends on the relative electronegativities of the bonded atoms.
Bonding In Methane CH4
The formation of molecular orbitals in ethane
The formation of molecular orbitals in ethane
The Nature of Chemical Bonds: Valence Bond Theory
Bond length
The distance between nuclei at the minimum energy point
Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
The Nature of Chemical Bonds: Valence Bond Theory
Bond stre...
ExamplePredicting the Structures of Simple Molecules
Solution
There is only one way that two hydrogens, one carbon, and one oxygen can combine
Like the carbon atoms in ethylene, the carbon atom in formaldehyde is sp2-hybridized
The Nature of Chemical Bonds: Molecular Orbital Theory
Molecular Orbital Theory (MO)
A description of covalent bond formation as resulting from a mathematical combination of atomic orbitals (wave functions) to form molecular orbitals
Additive combination of tw...
the mathematics of points and lines and curves and surfaces
Polarity of Covalent Bonds
In a polar covalent bond,
the more electronegative atom gains a greater fraction of the shared electrons and acquires a partial negative charge; indicated by δ- or the head of a crossed arrow
the less electronegative atom has a lesser fraction of the shared electrons and acquires a partial positive charge; indicated by δ+ or the tail of a crossed arrow
Polarity of Molecules
Water, H2O, has two polar bonds and, because of its geometry, is a polar molecule.
a multivalent nonmetallic element of the nitrogen family that occurs commonly in inorganic phosphate rocks and as organic phosphates in all living cells; is highly reactive and occurs in several allotropic forms
Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
Oxygen
Methanol CH3OH
Methyl alcohol
Bonds are close to the109.5º tetrahedral angle
Two of the four sp3 hybrid orbitals on oxygen are occupied by nonbonding electron lone pairs
Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
Covalent bonds formed by other elements can also be described using hybrid orbitals
Nitrogen
Methylamine CH3NH2
Organic derivative of ammonia and the substance responsible for the odor of rotting f...
Bonding In Methane CH4
The formation of molecular orbitals in ethane
The formation of molecular orbitals in ethane
The Nature of Chemical Bonds: Valence Bond Theory
Bond length
The distance between nuclei at the minimum energy point
Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
The Nature of Chemical Bonds: Valence Bond Theory
Bo...
the act of bringing things together to form a new whole
The Nature of Chemical Bonds: Valence Bond Theory
Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals
Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
H-H bond is cylindrically symmetrical
Bonds formed by head-on overlap of two atomic orbitals along a line drawn between the ...
Polarity of Covalent Bonds
Although all covalent bonds involve sharing of electron pairs, they differ in the degree of sharing:
nonpolar covalent bond: electrons are shared equally
polar covalent bond: electron sharing is not equal
the degree of sharing depends on the relative electronegativities of the bonded atoms.
The Nature of Chemical Bonds: Valence Bond Theory
Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals
Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
H-H bond is cylindrically symmetrical
Bonds formed by head-on overlap of two atomic orbitals along a line drawn between the ...
a colorless, odorless gas; the lightest chemical element
The Nature of Chemical Bonds: Valence Bond Theory
Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals
Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
H-H bond is cylindrically symmetrical
Bonds formed by head-on overlap of two atomic orbitals along a line drawn betwe...
The Nature of Chemical Bonds: Valence Bond Theory
Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals
Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
H-H bond is cylindrically symmetrical
Bonds formed by head-on overlap of two atomic orbitals along a line drawn between the ...
The Nature of Chemical Bonds: Valence Bond Theory
Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals
Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
H-H bond is cylindrically symmetrical
Bonds formed by head-on overlap of two atomic orbitals along a line drawn between the ...
Bonding In Methane CH4
The formation of molecular orbitals in ethane
The formation of molecular orbitals in ethane
The Nature of Chemical Bonds: Valence Bond Theory
Bond length
The distance between nuclei at the minimum energy point
Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
The Nature of Chemical Bonds: Valence Bond Theory
Bond stre...
sp2 Hybrid Orbitals and the Structure of Ethylene
σ bond in ethylene formed by head-on overlap of two sp2 hybrid orbitals
Two non-hybridized 2p orbitals overlap sideways forming a bond
Carbon-carbon double bond is shorter and stronger than carbon-carbon single bond
sp Hybrid Orbitalsand the Structure of Acetylene
sp hybridized orbital
A hybrid orbital derived from the combination of one s and one p atomic orbital
The two sp hybrids are oriented at an angle of 180º...
Polarity of Covalent Bonds
In a polar covalent bond,
the more electronegative atom gains a greater fraction of the shared electrons and acquires a partial negative charge; indicated by δ- or the head of a crossed arrow
the less electronegative atom has a lesser fraction of the shared electrons and acquires a partial positive charge; indicated by δ+ or the tail of a crossed arrow
Polarity of Molecules
Water, H2O, has two polar bonds and, because of its geometry, is a polar molecule.
The Nature of Chemical Bonds: Valence Bond Theory
Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals
Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
H-H bond is cylindrically symmetrical
Bonds formed by head-on overlap of two atomic orbitals along a line drawn between the ...
VSEPR Model
Predict the shape of ammonia, NH3
The Lewis structure shows nitrogen surrounded by four regions of electron density; three regions contain single pairs of electrons, and the fourth contains an unshared pair of electrons.
produced by reactions involving atomic or molecular changes
The Nature of Chemical Bonds: Valence Bond Theory
Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals
Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
H-H bond is cylindrically symmetrical
Bonds formed by head-on overlap of two atomic orbitals along a line drawn betwe...
tending or having the power to protect or prevent decay
Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
Oxygen
Methanol CH3OH
Methyl alcohol
Bonds are close to the109.5º tetrahedral angle
Two of the four sp3 hybrid orbitals on oxygen are occupied by nonbonding electron lone pairs
Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
Covalent bonds formed by other elements can also be described using hybrid orbitals
Nitrogen
Methylamine CH3NH2
Organic derivative of ammonia and the substance responsible for the odor of rotting f...
Bonding In Methane CH4
The formation of molecular orbitals in ethane
The formation of molecular orbitals in ethane
The Nature of Chemical Bonds: Valence Bond Theory
Bond length
The distance between nuclei at the minimum energy point
Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
The Nature of Chemical Bonds: Valence Bond Theory
Bond stre...
The Nature of Chemical Bonds: Valence Bond Theory
Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals
Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
H-H bond is cylindrically symmetrical
Bonds formed by head-on overlap of two atomic orbitals along a line drawn betwe...
The Nature of Chemical Bonds: Valence Bond Theory
Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals
Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
H-H bond is cylindrically symmetrical
Bonds formed by head-on overlap of two atomic orbitals along a line drawn between the ...
The Nature of Chemical Bonds: Valence Bond Theory
Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals
Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
H-H bond is cylindrically symmetrical
Bonds formed by head-on overlap of two atomic orbitals along a line drawn between the ...
The Nature of Chemical Bonds: Valence Bond Theory
Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals
Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
H-H bond is cylindrically symmetrical
Bonds formed by head-on overlap of two atomic orbitals along a line drawn between the ...
Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
Oxygen
Methanol CH3OH
Methyl alcohol
Bonds are close to the109.5º tetrahedral angle
Two of the four sp3 hybrid orbitals on oxygen are occupied by nonbonding electron lone pairs
Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
Covalent bonds formed by other elements can also be described using hybrid orbitals
Nitrogen
Methylamine CH3NH2
Organic derivative of ammonia and the substance responsible for the odor of rotting f...
Bonding In Methane CH4
The formation of molecular orbitals in ethane
The formation of molecular orbitals in ethane
The Nature of Chemical Bonds: Valence Bond Theory
Bond length
The distance between nuclei at the minimum energy point
Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
The Nature of Chemical Bonds: Valence Bond Theory
Bo...
with a design in which one element covers a part of another
The Nature of Chemical Bonds: Valence Bond Theory
Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals
Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
H-H bond is cylindrically symmetrical
Bonds formed by head-on overlap of two atomic orbitals along a line drawn betwe...
Bonding In Methane CH4
The formation of molecular orbitals in ethane
The formation of molecular orbitals in ethane
The Nature of Chemical Bonds: Valence Bond Theory
Bond length
The distance between nuclei at the minimum energy point
Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
The Nature of Chemical Bonds: Valence Bond Theory
Bond stre...
Polarity of Covalent Bonds
Although all covalent bonds involve sharing of electron pairs, they differ in the degree of sharing:
nonpolar covalent bond: electrons are shared equally
polar covalent bond: electron sharing is not equal
the degree of sharing depends on the relative electronegativities of the bonded atoms.
deduct; calculate the difference between two numbers
The Nature of Chemical Bonds: Valence Bond Theory
Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals
Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
H-H bond is cylindrically symmetrical
Bonds formed by head-on overlap of two atomic orbitals along a line drawn between the ...
ExamplePredicting the Structures of Simple Molecules
Solution
There is only one way that two hydrogens, one carbon, and one oxygen can combine
Like the carbon atoms in ethylene, the carbon atom in formaldehyde is sp2-hybridized
The Nature of Chemical Bonds: Molecular Orbital Theory
Molecular Orbital Theory (MO)
A description of covalent bond formation as resulting from a mathematical combination of atomic orbitals (wave functions) to form molecular orbitals
Additive combination of tw...
The Nature of Chemical Bonds: Valence Bond Theory
Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals
Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
H-H bond is cylindrically symmetrical
Bonds formed by head-on overlap of two atomic orbitals along a line drawn betwe...
Polarity of Covalent Bonds
In a polar covalent bond,
the more electronegative atom gains a greater fraction of the shared electrons and acquires a partial negative charge; indicated by δ- or the head of a crossed arrow
the less electronegative atom has a lesser fraction of the shared electrons and acquires a partial positive charge; indicated by δ+ or the tail of a crossed arrow
Polarity of Molecules
Water, H2O, has two polar bonds and, because of its geometry, is a polar molecule.
ExamplePredicting the Structures of Simple Molecules
Solution
There is only one way that two hydrogens, one carbon, and one oxygen can combine
Like the carbon atoms in ethylene, the carbon atom in formaldehyde is sp2-hybridized
The Nature of Chemical Bonds: Molecular Orbital Theory
Molecular Orbital Theory (MO)
A description of covalent bond formation as resulting from a mathematical combination of atomic orbitals (wave functions) to form molecular orbitals
Additive combination of tw...
characterized by denial or opposition or resistance
Polarity of Covalent Bonds
In a polar covalent bond,
the more electronegative atom gains a greater fraction of the shared electrons and acquires a partial negative charge; indicated by δ- or the head of a crossed arrow
the less electronegative atom has a lesser fraction of the shared electrons and acquires a partial positive charge; indicated by δ+ or the tail of a crossed arrow
Polarity of Molecules
Water, H2O, has two polar bonds and, because of its geometry, is a polar molecule.
a scientist who studies elements that make up matter
VSEPR Model
sp2 Hybrid Orbitals and the Structure of Ethylene
σ bond in ethylene formed by head-on overlap of two sp2 hybrid orbitals
Two non-hybridized 2p orbitals overlap sideways forming a bond
Carbon-carbon double bond is shorter and stronger than carbon-carbon single bond
sp Hybrid Orbitalsand the Structure of Acetylene
sp hybridized orbital
A hybrid orbital derived from the combination of one s and one p atomic orbital
The two sp hybrids are oriented at an angle of 180º...
The Nature of Chemical Bonds: Valence Bond Theory
Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals
Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
H-H bond is cylindrically symmetrical
Bonds formed by head-on overlap of two atomic orbitals along a line drawn betwe...
the act of successfully defending against an attack
Bonding In Methane CH4
The formation of molecular orbitals in ethane
The formation of molecular orbitals in ethane
The Nature of Chemical Bonds: Valence Bond Theory
Bond length
The distance between nuclei at the minimum energy point
Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
The Nature of Chemical Bonds: Valence Bond Theory
Bond stre...
Polarity of Covalent Bonds
Although all covalent bonds involve sharing of electron pairs, they differ in the degree of sharing:
nonpolar covalent bond: electrons are shared equally
polar covalent bond: electron sharing is not equal
the degree of sharing depends on the relative electronegativities of the bonded atoms.
the cardinal number that is the sum of one and one
Polarity of Covalent Bonds
In a polar covalent bond,
the more electronegative atom gains a greater fraction of the shared electrons and acquires a partial negative charge; indicated by δ- or the head of a crossed arrow
the less electronegative atom has a lesser fraction of the shared electrons and acquires a partial positive charge; indicated by δ+ or the tail of a crossed arrow
Polarity of Molecules
Water, H2O, has two polar bonds and, because of its geometry, is a polar molecule.
exhibiting equivalence or correspondence among constituents
The Nature of Chemical Bonds: Valence Bond Theory
Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals
Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
H-H bond is cylindrically symmetrical
Bonds formed by head-on overlap of two atomic orbitals along a line drawn betwe...
Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
Oxygen
Methanol CH3OH
Methyl alcohol
Bonds are close to the109.5º tetrahedral angle
Two of the four sp3 hybrid orbitals on oxygen are occupied by nonbonding electron lone pairs
Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
Covalent bonds formed by other elements can also be described using hybrid orbitals
Nitrogen
Methylamine CH3NH2
Organic derivative of ammonia and the substance responsible for the odor of ro...
Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
Oxygen
Methanol CH3OH
Methyl alcohol
Bonds are close to the109.5º tetrahedral angle
Two of the four sp3 hybrid orbitals on oxygen are occupied by nonbonding electron lone pairs
Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
Covalent bonds formed by other elements can also be described using hybrid orbitals
Nitrogen
Methylamine CH3NH2
Organic derivative of ammonia and the substance responsible for the odor of rotting f...
the process of decay caused by bacterial or fungal action
Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
Oxygen
Methanol CH3OH
Methyl alcohol
Bonds are close to the109.5º tetrahedral angle
Two of the four sp3 hybrid orbitals on oxygen are occupied by nonbonding electron lone pairs
Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
Covalent bonds formed by other elements can also be described using hybrid orbitals
Nitrogen
Methylamine CH3NH2
Organic derivative of ammonia and the substance responsible for the odor of rottin...
The Nature of Chemical Bonds: Valence Bond Theory
Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals
Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
H-H bond is cylindrically symmetrical
Bonds formed by head-on overlap of two atomic orbitals along a line drawn between the ...
The Nature of Chemical Bonds: Valence Bond Theory
Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals
Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
H-H bond is cylindrically symmetrical
Bonds formed by head-on overlap of two atomic orbitals along a line drawn between the ...
Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
Oxygen
Methanol CH3OH
Methyl alcohol
Bonds are close to the109.5º tetrahedral angle
Two of the four sp3 hybrid orbitals on oxygen are occupied by nonbonding electron lone pairs
Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
Covalent bonds formed by other elements can also be described using hybrid orbitals
Nitrogen
Methylamine CH3NH2
Organic derivative of ammonia and the substance responsible for the odor of rotting f...
The Nature of Chemical Bonds: Valence Bond Theory
Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals
Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
H-H bond is cylindrically symmetrical
Bonds formed by head-on overlap of two atomic orbitals along a line drawn betwe...
existing alone or consisting of one entity or part or aspect or individual
Bonding In Methane CH4
The formation of molecular orbitals in ethane
The formation of molecular orbitals in ethane
The Nature of Chemical Bonds: Valence Bond Theory
Bond length
The distance between nuclei at the minimum energy point
Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
The Nature of Chemical Bonds: Valence Bond Theory
Bond stre...
consisting of or involving two parts or components usually in pairs
Bonding In Methane CH4
The formation of molecular orbitals in ethane
The formation of molecular orbitals in ethane
The Nature of Chemical Bonds: Valence Bond Theory
Bond length
The distance between nuclei at the minimum energy point
Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
The Nature of Chemical Bonds: Valence Bond Theory
Bond stre...
characterized by or displaying affirmation or acceptance
Polarity of Covalent Bonds
In a polar covalent bond,
the more electronegative atom gains a greater fraction of the shared electrons and acquires a partial negative charge; indicated by δ- or the head of a crossed arrow
the less electronegative atom has a lesser fraction of the shared electrons and acquires a partial positive charge; indicated by δ+ or the tail of a crossed arrow
Polarity of Molecules
Water, H2O, has two polar bonds and, because of its geometry, is a polar molecule.
the cardinal number that is the sum of three and one
The Nature of Chemical Bonds: Valence Bond Theory
Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals
Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
H-H bond is cylindrically symmetrical
Bonds formed by head-on overlap of two atomic orbitals along a line drawn between the ...
Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
Oxygen
Methanol CH3OH
Methyl alcohol
Bonds are close to the109.5º tetrahedral angle
Two of the four sp3 hybrid orbitals on oxygen are occupied by nonbonding electron lone pairs
Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
Covalent bonds formed by other elements can also be described using hybrid orbitals
Nitrogen
Methylamine CH3NH2
Organic derivative of ammonia and the substance responsible for the odor of rotting f...
The Nature of Chemical Bonds: Valence Bond Theory
Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals
Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
H-H bond is cylindrically symmetrical
Bonds formed by head-on overlap of two atomic orbitals along a line drawn betwe...
Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
Oxygen
Methanol CH3OH
Methyl alcohol
Bonds are close to the109.5º tetrahedral angle
Two of the four sp3 hybrid orbitals on oxygen are occupied by nonbonding electron lone pairs
Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
Covalent bonds formed by other elements can also be described using hybrid orbitals
Nitrogen
Methylamine CH3NH2
Organic derivative of ammonia and the substance responsible for the odor of rotting f...
come into the possession of something concrete or abstract
Polarity of Covalent Bonds
In a polar covalent bond,
the more electronegative atom gains a greater fraction of the shared electrons and acquires a partial negative charge; indicated by δ- or the head of a crossed arrow
the less electronegative atom has a lesser fraction of the shared electrons and acquires a partial positive charge; indicated by δ+ or the tail of a crossed arrow
Polarity of Molecules
Water, H2O, has two polar bonds and, because of its geometry, is a polar molecule.
The Nature of Chemical Bonds: Valence Bond Theory
Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals
Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
H-H bond is cylindrically symmetrical
Bonds formed by head-on overlap of two atomic orbitals along a line drawn betwe...
Polarity of Covalent Bonds
Although all covalent bonds involve sharing of electron pairs, they differ in the degree of sharing:
nonpolar covalent bond: electrons are shared equally
polar covalent bond: electron sharing is not equal
the degree of sharing depends on the relative electronegativities of the bonded atoms.
sp2 Hybrid Orbitals and the Structure of Ethylene
σ bond in ethylene formed by head-on overlap of two sp2 hybrid orbitals
Two non-hybridized 2p orbitals overlap sideways forming a bond
Carbon-carbon double bond is shorter and stronger than carbon-carbon single bond
sp Hybrid Orbitalsand the Structure of Acetylene
sp hybridized orbital
A hybrid orbital derived from the combination of one s and one p atomic orbital
The two sp hybrids are oriented at an angle ...
a stable situation in which forces cancel one another
Bonding In Methane CH4
The formation of molecular orbitals in ethane
The formation of molecular orbitals in ethane
The Nature of Chemical Bonds: Valence Bond Theory
Bond length
The distance between nuclei at the minimum energy point
Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
The Nature of Chemical Bonds: Valence Bond Theory
Bo...
ExamplePredicting the Structures of Simple Molecules
Solution
There is only one way that two hydrogens, one carbon, and one oxygen can combine
Like the carbon atoms in ethylene, the carbon atom in formaldehyde is sp2-hybridized
The Nature of Chemical Bonds: Molecular Orbital Theory
Molecular Orbital Theory (MO)
A description of covalent bond formation as resulting from a mathematical combination of atomic orbitals (wave functions) to form molecular orbitals
Additive combination of tw...
characterized by action or forcefulness of personality
Bonding In Methane CH4
The formation of molecular orbitals in ethane
The formation of molecular orbitals in ethane
The Nature of Chemical Bonds: Valence Bond Theory
Bond length
The distance between nuclei at the minimum energy point
Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
The Nature of Chemical Bonds: Valence Bond Theory
Bo...
The Nature of Chemical Bonds: Valence Bond Theory
Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals
Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
H-H bond is cylindrically symmetrical
Bonds formed by head-on overlap of two atomic orbitals along a line drawn betwe...
Polarity of Covalent Bonds
In a polar covalent bond,
the more electronegative atom gains a greater fraction of the shared electrons and acquires a partial negative charge; indicated by δ- or the head of a crossed arrow
the less electronegative atom has a lesser fraction of the shared electrons and acquires a partial positive charge; indicated by δ+ or the tail of a crossed arrow
Polarity of Molecules
Water, H2O, has two polar bonds and, because of its geometry, is a polar molecule.
of or pertaining to or of the nature of mathematics
ExamplePredicting the Structures of Simple Molecules
Solution
There is only one way that two hydrogens, one carbon, and one oxygen can combine
Like the carbon atoms in ethylene, the carbon atom in formaldehyde is sp2-hybridized
The Nature of Chemical Bonds: Molecular Orbital Theory
Molecular Orbital Theory (MO)
A description of covalent bond formation as resulting from a mathematical combination of atomic orbitals (wave functions) to form molecular orbitals
Additive combinatio...
Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
Oxygen
Methanol CH3OH
Methyl alcohol
Bonds are close to the109.5º tetrahedral angle
Two of the four sp3 hybrid orbitals on oxygen are occupied by nonbonding electron lone pairs
Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
Covalent bonds formed by other elements can also be described using hybrid orbitals
Nitrogen
Methylamine CH3NH2
Organic derivative of ammonia and the substance responsible for the odor of rotting f...
ExamplePredicting the Structures of Simple Molecules
Solution
There is only one way that two hydrogens, one carbon, and one oxygen can combine
Like the carbon atoms in ethylene, the carbon atom in formaldehyde is sp2-hybridized
The Nature of Chemical Bonds: Molecular Orbital Theory
Molecular Orbital Theory (MO)
A description of covalent bond formation as resulting from a mathematical combination of atomic orbitals (wave functions) to form molecular orbitals
Additive combination of tw...
formed or developed from something else; not original
The Nature of Chemical Bonds: Valence Bond Theory
Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals
Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
H-H bond is cylindrically symmetrical
Bonds formed by head-on overlap of two atomic orbitals along a line drawn between the ...
The Nature of Chemical Bonds: Valence Bond Theory
Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals
Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
H-H bond is cylindrically symmetrical
Bonds formed by head-on overlap of two atomic orbitals along a line drawn between the ...
a Scandinavian language that is the official language of Denmark
VSEPR Model
sp2 Hybrid Orbitals and the Structure of Ethylene
σ bond in ethylene formed by head-on overlap of two sp2 hybrid orbitals
Two non-hybridized 2p orbitals overlap sideways forming a bond
Carbon-carbon double bond is shorter and stronger than carbon-carbon single bond
sp Hybrid Orbitalsand the Structure of Acetylene
sp hybridized orbital
A hybrid orbital derived from the combination of one s and one p atomic orbital
The two sp hybrids are oriented at an angle of 180º...
having few parts; not complex or complicated or involved
Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
Oxygen
Methanol CH3OH
Methyl alcohol
Bonds are close to the109.5º tetrahedral angle
Two of the four sp3 hybrid orbitals on oxygen are occupied by nonbonding electron lone pairs
Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
Covalent bonds formed by other elements can also be described using hybrid orbitals
Nitrogen
Methylamine CH3NH2
Organic derivative of ammonia and the substance responsible for the odor of rotting f...
an item of information that is typical of a class or group
Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
Oxygen
Methanol CH3OH
Methyl alcohol
Bonds are close to the109.5º tetrahedral angle
Two of the four sp3 hybrid orbitals on oxygen are occupied by nonbonding electron lone pairs
Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
Covalent bonds formed by other elements can also be described using hybrid orbitals
Nitrogen
Methylamine CH3NH2
Organic derivative of ammonia and the substance responsible for the odor of rotting f...
projectile with a thin shaft intended to be shot from a bow
Polarity of Covalent Bonds
In a polar covalent bond,
the more electronegative atom gains a greater fraction of the shared electrons and acquires a partial negative charge; indicated by δ- or the head of a crossed arrow
the less electronegative atom has a lesser fraction of the shared electrons and acquires a partial positive charge; indicated by δ+ or the tail of a crossed arrow
Polarity of Molecules
Water, H2O, has two polar bonds and, because of its geometry, is a polar molecule.
The Nature of Chemical Bonds: Valence Bond Theory
Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals
Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
H-H bond is cylindrically symmetrical
Bonds formed by head-on overlap of two atomic orbitals along a line drawn between the ...
being the only one; single and isolated from others
Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
Oxygen
Methanol CH3OH
Methyl alcohol
Bonds are close to the109.5º tetrahedral angle
Two of the four sp3 hybrid orbitals on oxygen are occupied by nonbonding electron lone pairs
Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
Covalent bonds formed by other elements can also be described using hybrid orbitals
Nitrogen
Methylamine CH3NH2
Organic derivative of ammonia and the substance responsible for the odor of ro...
Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
Oxygen
Methanol CH3OH
Methyl alcohol
Bonds are close to the109.5º tetrahedral angle
Two of the four sp3 hybrid orbitals on oxygen are occupied by nonbonding electron lone pairs
Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
Covalent bonds formed by other elements can also be described using hybrid orbitals
Nitrogen
Methylamine CH3NH2
Organic derivative of ammonia and the substance responsible for the odor of rottin...
Bonding In Methane CH4
The formation of molecular orbitals in ethane
The formation of molecular orbitals in ethane
The Nature of Chemical Bonds: Valence Bond Theory
Bond length
The distance between nuclei at the minimum energy point
Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
The Nature of Chemical Bonds: Valence Bond Theory
Bond stre...
Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
Oxygen
Methanol CH3OH
Methyl alcohol
Bonds are close to the109.5º tetrahedral angle
Two of the four sp3 hybrid orbitals on oxygen are occupied by nonbonding electron lone pairs
Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
Covalent bonds formed by other elements can also be described using hybrid orbitals
Nitrogen
Methylamine CH3NH2
Organic derivative of ammonia and the substance responsible for the odor of ro...
The Nature of Chemical Bonds: Valence Bond Theory
Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals
Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
H-H bond is cylindrically symmetrical
Bonds formed by head-on overlap of two atomic orbitals along a line drawn betwe...
The Nature of Chemical Bonds: Valence Bond Theory
Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals
Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
H-H bond is cylindrically symmetrical
Bonds formed by head-on overlap of two atomic orbitals along a line drawn betwe...
Bonding In Methane CH4
The formation of molecular orbitals in ethane
The formation of molecular orbitals in ethane
The Nature of Chemical Bonds: Valence Bond Theory
Bond length
The distance between nuclei at the minimum energy point
Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
The Nature of Chemical Bonds: Valence Bond Theory
Bo...
Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
Oxygen
Methanol CH3OH
Methyl alcohol
Bonds are close to the109.5º tetrahedral angle
Two of the four sp3 hybrid orbitals on oxygen are occupied by nonbonding electron lone pairs
Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
Covalent bonds formed by other elements can also be described using hybrid orbitals
Nitrogen
Methylamine CH3NH2
Organic derivative of ammonia and the substance responsible for the odor of ro...
Polarity of Covalent Bonds
In a polar covalent bond,
the more electronegative atom gains a greater fraction of the shared electrons and acquires a partial negative charge; indicated by δ- or the head of a crossed arrow
the less electronegative atom has a lesser fraction of the shared electrons and acquires a partial positive charge; indicated by δ+ or the tail of a crossed arrow
Polarity of Molecules
Water, H2O, has two polar bonds and, because of its geometry, is a polar molecule.
The Nature of Chemical Bonds: Valence Bond Theory
Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals
Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
H-H bond is cylindrically symmetrical
Bonds formed by head-on overlap of two atomic orbitals along a line drawn between the ...
sp2 Hybrid Orbitals and the Structure of Ethylene
σ bond in ethylene formed by head-on overlap of two sp2 hybrid orbitals
Two non-hybridized 2p orbitals overlap sideways forming a bond
Carbon-carbon double bond is shorter and stronger than carbon-carbon single bond
sp Hybrid Orbitalsand the Structure of Acetylene
sp hybridized orbital
A hybrid orbital derived from the combination of one s and one p atomic orbital
The two sp hybrids are oriented at an angle ...
ExamplePredicting the Structures of Simple Molecules
Solution
There is only one way that two hydrogens, one carbon, and one oxygen can combine
Like the carbon atoms in ethylene, the carbon atom in formaldehyde is sp2-hybridized
The Nature of Chemical Bonds: Molecular Orbital Theory
Molecular Orbital Theory (MO)
A description of covalent bond formation as resulting from a mathematical combination of atomic orbitals (wave functions) to form molecular orbitals
Additive combination of tw...
The Nature of Chemical Bonds: Valence Bond Theory
Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals
Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
H-H bond is cylindrically symmetrical
Bonds formed by head-on overlap of two atomic orbitals along a line drawn betwe...
Polarity of Covalent Bonds
In a polar covalent bond,
the more electronegative atom gains a greater fraction of the shared electrons and acquires a partial negative charge; indicated by δ- or the head of a crossed arrow
the less electronegative atom has a lesser fraction of the shared electrons and acquires a partial positive charge; indicated by δ+ or the tail of a crossed arrow
Polarity of Molecules
Water, H2O, has two polar bonds and, because of its geometry, is a polar molecule.
part of an organism consisting of an aggregate of cells
Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
Oxygen
Methanol CH3OH
Methyl alcohol
Bonds are close to the109.5º tetrahedral angle
Two of the four sp3 hybrid orbitals on oxygen are occupied by nonbonding electron lone pairs
Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
Covalent bonds formed by other elements can also be described using hybrid orbitals
Nitrogen
Methylamine CH3NH2
Organic derivative of ammonia and the substance responsible for the odor of rotting f...
The Nature of Chemical Bonds: Valence Bond Theory
Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals
Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
H-H bond is cylindrically symmetrical
Bonds formed by head-on overlap of two atomic orbitals along a line drawn between the ...
(of quantities) imprecise but fairly close to correct
Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
Oxygen
Methanol CH3OH
Methyl alcohol
Bonds are close to the109.5º tetrahedral angle
Two of the four sp3 hybrid orbitals on oxygen are occupied by nonbonding electron lone pairs
Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
Covalent bonds formed by other elements can also be described using hybrid orbitals
Nitrogen
Methylamine CH3NH2
Organic derivative of ammonia and the substance responsible for the odor of ro...
The Nature of Chemical Bonds: Valence Bond Theory
Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals
Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
H-H bond is cylindrically symmetrical
Bonds formed by head-on overlap of two atomic orbitals along a line drawn between the ...
VSEPR Model
Predict the shape of ammonia, NH3
The Lewis structure shows nitrogen surrounded by four regions of electron density; three regions contain single pairs of electrons, and the fourth contains an unshared pair of electrons.
The Nature of Chemical Bonds: Valence Bond Theory
Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals
Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
H-H bond is cylindrically symmetrical
Bonds formed by head-on overlap of two atomic orbitals along a line drawn between the ...
VSEPR Model
Predict the shape of water, H2O
The Lewis structure shows oxygen surrounded by four regions of electron density; two regions contain single pairs of electrons, and the third and fourth contain unshared pairs of electrons.
Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
Oxygen
Methanol CH3OH
Methyl alcohol
Bonds are close to the109.5º tetrahedral angle
Two of the four sp3 hybrid orbitals on oxygen are occupied by nonbonding electron lone pairs
Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
Covalent bonds formed by other elements can also be described using hybrid orbitals
Nitrogen
Methylamine CH3NH2
Organic derivative of ammonia and the substance responsible for the odor of ro...
Bonding In Methane CH4
The formation of molecular orbitals in ethane
The formation of molecular orbitals in ethane
The Nature of Chemical Bonds: Valence Bond Theory
Bond length
The distance between nuclei at the minimum energy point
Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
The Nature of Chemical Bonds: Valence Bond Theory
Bo...
a whole formed by a union of two or more elements or parts
Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
Oxygen
Methanol CH3OH
Methyl alcohol
Bonds are close to the109.5º tetrahedral angle
Two of the four sp3 hybrid orbitals on oxygen are occupied by nonbonding electron lone pairs
Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
Covalent bonds formed by other elements can also be described using hybrid orbitals
Nitrogen
Methylamine CH3NH2
Organic derivative of ammonia and the substance responsible for the odor of rotting f...
The Nature of Chemical Bonds: Valence Bond Theory
Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals
Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
H-H bond is cylindrically symmetrical
Bonds formed by head-on overlap of two atomic orbitals along a line drawn between
smallest whole number or a numeral representing this number
The Nature of Chemical Bonds: Valence Bond Theory
Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals
Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
H-H bond is cylindrically symmetrical
Bonds formed by head-on overlap of two atomic orbitals along a line drawn between the ...
Bonding In Methane CH4
The formation of molecular orbitals in ethane
The formation of molecular orbitals in ethane
The Nature of Chemical Bonds: Valence Bond Theory
Bond length
The distance between nuclei at the minimum energy point
Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
The Nature of Chemical Bonds: Valence Bond Theory
Bond stre...
Polarity of Covalent Bonds
Although all covalent bonds involve sharing of electron pairs, they differ in the degree of sharing:
nonpolar covalent bond: electrons are shared equally
polar covalent bond: electron sharing is not equal
the degree of sharing depends on the relative electronegativities of the bonded atoms.
Bonding In Methane CH4
The formation of molecular orbitals in ethane
The formation of molecular orbitals in ethane
The Nature of Chemical Bonds: Valence Bond Theory
Bond length
The distance between nuclei at the minimum energy point
Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
The Nature of Chemical Bonds: Valence Bond Theory
Bond stre...
Polarity of Covalent Bonds
Although all covalent bonds involve sharing of electron pairs, they differ in the degree of sharing:
nonpolar covalent bond: electrons are shared equally
polar covalent bond: electron sharing is not equal
the degree of sharing depends on the relative electronegativities of the bonded atoms.
a specific identifiable position in a continuum or series
Polarity of Covalent Bonds
Although all covalent bonds involve sharing of electron pairs, they differ in the degree of sharing:
nonpolar covalent bond: electrons are shared equally
polar covalent bond: electron sharing is not equal
the degree of sharing depends on the relative electronegativities of the bonded atoms.
the property of being physically or mentally powerful
Bonding In Methane CH4
The formation of molecular orbitals in ethane
The formation of molecular orbitals in ethane
The Nature of Chemical Bonds: Valence Bond Theory
Bond length
The distance between nuclei at the minimum energy point
Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
The Nature of Chemical Bonds: Valence Bond Theory
Bond s...
the linear extent in space from one end to the other
Bonding In Methane CH4
The formation of molecular orbitals in ethane
The formation of molecular orbitals in ethane
The Nature of Chemical Bonds: Valence Bond Theory
Bond length
The distance between nuclei at the minimum energy point
Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
The Nature of Chemical Bonds: Valence Bond Theory
Bo...
Bonding In Methane CH4
The formation of molecular orbitals in ethane
The formation of molecular orbitals in ethane
The Nature of Chemical Bonds: Valence Bond Theory
Bond length
The distance between nuclei at the minimum energy point
Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
The Nature of Chemical Bonds: Valence Bond Theory
Bond stre...
the property created by the space between two objects
Bonding In Methane CH4
The formation of molecular orbitals in ethane
The formation of molecular orbitals in ethane
The Nature of Chemical Bonds: Valence Bond Theory
Bond length
The distance between nuclei at the minimum energy point
Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
The Nature of Chemical Bonds: Valence Bond Theory
Bo...
Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
Oxygen
Methanol CH3OH
Methyl alcohol
Bonds are close to the109.5º tetrahedral angle
Two of the four sp3 hybrid orbitals on oxygen are occupied by nonbonding electron lone pairs
Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
Covalent bonds formed by other elements can also be described using hybrid orbitals
Nitrogen
Methylamine CH3NH2
Organic derivative of ammonia and the substance responsible for the odor of ro...
Bonding In Methane CH4
The formation of molecular orbitals in ethane
The formation of molecular orbitals in ethane
The Nature of Chemical Bonds: Valence Bond Theory
Bond length
The distance between nuclei at the minimum energy point
Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
The Nature of Chemical Bonds: Valence Bond Theory
Bond stre...
ExamplePredicting the Structures of Simple Molecules
Solution
There is only one way that two hydrogens, one carbon, and one oxygen can combine
Like the carbon atoms in ethylene, the carbon atom in formaldehyde is sp2-hybridized
The Nature of Chemical Bonds: Molecular Orbital Theory
Molecular Orbital Theory (MO)
A description of covalent bond formation as resulting from a mathematical combination of atomic orbitals (wave functions) to form molecular orbitals
Additive combinatio...
ExamplePredicting the Structures of Simple Molecules
Solution
There is only one way that two hydrogens, one carbon, and one oxygen can combine
Like the carbon atoms in ethylene, the carbon atom in formaldehyde is sp2-hybridized
The Nature of Chemical Bonds: Molecular Orbital Theory
Molecular Orbital Theory (MO)
A description of covalent bond formation as resulting from a mathematical combination of atomic orbitals (wave functions) to form molecular orbitals
Additive combinatio...
Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
Oxygen
Methanol CH3OH
Methyl alcohol
Bonds are close to the109.5º tetrahedral angle
Two of the four sp3 hybrid orbitals on oxygen are occupied by nonbonding electron lone pairs
Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
Covalent bonds formed by other elements can also be described using hybrid orbitals
Nitrogen
Methylamine CH3NH2
Organic derivative of ammonia and the substance responsible for the odor of ro...
The Nature of Chemical Bonds: Valence Bond Theory
Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals
Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
H-H bond is cylindrically symmetrical
Bonds formed by head-on overlap of two atomic orbitals along a line drawn between the ...
Bonding In Methane CH4
The formation of molecular orbitals in ethane
The formation of molecular orbitals in ethane
The Nature of Chemical Bonds: Valence Bond Theory
Bond length
The distance between nuclei at the minimum energy point
Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
The Nature of Chemical Bonds: Valence Bond Theory
Bond stre...
The Nature of Chemical Bonds: Valence Bond Theory
Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals
Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
H-H bond is cylindrically symmetrical
Bonds formed by head-on overlap of two atomic orbitals along a line drawn between the ...
the real physical matter of which a person or thing consists
Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
Oxygen
Methanol CH3OH
Methyl alcohol
Bonds are close to the109.5º tetrahedral angle
Two of the four sp3 hybrid orbitals on oxygen are occupied by nonbonding electron lone pairs
Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
Covalent bonds formed by other elements can also be described using hybrid orbitals
Nitrogen
Methylamine CH3NH2
Organic derivative of ammonia and the substance responsible for the odor of ro...
a marking that consists of lines that intersect each other
Polarity of Covalent Bonds
In a polar covalent bond,
the more electronegative atom gains a greater fraction of the shared electrons and acquires a partial negative charge; indicated by δ- or the head of a crossed arrow
the less electronegative atom has a lesser fraction of the shared electrons and acquires a partial positive charge; indicated by δ+ or the tail of a crossed arrow
Polarity of Molecules
Water, H2O, has two polar bonds and, because of its geometry, is a polar molecule.
ExamplePredicting the Structures of Simple Molecules
Solution
There is only one way that two hydrogens, one carbon, and one oxygen can combine
Like the carbon atoms in ethylene, the carbon atom in formaldehyde is sp2-hybridized
The Nature of Chemical Bonds: Molecular Orbital Theory
Molecular Orbital Theory (MO)
A description of covalent bond formation as resulting from a mathematical combination of atomic orbitals (wave functions) to form molecular orbitals
Additive combination of tw...
Bonding In Methane CH4
The formation of molecular orbitals in ethane
The formation of molecular orbitals in ethane
The Nature of Chemical Bonds: Valence Bond Theory
Bond length
The distance between nuclei at the minimum energy point
Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
The Nature of Chemical Bonds: Valence Bond Theory
Bond stre...
Bonding In Methane CH4
The formation of molecular orbitals in ethane
The formation of molecular orbitals in ethane
The Nature of Chemical Bonds: Valence Bond Theory
Bond length
The distance between nuclei at the minimum energy point
Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
The Nature of Chemical Bonds: Valence Bond Theory
Bo...
a visible clue that something has happened or is present
ExamplePredicting the Structures of Simple Molecules
Solution
There is only one way that two hydrogens, one carbon, and one oxygen can combine
Like the carbon atoms in ethylene, the carbon atom in formaldehyde is sp2-hybridized
The Nature of Chemical Bonds: Molecular Orbital Theory
Molecular Orbital Theory (MO)
A description of covalent bond formation as resulting from a mathematical combination of atomic orbitals (wave functions) to form molecular orbitals
Additive combination of tw...
the posterior part of the body of a vertebrate especially when elongated and extending beyond the trunk or main part of the body
Polarity of Covalent Bonds
In a polar covalent bond,
the more electronegative atom gains a greater fraction of the shared electrons and acquires a partial negative charge; indicated by δ- or the head of a crossed arrow
the less electronegative atom has a lesser fraction of the shared electrons and acquires a partial positive charge; indicated by δ+ or the tail of a crossed arrow
Polarity of Molecules
Water, H2O, has two polar bonds and, because of its geometry, is a polar molecule.
Polarity of Covalent Bonds
Although all covalent bonds involve sharing of electron pairs, they differ in the degree of sharing:
nonpolar covalent bond: electrons are shared equally
polar covalent bond: electron sharing is not equal
the degree of sharing depends on the relative electronegativities of the bonded atoms.
The Nature of Chemical Bonds: Valence Bond Theory
Bonding theory that describes a covalent bond as resulting from the overlap of two atomic orbitals
Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms, thus bonding the two atoms together
H–H bond results from the overlap of two singly occupied hydrogen 1s orbitals
H-H bond is cylindrically symmetrical
Bonds formed by head-on overlap of two atomic orbitals along a line drawn betwe...
Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
Oxygen
Methanol CH3OH
Methyl alcohol
Bonds are close to the109.5º tetrahedral angle
Two of the four sp3 hybrid orbitals on oxygen are occupied by nonbonding electron lone pairs
Hybridization of Nitrogen, Oxygen, Phosphorus, and Sulfur
Covalent bonds formed by other elements can also be described using hybrid orbitals
Nitrogen
Methylamine CH3NH2
Organic derivative of ammonia and the substance responsible for the odor of ro...
Polarity of Molecules
A molecule will be polar if:
it has polar bonds, and
its centers of partial positive and partial negative charges lie at different places within the molecule.
Bonding In Methane CH4
The formation of molecular orbitals in ethane
The formation of molecular orbitals in ethane
The Nature of Chemical Bonds: Valence Bond Theory
Bond length
The distance between nuclei at the minimum energy point
Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
The Nature of Chemical Bonds: Valence Bond Theory
Bond stre...
not the same one or ones already mentioned or implied
Bonding In Methane CH4
The formation of molecular orbitals in ethane
The formation of molecular orbitals in ethane
The Nature of Chemical Bonds: Valence Bond Theory
Bond length
The distance between nuclei at the minimum energy point
Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
The Nature of Chemical Bonds: Valence Bond Theory
Bo...
ExamplePredicting the Structures of Simple Molecules
Solution
There is only one way that two hydrogens, one carbon, and one oxygen can combine
Like the carbon atoms in ethylene, the carbon atom in formaldehyde is sp2-hybridized
The Nature of Chemical Bonds: Molecular Orbital Theory
Molecular Orbital Theory (MO)
A description of covalent bond formation as resulting from a mathematical combination of atomic orbitals (wave functions) to form molecular orbitals
Additive combinatio...
an artifact that has been created by someone or some process
Bonding In Methane CH4
The formation of molecular orbitals in ethane
The formation of molecular orbitals in ethane
The Nature of Chemical Bonds: Valence Bond Theory
Bond length
The distance between nuclei at the minimum energy point
Because a covalent bond is dynamic, like a spring, the characteristic bond length is the equilibrium distance between the nuclei of two atoms that are bonded to each other
The Nature of Chemical Bonds: Valence Bond Theory
Bond stre...
animal reproductive body consisting of an ovum or embryo together with nutritive and protective envelopes; especially the thin-shelled reproductive body laid by e.g. female birds
ExamplePredicting the Structures of Simple Molecules
Solution
There is only one way that two hydrogens, one carbon, and one oxygen can combine
Like the carbon atoms in ethylene, the carbon atom in formaldehyde is sp2-hybridized
The Nature of Chemical Bonds: Molecular Orbital Theory
Molecular Orbital Theory (MO)
A description of covalent bond formation as resulting from a mathematical combination of atomic orbitals (wave functions) to form molecular orbitals
Additive combination of tw...
Polarity of Covalent Bonds
Although all covalent bonds involve sharing of electron pairs, they differ in the degree of sharing:
nonpolar covalent bond: electrons are shared equally
polar covalent bond: electron sharing is not equal
the degree of sharing depends on the relative electronegativities of the bonded atoms.
Created on Wed Sep 23 07:17:19 EDT 2009
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