lecture 16 c1403october 31, 2005
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Lecture 16 C1403October 31, 2005. 18.1Molecular orbital theory: molecular orbitals and diatomic molecules. 18.2Valence bond theory: hybridized orbitals and polyatomic molecules. Bond order, bond lengths, connections of MO theory and VB theory with Lewis structures. +. +. +. +. _. _. +. - PowerPoint PPT PresentationTRANSCRIPT
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Lecture 16 C1403October 31, 2005
18.1 Molecular orbital theory: molecular orbitals and diatomic molecules
18.2 Valence bond theory: hybridized orbitals and polyatomic molecules
Bond order, bond lengths, connections of MO theory and VB theory with Lewis structures
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Making of a z and z* orbital from overlap of two 2pz orbitals
Making of a x and x* orbital from overlap of two 2px orbitals
Making of a y and y* orbital from overlap of two 2py orbitals
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Potential energy curves for the and * orbitals of a diatomic molecule
Distance dependence of the energy of a and * orbital
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The reason for the “switch” in the s and p MOs
Larger gap between 2s and 2p with increasing Z
Switch
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O2 Bond length = 1.21ÅO2
+ Bond length = 1.12 ÅO2
- Bond length = 1.26 ÅO2
2- Bond length = 1.49 Å
Bond order?
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Compare the Lewis and MO structures of diatomic molecules
C2
N2
O2
F2
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What is the bond order of NO in Lewis terms and MO theory?
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Double bonds and triple bonds
18.2 Polyatomic molecules
Valence bond versus molecular orbital theory
Hybridization of atomic orbitals to form molecular orbitals
sp, sp2 and sp3 hybridized orbitals
Hybridized orbitals and Lewis structures and molecular geometries
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18.218.2Bonding in Methane andBonding in Methane and
Orbital HybridizationOrbital Hybridization
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tetrahedraltetrahedral
bond angles = 109.5°bond angles = 109.5°
bond distances = 110 pmbond distances = 110 pm
but structure seems inconsistent but structure seems inconsistent withwithelectron configuration of carbonelectron configuration of carbon
Structure of MethaneStructure of MethaneStructure of MethaneStructure of Methane
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Electron configuration of carbonElectron configuration of carbonElectron configuration of carbonElectron configuration of carbon
22ss
22pponly two unpaired only two unpaired electronselectrons
should form should form bonds to only two bonds to only two hydrogen atomshydrogen atoms
bonds should be bonds should be at right angles to at right angles to one anotherone another
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22ss
22pp
Promote an electron from the Promote an electron from the 22s s to the 2to the 2pp orbital orbital
spsp33 Orbital Hybridization Orbital Hybridizationspsp33 Orbital Hybridization Orbital Hybridization
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22ss
22pp 22pp
22ss
spsp33 Orbital Hybridization Orbital Hybridizationspsp33 Orbital Hybridization Orbital Hybridization
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22pp
22ss
spsp33 Orbital Hybridization Orbital Hybridizationspsp33 Orbital Hybridization Orbital Hybridization
Mix together (hybridize) the 2Mix together (hybridize) the 2s s orbital and the three 2orbital and the three 2pp orbitals orbitals
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22pp
22ss
spsp33 Orbital Hybridization Orbital Hybridizationspsp33 Orbital Hybridization Orbital Hybridization
2 2 spsp33
4 equivalent half-filled 4 equivalent half-filled orbitals are consistent orbitals are consistent with four bonds and with four bonds and tetrahedral geometrytetrahedral geometry
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Shapes of orbitalsShapes of orbitalsShapes of orbitalsShapes of orbitals
ss
pp
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Nodal properties of orbitalsNodal properties of orbitalsNodal properties of orbitalsNodal properties of orbitals
ss
pp ++ ––
++
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Shape of spShape of sp33 hybrid orbitals hybrid orbitalsShape of spShape of sp33 hybrid orbitals hybrid orbitals
ss
pp ++ ––
++
take the take the ss orbital and place orbital and place it on top of the it on top of the pp orbital orbital
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Shape of spShape of sp33 hybrid orbitals hybrid orbitalsShape of spShape of sp33 hybrid orbitals hybrid orbitals
s + ps + p ++ ––++
reinforcement of electron wave in reinforcement of electron wave in regions where sign is the same regions where sign is the same destructive interference in regions destructive interference in regions of opposite sign of opposite sign
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Shape of spShape of sp33 hybrid orbitals hybrid orbitalsShape of spShape of sp33 hybrid orbitals hybrid orbitals
sp sp hybridhybrid
orbital shown is orbital shown is spsp hybrid hybrid
analogous procedure using three analogous procedure using three ss orbitals orbitals and one and one p p orbital gives orbital gives spsp33 hybrid hybrid
shape of shape of spsp33 hybrid is similar hybrid is similar
++ ––
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Shape of spShape of sp33 hybrid orbitals hybrid orbitalsShape of spShape of sp33 hybrid orbitals hybrid orbitals
sp sp hybridhybrid
hybrid orbital is not symmetricalhybrid orbital is not symmetricalhigher probability of finding an electron on higher probability of finding an electron on one side of the nucleus than the otherone side of the nucleus than the otherleads to stronger bondsleads to stronger bonds
++ ––
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––
++ ––
The C—H The C—H Bond in Methane Bond in MethaneThe C—H The C—H Bond in Methane Bond in Methane
spsp33ss CH
H—C H—C CH
gives a gives a bond. bond.
In-phase overlap of a half-filled 1In-phase overlap of a half-filled 1ss orbital of orbital of hydrogen with a half-filled hydrogen with a half-filled spsp33 hybrid orbital of hybrid orbital of carbon: carbon:
++
++
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Justification for Orbital Hybridization Justification for Orbital Hybridization Justification for Orbital Hybridization Justification for Orbital Hybridization
consistent with structure of methaneconsistent with structure of methane
allows for formation of 4 bonds rather than 2allows for formation of 4 bonds rather than 2
bonds involving bonds involving spsp3 3 hybrid orbitals are stronger hybrid orbitals are stronger
than those involving than those involving ss--s s overlap or overlap or pp--pp overlap overlap
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18.218.2spsp33 Hybridization Hybridization
and Bonding in Ethaneand Bonding in Ethane
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Structure of EthaneStructure of EthaneStructure of EthaneStructure of Ethane
CHCH33CHCH33
CC22HH66
tetrahedral geometry at each tetrahedral geometry at each carboncarbon
C—H bond distance = 110 pmC—H bond distance = 110 pm
C—C bond distance = 153 pmC—C bond distance = 153 pm
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In-phase overlap of half-filled In-phase overlap of half-filled spsp33 hybrid hybridorbital of one carbon with half-filled orbital of one carbon with half-filled spsp33
hybrid orbital of another.hybrid orbital of another.
Overlap is along internuclear axis to give a Overlap is along internuclear axis to give a bond. bond.
The C—C The C—C Bond in Ethane Bond in EthaneThe C—C The C—C Bond in Ethane Bond in Ethane
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The C—C The C—C Bond in Ethane Bond in EthaneThe C—C The C—C Bond in Ethane Bond in Ethane
In-phase overlap of half-filled In-phase overlap of half-filled spsp33 hybrid hybridorbital of one carbon with half-filled orbital of one carbon with half-filled spsp33
hybrid orbital of another.hybrid orbital of another.
Overlap is along internuclear axis to give a Overlap is along internuclear axis to give a bond. bond.
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18.218.2spsp22 Hybridization Hybridization
and Bonding in Ethyleneand Bonding in Ethylene
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CC22HH44
HH22C=CHC=CH22
planarplanar
bond angles: bond angles: close to 120°close to 120°
bond distances: bond distances: C—H = 110 pmC—H = 110 pm
C=C = 134 pmC=C = 134 pm
Structure of EthyleneStructure of EthyleneStructure of EthyleneStructure of Ethylene
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22ss
22pp
Promote an electron from the Promote an electron from the 22s s to the 2to the 2pp orbital orbital
spsp2 2 Orbital HybridizationOrbital Hybridizationspsp2 2 Orbital HybridizationOrbital Hybridization
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22ss
22pp 22pp
22ss
spsp22 Orbital Hybridization Orbital Hybridizationspsp22 Orbital Hybridization Orbital Hybridization
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22pp
22ss
spsp2 2 Orbital HybridizationOrbital Hybridizationspsp2 2 Orbital HybridizationOrbital Hybridization
Mix together (hybridize) the 2Mix together (hybridize) the 2s s orbital and two of the three 2orbital and two of the three 2pp orbitals orbitals
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22pp
22ss
spsp22 Orbital Hybridization Orbital Hybridizationspsp22 Orbital Hybridization Orbital Hybridization
2 2 spsp22
3 equivalent half-filled 3 equivalent half-filled spsp22 hybrid orbitals plus hybrid orbitals plus 1 1 pp orbital left orbital left unhybridizedunhybridized
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spsp22 Orbital Hybridization Orbital Hybridizationspsp22 Orbital Hybridization Orbital Hybridization
2 2 spsp22
2 of the 3 2 of the 3 spsp22 orbitals orbitals
are involved in are involved in bonds bonds
to hydrogens; the otherto hydrogens; the other
is involved in a is involved in a bond bond
to carbonto carbon
pp
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spsp22 Orbital Hybridization Orbital Hybridizationspsp22 Orbital Hybridization Orbital Hybridization
2 2 spsp22
pp
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Bonding in EthyleneBonding in Ethylene Bonding in EthyleneBonding in Ethylene
2 2 spsp22
the unhybridized the unhybridized pp orbital of orbital of
carbon is involved in carbon is involved in bonding bonding
to the other carbon to the other carbon
pp
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Bonding in EthyleneBonding in Ethylene Bonding in EthyleneBonding in Ethylene
2 2 spsp22
pp
each carbon has an unhybridized 2each carbon has an unhybridized 2pp orbital orbital
axis of orbital is perpendicular to the plane of the axis of orbital is perpendicular to the plane of the
bonds bonds
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Bonding in EthyleneBonding in Ethylene Bonding in EthyleneBonding in Ethylene
2 2 spsp22
pp
side-by-side overlap of half-filledside-by-side overlap of half-filled
pp orbitals gives a orbitals gives a bondbond
double bond in ethylene has a double bond in ethylene has a
component and a component and a component component
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Hybridization and methane: CH4
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sp3 hybridization and ethylene: H2C=CH2
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Ground state > excite one electron > mix orbitals:
Acetylene
C C HH
C NH
one s orbital and one p orbital = two sp orbitals
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Other examples of sp2 and sp hybridized carbon
Formaldehyde: H2C=O Carbon dioxide: O=C=O
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d2sp3 hybridization
dsp3 hybridization
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Hybrid orbitals are constructed on an atom to reproduce the electronic arrangement characteristics that will yield the experimental shape of a molecule
SN = 2
SN = 3
SN = 4
SN = 5
SN = 6
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BeF2: SN = 2 = sp
BF3: SN = 3 = sp2
CH4: SN = 4 = sp3
PF5: SN = 5 = sp3d
SF6: SN = 6 = sp3d2
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Describe the bonding for ethane, ethene and acetylene in terms of overlap of hybridized
orbitals
Ethane:
Ethylene:
Acetylene: