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Tetrahedral one s three p four sp3 none
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Octahedral one s three p two d six sp3d2 three d
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Orientation
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Hybridization of s, p, and d orbitals
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sp hybridization results from the overlap of an s orbital with one p orbital Two sp hybrid orbitals are formed with a bond angle of 180 This is a linear orientation
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2 2 sp hybridization results from the overlap of an s orbital with two p orbitals Three sp hybrid orbitals are formed with a trigonal planar orientation and a bond angle of 120
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Bonding 155
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One place this type of bonding occurs is in the formation of the carbon-to-carbon double bond, as will be discussed later 3 sp hybridization results from the mixing of one s orbital and three p orbitals, giving four 3 3 sp hybrid orbitals with a tetrahedral geometric orientation This sp hybridization is found in carbon when it forms four single bonds 3 sp d hybridization results from the blending of an s orbital, three p orbitals, and one d 3 orbital The result is five sp d orbitals with a trigonal bipyramidal orientation This type of bonding occurs in compounds like PCl5 Note that this hybridization is an exception to the octet rule 3 2 sp d hybridization occurs when one s, three p, and two d orbitals are mixed, giving an octahedral arrangement SF6 is an example Again, this hybridization is an exception to the octet rule If one starts with this structure and one of the bonding pairs becomes a lone pair, then a square pyramidal shape results, while two lone pairs gives a square planar shape
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sp2 sp2 H H1s sp2 H
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sp2 sp2 H H sp2 H H1s H C C H H
Combined unhybridized 2p
Hybridization in ethylene, H2C=CH2
Figure 118 shows the hybridization that occurs in ethylene, H2C=CH2 Each carbon 2 has undergone sp hybridization On each carbon, two of the hybrid orbitals have overlapped with an s orbital on a hydrogen atom, to form a carbon-to-hydrogen covalent bond 2 2 The third sp hybrid orbital has overlapped with the sp hybrid on the other carbon to form a carbon-to-carbon covalent bond Note that the remaining p orbital on each carbon that has not undergone hybridization is also overlapping above and below a line joining the carbons In ethylene there are two types of bond In sigma ( ) bonds, the overlap of the orbitals occurs on a line between the two atoms involved in the covalent bond In ethylene, the C H bonds and one of the C C bonds are sigma bonds In pi ( ) bonds, the overlap of orbitals occurs above and below a line through the two nuclei of the atoms involved in the bond A double bond always is composed of one sigma and one pi bond A carbon-tocarbon triple bond results from the overlap of an sp hybrid orbital and two p orbitals on one carbon, with the same on the other carbon In this situation there will be one sigma bond (overlap of the sp hybrid orbitals) and two pi bonds (overlap of two sets of p orbitals)
Molecular Orbital Theory
Still another model to represent the bonding that takes place in covalent compounds is the molecular orbital theory In the molecular orbital (MO) theory of covalent bonding, atomic orbitals (AOs) on the individual atoms combine to form orbitals that encompass the
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entire molecule These are called molecular orbitals (MOs) These molecular orbitals have definite shapes and energies associated with them When two atomic orbitals are added, two molecular orbitals are formed, one bonding and one antibonding The bonding MO is of lower energy than the antibonding MO In the molecular orbital model the atomic orbitals are added together to form the molecular orbitals Then the electrons are added to the molecular orbitals, following the rules used previously when filling orbitals: lowest-energy orbitals get filled first, maximum of two electrons per orbital, and half fill orbitals of equal energy before pairing electrons (see 3) When s atomic orbitals are added, one sigma bonding ( ) and one sigma antibonding ( *) molecular orbital are formed Figure 119 shows the molecular orbital diagram for H2
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