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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

where the second equality comes from Eq (1154) Integration of this equation for a phase from Tm,to T gives:

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Equation (1480)is applied separately to the solid and liquid phases The resulting expressions are substituted into Eq (1479),which is then reduced by the identity:

-(ffF>" - H ~ '= -[(Hf - H f g )- ( f f : )

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W H AT I T TA K E S T O B E # 1

This yields the exact expression:

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

ffjg)]

Evaluation of the integral proceeds as follows:

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and Hence, for a phase,

Answer the following questions You have 15 minutes, and you may not use a calculator You may use the tables at the back of the book Answer each of the following with respect to chemical bonding and structure

Applying Eq (1482) separately to the solid and liquid phases and performing the integration required by Eq (1481) yields:

where integral I is defined by:

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