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Chapter 14: Q14.20E (page 599)

Give the expected hybridization of the central atom for the molecules in Exercises 99 and 100 from Chapter 13.

Short Answer

Expert verified

The expected hybridization of the central atom for the molecules are given below.

Step by step solution

Expected hybridization of central atom for exercise 99

In exercise 88

$d s p^{3}$ hybridization: XeCl₂
$d s p^{3}$ hybridization: ICl₃
$d s p^{3}$ hybridization: TeF₄
$d s p^{3}$ hybridization: PCl₅

They have a trigonal bipyramidal shape.

Expected hybridization of central atom for exercise 100

In exercise 94

$d^{2} s p^{3}$ hybridization: ICl₅
$d^{2} s p^{3}$ hybridization: XeCl₄
$d^{2} s p^{3}$ hybridization: SeCl₆

They have an octahedral shape.

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Most popular questions from this chapter

The microwave spectrum of ${}^{12}{C^{16}} O$ shows that the transition from J = 0 to J = 1 requires electromagnetic radiation with a wavelength of $2.60 \times 10^{- 3} m$ .

a. Calculate the bond length of CO. See Exercise 60for the atomic mass of ${}^{16}O$ .

b. Calculate the frequency of radiation absorbed in a rotational transition from the second to the third excited state of CO.

Given that the ionization energy of $F_{2}^{-}$ is 290 kJ/mol, do the following

a. Calculate the bond energy of $F_{2}^{-}$ . You will need to look up the bond energy of $F_{2}$ and ionization energy of $F^{-}$

b. Explain the difference in bond energy between $F_{2}^{-}$ and $F_{2}$ using MO theory.

Using bond energies from Table 13.6, estimate the barrier to rotation around a carbon-carbon double bond. To do this, consider what must happen to go from in terms of making and breaking chemical bonds; that is, what happens to the p bond?

The ${sp}^{2}$ hybrid atomic orbitals have the following general form:

role="math" localid="1663746599823" $ϕ_{1} = \sqrt{\frac{1}{3}} ϕ_{s} + 2 {Aϕ}_{px} ϕ_{2} = \sqrt{\frac{1}{3}} ϕ_{s} - 2 {Aϕ}_{px} + {Bϕ}_{py} ϕ_{3} = \sqrt{\frac{1}{3}} ϕ_{s} - 2 {Aϕ}_{px} - {Bϕ}_{py}$

where, $Φ_{s}, Φ_{px}$ androle="math" localid="1663746751426" $Φ_{py}$ represent orthonormal (normalized and orthogonalized) atomic orbitals. Calculate the values of Aand B.

Consider the molecular orbital electron configurations for $N_{2}$ , $N_{2}^{+}$ , and $N_{2}^{-}$ . For each compound or ion, fill in the table below with the correct number of electrons in each molecular orbital.

MO	$N_{2}$	role="math" localid="1663764752673" $N_{2}^{+}$	role="math" localid="1663764766917" $N_{2}^{-}$
role="math" localid="1663764800461" $σ_{2 p^{*}}$
role="math" localid="1663764811953" $π_{2 p^{*}}$
role="math" localid="1663764822519" $σ_{2 p}$
role="math" localid="1663764834336" $π_{2 p}$
role="math" localid="1663764966754" $σ_{2 s^{*}}$
role="math" localid="1663764978558" $σ_{2 s}$

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Give the expected hybridization of the central atom for the molecules in Exercises 99 and 100 from Chapter 13.

Short Answer

Step by step solution

Expected hybridization of central atom for exercise 99

Expected hybridization of central atom for exercise 100

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Most popular questions from this chapter

Recommended explanations on Chemistry Textbooks

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