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Chapter 9: Problem 52

What is the hybridization of the central atom in (a) \(\mathrm{SiCl}_{4}\), \((\mathbf{b}) \mathrm{HCN},(\mathbf{c}) \mathrm{SO}_{3},(\mathbf{d}) \mathrm{TeCl}_{2} ?\)

Short Answer

Expert verified
The hybridizations of the central atoms in the given compounds are: (a) SiCl₄: \(sp^3\); (b) HCN: \(sp\); (c) SO₃: \(sp^2\); and (d) TeCl₂: \(sp^3\).

Step by step solution

01

Determine the electron domain count for each central atom

For SiCl₄, the central atom Si has four single bonds (sigma bonds) with four Cl atoms, and no lone pairs. So, the electron domain count is 4. For HCN, the central atom C has one sigma bond with H, a triple bond with one sigma bond and two pi bonds with N, and no lone pairs. So, the electron domain count is 2. For SO₃, the central atom S has a resonance structure with three double bonds (one sigma bond and one pi bond each) to three O atoms, and no lone pairs. So, the electron domain count is 3. For TeCl₂, the central atom Te has two single bonds (sigma bonds) with two Cl atoms, plus two lone pairs. So, the electron domain count is 4.
02

Determine the hybridization based on electron domain count

For Si in SiCl₄, with an electron domain count of 4, the hybridization is sp³ (s¹p³). For C in HCN, with an electron domain count of 2, the hybridization is sp (s¹p¹). For S in SO₃, with an electron domain count of 3, the hybridization is sp² (s¹p²). For Te in TeCl₂, with an electron domain count of 4, the hybridization is sp³ (s¹p³). Now we have determined the hybridization for the central atom in each of the given compounds: (a) SiCl₄: sp³ hybridization (b) HCN: sp hybridization (c) SO₃: sp² hybridization (d) TeCl₂: sp³ hybridization

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Most popular questions from this chapter

(a) Does SCl\(_{2}\) have a dipole moment? If so, in which direction does the net dipole point? (b) Does BeCl\(_{2}\) have a dipole moment? If so, in which direction does the net dipole point?

(a) If you combine two atomic orbitals on two different atoms to make a new orbital, is this a hybrid orbital or a molecular orbital? (b) If you combine two atomic orbitals on one atom to make a new orbital, is this a hybrid orbital or a molecular orbital? (c) Does the Pauli exclusion principle (Section 6.7) apply to MOs? Explain.

Place the following molecules and ions in order from smallest to largest bond order: \(\mathrm{H}_{2}^{+}, \mathrm{B}_{2}, \mathrm{N}_{2}^{+}, \mathrm{F}_{2}^{+},\) and \(\mathrm{Ne}_{2}\) .

Give the electron-domain and molecular geometries for the following molecules and ions: (a) \(\mathrm{HCN},(\mathbf{b}) \mathrm{SO}_{3}^{2-},(\mathbf{c}) \mathrm{SF}_{4}\) \((\mathbf{d}) \mathrm{PF}_{6},(\mathbf{e}) \mathrm{NH}_{3} \mathrm{Cl}^{+},(\mathbf{f}) \mathrm{N}_{3}^{-}\)

The nitrogen atoms in \(\mathrm{N}_{2}\) participate in multiple bonding, whereas those in hydrazine, \(\mathrm{N}_{2} \mathrm{H}_{4},\) do not. (a) Draw Lewis structures for both molecules. (b) What is the hybridization of the nitrogen atoms in each molecule? (c) Which molecule has the stronger \(N-N\) bond?
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