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Chapter 9: Problem 22

How many electron domains are surrounding the central atoms which adopt the following geometries? (a) linear (b) trigonal planar (c) trigonal pyramidal (d) trigonal bipyramidal.

Short Answer

Expert verified
The number of electron domains surrounding the central atoms for each geometry is as follows: (a) Linear: 2, (b) Trigonal planar: 3, (c) Trigonal pyramidal: 4, and (d) Trigonal bipyramidal: 5.

Step by step solution

01

(a) Linear

1. The linear geometry has two atoms bonded to the central atom. So, there are two bonds. 2. Since the geometry is linear, there are no lone pairs. 3. The number of electron domains is the sum of the number of bonds and lone pairs. Number of electron domains = 2 bonds + 0 lone pairs = 2.
02

(b) Trigonal Planar

1. The trigonal planar geometry has three atoms bonded to the central atom. So, there are three bonds. 2. In trigonal planar geometry, there are no lone pairs. 3. The number of electron domains is the sum of the number of bonds and lone pairs. Number of electron domains = 3 bonds + 0 lone pairs = 3.
03

(c) Trigonal Pyramidal

1. The trigonal pyramidal geometry has three atoms bonded to the central atom. So, there are three bonds. 2. In trigonal pyramidal geometry, there is one lone pair. 3. The number of electron domains is the sum of the number of bonds and lone pairs. Number of electron domains = 3 bonds + 1 lone pair = 4.
04

(d) Trigonal Bipyramidal

1. The trigonal bipyramidal geometry has five atoms bonded to the central atom. So, there are five bonds. 2. In trigonal bipyramidal geometry, there are no lone pairs. 3. The number of electron domains is the sum of the number of bonds and lone pairs. Number of electron domains = 5 bonds + 0 lone pairs = 5. So, the central atoms of linear, trigonal planar, trigonal pyramidal, and trigonal bipyramidal geometries have 2, 3, 4, and 5 electron domains, respectively.

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Most popular questions from this chapter

(a) Which geometry and central atom hybridization would you expect in the series $\mathrm{BH}_{4}^{-}, \mathrm{CH}_{4}, \mathrm{NH}_{4}{ }^{+} ?(\mathbf{b})$ What would you expect for the magnitude and direction of the bond dipoles in this series? (c) Write the formulas for the analogous species of the elements of period 3 ; would you expect them to have the same hybridization at the central atom?

In which of the following AF \(_{n}\) molecules or ions is there more than one \(\mathrm{F}-\mathrm{A}-\mathrm{F}\) bond angle: $\mathrm{PF}_{6}^{-}, \mathrm{SbF}_{\mathrm{s}}, \mathrm{SF}_{4} ?$

(a) Sketch the molecular orbitals of the \(\mathrm{H}_{2}^{-}\) ion and draw its energy-level diagram. (b) Write the electron configuration of the ion in terms of its MOs. (c) Calculate the bond order in \(\mathrm{H}_{2}^{-}\). (d) Suppose that theion is excited by light, sothat an electron moves from a lower-energy to a higher-energy molecular orbital. Would you expect the excited-state \(\mathrm{H}_{2}^{-}\) ion to be stable? (e) Which of the following statements about part (d) is correct: (i) The light excites an electron from a bonding orbital to an antibonding orbital, (ii) The light excites an electron from an antibonding orbital to a bonding orbital, or (iii) In the excited state there are more bonding electrons than antibonding electrons?

Draw sketches illustrating the overlap between the following orbitals on two atoms: (a) the \(2 s\) orbital on each atom, (b) the \(2 p_{z}\) orbital on each atom (assume both atoms are on the \(z\) -axis), \((\mathbf{c})\) the 2 s orbital on one atom and the \(2 p_{2}\) orbital on the other atom.

What is the hybridization of the central atom in (a) \(\mathrm{PBr}_{5}\), (b) \(\mathrm{CH}_{2} \mathrm{O},\) (c) \(\mathrm{O}_{3},(\mathbf{d}) \mathrm{NO}_{2} ?\)
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