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Chapter 9: Problem 86

An \(\mathrm{AB}_{2}\) molecule is described as having a tetrahedral geometry. (a) How many nonbonding domains are on atom A? (b) Based on the information given, which of the following is the molecular geometry of the molecule: (i) linear, (ii) bent, (iii) trigonal planar, or (iv) tetrahedral?

Short Answer

Expert verified
(a) There are 2 nonbonding domains on atom A. (b) The molecular geometry of the \(\mathrm{AB}_{2}\) molecule is (iv) tetrahedral.

Step by step solution

01

Identifying the number of nonbonding domains on atom A

In an \(\mathrm{AB}_{2}\) molecule, there are two bonding domains surrounding atom A, as it is connected to two B atoms. Each bonding domain consists of a pair of electrons shared between atom A and one of the B atoms. To determine how many nonbonding domains are present on atom A, we need to find out how many electron pairs are not involved in forming bonds. The molecule is described as having a tetrahedral geometry, which implies that there must be four total domains surrounding atom A (including both bonding and nonbonding domains). Thus, the number of nonbonding domains can be calculated as follows: \[Number\,of\,nonbonding\,domains = Total\,domains - Bonding\,domains\]
02

Calculate the number of nonbonding domains on atom A

Using the formula from Step 1, we can calculate the number of nonbonding domains on atom A: \[Number\,of\,nonbonding\,domains = 4 - 2\] \[Number\,of\,nonbonding\,domains = 2\] So there are 2 nonbonding domains on atom A. Answer (a): 2
03

Identifying the molecular geometry of the molecule

Since we know the total domains surrounding atom A and the number of nonbonding domains, we can now identify the molecular geometry of the \(\mathrm{AB}_{2}\) molecule. The molecular geometry can be one of the following based on the information given: (i) linear (ii) bent (iii) trigonal planar (iv) tetrahedral However, recall that we are given that the molecule has a tetrahedral geometry, implying that the molecular geometry must be tetrahedral. In the case of an \(\mathrm{AB}_{2}\) molecule with a tetrahedral geometry, the structure consists of 2 bonding domains and 2 nonbonding domains, and the B-A-B angle would be less than that of a regular tetrahedron, which is 109.5°. Answer (b): (iv) tetrahedral

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Most popular questions from this chapter

In which of these molecules or ions does the presence of nonbonding electron pairs produce an effect on molecular shape? (a) $\mathrm{CO}_{2},(\mathbf{b}) \mathrm{CH}_{2} \mathrm{Br}_{2,}(\mathbf{c}) \mathrm{OF}_{2},(\mathbf{d}) \mathrm{BCl}_{3},(\mathbf{e}) \mathrm{SF}_{6}$

(a) What is the difference between hybrid orbitals and molecular orbitals? (b) How many electrons can be placed into each MO of a molecule? (c) Can antibonding molecular orbitals have electrons in them?

(a) Boron trichloride \(\left(\mathrm{BCl}_{3}\right)\) and the carbonate ion \(\left(\mathrm{CO}_{3}^{2-}\right)\) are both described as trigonal. What does this indicate about their bond angles? (b) The \(\mathrm{PCl}_{3}\) molecule is trigonal pyramidal, while \(\mathrm{ICl}_{3}\) is T-shaped. Which of these molecules is flat?

For each statement, indicate whether it is true or false. (a) \(\ln\) order to make a covalent bond, the orbitals on each atom in the bond must overlap. (b) A \(p\) orbital on one atom cannot make a bond to an \(s\) orbital on another atom. \((\mathbf{c})\) Lone pairs of electrons on an atom in a molecule influence the shape of a molecule. (d) The 1 s orbital has a nodal plane. \((\mathbf{e})\) The \(2 p\) orbital has a nodal plane.

In ozone, \(\mathrm{O}_{3}\), the two oxygen atoms on the ends of the molecule are equivalent to one another. (a) What is the best choice of hybridization scheme for the atoms of ozone? (b) For one of the resonance forms of ozone, which of the orbitals are used to make bonds and which are used to hold nonbonding pairs of electrons? (c) Which of the orbitals can be used to delocalize the \(\pi\) electrons? (d) How many electrons are delocalized in the \(\pi\) system of ozone?
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