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Chapter 1: Q-1-46P (page 2)

Which of the following molecules would you expect to have a dipole moment of zero? To answer parts g and h, you may need to review the Problem Solving Strategy on p. 39.

Short Answer

Expert verified

BeCl2, BF3, have zero dipole moment.

Step by step solution

01

Finding out the electronic configuration.

BeCl2

Electronic configuration: 1s22s22p0

BF3

Electronic configuration of Boron: 1s22s22p1

02

finding out the dipole moment.

BeCl2

BeCl2is sp hybridised thus has linear structure, bond angle is 180.

Cl-Be-Cl .As a result the dipole moments on both sides cancel each other and the net dipole moment is zero.

BF3

BF3 has sp2 hybridisation, thus is trigonal planar in shape.

The resultant dipole moment of any two bonds is equal and opposite to the dipole moment of the third bond. Thus cancels each other and gives a zero dipole moment.

The resultant dipole moment of any two bonds is equal and opposite to the dipole moment of the third bond. Thus cancels each other and gives a zero dipole moment.

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Most popular questions from this chapter

Indicate the kind of molecular orbital (σ ,σ *,π ,π *) that results when the two atomic orbitals are combined:

Predict the approximate bond angles for

  1. The C-N-C bond angle in(CH3)2 NH2+.
  2. The C-N-H bond angle in CH3CH2NH2.
  3. The H-C-N bond angle in(CH3)2NH.
  4. The H-C-O bond angle in CH3OCH3.

How many valence electrons do the following atoms have?

  1. Boron 2. nitrogen 3. oxygen 4. Fluorine

a. Which bond will be longer?

b. Which bond will be stronger?

  1. C-Cl or C-l
  2. C-C or C-l
  3. H-Cl or H-F

Draw Lewis structure of the following

a.CH3CHO

b.CH3OCH3

c.CH3COOH
See all solutions

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