Molecular Shapes & Valence Bond Theory - Part 2 of 2 Exam Prep

12. Molecular Shapes & Valence Bond Theory - Part 2 of 2

Problem 1
Problem 2
Problem 3
Problem 4
Problem 5
Problem 6
Problem 7
Problem 8
Problem 9
Problem 10
Problem 11

12. Molecular Shapes & Valence Bond Theory - Part 2 of 2

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12. Molecular Shapes & Valence Bond Theory - Part 2 of 2

11 problems

1PRACTICE PROBLEM

Indigo is an organic compound that is a derivative of indole. Most of the indigo dye produced today is consumed to dye cotton yarn - to make denim and blue jeans. The chemical structure of indigo is given below. Determine the number of unhybridized orbitals on N and C atoms in indigo. [Hint: Due to resonance stabilization/aromaticity N is sp² hybridized.]

Chemical structure of indigo, highlighting hybridization for N and C atoms.

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2PRACTICE PROBLEM

Draw a diagram that illustrates the position and geometry of the p orbitals in ozone (O₃). Using a localized valence bond model for σ bonds and a delocalized MO model for π bonds, explain the bonding in the compound.

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3PRACTICE PROBLEM

Draw a molecular orbital diagram for a chain containing 5 sodium atoms and identify the number of molecular orbitals.

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4PRACTICE PROBLEM

If the He₂⁺ ion was excited by light to move an electron:

a) there would be more antibonding electrons than bonding electrons In the excited state.

b) the light would excite the electron from a higher energy MO to a lower energy MO.

c) the light would excite the electron from a lower energy MO to a higher energy MO.

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5PRACTICE PROBLEM

Using the MO diagram similar to F₂, determine whether Cl₂^– ion is diamagnetic or paramagnetic.

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6PRACTICE PROBLEM

If all the electrons in a substance are paired and it is weakly repelled by a magnetic field, is it paramagnetic or diamagnetic? Among the following substances, choose the molecules or ions with the previously described characteristics: N₂⁺, O₂^2–, B₂^–, C₂⁺, F₂²⁺

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7PRACTICE PROBLEM

When fuel is burned at a high temperature, NO is produced. What is the valence molecular orbital electron configuration for NO if it has the same energy order as H₂?

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8PRACTICE PROBLEM

Select the species that have unpaired electrons based on electron configurations

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9PRACTICE PROBLEM

Draw molecular orbital diagrams for the following molecules/ions: F₂⁺, F₂, and F₂^–. Identify which of the three is the most stable and determine the bond order for each. Which is/are paramagnetic?

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10PRACTICE PROBLEM

Which molecule between S₂, S₂^- and S₂^2- has the highest bond order based on MO theory?

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11PRACTICE PROBLEM

To answer the following questions, use the given molecular orbital diagram below.

A. How many unpaired electrons are in NO?

a. 0 b. 1 c. 2 d. 3

B. What is the bond order of CO?

a. 1.5 b. 2 c. 2.5 d. 3

C. Which of the following is not paramagnetic?

a. NO⁺ b. OF c. NO d. CO⁺