12. Molecular Shapes & Valence Bond Theory

MO Theory: Bond Order

12. Molecular Shapes & Valence Bond Theory

MO Theory: Bond Order

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MO Theory: Bond Order Concept 1

MO Theory: Bond Order Example 1

MO Theory: Bond Order Concept 2

MO Theory: Bond Order Example 2

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Introduction to Molecular Orbital Theory

29:56

Introduction to Molecular Orbital Theory

Molecular Orbital Theory - Bonding & Antibonding MO - Bond Order

The Organic Chemistry Tutor

The Molecular Orbital Theory.

Molecular Orbital Theory III: Bond Order and Stability

1.4 Molecular Orbital Theory

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Multiple Choice

Apply Molecular Orbital Theory to determine the bond order of HHe⁺ion.

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Multiple Choice

Apply molecular orbital theory to predict which species has the strongest bond.

a) O₂ b) O₂^– c) O₂⁺ d) All the bonds are equivalent

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Multiple Choice

Using Molecular Orbital Theory, answer the following questions dealing with carbon mononitride, CN.

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Multiple Choice

Which of the following is not consistent with the valence bond theory description of the formation of a chemical bond?

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Textbook Question

The C2 molecule has a MO diagram similar to N2 (Figure 8.22a). What is the bond order of C2 and is it paramagnetic or diamagnetic? (LO 8.12) (a) Bond order = 2, diamagnetic (b) Bond order = 2, paramagnetic (c) Bond order = 0, paramagnetic (d) Bond order = 3>2, diamagnetic

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Textbook Question

Consider the H2+ ion. (d) What is the bond order in H2+?

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Textbook Question

Consider the H2+ ion. (e) Suppose that the ion is excited by light so that an electron moves from a lower-energy to a higher-energy MO. Would you expect the excited-state H2+ ion to be stable or to fall apart?

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Textbook Question

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Textbook Question

Draw an MO energy diagram and predict the bond order of Li2+ and Li2-. Do you expect these molecules to exist in the gas phase?

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Textbook Question

Using the molecular orbital energy ordering for second-row homonuclear diatomic molecules in which the p2p orbitals lie at lower energy than the s2p, draw MO energy diagrams and predict the bond order in a molecule or ion with each number of total valence electrons. Will the molecule or ion be diamagnetic or paramagnetic? d. 9

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Textbook Question

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Textbook Question

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Textbook Question

Explain the following: (c) The O22 + ion has a stronger O—O bond than O2 itself.

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Textbook Question

Using the molecular orbital energy ordering for second-row homonuclear diatomic molecules in which the p2p orbitals lie at higher energy than the s2p, draw MO energy diagrams and predict the bond order in a molecule or ion with each number of total valence electrons. Will the molecule or ion be diamagnetic or paramagnetic? d. 14

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Textbook Question

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Textbook Question

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Textbook Question

Use molecular orbital theory to predict if each molecule or ion exists in a relatively stable form. a. H22 -

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Textbook Question

Apply molecular orbital theory to predict if each molecule or ion exists in a relatively stable form. a. C22+ b. Li2 c. Be22+ d. Li22-

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Textbook Question

Using Figures 9.35 and 9.43 as guides, draw the molecular orbital electron configuration for (d) Ne22 +. In each case indicate whether the addition of an electron to the ion would increase or decrease the bond order of the species.

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Textbook Question

If we assume that the energy-level diagrams for homonuclear diatomic molecules shown in Figure 9.43 can be applied to heteronuclear diatomic molecules and ions, predict the bond order and magnetic behavior of (d) ClF.

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Textbook Question

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Textbook Question

According to MO theory, which molecule or ion has the shortest bond length? O2, O2- , O22 -

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Textbook Question

According to MO theory, which molecule or ion has the highest bond energy? O2, O2- , O22 -

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Textbook Question

According to MO theory, which molecule or ion has the highest bond order? O2, O2- , O22 -

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Textbook Question

Determine the electron configurations for CN+, CN, and CN-. (a) Which species has the strongest C¬N bond?

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Textbook Question

Draw an MO energy diagram for CO. (Use the energy ordering of O2.) Predict the bond order and make a sketch of the lowest energy bonding molecular orbital.

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Textbook Question

Draw an energy diagram for HCl. Predict the bond order and make a sketch of the lowest energy bonding molecular orbital.

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Textbook Question

Draw a molecular orbital energy diagram for ClF. (Assume that the sp orbitals are lower in energy than the p orbitals.) What is the bond order in ClF?

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Textbook Question

Draw Lewis structures and MO diagrams for CN+ , CN, and CN- . According to the Lewis model, which species is most stable?

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Textbook Question

Use the MO energy diagram in Figure 8.22b to describe the bonding in O2+, O2, and O2-. Which of the three is likely to be stable? What is the bond order of each? Which contain unpaired electrons?

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Textbook Question

The C2 molecule can be represented by an MO diagram similar to that in Figure 8.22a. (b) To increase the bond order of C2, should you add or remove an electron?

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Textbook Question

Calcium carbide, CaC2, reacts with water to produce acetylene, C2H2, and is sometimes used as a convenient source of that substance. Use the MO energy diagram in Figure 8.22a to describe the bonding in the carbide anion, C22-. What is its bond order?

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Textbook Question

One of the molecular orbitals of the H2- ion is sketched below: (d) Compared to the H¬H bond in H2, the H¬H bond in H2- is expected to be which of the following: (i) Shorter and stronger, (ii) longer and stronger, (iii) shorter and weaker, (iv) longer and weaker, or (v) the same length and strength?

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Textbook Question

At high temperatures, sulfur vapor is predominantly in the form of S21g2 molecules. (d) When two electrons are added to S2, the disulfide ion S22- is formed. Is the bond length in S22- likely to be shorter or longer than the bond length in S2? Explain.

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Textbook Question

Place the following molecules and ions in order from smallest to largest bond order: N22+, He2+, Cl2 H2-, O22-.

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Textbook Question

Carbon monoxide is produced by incomplete combustion of fossil fuels. (c) What is the bond order of CO? Does this match the bond order predicted by the electron-dot structure?

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Textbook Question

The energy-level diagram in Figure 9.36 shows that the sideways overlap of a pair of p orbitals produces two molecular orbitals, one bonding and one antibonding. In ethylene there is a pair of electrons in the bonding π orbital between the two carbons. Absorption of a photon of the appropriate wavelength can result in promotion of one of the bonding electrons from the p2p to the p*2p molecular orbital. (c) Is the C¬C bond in ethylene stronger or weaker in the excited state than in the ground state? Why?

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Open Question

Determine the bond order in a molecule or ion with 12 valence electrons.

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Open Question

Use the molecular orbital diagram shown to determine which of the following is most stable.

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Open Question

Use molecular orbital theory to predict whether or not each of the following molecules or ions should exist in a relatively stable form.

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Open Question

Use the molecular orbital diagram shown to determine which of the following is least stable.

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Open Question

Complete the molecular orbital diagram for CN⁻. Note that the 1𝑠 orbitals are not shown.

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12. Molecular Shapes & Valence Bond Theory

MO Theory: Bond Order

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