The valence electron configurations of several atoms are shown here. How many bonds can each atom make without hybridization? b. P 3s²3p³

The valence electron configurations of several atoms are shown here. How many bonds can each atom make without hybridization? c. F 2s²2p⁵

The valence electron configurations of several atoms are shown here. How many bonds can each atom make without hybridization? a. B 2s²2p¹ b. N 2s²2p³

The valence electron configurations of several atoms are shown here. How many bonds can each atom make without hybridization? c. O 2s²2p⁴

Write orbital diagrams (boxes with arrows in them) to represent the electron configurations—without hybridization—for all the atoms in SF₂. Circle the electrons involved in bonding. Draw a three-dimensional sketch of the molecule and show orbital overlap. What bond angle do you expect from the unhybridized orbitals? How well does valence bond theory agree with the experimentally measured bond angle of 98.2° ?

Write orbital diagrams (boxes with arrows in them) to represent the electron configuration of carbon before and after sp³ hybridization.

Write orbital diagrams (boxes with arrows in them) to represent the electron configurations of carbon before and after sp hybridization.

Which hybridization scheme allows the formation of at least one p bond? sp³, sp², sp³d²

Which hybridization scheme allows the central atom to form more than four bonds? sp³, sp³d, sp²

Write a hybridization and bonding scheme for each molecule. Sketch the molecule, including overlapping orbitals, and label all bonds using the notation shown in Examples 11.6 and 11.7. a. CCl4

Write a hybridization and bonding scheme for each molecule. Sketch the molecule, including overlapping orbitals, and label all bonds using the notation shown in Examples 11.6 and 11.7. b. NH3

Write a hybridization and bonding scheme for each molecule. Sketch the molecule, including overlapping orbitals, and label all bonds using the notation shown in Examples 11.6 and 11.7. c. OF2

Write a hybridization and bonding scheme for each molecule or ion. Sketch the structure, including overlapping orbitals, and label all bonds using the notation shown in Examples 11.6 and 11.7. a. COCl2 (carbon is the central atom)

Write a hybridization and bonding scheme for each molecule or ion. Sketch the structure, including overlapping orbitals, and label all bonds using the notation shown in Examples 11.6 and 11.7. d. I3–

Write a hybridization and bonding scheme for each molecule or ion. Sketch the structure, including overlapping orbitals, and label all bonds using the notation shown in Examples 10.6 and 10.7. a. SO₃^2-

Write a hybridization and bonding scheme for each molecule that contains more than one interior atom. Indicate the hybridization about each interior atom. Sketch the structure, including overlapping orbitals, and label all bonds using the notation shown in Examples 10.6 and 10.7. c. C₂H₆ (skeletal structure H₃CCH₃)

Consider the structure of the amino acid alanine. Indicate the hybridization about each interior atom.

Consider the structure of the amino acid aspartic acid. Indicate the hybridization about each interior atom.

Sketch the bonding molecular orbital that results from the linear combination of two 1s orbitals. Indicate the region where interference occurs and state the kind of interference (constructive or destructive).

Draw an MO energy diagram and predict the bond order of Be₂⁺ and Be₂^- . Do you expect these molecules to exist in the gas phase?

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?

Sketch the bonding and antibonding molecular orbitals that result from linear combinations of the 2p_x atomic orbitals in a homonuclear diatomic molecule. (The 2p_x orbitals are those whose lobes are oriented along the bonding axis.)

Sketch the bonding and antibonding molecular orbitals that result from linear combinations of the 2p_z atomic orbitals in a homonuclear diatomic molecule. (The 2p_z orbitals are those whose lobes are oriented perpendicular to the bonding axis.) How do these molecular orbitals differ from those obtained from linear combinations of the 2p_y atomic orbitals? (The 2p_y orbitals are also oriented perpendicular to the bonding axis, but also perpendicular to the 2p_z orbitals.)

Using the molecular orbital energy ordering for second-row homonuclear diatomic molecules in which the π_2p orbitals lie at lower energy than the σ_2p, 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? a. 4 b. 6

Using the molecular orbital energy ordering for second-row homonuclear diatomic molecules in which the π_2p orbitals lie at lower energy than the σ_2p, 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? c. 8

Using the molecular orbital energy ordering for second-row homonuclear diatomic molecules in which the π_2p orbitals lie at lower energy than the σ_2p, 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?? b. 6 d. 9

Using the molecular orbital energy ordering for second-row homonuclear diatomic molecules in which the π_2p orbitals lie at higher energy than the σ_2p, 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? a. 10

Using the molecular orbital energy ordering for second-row homonuclear diatomic molecules in which the π_2p orbitals lie at higher energy than the σ_2p, 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? c. 13