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. 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 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_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?? 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

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? d. 14

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

Use molecular orbital theory to predict if each molecule or ion exists in a relatively stable form. a. F22–

According to MO theory, which molecule or ion has the highest bond order? O₂, O₂^- , O₂^2-

According to MO theory, which molecule or ion has the highest bond energy? O₂, O₂^- , O₂^2-

According to MO theory, which molecule or ion has the shortest bond length? O₂, O₂^- , O₂^2-

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.

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

The genetic code is based on four different bases with the structures shown here. Assign a geometry and hybridization to each interior atom in these four bases. d. guanine

The structure of acetylsalicylic acid (aspirin) is shown here. How many π bonds are present in acetylsalicylic acid?

The structure of acetylsalicylic acid (aspirin) is shown here. How many sigma bonds?

Most vitamins can be classified as either fat soluble, which results in their tendency to accumulate in the body (so that taking too much can be harmful), or water soluble, which results in their tendency to be quickly eliminated from the body in urine. Examine the structural formulas and space-filling models of these vitamins and determine whether each one is fat soluble (mostly nonpolar) or water soluble (mostly polar). (a) vitamin C

Most vitamins can be classified as either fat soluble, which results in their tendency to accumulate in the body (so that taking too much can be harmful), or water soluble, which results in their tendency to be quickly eliminated from the body in urine. Examine the structural formulas and space-filling models of these vitamins and determine whether each one is fat soluble (mostly nonpolar) or water soluble (mostly polar). (c) niacin (vitamin B3)

Water does not easily remove grease from dishes or hands because grease is nonpolar and water is polar. The addition of soap to water, however, allows the grease to dissolve. Study the structure of sodium stearate (a soap) and describe how it works.