91Ó°ÊÓ

Give the ground-state electron configuration for each of the following elements: (a) Oxygen (b) Nitrogen (c) Sulfur

Draw a molecule of chloroform, CHCl \(_{3}\), using solid, wedged, and dashed lines to show its tetrahedral geometry.

What are likely formulas for the following substances? (a) CCl? (b) AlH? (c) \(\mathrm{CH}_{?} \mathrm{Cl}_{2}\) (d) \(\mathrm{SiF}_{?}\) (e) \(\mathrm{CH}_{3} \mathrm{NH}_{?}\)

Write line-bond structures for the following substances, showing all nonbonding electrons: (a) \(\mathrm{CHCl}_{3}\), chloroform (b) \(\mathrm{H}_{2} \mathrm{~S}\), hydrogen sulfide (c) \(\mathrm{CH}_{3} \mathrm{NH}_{2}\), methylamine (d) \(\mathrm{CH}_{3} \mathrm{Li}\), methyllithium

Why can't an organic molecule have the formula \(\mathrm{C}_{2} \mathrm{H}_{7} ?\)

Draw a line-bond structure for propane, \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CH}_{3}\). Predict the value of each bond angle, and indicate the overall shape of the molecule.

Draw a line-bond structure for propene, \(\mathrm{CH}_{3} \mathrm{CH}=\mathrm{CH}_{2}\). Indicate the hybridization of the orbitals on each carbon, and predict the value of each bond angle.

Draw a line-bond structure for 1,3 -butadiene, \(\mathrm{H}_{2} \mathrm{C}=\mathrm{CH}-\mathrm{CH}=\mathrm{CH}_{2} .\) Indicate the hybridization of the orbitals on each carbon, and predict the value of each bond angle.

Draw a line-bond structure for propyne, \(\mathrm{CH}_{3} \mathrm{C} \equiv \mathrm{CH} .\) Indicate the hybridization of the orbitals on each carbon, and predict a value for each bond angle.

Propose skeletal structures for compounds that satisfy the following molecular formulas. There is more than one possibility in each case. (a) \(\mathrm{C}_{5} \mathrm{H}_{12}\) (b) \(\mathrm{C}_{2} \mathrm{H}_{7} \mathrm{~N}\) (c) \(\mathrm{C}_{3} \mathrm{H}_{6} \mathrm{O}\) (d) \(\mathrm{C}_{4} \mathrm{H}_{9} \mathrm{Cl}\)