91Ó°ÊÓ

Show the dipole arrow for each of the following bonds: (6.7) a. \(\mathrm{Si}-\mathrm{Cl}\) b. \(\mathrm{C}-\mathrm{N}\) c. \(\mathrm{F}-\mathrm{Cl}\) d. \(\mathrm{C}-\mathrm{F}\) e. \(\mathrm{N}-\mathrm{O}\)

Show the dipole arrow for each of the following bonds: (6.7) a. \(\mathrm{P}-\mathrm{O}\) b. \(\mathrm{N}-\mathrm{F}\) c. \(\mathrm{O}-\mathrm{Cl}\) d. \(\mathrm{S}-\mathrm{Cl}\) e. \(\mathrm{P}-\mathrm{F}\)

For each of the following, draw the Lewis structure and determine the shape: (6.6,6.8) a. \(\mathrm{NF}_{3}\) b. \(\mathrm{SiBr}_{4}\) c. \(\mathrm{CSe}_{2}\)

For each of the following, draw the Lewis structure and determine the shape: (6.6,6.8) a. \(\mathrm{COCl}_{2}\) (C is the central atom) b. \(\mathrm{HCCH}\) c. \(\mathrm{SO}_{2}\)

Classify the following molecules as polar or nonpolar: (6.8) a. \(\mathrm{ClF}_{3}\) b. \(\mathrm{CO}_{2}\) c. \(\mathrm{HBr}\)

Classify each of the following molecules as polar or nonpolar: (6.8,6.9) a. \(\mathrm{GeH}_{4}\) b. \(\mathrm{I}_{2}\) c. \(\mathrm{CF}_{3} \mathrm{Cl}\) d. \(\mathrm{PCl}_{3}\) e. \(\mathrm{BCl}_{3}\) f. \(\mathrm{SCl}_{2}\)

Indicate the major type of intermolecular forces \(-(1)\) ionic bonds, (2) dipole-dipole attractions, ( 3 ) hydrogen bonds, (4) dispersion forces-that occurs between particles of the following: (6.9) a. \(\mathrm{NF}_{3}\) b. ClF c. \(\mathrm{Br}_{2}\) d. \(\mathrm{Cs}_{2} \mathrm{O}\) e. \(\mathrm{C}_{4} \mathrm{H}_{10}\) f. \(\mathrm{CH}_{3} \mathrm{OH}\)

Indicate the major type of intermolecular forces- (1) ionic bonds, (2) dipole- dipole attractions, ( 3 ) hydrogen bonds, (4) dispersion forces-that occurs between particles of the following: (6.9) a. \(\mathrm{CHCl}_{3}\) b. \(\mathrm{H}_{2} \mathrm{O}\) c. \(\mathrm{LiCl}\) d. \(\mathrm{OBr}_{2}\) e. HBr f. IBr

Identify the group number in the periodic table of \(\mathrm{X},\) a representative element, in each of the following ionic compounds: (6.2) a. \(\mathrm{XCl}_{2}\) b. \(\mathrm{X}_{2} \mathrm{CO}_{3}\) c. \(\mathrm{XBr}_{4}\)

Classify each of the following as ionic or molecular, and name each: (6.2,6.3,6.4,6.5) a. \(\mathrm{Na}_{2} \mathrm{O}\) b. \(\mathrm{WO}_{2}\) c. \(\mathrm{BaCO}_{3}\) d. \(\mathrm{NF}_{3}\) e. \(\mathrm{CS}_{2}\) f. \(\mathrm{Cs}_{3} \mathrm{PO}_{4}\) g. \(\mathrm{K}\left(\mathrm{AuCl}_{4}\right)\) h. \(\mathrm{Cl}_{2}\)