A hydride of silicon prepared by the reaction of $\mathrm{Mg} 2 \mathrm{Si}$ with acid exerted a pressure of 306 torr at $26^{\circ} \mathrm{C}$ in a bulb with a volume of $57.0 \mathrm{~mL}$. If the mass of the hydride was $0.0861 \mathrm{~g}$, what is its molecular mass? What is the molecular formula for the hydride?

Why is boron limited to a maximum coordination number of four in its compounds?

Write a balanced equation for the reaction of elemental boron with each of the following (most of these reactions require high temperature): (a) $\mathrm{F}_2$ (b) $\mathrm{O}_2$ (c) $\mathrm{S}$ (d) $\mathrm{Se}$ (e) $\mathrm{Br}_2$

ame each of the following compounds: (a) $\mathrm{TeO}_2$ (b) $\mathrm{Sb}_2 \mathrm{~S}_3$ (c) $\mathrm{GeF}_4$ (d) $\mathrm{SiH}_4$ (e) $\mathrm{GeH}_4$

Silicon reacts with sulfur at elevated temperatures. If $0.0923 \mathrm{~g}$ of silicon reacts with sulfur to give $0.3030 \mathrm{~g}$ of silicon sulfide, determine the empirical formula of silicon sulfide.

Classify each of the following molecules as polar or nonpolar. You may wish to review the chapter on chemical bonding. (a) $\mathrm{SiH}_4$ (b) $\mathrm{Si}_2 \mathrm{H}_6$ (c) $\mathrm{SiCl}_3 \mathrm{H}$ (d) $\mathrm{SiF}_4$ (e) $\mathrm{SiCl}_2 \mathrm{~F}_2$

Describe the hybridization and the bonding of a silicon atom in elemental silicon.

Describe the hybridization of silicon and the molecular structure of the following molecules and ions: (a) $\left(\mathrm{CH}_3\right)_3 \mathrm{SiH}$ (b) $\mathrm{SiO}_4^{4-}$ (c) $\mathrm{Si}_2 \mathrm{H}_6$ (d) $\mathrm{Si}(\mathrm{OH})_4$ (e) $\mathrm{SiF}_6{ }^{2-}$

Write a Lewis structure for each of the following molecules and ions: (a) $\left(\mathrm{CH}_3\right)_3 \mathrm{SiH}$ (b) $\mathrm{SiO}_4^{4-}$ (c) $\mathrm{Si}_2 \mathrm{H}_6$ (d) $\mathrm{Si}(\mathrm{OH})_4$ (e) $\mathrm{SiF}_6$ 2-

Using only the periodic table, write the complete electron configuration for silicon, including any empty orbitals in the valence shell. You may wish to review the chapter on electronic structure.

Describe the hybridization of boron and the molecular structure about the boron in each of the following: (a) $\mathrm{H}_3 \mathrm{BPH}_3$ (b) $\mathrm{BF}_4{ }^{-}$ (c) $\mathrm{BBr}_3$ (d) $\mathrm{B}\left(\mathrm{CH}_3\right) 3$ (e) $\mathrm{B}(\mathrm{OH})_3$

Predict the formulas for the nine compounds that may form when each species in column 1 of Table below reacts with each species in column 2.

Write a Lewis structure for each of the following molecules or ions. You may wish to review the chapter on chemical bonding. (a) $\mathrm{H}_3 \mathrm{BPH}_3$ (b) $\mathrm{BF}_4^{-}$ (c) $\mathrm{BBr}_3$ (d) $\mathrm{B}\left(\mathrm{CH}_3\right)_3$ (e) $\mathrm{B}(\mathrm{OH})_3$

Give the hybridization of the metalloid and the molecular geometry for each of the following compounds or ions. You may wish to review the chapters on chemical bonding and advanced covalent bonding for relevant examples. (a) $\mathrm{GeH}_4$ (b) $\mathrm{SbF}_3$ (c) $\mathrm{Te}(\mathrm{OH}) 6$ (d) $\mathrm{H}_2 \mathrm{Te}$ (e) $\mathrm{GeF}_2$ (f) $\mathrm{TeCl}_4$ (g) $\mathrm{SiF}_6 2-$ (h) $\mathrm{SbCl}_5$ (i) $\mathrm{TeF}_6$