91Ó°ÊÓ

Describe the difference between ionic and covalent bonding.

Which of the following compounds are likely to have covalent bonds? (a) \(\mathrm{HF}\) (c) \(\mathrm{NCl}_{3}\) (e) \(\mathrm{CF}_{4}\) (b) \(\mathrm{NaF}\) (d) \(\mathrm{MgBr}_{2}\)

Identify the bonding in each of the following substances as ionic or covalent. (a) \(\mathrm{NaCl}\) (c) \(\mathrm{CH}_{4}\) (b) \(\mathrm{H}_{2}\) (d) \(\mathrm{SiO}_{2}\)

Which of the following compounds are likely to occur as solids at room temperature? (a) \(\mathrm{BrCl}\) (d) \(\mathrm{CaO}\) (b) \(\mathrm{CaCO}_{3}\) (e) NO (c) \(\mathrm{SO}_{2}\)

Predict whether each of the following substances is likely to have a relatively high or low boiling point. (a) \(\mathrm{TlCl}_{3}\) (d) \(\mathrm{CaO}\) (b) \(\mathrm{CsCl}\) (e) \(\mathrm{O}_{2}\) (c) \(\mathrm{CO}_{2}\)

Compare the electronegativity of metallic and nonmetallic elements.

Decide which bond in each pair is polar and explain your reasoning. Place \(\delta+\) and \(\delta\) - superscripts on the element symbols for each polar bond to indicate the direction of the polarity. (a) \(\mathrm{F}-\mathrm{F}\) and \(\mathrm{C}-\mathrm{F}\) (c) \(\mathrm{O}-\mathrm{O}\) and \(\mathrm{N}-\mathrm{O}\) (b) \(\mathrm{O}-\mathrm{H}\) and \(\mathrm{H}-\mathrm{H}\)

Draw Lewis symbols showing the valence electrons of the following atoms. (a) \(\mathrm{Kr}\) (c) \(\mathrm{F}\) (e) \(\mathrm{Ba}\) (b) \(\mathrm{Sb}\) (d) In (f) \(\mathrm{N}\)

Draw Lewis symbols showing the valence electrons of the following ions. (a) \(\mathrm{Cl}^{-}\) (c) \(\mathrm{S}^{2-}\) (e) \(\mathrm{B}^{3+}\) (b) \(\mathrm{Sc}^{3+}\) (d) \(\mathrm{Ba}^{2+}\)

Explain why \(\mathrm{K}^{+}\)is known in nature, but \(\mathrm{K}^{2+}\) is not.