Chapter 2

On the basis of the expected charges on the monatomic ions, give the chemical formula of each of the following compounds: (a) manganese(II) telluride; (b) barium arsenide; (c) silicon nitride; (d) lithium bismuthide: (c) zirconium(IV) chloride.

Write the Lewis structure of (a) \(\mathrm{SCl}_{2} ;\) (b) \(\mathrm{AsH}_{3} ;\) (c) \(\mathrm{GeCl}_{4} ;\) (d) \(\mathrm{SnCl}_{2}\).

Write the Lewis structure of (a) ammonium ion, \(\mathrm{NH}_{4}{ }^{*}\); (b) hypochlorite ion, \(\mathrm{ClO}^{-}\); (c) tetrafluoroborate ion, \(\mathrm{BF}_{4}^{-} .\)

Write the complete Lewis structure for (a) ammonium chloride; (b) potassium phosphide; (c) sodium hypochlorite

Write the complete Lewis structure for (a) zinc cyanide; (b) potassium tetrafluoroborate; (c) barium peroxide (the peroxide ion is \(\mathrm{O}_{2}^{2}\) ).

Write the complete Lewis structure for (a) formaldehyde, HCHO, which as its aqueous solution "formalin" is used to preserve biological specimens; (b) methanol, \(\mathrm{CH}_{3} \mathrm{OH}\), the toxic compound also called wood alcohol; (c) glycine, \(\mathrm{CH}_{2}\left(\mathrm{NH}_{2}\right) \mathrm{COOH}\), the simplest of the amino acids, the building blocks of protcins.

Write Lewis structures that contribute to the resonance hybrid of \(\mathrm{SO}_{2}\).

Draw Lewis structures and determine the formal charge on each atom in (a) \(\mathrm{NO}^{+}\); (b) \(\mathrm{NH}_{2}^{-}\); (c) \(\mathrm{CH}_{3}^{-}\).

Using only Lewis structures that obey the octet rule, determine the formal charge on each atom in (a) \(\mathrm{CH}_{3}^{+} ;\)(b) \(\mathrm{ClO}^{-} ;\)(c) \(\mathrm{CN}^{-}\)

Write Lewis structures, including typical contributions to the resonance structure (where appropriate, allow for the possibility of octet expansion, including double bonds in different positions), for (a) sulfite ion; (b) hydrogen sulfite ion; (c) perchlorate ion; (d) nitrite ion.