Chapter 2

\(2.5\) Give the number of valence clectrons for each of the following elements: (a) Ga; (b) Be; (c) Cr; (d) Sn.

\(2.6\) Give the number of valence electrons for each of the following elements: (a) As; (b) \(\mathrm{V}_{\text {; (c) } \mathrm{Cl} \text {; (d) } \mathrm{Ba} \text {. }\)

2.7 Give the ground-state clectron configuration expected for cach of the following ions: (a) \(\mathrm{Sb}^{3+}\); (b) \(\mathrm{Sn}^{2+}\); (c) \(\mathrm{W}^{2+}\); (d) \(\mathrm{S}^{2-}\).

\(2.8\) Give the ground-state clectron configuration expected for each of the following ions: (a) \(\mathrm{Ga}^{+}\); (b) \(\mathrm{Tc}^{4+}\); (c) \(\mathrm{Se}^{4+}\); (d) \(\mathrm{Br}^{3+}\).

\(2.9\) Predict the ground-state clectron configuration of the following metal ions: (a) \(\mathrm{Cr}^{2+}\); (b) \(\mathrm{V}^{3+}\); (c) \(\mathrm{Zr}^{2+}\); (d) \(\mathrm{Pd}^{2}\)

2.10 Predict the ground-state clectron configuration of the following metal ions: (a) \(\mathrm{Mn}^{+} ;\)(b) \(\mathrm{Os}^{2+}\); (c) \(\mathrm{Rh}^{4}\); (d) \(\mathrm{Hg}^{2+}\).

\(2.12\) Which M ions (M = metal) are predicted to have the following ground- state clectron configurations: (a) \([A r] 3 d^{1}\); (b) [Kr] \(4 d^{10}\); (c) \([\mathrm{Kr}] 4 d^{10} 5^{2} 5 p^{2}\); (d) [Xel \(5 d^{10} 6 s^{2}\) ?

2.13 For cach of the following ground-state atoms, predict the type of orbital \((1 s, 2 p, 3 d, 4 f\), and so on) from which an electron will need to be removed to form the \(+1\) ions: (a) \(\mathrm{Zn}\); (b) \(\mathrm{Cl}\); (c) \(\mathrm{Al}\); (d) \(\mathrm{Cu}\).

2.14 For each of the following ground-state ions, predict the type of orbital \((1 s, 2 p, 3 d, 4 f\), and so on) from which an electron will need to be removed to form the ions of one greater positive charge: (a) \(\mathrm{Ti}^{2+}\); (b) \(\ln ^{+} ;\)(c) \(\mathrm{Te}^{2-} ;\) (d) \(\mathrm{Ag}^{+} .\)

Write the most likely charge for the ions formed by each element: (a) Li; (b) \(S\); (c) Ca; (d) AI.

Write the most likely charge for the ions formed by each elcment: (a) F; (b) Ba; (c) Se; (d) O.

Predict the number of valence clectrons present for cach of the following ions: (a) \(\mathrm{Sb}^{3+}\); (b) \(\mathrm{Rh}^{+}\); (c) \(\mathrm{Co}^{2+}\); (d) \(\mathrm{Ru}^{3+}\).

lodine can exist in both positive and negative oxidation states. What is the maximum (a) positive and (b) negative oxidation number that iodine may have? (c) Determine the clectron configurations for each of these states. (d) Explain how you arrived at these values.

\(2.21\) What is the ground-state clectron configuration expected for each of the folluwing ions: (a) \(B i^{34}\); (b) \(\mathrm{Sn}^{4+} ;\) (c) \(\mathrm{P}^{3-} ;\) (d) \(\mathrm{Br}^{-} ;\)(e) \(\mathrm{Ni}^{2+}\) ?

Give the ground-state electron configuration predicred for each of the following ions: (a) \(\ln ^{+}\); (b) \(\mathrm{Cu}^{+} ;\)(c) \(\mathrm{Pb}^{2+} ;\) (d) \(\mathrm{Se}^{2-}\).

\( For each of the following ground-state ions, predict the type of orbital \)(1 s, 2 p, 3 d, 4 f\(, and so on) in which the clectrons of highest energy will reside: (a) \)\mathrm{Ti}^{3+}\(; (b) \)\ln ^{4}\( (c) \)\mathrm{Te}^{2-}\(; (d) \)\mathrm{Ag}^{+}$.

For each of the following ground-state ions, predict the type of orbital \((1 s, 2 p, 3 d, 4 f\), and so on) in which the electrons of highest energy will reside: (a) \(\mathrm{Fe}^{2+}\); (b) \(\mathrm{Bi}^{3+}\); (c) \(\mathrm{As}^{3+}\); (d) \(\mathrm{Os}^{+}\).

On the basis of the expected charges on the monatomic ions, give the chemical formula of each of the following compounds: (a) magnesium arsenide; (b) indium sulfide; (c) aluminum hydride; (d) hydrogen telluride; (c) bismuth(III) fluoride.

On the basis of the expected charges on the monatomic ions, give the chemical formula of each of the following compounds: (a) sodium sulfide;(b) lithium nitride; (c) calcium chloride; (d) gallium arsenide; (c) cobalt(III) oxide.

On the basis of the expected charges on the monatomic ions, give the chemical formula of each of the following compounds: (a) gallium arsenide; (b) magnesium oxide; (c) ahuminum telluride; (d) ruthenium(IV) oxide; (c) vanadium(V) oxide.

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, \(\mathrm{NH}_{4}{\underline{\phantom{xx}}}^{*}\); (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.

Write Lewis structures, including typical contributions to the resonance structure (where appropriate, allow for the possibility of octer expansion), for (a) dihydrogen phosphate ion; (b) sulfite ion; (c) chlorate ion; (d) nitrate ion.

Which of the following species are radicals: (a) \(\mathrm{NO}\); (b) \(\mathrm{CH}_{3}^{*}\); (c) \(\mathrm{BF}_{4}\); (d) \(\mathrm{BrO}\) ?

Write the Lewis structures for the following reactive species found to contribute to the destruction of the ozone layer and indicate which are radicals: (a) chlorine monoxide, \(\mathrm{ClO}\); (b) dichloroperoxide, \(\mathrm{Cl}-\mathrm{O}-\mathrm{O}-\mathrm{Cl}\); (c) chlorine nitrate, \(\mathrm{ClONO}_{2}\) (the central \(\mathrm{O}\) atom is attached to the \(\mathrm{Cl}\) atom and to the \(\mathrm{N}\) atom of the \(\mathrm{NO}_{2}\) group); (d) chlorine peroxide, \(\mathrm{Cl}-\mathrm{O}-\mathrm{O}\).

Write Lewis structures and state the number of lone pairs on the central atom of the following compounds: (a) \(\mathrm{ClF}_{3}\) (b) AsF \(_{5} ;\) (c) \(\mathrm{SF}_{4}\).

Identify the following species as Lewis acids or Lewis bases; (a) \(\mathrm{NH}_{3}\); (b) \(\mathrm{BF}_{3}\); (c) \(\mathrm{Ag}^{*}\); (d) \(\mathrm{F}\).

Identify the following species as Lewis acids or Lewis bases: (a) \(\mathrm{H}^{+}\); (b) \(\mathrm{A}^{3+}\); (c) \(\mathrm{CN}^{-}\); (d) \(\mathrm{NO}_{2}{\underline{\phantom{xx}}}^{-}\).

Identify the Lewis acid and the Lewis base, and then write the product (a complex) for the following Lewis acid-base reactions: (a) \(\mathrm{PF}_{5}+\mathbf{F}^{-} \rightarrow\) ? (b) \(\mathrm{SO}_{2}+\mathrm{Cl}^{-} \rightarrow\) ?

Arrange the cations \(\mathrm{Rb}^{+}\), \(\mathrm{Be}^{2+}\), and \(\mathrm{Sr}^{2+}\) in order of increasing polarizing power. Give an explanation of your arrangement.

Arrange the cations \(\mathrm{K}^{+}, \mathrm{Mg}^{2+}, \mathrm{Al}^{3+}\), and \(\mathrm{Cs}^{+}\)in order of increasing polarizing power. Give an explanation of your arrangement.

Arrange the ions \(\mathrm{Cl}^{-}, \mathrm{Br}^{-}, \mathrm{N}^{3-}\), and \(\mathrm{O}^{2-}\) in order of increasing polarizability, giving reasons for your decisions.

Arrange the ions \(\mathrm{N}^{3-}, \mathrm{P}^{3-}\), 1 , and \(\mathrm{At}^{-}\)in order of increasing polarizability, giving reasons for your decisions.

For each pair, determine which compound has bonds with greater ionic character: (a) \(\mathrm{PH}_{3}\) or \(\mathrm{NH}_{3}\); (b) \(\mathrm{SO}_{2}\) or \(\mathrm{NO}_{2}\); (c) \(\mathrm{SF}_{6}\) or \(\mathrm{IF}_{5}\).

Using your knowledge of Lewis structures, predict which of the following molecules or ions of the set will have the longest indicated bond length: (a) the \(\mathrm{C}-\mathrm{O}\) bond in \(\mathrm{CO}, \mathrm{CO}_{2}\), or \(\mathrm{CO}_{3}{\underline{\phantom{xx}}}^{2}\); (b) the \(\mathrm{S}-\mathrm{O}\) bond in \(\mathrm{SO}_{2}, \mathrm{SO}_{3}\), or \(\mathrm{SO}_{3}^{2}\); (c) the \(\mathrm{C}-\mathrm{N}\) bond in \(\mathrm{HCN}\), \(\mathrm{CH}_{2} \mathrm{NH}\), or \(\mathrm{CH}_{3} \mathrm{NH}_{2}\).

Using your knowledge of Lewis structures, predict which of the following molecules of a set will have the longest indicated bond length: (a) \(\mathrm{N}-\mathrm{O}\) bond in \(\mathrm{NO}, \mathrm{NO}_{2}\), or \(\mathrm{NO}_{3}{\underline{\phantom{xx}}}^{-}\); (b) \(\mathrm{C}-\mathrm{C}\) bond in \(\mathrm{C}_{2} \mathrm{H}_{2}, \mathrm{C}_{2} \mathrm{H}_{4}\), or \(\mathrm{C}_{2} \mathrm{H}_{6}\) (c) \(\mathrm{C}-\mathrm{O}\) bond in \(\mathrm{CH}_{3} \mathrm{OH}, \mathrm{CH}_{2} \mathrm{O}\), or \(\mathrm{CH}_{3} \mathrm{OCH}_{3}\).

Sodium fluoride and sodium chloride both crystallize into the same type of structure. Which do you predict to have the higher lattice energy, NaF or \(\mathrm{NaCl}\) ?

Give the number of valence electrons for the following elements (a) Pb; (b) B; (c) Si; (d) Bi.

Which \(\mathrm{M}^{3+}\) ions \((\mathrm{M}=\) metal) are predicted to have the following ground-state electron configurations: (a) \(\mid \mathrm{Ar}] 3 d^{\prime} ;\) (b) \(\left.\mid \mathrm{Ar}\right] 3 d^{3} ;\) (c) \([K r] 4 d^{3} ;\) (d) [Kr]4d?

Which \(\mathrm{M}^{2}\) ions are predicted to have the following ground-state electron configurations: (a) \([\mathrm{Ar}] 3 d^{7} ;\) (b) \([\mathrm{Kr}] 4 d^{7} ;\) (c) \([\mathrm{Kr}] 4 d^{10} 5 s^{2} ;\) (d) [Xe] \(5 d^{10}\) ?

On the basis of the expectod charges of the monatomic ions, give the chemical formula of each of the following compounds: (a) vanadium(V) oxide; (b) lead(IV) oxide; (c) thallium(III) oxide.

On the basis of the expected charges of the monatomic ions, give the chemical formula of each of the following compoundss (a) iron(II) sulfide; (b) cobalt(III) chloride; (c) lithium phosphide.