Chapter Questions
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(a) Are the covalences and group numbers (numbers of valence electrons) of the elements in Table 1-1 related? $(b)$ Do all the elements in Table $1-1$ attain an octet of valence electrons in their bonded states? (c) Why aren't Group I elements included in Table 1-1?
Write structural and condensed formulas for (a) three isomers with molecular formula $\mathrm{C}_5 \mathrm{H}_{12}$ and $(b)$ two isomers with molecular formula $\mathrm{C}_3 \mathrm{H}_6$.
Write Lewis structures for (a) hydrazine, $\mathrm{N}_2 \mathrm{H}_4 ;(b)$ phosgene, $\mathrm{COCl}_2 ;(c)$ nitrous acid, $\mathrm{HNO}_2$.
Why is none of the following Lewis structures for $\mathrm{COCl}_2$ correct?(Figure can't copy)
Use the Lewis-Langmuir octet rule to write Lewis electron-dot structures for: (a) $\mathrm{HCN},(b), \mathrm{CO}_2$, (c) $\mathrm{CCl}_4$ and (d) $\mathrm{C}_2 \mathrm{H}_6 \mathrm{O}$.
Determine the positive or negative charge, if any, on:(Figure can't copy)
Each of the following molecules and ions can be thought to arise by coordinate covalent bonding. Write an equation for the formation of each one and indicate the donor and acceptor molecule or ion. (a) $\mathrm{NH}_4^{+}(b)$ $\mathrm{BF}_4^{-}(c)\left(\mathrm{CH}_3\right)_2 \mathrm{OMgCl}_2(d) \mathrm{Fe}(\mathrm{CO})_5$
Show how the ionic compound $\mathrm{Li}^{+} \mathrm{F}^{-}$forms from atoms of $\mathrm{Li}$ and $\mathrm{F}$.
Methane, $\mathrm{CH}_4$; ethane, $\mathrm{C}_2 \mathrm{H}_6$; and propane, $\mathrm{C}_3 \mathrm{H}_8$ are the first three members of the alkane homologous series. By what structural unit does each member differ from its predecessor?
(a) Write possible Lewis structural formulas for (1) $\mathrm{CH}_4 \mathrm{O} ;$ (2) $\mathrm{CH}_2 \mathrm{O}$; (3) $\mathrm{CH}_2 \mathrm{O}_2$; (4) $\mathrm{CH}_5 \mathrm{~N}$; (5) $\mathrm{CH}_3 \mathrm{SH}$. (b) Indicate and name the functional group in each case.
Determine the formal charge on each atom in the following species: (a) $\mathrm{H}_3 \mathrm{NBF}_3$ : (b) $\mathrm{CH}_3 \mathrm{NH}_3^{+}$; and (c) $\mathrm{SO}_4^{2-}$.
Show how $(a) \mathrm{H}_3 \mathrm{NBF}_3$ and $(h) \mathrm{CH}_3 \mathrm{NH}_3^{+}$can be formed from coordinate covalent bonding. Indicate the donor and acceptor, and show the formal charges.
Why are the compounds of carbon covalent rather than ionic?
Classify the following as (i) branched chain, (ii) unbranched chain, (iii) cyclic, (iv) multiple bonded, or (v) heterocyclic:(Figure can't copy)
Refer to a Periodic Chart and predict the covalences of the following in their hydrogen compounds: (a) $\mathrm{O}$; (b) $\mathrm{S}$; (c) $\mathrm{Cl} ;(d) \mathrm{C} ;(e) \mathrm{Si} ;(f) \mathrm{P} ;(g) \mathrm{Ge} ;(h) \mathrm{Br} ;(i) \mathrm{N} ;(j) \mathrm{Se}$.
Which of the following are isomers of 2-hexene, $\mathrm{CH}_3 \mathrm{CH}=\mathrm{CHCH}_2 \mathrm{CH}_2 \mathrm{CH}_3$ ?(a) $\mathrm{CH}_3 \mathrm{CH}_2 \mathrm{CH}=\mathrm{CHCH}_2 \mathrm{CH}_3$(b) $\mathrm{CH}_2=\mathrm{CHCH}_2 \mathrm{CH}_2 \mathrm{CH}_2 \mathrm{CH}_3$(c) $\mathrm{CH}_3 \mathrm{CH}_2 \mathrm{CH}_2 \mathrm{CH}=\mathrm{CHCH}_3$(Figure can't copy)
Find the formal charge on each element of(Figure can't copy)and the net charge on the species $\left(\mathrm{BF}_3 \mathrm{Ar}\right)$.
Write Lewis structures for the nine isomers having the molecular formula $\mathrm{C}_3 \mathrm{H}_6 \mathrm{O}$, in which $\mathrm{C}, \mathrm{H}$, and $\mathrm{O}$ have their usual covalences; name the functional group(s) present in each isomer.