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Chapter 18: Q74E (page 1045)
Write equations showing the stepwise ionization of phosphorous acid.
Phosphorous acid, \({H_3}P{O_3}\) is a diprotic acid containing two protons that can be ionised.
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Why does hydrogen not exhibit an oxidation state of -1 when bonded to nonmetals?
What is the molecular structure of each of the following molecules?
(a)\(Xe{F_2}\) (b) \({\rm{Xe}}{{\rm{F}}_{\rm{4}}}\) (c) \({\rm{Xe}}{{\rm{O}}_{\rm{3}}}\) (d) \({\rm{Xe}}{{\rm{O}}_{\rm{4}}}\) (e) \({\rm{XeO}}{{\rm{F}}_{\rm{4}}}\)
Write a Lewis structure for each of the following molecules or ions. You may wish to review the chapter on chemical bonding.
\((a)\;{{\rm{H}}_3}{\rm{BP}}{{\rm{H}}_3}\)
\((b)\;{\rm{BF}}_4^ - \)
\((c)\;{\rm{BB}}{{\rm{r}}_3}\)
\((d)\;{\rm{B}}{\left( {{\rm{C}}{{\rm{H}}_3}} \right)_3}\)
\((e)\;{\rm{B}}{({\rm{OH}})_3}\)
Carbon forms a number of allotropes, two of which are graphite and diamond. Silicon has a diamond structure. Why is there no allotrope of silicon with a graphite structure?
What is the oxidation state of the halogen in each of the following?
\(\begin{array}{l}(a){{\rm{H}}_5}{\rm{I}}{{\rm{O}}_6}\\(b){\rm{IO}}_4^ - \\(c){\rm{Cl}}{{\rm{O}}_2}\\(d){\rm{IC}}{{\rm{l}}_3}\\(e){F_2}\end{array}\)
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