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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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Which halogen has the highest ionization energy? Is this what you would predict based on what you have learned about periodic properties?
Explain why, at room temperature, fluorine and chlorine are gases, bromine is a liquid, and iodine is a solid.
Nitrogen in the atmosphere exists as very stable diatomic molecules. Why does phosphorus form less stable \({{\bf{P}}_4}\)molecules instead of \({{\bf{P}}_2}\)molecules?
Determine the oxidation state of sulfur in\({\rm{S}}{{\rm{F}}_6},{\rm{S}}{{\rm{O}}_2}\;{{\rm{F}}_2}\), and KHS.
Give the hybridization of the metalloid and the molecular geometry for each of the following compounds or ions. You may wish to review the chapters on chemical bonding and advanced covalent bonding for relevant examples.
\((a){\rm{Ge}}{{\rm{H}}_4}\)
\((b){\rm{Sb}}{{\rm{F}}_3}\)
\((c){\rm{Te}}{({\rm{OH}})_6}\)
\((d){{\rm{H}}_2}{\rm{Te}}\)
\((e){\rm{Ge}}{{\rm{F}}_2}\)
\((f){\rm{TeC}}{{\rm{l}}_4}\)
\((g){\rm{SiF}}_6^{2 - }\)
\((h){\rm{SbC}}{{\rm{l}}_5}\)
\((i){\rm{Te}}{{\rm{F}}_6}\)
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