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Chapter 7: Q87 E (page 402)
Explain the difference between electron-pair geometry and molecular structure.
The main difference between electron-pair geometry and molecular structure is that the latter considers the bonding-pair geometry whereas the former considers placement of electrons.
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Which of the following compounds requires the most energy to convert one mole of the solid into separate ions?
(a) \({{\rm{K}}_{\rm{2}}}{\rm{S}}\)
(b) \({{\rm{K}}_{\rm{2}}}{\rm{O}}\)
(c) \({\rm{CaS}}\)
(d) \({\rm{C}}{{\rm{s}}_{\rm{2}}}{\rm{S}}\)
(e) \({\rm{CaO}}\)
Identify the atoms that correspond to each of the following electron configurations. Then, write the Lewis symbol for the common ion formed from each atom: (a)\({\text{1}}{{\text{s}}^{\text{2}}}{\text{2}}{{\text{s}}^{\text{2}}}{\text{2}}{{\text{p}}^{\text{5}}}\)(b)\({\text{1}}{{\text{s}}^{\text{2}}}{\text{2}}{{\text{s}}^{\text{2}}}{\text{2}}{{\text{p}}^{\text{6}}}{\text{3}}{{\text{s}}^{\text{2}}}\)(c)\({\text{1}}{{\text{s}}^{\text{2}}}{\text{2}}{{\text{s}}^{\text{2}}}{\text{2}}{{\text{p}}^{\text{6}}}{\text{3}}{{\text{s}}^{\text{2}}}{\text{3}}{{\text{p}}^{\text{6}}}{\text{4}}{{\text{s}}^{\text{2}}}{\text{3}}{{\text{d}}^{{\text{10}}}}\)(d)\({\text{1}}{{\text{s}}^{\text{2}}}{\text{2}}{{\text{s}}^{\text{2}}}{\text{2}}{{\text{p}}^{\text{6}}}{\text{3}}{{\text{s}}^{\text{2}}}{\text{3}}{{\text{p}}^{\text{6}}}{\text{4}}{{\text{s}}^{\text{2}}}{\text{3}}{{\text{d}}^{{\text{10}}}}{\text{4}}{{\text{p}}^{\text{4}}}\)(e)\({\text{1}}{{\text{s}}^{\text{2}}}{\text{2}}{{\text{s}}^{\text{2}}}{\text{2}}{{\text{p}}^{\text{6}}}{\text{3}}{{\text{s}}^{\text{2}}}{\text{3}}{{\text{p}}^{\text{6}}}{\text{4}}{{\text{s}}^{\text{2}}}{\text{3}}{{\text{d}}^{{\text{10}}}}{\text{4}}{{\text{p}}^{\text{1}}}\).
From its position in the periodic table, determine which atom in each pair is more electronegative: (a)\({\rm{N or P}}\)(b)\({\rm{N or Ge}}\)(c)\({\rm{S or F}}\)(d)\({\rm{Cl or S}}\)(e)\({\rm{H or C}}\)(f)\({\rm{Se or P}}\)(g)\({\rm{C or Si}}\).
Write the Lewis symbols of the ions in each of the following ionic compounds and the Lewis symbols of the atom from which they are formed: (a) \({\rm{MgS}}\) (b) \({\rm{A}}{{\rm{l}}_{\rm{2}}}{{\rm{O}}_{\rm{3}}}\) (c) \({\rm{GaC}}{{\rm{l}}_{\rm{3}}}\) (d) \({{\rm{K}}_{\rm{2}}}{\rm{O}}\) (e) \({\rm{L}}{{\rm{i}}_{\rm{3}}}{\rm{N}}\) (f) \({\rm{KF}}\) .
A molecule with the formula\({\rm{A}}{{\rm{B}}_{\rm{3}}}\), in which A and B represent different atoms, could have one of three different shapes. Sketch and name the three different shapes that this molecule might have. Give an example of a molecule or ion that has each shape.
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