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Chapter 7: Q95E (page 403)

Identify the electron pair geometry and the molecular structure of each of the following molecules:

  1. \({\rm{CNIO}}\) (N is the central atom)
  2. \({\rm{C}}{{\rm{S}}_{\rm{2}}}\)
  3. \({\rm{C}}{{\rm{l}}_{\rm{2}}}{\rm{CO}}\)(C is the central atom)
  4. \({\rm{C}}{{\rm{l}}_{\rm{2}}}{\rm{SO}}\)(S is the central atom)
  5. \({\rm{S}}{{\rm{O}}_{\rm{2}}}{\rm{\;}}{{\rm{F}}_{\rm{2}}}\)(S is the central atom)
  6. \({\rm{Xe}}{{\rm{O}}_{\rm{2}}}{\rm{\;}}{{\rm{F}}_{\rm{2}}}\)(Xe is the central atom)
  7. \({\rm{ClOF}}_{\rm{2}}^{\rm{ + }}\)(Cl is the central atom)

Short Answer

Expert verified

Electron-pair geometry considers the placement of all electrons. Molecular structure considers only the bonding-pair geometry.

Step by step solution

01

Concept Introduction

The three-dimensional arrangement of atoms in a molecule is predicted by the VSEPR theory. It takes the shape of minimum repulsion.

02

Find the electron pair geometry and the molecular structure

Therefore, the arrangement of all electrons is taken into account by electron-pair geometry. Only the bonding-pair geometry is taken into account in molecular structure calculations.

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Most popular questions from this chapter

Is the \({\rm{C}}{{\rm{l}}_{\rm{2}}}{\rm{BBC}}{{\rm{l}}_{\rm{2}}}\)molecule polar or nonpolar?

Question: Which bond in each of the following pairs of bonds is the strongest?

(a) \({\rm{C - C}}\) or \({\rm{C = C}}\)

(b) \({\rm{C - N}}\) or \({\rm{C}} \equiv {\rm{N}}\)

(c) \({\rm{C}} \equiv {\rm{O}}\) or \({\rm{C = O}}\)

(d) \({\rm{H - F}}\) or \({\rm{H - Cl}}\)

(e) \({\rm{C - H}}\) or \({\rm{O - H}}\)

(f) \({\rm{C - N}}\) or \({\rm{C - O}}\)

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)\({\text{1}}{{\text{s}}^{\text{2}}}{\text{2}}{{\text{s}}^{\text{2}}}{\text{2}}{{\text{p}}^{\text{6}}}{\text{3}}{{\text{s}}^{\text{2}}}{\text{3}}{{\text{p}}^{\text{6}}}{\text{4}}{{\text{s}}^{\text{2}}}{\text{3}}{{\text{d}}^{{\text{10}}}}{\text{4}}{{\text{p}}^{\text{1}}}\).

The lattice energy of \({\rm{KF}}\) is \({\rm{794kJ/mol}}\), and the interionic distance is \({\rm{269 pm}}\). The \({\rm{Na - F}}\) distance in \({\rm{NaF}}\), which has the same structure as \({\rm{KF}}\), is \({\rm{231 pm}}\). Which of the following values is the closest approximation of the lattice energy of \({\rm{NaF}}\): \({\rm{682 kJ/mol, 794 kJ/mol, 924 kJ/mol, 1588 kJ/mol,}}\) or \({\rm{3175 kJ/mol}}\)? Explain your answer.

(a) sulphur dioxide, \({\rm{S}}{{\rm{O}}_{\rm{2}}}\)

(b) carbonate ion, \({\rm{CO}}_{\rm{3}}^{{\rm{2 - }}}\)

(c) hydrogen carbonate ion, \({\rm{HCO}}_{\rm{3}}^{\rm{ - }}\) (\({\rm{C}}\) is bonded to an \({\rm{OH}}\) group and two \({\rm{O}}\) atoms)

(d) pyridine:

(e) the allyl ion:
See all solutions

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