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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

Question: Use principles of atomic structure to answer each of the following:

(a) The radius of the \({\rm{Ca}}\) atom is \({\rm{197 pm}}\); the radius of the \({\rm{C}}{{\rm{a}}^{{\rm{2 + }}}}\) ion is \({\rm{99 pm}}\). Account for the difference.

(b) The lattice energy of \({\rm{CaO(s)}}\) is \({\rm{ - 3460 kJ/mol}}\); the lattice energy of \({{\rm{K}}_{\rm{2}}}{\rm{O}}\) is \({\rm{ - 2240 kJ/mol}}\). Account for the difference.

(c) Given these ionization values, explain the difference between \({\rm{Ca}}\) and \({\rm{K}}\) with regard to their first and second ionization energies.

(d) The first ionization energy of \({\rm{Mg}}\) is \({\rm{738 kJ/mol}}\) and that of \({\rm{Al}}\) is \({\rm{578 kJ/mol}}\). Account for this difference.

From their positions in the periodic table, arrange the atoms in each of the following series in order of increasing electronegativity: (a)\({\rm{C, F, H, N, O}}\)(b)\({\rm{Br, Cl, F, H, I }}\)(c)\({\rm{F, H, O, P, S }}\)(d)\({\rm{Al, H, Na, O, P}}\)(e)\({\rm{Ba, H, N, O, As}}\).

Write resonance forms describing the distribution of electrons in each molecule or ion.

a) selenium dioxide, \({\rm{OSeO}}\)

(b) nitrate ion, \({\rm{NO}}_{\rm{3}}^{\rm{ - }}\)

(c) nitric acid, \({\rm{HN}}{{\rm{O}}_{\rm{3}}}\) (\({\rm{N}}\) is bonded to an \({\rm{OH}}\) group and two \({\rm{O}}\) atoms)

(d) benzene, \({{\rm{C}}_{\rm{6}}}{{\rm{H}}_{\rm{6}}}\):

(e) the formate ion:

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.

What feature of a Lewis structure can be used to tell if a molecule’s (or ion’s) electron-pair geometry and molecular structure will be identical?
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