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Chapter 7: Q81 E (page 402)

Which compound in each of the following pairs has the larger lattice energy? Note: \({\rm{B}}{{\rm{a}}^{{\rm{2 + }}}}\) and \({{\rm{K}}^{\rm{ + }}}\) have similar radii; \({{\rm{S}}^{{\rm{2 - }}}}\) and \({\rm{C}}{{\rm{l}}^{\rm{ - }}}\) have similar radii. Explain your choices.

(a) \({{\rm{K}}_{\rm{2}}}{\rm{O}}\) or \({\rm{N}}{{\rm{a}}_{\rm{2}}}{\rm{O}}\)

(b) \({{\rm{K}}_{\rm{2}}}{\rm{S}}\) or \({\rm{BaS}}\)

(c) \({\rm{KCl}}\) or \({\rm{BaS}}\)

(d) \({\rm{BaS}}\) or \({\rm{BaC}}{{\rm{l}}_{\rm{2}}}\)

Short Answer

Expert verified
  1. \({\rm{N}}{{\rm{a}}_{\rm{2}}}{\rm{O}}\) has greater lattice energy.
  2. \({\rm{BaS}}\) has greater lattice energy.
  3. \({\rm{BaS}}\) has greater lattice energy.
  4. \({\rm{BaS}}\) has greater lattice energy

Step by step solution

01

Concept Introduction

The energy required to dissociate the ions in a crystal lattice into individual gaseous ions is known as lattice energy.

02

Larger Lattice Energy between \({{\rm{K}}_{\rm{2}}}{\rm{O}}\) and \({\rm{N}}{{\rm{a}}_{\rm{2}}}{\rm{O}}\)

(a)

Since\({\rm{N}}{{\rm{a}}^{\rm{ + }}}\)has a smaller radius than\({{\rm{K}}^{\rm{ + }}}\).This leads to\({\rm{N}}{{\rm{a}}_{\rm{2}}}{\rm{O}}\)having larger lattice energy than\({{\rm{K}}_{\rm{2}}}{\rm{O}}\).

Therefore,\({\rm{N}}{{\rm{a}}_{\rm{2}}}{\rm{O}}\)has lattice energy than\({{\rm{K}}_{\rm{2}}}{\rm{O}}\).

03

Larger Lattice Energy between \({{\rm{K}}_{\rm{2}}}{\rm{S}}\) and \({\rm{BaS}}\)

(b)

Since there are higher charges on\({\rm{Ba}}\)than\({\rm{K}}\), whereas radii of the ions are almost similar.

Therefore, \({\rm{BaS}}\) has larger lattice energy than \({{\rm{K}}_{\rm{2}}}{\rm{S}}\).

04

Larger Lattice Energy between \({\rm{KCl}}\) and \({\rm{BaS}}\)

(c)

Since there are higher charges on \({\rm{Ba}}\) and \(S\), whereas radii of the ions are almost similar.

Therefore, \({\rm{BaS}}\) has larger lattice energy than \({\rm{KCl}}\).

05

Larger Lattice Energy between \({\rm{BaS}}\) and \({\rm{BaC}}{{\rm{l}}_{\rm{2}}}\)

(d)

Since there are higher charges on \({\rm{S}}\) than \({\rm{Cl}}\), whereas radii of the ions are almost similar.

Therefore, \({\rm{BaS}}\) has larger lattice energy than \({\rm{BaC}}{{\rm{l}}_2}\).

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Most popular questions from this chapter

The lattice energy of \({\rm{LiF}}\) is \({\rm{1023 kJ/mol}}\), and the \({\rm{Li - F}}\) distance is \({\rm{201 pm}}\). \({\rm{MgO}}\) crystallizes in the same structure as \({\rm{LiF}}\) but with a \({\rm{Mg - O}}\) distance of \({\rm{205 pm}}\). Which of the following values most closely approximates the lattice energy of \({\rm{MgO}}\): \({\rm{256 kJ/mol, 512 kJ/mol, 1023 kJ/mol, 2046 kJ/mol,}}\) or \({\rm{4008 kJ/mol}}\)? Explain your choice.

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

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)

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:

From its position in the periodic table, determine which atom in each pair is more electronegative: (a)\({\rm{Br or Cl}}\)(b)\({\rm{N or O}}\)(c)\({\rm{S or O}}\)(d)\({\rm{P or S}}\)(e)\({\rm{Si or N}}\)(f)\({\rm{Ba or P}}\)(g)\({\rm{N or K}}\).
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