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Chapter 7: Q83 E (page 402)

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) \({\rm{CaO}}\)

Short Answer

Expert verified
  1. For \(CsF\) the amount energy required to convert one mole of the solid into separate ions is lower as compared as to \({\rm{CaO}}\) and \(CsF\).
  2. For\(CsF\)the amount energy required to convert one mole of the solid into separate ions islower as compared as to\({\rm{CaO}}\)and\(CsF\).
  3. For\({\rm{CaS}}\)the amount energy required to convert one mole of the solid into separate ions islower as compared as to\({\rm{CaO}}\).
  4. For\(CsF\)the amount energy required to convert one mole of the solid into separate ions islower as compared as to\({\rm{CaO}}\)and\(CsF\).
  5. For \({\rm{CaO}}\) the amount energy required to convert one mole of the solid into separate ions will be greatest as compared to others.

Step by step solution

01

Concept Introduction

Lattice energy can be defined as the energy that is required to dissociate an ionic crystal into gaseous ion.

02

Lattice Energy of Dipotassium Mon sulphide

(a)

Lattice energy is defined as energy that is required to convert the solid into separate ions and this can be explained on the basis of inter-ionic distance as well as by magnitude of charge present on ions.

Since\({{\rm{K}}_{\rm{2}}}{\rm{S}}\)has lower charge than\({\rm{CaO}}\)and\({\rm{CaS}}\)therefore it will not have largest lattice energy.

Therefore, the lattice energy of \({{\rm{K}}_{\rm{2}}}{\rm{S}}\) is low.

03

Lattice Energy of Potassium Oxide

(b)

Lattice energy is defined as energy that is required to convert the solid into separate ions and this can be explained on the basis of inter-ionic distance as well as by magnitude of charge present on ions.

Since\({{\rm{K}}_{\rm{2}}}{\rm{O}}\)has lower charge than\({\rm{CaO}}\)and\({\rm{CaS}}\)therefore it will not have largest lattice energy.

Therefore, the lattice energy of \({{\rm{K}}_{\rm{2}}}{\rm{O}}\) is low.

04

Lattice Energy of Calcium Sulphide

(c)

Lattice energy is defined as energy that is required to convert the solid into separate ions and this can be explained on the basis of inter-ionic distance as well as by magnitude of charge present on ions. \({\rm{CaS}}\) has larger charge but \(S\) is greater in size than \(O\). So, inter-sonic distance will be higher in \({\rm{CaS}}\).

Therefore, the lattice energy of \({\rm{CaS}}\) is less than \({\rm{CaO}}\).

05

Lattice Energy of Caesium Sulphide

(d)

Lattice energy is defined as energy that is required to convert the solid into separate ions and this can be explained on the basis of inter-ionic distance as well as by magnitude of charge present on ions.

Since\({\rm{C}}{{\rm{s}}_2}S\)has lower charge than\({\rm{CaO}}\)and\({\rm{CaS}}\)therefore it will not have largest lattice energy.

Therefore, the lattice energy of \({\rm{C}}{{\rm{s}}_2}S\) is low.

06

 Step 6: Lattice Energy of Oxo calcium

(e)

Lattice energy is defined as energy that is required to convert the solid into separate ions and this can be explained on the basis of inter-ionic distance as well as by magnitude of charge present on ions.

\({\rm{CaO}}\) has smaller charge and \(O\) is smaller in size than \(S\). So, inter-sonic distance will be lower in \({\rm{CaO}}\).

Therefore, the lattice energy of \({\rm{CaO}}\) is greater than \({\rm{CaS}}\).

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Most popular questions from this chapter

Predict the charge on the monatomic ions formed from the following atoms in binary ionic compounds: (a) \({\rm{I}}\) (b) \({\rm{Sr}}\) (c) \({\rm{K}}\) (d) \({\rm{N}}\) (e) \({\rm{S}}\) (f) \({\rm{In}}\).

Which of the following molecules and ions contain polar bonds? Which of these molecules and ions have dipole moments?

  1. \({\rm{Cl}}{{\rm{F}}_{\rm{5}}}\)
  2. \({\rm{Cl}}{{\rm{O}}_{\rm{2}}}{\rm{ - }}\)
  3. \({\rm{TeC}}{{\rm{l}}_{\rm{4}}}^{{\rm{2 - }}}\)
  4. \({\rm{PC}}{{\rm{l}}_{\rm{3}}}\)
  5. \({\rm{Se}}{{\rm{F}}_{\rm{4}}}\)
  6. \({\rm{P}}{{\rm{H}}_{\rm{2}}}^{\rm{ - }}\)
  7. \({\rm{Xe}}{{\rm{F}}_{\rm{2}}}\)

Question: Using the standard enthalpy of formation data in Appendix G, show how the standard enthalpy of formation of \({\rm{HCl(g)}}\) can be used to determine the bond energy.

Predict which of the following compounds are ionic and which are covalent, based on the location of their constituent atoms in the periodic table:

(a) \({\rm{C}}{{\rm{l}}_{\rm{2}}}{\rm{CO}}\) (b) \({\rm{MnO}}\) (c) \({\rm{NC}}{{\rm{l}}_{\rm{3}}}\) (d) \({\rm{CoB}}{{\rm{r}}_{\rm{2}}}\) (e) \({{\rm{K}}_{\rm{2}}}{\rm{S}}\) (f) \({\rm{CO}}\) (g) \({\rm{Ca}}{{\rm{F}}_{\rm{2}}}\) (h) \({\rm{HI}}\) (i) \({\rm{CaO}}\) (j) \({\rm{IBr}}\) (k) \({\rm{C}}{{\rm{O}}_{\rm{2}}}\) .

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)
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