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Chapter 7: Q82 E (page 402)

Which of the following compounds requires the most energy to convert one mole of the solid into separate ions?

(a) \({\rm{MgO}}\)

(b) \({\rm{SrO}}\)

(c) \({\rm{KF}}\)

(d) \({\rm{CsF}}\)

(e) \({\rm{Mg}}{{\rm{F}}_{\rm{2}}}\)

Short Answer

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

Step by step solution

01

Concept Introduction

The lattice energy is the change of energy happening when 1 mole of a solid ionic compound forms in its gaseous state.

02

Lattice Energy of Magnesium Oxide

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.

\(MgO\) has smaller charge and \(Mg\) is smaller in size than \(Sr\). So, inter-sonic distance will be lower in \(MgO\).

Therefore, the lattice energy of \(MgO\) is greater than \(SrO\).

03

Lattice Energy of Strontium Oxide

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.\(SrO\)has larger charge but\(Sr\)is greater in size than\(Mg\). So, inter-sonic distance will be higher in\(SrO\).

Therefore, the lattice energy of \(SrO\) is less than \(MgO\).

04

Step 4: Lattice Energy of Potassium Fluoride

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\(KF\)has lower charge than\(MgO\)and\(SrO\)therefore it will not have largest lattice energy.

Therefore, the lattice energy of \(KF\) is low.

05

Lattice Energy of Caesium Fluoride

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\(CsF\)has lower charge than\(MgO\)and\(SrO\)therefore it will not have largest lattice energy.

Therefore, the lattice energy of \(CsF\) is low.

06

Lattice Energy of Magnesium Fluoride

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\({\rm{Mg}}{{\rm{F}}_{\rm{2}}}\)has lower charge than\(MgO\)and\(SrO\)therefore it will not have largest lattice energy.

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

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Most popular questions from this chapter

Question: Complete the following Lewis structure by adding bonds (not atoms), and then indicate the longest bond:

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 \({\rm{BaC}}{{\rm{l}}_{\rm{2}}}\)

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.

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) \({\rm{In}}\).

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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