Question

Arrange the following substances in order of decreasing magnitude of lattice energy. Rank the compounds in order of decreasing magnitude of lattice energy.

MgO,
CaO,
NaF,
KCl

Answer 1

Answer:MgO>CaO>NaF>KCl

Explanation:

The lattice energy is one that depend on the attraction between oppositely charged ions in a compound/substance.

Following up with this the greatest forces of attraction will exist between ions that have the smallest radii.

And, because the attraction depends on the product of the charges, we prioritize ions with the greatest charge.

The smallest pair of ions will be able to get closest to each other relative to others. This implied that the smallest distance between centres will have the largest lattice energies relative to others.

Answer 2

Arranging the chemical compounds in order of decreasing magnitude of lattice energy, we have:

MgO.

CaO.

NaF.

KCl.

Lattice energy can be defined as a measure of the energy required to dissociate one (1) mole of an ionic compound into its constituent anions and cations, in the gaseous state.

Hence, it is typically used to measure the bond strength of ionic compounds.

Generally, lattice energy is inversely proportional to the size of the ions and directly proportional to their electric charges.

Magnesium oxide (MgO) comprises the following ions:

• $Mg^{2+}$ and $O^{2-}$ (-3795 kJ/mol)

Calcium oxide (CaO) comprises the following ions:

• $Ca^{2+}$ and $O^{2-}$  (-3460 kJ/mol)

Sodium fluoride (NaF) comprises the following ions:

• $Na^+$ and $Fl^-$     (904 kJ/mol)

Potassium chloride (KCl) comprises the following ions:

• $K^+$ and $Cl^-$     (698 kJ/mol)

From the above, we can deduce that there is an increase in the charge possessed by the ionic chemical compounds and as such this would result in an increase in the lattice energy.

In order of decreasing magnitude of lattice energy, the chemical compounds are arranged as:

I. MgO.

II. CaO.

III. NaF.

IV. KCl.

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