Magnesium oxide (MgO) has a significantly higher melting point (2,852^\circ\text{C}) than … — JAMB UTME

Magnesium oxide ( $MgO$ ) has a significantly higher melting point ( $2,852^\circ\text{C}$ ) than sodium fluoride ( $NaF$ ) ( $996^\circ\text{C}$ ) primarily because the product of the ionic charges in $MgO$ is four times greater than in $NaF$ , resulting in stronger electrostatic forces within the crystal lattice. Is this statement true or false?

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The statement is true because the strength of electrovalent bonding and lattice energy increases proportionally with the product of the ionic charges.

The statement is correct because electrovalent bond strength is governed by Coulomb's Law of electrostatic attraction. Doubly charged cations and anions (

Mg^{2+}

and

O^{2-}

) experience an electrostatic force four times stronger than singly charged ions (

Na^+

and

F^-

) of comparable size, yielding a substantially higher lattice energy and melting point.

Adım Adım Çözüm

Identify the constituent ions and their respective charges for both ionic compounds.

MgO

, the ions are

Mg^{2+}

and

O^{2-}

. In

NaF

, the ions are

Na^+

and

F^-

Electrostatic attraction depends fundamentally on the magnitude of nuclear charges transferred during ionic bond formation.

Calculate the product of the ionic charges for each compound.

For

MgO

|(+2) \times (-2)| = 4

. For

NaF

|(+1) \times (-1)| = 1

Coulomb's Law states that electrostatic force is proportional to the product of the charges (

q_1 q_2

Relate the charge product to lattice energy and physical properties such as melting point.

A higher lattice energy requires more thermal energy to break the rigid giant ionic lattice, leading to a much higher melting point for

MgO

than

NaF

Melting point directly reflects the magnitude of the electrostatic attraction holding the ions in their solid lattice positions.

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Factors Affecting Ionic Lattice Energy and Melting Points

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