The values of two lattice energies are given below: NaF -915 kJ mol -1 ; MgO -3933 kJ mol -1 Which of the following correct statements help to explain the difference between these two values?

Question

The values of two lattice energies are given below: NaF -915 kJ mol -1 ; MgO -3933 kJ mol -1 Which of the following correct statements help to explain the difference between these two values? (A) In each of these compounds, the ions are isoelectronic (B) The attraction between doubly charged ions is about four times than that between singly charged ions (C) The interionic distance in NaF is greater than that in MgO (D) The interionic distance in NaF is smaller than that in MgO

Tardigrade Admin · Accepted Answer

Higher magnitude of charge and smaller interionic radius of MgO are responsible for higher lattice energy.

Q. The values of two lattice energies are given below:
$N a F - 915 k J m o l^{- 1}; M g O - 3933 k J m o l^{- 1}$
Which of the following correct statements help to explain the difference between these two values?

In each of these compounds, the ions are isoelectronic

The attraction between doubly charged ions is about four times than that between singly charged ions

The interionic distance in $N a F$ is greater than that in $M g O$

The interionic distance in $N a F$ is smaller than that in $M g O$

Higher magnitude of charge and smaller interionic radius of $M g O$ are responsible for higher lattice energy.

Q. The values of two lattice energies are given below: NaF−915kJmol−1;MgO−3933kJmol−1 Which of the following correct statements help to explain the difference between these two values?