Ionic Solids and Lattice Enthalpy

. Identify the correct order of standard enthalpy of formation of sodium halides.

What is an ionic compound.

Ionic compounds are exists as _____.

Write the formation of magnesium chloride (${\mathrm{MgCl}}_2$) with the help of electron dot structure.

Ionic compounds in solid state do not conduct electricity, but in molten state are good conductors of electricity. Why?

The crystalline structure of $\mathrm{NaCl}$ is body centered cubic.

How many ${\mathrm{Cl}}^{-}$ ions surround ${\mathrm{Na}}^{+}$ in the crystal lattice of $\mathrm{NaCl}$.

Discuss the crystal structure of sodium chloride.

Electron gain enthalpy affects in the formation of an ionic bond. Explain.

Explain the role of electron gain enthalpy in the formation of an ionic bond.

What is the necessary condition for the formation of an ionic bond?

Ionisation energy is the necessary condition for the formation of an ionic bond. Justify.

How size can affect the tendency to remove the electron?

More the size of a metal atom, easier is to remove the electron. Justify.

Discuss the crystal structure of sodium chloride.

The ions in a solid ionic compound are randomly arranged.

Define ionic compounds.

What are the necessary conditions for the formation an ionic bond.

When sodium and fluorine react to form sodium fluoride, which of the following processor occur?

$\left(\mathrm{i}\right)$ Sodium atom loses valence electrons

$\left(\mathrm{ii}\right)$ Fluorine atom loses electrons

$\left(\mathrm{iii}\right)$ Fluorine atom gains electron

$\left(\mathrm{iv}\right)$ Sodium atom gains electron