Ionic bond - formation, factors and lattice enthalpy — NEET & JEE Questions

Question 1 · difficulty L1 · recall

An ionic bond is primarily the electrostatic attraction between

• A. oppositely charged ions
• B. two neutral atoms sharing one electron pair
• C. two nuclei with no electrons
• D. identical anions

Question 2 · difficulty L2 · understanding

The number of following factors which affect the percent covalent character of the ionic bond is _________ (A) Polarising power of cation (B) Extent of distortion of anion (C) Polarisability of the anion (D) Polarising power of anion

Question 3 · difficulty L2 · understanding

Arrange the bonds in order of increasing ionic character in the molecules. $\mathrm{LiF}$, $\mathrm{K}_2 \mathrm{O}, \mathrm{N}_2, \mathrm{SO}_2$ and $\mathrm{ClF}_3$ :

• A. $\mathrm{N}_2<\mathrm{SO}_2<\mathrm{ClF}_3<\mathrm{K}_2 \mathrm{O}<\mathrm{LiF}$
• B. $\mathrm{ClF}_3<\mathrm{N}_2<\mathrm{SO}_2<\mathrm{K}_2 \mathrm{O}<\mathrm{LiF}$
• C. $\mathrm{LiF}<\mathrm{K}_2 \mathrm{O}<\mathrm{ClF}_3<\mathrm{SO}_2<\mathrm{N}_2$
• D. $\mathrm{N}_2<\mathrm{ClF}_3<\mathrm{SO}_2<\mathrm{K}_2 \mathrm{O}<\mathrm{LiF}$

Question 4 · difficulty L2 · understanding

Formation of an ionic compound is favoured when the metal has relatively

• A. low ionisation enthalpy
• B. very high ionisation enthalpy
• C. zero tendency to lose electrons
• D. high electron affinity for gaining several electrons

Question 5 · difficulty L3 · understanding

Which of the following is least ionic?

• A. CoCl$$_2$$
• B. KCl
• C. BaCl$$_2$$
• D. AgCl

Question 6 · difficulty L3 · understanding

The correct set from the following in which both pairs are in correct order of melting point is :

• A. LiCl > LiF ; NaCl > MgO
• B. LiCl > LiF ; MgO > NaCl
• C. LiF > LiCl ; NaCl > MgO
• D. LiF > LiCl ; MgO > NaCl

Question 7 · difficulty L3 · understanding

Which one of the following represents all isoelectronic species ?

• A. $$\mathrm{Na}^{+}, \mathrm{Cl}^{-}, \mathrm{O}^{-}, \mathrm{NO}^{+}$$
• B. $$\mathrm{N}_2 \mathrm{O}, \mathrm{N}_2 \mathrm{O}_4, \mathrm{NO}^{+}, \mathrm{NO}$$
• C. $$\mathrm{Na}^{+}, \mathrm{Mg}^{2+}, \mathrm{O}^{-}, \mathrm{F}^{-}$$
• D. $$\mathrm{Ca}^{2+}, \mathrm{Ar}, \mathrm{K}^{+}, \mathrm{Cl}^{-}$$

Question 8 · difficulty L3 · application

Which pair is most likely to form a strongly ionic compound?

• A. Na and Cl
• B. C and H
• C. N and O
• D. Cl and Br

Question 9 · difficulty L4 · application

Which change generally increases the magnitude of lattice enthalpy for otherwise comparable ionic solids?

• A. Increasing ionic charges
• B. Increasing ionic radii
• C. Increasing distance between ion centres
• D. Reducing electrostatic attraction

Question 10 · difficulty L4 · application

Which compound would generally be expected to have a larger lattice enthalpy magnitude, MgO or NaCl?

• A. MgO
• B. NaCl
• C. They must be identical
• D. It cannot be compared from ionic charge