1. Which of the following are arranged in increasing order of solubilities?
a) \[CaCO_{3}<KHCO_{3}<NaHCO_{3}\]
b) \[NaHCO_{3}<KHCO_{3}<CaCO_{3}\]
c) \[KHCO_{3}<NaHCO_{3}<CaCO_{3}\]
d) \[CaCO_{3}<NaHCO_{3}<KHCO_{3}\]
Explanation: Lesser the lattice energy, more will be the solubility in H2O
2. Which of the following is least soluble in water?
a) \[BeSO_{4}\]
b) \[BaSO_{4}\]
c) \[CaSO_{4}\]
d) \[SrSO_{4}\]
Explanation: \[BaSO_{4}\]
3. Which of the following sulphates has highest solubility in water?
a) \[BaSO_{4}\]
b) \[CaSO_{4}\]
c) \[BeSO_{4}\]
d) \[MgSO_{4}\]
Explanation: \[BeSO_{4}\]
4. The ion having highest mobility in aqueous solution is
a) \[Be^{2+}\]
b) \[Mg^{2+}\]
c) \[Ca^{2+}\]
d) \[Ba^{2+}\]
Explanation: Ba2+ is least hydrated hence its size becomes lesser than any other hydrated alkaline earth metal cation and therefore has the highest ionic mobility.
5. Which one of the following is least soluble in water?
a) \[BaF_{2}\]
b) \[MgF_{2}\]
c) \[CaF_{2}\]
d) \[SrF_{2}\]
Explanation: As we move down the group, the lattice energies of fluorides decrease more rapidly than the hydration energy and hence the solubilities of the fluorides increase from top to bottom within a group.
6. The characteristic outer electronic configuration of alkaline earth metals is
a) \[ns^{1}\]
b) \[ns^{2}\]
c) \[ns^{2}np^{2}\]
d) \[ns^{2}np^{1}\]
Explanation: \[ns^{2}\]
7. Which of the following is strongest base?
a) \[Al\left(OH\right)_{3}\]
b) \[Mg\left(OH\right)_{2}\]
c) \[Ca\left(OH\right)_{2}\]
d) \[Ba\left(OH\right)_{2}\]
Explanation: \[Ba\left(OH\right)_{2}\]
8. As the alkaline earth metals (except Be) tend to lose their valence electrons readily, they act as
a) weak oxidising agents
b) weak reducing agents
c) strong oxidising agents
d) strong reducing agents
Explanation: Lower the I.E. or higher the negative electrode potential, stronger is the reducing agent
9. Which of the alkaline earth metals is the strongest reducing agent?
a) Ca
b) Sr
c) Ba
d) Mg
Explanation: Ba
10. The correct order of increasing ionic character is
a) \[BeCl_{2}<MgCl_{2}<CaCl_{2}<BaCl_{2}\]
b) \[BeCl_{2}<MgCl_{2}<BaCl_{2}<CaCl_{2}\]
c) \[BeCl_{2}<BaCl_{2}<MgCl_{2}<CaCl_{2}\]
d) \[BaCl_{2}<CaCl_{2}<MgCl_{2}<BeCl_{2}\]
Explanation: \[BeCl_{2}<MgCl_{2}<CaCl_{2}<BaCl_{2}\]