Question

Consider the following statements and arrange in the order of true/ false as given in the codes.
$S_1:N{a}_2{O}_2<MgO<ZnO<P_4{O}_{10}$: Acidic property.
$S_2$: Na < Si < Mg < Al: First ionisation energy.
$S_3$: F > Cl > Br : Electron affinity.

• A. TTT
• B. TTF
• C. TFF
• D. TFT

Answer 1

Answer: (C)

TFF

$S_1:N{a}_2{O}_2<MgO<ZnO<P_4{O}_{10}:$ as non-metallic character increases the acidic character increases, $MgO,N{a}_{2}O$ are basic, ZnO amphoteric and $P_4{O}_{10}$ acidic.

$S_2$: Mg has a higher first ionization energy than Na due to a small size and higher nuclear charge. Mg has higher than Al because of $n{s}^2$ configuration (has extra stability and high electron penetration power of s-subshell electrons) and Si has higher than Al because of higher nuclear charge and small size. $I{E}_1:Na=496,Al=577,Mg=737$ and Si=786 kJ/mole.

$S_3$: There is more interelectronic repulsion in 2p-subshell of fluorine than chlorine (3p). So extra electron will be added easily in 3p-subshell of chlorine as compared to 2p-subshell of fluorine. Down the group electron affinity values generally decreases with increasing atomic number due to increase in atomic size. So $Cl>F>Br$.