Chapter 3

The element with the highest first ionization potential is (a) boron (b) carbon (c) nitrogen (d) oxygen

The \(1^{\text {st }}, 2^{\text {nd }}\), and the \(3^{\text {rd }}\) ionization enthalpies, \(I_{1}, I_{2}\), and \(I_{3}\), of four atoms with atomic numbers \(n, n+1, n+2\), and \(n+3\), where \(n<10\), are tabulated below. What is the value of \(n ?\) $$ \begin{array}{|c|c|c|c|} \hline {\begin{array}{c} \text { Atomic } \\ \text { number } \end{array}} & & {\text { Ionization Enthalpy }(\mathrm{kJ} / \mathrm{mol})} \\\ { 2 - 4 } & I_{1} & I_{,} & I_{3} \\ \hline n & 1681 & 3374 & 6050 \\ \hline n+1 & 2081 & 3952 & 6122 \\ \hline n+2 & 496 & 4562 & 6910 \\ \hline n+3 & 738 & 1451 & 7733 \\ \hline \end{array} $$

Among the following, the number of elements showing only one nonzero oxidation state is : \(\mathrm{O}, \mathrm{Cl}, \mathrm{F}, \mathrm{N}, \mathrm{P}, \mathrm{Sn}, \mathrm{Tl}, \mathrm{Na}, \mathrm{Ti}\)

On Mulliken scale, the average of ionization potential and electron affinity is known as ..............

The energy released when an electron is added to a neutral gaseous atom is called .......... of the atom.

True/ False The basic nature of the hydroxides of group 13 (Gr. III B) decreases progressively down the group.

The decreasing order of electron affinity of \(\mathrm{F}, \mathrm{Cl}\), Br \(\mathrm{isF}>\mathrm{Cl}>\mathrm{Br}\).

The option(s) with only amphoteric oxides is(are) (a) \(\mathrm{Cr}_{2} \mathrm{O}_{3}, \mathrm{BeO}, \mathrm{SnO}, \mathrm{SnO}_{2}\) (b) \(\mathrm{Cr}_{2} \mathrm{O}_{3}, \mathrm{CrO}, \mathrm{SnO}, \mathrm{PbO}\) (c) \(\mathrm{NO}, \mathrm{B}_{2} \mathrm{O}_{3}, \mathrm{PbO}, \mathrm{SnO}_{2}\) (d) \(\mathrm{ZnO}, \mathrm{Al}_{2} \mathrm{O}_{3}, \mathrm{PbO}, \mathrm{PbO}_{2}\)

Ionic radii of (a) \(\mathrm{Ti}^{4+}<\mathrm{Mn}^{7+}\) (b) \({ }^{35} \mathrm{Cl}^{-}<{ }^{37} \mathrm{Cl}^{-}\) (c) \(\mathrm{K}^{+}>\mathrm{Cl}^{-}\) (d) \(\mathrm{P}^{3+}>\mathrm{P}^{5+}\)

Sodium sulphate is soluble in water whereas barium sulphate is sparingly soluble because : (a) the hydration energy of sodium sulphate is more than its lattice energy (b) the lattice energy of barium sulphate is more than its hydration energy (c) the lattice energy has no role to play in solubility (d) the hydration energy of sodium sulphate is less than its lattice energy.

Read the following statement and explanation and answer as per the options given below : ASSERTION : The first ionization energy of Be is greater than that of B. REASON : \(2 p\) orbital is lower in energy than \(2 s\)

Arrange the following in : (i) Arrange the following ions in order of their increasing radii: \(\mathrm{Li}^{+}\), \(\mathrm{Mg}^{2+}, \mathrm{K}^{+}, \mathrm{Al}^{3+}\) (ii) Increasing order of basic character : \(\mathrm{MgO}, \mathrm{SrO}, \mathrm{K}_{2} \mathrm{O}, \mathrm{NiO}, \mathrm{Cs}_{2} \mathrm{O}\) (iii) Increasing order of ionic size : \(\mathrm{N}^{3-}, \mathrm{Na}^{+}, \mathrm{F}^{-}, \mathrm{O}^{2-}, \mathrm{Mg}^{2+}\) (iv) Increasing size : \(\mathrm{Cl}^{-}, \mathrm{S}^{2-}, \mathrm{Ca}^{2+}, \mathrm{Ar}\) (v) Increasing first ionization potential: Mg, Al, Si, Na (vi) Increasing acidic property: \(\mathrm{ZnO}, \mathrm{Na}_{2} \mathrm{O}_{2}, \mathrm{P}_{2} \mathrm{O}_{5}, \mathrm{MgO}\) (vii) Decreasing ionic size : \(\mathrm{Mg}^{2+}, \mathrm{O}^{2-}, \mathrm{Na}^{+}, \mathrm{F}^{-}\)

The first ionization energy of carbon atom is greater than that of boron atom whereas, the reverse is true for the second ionization energy.