Chapter 12

The element with atomic number 12 belongs to ......... group and .......... period. (a) IA, third (b) IIIA third (c) IIA, third (d) IIA, second

An element having atomic number 56 belongs to (a) lanthanides (b) actinides (c) alkaline earth metals (d) none of these

The maximum valency of an element having atomic number seven is (a) 1 (b) 3 (c) 5 (d) 7

The number of elements present in the fifth period of periodic table is (a) 10 (b) 8 (c) 32 (d) 18

An example of amphoteric oxide is (a) \(\mathrm{Ti}_{2} \mathrm{O}_{2}\) (b) \(\mathrm{MgO}\) (c) \(\mathrm{Cl}_{2} \mathrm{O}_{7}\) (d) \(\mathrm{Al}_{2} \mathrm{O}_{3}\)

The elements with atomic numbers \(9,17,35,53\) and 85 (a) noble gases (b) light metals (c) halogens (d) heavy metals

Which one of the following is a metalloid? (a) phosphorus (b) antimony (c) nitrogen (d) bismuth

The correct order of atomic radii is (a) \(\mathrm{F}<\mathrm{K}<\mathrm{Na}<\mathrm{Li}\) (b) \(\mathrm{Li}<\mathrm{Na}<\mathrm{K}<\mathrm{F}\) (c) \(\mathrm{F}<\mathrm{Li}<\mathrm{Na}<\mathrm{K}\) (d) \(\mathrm{Na}<\mathrm{K}<\mathrm{Li}<\mathrm{F}\)

Ionic radii are (a) inversely proportional to effective nuclear charge (b) inversely proportional to square of effective nuclear charge (c) directly proportional to effective nuclear charge (d) directly proportional to square of effective nuclear charge

Which of the following oxides is most basic? (a) \(\mathrm{Bi}_{2} \mathrm{O}_{3}\) (b) \(\mathrm{SeO}_{2}\) (c) \(\mathrm{Al}_{2} \mathrm{O}_{3}\) (d) \(\mathrm{Sb}_{2} \mathrm{O}_{3}\)

The outermost configuration of the most electronegative elements is (a) \(\mathrm{ns}^{2} \mathrm{np}^{3}\) (b) \(\mathrm{ns}^{2} \mathrm{np}^{6}\) (c) \(\mathrm{ns}^{2} \mathrm{np}^{4}\) (d) \(\mathrm{ns}^{2} \mathrm{np}^{3}\)

Which of the following is the atomic number of a metal? (a) 32 (b) 34 (c) 36 (d) 38

Which of the following has maximum ionization potential? (a) \(\mathrm{Al}\) (b) \(\mathrm{P}\) (c) Si (d) \(\mathrm{Mg}\)

The first ionization potential will be maximum for (a) uranium (b) iron (c) hydrogen (d) lithium

The most acidic oxide is (a) \(\mathrm{MgO}\) (b) \(\mathrm{CaO}\) (c) \(\mathrm{Na}_{2} \mathrm{O}\) (d) \(\mathrm{Al}_{2} \mathrm{O}_{3}\)

The atomic radius decreases in a period due to (a) increase in nuclear attraction (b) decrease in nuclear attraction (c) increase in number of electrons (d) decrease in number of electrons

The correct order of decreasing first ionization potential is (a) \(\mathrm{Ca}>\mathrm{K}>\mathrm{Rb}>\mathrm{Cs}\) (b) \(\mathrm{Cs}>\mathrm{Rb}>\mathrm{K}>\mathrm{Ca}\) (c) \(\mathrm{Ca}>\mathrm{Cs}>\mathrm{Rb}>\mathrm{K}\) (d) \(\mathrm{K}>\mathrm{Rb}>\mathrm{Cs}>\mathrm{Ca}\)

The electron affinity of Be is similar to (a) \(\mathrm{He}\) (b) B (c) \(\mathrm{Li}\) (d) \(\mathrm{Na}\)

Which one of the following represents the correct order of electronegativity? (a) \(\mathrm{P}>\mathrm{O}>\mathrm{N}\) (b) \(\mathrm{N}>\mathrm{P}>\mathrm{O}\) (c) \(\mathrm{O}>\mathrm{N}>\mathrm{P}\) (d) \(\mathrm{N}>\mathrm{O}>\mathrm{P}\)

The transition metal with least atomic number is (a) Os (b) \(\mathrm{Zr}\) (c) \(\mathrm{Pt}\) (d) \(\mathrm{Ru}\)

Correct order of radii is (a) \(\mathrm{Na}<\mathrm{Li}<\mathrm{K}\) (b) \(\mathrm{N}<\mathrm{Be}<\mathrm{B}\) (c) \(\mathrm{Cf}<\mathrm{S}^{2-}<\mathrm{P}^{3-}\) (d) \(\mathrm{Fe}^{3+}<\mathrm{Fe}^{2+}<\mathrm{Fe}^{4+}\)

The element having highest electron affinity is (a) bromine (b) iodine (c) fluorine (d) chlorine

Which of the following is a favourable factor for cation formation? (a) high electron affinity (b) high electronegativity (c) small atomic size (d) low ionization potential

The order of first ionization energies of the elements \(\mathrm{Li}, \mathrm{Be}, \mathrm{B}, \mathrm{Na}\) is (a) \(\mathrm{Be}>\mathrm{Li}>\mathrm{B}>\mathrm{Na}\) (b) \(\mathrm{B}>\mathrm{Be}>\mathrm{Li}>\mathrm{Na}\) (c) \(\mathrm{Na}>\mathrm{Li}>\mathrm{B}>\mathrm{Be}\) (d) \(\mathrm{Be}>\mathrm{B}>\mathrm{Li}>\mathrm{Na}\)

Which of the following is an inert gas? (a) \(\mathrm{O}_{2}\) (b) argon (c) \(\mathrm{N}_{2}\) (d) \(\mathrm{H}_{2}\)

The outermost electronic configuration of the most electronegative element is (a) \(\mathrm{ns}^{2} \mathrm{np}^{3}\) (b) \(\mathrm{ns}^{2} \mathrm{np}^{4}\) (c) \(\mathrm{ns}^{2} \mathrm{np}^{5}\) (d) \(\mathrm{ns}^{2} \mathrm{np}^{6}\)

Which one of the following hydroxides is insoluble in water? (a) \(\mathrm{Ca}(\mathrm{OH})_{2}\) (b) \(\mathrm{Ba}(\mathrm{OH})_{2}\) (c) \(\mathrm{Mg}(\mathrm{OH})_{2}\) (d) \(\mathrm{Sr}(\mathrm{OH})_{2}\)

The electronic configuration of four different elements is given below. Identify the group IV element among these. (a) \([\mathrm{He}] 2 \mathrm{~s}^{1}\) (b) \([\mathrm{Ne}] 3 \mathrm{~s}^{2}\) (c) \([\mathrm{Ne}] 3 \mathrm{~s}^{2} 3 \mathrm{p}^{2}\) (d) \([\mathrm{Ne}] 3 \mathrm{~s}^{2} 3 \mathrm{p}^{5}\)

An atom has electronic configuration: Is \(2 \mathrm{~s}^{2} 2 \mathrm{p}^{6} 3 \mathrm{~s}^{2}\) \(3 \mathrm{p}^{6} 3 \mathrm{~d}^{3} 4 \mathrm{~s}^{2}\), you will place it in (a) \(\mathrm{V}\) group (b) \(\mathrm{XV}\) group (c) II group (d) III group

Sodium forms \(\mathrm{Na}^{+}\)ion but it does not form \(\mathrm{Na}^{2+}\) be cause of (a) very low value of (IE), and (IE), (b) very high value of \((\mathrm{IE})\), and \((\mathrm{IE})_{2}\) (c) low value of (IE), and low value of \((\mathrm{IE})_{2}\) (d) low value of (IE), and high value of (IE) \(_{2}\)

Which of the electronic configuration represents a noble gas? (a) \(1 \mathrm{~s}^{2}, 2 \mathrm{~s}^{2}, 2 \mathrm{p}^{6}, 3 \mathrm{~s}^{2}, 3 \mathrm{p}^{6}\) (b) \(1 \mathrm{~s}^{2}, 2 \mathrm{~s}^{2}, 2 \mathrm{p}^{6}, 3 \mathrm{~s}^{2}, 3 \mathrm{p}^{3}\) (c) \(1 \mathrm{~s}^{2}, 2 \mathrm{~s}^{2}, 2 \mathrm{p}^{6}, 3 \mathrm{~s}^{2}, 3 \mathrm{p}^{1}\) (d) \(1 \mathrm{~s}^{2}, 2 \mathrm{~s}^{2}, 2 \mathrm{p}^{6}, 3 \mathrm{~s}^{2}, 3 \mathrm{p}^{4}\)

Ionic radius (in A) of \(\mathrm{As}^{3+}, \mathrm{Sb}^{3+}\) and \(\mathrm{Bi}^{3+}\) follow the order (a) \(\mathrm{As}^{3+}>\mathrm{Sb}^{3+}>\mathrm{Bi}^{3+}\) (b) \(\mathrm{Sb}^{3+}>\mathrm{Bi}^{3+}>\mathrm{As}^{3+}\) (c) \(\mathrm{Bi}^{3+}>\mathrm{As}^{3+}>\mathrm{Sb}^{3+}\) (d) \(\mathrm{Bi}^{3+}>\mathrm{Sh}^{3+}>\mathrm{As}^{3+}\)

Identify the least stable ion amongst the following: (a) Li- (b) \(\mathrm{Be}^{-}\) (c) B- (d) \(\mathrm{C}-\)

The set representing the correct order of first ionization potential is (a) \(\mathrm{K}>\mathrm{Na}>\mathrm{Li}\) (b) \(\mathrm{Br}>\mathrm{Mg}>\mathrm{Ca}\) (c) \(\mathrm{B}>\mathrm{C}>\mathrm{N}\) (d) Ge \(>\mathrm{Si}>\mathrm{C}\)

General electronic configuration of lanthanides is (a) \((\mathrm{n}-2) \mathrm{f}^{1-14}(\mathrm{n}-1) \mathrm{s}^{2} \mathrm{p}^{6} \mathrm{~d}^{0-1} \mathrm{~ns}^{2}\) (b) \((\mathrm{n}-2) \mathrm{f}^{0-14}(\mathrm{n}-1) \mathrm{d}^{0-1} \mathrm{~ns}^{2}\) (c) \((\mathrm{n}-2) \mathrm{f}^{0-14}(\mathrm{n}-1) \mathrm{d}^{10} \mathrm{~ns}^{2}\) (d) \((n-2) f^{0-1}(n-1) f^{1-14} n s^{2}\)

Property of alkaline earth metals that increases with their atomic number is (a) ionization energy (b) solubility of their hydroxides (c) solubility of their sulphates (d) electronegativity

With reference to the concept of ionization energy, which one of the following set is correct? (a) \(\mathrm{Cs}>\mathrm{U}>\mathrm{B}\) (b) \(\mathrm{U}>\mathrm{K}>\mathrm{Cs}\) (c) \(\mathrm{Cs}<\mathrm{U}<\mathrm{K}\) (d) \(\mathrm{B}>\mathrm{U}>\mathrm{K}\)

For electron affinity of halogens which of the following is correct? (a) \(\mathrm{F}>\mathrm{I}\) (b) \(\mathrm{F}>\mathrm{CI}\) (c) \(\mathrm{Br}>\mathrm{Cl}\) (d) \(\mathrm{Br}>\mathrm{F}\)

The electronic configuration of the most electronegative element is (a) \(1 \mathrm{~s}^{2}, 2 \mathrm{~s}^{2}, 2 \mathrm{p}^{5}\) (b) \(\mathrm{Is}^{2}, 2 \mathrm{~s}^{2}, 2 \mathrm{p}^{4}, 3 \mathrm{~s}^{1}\) (c) \(1 \mathrm{~s}^{2}, 2 \mathrm{~s}^{2}, 2 \mathrm{p}^{6}, 3 \mathrm{~s}^{1}, 3 \mathrm{p}^{5}\) (d) \(1 \mathrm{~s}^{2}, 2 \mathrm{~s}^{2}, 2 \mathrm{p}^{6}, 3 \mathrm{~s}^{2}, 3 \mathrm{p}^{5}\)

Let electronegativity, ionization energy and electronicaffinity be represented as EN, IP and EA respectively. Which one of the following equation is correct according to Mulliken? (a) \(\mathrm{EN}=\mathrm{IP} \times \mathrm{EA}\) (b) \(\mathrm{EN}=\mathrm{IP} / \mathrm{EA}\) (c) \(\mathrm{EN}=\frac{\mathrm{IP}+\mathrm{EA}}{2}\) (d) \(\mathrm{EN}=\mathrm{IP}-\mathrm{EA}\)

Which of the following order is correct for the size of \(\mathrm{Fe}^{3+}, \mathrm{Fe}\) and \(\mathrm{Fe}^{2+} ?\) (a) \(\mathrm{Fe}<\mathrm{Fe}^{2+}<\mathrm{Fe}^{3+}\) (b) \(\mathrm{Fe}^{2+}<\mathrm{Fe}^{3+}<\mathrm{Fe}\) (c) \(\mathrm{Fe}<\mathrm{Fe}^{3+}<\mathrm{Fe}^{2+}\) (d) \(\mathrm{Fe}^{3+}<\mathrm{Fe}^{2+}<\mathrm{Fe}\)

In the following, the element with the highest ionization energy is (a) \([\mathrm{Ne}] 3 \mathrm{~s}^{2} 3 \mathrm{p}^{1}\) (b) \([\mathrm{Ne}] 3 \mathrm{~s}^{2} 3 \mathrm{p}^{3}\) (c) \([\mathrm{Ne}] 3 \mathrm{~s}^{2} 3 \mathrm{p}^{2}\) (d) \([\mathrm{Ne}] 3 \mathrm{~s}^{2} 3 \mathrm{p} 4\)

Property of alkaline earth metals that increases with their atomic number is (a) ionization energy (b) solubility of their hydroxides (c) solubility of their sulphates (d) electronegativity

Which corresponds to the most electropositive character? (a) \([\mathrm{Xe}] 6 \mathrm{~s}^{1}\) (b) \([\mathrm{Xe}] 6 \mathrm{~s}^{2}\) (c) \([\mathrm{He}] 2 \mathrm{~s}^{1}\) (d) \([\mathrm{He}] 2 \mathrm{~s}^{1}\)

Arrange \(\mathrm{S}, \mathrm{O}\) and Se in the ascending order of electron affinity. (a) \(\mathrm{S}<\mathrm{Se}<\mathrm{O}\) (b) \(\mathrm{Se}<\mathrm{O}<\mathrm{S}\) (c) \(\mathrm{Se}<\mathrm{S}<\mathrm{O}\) (d) \(\mathrm{S}<\mathrm{O}<\mathrm{Se}\)

Let IP stand for ionization potential. Then element for which the value of \(\mathrm{IP}_{1}, \mathrm{IP}_{2}, \mathrm{IP}_{3}, \mathrm{IP}_{4}\) are \(50,100,250\) and \(2051 \mathrm{eV}\) respectively, is (a) \(\mathrm{Al}\) (b) \(\mathrm{Na}\) (c) \(\mathrm{Mg}\) (d) \(\mathrm{Si}\)

The correct order of electronegativity for \(\mathrm{O}, \mathrm{O}^{+}\)and \(\mathrm{O}^{-}\)is (a) \(\mathrm{O}^{-}>\mathrm{O}>\mathrm{O}^{+}\) (b) \(\mathrm{O}>\mathrm{O}^{+}>\mathrm{O}^{-}\) (c) \(\mathrm{O}^{+}>\mathrm{O}^{->} \mathrm{O}\) (d) \(\mathrm{O}^{+}>\mathrm{O}>\mathrm{O}^{-}\)

Which of the following statements is true about effective nuclear charge? (a) \(\mathrm{Z}_{\text {eff }}\) decreases from top to bottom (b) \(\mathrm{Z}_{\text {eff }}\) increases from top to bottom (c) \(Z_{\text {eff }}\) increases as we move from left to right in periodic table (d) \(Z_{e f f}=Z \times \sigma\) (here \(\sigma\) is screening constant)

The ionization potential of \(\mathrm{K}^{+}\)is \(2.4 \mathrm{eV}\). The electron affinity of \(\mathrm{K}^{+}\)will be (a) \(1.2 \mathrm{eV}\) (b) \(2.4 \mathrm{eV}\) (c) \(4.2 \mathrm{eV}\) (d) \(8.4 \mathrm{eV}\)

Let IP stand for ionization potential. The IP, and \(\mathrm{IP}_{2}\) of \(\mathrm{Mg}\) are 178 and \(348 \mathrm{kcal} \mathrm{mol}^{-1} .\) The energy required for the following reaction is \(\mathrm{Mg} \longrightarrow \mathrm{Mg}^{2+}+2 \mathrm{e}-\) (a) \(+178 \mathrm{kcal}\) (b) \(+526 \mathrm{kcal}\) (c) \(-170 \mathrm{kcal}\) (d) \(-526 \mathrm{kcal}\)