Electronegativity and Electron Gain Enthalpy

Q.

Among the elements H, F, Cl, Br, which is likely to have maximum electron affinity and why?

Q.

The possibility of finding an electron in an orbital was conceived by

1. Rutherford

2. Bohr

3. Heisenberg

4. Schrodinger

Q. Which of the following sets has strongest tendency to form anions?

1. Ga, Ni, Tl
2. Na, Mg, Al
3. N, O, F
4. V, Cr, Mn.

Q. What is the value of Electron gain enthalpy of $N{a}^{+}$, if $I{E}_1$ of $Na=5.1eV$ .

1. $-5.1eV$
2. $5.1eV$
3. $10.2eV$
4. $-10.2eV$

Q. Which of the following has the least negative electron gain enthalpy?

1. P
2. S
3. CI
4. F

Q. Which of the following trend is/are correct?

1. $Cl{O}_2>S{O}_2>C{O}_2>P_2{O}_5\text{(acidic nature)}$
2. $Na>Si>Al>Mg\text{(second I. P.)}$
3. $S>Se>Te>O\text{(electron affinity)}$
4. $H_{3}P{O}_2>H_{3}P{O}_3>H_{3}P{O}_4\left(K{a}_1\right)$

Q. Which of the following statements is incorrect?

1. The elements having large negative values of electron gain enthalpy generally act as strong oxidising agents
2. The elements having low values of ionisation enthalpy act as strong reducing agents
3. The formation of $S^{2-}\left(g\right)$ from $S\left(g\right)$ is an exothermic process
4. Larger is the magnitude of electron gain enthalpy, easier is the formation of anion

Q. Which of the following represents the correct order of increasing negative electron gain enthalpy for elements $O,FandCl$?

1. $Cl<F<O$
2. $O<F<Cl$
3. $F<O<Cl$
4. $O<Cl<F$

Q. Which of the following sets has strongest tendency to form anions?

1. Ga, Ni, Tl
2. Na, Mg, Al
3. N, O, F
4. V, Cr, Mn.

Q. The absolute value of the electron gain enthalpy of halogens satisfies:

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1. $Cl>Br>F>I$
2. $F>Cl>Br>I$
3. $I>Br>Cl>F$
4. $Cl>F>Br>I$

Q. The formation of oxide ion, $O^{2-}\left(g\right)$, from oxygen atom requires first an exothermic and then an endothermic step as shown below:
$O\left(g\right)+e^{-}\to O_{\left(g\right)}^{-};{}_{\Delta f}{\text{H}}^{\ominus }=-141{\text{kJ mol}}^{-1}$
$O^{-}\left(g\right)+e^{-}\to O_{\left(g\right)}^{2-};{}_{\Delta f}{\text{H}}^{\ominus }=+780{\text{kJ mol}}^{-1}$
Thus the process of formation of $O^{2-}$ in gas phase is unfavourable even thought $O^{2-}$ is isoelectric with neon. It is due to the fact that,

1. Oxygen is more electropositive
2. Addition of electron in oxygen results in larger size of the ion
3. Electron repulsion outweighs the stability gained by achieving noble gas configuration
4. $O^{-}$ ion has comparatively smaller size than oxygen atom

Q. Match the increasing orders given in column I with the property(ies) given in column II.

Column I	Column II
(A) $N{a}^{+}<F^{-}<O^{2-}<N^{3-}$	(p) electronegativity
(B) $L{i}^{+}$ < $N{a}^{+}$ < $K^{+}$ < $R{b}^{+}$ < $C{s}^{+}$	(q) Ionisation energy
(C) $O<S<F<Cl$	(r) Size
(D) $C{l}^{-}<K^{+}<C{a}^{2+}<S{c}^{3+}$	(s) Electron affinity

1. (A-r) ; (B-r) ; (C-s) ; (D-p, q, s)
2. (A-r) ; (B-r) ; (C-s) ; (D-p, q, s)
3. (A-r) ; (B-r) ; (C-s) ; (D-p, q, s)
4. (A-r) ; (B-q) ; (C-s) ; (D-p, q, s)

Q. Match the increasing orders given in column I with the property(ies) given in column II.

Column I	Column II
(A) $N{a}^{+}<F^{-}<O^{2-}<N^{3-}$	(p) electronegativity
(B) $L{i}^{+}$ < $N{a}^{+}$ < $K^{+}$ < $R{b}^{+}$ < $C{s}^{+}$	(q) Ionisation energy
(C) $O<S<F<Cl$	(r) Size
(D) $C{l}^{-}<K^{+}<C{a}^{2+}<S{c}^{3+}$	(s) Electron affinity

1. (A-r) ; (B-r) ; (C-s) ; (D-p, q, s)
2. (A-r) ; (B-r) ; (C-s) ; (D-p, q, s)
3. (A-r) ; (B-r) ; (C-s) ; (D-p, q, s)
4. (A-r) ; (B-q) ; (C-s) ; (D-p, q, s)