Ionization Energy and Electron Affinity

Q.

The element with lowest ionization energy among the following is:

1. Rb

2. Na

3. Li

4. K

Q. The energy associated with the second orbit of Li2+ is (Ionisation energy of H atom is 2.18 × 10–18 J/atom)

Q. 50.In the plot of ionisation enthalpy versus atomic number peaks are occupied by

Q. Atoms of the which of the following groups possess the lowest ionization energy

1. I A
2. II A
3. III A
4. Zero

Q.

Among group 15 elements, the one having a negative electron affinity is:

1. Nitrogen

2. Phosphorus

3. Antimony

4. Bismuth

Q.

Which element acts as strong reducing agent?

1. Those elements that can share electron

2. he elements which readily lose electron

3. The elements which readily gain electron

4. None of these

Q. Ionization potential and electron affinity of fluorine are $17.42$ and $3.45eV$ respectively. The electronegativity of fluorine on Mulliken scale and Pauling scale is $x$ & $y$ respectively, then $\frac{(x+y)}{1.011}$is:

1. 12
2. 13
3. 14
4. 15

Q. Fill in the blank
Formation of a compound through ionic bond _____ the ionization energy of the metal ion.

1. Does not depends on
2. Is independent regarding
3. May or may not depend on
4. Depend on

Q. The first and the second ionisation energies of magnesium are 7.646 eV and 15.035 eV respectively. The amount of energy in kJ needed to convert all the atoms of magnesium into $M{g}^{2+}$ ions present in 24 mg of magnesium vapour will be:
(Given $1eV=96.5kJmo{l}^{–1}$).

1. $2.455kJ$
2. $2.188kJ$
3. $1.094kJ$
4. $4.370kJ$

Q. Peroxide and superoxide ions are, respectively:

1. diamagnetic and diamagnetic
2. paramagnetic and paramagnetic
3. diamagnetic and paramagnetic
4. paramagnetic and diamagnetic

Q. The amount of energy released when a million atoms of iodine are completely converted into $I^{–}$ ions in the vapour state according to the equation, $I\left(g\right)+e^{–}\to I^{–}\left(g\right)$ is $5.0\times {10}^{–13}$ J.
Calculate the electron gain enthalpy of iodine in terms of $kJmo{l}^{–1}$.

1. $-150.5kJ/mol$
2. $-301kJ/mol$
3. $-602kJ/mol$
4. $-30.1kJ/mol$

Q. The correct order of negative electron gain enthalpy of the given elements is

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