Which is the correct order of ionization energies?

1. F^-> F >Cl^->Cl

2. F >Cl>Cl^-> F^-

3. F^->Cl^->Cl> F

4. F^->Cl^-> F >Cl

The atomic radii of the elements across the second period of the periodic table

1. Decrease due to increase in atomic number

2. Decrease due to increase in effective nuclear charge 

3. Decrease due to increase in atomic wights 

4. increase due to increase in the effective nulear charge

The radii of the first bohr orbit of H(r_H), He⁺ (r_He⁺) and Li2+(r_Li²⁺) are in the order:

1.  r_H = r_He⁺ = r_Li⁺²

2.  r_H < r_He⁺ < r_Li²⁺

3.  r_H > r_He⁺ > r_Li²⁺

4.  r_He⁺ < r_H < r_Li²⁺

The first ionization enthalpies for three elements are 1314, 1680, and 2080 kJ $mo{l}^{-1}$ respectively. These elements are:

1. O, F and Ne

2. F, O and Ne

3. Ne, F and O

4. F, Ne and O

The electronic configuration of an element with the largest difference between the $1^{\mathrm{st} }\mathrm{and} 2^{\mathrm{nd}}$ ionization energies is

1.  $1s^2 2s^2 2p^6$

2.  $1s^2 2s^2 2p^6 3s^1$

3.  $1s^2 2s^2 2p^{6}3s^2$

4.  $1s^2 2s^2 2p^1$

Among the elements Li, N, C and Be, one with the largest atomic radius is

1.  Li

2.  N

3.  C

4.  Be

The first ionisation energy of Na, B, N and O atoms follows the order 

1.  B < Na < O < N

2.  Na < B < O < N

3.  Na < O < B < N

4.  O < Na < N < B

Among ${\mathrm{P}}_2{\mathrm{O}}_5, {\mathrm{As}}_2{\mathrm{O}}_3, {\mathrm{Sb}}_2{\mathrm{O}}_3 \mathrm{and} {\mathrm{Bi}}_2{\mathrm{O}}_3$, the most acidic oxide is:

1.  $P_2{O}_5$

2.  $A{s}_2{O}_3$

3.  $S{b}_2{O}_3$

4.  $B{i}_2{O}_3$

The first four ionization energy values of metal are 191, 587, 872 and 5962 kcal/mol respectively. The number of valence electrons in the element is

1.  1

2.  2

3.  3

4.  5

The outermost electronic configuration of the most electronegative element is 

1.  $n{s}^2, n{p}^3$

2.  $n{s}^2, n{p}^6\left(n-1\right)d^5$

3.  $n{s}^2, n{p}^5$

4.  $n{s}^2, n{p}^6$