The electronic configuration of four elements are :
(I)   [Kr]5s¹
(II)  [Rn]5f¹⁴6d¹7s²
(III) [Ar]3d¹⁰4s²4p⁵
(IV) [Ar]3d⁶4s²

Consider the following statements :
(i) I Shows variable oxidation state
(ii) II is a d-block element
(iii) The compound formed between I and III is covalent
(iv) IV shows single oxidation state

Which statement is True (T) or False (F)?

1. FTFF
2. FTFT
3. FFTF
4. FFFF

If the ionic radii of K⁺ and F^- are nearly the same (i.e., 1.34 Å), what are the atomic radii of K and F respectively?

X_(g)→ X⁺_(g) + e^- , ∆H = +720 KJ mol^-1

Calculate the amount of energy required to convert 110 mg of ‘X’ atom in gaseous state into X⁺ion. (Atomic wt. for X = 7 g/mol)

Which is the correct order of ionization energies?

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