The process requiring the absorption of energy is :

1. $F\to F^{-}$

2. $H\to H^{-}$

3. $Cl\to C{l}^{-}$

4. $O\to O^{2-}$

Consider the following statements:

(I) Rutherford name was associated with the development of periodic table.

(II) A metal M having electronic configuration $1s^2, 2s^2, 2p^6, 3s^2, 3p^6 ,3d^{10}, 4s^1$ is d-block element.

(III) Diamond is  an element.

(IV) The electronic configuration of the most electronegative elements is $1s^2, 2s^2, 2p^5,$ 

and select the correct one from the given codes.

(A) I, II, IV                                      (B) I, II, III, IV

(C) II, IV                                         (D) I, III, IV

There are four elements 'p', 'q', 'r' and 's' having atomic number Z-1, Z, Z+1 and Z+2 respectively. If there element 'q' is an inert gas, select the correct answers from the following statements.

(i) 'p' has most negative electron gain enthalpy in the respective period.

(ii) 'r' is an alkali metal.

(iii) 's' exists in +2 oxidation state.

(1) (i) and (ii)                     

(2) (ii) and (iii)

(3) (i) and (iii)                     

(4) (i), (ii) and (iii)

Given below are four orders for the size of the species. Choose the correct ones:

(a) ${\mathrm{Al}}^{3+}<{\mathrm{Mg}}^{2+}<{\mathrm{Na}}^{+}<{\mathrm{F}}^{-}$

(b) ${\mathrm{Al}}^{3+}<{\mathrm{Mg}}^{2+}<$ ${\mathrm{Li}}^{+}<{\mathrm{K}}^{+}$

(c) ${\mathrm{Fe}}^{4+}<{\mathrm{Fe}}^{3+}<{\mathrm{Fe}}^{2+}<\mathrm{Fe}$

(d) $\mathrm{Mg}>\mathrm{Al}>\mathrm{Si}>\mathrm{P}$

1. (a), (b) & (c)                       

2. (b), (c) & (d)

3. (a), (c)                          

4. (a), (b), (c) & (d)

Which of the following orders are correct for the ionization energies?

(A) \(  B a   <   S r   <   C a        \)                  
(B) \(S^{2 -} < S   < S^{2 +}\)
(C) \(C   <   O < N\)
(D) \(M g   <   A l   <   S i\)

1. A, B and D                             
2. A, C and D
3. A, B and C                             
4. A, B, C and D

The electron gain enthalpies of halogens in kJ mol^-1 are given below.

F =-332, Cl =-349, Br =-325, I =-295.

The lesser negative value for F as compared to that of Cl is due to:
 

1. Strong electron-electron repulsions in the compact 2p-subshell of F.

2. Weak electron-electron repulsions in the bigger 3p-subshell of Cl.

3. Smaller electronegativity value of F than Cl.

4. 1 & 2 both 

Which of the following statements are correct ?

1. (i), (iii) and (iv)                     
2. (ii), (iii) and (iv)
3. (i), (ii) and (iv)                         
4. (i), (ii) and (iii)  

Which of the following statements is not correct?

(1) The first ionization energies (in KJ $mo{l}^{-1}$) of carbon, silicon, germanium, tin, and lead are 1086, 786, 761, 708 and 715 respectively.

(2) Down the group, electronegativity decreases from B to Tl in boron family.

(3) Among oxides of the elements of carbon family, CO is neutral, GeO is acidic and SnO is amphoteric.

(4) The 4f- and 5f- inner transition elements are placed separately at the bottom of the periodic table to maintain its structure.

The correct order among the following options is: 

1. F > N > C > Si > Ga - Non-metallic character.

2. F > Cl > O >N - Oxidising property.

3. C < Si > P > N  - Electron affinity value.

4. All of the above.

Which of the following statements is correct for an element that forms oxides in different oxidation states?