The electronic configuration of Palladium is:

1. [Kr] 5f³ 6d¹ 7s²

2. [Kr] 5f⁵ 6d¹ 7s²

3. [Kr] 5f² 6d¹ 7s²

4. None of the above.

The element having very high electron affinity but zero ionisation enthalpy is:

1. He (due to inert gas configuration)

2. Be (due to fully filled subshell)

3. H (due to presence of allotropes)

4. None of the above

Which of the following correctly represents both the increasing order of ionic radii and
 the decreasing order of the number of protons?

1. Ca⁺², K⁺, Cl^-, S^-2

2. Cl^-, Ca⁺², K⁺, S^-2

3. S^-2, Cl^-, Ca⁺², K⁺

4. None of the above

Element/Ion that has the highest electron affinity is:

 The correct order for electron affinity of halogens is :

1. Br > F

2. F > Cl

3. Br > Cl

4. F > I

Which of the following species has the smallest ionic radius?

Which electronic configuration corresponds to the outermost shell of chalcogens?

1. ${\mathrm{ns}}^2{\mathrm{np}}^3$ $$ $$ $$    

2. ${\mathrm{ns}}^2{\mathrm{np}}^4$ $$ $$ $$     

3. ${\mathrm{ns}}^2{\mathrm{np}}^5$           

4. ${\mathrm{ns}}^2{\mathrm{np}}^6$

The incorrect match among the following is:

1. B < C < N < O (increasing first ionisation enthalpy)

2. I < Br < F < Cl (increasing electron gain enthalpy)

3. Li < Na < K < Rb (increasing metallic radius)

4. Al³⁺ < Mg²⁺ < Na⁺ <F^- (increasing ionic size)

The correct sequence of increasing radii is - 

The correct order of increasing electron gain enthalpy with a negative sign for the elements O, S, F, and Cl is : 

1. Cl < F < S < O                   

2. O < S < F < Cl

3. F < S < O < Cl                   

4. S < O < Cl < F