Arrange N, O and S in order of decreasing electron affinity:

1. S > O > N

2. O > S > N

3. N > O > S

4. S > N > O

The increasing order of electron affinity of the elements (with the given electron configurations) is:

(I) $1{\mathrm{s}}^{2}2{\mathrm{s}}^{2}2{\mathrm{p}}^{6}3{\mathrm{s}}^{2}3{\mathrm{p}}^5$

(II) $1{\mathrm{s}}^{2}2{\mathrm{s}}^{2}2{\mathrm{p}}^3$

(III) $1{\mathrm{s}}^{2}2{\mathrm{s}}^{2}2{\mathrm{p}}^5$

(IV) $1{\mathrm{s}}^{2}2{\mathrm{s}}^{2}2{\mathrm{p}}^{6}3{\mathrm{s}}^1$

1. II < IV < III < I

2. I < II < III < IV

3. I < III < II < IV

4. IV < III < II < I

The process requiring absorption of energy is:

1.  $\mathrm{N}\to {\mathrm{N}}^{-}$

2. $\mathrm{F}\to {\mathrm{F}}^{-}$

3. $\mathrm{Cl}\to {\mathrm{Cl}}^{-}$

4. $\mathrm{H}\to {\mathrm{H}}^{-}$

Which of the following electronic configuration represents a sudden large gap between the values of second and third ionisation energies of an element?

Element having highest I.P value is :

1. Ne

2. He

3. Be

4. N

Which of the following atomic species has maximum ionisation energy?

1. O^-

2. S^-

3. Se^-

4. Te^-

Which of the following arrangements shows the correct order of decreasing paramagnetism?

1. N>Al>O>Ca

2. N>O>Al>Ca

3. O>N>Al>Ca

4. O>N>Ca>Al

Which of the following sets of atomic numbers corresponds to elements of group 16?

1. 8,16, 32, 54

2. 16, 34, 54, 86

3. 8,16, 34, 52

4. 10,16, 32, 50

Sodium generally does not show oxidation state of +2, because of its: 

 

1. High first ionization potential

2. High second ionization potential 

3. Large ionic radius

4. High electronegativity

Assuming that elements are formed to complete the seventh period, the atomic number of alkaline earth metal of the eighth period would be:

1. 113

2. 120

3. 119

4. 106