If the ionization enthalpy and negative electron gain enthalpy of an element are 275 and 86 kcal $mo{l}^{-1}$ respectively, then the electronegativity of the element on the Pauling scale is:

1. 2.8                                     

2. 0.0

3. 4.0                                     

4. 2.6

The incorrect statement is:

(1) The second ionisation energy of Se is greater than that of second ionisation energy of As 

(2) The first ionisation energy of $C^{2+}$ ion is greater than that of first ionisation energy of $N^{2+}$ ion

(3) The third ionisation energy of F is greater than that of third ionisation energy of O

(4) Helogens have highest I.E. in respective period

Consider the following ionisation reactions :

I.E. (kJ $mo{l}^{-1}$)

$A_{\left(g\right)}\to A_{\left(g\right)}^{+}+e^{-}<mspace\; width="1em"></mspace>,<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>A_1$
$B_{\left(g\right)}^{+}\to B_{\left(g\right)}^{2+}+e^{-},<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>B_2$
$C_{\left(g\right)}^{+}\to C_{\left(g\right)}^{2+}+e^{-},<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>C_2$
$B_{\left(g\right)}\to B_{\left(g\right)}^{+}+e^{-},<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>B_1$
$C_{\left(g\right)}\to C_{\left(g\right)}^{+}+e^{-},<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>C_1$
$C_{\left(g\right)}^{2+}\to C_{\left(g\right)}^{3+}+e^{-},<mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace><mspace\; width="1em"></mspace>C_3$

If monovalent positive ion of A, divalent positive ion of B and trivalent positive ion of C have zero electron. Then incorrect order of corresponding I.E. is :

(1) $C_3>C_2>B_2$                       

(2) $B_1>A_1>C_1$

(3) $C_3>C_2>B_2$                       

(4) $B_2>C_3>A_1$

The incorrect match among the following options is:

Which of the following order is correct for the property mentioned in brackets?

$\left(a\right)<mspace\; width="1em"></mspace>S^{2-}>C{l}^{-}>K^{+}>C{a}^{2+}$                 (Ionisation energy)

$\left(b\right)<mspace\; width="1em"></mspace>C<N<F<O$                              (2nd Ionisation energy)

$\left(c\right)<mspace\; width="1em"></mspace>B>Al>Ga>In>Tl$                     (Electronegativity)

$\left(d\right)N{a}^{+}>L{i}^{+}>M{g}^{2+}>B{e}^{2+}>A{l}^{3+}$    (Ionic radius)

${\mathrm{IP}}_1$ and ${\mathrm{IP}}_2$ for Mg are 178 Kcal mol^–1 and 348 Kcal ${\mathrm{mol}}^{-1}$, respectively. The energy required for the reaction, $\mathrm{Mg}\to {\mathrm{Mg}}^{2+}$ $+$ $2{\mathrm{e}}^{-}$ will be:

1. +170 Kcal ${\mathrm{mol}}^{-1}$

2. +526 Kcal ${\mathrm{mol}}^{-1}$

3. –170 Kcal ${\mathrm{mol}}^{-1}$

4. –526 Kcal ${\mathrm{mol}}^{-1}$

Incorrect statement about characteristics regarding halogens is :

1. Ionization energy decreases with increase in atomic number.

2. Electronegativity decreases with increase in atomic number.

3. Electron affinity decreases with increase in atomic number.

4. Enthalpy of fusion increases with increase in atomic number. 

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 $1s^2,<mspace\; width="1em"></mspace>2s^2,<mspace\; width="1em"></mspace>2p^6,<mspace\; width="1em"></mspace>3s^2,<mspace\; width="1em"></mspace>3p^6<mspace\; width="1em"></mspace>,3d^{10},<mspace\; width="1em"></mspace>4s^1$ is d-block element.

(III) Diamond is  an element.

(IV) The electronic configuration of the most electronegative elements is $1s^2,<mspace\; width="1em"></mspace>2s^2,<mspace\; width="1em"></mspace>2p^5,$ 

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)