The ground state electronic configurations of the elements, U,V,W,X,and Y (these symbols do not have any chemical significance) are as follows:
\(\begin{array}{ll} \mathrm U & 1 s^2 2 s^2 2 p^3 \\ \mathrm{V} & 1 s^2 2 s^2 2 p^6 3 s^1 \\ \mathrm{W} & 1 s^2 2 s^2 2 p^6 3 s^2 3 p^2 \\ \mathrm{X} & 1 s^2 2 s^2 2 p^6 3 s^2 3 p^6 3 d^5 4 s^2 \\ \mathrm{Y} & 1 s^2 2 s^2 2 p^6 3 s^2 3 p^6 3 d^{10} 4 s^2 4 p^6 \end{array}\)

Determine which sequence of elements satisfies the following statements :

(i)	Element forms a carbonate that is not decomposed by heating
(ii)	An element is most likely to form coloured ionic compounds
(iii)	Element has the largest atomic radius
(iv)	Element forms only an acidic oxide

1. V W Y U
2. V X Y W
3. V W Y X
4. V X W U

Which one will show variable oxidation state?

(I) $\left[Kr\right]5s^1$                                 (II) $\left[Rn\right]5f^{14}6d^{1}7s^2$
(III)$\left[Ar\right]3d^{10}4s^{2}4p^5$                    (IV) $\left[Ar\right]3d^{6}4s^2$

If period number and group number of any representative element(s) are same then which of the following statement is incorrect regarding such type element(s) in their ground state?

(1) The possible value of principal quantum number is 2

(2) The possible value of azimuthal quantum number is zero

(3) The possible value of magnetic quantum number is 1

(4) The species could be paramagnetic

How does the energy gap between successive energy levels in an atom vary from low to high n values?

(1) All energy gaps are the same

(2) The energy gap decreases as  n increases

(3) The energy gap increases as  n  increases 

(4) The energy gap changes unpredictably as  n  increases

In alkaline earth metals, the properties, among the following, that will increase from Be to Ba are:

(i) Atomic radius
(ii) Ionisation energy
(iii) Nuclear charge

The incorrect order of ionic size among the following is :

(1)$\mathrm{<mspace\; width="1em"></mspace>L}{a}^{3+}>G{d}^{3+}>E{u}^{3+}>L{u}^{3+}$           (2)${\mathrm{<mspace\; width="1em"></mspace>V}}^{2+}>V^{3+}>V^{4+}>V^{5+}$

(3) $T{l}^{+}>I{n}^{+}>S{n}^{2+}>S{b}^{3+}$                (4)${\mathrm{<mspace\; width="1em"></mspace>K}}^{+}>S{c}^{3+}>V^{5+}>M{n}^{7+}$

Aqueous solutions of two compounds $M_1-O-H<mspace\; width="1em"></mspace>and<mspace\; width="1em"></mspace>M_2-O-H$ are prepared in two different beakers. If, the electronegativity of $M_1=3.4<mspace\; width="1em"></mspace>,<mspace\; width="1em"></mspace>M_2=1.2,<mspace\; width="1em"></mspace>O=3.5<mspace\; width="1em"></mspace>and<mspace\; width="1em"></mspace>H=2.1,$ then the nature of two solutions will be respectively:

(a) acidic, basic             (b) acidic, acidic

(c) basic, acidic             (d) basic, basic

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

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) $B_2>C_3>A_1$

Find the incorrect match among the following electronic configurations and their corresponding period and group numbers.