The first four ionization energy values of metal are 191, 587, 872 and 5962 kcal/mol respectively. The number of valence electrons in the element is

1.  1

2.  2

3.  3

4.  5

The outermost electronic configuration of the most electronegative element is 

1.  $n{s}^2, n{p}^3$

2.  $n{s}^2, n{p}^6\left(n-1\right)d^5$

3.  $n{s}^2, n{p}^5$

4.  $n{s}^2, n{p}^6$

Of the following, the ion with the largest size is

1.  $O^{2-}$

2.  $N{a}^{+}$

3.  $F^{-}$

4.  $A{l}^{3+}$

Arrange the first ionization enthalpies of Na, Mg, Al, and Si in ascending order:

1. Na < Mg > Al < Si

2. Na > Mg > Al > Si

3. Na < Mg < Al < Si

4. Na > Mg > Al < Si

Electronic configuration of chalcogens in their outermost orbit is:

1. s² p³

2. s² p⁴

3. s² p⁵

4. s² p⁶

Which of the following is smallest in size?

1. Na⁺

2. F^–

3. O^2–

4. N^3–

When a neutral atom is converted into a cation,there is

1. Decrease in the atomic number

2. An increase in the atomic number

3. An increase in size

4. A decrease in size

Which of the following statements accurately describes the electron affinity trend among halogens?

1. Br > F

2. F > Cl

3. Br > Cl

4. F > I

Which one of the elements has highest ionisation energy?

1. [Ne] 3s² 3p¹

2. [Ne] 3s² 3p²

3. [Ne] 3s² 3p³

4. [Ar] 3d¹⁰ 4s² 4p²

The electronegativity of the following elements increases in the order:

1. C, N, Si, P

2. N, Si, C, P

3. Si, P, C, N

4. P, Si, N, C