The general outer electronic configuration of s, p, d , and f-block elements respectively would be :

1.	ns1-2, nd2np1-6, (n-1)d1-10np0-2, (n-2)f1-14(n-1)d0-10ns2
2.	ns1-2, ns2np1-6, (n-1)f1-10ns0-2, (n-2)g1-14(n-1)d0-1ns2
3.	ns1-2, ns2np1-6, (n-1)d1-10ns1-2, (n-2)f1-14(n-1)d0-1 ns2
4.	np1-2, nd2np1-6, (n-1)d1-10ns0-2, (n-2)f1-14(n-1)d0-10ns2

The position of elements with an outer electronic configuration as $(n-2) f^7(n-1)d^{1}n{s}^2, n = \mathrm{6\; :}$

1. 6^th period and 10^th group.

2.  7^th period and 3^rd group.

3.  6^th period and 3^rd group.

4. 7^th period and 9^th group.

1st (∆H₁) and 2nd  (∆H₂) Ionization Enthalpies (in kJ mol^–1) and the (∆_egH) Electron Gain Enthalpy (in kJ mol^–1) of a few elements are given below:

The most reactive metal is-
1. VI
2. III
3. I
4. II

The formula of the stable binary compounds that would be formed by 
an element having atomic number 71 and fluorine:

The factor that does not affect the valence electron is: 

The size of isoelectronic species: F^–, Ne and Na⁺, is affected by :

The incorrect statement about ionization enthalpy is -

Match the following isoelectronic species in column I and column II : 

The correct order of ionization energy of W, X, Y and Z is-

Consider the following curve:

   
X represents group with highest atomic radius. The element that belongs to Y group can be :