Question

Group the following electron configurations in pairs that would represent similar chemical properties at their atoms;

Answer 1

Answer: Pairs are:  (a) and (d), (b) and (f), (c) and (e)

Explanation:

In a periodic table, elements are arranged in 18 vertical columns known as groups and 7 horizontal rows known as periods.

Elements arranged in a group show similar chemical properties because of the presence of same number of valence electrons.

Valence electrons are defined as the electrons which are present in the outermost shell of an atom. Outermost shell has the highest value of 'n' that is principal quantum number.

For the given options:

• For a:

The given electronic configuration is:  $1s^22s^22p^63s^2$

The number of valence electrons in the given configuration are 2

• For b:

The given electronic configuration is:  $1s^22s^22p^63s^3$

The number of valence electrons in the given configuration are [2 + 3] = 5

• For c:

The given electronic configuration is:  $1s^22s^22p^63s^23p^64s^23d^{10}4p^6$

The number of valence electrons in the given configuration are [2 + 6] = 8

• For d:

The given electronic configuration is:  $1s^22s^2$

The number of valence electrons in the given configuration are 2

• For e:

The given electronic configuration is:  $1s^22s^22p^6$

The number of valence electrons in the given configuration are [2 + 6] = 8

• For f:

The given electronic configuration is:  $1s^22s^22p^63s^23p^3$

The number of valence electrons in the given configuration are [2 + 3] = 5

Electronic configuration of (a) and (d) will form a pair, (b) and (f) will form a pair, (c) and (e) will form a pair and will have similar chemical properties.

Hence, the pairs are:  (a) and (d), (b) and (f), (c) and (e)