Question

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The electronic configuration of the outermost shell of the most electronegative element is
(a) 2s²2p
(b) 3s 3p
(c) 4s4p
(d) 5s5p
How many significant figures should be present in the answer of the following calculations?
2.5x1.25x3.5/2.0
First member of each group of representative elements (i.e., s and p-block elements) shows
anomalous behaviour. Illustrate with two examples
How would you explain the fact that first ionization enthalpy of sodium is lower than that of
magnesium but its second ionization enthalpy is higher than that of magnesium?
Or
Arrange the elements N, P, O and S in the order of
(i) increasing first ionisation enthalpy.
(ii) increasing non-metallic character.
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Answer 1

Answer:

I didn't know the answer

Answer 2

Arranging N, P, O, and S in the order of-

(i) Increasing first ionisation enthalpy: S<P<O<N

Generally, the value of ionisation energy increases on moving across the period and decreases down the group. However, ionisation energy of N is greater than that of O due to the extra-stability of half-filled p orbitals. Likewise, ionisation energy of P is greater than S.

(ii) Increasing non-metallic character: P<S<N<O

Non-metallic character refers to the tendency of an atom to gain electrons in a reaction. It also increases from left to right in a period and decreases from top to bottom in a group.