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(A): Nitrogen is unable to show a valenc...

(A): Nitrogen is unable to show a valency more than three.
(R): Nitrogen does not have vacant d-orbitals in its valence shell. 

A

Both (A) and (R ) are true and (R ) is the correct explanation of (A)

B

Both (A) and (R ) are true and (R ) is not the correct explanation of (A)

C

(A) is true but (R ) is false

D

Both (A) and (R ) are false

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Passage-IV : Sulphur and rest of the elements of group 16 are less electronegative than oxygen. Therefore, their atoms cannot take up electrons easily. They can acquire ns^(2)np^(6) configuration by sharing two electrons with the atoms of other elements and thus, exhibit +2 oxidation state in their compounds. In addition to this, their atoms have vacant d-orbitals in their valence shell to which electrons can be promoted from the p and s-orbitals of the shell. As a result, they can show +4 and +6 oxidation states shell. Like sulphur, oxygen does not show +4 and +6 oxidation states. The reason is :

Passage-IV : Sulphur and rest of the elements of group 16 are less electronegative than oxygen. Therefore, their atoms cannot take up electrons easily. They can acquire ns^(2)np^(6) configuration by sharing two electrons with the atoms of other elements and thus, exhibit +2 oxidation state in their compounds. In addition to this, their atoms have vacant d-orbitals in their valence shell to which electrons can be promoted from the p and s-orbitals of the shell. As a result, they can show +4 and +6 oxidation states shell. The nature of the compounds of sulphur having +4 oxidation state is :

Which element has (a) two shells, both of which are completely filled with electrons ? (b) the electronic congiguration 2, 8, 2 ? (c) a total of three shells, with four electrons in its valence shell ? (d) a total of two shells, with three electrons in its valence shell ? (e) twice as many electrons in its seconds shell as in its first shell ?