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Although PF5, PCl5 and PBr5 are known, t...

Although `PF_5, PCl_5` and `PBr_5` are known, the pentahalides of nitrogen have not been observed.
Phosphorous has lower electronegativity than nitrogen.

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The correct Answer is:
B
`(A)` and `( R)` are both correct but `( R)` is not correct explanation for `(A)`. Nitrogen does not form pentahalides because it does not have `d-"orbitals"`. The electronegativity of `P` is less than that of `N`.
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Why nitrogen trihalide cannot be oxidised to pentahalide whereas phosphorous trihaldes can be oxidised to pentahalide ?

प्रक्कथन : यद्यपि `PF_(5), PCl_(5)` और `PBr_(3)` ज्ञात हैं, किन्तु नाइट्रोजन के पेण्टा हैलाइड ज्ञात नहीं हैं |
कारण : नाइट्रोजन की अपेक्षा फॉस्फोरस की ऋणविद्युतता कम होती है |

Assertion `BF_(3)` has greater dipole momnet than `H_(2)S`
Reasoning Fluorine is more electronegative than sulphur .

Assertion : Pentahalides of phosphorus are known but not those of nitrogen.
Reason : Phosphorus has lower electronegativity than nitrogen.

`PCl_(5)` is known but `NCl_(5)` is not known.
Or Nitrogen does not form pentahalide.

कथन I यद्यपि तथा ज्ञात है , किन्तु नाइट्रोजन के पेन्टाहैलाइड ज्ञात नहीं है ।
कथन II फॉस्फोरस की विघुत -ऋणात्मकता नाइट्रोजन से कम होती है ।

Nitrogen does not form pentahalides as it does not have ............ .

PCI_(5) is known but NCI_(5) is not known. Or Nitrogen does not form pentahalide.

Why phosphorous has higher electron affinity than nitrogen?

(A) : PF_(5),PCl_(5) and PBr_(3) are known, the pentahalides of nitrogen have not been observed (R ) Phosphorous has lower electronegativity than nitrogen.

Pentahalides of phosphorus are known, but not pentahydride. Why?

वक्तव्य I यद्यपि `PF_5,PCl_5`, और `PBr_3` ज्ञात हैं, किन्तु नाइट्रोजन के पेण्टा हैलाइड ज्ञात नहीं हैं।
वक्तव्य II नाइट्रोजन की अपेक्षा फॉस्फोरस की ऋणविद्युतता कम होती है।

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