Nitrogen (N) and phosphorous (P) are both Group 5 A elements, so you might expec

Question

Nitrogen (N) and phosphorous (P) are both Group 5 A elements, so you might expect that they would have similar chemical properties. Indeed, nitrogen will combine with three hydrogen atoms to form ammonia, NH_3. and phosphorous will combine with three hydrogen atoms to form phosphine, PH_3. However, phosphorous is able to combine with five chlorine atoms to make phosphorous pentachloride, PCl_5. The analogous nitrogen compound, NCI_5 does not exist A valid explanation for this observation is: Phosphorous, Period 3, has d orbitals available for bonding. Nitrogen, in Period 2, docs not. Phosphorous has more valance electrons than nitrogen, and can therefore form more bonds. Phosphorous has a larger atomic radius, so it can "fit" more atoms around it. Phosphorous forms a +5 action that is capable of bonding with five Cl+ anions.

Explanation / Answer

The correct answer is a.

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