Question:

Phosphorus cannot form $PH_5$ with its outer electronic configuration as $3s^23p^3$ because

Updated On: Jul 6, 2022
  • phosphorus cannot show $+5$ oxidation state
  • $PH_5$ is not a stable compound
  • $\Delta_aH$ value of dihydrogen and $\Delta_{eg}H$ value of hydrogen do not favour higher oxidation state of phosphorus
  • phosphorus is not very reactive hence does not form $PH_5$
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The Correct Option is C

Solution and Explanation

Since higher oxidation state of $P$ is not favoured by high $\Delta_aH$ of dihydrogen and $\Delta_{eg}H$ of hydrogen, $P$ does not form $PH_5$ though it exhibits $+3$ and $+5$ oxidation states.
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Notes on dihydrogen

Concepts Used:

Dihydrogen

Dihydrogen is the homonuclear diatomic molecule built from two hydrogen atoms. This molecule characterizes a covalent bond between two hydrogen atoms, satisfying each of their required pair configurations.

Structure of Dihydrogen:

The dihydrogen molecule characterizes a single covalent bond between the two hydrogen atoms that comprise it. This molecule has a linear shape and is nonionic in nature. Each hydrogen atom comes up with one electron towards the covalent bond.

Properties of Dihydrogen:

  • At Standard Temperature and Pressure (STP), dihydrogen exists in the gaseous state.
  • The melting point of H2 is 13.99 Kelvin. Transforming this value to the celsius scale, the melting point of dihydrogen can be expressed as -259.16 degrees celsius.
  • The boiling point correlated with dihydrogen corresponds to 20.271 on the Kelvins scale. Transforming this value into the celsius scale, the boiling point of H2 can be represented as -252.879 degrees celsius.
  • The latent heat of fusion associated with the H2 molecule correlates to 0.117 kilojoules per mole.
  • The latent heat of vaporization (also known as the enthalpy of vaporization) of dihydrogen is equivalent to 0.904 kilojoules per mole.