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mina [271]
3 years ago
14

How many single covalent bonds must a phosphorus atom form to have a complete octet in its valence shell? how many single covale

nt bonds must a phosphorus atom form to have a complete octet in its valence shell? 3 1 4 0 2?
Chemistry
2 answers:
charle [14.2K]3 years ago
4 0
Phosphorus   atom require to  form    3  single  covalent  bond  to  have  a  complete  octet  in  its  valence  shell.   Phosphorus  has  a  electron  configuration  2.8.5  hence  require  to  gain  three electrons  to  acquire  the octet  electron  configuration that  is an  electron  configuration  of  2.8.8.
Sonja [21]3 years ago
3 0

Answer: Option (a) is the correct answer.

Explanation:

Atomic number of phosphorous is 15 and its electronic configuration is [Ne]3s^{2}3p^{3}.

As there are 3 valence electrons in a single phosphorous atom. Therefore, to attain stability it will readily lose three electrons and thus forms a P^{3+} charge.

For example, in PCl_{3} there will be sharing of electrons between the phosphorous and chlorine atom.

Hence, a phosphorous atom can share its three valence electrons and thus forms three covalent bonds to have a complete octet in its valence shell.

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