Answer:
[tex]H-C\equiv P^{\cdot\cdot_{}}_{}[/tex]
Explanation:
Here, we want to draw the lewis structure of HCP
We have the participating compound as, hydrogen with 1 valence electron, carbon with 4 valence electrons and phosphorus with 5 valence electrons
We would have three bonds between the carbon and the phosphorus, then we have a bond between the hydrogen and the carbon
That would leave a pair of non-bonding electrons on the phosphorus
We have the diagram as follows:
[tex]H-C\equiv P^{\cdot\cdot_{}}_{}[/tex]
Now, let us look at the options:
option A is wrong as the bond in a triple bond
option B is correct, there are no lone pairs on C
option C is correct as the C-H bond is a single bond
option D is correct as there is a pair of electron on the phosphorus atom
