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Bonding AQA A Level Chemistry

How would you work out the shape of the POCl3 molecule please?
Original post by anon25x
How would you work out the shape of the POCl3 molecule please?

Treat the P=O bond like a normal bonding pair.

Using this, can you now work out how many bonding regions are there around the phosphorus atom?
Reply 2
Original post by TypicalNerd
Treat the P=O bond like a normal bonding pair.

Using this, can you now work out how many bonding regions are there around the phosphorus atom?


Is it 3 ? Thanks for the help !
Original post by anon25x
Is it 3 ? Thanks for the help !

You have the P=O and all three of the P-Cl bonds. Think again.
Reply 4
Original post by TypicalNerd
You have the P=O and all three of the P-Cl bonds. Think again.

Oh yeah sorry I meant the P=O goes upwards and there are 3 P-Cl bonds around the Phosphorus
Original post by anon25x
Oh yeah sorry I meant the P=O goes upwards and there are 3 P-Cl bonds around the Phosphorus


So that’s 4 bonding regions in total…


How many lone pairs are there? (Hint: draw a dot-and-cross diagram)
Reply 6
Original post by TypicalNerd
So that’s 4 bonding regions in total…


How many lone pairs are there? (Hint: draw a dot-and-cross diagram)


Are the 0 lone pairs?And 4 bonding pairs
Original post by anon25x
Are the 0 lone pairs?And 4 bonding pairs

Correct. So what shape would you expect a molecule with no lone pairs and 4 bonding pairs to have?

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