How many pπ-pπ and dπ-dπ in h3po4
Answers
Answer:
❖ dπ–pπ Bonds
This is a special type of bonding found in the molecular species having a central atom with d or p valence shell and surrounding groups with empty, partially or completely filled p or d orbitals. In addition to direct overlap resulting in the σ-bonding, dπ–pπ bonds are formed by the sidewise overlap.
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There is no pπ-pπ and dπ-dπ bonding in H₃PO₄.
Instead, there is a special type of bonding i.e., pπ-dπ bonding.
As we see in the structure that phosphorus (P) is the central atom bonded by 4 oxygen atoms.
P = 1s² 2s² 2p⁶ 3s² 3p³ 3d⁰ (in ground state)
In the above electronic configuration, there are 3 unpaired electrons in 3p sub-shell.
After excitation of one electron from 3s sub-shell.
P = 1s² 2s² 2p⁶ 3s¹ 3p³ 3d¹ (in excited state)
In the above electronic configuration, there are 5 unpaired electrons in 3s, 3p and 3d sub-shell.
Now, there are 4 σ bonds of sp³ hybridisation. This means that 4 electrons are used in σ bonding. Only one unpaired electron of d sub-shell is left which will participate in π bonding for sure.
If we take a look at oxygen electronic configuration,
O = 1s² 2s² 2p⁴
From this we get that the electron which will participate in the bonding belongs to p sub-shell.
So, the bond formation will takes place between electron in p sub-shell of oxygen atom and d sub-shell of phosphorus atom. So, there will be pπ-dπ bonding.
Here, p and d refers to those subshell which take part in bonding and π denotes the bonding (as we know that there are only two types of bonding on the basis of overlapping - σ bonding and π bonding).
