Chemistry, asked by Zaeba, 20 days ago

Describe the orbital overlapping of ethene and ethyne.​

Answers

Answered by sophiaaa7081
2

Answer:

Explanation:

In the ethene molecule, the carbon atoms are sp2 hybridized. One unpaired electron in the p orbital remains unchanged. The two carbon atoms form a sigma bond in the molecule by overlapping two sp2 orbitals. In ethylene, each carbon combines with three other atoms rather than four.

Answered by anamikab5bkvpngd
2

Answer:

BONDING IN ETHENE

Important! You will find this much easier to understand if you first read the article about the bonding in methane.

You may also find it useful to read the article on orbitals if you aren't sure about simple orbital theory.

Ethene, C2H4

The simple view of the bonding in ethene

At a simple level, you will have drawn ethene showing two bonds between the carbon atoms.

Each line in this diagram represents one pair of shared electrons.

Ethene is actually much more interesting than this.

An orbital view of the bonding in ethene

Ethene is built from hydrogen atoms (1s1) and carbon atoms (1s22s22px12py1).

The carbon atom doesn't have enough unpaired

electrons to form the required number of bonds, so it needs to promote one of the 2s2 pair into the empty 2pz orbital. This is exactly the same as happens whenever carbon forms bonds - whatever else it ends up joined to.

So the first thing that happens is . . .

Promotion of an electron

There is only a small energy gap between the 2s and 2p orbitals, and an electron is promoted from the 2s to the empty 2p to give 4 unpaired electrons. The extra energy released when these electrons are used for bonding more than compensates for the initial input.

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