Question

the type of overlapping is not observed in the formation of ethylene molecule​

Answer 1

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, C 2H4

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 (1s 1) and

carbon atoms (1s 22s 22p x 12p y 1).

The carbon atom doesn't have enough unpaired

electrons to form the required number of bonds,

so it needs to promote one of the 2s 2 pair into

the empty 2p z 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.

Answer 2

Answer:

σsp2 - p overlap is not possible

Explanation:

One sp2 - sp2 overlap

Four sp2 - s overlaps

One p - p overlap

so σsp2 - p overlap is not possible

The atoms come together by collisions. What does this signify at the atomic level, though. The process in which two atoms come so close to one another that they enter one other's orbitals and create a new hybridised orbital in which the bonding pair of electrons resides is referred to as this circumstance. This hybridised orbital is stable because it has less energy than the atomic orbital. It is in the state of least energy. Orbital overlap is the term for this little orbital penetration.

The two participating atoms, their sizes, and the valence electrons all affect how much overlap there is. In general, the connection formed between the two atoms is stronger the more overlap there is. Consequently, in accordance with the orbital overlap theory, atoms combine by forming a lower energy state where their valence electrons with opposite spin link together to create covalent bonds. This is accomplished by their orbitals crossing one other.

In his explanation of the chemical bond angles discovered by testing, Linus Pauling underlined the significance of orbital overlap, which serves as the foundation for the idea of orbital hybridization.

See more:

https://brainly.in/question/6274934

#SPJ3