What is hybridization(chemistry 5 marks)
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Hybridization happens when atomicorbitals mix to form a new atomic orbital. The new orbital can hold the same total number of electrons as the old ones. The properties and energy of the new, hybridized orbital are an 'average' of the original unhybridized orbitals.
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Hybridization happens when atomic orbitals mix to form a new atomic orbital. The new orbital can hold the same total number of electrons as the old ones. The properties and energy of the new, hybridized orbital are an 'average' of the original unhybridized orbitals.
The concept of hybridization was introduced because it was the best explanation for the fact that all the C - H bonds in molecules like methane are identical.
Example
In their ground state, carbon atoms naturally have electron configuration 1s2 2s22p2.
The four outermost electrons, i.e. those in the 2s and 2p sublevels are available to form chemical bonds with other atoms.
The 2s orbital is capable of holding up to two electrons, and there are three 2p orbitals, each capable of holding up to two electrons, which means the 2p orbitals can hold up to six electrons.
Individually, these electron orbitals look something like this. (Each is centered on carbon's nucleus and the p orbitals make angles of 90° with one another.)
The two lobes of a p orbital, one shaded, the other not, represent different phases of the wave function Ψ.
When a p orbital meets another orbital, their phases can interfere constructively or destructively. This is shown in the schematic below: an s orbital and a p orbital come together and hybridize. Like sign phases interfere constructively. There is destructive interference if the signs of the phases are different.
The end result is an sp hybrid orbital.
Taking it further, the 2s orbital and the three 2p orbitals can hybridize to form a new hybrid orbital, called sp3, which is capable of holding up to eight electrons.
The shape of molecules like methane, CH4, with bond angles of 109.5°, is consistent with sp3 hybridization of carbon atoms.
HOPE IT HELPS.
The concept of hybridization was introduced because it was the best explanation for the fact that all the C - H bonds in molecules like methane are identical.
Example
In their ground state, carbon atoms naturally have electron configuration 1s2 2s22p2.
The four outermost electrons, i.e. those in the 2s and 2p sublevels are available to form chemical bonds with other atoms.
The 2s orbital is capable of holding up to two electrons, and there are three 2p orbitals, each capable of holding up to two electrons, which means the 2p orbitals can hold up to six electrons.
Individually, these electron orbitals look something like this. (Each is centered on carbon's nucleus and the p orbitals make angles of 90° with one another.)
The two lobes of a p orbital, one shaded, the other not, represent different phases of the wave function Ψ.
When a p orbital meets another orbital, their phases can interfere constructively or destructively. This is shown in the schematic below: an s orbital and a p orbital come together and hybridize. Like sign phases interfere constructively. There is destructive interference if the signs of the phases are different.
The end result is an sp hybrid orbital.
Taking it further, the 2s orbital and the three 2p orbitals can hybridize to form a new hybrid orbital, called sp3, which is capable of holding up to eight electrons.
The shape of molecules like methane, CH4, with bond angles of 109.5°, is consistent with sp3 hybridization of carbon atoms.
HOPE IT HELPS.
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