The various factors which influence electronegativity are
1. Atomic Radius
Electronegativity decreases with increase in size of atom.
2. Nuclear Charge
Electronegativity increases with increasing nuclear charge.
3. Screening Effect
Increase in number of inner electrons tends to decrease the electronegativity due to screening effect.
1. Atomic Radius
Electronegativity decreases with increase in size of atom.
2. Nuclear Charge
Electronegativity increases with increasing nuclear charge.
3. Screening Effect
Increase in number of inner electrons tends to decrease the electronegativity due to screening effect.
please give more factors related with hybridization
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DeleteIonisation energy and electron affinity
ReplyDeleteHigher Ionisation energy and electron affinity lead to higher electronegativity.
Number and nature of atoms
The electronegativity depends on the number and nature of atoms bonded to it.
Type of hybridization
The electronegativity increases with the increase in 's' character in the hybrid orbital. This is because the 's' orbitals being more near to the nucleus have greater tendency to attract the shared pair of electron.
Charge on the ion
A cation has high electronegativity while an anion has less electronegativity than its parent atom. A cation with a higher positive charge is more electronegative.
Variation along a period
As the nuclear charge increases from going left to right in a period because the electrons enter the same shell, the shielding is less effective. Thus the increased nuclear charge attract the shared pair of electrons more strongly resulting in higher electronegativity from going left to right in a period.
Variation down the group
Electronegativity decreases down the group because the atomic size increases. The larger the size of the atom the lesser the tendency to attract the shared pair of electrons.
Can you explain how the nature of bounded atom affect electronegativity
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