A chemical feature known as Electronegativity describes an atom’s ability to draw shared-pair electrons to itself within a molecule. Factors affecting electronegativity includes atomic size, nuclear charge and effect of substitute.
The electronegativity of atoms on the left and right sides of the periodic table varies significantly. It will be regarded as the primary determinant in chemical bonding because it is a significant quantity in establishing the type of bonds that exist between components.
Below is a list of the elements’ periodic tables along with a table of their electronegativities.
Nuclear charge, shielding, and atomic radius all have an impact on electronegativity. In the periodic table, the electronegativity falls as you move down a group. The electronegativity rises as you move from one era to the next in the periodic table.
Factors affecting electronegativity includes the following elements;
- Atomic size:
- As an atom’s size increases, its electronegativity falls.
- Since electrons are farther from the nucleus, there is less force of attraction between them, and larger atomic sizes will have lower electronegativity values.
- Nuclear Charge:
- As nuclear charge rises, electronegativity rises as well.
- A higher electronegativity value will be produced by a higher nuclear charge value.
- This occurs as a result of stronger electron attraction brought on by an increase in nuclear charge.
- The impact of the substitute
- An increase in inner electron density tends to decrease electronegativity because of the screening effect.
- The type of substituent that is bonded to an atom determines its electronegativity.
- As opposed to CH₃I, the carbon atom in CH₃I gains a larger positive charge ion.
- As a result, the C-atom in CH₃I is more electronegative than it is in CH₃I. A change in an atom’s electronegativity brought on by substituents alters the atom’s chemical behavior.
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