Answer :
As we travel down the group in the current periodic table, the atomic number rises. Although the nuclear charge likewise rises, the effect of the rise is mitigated by the addition of one shell. As we descend the group, electronegativity's value drops. For instance, in the halogen group, the electronegativity value falls as we proceed from fluorine to astatine.
Electronegativity is the propensity of an atom in a molecule to draw the shared pair of electrons toward itself.
Because it is merely a propensity, this attribute has no dimensions. It essentially represents the final consequence of atoms' propensities to attract electron pairs that form bonds in various elements. On several scales, we quantify electronegativity. Linus Pauling created the most widely used scale.
An atom's ability to attract the electrons of a bond grows with electronegativity, a feature of an atom. In a covalent bond, atoms that are bound together and have similar electronegativity values share electrons equally.
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