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How does the electronegativity of p-block elements change across a period?

Last updated date: 21st Jul 2024
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Hint: Modern periodic table consists of 18 vertical columns known as groups arranged as left to right and seven horizontal rows known as periods arranged from top to bottom. In this periodic table elements are arranged according to their atomic number and this table divides the elements into s, p, d and f-block elements on the basis of their valence shell electrons.

Complete answer:
Electronegativity can be defined as the tendency of an atom in a molecule to attract the shared pair of electrons towards itself and electronegativity is said to be a dimensionless property because it is only tendency.
Electronegativity represents the net result of the tendencies of atoms in different elements to attract the bond-forming electron pairs. We measure electronegativity on the scale designed by Linus Pauling. According to this scale fluorine is the most electronegative element with a value of 4.0 and cesium is the least electronegative element with a value of 0.7.
Electronegativity generally increases as we move from left to right across a period in a periodic table and decreases as we move down a group. This can be explained as we go from left to right across a period then nuclear charge is increasing faster than the electron shielding so the attracting power of atoms for the valence electrons increases.
Hence we can say that electronegativity of p-block elements increases across a period.

As we move towards the left of the periodic table then their valence shells are less than half full so atoms tend to lose electrons and have less electronegativity similarly if we move towards right then it has high electronegativity.