• Electronegativity?varies across?Periods?and down the Groups of the Periodic Table

Down a group

• There is a?decrease?in?electronegativity?going down the Group
• The?nuclear charge increases?as more protons are being added to the nucleus
• However, each element has an extra filled electron shell, which increases?shielding
• The addition of the extra shells increases the distance between the nucleus and the outer electrons resulting in?larger?atomic radii
• Overall, there is decrease in attraction between the nucleus and outer bonding electrons

Electronegativity decreases going down the groups of the periodic table

Across a period

• Electronegativity?increases?across a Period
• The?nuclear charge increases?with the addition of protons to the nucleus
• Shielding?remains reasonably the?same?across the Period as no new shells are being added to the atoms
• The nucleus has an increasingly strong attraction for the bonding pair of electrons of atoms across the Period of the Periodic Table
• This results in?smaller atomic radii

Electronegativity increases going across the periods of the Periodic Table

Trends down a group & across a period table