Judging from their relative positions in the Periodic Table, which atom in each set is

Key concepts

Electronegativity

Ability of an atom to attract the shared pair of electrons towards it. It is a measure of the force of an atom’s attraction for electrons.

The most widely used scale of electronegativities was devised by Linus Pauling in the 1930s.

Electronegativity in periods

Generally increase from left to right within a period of the Periodic Values increase from left to right because the increasing positive charge on the nucleus results in a greater force of attraction for the atom’s valence electrons.

Electronegativity in Groups

Generally decrease from top to bottom within a group.

Electronegativity decreases from top to bottom because the increasing distance of the valence electrons from the nucleus results in a lower attraction between the nucleus and these electrons.

Step 1 of 4

We have to find which atom in each set is more electronegative judging from the relative position in the periodic table.

(a) Carbon or nitrogen     (b) Chlorine or bromine     (c) Oxygen or sulfur

Electronegativity is the ability of an atom to attract the shared pair of electrons towards it. It is a measure of the force of an atom’s attraction for electrons.