Question

Consider the positions of carbon, nitrogen, potassium, and calcium on the periodic table. The atoms of which element attract electrons most strongly in chemical bonds? A. Carbon B. Calcium C. Nitrogen D. Potassium

Answer 1

C. Nitrogen

Step-by-step explanation:

Potassium (K) belongs to Group 1 (alkali metal series) and period 4

Calcium (Ca) belongs to group 2 (alkaline earth metals) and period 4

Carbon (C) belongs to group 14 and period 2

Nitrogen (N) belongs to group 15 and period 2

The ability of atoms to attract a pair of bonding electrons towards itself is referred by the term electronegativity. This tendency increases on moving from left to right across a period as more electrons are added to the same valence shell. This increases the force of attraction between the electrons and the nucleus. In contrast, electronegativity decreases down a group as electrons are now being added to new shells that are further away from the nucleus.

Therefore, based on the given options, N which is farthest to the right of the periodic table will be the most electronegative and will attract electrons more strongly in chemical bonds.

Answer 2

The atoms of which element attract electrons most strongly in chemical bonds is : C. Nitrogen
From the option above, nitrogen has a configuration of the electrons in its atom that will attract electrons most strongly

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