[tex]\boxed{{\text{C) N}}}[/tex] has the greatest attraction for electrons in a chemical bond.
Further explanation:
Electronegativity:
It is the tendency of an atom to attract the shared electrons in the bond towards itself. More the electronegativity of the atom, higher will be its tendency to attract the bonding electrons towards itself. The electronegative atom develops a partial negative charge and the electropositive atom develops a partial positive charge.
Electronegativity trends in the periodic table:
Along the period, electronegativity increases due to the increase in the nuclear charge. This results in the strong attraction of electrons.
Down the group, electronegativity decreases due to an increase in the size of elements. This results in a lesser attraction between the nucleus and the electron.
All the given elements (As, Bi, N, P) are present in the same group of the periodic table. Nitrogen is present at the top of the group so it has the highest electronegativity among the given elements. Phosphorus is present below nitrogen but above As and Bi so its electronegativity is less than nitrogen but more than the remaining elements. Arsenic is present above Bi so it has more electronegativity than Bi. Bismuth is present at the bottom of the group so it has the least electronegativity among the given elements.
Therefore, nitrogen has the greatest tendency to attract electrons towards itself in a chemical bond.
Learn more:
1. Which ion was formed by providing the second ionization energy? https://brainly.com/question/1398705
2. Write a chemical equation representing the first ionization energy for lithium: https://brainly.com/question/5880605
Answer details:
Grade: High School
Subject: Chemistry
Chapter: Periodic classification of elements
Keywords: electronegativity, electron, N, P, As, Bi, group, period, increase, decrease, attraction, chemical bond, nitrogen, phosphorus, arsenic, bismuth.
