Question

1 can explain why an ionic compound forms using concepts of attractive force and electronegativity
Two students draw the Bohr models of sodium and chlorine and attempt to explain how they can form an ionic bond using the concept of electronegativity.
Bohr model of Sodium atom
Definition of electronegativity:
a measure of the ability of an atom's nucleus to attract electrons from a different atom within a chemical bond
12 N
Bohr model of Chlorine atom
17 P
18 N
Student A says that an ionic bond is formed when chlorine attracts in the electron away from sodium.
Student B says that an ionic bond is formed when the sodium gives away its electron to chlorine.
1. Using the definition of electronegativity and the concept of attractive force explain which student (A or B) has a better understanding of how ionic bonds form.
( points)
Student
B whas a better understanding of how ionic bonds form. This is because the more electronegative V atom will attract v the electrons to form the ions.

Answer 1

Student A has the better understanding.

Why: Electronegativity measures how strongly an atom’s nucleus attracts electrons in a bond. Chlorine is much more electronegative than sodium (Cl ≈ 3.0–3.2, Na ≈ 0.9), so Cl’s nucleus exerts a stronger attractive force on the valence electron involved. That stronger attraction pulls the single valence electron away from Na, producing Na+ and Cl–. The resulting ionic bond is the electrostatic attraction between those oppositely charged ions.

Comment on Student B: saying “sodium gives away its electron” correctly states the outcome, but it doesn’t identify the driving cause — the difference in electronegativity and the stronger attractive force of Cl’s nucleus. Both phrasings describe the same end result, but Student A’s explanation points to the correct underlying reason.