CorrectQuestion: Which of the following best describes the role of electronegativity in determining bond polarity? - Redraw

Understanding the Context

What Is Electronegativity?

Electronegativity is a chemical property that measures an atom’s ability to attract shared electrons in a covalent bond. Developed by Linus Pauling, electronegativity values increase across a period and decrease down a group in the periodic table.

How Electronegativity Affects Bond Polarity

Key Insights

Bond polarity arises when two bonded atoms have unequal sharing of electrons. This unequal sharing occurs due to a difference in electronegativity between the atoms. The atom with higher electronegativity pulls the shared electron density closer, creating a dipole—a molecule with partial negative (δ⁻) charge on the more electronegative atom and partial positive (δ⁺) charge on the less electronegative atom.

Here’s the key rule:
Bond polarity exists whenever there is a difference in electronegativity between the bonded atoms.

Categorizing Bond Polarity Based on Electronegativity Differences

To determine bond polarity, chemists compare the electronegativity values of the involved atoms:

Final Thoughts

• Nonpolar covalent bond:
  Electronegativity difference ≤ 0.4 (e.g., H–H, Cl–Cl)
  Electrons shared almost equally.

• Polar covalent bond:
  Electronegativity difference > 0.4 but < ~1.7 (e.g., H–Cl, O–H)
  Electrons drawn toward the more electronegative atom.

• Ionic bond (extreme case):
  Electronegativity difference ≥ ~1.7 (e.g., Na–Cl)
  Electrons effectively transferred, forming full charges.

CorrectQuestion Breakdown: Which Best Describes Electronegativity’s Role?

CorrectQuestion: Which of the following best describes the role of electronegativity in determining bond polarity?
– The correct answer is: Electronegativity determines the extent of unequal electron sharing in a covalent bond, directly influencing whether a bond is polar, nonpolar, or ionic.