Is Br2 Polar or Nonpolar?

Why is Br2 Nonpolar?

Bromine is a diatomic molecule with two identical bromine atoms sharing a single covalent bond. Both atoms have the same electronegativity (2.96), so electrons are shared equally and no dipole moment forms. Br2 is completely nonpolar.

• Symmetric linear geometry (180°): The atoms are arranged symmetrically around the central atom. This forces all bond dipoles to point in directions that cancel each other out exactly.
• Weak bond polarity: The small electronegativity difference (0.00) between Br and Br produces only weakly polar bonds, and the symmetric geometry cancels even these.
• Zero net dipole (0 D): Because all bond dipoles cancel, the net dipole moment is 0 D. Any molecule with zero net dipole moment is classified as nonpolar.

Molecular Geometry of Br2

Br2 has a linear molecular geometry with a bond angle of 180°. Here is why this shape determines polarity:

• The linear arrangement places all outer atoms at equal angles (180°) from the central atom, creating perfect spatial symmetry.
• Each bond dipole has an equal and opposite counterpart — they cancel in pairs, leaving no net charge separation.
• Symmetry is the key: even if the individual bonds are polar, the linear geometry ensures a net dipole of 0 D.

Electronegativity and Polarity

Electronegativity measures how strongly an atom attracts bonding electrons. A difference greater than ~0.5 on the Pauling scale generally means the bond is polar.

In Br2:

• Br (central atom) electronegativity: 2.96
• Br (outer atom) electronegativity: 2.96
• Difference: 0.00 — below the ~0.5 threshold, so the Br–Br bonds are only weakly polar

With a small electronegativity difference (0.00) and a symmetric linear geometry, Br2 is nonpolar with a net dipole of 0 D.

Is Br2 Polar or Nonpolar? (Quick Answer)

Br2 (Bromine) is nonpolar. Br2 is a nonpolar molecule because both bromine atoms are identical and there is no charge separation across the bond.