Nonpolar Bond
Definition and meaning of Nonpolar Bond in chemistry.
A nonpolar bond is a covalent bond in which two atoms share electrons equally or nearly equally because their electronegativities are the same or very similar.
In more detail
When atoms have identical or very similar electronegativity values, they pull on the shared electron pair with equal force, resulting in equal distribution. This equal sharing creates no net dipole moment across the bond. Nonpolar bonds are common in homonuclear diatomic molecules such as hydrogen (H2), oxygen (O2), and nitrogen (N2), where both atoms are identical. Carbon-hydrogen bonds are also approximately nonpolar due to the similar electronegativities of these elements.
Key facts
| Electronegativity difference | 0 to approximately 0.5 |
|---|---|
| Common examples | H2, O2, N2, Cl2 |
| Dipole moment | Zero or negligible |
| Field | General Chemistry |
Molecular oxygen (O2) is a classic example; both oxygen atoms have identical electronegativity and share electrons equally, resulting in a purely nonpolar bond.
Frequently asked questions
How is a nonpolar bond different from a polar bond?
In a polar bond, atoms have significantly different electronegativities and share electrons unequally, creating a permanent dipole moment. In a nonpolar bond, electronegativities are similar or identical, resulting in equal electron sharing and no dipole.
Are homonuclear diatomic molecules always nonpolar?
Yes. Homonuclear diatomic molecules like H2, N2, O2, and Cl2 always have nonpolar bonds because both atoms are identical and have the same electronegativity.