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# Nonpolar Covalent Bond

The idea of polarity is almost similar to what we get to see in north and south poles of a magnet. But in case of bond polarity the terms are rather positive and negative instead of the terms used in magnets. A bond has a polarity when the shared pair of electrons is shared unequally and when one of the bonding atoms has more electron pulling power than the other atom the shared pair of electrons is located closer to that atom.

The signs of negative and positive are designated with delta negative and delta positive notation which indicates partial negative and particle positive charge. This is little different from partial negative and partial positive charge as this is just a matter of degree.

## Non Polar Covalent Bond Definition

Although all covalent bonds involve the sharing of electrons they widely differ in the degree of sharing and based on this we classify the covalent bonds into two categories of nonpolar covalent and polar covalent which basically differs in electronegativity between bonded atoms.

In a nonpolar covalent bond electrons are shared equally and there is no sharp dividing line between polar and nonpolar covalent and as per thumb rule the Non polar covalent would be considered for if the electronegativity difference between bonding atoms is less than 0.5 and hence anything greater than this value will be considered for anything but nonpolar bond.

For example the difference of electronegativity between hydrogen and Chlorine in the bond of H-Cl is found to be 3.0 – 2.1 = 0.9 and hence it is considered as polar covalent bond. While the bonding between carbon and hydrogen, the electronegativity difference is 2.5 – 2.1 = 0.4 which classifies this as nonpolar covalent bond. The increasing difference in electronegativity is directly related to increasing bond polarity.

## What is Nonpolar Covalent Bond?

In a nonpolar covalent bond the shared electrons are not drawn substantially closer to either of the two atoms and as per the rule the chemists have coded it as electronegativity difference in the range of 0 to 0.5 results in nonpolar covalent bond. Any molecule with same bonded atoms would definitely qualify for such covalent bonds. For example the bromine molecule has the same electronegativity difference between the atoms is zero.

This could work out as the shared electrons is not pulled to either end of the molecule which resulted in a nonpolar bond. The description of delta positive and delta negative notation is not required for this molecule as the electrons are uniformly distributed. Non polar covalent bonds are typically bonding pattern where the atoms remain electrically neutral as each shared electron stay away from each other where each of are either of same atoms or having same electronegativity value.

## Nonpolar Covalent Bond Examples

Nonpolar covalent examples for molecules life hydrogen or fluorine diatomic forms where there is aequal sharing of electron pairs. Both the hydrogen atoms in hydrogen molecule as well as the fluorine atoms in fluorine molecule displays equal sharing of bonding electrons and hence is considered as nonpolar covalent bond.

The bonds in hydrogen molecule, fluorine molecule, nitrogen tri chloride (both nitrogen and chlorine have equal abilities to attract electrons) and are considered as nonpolar.

 Non polar covalent molecule Molecule Formula Hydrogen $H_{2}$ Fluorine $F_{2}$ Nitrogen tri chloride $NCl_{2}$ Methane $CH_{4}$ Bromine $Br_{2}$

## Nonpolar Covalent Bond Molecules

There are two types of covalent bonds and the type of bond in a molecule is determined by an atoms ability to share its electrons. A nonpolar covalent bond is formed when atoms share their electrons equally due to the identical atoms presence and as neither atoms could dominate in controlling the shared electrons. The electrons being equally shared makes the molecule as nonpolar in character.

In case we are looking at polar molecules, the bonded atoms become partially positive as one of the bonded atoms loses controls of the electrons. In case of nonpolar bonds none of the bonded atoms never lose control of their electrons and hence never obtain partial positive charge or partial negative charge.