Covalent Bonds: Predicting Bond Polarity and Ionic Character

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  1. 0:05 Covalent Bonds
  2. 1:01 Electronegativity
  3. 1:58 Polar and Nonpolar Covalent Bonds
  4. 2:50 Ionic Character
  5. 4:11 Lesson Summary
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Taught by

Amy Meyers

Amy holds a Master of Science. She has taught science at the high school and college levels.

Learn about covalent bonds and their two types: nonpolar covalent bonds and polar covalent bonds. Discover how to predict the type of bond that will form based on the periodic table. Learn what ionic character means and how to determine it.

Covalent Bonds

Do you like to play basketball? Do you like to drive in a car that has tires? You can thank Mr. Goodyear. Naturally, rubber is sticky when warm and brittle when cold. It doesn't make good balls or good tires. In 1839, Charles Goodyear accidentally dropped a mixture of sulfur and natural rubber on a hot stove. The mixture heated up and became tough and elastic, forming vulcanized rubber. Why did it change properties? They changed because of the covalent bonds that formed between the rubber and sulfur.

Covalent bonds transform sulfur and natural rubber into vulcanized rubber when heated

A covalent bond is formed when atoms share one or more pairs of electrons. This is opposed to an ionic bond, where electrons are actually transferred from one atom to another. You can remember the difference by thinking that the 'C' in 'covalent' is kind of like an 'S' in 'share.' Covalent bonds share electrons. Ionic bonds transfer electrons. The 'I' in 'ionic' is like the 'T' in 'transfer.'


Just to review for a quick moment, electrons are negatively charged, so if an atom has more electrons than protons, it's going to have a negative charge. Electronegativity is the ability of an atom to attract shared pairs of electrons to it, so the more electronegative the atom is, the more it will attract electrons.

In general, metals, which mostly reside on the left side of the periodic table, are less electronegative than the non-metals, so non-metals would be more likely to attract electrons. The size of an atom also contributes to its electronegativity. In smaller atoms, the electrons are closer to their nucleus, which has its own strong attraction to its electrons and to the electrons of the other atom, so they have greater electronegativity.

Smaller atoms have greater electronegativity because their electrons are closer to the nucleus
Smaller Atoms Have Greater Electronegativity

So to summarize this part, the smaller, non-metal atoms have greater electronegativity than the bigger metal atoms. Upper right on the periodic table is more electronegative than the lower left.

Polar and Nonpolar Covalent Bonds

When two atoms that are sharing electrons attract the electrons with the same force, a nonpolar covalent bond is formed. A nonpolar covalent bond is a covalent bond in which the shared electrons are shared equally. A polar covalent bond is a covalent bond in which the shared electrons are more attracted to one of the atoms than the other, thereby forming a polar molecule. The shared electrons are more likely to be near the atom whose electronegativity is higher.

If the difference in electronegativity is too great, the atom in a molecule won't share the electrons. Instead, one atom will take them from the other. When this happens, the bond won't be a covalent bond but rather an ionic bond because the electrons were transferred, or taken from one.

Just remember that electronegativity is only a general guide for what kind of bond is formed, and like all rules, there are exceptions.

Ionic Character

Remember that a covalent bond is when electrons are shared between two atoms. When two different elements are covalently bonded, the electrons aren't shared equally. One of the elements will attract the electron more than the other. This makes it behave a bit like an ionic bond (which is when electrons are transferred between elements).

Covalent bonds behave similarly to ionic bonds; one element attracts electrons more than the other
Ionic Bond Behavior

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