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Electronegative

An atom which tends to gain electrons and form negative ions during chemical reactions

Polar molecules

Covalent molecules which contain dipoles.

Hydrogen bond

An intermolecular attractive force between hydrogen, when it is covalently bonded to a highly electronegative atom (fluorine, oxygen or nitrogen), and an oxygen, nitrogen or fluorine atom on another molecule.

Covalent bonds

Formed when atoms share electrons to achieve a stable outer shell; a covalent bond is a shared pair of electrons.

Ionic bonds

Bonds formed by the complete transfer of one or more electron from one atom to another, so both achieve a stable outer shell. The positive and negative ions formed are held together by strong electrostatic forces - these are ionic bonds.

Dipoles

Slightly charged regions in covalent molecules which arise because electrons spend more time close to one atom than another

Chemical bonds

The properties of the chemicals which make up all organisms depend on the nature of the chemical bonds which hold them together. Remember that in chemical reactions the electrons are rearranged to ensure that the atoms within the new compound all have a stable outer shell of electrons, giving them the configuration of a noble gas. In summary:

Ionic bonds: Formed by the complete transfer of one or more electrons from one atom to another, so both achieve a stable outer shell. The atoms which lose electrons in an ionic bond form positive ions, and atoms which gain electrons form negative ions. They are held together by strong electrostatic forces between the positive and negative particles to form ionic compounds.

Ionic bonding between sodium and chlorine atoms

Ionic bonding between sodium and chlorine atoms

Covalent bonds: Formed when atoms share electrons to achieve a stable outer shell. A covalent bond is a shared pair of electrons. Covalently bonded atoms form covalent molecules.

Covalent bonding between nitrogen and hydrogen atoms

Covalent bonding between nitrogen and hydrogen atoms

Polar molecules and hydrogen bonds

Many biologically important molecules are covalent, but the negative electrons in covalent molecules are not always evenly distributed. The electrons may spend more time close to one of the atoms than to another, because some atoms are more electronegative than others. As a result, some parts of the molecule will be slightly negative and some slightly positive. The slightly charged regions are called dipoles and the charges are written as δ+ or δ-. When covalent molecules have dipoles they are known as polar molecules.

Polar molecules are held together by electrostatic forces. These are much weaker than ionic bonds, but because they form between all of the molecules in a substance, there are a lot of them and they can have a major effect on the chemistry of the compound.

Hydrogen bonds are the best known example of these dipole:dipole attractive forces. They occur when hydrogen atoms are covalently bonded to extremely electronegative atoms such as oxygen, nitrogen or fluorine. For example, when oxygen and hydrogen are covalently bonded to form a hydroxyl group (-OH), the oxygen always has the greater share of the electrons than the hydrogen and so the molecules have some polar nature.

Organic compounds often contain hydroxyl groups, giving them a polar nature. Hydrogen bonds have a huge influence of the properties of many biologically important molecules including water.