A covalent bond is formed when two atoms share a pair of electrons. Covalent bonding occurs in most non-metalelements, and in compounds formed between non-metals.
These shared electrons are found in the outer shells of the atoms. Usually each atom contributes one electron to the shared pair of electrons.
The slideshow shows how a covalent bond forms between a hydrogen atom and a chlorine atom, making hydrogen chloride.
Properties of Covalent Bonds
Covalent bonds between atoms are very strong
When two or more atoms are chemically bonded together, they form ‘molecules’
Covalently bonded substances may consist of small molecules or giant structures
Weak intermolecular forces exist between individual molecules
Shared electrons are called bonding electrons and occur in pairs
Electrons on the outer shell which are not involved in the covalent bond(s) are called non-bonding electrons (or lone pairs)
Simple covalent molecules do not conduct electricity as they do not contain free electrons
Limitations of Models for Simple Covalent Molecules
Dot and Cross Diagrams
Advantages:
Useful for illustrating the transfer of electrons
Indicates from which atom the bonding electrons come from
Disadvantages:Fails to illustrate the 3Darrangements of the atoms and electron shells
Doesn’t indicate the relative sizes of the atoms
Ball and Stick Model
Advantages:
Useful for illustrating the arrangement of atoms in 3D space
Especially useful for visualizing the shape of a molecule
Disadvantages:
Fails at indicating the movement of electrons
The atoms are placed far apart from each other, which in reality is not the case as the gaps between atoms are much smaller
2D Representations of MoleculesAdvantages:
Displayed formulae are 2D representations and are basically simpler versions of the ball and stick model
Adequately indicate what atoms are in a molecule and how they are connected
Disadvantages:
Fail to illustrate the relative sizes of the atoms and bonds
Cannot give you an idea of the shape of a molecule and what it looks like in 3D space