Chemical Bonding: Principles, Structures, and Forces

Chemical Bonding

Chemical bonding occurs when two or more atoms are close enough to produce an attractive force between the electrons of individual atoms and the nuclei of other atoms. If this force is strong enough to hold the atoms together, a chemical bond is formed.

Electronegativity and Bond Polarity

Electronegativity is the ability of an atom to attract shared electrons within a covalent bond with another element. The greater the difference in electronegativity between atoms, the more polar the bond will be.

The Octet Rule

Proposed in 1916 by Gilbert Newton Lewis, the octet rule states that atoms tend to gain, lose, or share electrons to achieve a stable electron configuration similar to that of a noble gas. These elements, located on the far right of the periodic table, are chemically inert.

Lewis Structures

Also known as electron dot diagrams, Lewis structures are graphical representations showing the bonds between atoms in a molecule and any existing lone pairs of electrons. These diagrams are used to represent molecules formed by covalent bonds and coordination complexes.

Types of Chemical Bonds

• Metallic Bond: In a metal, bonding electrons are delocalized throughout a structure of atoms.
• Ionic Bond: These consist of electrostatic attraction between electrically charged ions of opposite signs.
• Covalent Bond: These are the forces that hold non-metal atoms together.

Intermolecular Forces

• Hydrogen Bonding: An attractive force between an electronegative atom and a hydrogen atom covalently bonded to another electronegative atom.
• Van der Waals Forces: Attractive or repulsive forces between molecules, or parts of a single molecule, excluding those due to covalent bonds or electrostatic interactions of ions.
• London Dispersion Forces: These result from the attraction between positive and negative induced dipoles in adjacent molecules.