Bonding and Structure

Metallic Bonding

Intermolecular Forces of Attraction

Ionic Bonding

Covalent Bonding

Metallic Structures

Ionic Structures

Dipole-dipole

Hydrogen bonds

When Hydrogen bonds with Nitrogen, Oxygen or Flourine

Strongest intermolecular forces

Bonds between polar molecules

London Dispersion Forces

Temporary dipole generated, resulting in electrostatic attraction between σ+ ion of one molecule and σ- ion of another molecule

Force exists in all molecules

Weakest force of attraction

Factors that affect the magnitude of London Forces

Size of the electron cloud

Shape of molecule

Number of Electrons

Attraction between positive end of one permanent dipole of a molecule and the negative end of another permanent dipole of another molecule.

Non-metals bonding with metals

Atoms either lose or gain electrons to attain a noble gas configuration

When a non-metal gains electrons, it is reduced, becoming an anion

Ionic compounds are typically solids under normal conditions.

Ionic bonds are strong #

Lattice-type structure

Every Sodium atom is surrounded by 4 Chlorine atoms, and every Chlorine atom is surrounded by 4 Sodium atoms

Usually occurs when non-metals bond with non-metals

When a metal loses electrons, it is oxidized, becoming a cation

Atoms share electrons to attain a noble gas electron configuration

The ionic bond is due to electrostatic attraction between oppositely charged ions.

A covalent bond is formed by the electrostatic attraction between a shared pair of electrons and the positively charged nuclei.

Bond Strength and Bond Length

There can be single, double, and triple bonds between atoms. An electron pair is involved in a bond.

As bond numbers increase between two atoms, the strength of the bond increases and the length of the bond decreases

Metallic bonding is the electrostatic attraction between the positively charged atomic nuclei of metal atoms and the delocalized electrons in the metal. #

Bonding between metals

Malleable because positive ions are surrounded by electrons all around - 360˚