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˚