Polarity & Dipole Moments Electronegativity is the ability of an atom to draw a pair of electrons towards itself in a covalent bond Electronegativity increases across a Period and decreases goi...
Hydrogen Bonding Hydrogen bonding Hydrogen bonding is the strongest form of intermolecular bonding Intermolecular bonds are bonds between molecules Hydrogen bonding is a type of permanent dipole – ...
Covalent Bonding: Bond Energy & Length Bond energy The bond energy is the energy required to break one mole of a particular covalent bond in the gaseous states Bond energy has units of kJ mol-1...
Covalent Bonding: Orbitals & Hybridisation Bond overlap in covalent bonds A single covalent bond is formed when two nonmetals combine Each atom that combines has an atomic orbital containing a ...
Dative Bonding: Definition & Examples In simple covalent bonds the two atoms involved shares electrons Some molecules have a lone pair of electrons that can be donated to form a bond with an el...
Covalent Bonding: Definition & Examples Covalent bonding occurs between two nonmetals A covalent bond involves the electrostatic attraction between nuclei of two atoms and the bonding electrons...
Metallic Bonding: Definition Metal atoms are tightly packed together in lattice structures When the metal atoms are in lattice structures, the electrons in their outer shells are free to move throu...
Ionic Bonding: Examples Sodium chloride Sodium is a Group 1 metal It loses its outer electron to form a sodium ion with a +1 charge (Na+) Chlorine is a Group 7 non-metal It gains 1 electron to form...
Ionic Bonding: Definition As a general rule, metals are on the left of the Periodic Table and nonmetals are on the right-hand side Ionic bonding involves the transfer of electrons from a metallic e...
