BONDING Flashcards
Ionic bonding
The electrostatic force between positive (cation) and negative (anions) ions
Ionic bonds have
- high melting and boiling points
- High temperature needed to overcome these electrostatic forces of attraction
In ioni bonding melting points are higher for
lattices with greater charges on ions due to the strong attraction between ions
Does not conduct electricity unless
- molten
- or dissolved in a solvent
if ionic bonds are in polar solvents
they break down the lattice and surround each ion in solution
outer shell electrons from a metal are transferred to
the outer shell of a non-metal
Ionic compounds form
Giant ionic lattices
3 key properties of ionic compounds
- High melting and boiling points
- solubility
- does not conduct electricity unless molten or dissolved in polar solvents
the solid state:ionic compounds
- The ions are in a fixed position
- no mobile charge carriers
The liquid state: ionic compounds
- solid ionic lattice breaks down
- The ions are now free to due to there being mobile carriers
Covalent Bonding is
Strong electrostatic attraction between a shared pair of electrons and the nuclei of bonded atom
In covalent bonding
The atrraction is localised between electrons
Diuble covalent bond
electrostatic atttraction between 2 shared pairs of electrons and the nuclei of bonding atoms
Dative covalent bond
a covalent bond in which the shared pair of electrons has been supplied by one of the bonding atoms
Covalent bonding structures
- small covalent structure
- giant covalent structure
- charged polyatomic ion
