Ionic bonding defition
electrostatic attraction between oppositely charged ion usually between non metal and metal
Cations and anions
oppositely charged
Ionic bonds are formed when electrons are transferred from one sapecies to another forming cations and anions
Non directional bonding
ionic bond happenings in all directions
Melting point In ionic compounds
high melting point as the attraction is very strong and requires lots of energy to overcome
cations
metals lose electrons from outershell forming positively charged cations
Anions
non metals gain electrons into their outer shell forminf negatively charged anions
Giant ionic lattice
formed by ionic compounds
Held together by strong electrostatic attraction between ions in all directions
Regular repeating patterns of alternationg cations and anions
Shape and arraangemetn of lattice depends on sized of ions
melting and boiling point Ionic compounds
ionic compounds are solid at room temperature
Strong electrostatic forces of attraction between oppositely charged ions require large amount of energy to overcome
Strength of ionic bonding increases with ionic charge - higher charge equate higher attraction
Boiling and melting of lattice
Boiling point are higher for lattice that contain higher ionic harge due to stronger attraction between ions - size not a factor
Solubility factors
breaking down ionic lattice
The polar molecules attracting and surrounding the ions
What do polar molecules do in water
brreak down or dirupt the ionic lattice and surround each ion in solution
Delta positive end surround negative anion
Delta negative of polar molecules surround positive cation
How do ionic charge and solubilty interlink
the greater the ionic charge the less soluble an ionic compounds is
General rule although
Electrical Conductivity SOLID
ionic compounds do not conduct electricity when solid
ions are fixed in solid lattice so no mobile charge carriers
electrical conductivity MOLTEN OR AQUEOUS
can conduct as ions are free to move and carry charge
