2.1-2.9

the electrostatic attraction between oppositely charged ions. mostly happens between metals and non-metals

hydroxide: OH^- nitrate NO3 ^- sulphate: SO4 ^2- Carbonate: CO3 ^2- hydrogen carbonate: HCO3 ^- Ammonium: NH4 ^+ Phosphate- PO4 ^3-

the symbol goes in the centre, draw the outer shell with dots and crosses put in a bracket with the charge by the top right corner and the ratio number next to the bottom right corner

the number of oppositely charged ions surrounding one ion in an ionic lattice structure

they have strong electrostatic forces of attraction which require lots of energy to break.

they are very brittle. any dislocation causes alike charges to be next to each other. these repel causing a fracture

only soluble in polar solvents. Solubility depends on the balance between the attraction of the oppositely charged ions to each other and the attraction of the separate ions to the solvent

only conductive when aqueous of molten. the ions need to be free to move but they are stuck in place when solid

the electrostatic force of attraction between the nucleus and the shared pair of electrons. only happens between non-metals

when atoms move electrons to an unoccupied orbital in the same energy level to form more covalent bonds

when one atom donates both electrons in a covalent bond.

it intermolecular forces are weak so very little energy is needed to separate the molecules

they don’t conduct electricity because there are no free ions or electrons

depends on the polarity. tend not to be soluble in water

a measure of the attraction between a bonded atom and the pair of electrons in the covalent bond

nuclear charge- higher charge causes a stronger attraction atomic radius- closer to the nucleus causes a stronger attraction shielding- more shielding causes more repulsion so the attraction is weaker

it decreases. the atomic radius and shielding increases. this causes a weaker attraction to the bonding electrons

it increases. the atomic radius decreases and the nuclear charge increases. this causes a stronger attraction to the bonding electrons.

the electrostatic force of attraction between metal cations and a sea of delocalised electrons.

they have a higher density. this is because the cations are packed together tightly

it’s very high. the attraction between cations and sea of electrons is very strong so lots of energy is required

they are insoluble. the attraction between metal cations and electrons is much stronger than the attraction between water and metal cations

its increases due to the atomic radius decreasing and the number of delocalised electron per atom increasing. the strength of attraction between electrons and metal cations increases so more energy is needed.

it decreases due to the atomic radius and shielding increasing. this makes the attraction weaker so less energy is required.