everything

acids in water

form hydrogen ions

base

substance that reacts with acid to produce a salt and water

alkali

base that is soluble in water

alkalis in water

form hydroxide ions

indicator

dye that changes colour whether its above or below a neutral ph

litmus

acid - red

alkali - blue

methyl orange

acid - red

alkali - yellow

phenolphthalein

acid - colourless

alkali - pink

neutralisation

reaction between an acid and a base to rpoduce a salt and water

concentration of acid

volume of acid in a litre or water

as the concentration of H+ ions increases by a factor of 10

the ph decreases by 1

acid + metal oxide

salt + water

acid + metal hydroxide

salt + water

acid + metal

salt + hydrogen

acid + metal carbonate

salt + water + carbon dioxide

hydrogen test

hydrogen makes a squeaky pop with a lighted splint

carbon dioxide test

limewater turns cloudy when carbon dioxide is bubbled through

precipitate

solid product of an aq solution

sodium potassium ammonium

soluble

nitrates

soluble

chlorides except silver and lead

soluble

sulfates excpet leadbarium and calcium

soluble

carbonates except sodium potassium and ammonium

insoluble

metal ions

lose electrons

nonmetal ions

gain electrons

stable electronic structure

when atoms gain or lose electrons to get a full outer shell

ionic bond

metal and nonmetal

cation

positive ion

anion

negative ion

electrostatic force

a force of attraction between opposite charges

ions high melting and boiling points

strong attraction between ions

ions conductivity

dont conduct when solid but conduct when in solution

ions solubility

many are soluble

ions structure

ionic lattice

covalent bond

pair of electrons is shared between two atoms

molecule

made up of two atoms held together by covalent bonds

compound

made up of atoms of more than 1 elements chemically joined together

simple molecular (covalent) low melting and boiling points

weak intermolecular forces

simple molecular (covalent) solubility

some are soluble

simple molecular (covalent) conductivity

most dont conduct

polymers

complex molecules made from simple molecules

giant covalent high melting and boiling points

strong covalent bonds

giant covalent solubility

insoluble

giant covalent conductivity

only graphite conducts

giant covalent structure

giant lattice

allotropes

made of the same atom but have different structures

fullerene

molecules made up of carbon

metallic conductivity

delocalised electrons carry electrical charge

metallic high melting and boiling points

strong metallic bond between a positive metal ion and delocalised negative electron

metallic solubility

insoluble