2.1.2 Compounds, formulae and equations Flashcards
give the charge of sodium
na+
give the charge of potassium
k+
give the charge of silver
ag+
give the charge of hydrogen
H+
give the charge of ammonium
nh4+
give the charge of copper 1
cu+
give the charge of magnesium
mg+2
give the charge of calcium
ca+2
give the charge of iron 2
fe+2
give the charge of zinc
zn+2
give the charge of lead 2
pb+2
give the charge of copper 2
cu+2
give the charge of nickel 2
ni+2
give the charge of aluminium
al+3
give the charge of chromium 3
cr+3
give the charge of iron 3
fe+3
give the charge of hydroxide
oh-
give the charge of sulphate
so4-2
give the charge of carbonate
co3-2
give the charge of nitrate
no3-
give the charge of hydrogencarbonate
hco3-
give the charge of phosphate
po4-3
give the charge of manganate
mno4-1
give the charge of chromate 4
cro4-2
give the charge of dichromate
cr2o7-2
give the charge of sulphite
so3-2
state the solubility of nitrates
all soluble
state the solubility of sulphates
mostly soluble except for lead sulphate and barium sulphate
state the solubility of chlorides, bromides and iodides
mostly soluble is except for lead and silver halides
state the solubility of carbonates
mostly insoluble except for sodium carbonate and potassium carbonate
state the solubility hydroxides
mostly insoluble except for sodium hydroxide and potassium hydroxide
state the solubility of oxides
all insoluble
acid + alkali =
salt + water
acid + metal carbonate =
salt + water + carbon dioxide
acid + metal oxide =
salt + water
displacement reaction
more reactive metal + less reactive metal compound solution =
more reactive metal compound solution + less reactive metal
precipitation reaction
AX (aq) + BY (aq) =
BX (s) + AY (aq)