Inorganic Chemistry

Metal oxides and hydroxides reaction with water

salt and water

why are metak oxides classes as bases

they react to neutralise and have pH greater thsn 7

general equations for metal oxides and acids

metal oxide + salt > salt and water

general equation for metal hydroxides and acids

metal hydroxide + acid > salt and water

why are sodium and potassium hyrdoxide different to other metal hudroxides

sodium and potassium hydroxide both soluble and dissolve in water and are called alkali

other metal hydroxides are insoluble and are called base

what is alumina and why is it amphoteric

alumina is al2o3 and can react as both a base and an acid

Bayer process

bauxite ore to al2o3

ore is mixed with sodium hydroxide

solution then cooled and hydrated forming al(oh)3

2al(oh)3 heated at 1000°C to 1200°C forming al2o3+ 3h2o

Hall Heroult

al2o3 to pure al

Electrolysis of alumina in cryolite to reduce melting point to 1200°C

Oxygen formed at positive cathode as negative oxide ions

carbon dioxide produced contributes to global warming

Requires high energy for heating at constant temperature and high electricity to perform electrolysis

Electrolysis of brine to produce naoh

Brine is known as sodium chloride solution

Chloride ions are negative and produced when attracted to positive anode

Hydrogen ions are positive and produced at negative cathode

Sodium hydroxide formed in the solution

sodium hydroxide can be used for making soap explosives and purifying aluminium

chlorine can be used in bleach disinfectants and manufacturing of pesticides

hydrogen used in haber process making ammonia and used as fuel in manufacturing chemicals

Haber Process

Iron is used as it is a transition metal and it is a heterogeneous catalyst used in ammonia production

during adsorption forms dative bonds between nitrogen and iron

during desorption the bonds between nitrogen is weakened snd broken forming nh3

transition metal

element which can form one or more ions with an incomplete d subshell

properties of transition metals

incomplete d subshells

form coloured compounds

variable oxidation states

catalyse reactions

complex ion formation

ligand

ion or molecule attactched to a metal atom through dative bond

complex ion

a central metal atom or ion surrounded by ligands with datice covalent bond

Catalyst

Speeds up rate of reaction while lowering activation energy

Transition metals act as catalysts due to variable oxidation states

Transition metal act as catalyst xue go

homogenous catalyst

Same state as the reactant and is always in aqueous solution

aqueous solution

heterogenous caralyst

different state to reactants