Metals Chemistry Notes

Metals Magnesium + oxygen → magnesium oxide White solid produced Magnesium + hydrochloric acid → Magnesium chloride + hydrogen Effervescence, heats up, Mg dissolves Copper sulphate + magnesium → magnesium sulphate + copper Black solid, solution becomes paler blue Group 1: Alkali Metals Group...

Metals Magnesium + oxygen → magnesium oxide White solid produced Magnesium + hydrochloric acid → Magnesium chloride + hydrogen Effervescence, heats up, Mg dissolves Copper sulphate + magnesium → magnesium sulphate + copper Black solid, solution becomes paler blue Group 1: Alkali Metals Group one are the most reactive metals Their reactivity increases down the group (Li→K) They react with water in similar ways: Effervescence Dissolve Move around Sodium also melts. Potassium also self-ignites with a lilac-coloured flame. Reaction taking place: Lithium + Water → Lithium Hydroxide + Hydrogen Reactions With Acids 4 metals are reacted with a strong acid: Ca Violent fizzing, heated up, white solid Cu No visible reaction Mg Effervescence, heats up, dissolved Zn Slight bubbles on surface A metal will only react with an acid if it is more reactive than hydrogen. Reactivity To determine relative reactivity of elements, we carry out displacement reactions. A more reactive metal will displace a less reactive one. CuSO4 FeSO4 MgSO4 ZnSO4 Cu X N N N Fe Y X N N Mg Y Y X Y Zn Y Y N X Pottassium P lease Sulphur S top Calcium C calling Magnesium M e Aluminium A a CARBON C lueless Zinc Z ebra Iron I nstead Tin T ry Lead L earning HDROGEN H ow Copper C opper Silver S aves Gold G gold People P eople Oxidation Oxidation and reduction can be defined in terms of electrons. Oxidation Reduction Is Is Loss of electrons Gaining of electrons E.g. 2Fe2O3 + 3C → 4Fe + 3CO2 Fe3+ + 3e- Iron is reduced because it gains 3 electrons