Metals Reactions: Extracting Metals - Chemistry Notes PDF

**[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]**...

**[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 (LiK) 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. CuSO~4~ FeSO~4~ MgSO~4~ ZnSO~4~ ---- --------- --------- --------- --------- 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. 2Fe~2~O~3~ + 3C 4Fe + 3CO~2~ Fe^3+^ + 3e^-^ Iron is reduced because it gains 3 electrons **[Extracting metals]** **Many metals exist in the earth's crust as ores** **An ore is a rock that contains enough compound worth to be extracting** **A few metals are found in their native state (pure metal not bonded to anything)** **These metals are very unreactive e.g. gold platinum** **Extracting metals from their ores depends on their reactivity** **Metals that are less reactive than carbon are extracted by displacement using carbon** **Iron oxide Iron + Carbon dioxide** **This process is known as reduction (removing O~2~)** **For elements more reactive than carbon, they are extracted using electrolysis**