The periodic table arranges elements in horizontal rows called periods and vertical columns called groups. It provides the symbol, name, and proton number of each element. Group 1 elements are alkali metals that react with oxygen and water. Transition metals are hard, colored solids that form complex compounds and are less reactive than alkali metals. The reactivity series lists metals in order of reactivity from most to least reactive. Displacement reactions occur when a more reactive metal displaces a less reactive one from a compound.
2. Periodic table Horizontal rows are called PERIODS Mendeleev The periodic table arranges all the elements in groups according to their properties. Vertical columns are called GROUPS
3. What does the periodic table tell you? The SYMBOL of the element The NAME of the element The PROTON NUMBER of the element Au Gold 79
5. Group 1 – The alkali metals 1) These metals all have to be stored under ____ because they react with _______ Some facts… 2) Reactivity increases as you go _______ the group. This is because the electrons are further away from the _______ every time a _____ is added, so they are given up more easily. 3) They all react with water to form an alkali (hence their name) and __________, e.g: Words – down, oil, shell, hydrogen, nucleus, water Potassium + water potassium hydroxide + hydrogen
6. The Transition Metals 1) This section includes metals like gold, mercury, iron, copper Some facts… 2) They are all ______ and solid (except _________) 3) They are ____ reactive than the alkali metals Words – hard, coloured, mercury, less 4) They can form __________ compounds
7. Some common symbols… Lithium Li Sodium Na Potassium K Calcium Ca Magnesium Mg Iron Fe Oxygen O Nitrogen N Sulphur S Copper Cu Zinc Zn Aluminium Al Gold Au Mercury Hg Fluorine F Chlorine Cl Hydrogen H Helium He
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12. An example question on reactivity Reacts slowly Reacts with steam only Reasonable reaction E Burns brightly Slow reaction Violent reaction D No reaction No reaction No reaction C Reacts slowly No reaction No reaction B Burns brightly Slow reaction Some reaction A Reaction with oxygen Reaction with water Reaction with dilute acid Metal
13. The Reactivity Series The Reactivity Series lists metals in order of reactivity: Potassium Sodium Calcium Magnesium Aluminium Carbon Zinc Iron Lead Copper Silver Gold Increasing reactivity
14. Displacement reactions A displacement reaction is one where a MORE REACTIVE metal will DISPLACE a LESS REACTIVE metal from a compound. Mg Magnesium SO 4 Cu Copper sulphate The magnesium DISPLACES the copper from copper sulphate SO 4 Mg Magnesium sulphate Cu Copper
15. Displacement reactions A displacement reaction is one where a MORE REACTIVE metal will DISPLACE a LESS REACTIVE metal from a compound. For example, if you drop some magnesium into copper sulphate a reaction will happen because magnesium is more reactive than copper, so the reaction is: Magnesium + copper sulphate copper + magnesium sulphate However, if you drop some copper into magnesium sulphate NOTHING will happen.
16. Some example reactions… Extension work – write down the equations for these reactions Copper + silver nitrate Copper + lead nitrate Zinc + lead nitrate Zinc + copper sulphate Observations Prediction Reaction
17. Some example reactions… Extension work – write down the equations for these reactions Reaction DID happen Copper + silver nitrate Reaction DID NOT happen Copper + lead nitrate Reaction DID happen Zinc + lead nitrate Reaction DID happen Zinc + copper sulphate Observations Prediction Reaction
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19. Neutralisation reactions When acids and alkalis react together they will NEUTRALISE each other. Neutralisation is an example of a displacement reaction: OH Na Sodium hydroxide Cl H Hydrochloric acid The sodium DISPLACES the hydrogen from HCl Cl Na Sodium chloride H 2 O Water
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21. Making salts Whenever an acid and alkali neutralise each other we are left with a salt, like a chloride or a sulphate. Complete the following table: Calcium nitrate + water Calcium hydroxide Potassium sulphate + water Potassium hydroxide Sodium chloride + water Sodium hydroxide Nitric acid Sulphuric acid Hydrochloric acid
22. Salts of transition metals These are the TRANSITION METALS – if we make a salt using a base made from one of these metals the procedure is different… 1) Drop the base into the acid… 2) Filter it to remove any leftover base 3) Evaporate it to get the salt
23. Extracting Metals Some definitions: A METAL ORE is a mineral or mixture of minerals from which it is “economically viable” to extract some metal. Most ores contain METAL OXIDES (e.g. rust = iron oxide). To “extract” a metal from a metal oxide we need to REDUCE the oxygen. This is called a REDUCTION reaction.
24. How do we do it? Potassium Sodium Calcium Magnesium Aluminium Carbon Zinc Iron Tin Lead Copper Silver Gold Platinum Increasing reactivity Metals ABOVE CARBON, because of their high reactivity, are extracted by ELECTROLYSIS Metals BELOW CARBON are extracted by heating them with carbon in a BLAST FURNACE These LOW REACTIVITY metals blatantly won’t need to be extracted because they are SO unreactive you’ll find them on their own, not in a metal oxide
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26. The Blast Furnace 1) HAEMATITE (iron ore), limestone and coke (carbon) are fed in here 2) Hot air is blasted in here 3) The carbon reacts with oxygen from the air to form carbon dioxide. 4) The carbon dioxide reacts with more carbon to form carbon monoxide 6) Molten slag (waste) is tapped off here 5) Carbon monoxide reduces iron oxide to iron. The molten iron is tapped off here Iron oxide + carbon monoxide iron + carbon dioxide
27. Electrolysis Molecule of solid copper chloride Molecule of solid copper chloride after being dissolved Chloride ion Copper ion
28. Electrolysis Electrolysis is used to extract a HIGHLY REACTIVE metal. When we electrolysed copper chloride the negative chloride ions moved to the positive electrode and the positive copper ions moved to the negative electrode – OPPOSITES ATTRACT!!! = chloride ion = copper ion
29. Redox reactions These happen during electrolysis: These two processes are called REDOX REACTIONS OILRIG – O xidation I s L oss of electrons R eduction I s G ain of electrons At the positive electrode the negative ions LOSE electrons to become neutral – this is OXIDATION At the negative electrode the positive ions GAIN electrons to become neutral – this is REDUCTION
30. Purifying Aluminium Aluminium has to be extracted from its ore (called ________) by electrolysis. This is because aluminium is very ___________. The ore is mixed with cryolite to lower its ________ ________. The ore is then melted so that the ions can ______. The positively charged aluminium ions gather at the ___________ electrode. Oxygen forms at the positive electrode and causes it to wear away, which means that they have to be __________ frequently. Words – melting point, replaced, negative, bauxite, reactive, move
