C1.1

C1.1

1. Atoms and Elements
1. Elements
  1. A substance that contains only one type of atom
2. Atoms
  1. An atom is the smallest particle of an element. Their nucleus contains, protons and neutrons. And the whole atom is orbited by electrons
3. All elements can be found in the periodic table
2. Inside atoms
1. Nucleus
  1. Protons
  2. Neutrons
2. Outside nucleus
  1. Electrons
    1. Maximum of 8 per shell
3. Particle charge
  1. Proton = +1
  2. Neutron = 0
  3. Electron = -1
3. Inside compounds
1. Compounds are made up of two or more elements chemically bonded together
2. Ionic bonds
  1. When a metal reacts with a non-metal
  2. Electrons transfer from one shell to another
    1. To gain a full outer shell of 8 electrons
4. Chemical reactions
1. Reactants
2. Products
3. Word equations
  1. e.g. Sodium+Chlorine --> Sodium Chloride
4. Formulae
  1. Tells us the number and type of atoms are joined afterthe reactions
5. Chemical equations
1. Symbol equations
  1. Must be balanced
  2. e.g. for burning titanium
    1. Ti + O2 --> TiO2
2. Atoms cannot be made or lost in chemical reactions
6. Limestone
1. Attractive, durable & strong
2. Acid rain
  1. Calcium carbonate + sulfuric acid --> Calcium sulfate + Carbon dioxide +water
  2. CaCO3 + H2SO4 --> CaSO4 + CO2 + H2O
  3. Sulfur dioxide
3. CaCO3
4. Quarrying
  1. Benefits
    1. Jobs
    2. Valuable products
      1. National income
  2. Problems
    1. Traffic (transport of material)
    2. Takes up land
      1. Picturesque villages / towns
7. The Lime Cycle
1. Calcium oxide
  1. CaCO3(s) --> CaO(s) + CO2(g)
2. Thermal decomposition
  1. When limestone is heated the mass decreases because carbon has been released as a gas which carries some of the mass
3. Making Calcium Hydroxide
  1. CaO(s) + H2O(l) --> Ca(OH)2 (s)
4. Calcium oxide and Calcium hydroxide
  1. Both are alkaline solutions with water
  2. Uses include;
    1. Neutralising excess acidity in lakes and soils
    2. Neutralising acidic waste gases from coal power stations
8. Products from limestone
1. Cement
  1. Powdered clay is added to crushed limestone and heated to 1450C, then add calcium sulfate powder
2. Mortar
  1. Used to secure bricks
3. Concrete
  1. Cement, sand and small stones
4. Thermal decomposition
  1. e.g. CuCO3(s) --> CuO(s) + CO2(g)
9. Magnificent Metals
1. Transition metals are located in the middle of the periodic table
2. Ores
  1. Ores are put into blast furnaces with a more reactive substance and heated
    1. Reactivity series
    2. Leaves ore and releases waste material
    3. e.g. tin oxide + carbon --> tin + carbon dioxide
10. Steel
1. From blast furnace 96% iron and 3% carbon and impurities
2. Cast iron
  1. Re--melting and adding scrap steel
3. Pure iron removes impurities from the blast furnace
4. Alloy
  1. Steel = iron, carbon and sometimes other metals
  2. Steel is harder and less bendy than pure iron because of atom arrangement
5. Low carbon steels are malleable and used from car body panels and food cans
6. Stainless steel
  1. Does not go rusty because they contain chromium atoms
  2. Cutlery, surgical instruments, kitchen appliances

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