1. Chemistry Unit 1

2. HAZARD SYMBOLS Radioactive Toxic Harmful/irritant
Match the symbol to its correct meaning:
Radioactive
Toxic
Harmful/irritant
Dangerous for the Environment
Oxidising
Corrosive
Highly Flammable
Explosive

3. THE ATMOSPHERE
As we are today, it was not always the case…

4. Water vapour
Carbon dioxide
NO OXYGEN
4.5 BILLION YEARS AGO..

5. AS TIME WENT ON.... 1. Water vapour cooled = OCEANS
2. Carbon dioxide DISSOLVED in oceans
Green plants EVOLVED; released OXYGEN

6. Formation of Rock Type of Rock Formed by Examples Sedimentary
Sediments in water under pressure
Sandstone
Chalk
Limestone
Metamorphic
Sedimentary rock heating, and under pressure
Marble
Slate
Igneous
Molten rock (magma) cooling slowly
Granite
Basalt

7. CHALK
CaCO3
LIMESTONE

8. USES of LIMESTONE:
For buildings
To make cement
The cement can make CONCRETE
Make glass

9. TOPIC: Limestone and Stuff...
Calcium Hydroxide
Ca(OH)2
Calcium Oxide
CaO
CaCO3
Calcium Carbonate
TOPIC: Limestone and Stuff...

10. Thermal Decomposition
CaCO3
CaO
HEAT
+ CO2

11. Test for Carbon Dioxide

12. CaO
QUICKLIME = CaO

13. CaO
WATER
EXPLOSIVE REACTION

14. REMINDER – how are these compounds made?
Calcium heat calcium carbon
Carbonate  oxide dioxide
calcium water calcium
oxide  hydroxide
QUICKLIME
VERY SLOWLY
SLAKED LIME

15. USES OF LIMESTONE PRODUCTS...
Neutralising acidic soils
To remove acidic gases from coal powered stations

16. Making Glass
Glass is made by heating silicon oxide with calcium oxide and sodium carbonate, the calcium oxide makes the glass waterproof (sodium carbonate can let water through glass, but does lower the temperature!)

17. Making Cement, Concrete and Mortar
Cement heat CaCO3 with clay
Mortar mix cement with sand and water
Concrete mix cement with gravel sand and water

18. ACID + ALKALI  SALT + WATER
WHAT HAPPENS WHEN ...
ACID + ALKALI  SALT + WATER
NEUTRALISATION!!

19. Indigestion Treatment
Too much acid in the stomach, needs alkaline indigestion tablets to neutralise it

20. NEUTRALISING ACIDS – KEY POINTS: General reaction for these are:
Only METAL OXIDES, HYDROXIDES and CARBONATES can be used to neutralise acids
General reaction for these are:
Acid + metal OXIDE  SALT + WATER
Acid + metal HYDROXIDE  SALT + WATER
ACID + metal CARBONATE  SALT + WATER + CARBON-DIOXIDE

21. The salt that is formed depends on the acid in the reaction:
Sulphuric acid  Sulphate salts
Nitric acid  Nitrate salts
Hydrochloric acid  Chloride salts

22. Sulfuric acid + Copper Oxide  Copper sulfate + water
Nitric acid Sodium hydroxide  Sodium nitrate + water
Hydrochloric acid + Copper carbonate  Copper chloride water +
Carbon dioxide

23. CLEARING UP AN ACID SPILL..... Using Calcium Carbonate Limestone!

24. ACID RAIN

25. Ca(OH)2
ACIDIC SOIL 
Ca(OH)2
NEUTRALISED SOIL 
Ca(OH)2
Ca(OH)2

26. Breaking stuff* down (*compounds) using electricity
electrolysis
Breaking stuff* down (*compounds) using electricity

27. Where electrolysis happens...
Battery – provides electricity -
Electrode (+)
Anode +
Electrode (-)
Cathode - +
Electrolyte – liquid with compounds (needing breaking)
Cell

28. Compounds the examiners want you to ELECTROLYSIZE....
1. HCl 2. NaCl 3. H2O

29. Electrolysis of liquid NaCl Chlorine: Collected as gas!- + - +
Na+
Cl-
Cl-
Cl-
Na+
Na+
Na+
Cl-

30. Electrolysis of liquid HCl
CHLORINE: Collected as gas!
HYDROGEN: Collected as gas! - + - + H+
Cl-
Cl-
Cl- H+ H+ H+
Cl-

31. OXYGEN: Collected as gas! HYDROGEN: Collected as gas!
Electrolysis of WATER
OXYGEN: Collected as gas!
HYDROGEN: Collected as gas! - + - + H+
O2-
O2-
O2- H+ H+ H+
O2-

32. CHLORINE It is a TOXIC gas USES: Treat water supplies; kills bacteria
Needed to make BLEACH
Make polymer.... POLY(CHLORETHENE) a.k.a PVC

33. CHEMICAL TESTS CHLORINE Bleaches damp LITMUS paper
OXYGEN Relights a glowing splint
HYDROGEN Lighted splint makes a SQUEAKY POP!

34. EXTRACTION of METALS

35. EXTRACTION of METALS
POTASSIUM SODIUM CALCIUM MAGNESIUM ALUMINIUM ZINC IRON TIN LEAD COPPER SILVER GOLD

36. Metals are found as ORES!
POTASSIUM OXIDE SODIUM OXIDE CALCIUM OXIDE MAGNESIUM OXIDE ALUMINIUM OXIDE ZINC OXIDE IRON OXIDE TIN OXIDE LEAD OXIDE COPPER SILVER GOLD
Metals are found as ORES!
Extracted using ELECTROLYSIS
Extracted using CARBON

37. EXTRACTION METHOD 1. CARBON + HEAT
ZINC OXIDE + CARBON  ZINC + CARBON DIOXIDE
IRON OXIDE + CARBON  IRON+ CARBON DIOXIDE
TIN OXIDE + CARBON  TIN + CARBON DIOXIDE
LEAD OXIDE + CARBON  LEAD + CARBON DIOXIDE

38. ELECTOLYSIS – Aluminium Oxide (BAUXITE)

39. PROPERTIES of METALS

40. STRONG
CONDUCTS ELECTRICITY
MALLEABLE (FLEXIBLE)
CONDUCTS HEAT
DUCTILE (WIRES)

41. ALUMINIUM
LOW DENSITY
CORROSION RESISTANT

42. COPPER
STRONG
HIGH Mpt
GOOD CONDUCTOR OF ELECTRICITY

43. GOLD
SHINY
EASY TO SHAPE
AMAZING ELECTRICAL CONDUCTOR
DOES NOT CORRODE

44. Why do metals higher up the reactivity series get more CORROSIVE?
CORROSION
Basically.... It’s when OXYGEN and reacts with metal.
OXIDATION!
Why do metals higher up the reactivity series get more CORROSIVE?

45. Why do metals higher up the reactivity series get harder to PURIFY?
PURIFICATION
Basically.... It’s when OXYGEN is removed from the metal.
REDUCTION!
Why do metals higher up the reactivity series get harder to PURIFY?

46. Rusting.... (corrosion of IRON)
Iron + oxygen  Iron Oxide (rust)

47. IRON
Iron Ore
Heat
Impure (cast) iron

48. Impure iron = BRITTLE PURE iron = TOO SOFT!
Purification
PURE iron = TOO SOFT!

49. PURE iron + (carbon) STEEL (alloy)

50. Alloys

51. Alloys

52. Alloys.... Smart alloys
e.g. Nitinol – nickel and titanium

55. CRUDE OIL A hydro-carbon is.... (2 marks)
A compound made from hydrogen and carbon atoms ONLY

56. FRACTIONAL DISTILLATION
Process of separating hydrocarbons based on different boiling points is called...
FRACTIONAL DISTILLATION

57. As you go up the fractional distillation column the...
Size of the hydrocarbon chains gets smaller
So, the boiling point gets lower
The flammability increases
The liquid gets (viscosity) less viscous

58. Most alkanes are used as fuels to produce useful forms of energy.
BURNING FUELS
Complete combustion
Incomplete combustion
Most alkanes are used as fuels to produce useful forms of energy.

59. When completely burned, alkanes form carbon dioxide and water.
Fuels
When completely burned, alkanes form carbon dioxide and water.
Hydrocarbon + oxygen 
carbon dioxide + water

60. 2. Reducing emissions Power stations burn COAL
(Coal contains SULPHUR), so when it burns it gives out SULPHUR DIOXIDE
When it rains, this makes SULPHURIC ACID, or ACID RAIN
SULPHUR DIOXIDE

61. SOLUTION
SULPHUR DIOXIDE
Ca(OH)2
Ca(OH)2
Neutral

62. COMPLETE combustion – burning fuel with PLENTY of
OXYGEN!

63. Complete the equation... 
Methane + Oxygen  Water + Carbon dioxide
CH4 + O2  H2O + CO2

64. INCOMPLETE combustion – burning fuel with NOT ENOUGH OXYGEN!

65. INCOMPLETE combustion – burning fuel with NOT ENOUGH
OXYGEN!
HYDROCARBON +  CARBON + CARBON DIOXIDE
OXYGEN CARBON MONOXIDE +WATER
Carbon as soot causes asthma, and dirt (smog)
Carbon monoxide ‘clogs’ up red blood cells, can be fatal.

66. Complete the equation... 
Methane + Oxygen CARBON + CARBON DIOXIDE + CARBON MONOXIDE +WATER
Methane +

67. CARBON MONOXIDE Why is it bad for us?
Toxic gas; it is colourless, odourless
 Carbon monoxide combines with haemoglobin; forms carboxy-haemoglobin
Prevents blood carrying oxygen 
 No oxygen reaches cells / no respiration / death

68. TEST FOR ALKANES AND ALKENES
1. ADD BROMINE WATER (brown/orange solution)....
RESULT  ALKANE (SINGLE BOND) - stays brown
RESULT  ALKENE (DOUBLE BOND) -
DECOLOURISED, goes from brown to COLOURLESS

69. CRACKING
What is it?
Breaking long chain hydrocarbons into smaller ones
Why do it?
High demand for shorter chain molecules
Products:
SHORTER chain ALKANE and an ALKENE

70. CRACKING The long hydrocarbons are heated up
so they turn into a gas (VAPOURISED)
They are passed over a catalyst.
THERMAL DECOMPOSITION takes place (They are broken down by the heat!)

71. POLYMERISATION What do we do with the left over alkenes?
Joining lots of monomers (small alkenes) to make very long chains, called polymers

72. POLMER PROBLEMS Not biodegradable
Fill up landfill site (for thousands of years)
Difficult to burn, they give off toxic gases

73. POLYMER USES Poly(ethene) Carrier bags, bottle, cling film
Poly(propene)
Carpets, ropes, furniture
Poly(chloroethene) PVC
Wellies, window frames, wire insulation
Poly(tetrafluoroethene)
PTFE
Non-stick pans, waterproof clothes

74. MONOMER
POLYMER

75. Carbon dioxide from burning fossil fuels causing a “greenhouse” effect
ENVIRONMENTAL ISSUES...
1. Global Warming
Main cause:
Carbon dioxide from burning fossil fuels causing a “greenhouse” effect

76. 2. Acid rain ENVIRONMENTAL ISSUES... Main cause:
sulphur compounds in fuels burning to form sulphur dioxide
nitrogen dioxide from car exhausts
.... dissolves in rainwater to produce an acidic solution

77. Making biofuel.. e.g. Ethanol
Made by fermenting SUGAR CANE and SUGAR BEET
Burns to give carbon dioxide and water
Cars adapted to use mixture of 10% ethanol and 90% petrol
Growing plants use the
carbon dioxide released
when they burn.

78. BIOFUELS PROS: CONS: It is renewable; petrol is finite
Production of BIOFUEL uses CO2 from atmosphere (carbon neutral)
Environmentally friendly
Increased labour – more jobs, tackle poverty
CONS:
Need lots of land to grow fuel
Losing land to grow food
Biodiversity and loss of habitats
Not 100% efficient

79. CLEAR SOLUTIONS

80. PRECIPITATES

81. Remember…
You will be expected to know the formulas’ of common compounds.
You will have to balance equations
You will have to be able to identify hazards, risks, and how to minimise them

82. C H E M I S T R Y
mark