1. Draw the line on your periodic table and answer the questions
Atoms and elements
Metals
Non-Metals
Draw the line on your periodic table and answer the questions

2. Draw the line on your periodic.
Give the names and symbols of 5 metals and 5 non-metals.
Lithium and sodium are in group 1 – find another element in group 1.
Sodium and magnesium are in period 3. Find another element in period 3.
What do you think a group is?
What do you think a period is?
Draw the line on your periodic.
Give the names and symbols of 5 metals and 5 non-metals.
Lithium and sodium are in group 1 – find another element in group 1.
Sodium and magnesium are in period 3. Find another element in period 3.
What do you think a group is?
What do you think a period is?

3. State the position of metals and non-metals in the periodic table.
All (Level 5)
Most (Level 6)
Some ( Level 7)
State the position of metals and non-metals in the periodic table.
Describe the structure of the atom. Including subatomic particles.
Explain how groups and periods help determine the electron structure of the atom.

4. Atoms and elements Mercury – only metallic element liquid at room temp
Bromine – only non-metallic element liquid at room temp.

5. Gases – atoms are further apart.
Atoms and elements
Solids and liquids – atoms are packed closely together. They are heavy for their size.
HIGH DENSITY
Gases – atoms are further apart.
LOW DENSITY

6. Keywords and definitions
Atom
Electron
Element
Neutron
Element symbol
Proton
Your homework is to find out what these terms mean.

7. Everything is made up of atoms

8. Atoms Each element contains only one type of atom. Many lithium atoms.
One lithium atom
Lithium atomic structure (unique)
Each element contains only one type of atom.

9. Nucleus – contain protons and neutrons.
The atom – very small
Shells – contain electrons that spin around the nucleus
Nucleus – contain protons and neutrons.

10. The nucleus is like a football in a football stadium (atom).
Size of the nucleus
The nucleus is like a football in a football stadium (atom).

11. Protons, neutrons and electrons
Subatomic particle
Relative charge
Proton
Neutron
Electron -1 +1
Clues:
Protons are attracted to electrons.
The overall charge of an atom is neutral.

12. Atoms are neutral Element Proton (+) Electron (-) Lithium 3 Magnesium12
Aluminium 13
The number of protons in an atom must be _______ to the number of electrons in an atom. This makes the overall charge of an atom neutral. The number of _______ in an atom does not have to be the same because they have no overall charge.

13. Groups and periods 1 2 3 4 5 1 2 3 4
Periods have elements increasing in atomic number. 5
Groups have elements with similar properties because they have the same number of electrons in their outer shell.

14. Plenary Quick test You will peer assess your work.
What is special about an element?
How are elements arranged in the periodic table?
What are the horizontal rows in the periodic table called?
What are the vertical columns in the periodic table called?
What is the centre part of an atom called?
What particles are found in the nucleus of the atom?
Which particles are found in shells around the nucleus?
What charge do electrons have?
You will peer assess your work.

15. Match the keywords to the definitions
Properties of metals
Literacy starter
Match the keywords to the definitions

16. Match properties of metals to their uses.
All (Level 5)
Most (Level 6)
Some ( Level 7)
Match properties of metals to their uses.
Describe what the different properties mean.
Explain why some metals are more malleable, better conductors or more dense.

17. Use your definition sheet to help you decide which property of metals is useful when making the item on your sheet.
You must write in full sentences explaining your choices.

18. Thermal conductors Metals are good thermal conductors
1. Saucepans are made of copper, iron, steel or aluminium
Metals are good thermal conductors
Most metals have high melting points

19. Ductile Metals are good electrical conductors
Most metals are ductile...
... they can be drawn out into wires
2. Electrical wires are made of copper
Most metals are flexible

20. Flexible Most metals are flexible
3. Springs are usually made of steel (an alloy of iron)
Most metals are flexible

21. Lustrous Metals are lustrous... ... shiny when polished or freshly cut
4. A lot of jewellery is made of gold
... shiny when polished or freshly cut
Most metals are ductile
Most metals are malleable...
... they can be beaten flat into sheets

22. Sonorous Most metals are sonorous...
5. Bells are made of bronze (an alloy of copper and tin) or brass (an alloy of copper and zinc)
Most metals are sonorous...
... they ring when hit, rather than make a dull thud

23. 6. The framework of skyscrapers is made of iron or steel girders
Most metals are strong and can be made into ALLOYS.
Because metals are flexible, buildings with a metal frame have some ‘give’ in them...
... meaning that they survive better during earthquakes
Iron and steel are much lighter than brick or stone so metal-framed buildings can be taller than masonry buildings

24. (The filament glows because it gets very hot – 2000 to 3000 ˚C)
7. The filament in light bulbs is made of tungsten
Metals are good electrical conductors
Most metals have a high melting point
(The filament glows because it gets very hot – 2000 to 3000 ˚C)

25. 8. Saw blades are made of steel
Most metals are hard
The harder the blade is, the less quickly it goes blunt

26. 9. Flashing – the joins on roofs are waterproofed with sheets of lead
Most metals are malleable...
... so the lead flashing can be moulded to the contours of the roof

27. 10. The casing on compasses is made of brass or aluminium
Most metals are NOT magnetic
Only iron, nickel and cobalt (and their alloys) are magnetic
If we made the casing of a compass from a magnetic metal it would shield the compass needle from the Earth’s magnetic field...
... so the compass would not work!

28. Plenary Quick test Roughly what fraction of the elements are metals?
Name the only metal which is not a solid at room temperature.
What does sonorous mean?
Name the properties that are common to all metals.
You will peer assess your work.

29. Properties of non - metals
Literacy starter
Fill in the blanks

30. There 92 naturally occurring elements in the _______ Table:
the majority of these elements are ______
The metals are found on the _____ and the centre of the Periodic Table
Metals share many _________ and chemical properties
_______ is the only metal which is liquid at room temperature
Iron, nickel and ______ are the only elements which are ________
magnetic
left
physical
metals
Periodic
Mercury
cobalt

31. State the properties of non metals.
All (Level 5)
Most (Level 6)
Some ( Level 7)
State the properties of non metals.
Describe the solutions metal and non-metal oxides make form water.
Predict whether a material is a metal or non metal from it’s properties.

32. Keywords and definitions
Heat
Magnetic
Shiny
Brittle
Sonorous
Electricity
Dull

33. Metals and Non-Metals Substance Metal or non-metal? Appearance
Is it flexible or brittle?
Is it hard or soft?
Does it conduct electricity?

34. cannot be bent into shape
They are not malleable
cannot be bent into shape

35. Brittle and dull

36. They do not conduct electricity or heat.
Poor conductors
They do not conduct electricity or heat.

37. Carbon
This is the exception – when carbon is in the form of graphite it does conduct.

38. Acidic or alkaline solutions?
When a metal oxide (iron oxide) dissolves in water it forms alkaline solutions.
When a non-metal oxide (carbon dioxide) dissolves in water it forms acidic solutions.

39. Properties of non-metals?
Insulator
Strong
Low melting point
Sonorous
Properties of non-metals?
Ductile
Low density
Brittle
Forms acidic
solutions
Malleable
High boiling point

40. Plenary
Quick test
Roughly what fraction of the elements are non - metals?
Which non-metal is liquid at room temperature?
Comment on the density of non-metals.
Do non-metals generally conduct electricity?
Which non-metal conducts electricity?
You will peer assess your work.

41. Mixtures
Literacy starter
Reading activity

42. State examples of types of mixtures.
All (Level 5)
Most (Level 6)
Some ( Level 7)
State examples of types of mixtures.
Describe the melting points of mixtures and pure substances.
Explain the properties of unusual elements.

43. Types of mixture
If there are two or more different atoms but they are not combined, they are a mixture of different elements.
If there are two or more different compounds, but they are not combined they are a mixture of compounds.

44. Mixtures and compounds
Mixtures are easy to separate.
Compounds are difficult to separate.
Mixtures do not have a fixed composition.
Compounds have a fixed composition.

45. Sea water
Is a mixture of particles of water, salts and gases. These particles are mixed together but not combined.

46. Rocks
Most rocks contain a mixture of different minerals. Minerals are compounds because they have a fixed composition. The exact proportion of different minerals in each rock differs, and therefore rocks are a mixture of minerals.

47. Air
Air is a mixture of gas particles. It is composed of about 80% nitrogen and 20% oxygen molecules. There are very small amounts of carbon dioxide, water vapour and noble gases.
These particle are mixed together but are not joined. Oxygen is needed for respiration and burning. Nitrogen is used to make fertilisers and explosives. Argon is placed inside light bulbs because it does not react with the filament. Neon is used in lights and barcode readers in shops.

48. Melting points of mixtures
liquid
Butter melting
Temperature (0C)
Solid
Time (mins)
Mixtures do not melt at one temperature. Each part of the mixture melts at its own melting point. Butter is a good example. You can see some parts melting quicker on a warm day.

49. Melting points and boiling points of pure substances.
Pure elements and compounds melt and boil at a particular temperature. The graph shows how when ice is heated it temperature increases.
At 0oC solid ice melts to form liquid water. The temperature stays the same until all the ice has melted. Once it has all melted the temperature increases.

50. Plenary Quick test You will peer assess your work.
Can mixtures be separated easily?
Why is a mixture different to a compound?
Can you have a mixture of compounds?
Do compounds have a fixed composition?
Do mixtures have a fixed composition?
Is sea water a mixture?
What does sea water contain?
What does air contain?
What percentage of air is nitrogen?
What are most rocks a mixture of?
You will peer assess your work.

51. Circle the correct spelling
Filtration and evaporation
Sonorous
Sonourous
Sonirous
Vigorousley
Vigorously
Vigoroucly
Grafight
Graphete
Graphite
Malleable
Malleble
Maleable
Ducteal
Ductile
Ducktile
Dencity
Density
Densite
Particle
Particel
Partical
Alley
Aloy
Alloy
Conductor
Conduckter
Conducter
Electriscity
Electricity
Electrisity
Literacy starter
Circle the correct spelling

52. All (Level 5)
Most (Level 6)
Some ( Level 7)
State two separation techniques needed to separate sand, salt and water.
Describe the terms, soluble, solvent, solute, insoluble, residue, solution.
Explain the term crystallisation and the process of gaining crystals from sea water.

53. Soluble and insoluble
Look at what these pictures show you. Think about what the word SOLUBLE and INSOLUBLE could mean.
Sand and water – sand is insoluble
Salt and water – salt is soluble

54. Filtration is used to separate a solid from a liquid.
In a mixture the constituent parts are not joined together so they can be separated easily.
Filtrate
Residue
Filtration is used to separate a solid from a liquid.

55. To separate a mixture of water, sand and salt.
Separation
Task 1
To separate a mixture of water, sand and salt.

56. Solution, solvent and solute
Solutions of solvents and solutes can be separated by evaporation. If crystals are formed it is called CRYSTALISATION.
If the solute was magnetic (iron), you could use a magnet.

57. Evaporation You will need: Your task:
after evaporation
before evaporation
Your task:
To heat 20cm3 of salt water until all of the water has evaporated. A white solid should remain, this is salt.
You will need:

58. Plenary Quick test In a mixture are constituent parts joined?
In a compound are constituent parts joined?
How should a mixture of solid and liquid be separated?
How can crystals of salt be obtained from a mixture of salt and water?
Which technique could be used to separate a mixture of different coloured dyes?
You will peer assess your work.

59. Match up the keywords to the definitions and pictures.

60. To know what is meant by boiling point.
Lesson Objectives
To know that distillation can be used to separate a liquid from the solids that are dissolved in it.
To know that distillation is a process in which evaporation of a liquid is followed by condensation.
To know what is meant by boiling point.
Level 4
Level 5
Level 6
I still feel unsure. I need some more help to understand.
I feel ok. I need to do some more work to check my understanding.
I am happy and feel I understand and can explain the main points. 60

61. Used to separate a solvent from a solution.
To know that distillation can be used to separate a liquid from the solids that are dissolved in it.
To know that distillation is a process in which evaporation of a liquid is followed by condensation.
To know what is meant by boiling point.
Used to separate a solvent from a solution.
What is coloured ink?
Is ink a single substance?
How can we find this out?
distillation

62. To know what is meant by boiling point.
To know that distillation can be used to separate a liquid from the solids that are dissolved in it.
To know that distillation is a process in which evaporation of a liquid is followed by condensation.
To know what is meant by boiling point.
Keywords: distillation, state, evaporation, boiling point
thermometer
water out
Liebig condenser
distillation flask
impure water
gauze
water in
beaker
tripod
heat
pure water

63. Important Words
Meaning bank
another name for a gas.
the liquid collected from the condenser.
the process of a gas changing to a liquid.
the temperature at which a liquid boils.
the process of a liquid changing to a gas.
the liquid left behind in the distillation flask.
Boiling
Boiling Point
Condensing
Distillate
Residue
Vapour

64. To know what is meant by boiling point.
To know that distillation can be used to separate a liquid from the solids that are dissolved in it.
To know that distillation is a process in which evaporation of a liquid is followed by condensation.
To know what is meant by boiling point.
Keywords: distillation, state, evaporation, boiling point
Distillation -

65. fractional distillation
To know that distillation can be used to separate a liquid from the solids that are dissolved in it.
To know that distillation is a process in which evaporation of a liquid is followed by condensation.
To know what is meant by boiling point.
Keywords: distillation, state, evaporation, boiling point
Fractional distillation – collecting liquids at different
boiling points.
It can be used to separate alcohol and water.
Alcohol boils at 780C, it passes into the condenser where
it forms pure alcohol.
fractional distillation 65

66. Plenary
Distillation SATS questions
You will peer assess your work.

67. To know what is meant by boiling point.
Review Objectives
To know that distillation can be used to separate a liquid from the solids that are dissolved in it.
To know that distillation is a process in which evaporation of a liquid is followed by condensation.
To know what is meant by boiling point.
Keywords: distillation, state, evaporation, boiling point
I still feel unsure. I need some more help to understand.
I feel ok. I need to do some more work to check my understanding.
I am happy and feel I understand and can explain the main points.

68. How soluble are the inks?
Chromatography
Measure the two distances labelled on the diagram.
If finished measure the start to the centre of spot for the other colours.
Numeracy starter
How soluble are the inks?

69. Safely carry out a chromatography practical.
All (Level 5)
Most (Level 6)
Some ( Level 7)
Safely carry out a chromatography practical.
Describe the chromatogram pattern in terms of solubility's.
Calculate the Rf values of the inks you used.

70. Chromatography
Can be used to separate mixture of different coloured dyes. The different dyes have different solubility's.

71. Calculating the Rf value – means ratio of fronts.
Chromatography
Calculating the Rf value – means ratio of fronts.

72. Separating Mixtures - chromatography

73. Rf values Colours of inks found in a black pen.
Distance from start to centre of spot
Distance from start to solvent front
Rf value

74. You will peer assess your work.
Plenary
Which technique could be used to separate a mixture of different coloured dyes? Explain in detail how chromatography works, include Rf values.
You will peer assess your work.

75. Name and number of each atom
Compounds
Formula
Name and number of each atom
CaCO3
CaO
MgCl2
CO2
1x Carbon, 2x Oxygen
H2O
FeS
H2SO4
Numeracy starter
How many atoms?

76. Design a table to record your results
All (Level 5)
Most (Level 6)
Some ( Level 7)
Design a table to record your results
Describe the signs of a chemical reaction.
Explain the term conservation of mass.

77. Compounds
Atoms may form molecules. A molecule consists of two or more atoms joined together.
If the atoms of two or more elements are joined together by chemical bonds, they form molecules of a compound.
If the atoms are of the same element, they form molecules of an element.

78. Forming compounds
During a chemical reaction a new molecular substance is formed.
Reactants
Products
Iron sulphur Iron sulphide
Fe S FeS
A compound has a fixed composition.

79. Forming compounds Watch aluminium iodide being formed.
Burn magnesium to make a new compound.
Look at the sulphur and iron elements, test both with a magnet.
Look at the iron and sulphur compound. Test this with a magnet.

80. Can compounds react?
If a chemical reaction takes place new substances are made.
The things to look out for to show a chemical reaction is occurring.
Temperature change
Gas is produced
Colour change
Bubbles show gas is produced. Some gas escapes into the air so the mass of the product is less.
Heat energy given out

81. Forming compounds
Design a table that will be able to record the names of the elements being used, name of the compound formed, observations and a word equation for the reaction.
Carry out the experiments safely recording accurate results.

82. Plenary You will peer assess your work. What does this represent.
If you saw bubbles in a chemical reaction, what is being made?
What piece of apparatus would you use to find out if temperature had increased?
What are the chemicals at the start of a reaction called?
What are the chemicals made by a chemical reaction called?
How can you tell if a chemical reaction has occurred when iron and sulphur react to form iron sulphide?
Do compounds have a fixed composition?
Can the elements in a compound be separated easily?
You will peer assess your work.

83. Naming compounds Literacy starter
Independent reading activity
Use a dictionary if you need help!

84. Name the compounds formed when elements react.
All
(Level 5)
Most (Level 6)
Some (Level 7)
Name the compounds formed when elements react.
Write a word/ symbol equation.
Balance symbol equations

85. Naming compounds
When atoms of two or more elements join together they form a compound.
If atoms join together in a reaction this can be shown by a word or symbol equation.
Iron sulphur Iron sulphide
Fe S FeS
The names of the compound is given by the two elements that have joined.
oxygen oxide
fluorine fluoride
bromine bromide
iodine iodide
sulphur sulphide

86. Naming simple compounds
It is easy to name simple compounds of metals and non-metals.
Write down the name of the metal
Write down the name of the non-metal but change the ending to “ide.”
1) magnesium 2) oxygen =
magnesium
oxide
1) sodium 2) chlorine =
sodium
chloride
oxygen
calcium
sulphur
silver
bromine
copper
Name of compound
Element 2
Element 1
copper bromide
silver sulphide
calcium oxide

87. Naming more complicated compounds
Many compounds contain more than two elements. Naming them can get complicated but for those containing two elements plus oxygen the name ending usually changes to –ate.
oxygen
bromine
aluminium
sulphur
copper
Element 3
nitrogen
sodium
magnesium nitrate
magnesium
nickel sulphate
nickel
Name of compound
Element 2
Element 1
sodium nitrate
copper sulphate
aluminium bromate

88. Compounds Level 5 – blue Level 6 - red Formula Name the compound CaCO3
CaO
MgCl2
FeS
H2SO4
PbBr
Level 5 – blue
Level 6 - red

89. Reactions
Sodium (Na) reacts with hydrochloric acid (HCl) , it forms sodium chloride (NaCl) and hydrogen gas (H2).
Reactants
Products
Word equation
Sodium and hydrochloric acid
Sodium chloride and hydrogen
Sodium + hydrochloric acid Sodium chloride + hydrogen
Symbol equation
Na + HCl NaCl + H2

90. Iron reacts with oxygen in the air to produce iron oxide.
Reactions
Potassium (K) reacts with chlorine (Cl2) to produce potassium chloride (KCl).
Sodium (Na) reacts with water (H2O) to produce sodium hydroxide (NaOH) and hydrogen gas (H2)
Iron reacts with oxygen in the air to produce iron oxide.
Calcium oxide (CaO) reacts with carbon dioxide to produce calcium carbonate (CaCO3).
Calcium carbonate reacts with water to produce calcium hydroxide Ca(OH)2 and carbon dioxide (CO2).

91. Word and symbol equations
Reactants
Products
Word equation
Symbol equation

92. Firstly you need an equation with the correct “formulae” in………
Firstly you need an equation with the correct “formulae” in………. You’ll probably be given this in the question
Just like this one
Mg + O2  MgO
Then all you do is list the atoms that are involved on each side of the arrow
Mg + O2  MgO Mg O

93. Mg + O2  MgO Mg + O2  MgO 2 Then start balancing:
[1] Just count up the atoms on each side
Mg + O2  MgO Mg O 1 1 2 1
[2] The numbers aren’t balanced so then add “BIG” numbers to make up for any shortages
Mg + O2  MgO Mg O 1 2 2 2 2
And adjust totals

94. WE SAY THAT THE EQUATION IS BALANCED!!
But the numbers still aren’t equal, so add another “BIG” number 2
Mg + O2  MgO Mg O 1 2 2
And adjust totals again
NOW BOTH SIDES HAVE EQUAL NUMBERS OF ATOMS
WE SAY THAT THE EQUATION IS BALANCED!!

95. Try to balance these equations using the same method:
[1] Na + Cl2  NaCl
[2] CH4 + O2  CO2 + H2O
[3] Li + HNO3  LiNO3 + H2
[4] Al + O2  Al2O3

96. How did you get on??
Here are the answers:
[1] 2 Na + Cl2  2 NaCl
[2] CH O2  CO H2O
[3] 2 Li + 2 HNO3  2 LiNO3 + H2
[4] 4 Al + 3 O2  2 Al2O3
HOPE YOU’VE GOT THE IDEA… REMEMBER TO CHECK THAT YOU CAN DO ELECTROLYSIS EQUATIONS TOO

97. Hope that makes things a bit clearer….
Just remember it’s all about balance

98. Plenary You will peer assess your work. Level 5 –
Write the three signs of a chemical reaction.
Name the compound formed when iron reacts with oxygen.
Name the compound formed when Potassium reacts with bromine.
Level 6
Write the compound formed when calcium, carbon can oxygen react.
Write the compound formed when hydrogen reacts with sulphur and oxygen.
Write a word equation for iron and sulphur making iron sulphide.
Level 7
5. Why must there be the same number of atoms on both sides of the equation?
6. Balance the equation Na + Cl NaCl
7. Balance the equation H2 + Cl HCl
8. Balance the equation C + CO CO
Plenary
You will peer assess your work.