C5thebicesterschool.org.uk/wp-content/uploads/2015/...C5 . Overview • Spheres of the earth •...
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C5
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Overview
• Spheres of the earth • Covalent Bonding • Dissolving • Precipitation • Ionic formulae • Giant covalent structures
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The Earth is the source of all our materials.
We get things from:
the atmosphere
the lithosphere
the hydrosphere
Chemicals from the Earth’s spheres
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Some of the useful materials we extract from the lithosphere are:
• coal, oil and gas
• aluminium
• zinc
• iron
• copper
• diamond and graphite
• building materials (clay, stone, gravel)
Chemicals from the Earth’s spheres
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Chemicals of the atmosphere
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Air is a mixture of gases including: • non-metal elements (e.g. N2, O2 and Ar) • compounds between non-metal elements (e.g. CO2). These chemicals are molecular. They have low melting and boiling points, so are gases at normal temperatures.
nitrogen (N2) oxygen (O2) argon (Ar) carbon dioxide (CO2)
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Overview
• Spheres of the earth • Covalent Bonding • Dissolving • Precipitation • Ionic formulae • Giant covalent structures
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• Attractive forces between molecules are weak.
• Small molecules are gases or liquids at room temperature.
oxygen (gas)
carbon dioxide
(gas)
attraction between molecules
water (liquid)
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• The bonds inside molecules are strong.
• Water molecules do not fall apart when the liquid boils and turns to steam.
water molecule
water molecule
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How are the atoms in an H2 molecule held together?
• To picture this you need to look at the structure of a hydrogen atom.
• The positively charged nucleus and the negatively charged electron attract each other.
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When two hydrogen atoms approach each other . . .
. . . the electron of one atom and the nucleus of the other atom start to attract each other.
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When the atoms are close, the attractions are so strong that a molecule of hydrogen (H2) is formed.
The atoms are held together by the attractions between the two nuclei and the shared pair of electrons. This is a single covalent bond.
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Chemists draw a line between element symbols to show a covalent bond.
H—H
hydrogen, H2
O O
oxygen, O2
N N
nitrogen, N2
O C O
carbon dioxide, CO2
H
H—C—H
H
methane, CH4
H H
H—C—C—O—H
H H
ethanol, C2H5OH
O H H
water, H2O
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Molecules have a definite shape.
methanol
water ethene
methane
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Chemists have different ways of describing molecules.
molecular formula
displayed formula with lines for covalent bonds
ball-and-stick model
space-filling model
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Overview
• Spheres of the earth • Covalent Bonding • Dissolving • Precipitation • Ionic formulae • Giant covalent structures
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Sun
evaporation
condensation
rain
rivers
weathering of rocks followed by dissolving of soluble salts
solutions of soluble salts and sediment end up in the sea
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+
When NaCl is added to water, the ions are pulled off the crystal structure and they become free to move in the water.
The ions can move independently, so a solution of NaCl in water conducts electricity.
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• A sodium chloride crystal is made up of millions of Na+ and Cl– ions arranged in a regular pattern called a crystal lattice.
• The lattice is responsible for the cubic shape of all sodium chloride crystals.
Crystals of sodium chloride
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Overview
• Spheres of the earth • Covalent Bonding • Dissolving • Precipitation • Ionic formulae • Giant covalent structures
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Overview
• Spheres of the earth • Covalent Bonding • Dissolving • Precipitation • Ionic formulae • Giant covalent structures
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Salts are ionic compounds containing positive and negative ions.
Overall the compound has no charge.
The positive and negative charges of the ions in the formula balance.
sodium ion Na+
chloride ion Cl-
+
sodium chloride NaCl
- + -
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What is the formula for copper(II) hydroxide?
Cu(OH)2
Copper(II) hydroxide
copper ion Cu2+
hydroxide ion OH-
2+
- 2+ - -
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What is the formula for magnesium chloride?
MgCl2
magnesium chloride
magnesium ion Mg2+
chloride ion Cl-
2+
- 2+ - -
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What is the formula for calcium sulfate?
CaSO4
calcium sulfate
calcium ion Ca2+
sulfate ion SO4
2-
2-
2+
2+ 2-
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What is the formula for calcium carbonate?
CaCO3
calcium carbonate
calcium ion Ca2+
carbonate ion CO3
2-
2-
2+
2+ 2-
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What is the formula for iron(III) oxide?
Fe2O3
iron(III) oxide
iron ion Fe3+
oxide ion O2-
3+
2- 3+ 3+ 2- 2- 2-
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Overview
• Spheres of the earth • Covalent Bonding • Dissolving • Precipitation • Ionic formulae • Giant covalent structures
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Other giant covalent structures include diamond and graphite.
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Diamond has carbon arranged so that each atom is attached to its neighbours by four covalent bonds. This is incredibly tough.
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Graphite has carbon atoms arranged in layers. These can easily slip over each other and detach, such as when a pencil line is drawn.
Covalent bonds between carbon atoms in the same layer are strong. Bonds between layers are weak.
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Overview
• Spheres of the earth • Covalent Bonding • Dissolving • Precipitation • Ionic formulae • Giant covalent structures
• Now a Quiz!
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A B
C D
Which of these four diagrams shows the best picture of the type of structure in . . . nitrogen gas?
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A B
C D
Which of these four diagrams shows the best picture of the type of structure in . . . gold?
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A B
C D
Which of these four diagrams shows the best picture of the type of structure in . . . silicon dioxide?
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A B
C D
Which of these four diagrams shows the best picture of the type of structure in . . . potassium chloride?
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A B
C D
Which of these four diagrams shows the best picture of the type of structure in . . . water?