C4 - The Periodic Table

chelskii96
Mind Map by , created over 6 years ago

Chemistry 2013 Mind Map on C4 - The Periodic Table, created by chelskii96 on 04/09/2013.

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chelskii96
Created by chelskii96 over 6 years ago
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C4 - The Periodic Table
1 Atomic Struture
1.1 Protons: positively charged, charge +1, mass 1
1.2 Neutrons: no relative charge, charge 0, mass 1.
1.3 Electrons are negatively charged, charge -1, mass 0.0005
1.4 Atomic Number = number of protons element contains found at the bottom of element on P.T
1.5 Mass Number = total number of protons and neutrons element contains
1.6 Isotopes = same element, same atomic number, different mass number.
2 Electronic Structure
2.1 Compound = two or more elements, chemically combined.
2.2 Chemical formula = symbols of all elements in a compound and number of atoms of each element.
2.3 Electrons occupy shells around the nucleus
2.3.1 first shell can home two electrons.
2.3.2 second and third shells can home up to eight electrons
3 Ionic Bonding
3.1 If an atom loses one or more electrons it becomes a positively charged ion
3.1.1 Hydrogen and metal atoms
3.2 If an atom gains one or more electrons it becomes a negatively charged ion
3.2.1 Non-metal atoms
3.3 Metal reacts with non-metal
3.3.1 Electrons transferred from metal to non-metal
3.3.1.1 Positive metal ions attract negative non-metal ions and form ionic bonds.
3.3.1.1.1 Dot and cross diagrams
4 Ionic Compounds
4.1 Giant ionic lattice
4.1.1 Structure repeated many times
4.1.2 Positive ions strongly attracted to negative ions.
4.2 Ionic bonds need a lot of energy to be broken
4.2.1 High Melting Point.
4.2.2 Can conduct electricity in a molten or liquid solution - ions are free to move around
5 Periodic Table
5.1 horizontal rows = period
5.2 vertical column = group
5.2.1 Elements in a group have similar properties
5.3 number of electron shells occupied = period element is found
5.3.1 Number of electrons in outer shell = group number
6 Covalent Bonding
6.1 two non-metals
6.2 Shared pair of electrons
6.3 Each covalent bond is shown as a straight line in displayed formula
6.4 Weak intermolecular forces
6.5 Low melting point
6.6 Does not conduct electricity
6.7 Shared electrons shown on diagram in shared area between atoms
7 Group One Elements
7.1 React vigorously with water to form alkaline solutions
7.1.1 Stored in oil to keep them away from water and air
7.2 Metal + Water = Metal Hydroxide + Hydrogen
7.2.1 2M + 2H20 = 2MOH + H2
7.3 reactivity increases as you go down the group.
7.4 In water, lithium keeps its shape, potassium and sodium melt and form silver balls
7.4.1 Potassium ignites explosively and burns with a lilac flame
7.4.1.1 Lithium disappears slowly, sodium disappears quickly and potassium disappears very quickly
7.5 Each have one electron in outer shell
7.6 Loss of electron = oxidation
7.6.1 M = (M+) + (e-)
7.7 Densities increase as you go down the group
7.8 Melting points increase as you go down the group
8 Flame Tests
8.1 Lithium burns red
8.2 Sodium burns orange
8.2.1 Potassium burns lilac
9 Group Seven Elements
9.1 Halogens - react with metal to make salts
9.1.1 Chlorine sterilises pools and tap water
9.1.2 Iodine is used as antiseptic on wounds
9.2 Chlorine is a green gas
9.2.1 Group Seven elements react vigorously with Group One
9.2.1.1 Metal Halide clouds produced
9.2.1.2 2M + X2 = 2MX (where M = group one and X = group 7)
9.3 Bromine is an orange liquid
9.4 Iodine is a grey solid
10 Displacement reactions
10.1 A more reactive group 7 will displace a less reactive group 7 from its metal hallide.
10.1.1 X2 + 2MY = Y2 + 2MX where X = group 7 and MY = metal hallide
10.1.1.1 Gain of electron = reduction
10.1.1.1.1 X2 + (2e-) = 2X-)
11 Transition Elements
11.1 between groups 2 and 3
11.1.1 They are all metals
11.1.1.1 Strong, malleable and shiny when cut
11.2 Copper compounds are often blue
11.3 Iron(II) compounds are often light green
11.3.1 Iron(III) compounds are often orangey brown
11.3.1.1 Often used as catalysts, EG: iron is used in the haber process.
11.3.1.2 Thermal Decomposition = substance breaks down to form two or more substances when heated
11.3.1.2.1 Metal carbonate = metal oxide + carbon dioxide
11.3.1.2.1.1 Normally causes a colour change
12 Precipitation reactions
12.1 Copper(II) - blue metal hydroxide precipitate
12.1.1 Iron (II) - grey/green metal hydroxide precipitate
12.1.1.1 Iron (III) - orange/brown metal hydroxide precipitate
13 Metal
13.1 Good conductor of electricity
13.1.1 hard, lustrous, malleable and have tensile strength
13.2 Metallic bonding - strong - high melting and boiling points
13.2.1 Closely packed ions
13.2.2 sea of delocalised electrons
13.2.2.1 Takes a lot of energy to overcome bonds
14 Water Purification
14.1 Water comes from underground aquifers, resevoirs, lakes and rivers.
14.1.1 contains many dissolved substances which need to be removed
14.2 Water can be used in industry as a solvent, a coolant or a cheap raw material
14.2.1 Sulfate ions can be detected by barium chloride solution
14.2.1.1 Sample of water in test tube, barium chloride added
14.2.1.1.1 Sulfate Ions present = white precipitate
14.2.1.1.1.1 Na2SO4 + BaCl2 = 2NaCl + BaSO4
14.2.2 Hallide ions can be detected by silver nitrate
14.2.2.1 Chloride Ions = White precipitate
14.2.2.2 bromide ions = cream precipitate
14.2.2.2.1 NaCl + AgNO3 = NaNO3 + AgCl
14.2.2.3 iodide ions = pale yellow precipitate
14.3 Only 3% of the Earth's water is fresh
14.3.1 Pollutants in water = nitrates, lead compounds and pesticides
14.3.1.1 Distillation can make pure water from sea water but requires lots of energy and is more expensive
14.3.2 Large suspended particles removed by sedimentation
14.3.2.1 Small suspended particles removed by filtration
14.3.2.1.1 chlorination kills microbes in the water

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