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41658
C4 - The Periodic Table
Description
Chemistry 2013 Mind Map on C4 - The Periodic Table, created by chelskii96 on 09/04/2013.
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chemistry 2013
chemistry 2013
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chelskii96
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chelskii96
over 11 years ago
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Resource summary
C4 - The Periodic Table
Atomic Struture
Protons: positively charged, charge +1, mass 1
Neutrons: no relative charge, charge 0, mass 1.
Electrons are negatively charged, charge -1, mass 0.0005
Atomic Number = number of protons element contains found at the bottom of element on P.T
Mass Number = total number of protons and neutrons element contains
Isotopes = same element, same atomic number, different mass number.
Electronic Structure
Compound = two or more elements, chemically combined.
Chemical formula = symbols of all elements in a compound and number of atoms of each element.
Electrons occupy shells around the nucleus
first shell can home two electrons.
second and third shells can home up to eight electrons
Ionic Bonding
If an atom loses one or more electrons it becomes a positively charged ion
Hydrogen and metal atoms
If an atom gains one or more electrons it becomes a negatively charged ion
Non-metal atoms
Metal reacts with non-metal
Electrons transferred from metal to non-metal
Positive metal ions attract negative non-metal ions and form ionic bonds.
Dot and cross diagrams
Ionic Compounds
Giant ionic lattice
Structure repeated many times
Positive ions strongly attracted to negative ions.
Ionic bonds need a lot of energy to be broken
High Melting Point.
Can conduct electricity in a molten or liquid solution - ions are free to move around
Periodic Table
horizontal rows = period
vertical column = group
Elements in a group have similar properties
number of electron shells occupied = period element is found
Number of electrons in outer shell = group number
Covalent Bonding
two non-metals
Shared pair of electrons
Each covalent bond is shown as a straight line in displayed formula
Weak intermolecular forces
Low melting point
Does not conduct electricity
Shared electrons shown on diagram in shared area between atoms
Group One Elements
React vigorously with water to form alkaline solutions
Stored in oil to keep them away from water and air
Metal + Water = Metal Hydroxide + Hydrogen
2M + 2H20 = 2MOH + H2
reactivity increases as you go down the group.
In water, lithium keeps its shape, potassium and sodium melt and form silver balls
Potassium ignites explosively and burns with a lilac flame
Lithium disappears slowly, sodium disappears quickly and potassium disappears very quickly
Each have one electron in outer shell
Loss of electron = oxidation
M = (M+) + (e-)
Densities increase as you go down the group
Melting points increase as you go down the group
Flame Tests
Lithium burns red
Sodium burns orange
Potassium burns lilac
Group Seven Elements
Halogens - react with metal to make salts
Chlorine sterilises pools and tap water
Iodine is used as antiseptic on wounds
Chlorine is a green gas
Group Seven elements react vigorously with Group One
Metal Halide clouds produced
2M + X2 = 2MX (where M = group one and X = group 7)
Bromine is an orange liquid
Iodine is a grey solid
Displacement reactions
A more reactive group 7 will displace a less reactive group 7 from its metal hallide.
X2 + 2MY = Y2 + 2MX where X = group 7 and MY = metal hallide
Gain of electron = reduction
X2 + (2e-) = 2X-)
Transition Elements
between groups 2 and 3
They are all metals
Strong, malleable and shiny when cut
Copper compounds are often blue
Iron(II) compounds are often light green
Iron(III) compounds are often orangey brown
Often used as catalysts, EG: iron is used in the haber process.
Thermal Decomposition = substance breaks down to form two or more substances when heated
Metal carbonate = metal oxide + carbon dioxide
Normally causes a colour change
Precipitation reactions
Copper(II) - blue metal hydroxide precipitate
Iron (II) - grey/green metal hydroxide precipitate
Iron (III) - orange/brown metal hydroxide precipitate
Metal
Good conductor of electricity
hard, lustrous, malleable and have tensile strength
Metallic bonding - strong - high melting and boiling points
Closely packed ions
sea of delocalised electrons
Takes a lot of energy to overcome bonds
Water Purification
Water comes from underground aquifers, resevoirs, lakes and rivers.
contains many dissolved substances which need to be removed
Water can be used in industry as a solvent, a coolant or a cheap raw material
Sulfate ions can be detected by barium chloride solution
Sample of water in test tube, barium chloride added
Sulfate Ions present = white precipitate
Na2SO4 + BaCl2 = 2NaCl + BaSO4
Hallide ions can be detected by silver nitrate
Chloride Ions = White precipitate
bromide ions = cream precipitate
NaCl + AgNO3 = NaNO3 + AgCl
iodide ions = pale yellow precipitate
Only 3% of the Earth's water is fresh
Pollutants in water = nitrates, lead compounds and pesticides
Distillation can make pure water from sea water but requires lots of energy and is more expensive
Large suspended particles removed by sedimentation
Small suspended particles removed by filtration
chlorination kills microbes in the water
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