Edexcel Igcse Chemistry

Front 1

Chemistry

Back 1

Unit 1: States of Matter, Atomic Structure, Ionic and Covalent Bonding, The Reactivity Series, Extraction of Metals

Unit 2: Acids & Alkalis, Salts, and Rates of Reaction

Unit 3: The Chemistry of Group 1 and Group 7 elements

Unit 4: Bonding; Mole calculations; Equilibria; Contact and Haber processes

Unit 5: Organic Chemistry, Energetics

Unit 6: Electrolysis, Industrial Production of Chemicals, Tests for Ions, Final Calculations

Front 2

Unit 1

Back 2

States of Matter, Atomic Structure, Ionic and Covalent Bonding, The Reactivity Series, Extraction of Metals

Front 3

1.1: understand the arrangement, movement and energy of the particles in each of the three states of matter: solid, liquid and gas

Back 3

Solids: Particles are touching, vibrate, low energy

Liquids: Particles touch, they move to fill gaps, some energy

Gas: Particles aren't touching, move freely, high energy

Front 4

1.2: understand how the interconversions of solids, liquids and gases are achieved and recall the names used for these interconversions

Back 4

Solid → Gas: increase in heat

Gas → Solid: decrease in heat

Front 5

1.3: explain the changes in arrangement, movement and energy of particles during these interconversions

Back 5

The more heat, the more energy

Front 6

1.4: describe and explain experiments to investigate the small size of particles and their movement including:

- dilution of coloured solutions

- diffusion experiments

Back 6

Dilution: a substance is put in a solvent to reduce its concentration

Diffusion: The movement of particles from an area of high concentration to an area of low concentration

Front 7

Diffusion

- Hydrochloric acid is put at one end of a tube, ammonia solution at the other

- A white ring of ammonium chloride appears where the gases meet

- Ring is closer to the HCL end

- Ammonia must have travelled faster, it got further

- Lighter particles move faster, ammonia is lighter

Back 7

Front 8

Dilution

- Put a coloured substance in water

- The colour will be lighter (diluted by the water)

- Dilution happens quicker higher temperature because of the energy in the particles

- So applying heat decreases the amount of time taken for the coloured substance to be fully diluted

Front 9

1.5: understand the terms atom and molecule

Back 9

An atom is made up of a nucleus (protons and neutrons) and orbitals with electrons on.

A molecule is two or more atoms bonded together.

Front 10

1.9: understand that atoms consist of a central nucleus, composed of protons and neutrons, surrounded by electrons, orbiting in shells

Back 10

- The protons and neutrons in the centre make up the nucleus

- The electrons are orbiting in shells (or orbitals)

Front 11

1.10: recall the relative mass and relative charge of a proton, neutron and electron

Back 11

Relative charge

Proton: +1

Neutron: No charge

Electron: -1

Relative mass

Proton: 1

Neutron: 1

Electron: 1/1836

Front 12

1.11: understand the terms atomic number, mass number, isotopes and relative atomic mass (Ar)

Back 12

Atomic number: number of protons (the same as number of electrons)

Mass number: number of protons + neutrons

Isotopes: Atoms of an element with different numbers of neutrons

Relative atomic mass (Ar): the mass of one atom of an element.

Front 13

1.13: understand that the Periodic Table is an arrangement of elements in order of atomic number

Back 13

Every atom in an element has the same atomic number.

Front 14

1.14: deduce the electronic configurations of the first 20 elements from their positions in the Periodic Table

Back 14

Groups are colmns in the periodic table; the group number represents the number of electrons on the outer shell.

Periods are rows on the periodic table; the row corresponds with number of shell.

So if you have an element on the third row down in group seven: it will have three shell and 7 electrons on its outer shell.

Front 15

1.15: deduce the number of outer electrons in a main group element from its position in the Periodic Table

Back 15

The groups (that's going down the periodic table) tell you how many electrons are on the outer shell.

Also note that the periods (going across) tell you the number of orbitals the atom has.

Front 16

1.30: recall the charges of common ions in this specification

Back 16

Front 17

1.21: write word equations and balanced chemical equations to represent the reactions studied in this specification

Back 17

Word equations have just the names of the reactants and products involved: Hydrogen + Oxygen > Water

Balanced equations are the symbols of the products and reactants including the numbers of each, there must be an equal number of each element on both sides of the equation, if there are not you can alter this by putting the right number infront of a symbol: 2H + O > H2O

Front 18

1.22: use the state symbols (s), (l), (g) and (aq) in chemical equations to represent solids, liquids, gases and aqueous solutions respectively

Back 18

(S) solid

(L) liquid

(G) gas

(Aq) aqueous/ solid dissolved in liquid

Front 19

2.30: describe how reactions with water and dilute acids can be used to deduce the following order of reactivity: potassium, sodium, lithium, calcium, magnesium, zinc, iron and copper

Back 19

potassium, sodium, lithium and calcium all react with water and acidsmagnesium, zinc and iron all react with acids (and very slowly with water.)

copper doesn't react with either.

The more vigorous the reaction the more reactive the metal. The more things a metal will react with, the more reactive the metal.

Front 20

2.32: understand oxidation and reduction as the addition and removal of oxygen respectively

Back 20

Oxidation is the gain of oxygen

Reduction is the loss of oxygen

Front 21

2.31: deduce the position of a metal within the reactivity series using displacement reactions between metals and their oxides, and between metals and their salts in aqueous solutions

Back 21

A metal oxide or a metal salt dissolved in water:

- introduce a more reactive metal and it will displace the current one

- introduce a less reactive metal and no displacement will take place

From this you can deduce which metals are more and less reactive.

Front 22

2.29: understand that metals can be arranged in a reactivity series based on the reactions of the metals and their compounds: potassium, sodium, lithium, calcium, magnesium, aluminium, zinc, iron, copper, silver and gold

Back 22

Front 23

1.29: understand oxidation as the loss of electrons and reduction as the gain of electrons

Back 23

Oxidation

Is

Loss (of electrons)

Reduction

Is

Gain (of electrons)

Front 24

2.33: understand the terms: redox, oxidising agent, reducing agent

Front 25

5.1: explain how the methods of extraction of the metals in this section are related to their positions in the reactivity series

Front 26

5.4: describe and explain the main reactions involved in the extraction of iron from iron ore (haematite), using coke, limestone and air in a blast furnace

Front 27

2.34: describe the conditions under which iron rusts

Front 28

2.35: describe how the rusting of iron may be prevented by grease, oil, paint, plastic and galvanising

Front 29

2.36: understand the sacrificial protection of iron in terms of the reactivity series

Front 30

5.1: explain how the methods of extraction of the metals in this section are related to their positions in the reactivity series

Front 31

5.4: describe and explain the main reactions involved in the extraction of iron from iron ore (haematite), using coke, limestone and air in a blast furnace

Front 32

2.34: describe the conditions under which iron rusts

Front 33

2.35: describe how the rusting of iron may be prevented by grease, oil, paint, plastic and galvanising

Front 34

2.36: understand the sacrificial protection of iron in terms of the reactivity series