It is 29 pages of GCSE Edexcel chemistry questions. These have been compiled from school and the textbooks supplied for GCSES. Over these 29 pages it covers the topics that will be needed to get a very high grade. In year 10 i was working at a grade 3 but by creating and using these questions I was...
Q1 What are the 4 chemical state symbols
A1 Solid, liquid, gas and aqueous
Q2 What is the chemical formula for A) water, B) carbon dioxide, C)chlorine, D) ammonia, E) hydrogen and F)
oxygen
A2 A) H20 B) CO2 C) Cl2 D) NH3 E) H2 F) O2
Q3 What are the chemical formulas for A) Ammonium B) Nitrate C) Sulphate D) Hydroxide E) Carbonate
A3 A) NH4 + B) N03 - C) SO4 2- D) OH - E) CO3 2-
Q4 What is included in an ionic equation
A4 Only the reacting particles and the products they form.
Q5 What is a hazard
A5 Anything that has the potential to cause harm/damage.
Q6 Describe the gold foil experiment and how it disproved the plum pudding model
A6 Alpha particles were fired at a thin sheet of gold foil
The plum pudding model predicted that all particles would go straight through or be deflected slightly.
Most particles passed through, however a few were deflected further than expected and a small number straight
back.
This suggested most of the atom is empty space with a positive nucleus in the centre.
Q7 An atom of potassium has an atomic number of 19 and a mass number of 39. Give the number of protons,
electrons, and neutrons
A7 Protons = 19, Electrons = 19 and Neutrons = 20
Q8 What are isotopes
A8 Different forms of the same element, which have the same number of protons but a different number of
neutrons.
Q9 What is relative atomic mass
A9 The average mass of one atom of the element, compared to 1/12 of the mass of one atom of carbon – 12.
Q10 Bromine has an atomic number of 35 and two isotopes – Bromine-79 and Bromine-81. Work out the RAM given
51% is bromine-79 and 49% is bromine-81
A10 (79 x 51) + (81 x 49) / 100 = 80
Q11 Give the configuration of aluminium (atomic number = 13)
A11 2:8:3
Q12 In which group and period of the periodic table would an element with the configuration 2:8:8:2 be?
A12 Group 2, Period 4
Q13 Explain why calcium chloride has a high – melting point
A13 A lot of energy is needed to break the strong attraction.
Q14 Explain why oxygen is a gas at room temperature
A14 The intermolecular forces between molecules break easier. This gives oxygen a lower boiling point.
Q15 Explain why nitrogen, doesn’t conduct electricity
A15 They aren’t charged/ don’t contain any free electrons.
Chemicals, particle model and molecules
,Carbon, formulas and RAM
Q1 What are fullerenes
A1 Molecules of carbon shaped like a hollow ball
Q2 What are examples of carbon – based giant covalent
A2 Diamond/ graphite and graphene
Q3 What are the electrons in the metallic bonding like
A3 Delocalised in the outer shell, meaning the are free to move and carry charge.
Q4 What are the physical properties of metals
A4 High melting/ boiling points
Aren’t soluble in water
Denser than non – metals
Malleable
Good conductors of heat and electricity
Q5 What does conservation of mass mean
A5 Mass cannot be created nor destroyed meaning there are the same number of atoms on each side of an
experiment.
Q6 What is relative formula mass
A6 The relative atomic mass of all atoms in a formula added together
Q7 What is empirical formula
A7 The smallest whole number of all atoms empirical formula.
Q8 What is the empirical formula of a compound with the molecular formula C4 H8 Cl2
A8 C2H8Cl
Q9 What is a mole
A9 One mole of atoms or molecules of any substance will have a mass in grams equal to the relative particle
mass of the substance.
Q10 Calculate the number of moles in 90g of water
A10 = 5
Q11 How many molecules are present in 3.5 moles of ammonia gas
A11 3.5 x (6.02 x 10^23) = 2.107 x 10^24
Q12 What is the formula for concentration
A12 Mass of solute / volume of solute
Q13 Calculate the mass of 02 moles of potassium bromide. (Mr of bromide = 119)
A13 0.2 x 119 = 23.8 moles
Q14 0.5 moles of substance x have a mass of 87g. What is the Relative formula mass.
A14 .5 = 174
Q15 What is the unit of measurement for A) Concentration B) Mass C) Volume
A15 A) g/dm^-3 B) g C) Dm^3
Q16 What mass of sodium hydroxide is contained in 200dm^3 of 55gdm^-3 solution
A16 200/1000 = 0.2 0.2 x 55 = 11g
,Q1 What is a limiting reactant
A1 The reactant that is used up in a reaction.
Q2 Describe the arrangement of particles and the forces between them in a solid
A2 Strong forces of attraction
Fixed positions
Definite shape and volume
They don’t have much energy
They only vibrate
Q3 Describe the arrangement of particles and the forces between them in a liquid
A3 Some force of attraction, but they tend to stick together
Don’t have a definite shape
Less energy than a solid
Constantly moving
Q4 Describe the arrangement of particles and the forces between them in a gas
A4 No forces of attraction
No shape or volume
The most energy out of all states
They are constantly moving
Q5 What are the 5 changes of state and what states are they between
A5 Melting: Solid -> Liquid
Freezing: Liquid -> Solid
Evaporating: Liquid -> Gas
Condensing: Gas -> Liquid
Sublimation: Solid -> Gas
Q6 What does purity mean
A6 Made up of a single element or compound.
Q7 Describe the simple distillation practical
A7 Pour the sample into a distillation flask
Set up the apparatus s the condenser connects to the flask and runs to a beaker at the bottom
Gradually heat the flask. The part of the substance with the lowest boiling point will evaporate
The vapor passes into the condenser where it cools and condenses to then flow into the beaker
Either mixture in both flasks will be pure when it stops evaporating
Q8 What is filtration used for
A8 To separate an insoluble solid from a liquid.
Q9 What is crystallisation used for
A9 To separate a soluble solid from a solution.
Q10 In paper chromatography what is the stationary phase
A10 Where the molecules can’t move, this can be a solid or really thick liquid.
Q11 What is the mobile phase
A11 Where the molecules can move, this is always a liquid or gas.
Q12 What is the formula for Rf value
A12 Distance travelled by solute / distance travelled by solvent.
States of matter, and separation methods
, Acids
Q1 What are the colour changes of A) Litmus paper B) Methyl orange C) Phenolphthalein
A1 A) Red in acidic, purple in neutral and blue in alkaline
B) Red in acidic and orange in neutral/ alkaline
C) Colourless in acidic and neutral and pink in alkaline
Q2 What is a strong acid
A2 An acid that ionises almost completely in water.
Q3 What is a weak acid
A3 An acid that does not ionise in a solution.
Q4 What does acid strength measure
A4 The proportion of the acid molecules that ionise in water.
Q5 What does acid concentration measure
A5 How much acid there is in a litre of water – how watered down the acid is.
Q6 What products do you get in the reactions:
A6 Acid + metal oxide -> Salt + water
Acid + metal hydroxide -> salt + water
Acid + metal -> Salt + hydrogen
Acid + metal carbonate -> Salt + water + carbon dioxide
Q7 What is a soluble substance
A7 Dissolves in water
Q8 Given the substances determine if its insoluble or soluble
A8 Common salts of sodium, potassium, and ammonium: Soluble
Nitrates: Soluble
Common Chlorides: Soluble (except silver and lead chloride)
Common sulphate: soluble (except lead, barium, and calcium sulphate)
Common carbonates: Insoluble (except sodium, potassium, and ammonium ones)
Q9 State whether the following salts are soluble or insoluble
A9 Potassium chloride: Soluble
Copper carbonate: Insoluble
Calcium sulfate: Insoluble
Ammonium hydroxide: Soluble
Q10 How do you make an insoluble salt
A10 Use a precipitation reaction. Pick the right two soluble salts and react them together to get the soluble salt.
Q11 How do you make a soluble salt using an acid and base
A11 Heat the acid in a water bath
Add the base to the acid to produce a soluble salt
Filter off the excess solid to get a solution containing only salt and water
Heat the solution gently, to evaporate the water
Leave the solution to cool and crystalise
Filter off the solid salt and leave it to dry
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