1. What can be deduced about two gases that have the same molecular mass?

A They have the same solubility in water at room temperature

B The have the same boiling point

C They have the same number of atoms in one molecule

D They have the same rate of diffusion at room temperature and pressure

2. Which of the following correctly describes the particles in dilute sugar solution at room

temperature?

Sugar molecules Water molecules

A

B

C

D

Widely separated, moving at random

Widely separated, moving at random

Widely separated, not moving

Close together, moving at random

Close together, moving at random

Close together, not moving

Widely separated, moving at random

Widely separated, Moving at random

3. The table shows the melting and boiling points of four pure substances.

At room temperature, which substance is a liquid and rapidly evaporates if left exposed to

air?

Substance Melting points/oC Boiling points/oC

A

B

C

D

-100

-7

-6

44

-35

58

225

280

4. An element X has two isotopes, which may be represented as 238X and 235X

How does 238X differ from 235X

A It has 3 more protons and 3 more electrons

B It has 3 more protons, but no more electrons

C It has 3 more neutrons and 3 more electrons.

D It has 3 more neutrons, but no more electrons.

5. Which graph shows the number of electrons in the outer shell of an atom, plotted against

the proton number for the first ten elements in the periodic table?

6. Which diagram represents the structure of quartz,SiO2?

7. What happens when a copper atom becomes copper(II) ion?

A It is oxidised by losing 2 electrons

B It is oxidised by gaining 2 electrons

C It is reduced by gaining 2 electrons

D It is reduced by losing 2 electons

8. Which compound has both ionic and covalent bonds?

A Ammonium chloride

B Carbon dioxide

C Ethyl ethanoate

D Sodium chloride

9. What is the ratio if the volume of 2g of hydrogen to the volume of 16g of methane, both

volumes at r.t.p

A 1 to 1

B 1 to 2

C 1 to 8

D 2 to 1

10. One mole of an organic compound is completely burnt in oxygen.

Which compound produces exactly three mole of water?

A Butane

B Butanol

C Ethanol

D Propene

11. The reaction between hydrochloric acid and calcium carbonate is shown.

Which volume of 1.0mol/dm3 of hydrochloric acid is needed to react completely with 1.0g of

calcium carbonate?

A 10cm3

B 20cm3

C 100cm3

D 200cm3

12. The diagram shows the electrolysis of aqueous copper(II) sulphate using copper electrodes.

Which graph show how the mass of the cathode changes during elcetolysis?

13. What happens when molten lead(II) chloride is electrolysed?

A Chloride ions gain electrons at the cathode

B Chloride ions lose electrons at the anode

C Lead(II) ions lose electrons at the cathode

D Lead(II) ions move towards the anode

14. What reacts with hydrochloric acid to give hydrogen?

A Ammonia

B Iron

C Silver

D Sodium hydroxide

15. The results of tests on compound X are shown.

test result

Add bromine water

Add aqueous sodium carbonate

Turn colourless

Carbon dioxide formed

What is compound X?

16. When must a substance be an alkane?

A When it burns easily in air and oxygen

B When it contains carbon and hydrogen

C When it has the general formula CnH2n-1

D When it is generally unreactive

17. In which reaction is dilute sulphuric acid is not behaving as an acid

A H2SO4 + 2NaOH Na2SO4 +2H2O

B H2SO4 + BaCl2 BaSO4 + 2HCl

C H2SO4 +CuO CuSO4+ H2O

D H2SO4 + Mg MgSO4 + H2

18. A sample of air is slowly passed through aqueous sodium hydroxide and then over heated

copper.

Which gases are removed by this process?

A Carbon dioxide and water vapour

B Carbon dioxide and oxygen

C Nitrogen and oxygen

D Nitrogen and water vapour

19. Yeast can be used to convert

A Ethanoic acid and oxygen.

B Ethanol and carbon dioxide

C Ethanol and oxygen

D Starch and carbon dioxide

1. The following is a list of formulae of organic compounds.

CH3COOH C2H5 C2H5OH C3H6 C7H14

Which of the above formulae fit the following description?

a) A compound which dissolves in water to form an acidic solution

b) A compound which is not a hydrocarbon

c) Two compounds which are from the some homologus series

d) Two compounds which react to form an ester

e) A compound which undergoes an addition reaction with steam

f) A compound which is oxidised by acidified potassium dichromate(VI) to give

ethanoic acid

2. Two naturally occurring ores of copper are cuprite, Cu2O and tenorite, CuO

a) Give the oxidation state of copper in each ore.

oxidation state of copper in Cu2O

oxidation state of copper in CuO

b) Copper can be extracted from tenorite by heating the ore with powdered carbon.

i. Write an equation for this reaction

ii. Explain, in terms of electrons, why the copper in tenorite has been reduced.

c) A sample of one of the ores was analysed and found to contain 4.48g copper and

1.12g oxygen

Calculate the empirical formula for the copper oxide in the ore and deduce the

name of the ore.

3. Complete the table.

Ion Formula Number of protons

Number of neutrons

Number of electrons

Potassium K+

Oxide O2-

In a sample of 100 atoms of potassium, there are 94 atoms of 39K and 6 atoms of 41K

a) Explain why these two forms of potassium are isotopes

b) Find the total mass of the 100 atoms of potassium. Hence find the average mass of

one atom

4. In separate experiments, powdered samples of metal X and metal Y reacted with solutions

of nickel(II) sulphate and of iron(II)sulphate. The following table shows how the colours of

the solutions changed.

Nickel(II) sulphate Iron(II) sulphate

Metal X Solution goes from green to colourless

Solution stays pale green

Metal Y Solution goes from green to colourless

Solution goes from pale green to colourless

a) Predict the order of reactivity for the four metals, X, Y, nickel and iron

Most reactive

Least reactive

b) Metal Y was placed in aqueous copper(II) sulphate.

i. What colour change was seen?

ii. Give one other observation

c) Write ionic equation, with state symbols, for the reaction between iron and aqueous

nickel(II) sulphate.

5. A metallic element, M, has the following properties

less dense than water soft melts below 100oC occurs naturally as its chloride, formula MCL the oxide of M reacts with water to form a soluble hydroxide

a) Suggest which group of the periodic table metal M belongs.

b) Suggest how metal M can be extracted from its compounds. Explain your reasoning.

c) Outline a method to prepare crystals of MCL, starting with the carbonate, M2CO3

d) 6.72g of MCL contains 1.42g of chlorine.

Calculate the number of moles of chlorine atoms in the sample, and hence suggest a

value for the relative atomic mass of M.