1
GCSE
HIGHER TIER
TOPIC TEST SERIES
SUBJECT: CHEMISTRY
PAPER: 1
FULL MARKS: 56 marks
Suggested Time: 45 Minutes
1
2
Q.1- (a). The table shows the number of electrons,neutrons and protons in particles
P,Q,R,S,T and V.
PARTICLES Number of Number of Number of
ELECTRONS NEUTRONS PROTONS
P 1 0 1*
Q 3 4 3
R 8 8 8
S 13 14 13
T 18 16 16
V 18 20 20
I. Which particle is negatively charged ion? (1 mark)
Put a cross in the box next to your answer.
A. P
B. S
C. T
D. V
Ii. Which particles are atoms of metals? (1 mark)
Put a cross in the box next to your answer.
A. P and R
B. Q and R
C. Q and S
D. Q,S and V
(b). Each element has an atomic mass number.
I. State what is meant by atomic mass number. (1 mark)
Ii. The atomic mass number of boron is 5.
2
3
Boron exists as two isotopes boron-10 and boron-11.
Use this information to explain why boron-10 and boron-11 are isotopes.(2 marks)
(c)Explain what is meant by the term relative atomic mass. (2 marks)
Q.2- (a). an atom of iron has an atomic number of 26 and a mass number of 56.
I. Complete the table to show the numbers of protons,neutrons,and electrons in this
atom of copper. (2 marks)
PARTICLE NUMBER
proton
neutron
electron
Ii. Iron is in period 4 of the periodic table.
State what information this gives about the number of shells that contain
electrons,in a copper atom. (1 mark)
Iii.Ferrum exists as isotopes.
Explain what is meant by the term isotopes. (2 marks)
Iv. A sample if Fe contains- (3 marks)
5.84% of iron-54 atom
91.76% of iron 56 atom
3
4
2,12% of iron 57 atom
0.28% of iron 58 atom.
Use this information to calculate the relative atomic mass of iron in this sample.
Relative atomic mass of iron=
(b). copper nitrate contains copper ions,��2+ ,and nitrate ions N�−
3.
I. Describe in terms of electrons how a copper atom,Cu,becomes a copper ion ��2+ .
(2 marks)
Ii. Write the formula of copper nitrate. (1 mark)
Q.3- an element M has the electron distribution 2+8+18+2
(a) . which group in the periodic table is element M likely to be in? (1 mark)
(b) . Predict whether element M is a poor or a good conductor of electricity. Give
reasons for your answer. (1 mark)
(c) Binary compounds contain two atoms per molecule,for example HCL. Identify an
element which could form a binary compound with element M. (1 mark)
(d) . Predict the formula of the carbonate of M.The formula of the carbonate ion is
��23 . (1 mark)
4
5
Q.4- for each of the following,name an element which matches the description.
(a) It is used as a fuel in nuclear reactors. (1 mark)
(b) It is the only non-metal which is a good conductor of electricity. (1 mark)
(c) Inert electrodes are made from this metal. (1 mark)
(d) This gaseous element is used to fill balloons in preference to hydrogen. (1 mark)
(e) An element which can form an ion of the type �3− . (1 mark)
(f) It has the same electrons distribution as the calcium ion,��2+ . (1 mark)
(g) The element is in period 5 and group IV. (1 mark)
Q.5- Use your copy of the periodic table to help your answer these question.
(a) Predict the formulas of each of the following compounds.
I. Barium oxide: (1 mark)
II. Boron oxide: (1 mark)
(b) Give the formulas of the following ions.
I. Sulphide: (1 mark)
II. Gallium: (1 mark)
5
6
(c) Draw a diagram showing the arrangement of the valency electrons in one of
molecule of the covalent compound nitrogen trichloride. (3 marks)
Use x to represent an electron from nitrogen atom.
Use o to represent an electron from a chlorine atom. (3 marks)
(d) Potassium and vanadium are elements in period IV.
I. State two differences in their physical properties. (2 marks)
Ii. Give two differences in their chemical properties. (2 marks)
(e) Fluorine and Astatine are halogens.use your knowledge of the other halogens to
predict the following.
I. The physical state of fluorine at r.t.p
The physical state of astatine at r.t.p. (2 marks)
Ii.Two similarities in their chemical properties. (2 marks)
6
7
Q.6- In periodic table,the elements are arranged in columns called groups and in
rows called Periods.
(a) I.Complete the table for some of the elements in period 3. (2 marks)
GROUP I II III IV V VI VII
NUMBER
symbol Na Mg Al Si P S Cl
Number of
Valency
electron
valency
Ii. What is the relationship between the group number and the number of valency
electrons? (2 marks)
Iii. Explain the relationship between the number of valency electrons and the
valency for the elements Na to Al. (4 marks)
For the elements P to Cl.
(b) across a period,the elements change from metallic to non-metallic.
I. Describe how the type of oxide changes across this period. (2 marks)
Ii.Describe how the type of bonding in the chlorides formed by these elements
changes across the period. (2 marks)
