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CHEMISTRY TERM 1 2022 TESTS (FEB & MARCH)

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Published by nurulhannahariffin, 2022-04-10 00:08:50

CHEMISTRY TERM 1 2022 TESTS (FEB & MARCH)

CHEMISTRY TERM 1 2022 TESTS (FEB & MARCH)

1

SEKOLAH MENENGAH SAYYIDINA ALI INTERNAL EXAMINATION
Year 10 SIMULATION TEST 2022

CANDIDATE
NAME

YEAR

CHEMISTRY 5070 / 22
Paper 2 Theory Term 1 2022
45 minutes
Candidates answer on the Question Paper.
No Additional Materials are required.

INSTRUCTIONS
● Answer all questions.
● Use a black or dark blue pen. You may use an HB pencil for any diagrams or graphs.
● Write your name and year in the boxes at the top of the page.
● Write your answer to each question in the space provided.
● Do not use an erasable pen or correction fluid.
● You may use a calculator.
● You should show all your working and use appropriate units.

INFORMATION
● The total mark for this paper is 43.
● The number of marks for each question or part question is shown in brackets [ ].
● The Periodic Table is printed in the question paper.

For Examiner’s Use
out of

43

This paper consists of 12 printed pages

2
1. Choose from the list of oxides to answer the questions.

Calcium oxide
Carbon dioxide
Copper (II) oxide
Silicon (IV) oxide
Sodium oxide
Sulfur dioxide
Sulfur trioxide

Zinc oxide
Each oxide can be used once, more than once or not at all.
Identify which oxide:
(a) Has a giant covalent structure

______________________________________________________________ [1]
(b) Reacts with acids and with alkalis

______________________________________________________________ [1]
(c) Contains a cation with a charge of +1

______________________________________________________________ [1]

[Total: 3]

3

2. Atoms and ions contain protons, neutrons and electrons.

(a) Complete Table 2.1.

Table 2.1

Proton Relative charge Relative mass
+1 1

Neutron

Electron

[3]

(b) Table 2.2 shows some information about six particles.

Table 2.2

Particle Number of protons Number of neutrons Number of electrons

A 37 48 37

B 53 74 54

C 92 143 92

D 92 143 89

E 92 146 92

F 94 150 92

(i) Deduce the nucleon number for particle A.
_________________________________________________________ [1]

(ii) Explain why particle B is a negative ion.
_________________________________________________________
_________________________________________________________ [1]

(iii) Identify two atoms that are isotopes of same element.
_________________ and _________________

Explain your answer.
_________________________________________________________
_________________________________________________________ [2]

[Total: 7]

4

3. Salts can be prepared by the reaction of acids with bases or alkalis and also by

precipitation reactions.

Aqueous sodium sulfate is used to prepare barium sulfate in a precipitation

reaction.

Ba2+ (aq) + SO42- (aq) BaSO4 (s)

In an experiment 20.0 cm3 of 0.550 mol/dm3 of barium nitrate is added to an excess

of sodium sulfate.

(a) Calculate the maximum mass of barium sulfate that could be made.
[Mr: BaSO4, 233]
Show your working.

Maximum mass of barium sulfate = ____________________ g [2]

(b) A mass of 1.92 g of dry barium sulfate is obtained.
Calculate the percentage yield of barium sulfate.

Percentage yield of barium sulfate = ______________________ % [1]
[Total: 3]

5

4. Calcium chloride, CaCl2, is an ionic compound.
(a) Deduce the electronic configuration for each of the ions in calcium chloride.
Calcium ion __________________________________________________
Chloride ion __________________________________________________

[2]

(b) Calcium chloride has a high melting point.
Explain why calcium chloride has a high melting point. Use ideas about the
structure and bonding.
_____________________________________________________________
_____________________________________________________________
_____________________________________________________________
_____________________________________________________________

[2]

[Total: 4]

6

5. A mixture of ethanoic acid, ethene and oxygen is passed over a catalyst at 200 °C

to manufacture ethenyl ethanoate, CH3COOCH=CH2.

CH3COOH + CH2=CH2 + ½ O2 CH3COOCH=CH2 + H2O

The reaction is exothermic.

(a) Draw a reaction pathway diagrams for this reaction on Fig. 6.1.

On your diagram label:

• The axes

• The reactants and products

• The enthalpy change of the reaction, ΔH

• The activation energy, Ea

Fig. 6.1

[4]

(b) Explain why the enthalpy change of the reaction is exothermic. •

Use ideas about bond breaking and bond making.

_____________________________________________________________

_____________________________________________________________

_____________________________________________________________

_____________________________________________________________ [2]

[Total: 6]

7

6. Peroxodisulfate ions, S2O82-, react with iodide ions in aqueous solution.

S2O82- (aq) + 2I- (aq) 2SO42- (aq) + I2 (aq)

(a) Iodide ions are oxidised in this reaction. State how the equation shows this.

_____________________________________________________________

_____________________________________________________________ [1]

(b) Table 7.1 shows how the relative rate of this reaction changes when different
concentration of peroxodisulfate ions and iodide ions are used.
Table 7.1

Using the information in Table 7.1, describe how increasing the concentration
of each of these ions affects the relative rate of reaction.
Peroxodisulfate ions
_____________________________________________________________
_____________________________________________________________

Iodide ions
_____________________________________________________________
_____________________________________________________________

[2]

(c) Iron (III) ions, Fe3+, catalyse this reaction. Explain how catalysts increases the
rate of a reaction.
_____________________________________________________________
_____________________________________________________________ [2]
[Total:5]

8

7. Copper reacts with concentration nitric acid to form copper (II) nitrate.

Cu (s) + 4HNO3 (aq) Cu(NO3)2 (aq) + 2NO2 (g) + 2H2O (l)

(a) State the meaning of (aq)

_____________________________________________________________

_____________________________________________________________ [1]

(b) An excess of copper is added to 25.0 cm3 of 16.0 mol/dm3 HNO3.
Use this information, together with the equation, to calculate the volume of
NO2 formed. The gas volume is measured at room temperature and pressure.
Show your working and state the units.

Volume of NO2 = _______________ [3]

(c) When heated, Cu(NO3)2 decomposes to form CuO, NO2 and O2. [1]
Construct the symbol equation for this reaction.
_____________________________________________________________

[Tota:5]

9
8. Iodine reacts with chlorine to form iodine (I) chloride, ICl.

(a) The dot-and-cross diagram for a molecule of iodine (I) chloride is similar to
that for a molecule of chlorine.
Draw the dot-and-cross diagrams for a molecule of iodine (I) chloride.
Show outer electrons only.

[1]

(b) Iodine (I) chloride reacts with chlorine to form iodine (III) chloride.
This reaction is investigated at 200 °C in a closed system.
The reversible reaction reaches an equilibrium.

ICl (g) + Cl2 (g) ⇌ ICl3 (g)

(i) Describe two features of a reversible reaction at equilibrium, in a closed
system.
In your answer, refer to the rate of reaction and to the concentrations of
reactants and product.
_________________________________________________________
_________________________________________________________
_________________________________________________________
_________________________________________________________
_________________________________________________________ [2]

10

(ii) The pressure of the equilibrium mixture is increased.
The temperature is kept at 200 °C.
ICl (g) is a dark brown gas. ICl3 (g) is a yellow gas.
Predict and explain what will happen to the colour of the equilibrium
mixture.
Prediction ________________________________________________
_________________________________________________________

Explanation _______________________________________________
_________________________________________________________
_________________________________________________________ [2]

[Total: 5]

11

9. Air contains a mixture of gases including the noble gases neon, argon, krypton and
xenon. These noble gases are monoatomic elements.
(a) State what is meant by monatomic.
______________________________________________________________
______________________________________________________________ [1]

(b) State why noble gases are unreactive.
______________________________________________________________
______________________________________________________________ [1]

(c) State why fractional distillation can be used to separate a liquid mixture of
neon, argon, krypton and xenon.
______________________________________________________________
______________________________________________________________ [1]

(d) State which noble gas, neon, argon, krypton or xenon, has the fastest rate of
diffusion at 20 °C.
______________________________________________________________

Explain your answer.
______________________________________________________________
______________________________________________________________

[2]

[Total: 5]

12

1

SEKOLAH MENENGAH SAYYIDINA ALI INTERNAL EXAMINATION
Year 10 SIMULATION TEST 2022

CANDIDATE
NAME

YEAR

CHEMISTRY 5070 / 22
Paper 2 Theory Term 1 2022
45 minutes
Candidates answer on the Question Paper.
No Additional Materials are required.

INSTRUCTIONS
● Answer all questions.
● Use a black or dark blue pen. You may use an HB pencil for any diagrams or graphs.
● Write your name and year in the boxes at the top of the page.
● Write your answer to each question in the space provided.
● Do not use an erasable pen or correction fluid.
● You may use a calculator.
● You should show all your working and use appropriate units.

INFORMATION
● The total mark for this paper is 43.
● The number of marks for each question or part question is shown in brackets [ ].
● The Periodic Table is printed in the question paper.

For Examiner’s Use
out of

43

This paper consists of 12 printed pages

2
1. Choose from the list of oxides to answer the questions.

Calcium oxide
Carbon dioxide
Copper (II) oxide
Silicon (IV) oxide
Sodium oxide
Sulfur dioxide
Sulfur trioxide

Zinc oxide
Each oxide can be used once, more than once or not at all.
Identify which oxide:

Graphite, diamond & silicon (IV) oxide
(a) Has a giant covalent structure

_S_il_ic_o_n__(I_V_)_o_x_id_e_________________________________________________ [1]
Amphoteric oxide HINT= ZAL

(b) Reacts with acids and with alkalis
__Z_in_c__o_xi_d_e_____________________________________________________ [1]

(c) Contains a cation with a charge of +1
__S_o_d_iu_m__o_x_i_d_e__________________________________________________ [1]

[Total: 3]

3

2. Atoms and ions contain protons, neutrons and electrons.
The way to write the charge of the subatomic
(a) Complete Table 2.1.
particle is the opposite way compared to the

Table 2.1 ions charges. E.g. Proton = +1 & Ca2+

Proton Relative charge Relative mass
+1 1

Neutron 0 1

Electron -1 0 or 0.0005

All 4 correct= 3 marks. 3 correct= 2 marks. 1 correct= 0 mark. [3]

(b) Table 2.2 shows some information about six particles.

Table 2.2

Particle Number of protons Number of neutrons Number of electrons

A 37 48 37

B 53 74 54

C 92 143 92

D 92 143 89

E 92 146 92

F 94 150 92

(i) Deduce the nucleon number for particle A. Nucleon= p + n = 85
__8_5______________________________________________________ [1]

(ii) Explain why particle B is a negative ion.
_H_a_s__m_o_r_e_e_l_e_c_tr_o_n_t_h_a_n_p_r_o_to_n_s_._B__h_a_s_a__5_4_e_l_e_c_tr_o_n_s_b_u_t_o_n_l_y_5_3__p_ro_t_ons

_________________________________________________________ [1]

There are 2 things we look out for! 1) ATOMS 2) Isotopes= same no. of proton but different no. of n
(iii) Identify two atoms that are isotopes of same element.
______C___________ and _________E________

Explain your answer.
Both__a_re__a_to_m__s_t_h_a_t _h_a_ve__th_e__s_a_m_e__p_ro_t_o_n_n_u__m_b_e_r_b_u_t_d_if_fe_r_e_n_t_m__a_ss_/_n_u_c_le_on number

_________________________________________________________ [2]
[Total: 7]

4

3. Salts can be prepared by the reaction of acids with bases or alkalis and also by

precipitation reactions.

Aqueous sodium sulfate is used to prepare barium sulfate in a precipitation

reaction. Reactant: barium nitrate & sodium sulfate
Ba2+ (aq) + SO42- (aq) BaSO4 (s) Product: barium sulfate

In an experiment 20.0 cm3 of 0.550 mol/dm3 of barium nitrate is added to an excess

2 formulas being of sodium sulfate. V= 20.0 cm3 = (20/1000) dm3= 0.02 dm3
used in (a).
Conc= mol/vol C= 0.55 mol/dm3
Mole= mass/mr (a) Calculate the maximum mass of barium sulfate that could be made.

[Mr: BaSO4, 233] Notice that the reactant : product is 1:1 mole ratio? Therefore the
Show your working. calculation is direct. No need to find which one is the limiting reagent.

Mole = c x v = 0.55 mol/dm3 x 0.02 dm3

Mole= 0.011 mol

Mass is therefore, mass= mole x Mr = 0.011 mol x 233 g/mol = 2.563 g = 2.56 g (3.s.f)

Maximum mass of barium sulfate = ________2_._56__________ g [2]
2.563 g (Make sure to use the real long value!!) is the theoretical amount. Meaning, if the reaction went perfectly 100
% well in the lab. But reality is not the 100 % perfect. That’s why we got 1.92 g instead.

(b) A mass of 1.92 g of dry barium sulfate is obtained.

Calculate the percentage yield of barium sulfate.

% yield= ( 1.92 g / 2.563 g ) x 100 = 74.9122 % = 74.9 %

Percentage yield of barium sulfate = _______7_4._9_%____________ % [1]
[Total: 3]

5

4. Calcium chloride, CaCl2, is an ionic compound.

(a) Deduce the electronic configuration for each of the ions in calcium chloride.
Calcium ion __2_._8_.8_____________________________________________
Chloride ion __2_._8_.8_____________________________________________

[2]

(b) Calcium chloride has a high melting point.
Explain why calcium chloride has a high melting point. Use ideas about the
structure and bonding.
_S_t_ru_c_t_u_re_:_G__ia_n_t_la_t_ti_c_e___________________________________________
_B_o_n_d_i_n_g_: _st_r_o_n_g_io_n_i_c_/ _s_tr_o_n_g_a_t_tr_a_c_ti_o_n_b_e_t_w_e_e_n_p_o_s_i_ti_v_e_io_n_s__a_n_d_n_e_g_a_t_iv_e__ions
_____________________________________________________________
_____________________________________________________________
[2]

[Total: 4]

6

5. A mixture of ethanoic acid, ethene and oxygen is passed over a catalyst at 200 °C

to manufacture ethenyl ethanoate, CH3COOCH=CH2.

CH3COOH + CH2=CH2 + ½ O2 CH3COOCH=CH2 + H2O

The reaction is exothermic.

(a) Draw a reaction pathway diagrams for this reaction on Fig. 6.1.

On your diagram label:

• The axes

• The reactants and products

• The enthalpy change of the reaction, ΔH

• The activation energy, Ea

Fig. 6.1

[4]

(b) Explain why the enthalpy change of the reaction is exothermic. •

Use ideas about bond breaking and bond making.

__B_o_n_d_b_r_e_a_k_in_g__is__e_n_d_o_th_e_r_m_i_c_A_N__D_b_o_n_d__m_a_k_i_n_g_i_s_e_x_o_th_e_r_m__ic__________
More energy released than absorbed.

_____________________________________________________________

_____________________________________________________________

_____________________________________________________________ [2]

[Total: 6]

7

6. Peroxodisulfate ions, S2O82-, react with iodide ions in aqueous solution.

S2O82- (aq) + 2I- (aq) 2SO42- (aq) + I2 (aq)

(a) Iodide ions are oxidised in this reaction. State how the equation shows this.

I_o_d_id_e__io_n_s__lo_s_e_e_l_e_c_tr_o_n_(_s_)_______________________________________
R__e_je_c_t_: _io_d_in_e__lo_s_e_s__e_le_c_tr_o_n_s______________________________________ [1]

(b) Table 7.1 shows how the relative rate of this reaction changes when different
concentration of peroxodisulfate ions and iodide ions are used.
Table 7.1

Using the information in Table 7.1, describe how increasing the concentration
of each of these ions affects the relative rate of reaction.
Peroxodisulfate ions
_In_c_r_e_a_s_e_s_r_a_te_/_d_o_u_b_l_in_g__th_e__c_o_n_ce_n_t_r_a_tio_n__d_o_u_b_le_s__th_e__ra_t_e______________
_____________________________________________________________

Iodide ions
_In_c_r_e_a_s_e_r_a_te_/_d_o_u_b_l_in_g__c_o_n_c_e_n_tr_a_ti_o_n_d_o_u_b_le_s__th_e__ra_t_e__________________

_____________________________________________________________

[2]

(c) Iron (III) ions, Fe3+, catalyse this reaction. Explain how catalysts increases the

rate of a reaction.

Activ_a_ti_o_n_e_n_e_r_g_y_d_e_c_r_e_a_se_s__[1_]________________________________________
More_p_a_r_ti_c_le_s__h_a_ve__e_n_e_r_g_y_a_b_o_v_e_t_h_a_t_o_f_th_e__a_c_ti_v_a_tio_n__e_n_e_r_g_y_[1__]/_s_o_g_r_e_a_te_r____ [2]
proportion of collisions are successful

[Total:5]

8

7. Copper reacts with concentration nitric acid to form copper (II) nitrate.

Cu (s) + 4HNO3 (aq) Cu(NO3)2 (aq) + 2NO2 (g) + 2H2O (l)

(a) State the meaning of (aq)
_A_q__u_e_o_u_s_/_s_o_lu__ti_o_n_i_n_w__a_te__r _____________________________________

_____________________________________________________________ [1]

(b) An excess of copper is added to 25.0 cm3 of 16.0 mol/dm3 HNO3.

Use this information, together with the equation, to calculate the volume of

NO2 formed. The gas volume is measured at room temperature and pressure.

Show your working and state the units. STEP 3: Volume of NO2= mole x 24 dm3
V (NO2) : 0.2 mol x 24 dm3
STEP 1: Find mole of HNO3 V (NO2): 4.8 dm3
v= 25.0 cm3 / 1000 = 0.025 dm3
C= 16 mol/dm3.
Since c= n/v, therefore n (HNO3) = c x v
n (HNO3) = 16 mol/dm3 x 0.025 dm3
n (HNO3) = 0.4 mol.

STEP 2: Find mole of NO2 using mole ratio

HNO3: NO2

4:2

0.4:x Volume of NO2 = ___4_.8__d_m_3_______ [3]
n(NO2)= (0.4 x 2 )/ 4
n(NO2) = 0.2 mol

For decomposition: its always 1 reactant who separate/ break down into several products

(c) When heated, Cu(NO3)2 decomposes to form CuO, NO2 and O2.

Construct the symbol equation for this reaction.
__2_C_u_(N__O_3)_2____________2_C_u_O__+_4_N_O_2_+__O_2 ___________________________ [1]

Cu(NO3)2 CuO + NO2 + O2

Cu= 1 [Tota:5]

N= 2

O= 6

How to balance?

1. Deal with the O on the LHS. Notice its 1+2+2 on the RHS? So add no. 2 infront

of CuO

2. Once you add the no. 2 on the RHS, you also add 2 infront of Cu(NO3)2

recount the no. of elements on the LHS.

You will get:

Cu=2

N=4

O=12.

3. Proceed to deal with the RHS. So add no. 4 infront of NO2. And you’re done.

9
The formula for this molecule (ICl) is GIVEN already. If you only got 2 element, sharing, how does the

venn diagram looks like?
8. Iodine reacts with chlorine to form iodine (I) chloride, ICl.

(a) The dot-and-cross diagram for a molecule of iodine (I) chloride is similar to

that for a molecule of chlorine.

Draw the dot-and-cross diagrams for a molecule of iodine (I) chloride.

Show outer electrons only. Dot-and-cross diagram can be used for ‘ionic’ and ‘covalent’.
BUT there are 2 things that tells us that this is covalent bonding.

1.Molecule

2.Between non-metals ONLY.

[1]

(b) Iodine (I) chloride reacts with chlorine to form iodine (III) chloride.
This reaction is investigated at 200 °C in a closed system.
The reversible reaction reaches an equilibrium.

ICl (g) + Cl2 (g) ⇌ ICl3 (g)

(i) Describe two features of a reversible reaction at equilibrium, in a closed
system.
In your answer, refer to the rate of reaction and to the concentrations of
reactants and product.
_R_a__te__o_f _fo_r_w_a_r_d_r_e_a_c_tio_n__is__th_e__s_a_m_e__a_s_r_a_te__o_f _b_a_c_kw__a_rd__re_a_c_t_io_n_.____
_T_h_e__c_o_n_c_e_n_tr_a_ti_o_n_s_o_f_r_e_a_c_ta_n_t_s_a_n_d_p_r_o_d_u_c_ts__d_o_n_o_t_c_h_a_n_g_e_.________
_________________________________________________________
_________________________________________________________
_________________________________________________________ [2]

10

(ii) The pressure of the equilibrium mixture is increased.
The temperature is kept at 200 °C.
ICl (g) is a dark brown gas. ICl3 (g) is a yellow gas.
Predict and explain what will happen to the colour of the equilibrium
mixture.
Prediction ________________________________________________
__T_h_e_c_o_lo_u_r__b_e_co_m__e_l_e_s_s_b_r_o_w_n_/_c_o_lo_u_r_b_e_c_o_m__e_s_m__o_re__y_e_ll_o_w________

Explanation _______________________________________________
Fewer mo_l_e_s_o_n__th_e__ri_g_h_t-_h_a_n_d_s_i_d_e_s_o_p_o_s_i_ti_o_n_o_f_e_q_u_i_lib_r_iu_m__m__o_v_e_s_t_o_t_h_e_r_ig_h_t_/ fewer moles
on the pro_d_u_c_t_s_i_d_e_s_o_p_o_s_i_ti_o_n_o_f_e_q_u_i_lib_r_iu_m__m__o_v_e_s_t_o_t_h_e_r_ig_h_t______________ [2]

[Total: 5]

Increasing pressure will favour the side with LESS moles.
ICl (g) + Cl2 (g) ⇌ ICl3 (g)
3 moles vs 1 moles
So forward reaction is favoured.

11

9. Air contains a mixture of gases including the noble gases neon, argon, krypton and
xenon. These noble gases are monoatomic elements.
(a) State what is meant by monatomic.
_E_x_i_st_a__s_a_to_m__s_(_a_n_d_n_o_t_a_s__m_o_l_e_c_u_le_s_)/_a__to_m__s_u_n_b_o_n_d_e_d_________________
______________________________________________________________ [1]

(b) State why noble gases are unreactive.
_H_a_s_a_s_t_a_b_le_e_l_ec_t_ro_n_i_c_a_rr_a_n_g_e_m_e_n_t/__at_o_m_s__do__n_o_t _n_e_ed__to__g_ai_n_o_r_l_o_se__el_e_c_tr_o_n_s__
Accept: complete valence shell/ stable outer octet
______________________________________________________________ [1]

(c) State why fractional distillation can be used to separate a liquid mixture of
neon, argon, krypton and xenon.
__H_a_v_e__d_if_fe_r_e_n_t _b_o_il_in_g_p_o_i_n_ts_______________________________________
______________________________________________________________ [1]

(d) State which noble gas, neon, argon, krypton or xenon, has the fastest rate of
diffusion at 20 °C.
_n_e_o_n__________________________________________________________

Explain your answer.
_H_a_s__th_e__s_m_a_ll_e_s_t _(r_e_la_t_iv_e_)_a_t_o_m_i_c_m__a_ss_/_a_t_o_m_s__h_a_v_e_t_h_e_s_m__a_lle_s_t_m__a_s_s_e_s___
______________________________________________________________

[2]

[Total: 5]

12

1

SEKOLAH MENENGAH SAYYIDINA ALI INTERNAL EXAMINATION
Year 10 TEST 2022

CANDIDATE
NAME

YEAR

CHEMISTRY 5070 / 22
Paper 2 Theory Term 1 2022
45 minutes
Candidates answer on the Question Paper.
Printed laminated Periodic Table provided separately.

INSTRUCTIONS
● Answer all questions.
● Use a black or dark blue pen. You may use an HB pencil for any diagrams or graphs.
● Write your name and year in the boxes at the top of the page.
● Write your answer to each question in the space provided.
● Do not use an erasable pen or correction fluid.
● You may use a calculator.
● You should show all your working and use appropriate units.

INFORMATION
● The total mark for this paper is 35.
● The number of marks for each question or part question is shown in brackets [ ].

For Examiner’s Use
out of

35

This paper consists of 10 printed pages

2

1. (a) Choose from the following lists of metals to answer the questions below.
Aluminium
Iron
Lead
Magnesium
Potassium
Silver
Vanadium

Each metal can be used once, more than once or not at all.

Which metal [1]
(i) Reacts with cold water to form an alkaline solution,

______________________________________________________________

(ii) Forms a protective oxide layer on its surface,
______________________________________________________________ [1]

(iii) Is the catalyst used in the industrial manufacture of ammonia,
______________________________________________________________ [1]

(iv) Is a sacrificial metal used to prevent iron pipes from rusting
______________________________________________________________ [1]

(v) Is in Period 5 of the Periodic Table
______________________________________________________________ [1]

3
(b) Draw a labelled diagram to show the structure of a typical metal

[2]
[Total: 7]

4
2. A student measured the volume of hydrogen produced over time when small pieces

of zinc reacted with excess sulfuric acid.
The results are shown in the graph below.

(a) Use the information from the graph to calculate the average speed of reaction
in the first two minutes.

[1]
(b) Explain why the reaction stopped after 6 minutes.

______________________________________________________________ [1]

5 [1]

(c) Copper catalyses this reaction.
(i) On the axes above, sketch a line to show the expected results for the
catalysed reaction.

(ii) Explain how a catalyst changes the speed of reaction.
______________________________________________________________ [1]

(d) Explain, using ideas about colliding particles, what happens to the speed of [2]
this reaction when larger particles of zinc are used.
______________________________________________________________
______________________________________________________________
______________________________________________________________

(e) Explain, using ideas about colliding particles, what happens to the speed of [2]
this reaction when the temperature of the reaction mixture is increased.
______________________________________________________________
______________________________________________________________
______________________________________________________________

[Total: 8]

6

3. Chlorine, bromine and iodine are non-metals in Group VII of the Periodic Table. [1]
Their molecules are diatomic.
(a) What do you understand by the term diatomic?
______________________________________________________________

(b) (i) Describe the trend in colour of the Group VII elements down the Group.
__________________________________________________________ [1]

(ii) In what physical state do the following elements exists at room
temperature and pressure?
Bromine ___________________________________________________
Iodine _____________________________________________________ [2]

(c) An aqueous solution of calcium hydroxide was titrated with 0.0150 mol/dm3

hydrochloric acid.

Ca(OH)2 + 2HCl CaCl2 + 2H2O

It required 6.00 cm3 of this aqueous hydrochloric acid to neutralise 20.0 cm3 of

the calcium hydroxide solution.

Calculate the concentration in mol/dm3, of the calcium hydroxide solution.

[3]
[Total: 7]

7
4. Diamond and graphite are two forms of carbon.

(a) (i) Describe two differences in the structure of diamond and graphite.
__________________________________________________________
__________________________________________________________ [2]
__________________________________________________________
__________________________________________________________

(ii) Explain, in terms of their structure, why graphite is soft but diamond is
hard.
__________________________________________________________
__________________________________________________________
__________________________________________________________
__________________________________________________________ [2]

(b) Tin is extracted by heating tin (IV) oxide, SnO2, with carbon in a furnace.

SnO2 + 2C Sn + 2CO

(i) How does this equation shows that tin (IV) oxide gets reduced?
__________________________________________________________
__________________________________________________________ [1]

8

(ii) Carbon monoxide has a triple covalent bond.
Draw the electronic structure of carbon monoxide. Show only the outer
electrons.

[2]

(iii) Carbon monoxide reacts with chromium to form chromium carbonyl.
The structure of chromium carbonyl is shown below.

Write the empirical formula for chromium carbonyl.
__________________________________________________________ [1]

[Total: 8]

9

5. Magnesium is a reactive metal. [1]
(a) Name the products formed when magnesium reacts with steam.
______________________________________________________________

(b) The equation shows the reaction which occurs when magnesium carbonate is

heated.

MgCO3 MgO +CO2

State the name given to this type of chemical reaction.
______________________________________________________________ [1]

(c) A student compared the action of heat on three solid metal carbonates.
She heated each carbonate using the apparatus shown below. In each case,
she recorded the length of time taken for the limewater to turn milky.

(i) State one factor that must be kept constant if the speeds of reaction are
to be compared in a fair way.
__________________________________________________________ [1]

10

(ii) The time taken for the limewater to turn milky for each metal carbonate is

shown in the table.

Metal carbonate Time taken for the limewater to

turn milky/ s

Copper carbonate 10

Magnesium carbonate 40

Zinc carbonate 24

Describe and explain these three results in terms of the reactivity of the [2]
metals.
__________________________________________________________
__________________________________________________________
__________________________________________________________
__________________________________________________________

[Total: 5]

1

SEKOLAH MENENGAH SAYYIDINA ALI INTERNAL EXAMINATION
Year 10 TEST 2022

CANDIDATE (source: W10_22)

MARKING SCHEMENAME

YEAR

CHEMISTRY 5070 / 22
Paper 2 Theory Term 1 2022
45 minutes
Candidates answer on the Question Paper.
Printed laminated Periodic Table provided separately.

INSTRUCTIONS
● Answer all questions.
● Use a black or dark blue pen. You may use an HB pencil for any diagrams or graphs.
● Write your name and year in the boxes at the top of the page.
● Write your answer to each question in the space provided.
● Do not use an erasable pen or correction fluid.
● You may use a calculator.
● You should show all your working and use appropriate units.

INFORMATION
● The total mark for this paper is 35.
● The number of marks for each question or part question is shown in brackets [ ].

For Examiner’s Use
out of

35

This paper consists of 10 printed pages

2

1. (a) Choose from the following lists of metals to answer the questions below.
Aluminium
Iron
Lead
Magnesium
Potassium
Silver
Vanadium

Each metal can be used once, more than once or not at all.

If the metal CAN react with COLD water, this metal is VERY REACTIVE

Which metal To be able to form Alkaline solution, the

(i) Reacts with cold water to form an alkaline solution, metal is from Group 1.

_P_o_t_a_s_s_i_u_m_____________________________________________________ [1]

A very important hint to reveal the identity of the metal [1]
(ii) Forms a protective oxide layer on its surface,

__A_l_u_m__in__iu_m____________________________________________________

Haber process- ammonia- catalyst: iron & Contact process- sulfuric acid- catalyst: vanadium (V) oxide
(iii) Is the catalyst used in the industrial manufacture of ammonia,

___I_ro__n________________________________________________________ [1]

(iv) Is a sacrificial metal used to prevent iron pipes from rusting

_M__a_g_n__e_s_iu_m____________________________________________________ [1]

(v) Is in Period 5 of the Periodic Table

__S_i_lv_e_r________________________________________________________ [1]

Sacrificial metal has to be more REACTIVE than Iron. The commonly used metal in Sacrificial &
galvanizing is Zinc. But we don’t have zinc in the options. Do take note (and this is from your TOPIC 9:
METALS notes as well) iron in the form of steel is used to make underground pipelines to carry oil
and gas. The magnesium bars are attached to the iron.

3

Do TAKE NOTE that you NEED TO LABEL & DRAW
(b) Draw a labelled diagram to show the structure of a typical metal

Positive sign in the centre of the atoms
labelled (metal) ions [1 MARK]

At least one electron drawn between [2]
the circles and labelled electron(s) [1
MARK]

[Total: 7]

4

2. A student measured the volume of hydrogen produced over time when small pieces

of zinc reacted with excess sulfuric acid. Reaction: Metal + acid salt + H2
The results are shown in the graph below.

TAKE NOTE
of the UNIT

X2, Y2
(2,25)

Calculate the
gradient

X1,Y1
(0,0)

TAKE NOTE of the UNIT
(a) Use the information from the graph to calculate the average speed of reaction

in the first two minutes.

Average speed of reaction= gradient= (Y2-Y1)/ (X2-X1)

= (25-0)/(2-0)= 12.5 cm3/min

Both VALUE & UNIT must be correct for [1 MARK] [1]

(b) Explain why the reaction stopped after 6 minutes.
__A_ll_t_he__Z_in_c_w_a_s_u_s_e_d_u_p_/_t_h_e_re__w_a_s_n_o_Z_in_c__le_ft_/_Z_in_c__is_li_m_i_ti_n_g_______________ [1]

5

(c) Copper catalyses this reaction.

(i) On the axes above, sketch a line to show the expected results for the

catalysed reaction. [1]

Line steeper from the 0,0 AND ending at the same level (40 cm3). (SEE RAINBOW INK)

(ii) Explain how a catalyst changes the speed of reaction.
____C_a_t_a_ly_s_t _lo_w_e_r_s_t_h_e_a_ct_iv_a_t_io_n_e_n_e_r_g_y_______________________________ [1]

(d) Explain, using ideas about colliding particles, what happens to the speed of
this reaction when larger particles of zinc are used. Notice the question are of COMPARATIVE nature?

_S_p_e_ed__o_f _re_a_c_ti_o_n_d_e_c_re_a_s_e_s_b_e_ca_u_s_e_s_m_a_l_le_r_s_u_rf_a_c_e _a_re_a_.___________________
_F_re_q_u_e_n_c_y_o_f_c_o_lli_s_io_n_s_d_e_c_re_a_s_e_s _/_fe_w_e_r_c_o_l_lis_io_n_s_p_e_r_m__in_u_t_e________________

______________________________________________________________ [2]

(e) Explain, using ideas about colliding particles, what happens to the speed of [2]

this reaction when the temperature of the reaction mixture is increased.

_S_p_e_e_d_o_f _re_a_c_t_io_n_i_n_cr_e_a_se_s_._________________________________________
_A_s_t_e_m_p_e_ra_t_u_r_e_in_c_r_ea_s_e_s_, p_a_r_t_ic_le_s_m__ov_e__fa_s_te_r_O_R__in_c_r_ea_s_e_k_i_ne_t_ic__en_e_r_g_y_______
More successful collisions.
______________________________________________________________

[Total: 8]

REFER to the [SUMMARY] Factors affecting
rate of reaction

6

3. Chlorine, bromine and iodine are non-metals in Group VII of the Periodic Table. [1]

Their molecules are diatomic.

(a) What do you understand by the term diatomic?
_M_o_l_e_cu_l_e_s _c_on_t_a_in_i_n_g_tw__o_a_t_o_m_s_jo_i_n_e_d_b_y_b_o_n_d___________________________

(b) (i) Describe the trend in colour of the Group VII elements down the Group.
_T_h_e_c_o_lo_u_r_g_e_ts_d_a_r_k_er__________________________________________ [1]

(ii) In what physical state do the following elements exists at room

temperature and pressure? [2]

Bromine __l_iq_u_id______________________________________________
Iodine ____s_o_li_d______________________________________________

Concentration so, c (HCl)= 0.015 mol/dm3
(c) An aqueous solution of calcium hydroxide was titrated with 0.0150 mol/dm3

hydrochloric acid.

Ca(OH)2 + 2HCl CaCl2 + 2H2O

It required 6.00 cm3 of this aqueous hydrochloric acid to neutralise 20.0 cm3 of

the calcium hydroxide solution. V (HCl)= 6 cm3 & V (Ca(OH)2)= 20 cm3 VERY important.
Calculate the concentration in mol/dm3, of the calcium hydroxide solution.
Notice the unit of volume
STEP 1: Write down all the known values given is cm3? Yet in the
concentration given is dm3?
Ca(OH)2 HCl You need to convert cm3 to
c? c 0.015 mol/dm3 dm3 by dividing it with
n? n?
v 20 cm3 ÷ 1000= 0.02 dm3 v 6 cm3 ÷ 1000 = 0.006 dm3 10000.

STEP 2: Calculate the mole of HCl
n(HCl) = c x v
= 0.015 mol/dm3 x 0.006 dm3
=0.00009 mol [1 MARK]

STEP 3: Using mole ratio, calculate the
mole of Ca(OH)2

Ca(OH)2 : HCl [3]
1: 2

? : 0.00009 [Total: 7]
n( Ca(OH)2 ) = 0.00009 mol / 2 = 0.000045 mol [1 MARK]

STEP 4: Use the formula to calculate the concentration of Ca(OH)2
C( Ca(OH)2 ) = n/v = 0.000045 mol / 0.02 dm3 = 0.00225 mol/dm3 [ 1 MARK]

7

4. Diamond and graphite are two forms of carbon. Diamond and graphite are the allotropes
of carbon. Allotropy is the existence of an
element in two or more different forms in
the same physical state.

Weak intermolecular forces

-In diamond, the atoms are arranged tetrahedrally and in graphite, the atoms are arranged in layers
-In diamond, there is NO delocalised electrons and in graphite, graphite HAS delocalised electrons.
(a) (i) Describe two differences in the structure of diamond and graphite.

__________________________________________________________

__________________________________________________________

__________________________________________________________

__________________________________________________________ [2]

(ii) Explain, in terms of their structure, why graphite is soft but diamond is
hard.
__________________________________________________________
__________________________________________________________
__________________________________________________________
__________________________________________________________ [2]

Graphite is soft because in graphite, the LAYERS can SLIDE due to WEAK FORCES between the layers. See your notes Topic 6

Diamond is hard because there is strong COVALENT bonding in ALL DIRECTIONS. Chemical reaction

(b) Tin is extracted by heating tin (IV) oxide, SnO2, with carbon in a furnace. (part 4) redox

NOTE: Reduction involves SnO2 + 2C Sn + 2CO

(i) loss of oxygen (ii) gain

in electron (iii) decrease
in oxidation number (i) How does this equation shows that tin (IV) oxide gets reduced?

Oxy_ge_n__is_r_e_m_o_v_e_d_f_ro_m__t_h_e_t_in_(I_V_)o_x_i_d_e/__o_xi_d_at_i_on__n_u_m_b_e_r_o_f_t_in_i_n_t_in_(_IV_)_o_x_i_de__decreases from +4
to O_/_t_in_l_o_se_s_o_x_y_g_e_n_____________________________________________ [1]

8
This is already a hint. Meaning, in the overlap
they have 6 e-

(ii) Carbon monoxide has a triple covalent bond.
Draw the electronic structure of carbon monoxide. Show only the outer
electrons. This makes the dot-and-cross diagram simpler since you just look at the Group no.
which tells us the no. of valence electron (aka the outer shell electron)

KEY: electron
CX
O

[2]

(iii) Carbon monoxide reacts with chromium to form chromium carbonyl.
The structure of chromium carbonyl is shown below.

This is a simple question asking you to first count
the number of each elements and then simplify it
(empirical formula).

There are times where you will be asked to do
Empirical calculations where the percentage
masses of each elements are given. But this
question is not that one. Its much simpler.

Write the empirical formula for chromium carbonyl.
____Cr_C_6_O_6_. _A_LL_O_W__:_C_r(_C_O_)_6 _____________________________________ [1]

Cr= 1 You cannot simplify the rest because Cr=1. [Total: 8]
C= 6 Hence, this is the empirical formula
O=6

Carbon is a reference for extraction. (Meaning only the elements 9
BELOW carbon can be EXTRACTED by using “carbon reduction”). How

to remember where Carbon is? The expensive LAPTOP, MAC BOOK.

5. Magnesium is a reactive metal. Remember, the reactivity series: PoSoCaMA(C)ZIL(H)CopSiGo

(a) Name the products formed when magnesium reacts with steam.

_M__a_gn_e_s_iu_m__o_x_id_e_a_n_d__h_yd_r_o_g_e_n______________________________________ [1]

Mg to Fe react with steam to form metal oxide & H2. Pb downwards no reaction.
(b) The equation shows the reaction which occurs when magnesium carbonate is

heated. “Carbonate” will always produce carbon

MgCO3 MgO +CO2 dioxide gas. Carbonate comes from
‘carbon’ and ‘ate’ which is oxygen.

This is a common question and you need to notice that there is only ONE reactant, which is being BROKEN DOWN into two or

more product. State the name given to this type of chemical reaction.

___d_ec_o_m__p_os_i_ti_o_n_________________________________________________ [1]

(c) A student compared the action of heat on three solid metal carbonates.
She heated each carbonate using the apparatus shown below. In each case,
she recorded the length of time taken for the limewater to turn milky.

The test for CO2 gas is using limewater. Limewater
turns milky.

(i) State one factor that must be kept constant if the speeds of reaction are

to be compared in a fair way.

__________________________________________________________ [1]

-Height / strength of Bunsen flame
-Same temperature of Bunsen flame
-Same distance of Bunsen flame from tube
-Mass of carbonate in the tube
-Same amount of limewater
-Same size of carbonate particles

10
Remember, the reactivity series: PoSoCaMA(C)ZIL(H)CopSiGo

(ii) The time taken for the limewater to turn milky for each metal carbonate is

M>Z> Cop where M is shown in the table.
the most reactive.
When you look at the Metal carbonate Time taken for the limewater to
time:
Most reactive (Mg)= 40 s turn milky/ s

Copper carbonate 10

Magnesium carbonate 40

Zinc carbonate 24

Zn= 24 s Describe and explain these three results in terms of the reactivity of the

And the LEAST reactive= metals.
Cu = 10 s.
___C_o_p_p_e_r _ca_r_b_o_n_a_te_t_a_k_e_s_th_e__sh_o_r_te_s_t_t_im_e__to__d_e_co_m__p_o_se__a_nd__m_a_g_n_e_si_u_m___
___c_a_rb_o_n_a_te__ta_k_e_s_t_h_e_lo_n_g_e_s_t _ti_m_e_t_o_d_e_c_o_m_p_o_s_e_. _[1__M_A_R_K_]_____________ [2]

The less reactive the metal, the faster the rate of decomposition. [1 MARK]
__________________________________________________________

__________________________________________________________

[Total: 5]

The question asked you to ‘describe’ and ‘explain’.

Describe PART: what do you NOTICE when you look at the table? What is happening?

Explain PART: tell them your CONCLUSION. Relate the situation observed with your PRIOR knowledge i.e. in this
case, the reactivity series of the metal.


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