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Chemistry
Higher Level
Paper 1

Monday 12 September 2022

1 hour

Instructions to candidates
 Do not open this examination paper until instructed to do so.
 Answer all the questions.
 For each question, choose the answer you consider to be the best and indicate your choice
on the answer sheet provided.
 The periodic table is provided for reference on page 2 of this examination paper.
 The maximum mark for this examination paper is [40 marks].

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1. How many molecules are present in 27.0 g of distilled water?

(Avogadro’s constant = 6 x 1023 mol-1)

A. 2.7 x 1024

B. 1.5

C. 9.0 x 1023

D. 4.5

2. 32 g of a metal, M, reacts with 8 g of oxygen to form an oxide. The formula of the oxide is MO.
What is the atomic mass of M in g mol-1?

A. 16

B. 32

C. 64

D. 128

3. What volume of ammonia, in dm3, can be made from 30 dm3 of nitrogen and 60 dm3 of hydrogen?
Assume that all volumes are measured at the same temperature and pressure and that the
reaction goes to completion according to the equation:
N2(g) + 3H2(g) → 2NH3(g)

A. 40
B. 60
C. 90
D. 180

4. Which solution contains the most amount of sodium hydroxide?

A. 10.0 cm3 of 0.700 mol dm-3 NaOH
B. 20.0 cm3 of 0.600 mol dm-3 NaOH
C. 30.0 cm3 of 0.500 mol dm-3 NaOH
D. 40.0 cm3 of 0.400 mol dm-3 NaOH

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5. Ethane burns in oxygen according to the equation below. What volume of oxygen, in dm 3, reacts
with 0.8 dm3 of ethane?
2C2H6(g) + 7O2(g) → 4CO2(g) + 6H2O(l)

A. 0.8
B. 1.6
C. 2.8
D. 5.6

6. Which statement about isotopes is correct?

A. Isotopes have the same molecular formula but a different structural formula.
B. Isotopes have the same number of neutrons in atoms of the element
C. Isotopes of atoms of the same element have the same electron configuration.
D. Isotopes of atoms of the same element have the same mass number

239 239
7. What is the difference between the two neutral atoms 93 Np and 94 Pu ?
A. The number of protons, neutrons and electrons
B. The number of protons and electrons only
C. The number of protons and neutrons only
D. The number of neutrons only

40
8. What is the number of electrons in one 20Ca 2+ ion?
A. 40
B. 20
C. 22
D. 18

39 40
9. The two isotopic abundances of element Z are 90% of 19Z and 10% of 19 Z . What is the relative
atomic mass of Z?
A. 39.10
B. 39.90
C. –39.50
D. 19

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10. Which species contains only one unpaired electron?

A. Fe2+
B. Sc3+
C. Cu2+
D. Cr3+

11. Which are the correct statements about orbitals?

I. The plane of px orbitals is at 90o to the planes of py and pz orbitals.
II. p orbitals can form new hybrid orbitals with s orbitals
III. A p orbital can contain a maximum of six electrons

A. I and II only
B. I and III only
C. II and III only
D. I, II and III

12. Which equation represents the fourth ionization energy of a metal M?

A. M 4+(g) → M 5+(g) + e –
B. M 3+(s) → M 4+(s) + e –
C. M(g) → M 4+(g) + 4e-
D. M 3+(g) → M 4+(g) + e-

13. What is the electronic configuration of an atom with Z = 52?

A. 1s2 2s2 2p6 3s2 3p6 4s2 3d104p6 5s2 4d105p4
B. [Kr]5s2 5d105p4
C. [Kr]5s2 4d104p4
D. 1s2 2s2 2p6 3s2 3p6 4s2 3d104p6 5s2 5p105d4

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14. An element is in period 3 and group 15 of the periodic table. How many electrons are present in
the highest occupied energy level of this element?

A. 3

B. 5

C. 13

D. 15

15. Which best describes the trends of electronegativity values within the periodic table?

A. The values increase across a period (from left to right) and decrease down a group.

B. The values increase across a period (from left to right) and increase down a group.

C. The values decrease across a period (from left to right) and decrease down a group.

D. The values decrease across a period (from left to right) and increase down a group.

16. Which is a correct statement about the halogens or their ions?

A. Halide ions are all oxidising agents with the fluoride ion being the strongest

B. Bromine can oxidise iodide ions.

C. Iodine can oxidise chloride ions.

D. Fluorine is a stronger reducing agent than iodine.

17. Which reaction produces a coloured substance?

A. The addition of sodium metal to water.

B. The addition of sulphur dioxide gas to water.

C. Burning sodium metal in chlorine gas.

D. The addition of chlorine gas to a solution of potassium iodide.

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18. Which supports the statement that aluminium oxide is amphoteric?

I. Al2O3 can react with strong acids and bases.
II. Al2O3 dissolves in water to give a neutral solution.
III. Al2O3 can react to form a salt with sodium hydroxide and with hydrochloric acid.
A. I and II only
B. I and III only
C. II and III only
D. I, II and III

19. Which species can act as ligands?

I. NH3

II. Cl-

III. SiCl4

A. I and II only

B. I and III only

C. II and III only

D. I, II and III

20. Which species will not be coloured?

A. Cu2SO4

B. Mn2O3

C. [Fe(H2O)6] 3+

D. Pt(NH3)2Cl2

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21. Which is most likely to result in the formation of an ionic bond?

A. When two highly electronegative elements react together.

B. When a highly electronegative element reacts with a group 2 element.

C. When a group 16 element reacts with a group 17 element.

D. When hydrogen reacts with a group 17 element.

22. Which substance contains both ionic and covalent bonds?

A. HCN

B. NaNO3

C. MgO

D. HCOOH

23. What is the shape of PCl5?

A. Square planar

B. Trigonal pyramidal

C. Trigonal bipyramidal

D. Pentahedral

24. Which is the best description of how π bonds are formed?

A. The axial overlap of an s and a p orbital

B. The sideways overlap of parallel p orbitals

C. The axial overlap of two p orbitals

D. The sideways overlap of an s and a p orbital

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25. What is the hybridization of the N atom in NO 3 – and NH3 respectively?

A. sp3 and sp3

B. sp2 and sp2

C. sp and sp3

D. sp2 and sp3

26. Which substance does not contain delocalized electrons?

A. Sodium metal

B. Sodium carbonate

C. Sodium iodide

D. Sodium ethanoate

27. Which is correct concerning the bonding between two carbon atoms?

A. Double bonds are formed when the two carbon atoms are sp 3 hybridized.

B. Double bonds are caused by the overlap of two π bonds.

C. π bonds are weaker than σ bonds.

D. Triple bonds are made up of two σ bonds and one π bond.

28. Which molecule or ion has the same shape as XeF 4?

A. ICl4 –

B. SiCl4

C. SCl4

D. PH4 +

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29. Which gives an acidic solution when dissolved in water?

A. CH3COOH

B. CH3CHO

C. CH3CH2OH

D. CH3COCH3

30. Which substance reacts with dilute nitric acid to produce hydrogen gas?

A. FeCO3

B. Fe(OH)3

C. Fe2O3

D. Fe

31. Which substance is not a base?

A. CuO

B. NaCl

C. NaHCO3

D. CuCO3

32. Which list contains only strong acids?

A. HCl, HNO3, H2CO3

B. HCl, HNO3, H2SO4

C. CH3COOH, H2CO3, H2SO4

D. H2SO4, CH3COOH, H2CO3

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33. Which can be used to distinguish between a solution of a strong monoprotic acid and a solution
of weak monoprotic acid with the same concentration?
I. Add zinc to each solution and measure the rate of formation of gas produced.
II. Add sodium hydroxide solution to each solution and measure the temperature change.
III. Measure the pH

A. I and II only
B. I and III only
C. II and III only
D. I, II and III

34. Which are reduced when repeated measurements of a physical quantity are made?
A. both random and systematic errors
B. only systematic errors
C. only random errors
D. neither systematic nor random errors

35. Before performing a titration, a student rinsed all her apparatus with distilled water but did not
dry it afterwards. Which will not affect the accuracy of her titration result?
A. Failure to rinse the burette with the solution it contains before filling it
B. Failure to rinse the pipette with the liquid it contains before filling it
C. Failure to dry the conical flask after washing with distilled water
D. Failure to thoroughly mix the contents of the volumetric flask before taking a sample by
pipette

36. Which of the following may cause systematic errors when used in an experiment?
I. A wrongly calibrated thermometer
II. A standard solution that has been prepared wrongly
III. Taking the reading from the top of the meniscus when using a pipette

A. I and II only
B. I and III only
C. II and III only
D. I, II and III

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37. A student determined the empirical formula of magnesium oxide by heating a known mass of
magnesium in air and weighing the product after the magnesium had burned. Which factors
would result in her calculated formula having a higher ratio of magnesium to oxygen than 1:1?
I. Not all the magnesium reacted
II. Some of the product escaped before it was weighed
III. Some of the product was magnesium nitride, Mg 3N2
A. I and II only
B. I and III only
C. II and III only
D. I, II and III

38. Which contains the same number of ions as the value of Avogadro’s constant?

A. 0.5 mol KBr

B. 0.5 mol CaBr2

C. 1.0 mol CaO

D. 1.0 mol K2O

39. What is the electron configuration of the Cr 3+ ion?

A. [Ar]4s1 3d5

B. [Ar]4s2 3d1

C. [Ar]3d3

D. [Ar]4s1 3d2

40. In what order do the orbitals increase in energy within the same level?

A. d < f < p < s

B. f < d < p < s

C. s < d < p < f

D. s < p < d < f

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