Question 1

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Question 2

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Question 3

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Question 4

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Question 5

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Successive ionisation energies for an element, Y, are shown in the table below.

Electrons removed	1st	2nd	3rd	4th	5th
Ionisation energy / kJ mol^-1	736	1450	7740	10500	13600

What is the most likely formula for the ion of Y?

Y⁺
Y²⁺
Y³⁺
Y⁴⁺

Key Concepts

Successive Ionisation Energies

Question 6

Marks: 1

Question 7

Marks: 1

Use a periodic table to deduce the correct information about the element tin, Sn (Z = 50)

	Number of occupied main energy levels	Number of electrons in the highest main energy level
A	4	4
B	4	14
C	5	4
D	5	14

Question 8

Marks: 1

Which complex is likely to be colourless?

[Zn(H₂O)₆]Cl₂
[NH₄]₂[Fe(H₂O)₆][SO₄]₂
K₃[Co(CN)₆]
[Ni(NH₃)₆][BF₄]₂

Key Concepts

Transition Elements

Question 9

Marks: 1

Which type of bonding can be described as ‘the electrostatic attraction between positive nuclei and electrons and occurs by the sharing of electrons’?

Hydrogen bonding
Ionic bonding
Metallic bonding
Covalent bonding

Question 10

Marks: 1

Which of the following are properties of transition metals?

They have variable oxidation states
They can behave as catalysts
They can have magnetic properties

I and II only
I and III only
II and III only
I, II and III

Key Concepts

Transition Elements

Question 11

Marks: 1

Which is a characteristic property of sodium oxide?

It turns moist litmus paper blue
It turns moist litmus paper red
When it dissolves in distilled water it forms a solution with pH less than 7
It reacts with magnesium metal

Question 12

Marks: 1

Sulfur forms the compound S₄N₄ with nitrogen, the structure is shown below. q10_4-2_ib_sl_hard_mcq

Which of the following statements about S₄N₄ is correct?

The sulfur atom marked x has two lone pairs
The sulfur atom marked y has two lone pairs
Each N atom has two lone pairs
The N-S-N bond angle will be larger than S=N=S bond angle

Question 13

Marks: 1

Which combination describes the PH₄⁺ ion?

	Molecular geometry	Central atom hybridisation
A	Tetrahedral	sp³
B	Square planar	sp³
C	Tetrahedral	sp²
D	Square planar	sp²

Key Concepts

Identifying Hybridisation

Question 14

Marks: 1

Which enthalpy changes correctly describe the following reactions?

Reaction 1: HNO₃ (aq) + NH₃ (aq) → NH₄NO₃ (aq)

Reaction 2: CuCO₃ (s) → CuO (s) + CO₂ (g)

Reaction 3: S (s) + O₂ (g) → SO₂ (g)

	ΔH^Ө_c	ΔH^Ө_f	ΔH^Ө_neut	ΔH^Ө_r
A	2	2	1	3
B	3	2	1	2
C	3	3	1	2
D	2	3	1	3

Question 15

Marks: 1

Bond energy calculations show the enthalpy of combustion for propene to be -1572.0 kJ mol^-1.

Compound	C₃H₆ (g)	CO₂ (g)	H₂O (l)	H₂O (g)
ΔH^Ө_f / kJ mol^-1	+20.0	-393.5	-285.8	-241.8

Using the enthalpy of formation data, which calculation correctly shows the percentage error between propene’s enthalpy of combustion values obtained from bond energy calculations and Hess’s Law calculations, assuming the bond energy calculation value is correct?

$\frac{- 1572.0}{((3 \times - 393.5) + (3 \times - 241.8) - (20)) - 1572.0} x 100$
$\frac{(3 \times - 393.5) + (3 \times - 241.8) - (20)}{- 1572.0} x 100$
$\frac{(3 \times - 393.5) + (3 \times - 241.8) + (20)}{- 1572.0} \times 100$
$\frac{((3 \times - 393.5) + (3 \times - 241.8) - (20)) - (- 1572.0)}{- 1572.0} \times 100$

Question 16

Marks: 1

The ΔG^ϴ_f values for the following substances are shown.

Substance	ΔG^ϴ_f (kJ mol^-1)
NH₃ (g)	-16.4
O₂ (g)	0
H₂O (g)	-228.6
NO (g)	87.6

Which of the following is the correct calculation to determine ΔG^ϴ?

4NH₃ (g) + 5O₂ (g) ⇌ 6H₂O (g) + 4NO (g)

(-228.6 + 87.6) + (-16.4)
(-16.4 x 4) - [(-228.6 x 6) + (87.6 x 4)]
[-228.6 + (87.6 x 4)] - (-16.4 x 4)
[(-228.6 x 6) + (87.6 x 4)] - (-16.4 x 4)

Key Concepts

Calculating ΔG° from ΔG° Formation

Question 17

Marks: 1

Which statements are correct for ionic compounds?

Solubility in water depends on the relative magnitude of the lattice energy compared to the hydration energy
Melting points of ionic compounds increase as the size of the cation increases
The enthalpy of solution for calcium chloride is represented by CaCl₂ (s) → CaCl₂ (aq)

I and II only
I and III only
II and III only
I, II and III

Key Concepts

Size & Charge of Ions & Lattice Enthalpy
Calculations from Dissolution Cycles

Question 18

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Question 19

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Question 20

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A student experimentally determined the rate expression for the reaction between iodine and propanone to be:

Rate = k [H⁺] [C₃H₆O]

Which graph is consistent with this information?

q2_16-1_-medium-rate-expression--reaction-mechanism_ib_hl

Key Concepts

Graphical Representations of Reaction Order

Question 21

Marks: 1

The following information was obtained for the rate constant, k, for a reaction at 25 ^OC

A	E_a	R
2.57 × 10⁹ s^–1	96.2 kJ mol^–1	8.31 J K^–1 mol^–1

Which expression correctly represents how to calculate the rate constant, k?

k = (2.57 x 10⁹) x e^{(-96.2 / 8.31×25)}
k = (2.57 x 10⁹) x e^{(-96.2 / 8.31×298)}
k = (2.57 x 10⁹) x e^{(-96200 / 8.31×25)}
k = (2.57 x 10⁹) x e^{(-96200 / 8.31×298)}

Key Concepts

The Arrhenius Equation

Question 22

Marks: 1

Consider the following reversible reaction:

3O₂ (g) ⇌ 2O₃ (g)

What is the value of K_cwhen the equilibrium concentrations are [O₂] = 4.0 mol dm^-3and [O₃] = 4.0 mol dm^-3 ?

0.25
4
16
64

Key Concepts

Equilibrium Problems

Question 23

Marks: 1

Which of the following equations is used when calculating the temperature, in Kelvin, at which a reaction becomes feasible if ΔH^Θ = x and ΔS^Θ = y.

T = $\frac{x}{y}$
T = x y
T = x + y
T = $\frac{y}{x}$

Key Concepts

Calculating ΔG° from the Gibbs Equation

Question 24

Marks: 1

In the Brønsted–Lowry theory of acids and bases, the difference between a conjugate acid and its conjugate base is the presence of which of the following?

a positive charge
a pair of electrons
a proton
a hydrogen atom

Question 25

Marks: 1

How many different types of ions can be found in acid rain, assuming it contains a mixture of sulfuric, sulfurous, nitric and nitrous acids?

4
5
6
7

Question 26

Marks: 1

Which of the following statements are correct for a titration between 0.10 mol dm^-3 propanoic acid and 0.10 mol dm^-3 potassium hydroxide?

The equivalence point will be at pH 7
The salt formed will hydrolyse to form an acidic salt
The salt formed will be CH₃COOK
At half equivalence point [CH₃CH₂COOH (aq)] = [CH₃CH₂COO^- (aq)]

Key Concepts

pH Curves
Salt Hydrolysis

Question 27

Marks: 1

Which of the following statements is correct?

As temperature increases, the pH value of pure water decreases
As temperature decreases, the pH value of pure water decreases
The pH of water is unaffected by temperature
Pure water is not neutral

Key Concepts

Relating Kw to Ka

Question 28

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Question 29

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Which of the following reactions could take place at the positive electrode (cathode) in a voltaic cell?

Cu²⁺ (aq) to Cu (s)
Br₂ (g) to Br^- (aq)
Co³⁺ (aq) to Co²⁺(aq)

I and II only
I and III only
II and III only
I, II and III

Question 30

Marks: 1

Consider these standard electrode potentials.

Fe²⁺ (aq) + 2e^- $⇌$ Fe (s) E^Θ = -0.45 V

Cu²⁺(aq) + 2e^- $⇌$ Cu (s) E^Θ = +0.15 V

Which is the correct working to determine E^Θ_cell?

E^Θ_cell= 0.15 - (-0.45)
E^Θ_cell= 0.15 + (-0.45)
E^Θ_cell= (-0.45) - 0.15
E^Θ_cell= 0.15 x (-0.45)

Key Concepts

Cell Potential Calculations

Question 31

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Question 32

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Which factors affect the rate of nucleophilic substitution in halogenoalkanes?

The nature of the attacking nucleophile
The structure of the halogenoalkane
The identity of the halogen

I and II only
I and III only
II and III only
I, II and III

Key Concepts

Factors Affecting Nucleophilic Substitution

Question 33

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Question 34

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An alkene, X, undergoes electrophilic addition with hydrogen bromide to form a halogenoalkane, Y, as the minor product.

The halogenoalkane, Y , can react with sodium hydroxide in aqueous conditions to form butan-1-ol.

What is the correct identity of the alkene, X?

2-methylpropene
But-1-ene
But-2-ene
Pent-1-ene

Question 35

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Question 36

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What is this molecule called?
q2_20-3_ib_hl_medium_mcq

Z-2-bromo-1-chloro-2-fluoroethene
E-2-bromo-1-chloro-2-fluoroethene
Z-1-bromo-2-chloro-1-fluoroethene
E-1-bromo-2-chloro-1-fluoroethene

Question 37

Marks: 1

The synthesis of 2-propyl propanoate can be carried out in two steps:

I

CH₃COCH₃ → CH₃CH(OH)CH₃

II

CH₃CH(OH)CH₃ → C₂H₅COOCH(CH₃)₂

What are the reagents needed in I and II?

	I	II
A	potassium dichromate(VI)	sulfuric acid, propanoic acid
B	sodium borohydride	sulfuric acid, propanoic acid
C	sodium borohydride	sulfuric acid, ethanoic acid
D	potassium dichromate(VI)	sulfuric acid, ethanoic acid

Question 38

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Question 39

Marks: 1

The ¹H NMR spectrum of CH₃CHCl₂ shows two signals.

What is the correct assignment of splitting patterns for these signals?

	CH₃ group	CH group
A	doublet	quartet
B	quartet	doublet
C	singlet	singlet
D	triplet	singlet

Key Concepts

High Resolution NMR

Question 40

Marks: 1

Which row correctly describes the splitting pattern observed on the ¹H NMR spectrum for each labelled hydrogen?

q2_21-1_spectroscopic-identification-of-organic-compounds_medium_ib_hl

One doublet and four triplets
One triplet, one quartet and one singlet
One triplet, one doublet and three singlets
One triplet, one quartet and three singlets

DP IB Chemistry: HL

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