Structure 1. Models of the particulate nature of matter

1.1 Introduction to the particulate nature of matter

1.2 The nuclear atom

1.3 Electron configurations

1.4 The mole

1.5 Ideal gases

Structure 2. Models of bonding and structure

2.1 The ionic model

2.2 The covalent model

2.3 The metallic model

2.4 From models to materials

Structure 3. Classification of matter

3.1 The periodic table

3.2 Functional groups: Organic compounds

Reactivity 1. What drives chemical reactions?

1.1 Measuring enthalpy changes

1.2 Energy cycles

1.3 Energy from fuels

Reactivity 2. How much, how fast and how far?

2.1 Amount of chemical change

2.2 Rate of chemical change

2.3 Extent of chemical change

Reactivity 3. What are the mechanisms of chemical change?

3.1 Proton transfer reactions

3.2 Electron transfer reactions

3.3 Electron sharing reactions (Radicals)

3.4 Electron-pair sharing reactions

IB Chemistry HL 2.1 Amount of chemical change Question Bank

[Maximum number: 4]

Two groups of students (Group A and Group B) carried out a project* on the chemistry of some group 7 elements (the halogens) and their compounds.

(a)

In the first part of the project, the two groups had a sample of iodine monochloride (a corrosive brown liquid) prepared for them by their teacher using the following reaction.

\mathrm{I}_{2}(\mathrm{~s})+\mathrm{Cl}_{2}(\mathrm{~g}) \rightarrow 2 \mathrm{ICl}(\mathrm{l})

The following data were recorded.

[ 4 ]

(i)

The iodine used in the reaction was in excess. Determine the theoretical yield, in g , of ICl(l).

[ 3 ]

(ii)

Calculate the percentage yield of ICl(l).

[ 1 ]

[Maximum number: 1]

Nitrogen monoxide, NO(g), is produced in internal combustion and jet engines.

(a)

In an exhaust pipe catalytic converter, NO reacts with carbon monoxide, CO , to form $\mathrm{N}_{2}$ .

[ 1 ]

(i)

Deduce the second product and the balanced equation for the reaction.

[ 1 ]

[Maximum number: 1]

Nitrogen dioxide, $\mathrm{NO}_{2}$ , is a brown, toxic and corrosive gas. It can be made in a school laboratory by heating a group II metal nitrate or by the reaction of copper, Cu , with concentrated nitric acid, $\mathrm{HNO}_{3}$ .

(a)

(i)

Deduce the coefficients in the equation for the reaction of Cu with concentrated $\mathrm{HNO}_{3}$ .

{ }_{-} \mathrm{Cu}(\mathrm{~s})+{ }_{-} \mathrm{HNO}_{3}(\mathrm{aq}) \rightarrow{ }_{-} \mathrm{Cu}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{aq})+{ }_{-} \mathrm{NO}_{2}(\mathrm{~g})+{ }_{-} \mathrm{H}_{2} \mathrm{O}(\mathrm{l})

[ 1 ]

[Maximum number: 3]

A powder has the following percentage composition by mass:
30.0 % sucrose, $\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}$
45.0 % citric acid, $\mathrm{C}_{6} \mathrm{H}_{8} \mathrm{O}_{7}$
25.0 \% sodium hydrogencarbonate, $\mathrm{NaHCO}_{3}$

In the presence of water, the powder effervesces as the citric acid reacts with the sodium hydrogencarbonate:

$3 \mathrm{NaHCO}_{3}(\mathrm{~s})+\mathrm{C}_{6} \mathrm{H}_{8} \mathrm{O}_{7}(\mathrm{aq}) \rightarrow \mathrm{Na}_{3}\left(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{O}_{7}\right)(\mathrm{aq})+3 \mathrm{CO}_{2}(\mathrm{~g})+3 \mathrm{H}_{2} \mathrm{O}(\mathrm{l})$

(a)

(i)

Determine the limiting reactant when 1.00 g of this powder reacts.

[ 3 ]

[Maximum number: 1]

A student determined the percentage of the active ingredient magnesium hydroxide, $\mathrm{Mg}(\mathrm{OH})_{2}$ , in a 1.24 g antacid tablet.

The antacid tablet was added to $50.00 \mathrm{~cm}^{3}$ of $0.100 \mathrm{~mol} \mathrm{dm}^{-3}$ sulfuric acid, which was in excess.

(a)

Calculate the amount of $\mathrm{H}_{2} \mathrm{SO}_{4}$ that reacted with $\mathrm{Mg}(\mathrm{OH})_{2}$ .

[ 1 ]

[Maximum number: 1]

4.0 g of solid sodium hydroxide is added to $0.10 \mathrm{dm}^{3}$ of $1.0 \mathrm{moldm}^{-3}$ aqueous sulfuric acid.

2 \mathrm{NaOH}(\mathrm{~s})+\mathrm{H}_{2} \mathrm{SO}_{4}(\mathrm{aq}) \rightarrow \mathrm{Na}_{2} \mathrm{SO}_{4}(\mathrm{aq})+2 \mathrm{H}_{2} \mathrm{O}(\mathrm{l})

Which statement is correct?

Neither reactant is in excess.

$0.10 \mathrm{~mol} \mathrm{Na}_{2} \mathrm{SO}_{4}$ is formed.

Excess $\mathrm{H}_{2} \mathrm{SO}_{4}$ remains in solution.

Excess NaOH remains in solution.

[Maximum number: 4]

3.26 g of iron powder are added to $80.0 \mathrm{~cm}^{3}$ of $0.200 \mathrm{~mol} \mathrm{dm}^{-3}$ copper(II) sulfate solution. The following reaction occurs:

\mathrm{Fe}(\mathrm{~s})+\mathrm{CuSO}_{4}(\mathrm{aq}) \rightarrow \mathrm{FeSO}_{4}(\mathrm{aq})+\mathrm{Cu}(\mathrm{~s})

(a)

(i)

Determine the limiting reactant showing your working.

[ 2 ]

(ii)

The mass of copper obtained experimentally was 0.872 g . Calculate the percentage yield of copper.

[ 2 ]

[Maximum number: 3]

Chlorine undergoes many reactions.

(a)

2.67 g of manganese(IV) oxide was added to $200.0 \mathrm{~cm}^{3}$ of $2.00 \mathrm{~mol} \mathrm{dm}^{-3} \mathrm{HCl}$ .

\mathrm{MnO}_{2}(\mathrm{~s})+4 \mathrm{HCl}(\mathrm{aq}) \rightarrow \mathrm{Cl}_{2}(\mathrm{~g})+2 \mathrm{H}_{2} \mathrm{O}(\mathrm{l})+\mathrm{MnCl}_{2}(\mathrm{aq})

[ 3 ]

(i)

Determine the limiting reactant, showing your calculations.

[ 2 ]

(ii)

Determine the excess amount, in mol , of the other reactant.

[ 1 ]

[Maximum number: 1]

0.10 mol of hydrochloric acid is mixed with 0.10 mol of calcium carbonate.

[Maximum number: 1]

Ammonium nitrate, $\mathrm{NH}_{4} \mathrm{NO}_{3}$ , is used as a high nitrogen fertilizer.

(a)

Solid ammonium nitrate can decompose to gaseous dinitrogen monoxide and liquid water.

[ 1 ]

(i)

Write the chemical equation for this decomposition.

[ 1 ]

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