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 1.1 Introduction to the particulate nature of matter Question Bank

[Maximum number: 2]

Iron(II) sulfide can be produced by heating powdered iron and sulfur together.

(a)

Describe the difference between an element and a compound.

[ 2 ]

[Maximum number: 1]

Which of the following are homogeneous mixtures?

I. An aqueous solution of sodium chloride
II. A mixture of pentane and hexane
III. A mixture of ethanol and water

I and II only

I and III only

II and III only

I, II and III

[Maximum number: 1]

Which equation represents sublimation?

$2 \mathrm{Al}(\mathrm{s})+3 \mathrm{I}_{2}(\mathrm{~g}) \rightarrow 2 \mathrm{AlI}_{3}(\mathrm{~s})$

$\mathrm{HgCl}_{2}(\mathrm{~s}) \rightarrow \mathrm{HgCl}_{2}(\mathrm{~g})$

$\mathrm{I}_{2}(\mathrm{~g}) \rightarrow \mathrm{I}_{2}(\mathrm{~s})$

$\mathrm{CaCO}_{3}(\mathrm{~s})+2 \mathrm{HCl}(\mathrm{aq}) \rightarrow \mathrm{CaCl}_{2}(\mathrm{aq})+\mathrm{CO}_{2}(\mathrm{~g})+\mathrm{H}_{2} \mathrm{O}(\mathrm{l})$

[Maximum number: 1]

What happens as ice melts at $0^{\circ} \mathrm{C}$ ?

I. Molecules gain kinetic energy and temperature increases.
II. Added energy overcomes hydrogen bonds between molecules.
III. Molecules gain sufficient energy to move from fixed positions.

I and II only

I and III only

II and III only

I, II and III

[Maximum number: 2]

Alkanes are commonly occurring organic compounds.

(a)

The first four straight chain alkanes are gases at room temperature.

Boiling points of straight chain alkanes

[ 2 ]

(i)

Explain why the volume occupied by a sample of propane increases sharply when the sample is heated up from 200 to 250 K at constant pressure.

[ 2 ]

[Maximum number: 2]

Physical properties of elements vary according to atomic number. Sections 6 to 9 of the data booklet list some of these properties.

Melting points and boiling points of elements 1 to 95

(a)

Deduce, giving a reason, the group of elements in the periodic table most likely to undergo sublimation.

[ 2 ]

[Maximum number: 1]

Which one of the following observations provides evidence that matter is composed of atoms?

The line emission spectra of hydrogen produce four visible lines.

Sodium chloride is soluble in water and conducts electricity in the aqueous state.

Water is a liquid at room temperature, but hydrogen sulfide and hydrogen selenide are gases.

12.0 g of carbon combines with either 16.0 g or 32.0 g of oxygen but never any other ratio.

[Maximum number: 1]

Students were asked to investigate how a change in concentration of hydrochloric acid, HCl , affects the initial rate of its reaction with marble chips, $\mathrm{CaCO}_{3}$ .

They decided to measure how long the reaction took to complete when similar chips were added to $50.0 \mathrm{~cm}^{3}$ of $1.00 \mathrm{~mol} \mathrm{dm}^{-3}$ acid and $50.0 \mathrm{~cm}^{3}$ of $2.00 \mathrm{~mol} \mathrm{dm}^{-3}$ acid.

Two methods were proposed:
(1) using small chips, keeping the acid in excess, and recording the time taken for the solid to disappear
(2) using large chips, keeping the marble in excess, and recording the time taken for bubbles to stop forming.

(a)

Annotate the balanced equation below with state symbols.

\mathrm{CaCO}_{3}\left(\_\right)+2 \mathrm{HCl}\left(\_\right) \rightarrow \mathrm{CaCl}_{2}\left(\_\right)+\mathrm{CO}_{2}\left(\_\right)+\mathrm{H}_{2} \mathrm{O}\left(\_\right)

[ 1 ]

[Maximum number: 2]

A student was given a mixture to separate and collect the individual components. The mixture contained sand, $\mathrm{SiO}_{2}(\mathrm{~s})$ , sodium chloride, NaCl(s), and iron filings, Fe(s). The student observed the original mixture and made the following hypothesis.

The iron would have the lowest percent by mass because it appeared to be present in the smallest quantity.

(a)

In a different experiment, the students needed to separate a mixture of methanol and butan-1-ol. State the best method to separate this mixture and the physical property used for the separation.

Separation method:

Physical property:

[ 2 ]

[Maximum number: 2]

Sodium thiosulfate solution reacts with dilute hydrochloric acid to form a precipitate of sulfur at room temperature.

\mathrm{Na}_{2} \mathrm{~S}_{2} \mathrm{O}_{3}(\mathrm{aq})+2 \mathrm{HCl}(\mathrm{aq}) \rightarrow \mathrm{S}(\mathrm{~s})+\mathrm{SO}_{2}(\mathrm{~g})+2 \mathrm{NaCl}(\mathrm{aq})+\mathrm{X}

(a)

Identify the formula and state symbol of X .

[ 1 ]

(b)

Suggest why the experiment should be carried out in a fume hood or in a well-ventilated laboratory.

[ 1 ]

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