IGCSE Chem Practice Test Ch01-04

Chapter 1 Kinetic Theory and Diffusion 1.1

Benzene melts at 5.5°C and boils at 80.1°C. Which one of the following statements is true about benzene?

A The only movement that the particles in benzene have at a temperature of 20°C is vibration about a fixed point.

B At 100°C, the particles in benzene are well scattered and moving at random.

C At 0°C, benzene is a liquid.

D If you cooled benzene from 100°C to 50°C, the change of state that happens at 80.1°C is called sublimation.

1.2

Choose the word from the list below that best describes the change of state which happens when a purple vapour turns into a purple solid on cooling.

A freezing

B sublimation

C condensation

D evaporation

1.3

Choose the word from the list below that best describes the change of state which happens when a few drops of water on a bench gradually disappear.

A freezing

B sublimation

C condensation

D evaporation

1.4

Choose the word from the list below that best describes the change of state which happens when colourless liquid naphthalene turns into white crystals.

A freezing

B sublimation

C condensation D evaporation

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1.5

Which one of the following statements about particles in solids, and liquids is not true?

A When a solid is heated, the particles vibrate faster and faster until the forces holding them together are broken, and they become free to move around.

B Particles in a liquid are quite closely packed, but have some freedom to move around.

C When a liquid is heated, the heat energy makes the particles lighter, which is why they escape more easily from the surface of a hot liquid than a cold one.

D For most substances, the particles in the liquid are slightly further apart than they are in the solid, and so the liquid is less dense than the solid.

1.6

The relative masses of the particles of four gases are:

helium 4

methane 16

oxygen 32

sulfur dioxide 64

The gas which diffuses most quickly is

A helium

B methane

C oxygen

D sulfur dioxide

1.7

Experiments show that if some brown bromine vapour is released into a large flask which is full of air, the colour spreads evenly through the flask over a minute or so. However, if the bromine is released into the same flask which contains a vacuum, the colour fills the whole flask in a fraction of a second. The reason for this is

A Bromine particles travel at about 200 metres per second in a vacuum, but only 100 metres per second through the air.

B Bromine particles are heavier than air particles, and heavy particles move more slowly than lighter ones.

C The vacuum sucks the bromine into it.

D In air, bromine particles keep bumping into air particles which slows the process down. In a vacuum, nothing gets in their way.

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1.8

This question is about an experiment to find out the relative speeds at which the gases ammonia and hydrogen chloride diffuse.

Which one of the following statements is not true?

A Hydrogen chloride particles travel faster than ammonia particles.

B The white ring is solid ammonium chloride produced where the ammonia and hydrogen chloride meet.

C Ammonia particles are lighter than hydrogen chloride particles.

D The time taken for the white ring to form will depend on the length of the tube.

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Chapter 2 Atomic Structure 2.1

Which one of the following statements is true for all elements?

Neutral atoms of the same element contain

A equal numbers of protons and neutrons.

B equal numbers of protons and electrons.

C equal numbers of neutrons and electrons.

D equal numbers of protons, neutrons and electrons.

2.2

Which one of the following statements about the isotopes of a particular element is wrong?

All the isotopes of a particular element have neutral atoms having

A the same atomic number.

B the same number of protons.

C the same number of neutrons.

D the same number of electrons.

2.3

You will need to refer to a copy of the Periodic Table to answer this question.

Which one of the following elements has the electronic structure in this diagram?

A beryllium

B fluorine

C neon

D chlorine

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2.4

You will need to refer to a copy of the Periodic Table to answer this question.

Which one of the following electronic structures represents sulfur?

A 2,8,6

B 2,8,8,8,6

C 2,8,18,4

D 2,6,8

2.5

You may need to refer to a copy of the Periodic Table to answer this question.

Which one of the following electronic structures does not represent a noble gas?

A 2,8

B 2

C 2,8,18,8

D 2,8,8,2

2.6

You will need to refer to a copy of the Periodic Table to answer this question.

Which one of the statements about an atom with an atomic number of 17, and a mass number of 35 is wrong?

A The atom is an isotope of chlorine.

B The electronic structure is 2,8,7.

C The atom contains 17 neutrons.

D It is an isotope of the same element as one with an atomic number of 17 and a mass number of 37.

2.7

You will need to refer to a copy of the Periodic Table to answer this question.

Which one of the following lists of electronic structures consists only of atoms of elements in the same Group of the Periodic Table?

A 2,8,1 2,8,2 2,8,3 B 1 2,1 2,8,1

C 2,7 2,8,1 2,8,5 D 2,2 2,8,2 2,8,8,2

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2.8

You will need to refer to a copy of the Periodic Table to answer this question.

How many electrons are there in the outer level of a strontium atom? The atomic number of strontium is 38.

A 2

B 4

C 6

D 8

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Chapter 3 Bonding 3.1

You will need to refer to a copy of the Periodic Table to answer this question.

A fluorine atom gains an electron to make a fluoride ion, F-. Which one of the following atoms or ions has a different electronic structure from a fluoride ion?

A Na+

B Ne

C Cl-

D Mg2+

3.2

You will need to refer to a copy of the Periodic Table to answer this question.

Which one of the following statements describes what happens when sodium combines with oxygen to form sodium oxide, an ionic compound?

A Two sodium atoms each give an electron to a single oxygen atom.

B One sodium atom gives an electron to one oxygen atom.

C One oxygen atom gives an electron to each of two sodium atoms.

D One oxygen atom gives an electron to one sodium atom.

3.3

You will need to refer to a copy of the Periodic Table to answer this question.

The two atoms in a molecule of oxygen, O2, are joined by

A an ionic bond

B a single covalent bond

C a double covalent bond

D a triple covalent bond

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3.4

You will need to refer to a copy of the Periodic Table to answer this question.

Water, H2O, is a covalent molecule. How many electrons are there in the outer energy level of the oxygen when the bonding is complete (including those shared with the hydrogens)?

A 2

B 4

C 6

D 8

3.5

You will need to refer to a copy of the Periodic Table to answer this question.

Boron trifluoride, is a covalent molecule. How many electrons are there in the outer energy level of the boron when the bonding is complete (including those shared with the fluorines)?

A 0

B 3

C 6

D 8

3.6

You will need to refer to a copy of the Periodic Table to answer this question.

Nitrogen reacts with lithium to form an ionic compound, lithium nitride. By considering what happens to the electrons when a lithium atom combines with a nitrogen atom, work out the charge on a nitride ion.

A +1

B –1

C +3

D –3

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3.7

You will need to refer to a copy of the Periodic Table to answer this question.

Sodium and magnesium metals are both examples of metallic bonding. A metal structure contains an array of positive ions in a sea of delocalised electrons.

Which one of the following statements is false?

A Sodium chloride and magnesium chloride also contain positive sodium and magnesium ions. Metallic bonding is just the same as ionic bonding.

B Delocalised electrons are electrons which aren’t attached to particular atoms, but are free to move throughout the structure.

C Each sodium atom contributes one electron to the sea of electrons; each magnesium atom contributes two electrons to the sea.

D The metallic bond is stronger in magnesium than in sodium.

3.8

Which one of the following statements about water is wrong?

A In liquid water, the molecules are attracted to their neighbours by relatively weak intermolecular forces.

B When you heat water to boiling point, the energy breaks the covalent bonds between the hydrogen and oxygen atoms to produce steam.

C When you cool water to freezing point, the water molecules are moving slowly enough that the intermolecular forces can hold them together as solid ice.

D Intermolecular forces in water are due to slight electrical distortions in water molecules which make some parts slightly negative and other parts slightly positive.

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Chapter 4 Structure 4.1

Which one of the following substances does not consist of a giant structure?

A ice

B copper

C sodium chloride

D graphite

4.2

From the descriptions, which one of the following substances consists of a giant structure?

A A white solid with a melting point of 801°C and a boiling point of 1413°C.

B A colourless poisonous gas.

C A white solid which melts at 80°C and boils at 218°C.

D A colourless liquid which boils at 78°C.

4.3

Potassium bromide has a giant ionic structure. Which one of the following is not likely to be true of potassium bromide?

A It is soluble in water.

B Solid potassium bromide conducts electricity.

C It has a high melting point and boiling point.

D It is likely to have brittle crystals.

4.4

Nickel is a metal. Which one of the following is most unlikely to be a property of pure nickel?

A It conducts electricity.

B It has a high melting point.

C It shatters if you hit a small piece with a hammer.

D It is a good conductor of heat.

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4.5

Octane, a component of petrol (gasoline), has a simple molecular structure. Which one of the following is not likely to be a property of octane?

A It is a liquid with a boiling point of 126°C.

B It is insoluble in water.

C The attractions between its molecules are not very strong.

D It conducts electricity.

4.6

A white crystalline solid melted at 681°C. It didn’t conduct electricity when it was solid, but did conduct when it was molten, when it showed signs of chemical change. The solid was soluble in water, but wouldn’t dissolve in alcohol.

Which one of the following is the most likely structure for the solid?

A metallic structure

B simple molecular structure

C giant covalent structure

D giant ionic structure

4.7

Silicon dioxide is a giant covalent structure consisting of strong silicon-oxygen bonds arranged in a 3-dimensional lattice. Which one of the following properties would you not expect silicon dioxide to have?

A Soluble in water

B Hard

C High melting point

D Insoluble in alcohol

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4.8

The diagram represents

A a compound

B a mixture of compounds

C a mixture of compounds and elements

D a mixture of elements

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