Free Printable AQA Chemistry Topic 1, 2 and 3: Atomic Structure and the Periodic Table, Bonding, Structure, and the Properties of Matter, and Quantitative Chemistry

1.

What is the Charge of a Proton?

a)

Positive Charge

b)

Negative Charge

c)

Neutral Charge

2.

What is the Charge of an Electron?

a)

Positive Charge

b)

Negative Charge

c)

Neutral Charge

3.

What is the Charge of a Neutron?

a)

Positive Charge

b)

Negative Charge

c)

Neutral Charge

4.

What does the Nucleus of an atom contain?

a)

Protons

b)

Electrons

c)

Neutrons

5.

Relative Atomic Mass = sum of (isotope abundance x isotope mass number/ sum of all abundances of all the isotopes

a)

ANSWER

b)

DO NOT CLICK

6.

What is a compound?

a)

A substance formed from a two or more elements held by chemical bonds

b)

A mixture of two or more chemicals which provides a useful outcome

7.

What is a Mixture?

a)

A substance formed from a two or more elements held by chemical bonds

b)

A mixture of elements or compounds which can be physically separated

8.

Which one is Filtration?

a)

Used if the product is an insoluble solid and needs to be separated from a liquid. Uses filter paper

b)

Used if the product is a soluble solid. Its placed in an evaporating basin and heated until crystals form

c)

Used if the product is a soluble solid. Its placed in an evaporating basin and heated until start crystals forming then the heat is removed letting the crystals form while cool. Its then Filtered out

9.

Which one is Evaporation?

a)

Used if the product is an insoluble solid and needs to be separated from a liquid. Uses filter paper

b)

Used if the product is a soluble solid. Its placed in an evaporating basin and heated until crystals form

c)

Used if the product is a soluble solid. Its placed in an evaporating basin and heated until start crystals forming then the heat is removed letting the crystals form while cool. Its then Filtered out

10.

Which one is Crystalisation?

a)

Used if the product is an insoluble solid and needs to be separated from a liquid. Uses filter paper

b)

Used if the product is a soluble solid. Its placed in an evaporating basin and heated until crystals form

c)

Used if the product is a soluble solid. Its placed in an evaporating basin and heated until start crystals forming then the heat is removed letting the crystals form while cool. Its then Filtered out

11.

What is Simple Distillation used for?

a)

Separating out Solutions

b)

Separating out a Mixture of Liquids

12.

What is Fractional Distillation used for?

a)

Separating out Solutions

b)

Separating out a Mixture of Liquids

13.

Which one is Simple Distillation?

a)

Solution is Heated. The part with the lowest boiling point evaporates, gets cooled and Condenses and gets collected.

b)

Mixture of liquids is Heated. They rise through a fractionating column the lowest boiling point is collected, temperature is raised and then the next one is collected.

14.

Which one is Fractional Distillation?

a)

Solution is Heated. The part with the lowest boiling point evaporates, gets cooled and Condenses and gets collected.

b)

Mixture of liquids is Heated. They rise through a fractionating column the lowest boiling point is collected, temperature is raised and then the next one is collected.

15.

What is the first step in developing the modern day model of an atom?

a)

John Dalton published his ideas about atoms. He thought that all matter was made of tiny particles called atoms, which he imagined as tiny spheres that could not be divided.

b)

J J Thomson carried out experiments and discovered the electron. He made the plum pudding model of the atom. In this model, the atom is a ball of positive charge with negative electrons embedded in it.

c)

Ernest Rutherford did the alpha scattering experiment through which he discovered that the mass of an atom is concentrated at its centre and the nucleus is positively charged. He called it the nuclear model.

d)

Niels Bohr did calculations that led him to suggest that electrons orbit the nucleus in shells. The shells are at certain distances from the nucleus.

e)

James Chadwick found evidence for the existence of particles in the nucleus with mass but no charge. These particles are called neutrons.

16.

What is the second step in developing the modern day model of an atom?

a)

John Dalton published his ideas about atoms. He thought that all matter was made of tiny particles called atoms, which he imagined as tiny spheres that could not be divided.

b)

J J Thomson carried out experiments and discovered the electron. He made the plum pudding model of the atom. In this model, the atom is a ball of positive charge with negative electrons embedded in it.

c)

Ernest Rutherford did the alpha scattering experiment through which he discovered that the mass of an atom is concentrated at its centre and the nucleus is positively charged. He called it the nuclear model.

d)

Niels Bohr did calculations that led him to suggest that electrons orbit the nucleus in shells. The shells are at certain distances from the nucleus.

e)

James Chadwick found evidence for the existence of particles in the nucleus with mass but no charge. These particles are called neutrons.

17.

What is the third step in developing the modern day model of an atom?

a)

John Dalton published his ideas about atoms. He thought that all matter was made of tiny particles called atoms, which he imagined as tiny spheres that could not be divided.

b)

J J Thomson carried out experiments and discovered the electron. He made the plum pudding model of the atom. In this model, the atom is a ball of positive charge with negative electrons embedded in it.

c)

Ernest Rutherford did the alpha scattering experiment through which he discovered that the mass of an atom is concentrated at its centre and the nucleus is positively charged. He called it the nuclear model.

d)

Niels Bohr did calculations that led him to suggest that electrons orbit the nucleus in shells. The shells are at certain distances from the nucleus.

e)

James Chadwick found evidence for the existence of particles in the nucleus with mass but no charge. These particles are called neutrons.

18.

What is the fourth step in developing the modern day model of an atom?

a)

John Dalton published his ideas about atoms. He thought that all matter was made of tiny particles called atoms, which he imagined as tiny spheres that could not be divided.

b)

J J Thomson carried out experiments and discovered the electron. He made the plum pudding model of the atom. In this model, the atom is a ball of positive charge with negative electrons embedded in it.

c)

Ernest Rutherford did the alpha scattering experiment through which he discovered that the mass of an atom is concentrated at its centre and the nucleus is positively charged. He called it the nuclear model.

d)

Niels Bohr did calculations that led him to suggest that electrons orbit the nucleus in shells. The shells are at certain distances from the nucleus.

e)

James Chadwick found evidence for the existence of particles in the nucleus with mass but no charge. These particles are called neutrons.

19.

What is the fifth step in developing the modern day model of an atom?

a)

John Dalton published his ideas about atoms. He thought that all matter was made of tiny particles called atoms, which he imagined as tiny spheres that could not be divided.

b)

J J Thomson carried out experiments and discovered the electron. He made the plum pudding model of the atom. In this model, the atom is a ball of positive charge with negative electrons embedded in it.

c)

Ernest Rutherford did the alpha scattering experiment through which he discovered that the mass of an atom is concentrated at its centre and the nucleus is positively charged. He called it the nuclear model.

d)

Niels Bohr did calculations that led him to suggest that electrons orbit the nucleus in shells. The shells are at certain distances from the nucleus.

e)

James Chadwick found evidence for the existence of particles in the nucleus with mass but no charge. These particles are called neutrons.

20.

What ions do Metals form when they react?

a)

Positive Ions

b)

Negative Ions

21.

Select all the properties of a Metal:

a)

Strong

b)

Malleable

c)

Conductive

d)

Brittle

22.

Select the 3 things that describe Group 1 Elements as you go DOWN the group:

a)

More Reactive

b)

Lower Melting/Boiling Point

c)

Higher relative atomic mass

d)

Less Reactive

e)

Higher Melting/Boiling Point

23.

Select the 3 things that describe Group 7 Elements as you go DOWN the group:

a)

More Reactive

b)

Lower Melting/Boiling Point

c)

Higher relative atomic mass

d)

Less Reactive

e)

Higher Melting/Boiling Point

24.

Which one describes a reaction between a Group 1 metal and Water?

a)

Vigorous Reaction to produce Hydrogen Gas and a Metal Hydroxide

b)

Vigorous Reaction when Heated to form Metal Chloride Salts

c)

Reacts to form a Metal Oxide

25.

Which one describes a reaction between a Group 1 metal and Chlorine?

a)

Vigorous Reaction to produce Hydrogen Gas and a Metal Hydroxide

b)

Vigorous Reaction when Heated to form Metal Chloride Salts

c)

Reacts to form a Metal Oxide

26.

What happens to the Boiling point of Nobel Gases as you go Down the Group?

a)

Increases

b)

Decreases

27.

What is Ionic Bonding?

a)

Happens when a Metal and a Non-Metal react together. They form oppositely charged ions and get strongly attracted by electrostatic forces.

b)

Happens when two Non-Metals react together. They share the electrons in their outer shells forming bonds.

c)

Happens when two Metals react together. The electrons in the outer shell are delocalised causing a strong attraction between the positive metal ions and the negative electrons.

28.

What is Covalent Bonding?

a)

Happens when a Metal and a Non-Metal react together. They form oppositely charged ions and get strongly attracted by electrostatic forces.

b)

Happens when two Non-Metals react together. They share the electrons in their outer shells forming bonds.

c)

Happens when two Metals react together. The electrons in the outer shell are delocalised causing a strong attraction between the positive metal ions and the negative electrons.

29.

What is Metallic Bonding?

a)

Happens when a Metal and a Non-Metal react together. They form oppositely charged ions and get strongly attracted by electrostatic forces.

b)

Happens when two Non-Metals react together. They share the electrons in their outer shells forming bonds.

c)

Happens when two Metals react together. The electrons in the outer shell are delocalised causing a strong attraction between the positive metal ions and the negative electrons.

30.

Which one is True?

a)

Ionic Compounds have a Giant Ionic Lattice they have Strong Electrostatic forces of attraction between oppositely charged ions in the lattice.

b)

Ionic Compounds have a Giant Ionic Lattice they have Strong Magnetic forces between the ions in the lattice.

31.

Which one is Diamond?

a)

Each Carbon atom forms four covalent bonds in a rigid Covalent structure

b)

Each Carbon atom forms three covalent bonds to create hexagonal layers. Each carbon atom has one delocalised electron

c)

A giant covailant structure of silicon and oxygen

32.

Which one is Graphite?

a)

Each Carbon atom forms four covalent bonds in a rigid Covalent structure

b)

Each Carbon atom forms three covalent bonds to create hexagonal layers. Each carbon atom has one delocalised electron

c)

A giant covailant structure of silicon and oxygen

33.

Which one is Silicon Dioxide(Sand) ?

a)

Each Carbon atom forms four covalent bonds in a rigid Covalent structure

b)

Each Carbon atom forms three covalent bonds to create hexagonal layers. Each carbon atom has one delocalised electron

c)

A giant covailant structure of silicon and oxygen

34.

Select the Correct equation for calculating concentration in g/dm^3

a)

concentration = mass of solute / volume of solvent

b)

concentration = moles of solute / volume of solvent

35.

Select the Correct equation for calculating concentration in mol/dm^3

a)

concentration = mass of solute / volume of solvent

b)

concentration = moles of solute / volume of solvent

36.

What type of elements bond with ionic bonds?

a)

A. Metals with metals

b)

B. Metals with non-metals

c)

C. Non-metals with non-metals

d)

D. Metals with compounds

37.

In an ionic bond, the metal ion is

a)

A. Positively charged because it has gained electrons

b)

B. Negatively charged because it has lost electrons

c)

C. Positively charged because it has lost electrons

d)

D. Neutral because it hasn’t lost or gained electrons

38.

In an ionic bond, the non-metal ion is

a)

A. Positively charged because it has gained electrons

b)

B. Negatively charged because it has gained electrons

c)

C. Positively charged because it has lost electrons

d)

D. Neutral because it hasn’t lost or gained electrons

39.

Why is graphite so soft?

a)

A. The atoms are arranged in hexagons in layers that are held together strongly

b)

B. The atoms are arranged in hexagons in layers that are held together weakly

c)

C. Carbon is strongly bonded to 3 other carbon atoms.

d)

D. Carbon is weakly bonded to 3 other carbon atoms.

40.

The delocalised electrons in a metal lattice come from the

a)

A. Outer shell of electrons

b)

B. The inner shells

c)

C. The nucleus

d)

D. The background atmosphere

41.

What element are diamond and graphite made up of?

a)

A. Sodium

b)

B. Carbon

c)

C. Carbon dioxide

d)

D. Silicon

42.

The number of bonds each carbon atom has in diamond is

a)

A. 6

b)

B. 5

c)

C. 3

d)

D. 4

43.

Why do simple molecules have low melting points?

a)

A. The intermolecular forces are very strong

b)

B. The intramolecular forces are very weak.

c)

C. The intramolecular forces are very strong.

d)

D. The intermolecular forces are very weak.

44.

Why don’t simple molecules don’t conduct electricity in any state?

a)

A. Their ions are not free to move.

b)

B. The covalent bonds are too strong.

c)

C. They don’t contain ions or free moving electrons.

d)

D. They are not solids

45.

What makes an atom energetically stable?

a)

A. Eight electrons in their inner shell.

b)

B. More neutrons than electrons.

c)

C. A full outer shell of electrons.

d)

D. More protons than neutrons.

46.

Which of these is a mixture?

a)

A. Carbon dioxide

b)

B. Sea water

c)

C. Sodium chloride

d)

D. Water

47.

How could we separate two or more liquids?

a)

A. Filtration

b)

B. Chromatography

c)

C. Fractional distillation

d)

D. Sieving

48.

How could a mixture of food colourings be separated?

a)

A. Chromatography

b)

B. Filtration

c)

C. Fractional distillation

d)

D. Sieving

49.

Which of these is a chemical reaction?

a)

A. Distillation

b)

B. Evaporation

c)

C. Melting

d)

D. Frying an egg

50.

What does the plum pudding model of the atom suggest?

a)

A. An atom has a positive nucleus orbited by negative electrons.

b)

B. An atom has a distinct nucleus.

c)

C. An atom is a ball of dilute positive charge with neutrons in it

d)

D. An atom is a ball of dilute positive charge with electrons in it.

51.

The nuclear model of the atom tells us that:

a)

A. The mass of the atom is concentrated at the centre

b)

B. An atom has protons, neutrons and electrons in the nucleus.

c)

C. An atom has electrons in the nucleus

d)

D. An atom has a nucleus made up of neutrons only

52.

Which of these statements best describes how scientific ideas became accepted?

a)

A. New evidence is discovered which is published if it is likely to make a lot of money.

b)

B. New evidence is discovered and published.

c)

C. New evidence is discovered, peer reviewed and published

d)

D. Scientists ignore new evidence if it does not agree with important theories.

53.

What is the relative atomic mass of sodium?

a)

11

b)

23

c)

46

d)

64

54.

What is the atomic mass of magnesium?

a)

2

b)

4

c)

12

d)

24

55.

What is the relative molecular mass of fluorine gas, F₂?

a)

19

b)

38

c)

9

d)

18

56.

What is the relative formula mass of NaOH?

a)

20

b)

39

c)

40

d)

45

57.

What is the relative molecular mass of CO₂?

a)

12

b)

16

c)

32

d)

44

58.

What is the mass number?

a)

the number of protons

b)

the number of protons and neutrons

c)

the number of neutrons

d)

the number of protons and electrons

59.

Iron forms an oxide with the formula Fe₂O₃.

What is the relative formula mass of this compound?

a)

A 76

b)

B 100

c)

C 136

d)

D 160

60.

The structure of an organic compound, X, is shown.

What is the molecular formula of X?

a)

A C₆H₉

b)

B C₆H₁₂

c)

C C₇H₁₂

d)

D C₇H1₄

61.

Which relative molecular mass, M_r, is not correct for the molecule given?

a)

A

b)

B

c)

C

d)

D

62.

At higher temperatures

a)

particles in an object have less energy

b)

particles in an object move faster

c)

a gas contracts

63.

A gas

a)

has a definite shape but no definite volume

b)

has a definite volume but no definite shape

c)

has fast-moving particles

64.

Freezing

a)

Solid to gas

b)

Liquid to solid

c)

Gas to solid

d)

Liquid to gas

65.

Boiling

a)

liquid to gas

b)

gas to solid

c)

gas to liquid

d)

solid to liquid

66.

Which state of matter has tightly packed molecules?

a)

solid

b)

liquid

c)

gas

67.

Which state of matter has a definite shape?

a)

solid

b)

liquid

c)

gas

68.

What is matter?

a)

Anything that has mass and volume

b)

The shape of an object

c)

How much an object weighs

d)

The pull of objects on one another

69.

Volume is.....

a)

the weight of an object

b)

the gravity of an object

c)

how much space an object takes up

d)

measured with a balance scale

70.

A material or object that does not easily allow heat, electricity, light, or sound to pass through is _____________

a)

conductor

b)

insulator

c)

wire

d)

solid

71.

My glass of ice water is sitting in the sun and has droplets of water on the outside of the glass. What is happening?

a)

condensation

b)

evaporation

c)

melting

d)

freezing

72.

Which state of matter has the highest kinetic energy?

a)

solid

b)

liquid

c)

gas

d)

matter

AQA Chemistry Topic 1, 2 and 3: Atomic Structure and the Periodic Table, Bonding, Structure, and the Properties of Matter, and Quantitative Chemistry

Total questions: 72

Worksheet time: 2hrs 36mins

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