Free Printable Chemistry Paper 1 (Foundation)

1.

What is the relative formula mass of CO₂?

a)

44

b)

32

c)

16

d)

56

2.

Calculate the % composition by mass of oxygen present in H₂SO₄.

a)

16.3%

b)

65.25%

c)

32.6%

d)

57.14%

3.

Formula mass of KBr

a)

119

b)

117g

c)

54

d)

62g

4.

What is the law of conservation of mass?

a)

Mass of products is more than mass of reactants

b)

Mass of reactants is less than mass of products

c)

Mass of reactants is equal to mass of products

5.

Choose a correct unit for concentration.

a)

g

b)

gdm

c)

g/dm³

d)

mol

6.

Give the equation for calculating concentration from the mass of substance and volume of solution.

a)

Concentration = mass x volume

b)

Concentration = mass ÷ volume

7.

50g of sodium hydroxide is dissolved in water to make up 200cm³ . What is the concentration in dm³.

a)

0.25 g/dm³

b)

2.5 g/dm³

c)

25 g/dm³

d)

250 g/dm³

8.

Which element is graphene made from?

a)

Carbon

b)

Copper

c)

Hydrogen

d)

Sodium

9.

Which structure is a fullerene?

a)

A

b)

B

c)

C

d)

D

10.

What type of forces act between the ions in an ionic compound?

a)

Electrostatic

b)

Frictional

c)

Gravitational

d)

Magnetic

11.

What are TWO properties of ionic compounds?

a)

Conducts electricity when molten

b)

High melting point

c)

Low melting point

d)

Small molecules

e)

Weak bonds between particles

12.

Each carbon atoms in graphite is joined to _______ other carbon atoms

a)

Two

b)

Three

c)

Four

13.

What type of bonding holds together the atoms in graphite?

a)

ionic

b)

covalent

c)

metallic

14.

What type of bonding holds together the atoms in graphite?

a)

ionic

b)

covalent

c)

metallic

15.

Why is graphite so soft and slippery?

a)

It is made of layers of atoms

b)

It is made of small molecules

c)

It is an ionic compound

16.

Diamond is made from what type of atoms?

a)

Carbon

b)

Nitrogen

c)

Oxygen

d)

Silicon

17.

The atoms in diamond are joined together by which type of bonds?

a)

Ionic

b)

Covalent

c)

Metallic

18.

In diamond each atom is joined to _______ others

a)

two

b)

three

c)

four

19.

Diamond is suitable for the cutting end of a drill bit because it is

a)

hard

b)

shiny

c)

soft

20.

Which structure has a very low boiling point?

a)

A

b)

B

c)

C

d)

D

e)

E

21.

What type of bond is in a molecule of hydrogen chloride?

a)

Ionic

b)

Covalent

c)

Metallic

22.

Give TWO reasons why hydrogen chloride is a gas at room temperature

a)

Hydrogen chloride has a low boiling point

b)

Hydrogen chloride has a high melting point

c)

Hydrogen chloride is made of simple molecules

d)

Hydrogen chloride does not conduct electricity

e)

Hydrogen chloride has a giant structure

23.

What type of bonding is preset in calcium oxide?

a)

Ionic

b)

Covalent

c)

Macromolecular

d)

Metallic

24.

What type of particle is this?

a)

An ion

b)

A lattice

c)

A molecule

d)

A polymer

25.

What type of structure is C₆₀?

a)

Diatomic

b)

Giant ionic

c)

A Fullerene

d)

Giant Metallic

26.

What type of structure is C₆₀?

a)

Diatomic

b)

Giant ionic

c)

A Fullerene

d)

Giant Metallic

27.

What type of bond is labelled A?

a)

Metallic

b)

Double

c)

Ionic

d)

Covalent

28.

This is propane. What type of bonding holds the atoms together?

a)

Ionic

b)

Covalent

c)

Metallic

29.

In silicon dioxide the bonds between atoms are

a)

Easily broken

b)

Very strong

c)

Weak

30.

What type of structure does this diagram represent?

a)

Ionic

b)

Metallic

c)

Alloy

d)

Covalent

31.

Which term would NOT apply to a metallic structure?

a)

High melting point

b)

Good insulator

c)

Delocalised electrons

d)

Malleable

32.

When can ionic substances conduct electricity?

a)

Never

b)

As a solid

c)

As a liquid

d)

As a solution

33.

An ionic bond forms when atoms ___________ electrons.

a)

gain

b)

share

c)

increase

d)

transfer

34.

If an atom loses two electrons what charge will it have?

a)

+ 2

b)

- 2

c)

+1

d)

-1

35.

4. What usually forms the positive ion?

a)

Metal

b)

Nonmetals

c)

None

36.

6. What usually forms the negative ion?

a)

Nonmetals

b)

Metal

c)

None

37.

What is the arrangement of particles in a metal? Choose 2

a)

Arranged in near rows

b)

Electrons are shared between particles

c)

Sea of delocalised electrons

d)

Particles are arranged in a random pattern

38.

What are the limitations of using dot and cross diagrams to represent covalent bonds? Choose 2

a)

Does not show the bond angles

b)

Does not show the shape of the molecule

c)

Is simple to draw

d)

Represents the electrons as being shared

39.

What are the properties of giant covalent structures?

a)

Low melting and boiling points

b)

Can conduct electricity

c)

Cannot Conduct electricity

d)

High melting and boiling points

40.

Why are metals malleable?

a)

The particles are not able to slide over each other

b)

The particles are able to slide over each other

41.

Why are alloys harder than pure metals?

a)

The different sized atoms distort the layers in the structure making it easier for them to slide over each other.

b)

The different sized atoms distort the layers in the structure making to more difficult for them to slide over each other.

c)

There is no difference in hardness.

42.

Why do small molecules have low melting and boiling points?

a)

Weak forces between molecules

b)

Strong forces between molecules

c)

The covalent bonds are broken more easily than giant molecules.

d)

Weak ionic bonds

43.

What change of state can occur at the boiling point?

a)

Freezing

b)

Melting

c)

Boiling

d)

Condensing

44.

Which state of matter contains particles in fixed positions?

a)

Liquid

b)

Gas

c)

Solid

45.

What two types of atoms make a covalent bond?

a)

2 Nonmetals

b)

1 Nonmetal and 1 Metal

c)

2 Metals

d)

2 Noble Gases

46.

Since covalent compounds do not have free charges, they are

a)

good conductors

b)

poor conductors

c)

ionic

d)

metallic

47.

In a covalent bond, one or more electrons are?

a)

shared

b)

lost

c)

gained

d)

transferred

48.

Protons have a charge of:

a)

-1

b)

+1

c)

-2

d)

+2

49.

If a you saw the following, K+; what does it tell you about the the ion.

a)

it has lost one electron

b)

it has lost one proton

c)

it has lost two electrons

d)

it is a negative ion

50.

If an atom has no charge, which of the following must be true?

a)

It has more neutrons than protons or electrons.

b)

There are only neutrons inside the atom.

c)

Its number of protons is equal to its number of electrons.

d)

The neutrons in the atom outnumber the electrons and protons.

51.

Why are dots and crosses used to show the electrons in the bonds?

a)

To show which atoms the electrons belong to

b)

Because this is what electrons looks like

c)

To show if the electron came from a metal

d)

To show if the electrons are gained or lost

52.

What is the basis of a metallic bond?

a)

the attraction of neutral metal atoms.

b)

the attraction between protons and neutrons.

c)

the attraction between positive metal ions and interlocking electrons.

d)

the attraction between positive metal ions and free floating electrons.

53.

Which of these is NOT an alloy?

a)

bronze

b)

copper

c)

brass

d)

stainless steel

54.

What does malleable mean?

a)

able to be shaped

b)

will break easily

c)

can be used for wire

d)

is shiny

55.

Magnesium bromide is an ionic compound with the chemical formula MgBr₂. What does the "2" tell you?

a)

There are 2 bromide ions for every magnesium ion

b)

Bromide has a 2- charge

c)

Bromide has a 2+ charge

d)

There are 2 magnesium ions to every bromide ion

56.

Elements on the LEFT side of the periodic table will most likely form:

a)

Positive ions

b)

Negative ions

c)

Neutral Ions

d)

None of these

57.

In an exothermic reaction, heat is ...

a)

taken in

b)

given out

58.

What type of reaction occurs in a hand warmer

a)

exothermic

b)

endothermic

59.

If a chemical reaction is EXOTHERMIC, the temperature would....

a)

Stay the same

b)

Increase

c)

Decrease

60.

In an endothermic reaction the system is releasing energy.

a)

True

b)

False

61.

Is the combustion of gasoline endothermic or exothermic?

a)

Endothermic

b)

Exothermic

62.

During an endothermic reaction in a beaker if we are part of the surroundings and touched the beaker, it would feel _______.

a)

Warm

b)

Cold

63.

If they energy required to break the bonds is greater than the energy given out by making new bonds the reaction is

a)

Exothermic

b)

Endothermic

c)

Neutralisation

64.

If they energy required to break the bonds is less than the energy given out by making new bonds the reaction is

a)

Exothermic

b)

Endothermic

c)

Neutralisation

65.

In an endothermic reaction the products have

a)

more energy than the reactants

b)

less energy than the reactants

c)

the same energy as the reactants

d)

no energy

66.

In an exothermic reaction the products have

a)

more energy than the reactants

b)

the same energy as the reactants

c)

less energy than the reactants

d)

no energy

67.

The required energy to start a reaction is called...

a)

initiation energy

b)

starting energy

c)

activation energy

d)

key energy

68.

This chart shows what type of reaction?

a)

exothermic

b)

combustion

c)

endothermic

d)

mesothermic

69.

This chart shows what type of reaction?

a)

endothermic

b)

mesothermic

c)

exothermic

d)

hotothermic

70.

A(n) _______ is a substance that increases reaction rate by lowering the activation energy of a reaction.

a)

activator

b)

inhibitor

c)

catalyst

d)

polymerase

71.

What is represented by letter A?

a)

Products

b)

Activation Energy

c)

Reactants

d)

Overall Energy Change

72.

What is represented by letter B?

a)

Products

b)

Activation Energy

c)

Reactants

d)

Overall Energy Change

73.

What is represented by letter D?

a)

Products

b)

Activation Energy

c)

Reactants

d)

Overall Energy Change

74.

What is represented by letter C?

a)

Products

b)

Activation Energy

c)

Reactants

d)

Overall Energy Change

75.

Which process is exothermic?

a)

Bond Breaking

b)

Bond Making

76.

In the reactivity series which of the following is the most reactive element?

a)

Copper

b)

Zinc

c)

Calcium

d)

Potassium

77.

In the following chemical reaction what will the products be?

Copper Sulfate + Iron -->

a)

Copper Sulfide + Iron

b)

Iron Sulfide + Copper

c)

Iron Sulfate + Copper

d)

Copper Sulfate + Iron

78.

What is the correct charge on a Magnesium ion

a)

Mg²⁺

b)

Mg^2-

c)

Mg⁺

d)

Mg^-

79.

How can we extract metals that are higher than Carbon in the reactivity series?

a)

Reduction reaction

b)

Electrolysis

c)

Phytomining

d)

Bioleaching

80.

In the diagram, which electrode is the anode?

a)

Left

b)

Right

81.

What is the charge on a Cation?

a)

Positive

b)

Negative

82.

What is the charge on an anion?

a)

Positive

b)

Negative

83.

Which of the following is the best statement to describe what happens to ions during electrolysis?

a)

Positive Cations will move to the Negative Cathode.

b)

Positive Cations will move to the Positive Cathode.

c)

Negative Cations will move to the positive Cathode

d)

Negative Cations will move the negative Cathode

84.

When an acid and alkali react together this is known as a ___________ reactiion.

a)

Combustion

b)

Displacement

c)

Neutralisation

d)

Endothermic

85.

What are the products of a neutralisation reaction?

a)

Salt and Hydrogen

b)

Salt and Water

c)

Excess acid and Hydrogen

d)

Excess alkali and Oxygen

86.

Which acid could be used to form Mg(NO₃)₂ in a metal and acid reaction?

a)

Hydrochloric

b)

Nitric

c)

Phosphoric

d)

Sulphuric

87.

What is the correct formula for Hydrochloric Acid?

a)

HC

b)

HCl

c)

HCL

d)

CLH

88.

Which of the following would not be part of the method to make crystals of Copper Sulphate?

a)

Dissolve Copper Oxide in Sulphuric Acid and heat gently in a water bath to produce copper sulphate solution.

b)

Heat Copper Sulphate solution gently to remove water from solution of Copper Sulphate.

c)

Heat at high temperatures until all of your Copper sulphate solution has evaporated.

d)

Allow crystals to form slowly over a number of days to produce a larger crystal size.

e)

Filter your Copper Oxide from the Copper sulphate solution to collect the filtrate in a beaker.

89.

During the electrolysis of Molten Aluminium Oxide (Al₂O_3(L)) what is added to the electrolyte to lower its melting point?

a)

Salt

b)

Cryolite

c)

Water

d)

Sulphuric Acid

90.

What is produced when an acid reacts with a metal carbonate e.g. MgCO₃?

a)

Salt + Water + Carbon Dioxide

b)

Salt + Carbon Dioxide

c)

Water + Carbon Dioxide

d)

Salt + Water

91.

During electrolysis the substance being separated is called

a)

Compound

b)

Mixture

c)

Electrolyte

d)

Cryolite

92.

Hydrochloric Acid + Calcium Hydroxide >

a)

Calcium Chloride + Water + Carbon-Dioxide

b)

Calcium Nitrate + Water + Carbon-Dioxide

c)

Calcium Phosphate + Water + Carbon-Dioxide

d)

Calcium Chloride + Carbon-Dioxide

93.

Sodium Hydroxide + Hydrochloric Acid >

a)

Sodium Chloride + Water

b)

Sodium Carbonate + Water + Carbon-Dioxide

c)

Sodium Nitrate + Water + Carbon-Dioxide

d)

Sodium Chloride + Carbon-Dioxide

94.

What is reduction in terms of oxygen?

a)

Gain of oxygen

b)

Loss of oxygen

95.

Which is the balanced symbol equation, with state symbols, for the reaction between zinc and hydrochloric acid?

a)

Zn(s) + 2HCl(aq) → ZnCl₂(aq) + H₂(g)

b)

Zn(s) + HCl(aq) → ZnCl₂(aq) + H₂(g)

c)

Zn + 2HCl → ZnCl₂ + H₂(g)

d)

Zn(s) + 2HCl(aq) → ZnCl₂(aq) + 2H₂(g)

96.

Zinc can be extracted from zinc oxide by heating it with carbon in the blast furnace. Carbon monoxide is also produced. Which reactant is oxidised?

a)

Zinc Oxide

b)

Carbon

97.

Which is the balanced symbol equation, with state symbols, for the reaction between zinc and hydrochloric acid?

a)

Zn(s) + 2HCl(aq) → ZnCl₂(aq) + H₂(g)

b)

Zn(s) + HCl(aq) → ZnCl₂(aq) + H₂(g)

c)

Zn + 2HCl → ZnCl₂ + H₂(g)

d)

Zn(s) + 2HCl(aq) → ZnCl₂(aq) + 2H₂(g)

98.

What is the charge of a Proton?

a)

Positive Charge

b)

Negative Charge

c)

Neutral Charge

99.

What is the Charge of an Electron?

a)

Positive Charge

b)

Negative Charge

c)

Neutral Charge

100.

What is the Charge of a Neutron?

a)

Positive Charge

b)

Negative Charge

c)

Neutral Charge

101.

What does the Nucleus of an atom contain?

a)

Protons

b)

Electrons

c)

Neutrons

102.

Which number tells you the amount of protons in an element?

a)

Atomic Number

b)

Mass Number

103.

Which number tells you the amount of protons and neutrons in an element?

a)

Atomic Number

b)

Mass Number

104.

What is an Isotope of a element?

a)

Element with same number of Protons but a different number of Neutrons.

b)

Element with same number of Neutrons but a different number of Protons.

105.

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

106.

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

107.

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

108.

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

109.

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

110.

What is Simple Distillation used for?

a)

Separating out Solutions

b)

Separating out a Mixture of Liquids

111.

What is Fractional Distillation used for?

a)

Separating out Solutions

b)

Separating out a Mixture of Liquids

112.

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.

113.

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.

114.

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.

115.

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.

116.

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.

117.

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.

118.

What is the picture displayed?

a)

atom

b)

element

c)

molecule

d)

compound

119.

What is the picture displayed?

a)

atom

b)

element

c)

molecule

d)

compound

120.

What is the picture displayed?

a)

atom

b)

element

c)

molecule

d)

compound

121.

How could a mixture of food colourings be separated?

a)

A. Chromatography

b)

B. Filtration

c)

C. Fractional distillation

d)

D. Sieving

122.

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.

123.

Who discovered the electron?

a)

A. Ernest Rutherford

b)

B. JJ Thompson

c)

C. Niels Bohr

d)

D. Copernicus

124.

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

125.

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.

126.

What is the definition of an isotope?

a)

A. Atoms of the same element that have different number of protons.

b)

B. Atoms of the same elements that have different number of electrons.

c)

C. Two atoms of the same elements that have different number of neutrons.

d)

D. Two molecules of water.

127.

What is 5?

a)

cooling tube

b)

condenser

c)

distillate

d)

water pump

128.

What is 6 and 7?

a)

6: water in / 7: water out

b)

6: water out / 7: water in

129.

What is filtration?

a)

A method used to separate a solid from a liquid that dissolves in the liquid

b)

A separating technique used to separate a mixture of a solid and liquid where the solid does not dissolve in the liquid

130.

Most simple water purification devices used in the home use filtration as their main method of purifying the water

a)

True

b)

False

131.

The part of the mixture that passes through the filter paper is called the

a)

residue

b)

filtrate

c)

suspension

132.

Identify the Reactants in this equation.

a)

A

b)

B

133.

How many oxygen atoms are present in the following?
4Ca(OH)₂

a)

4

b)

6

c)

8

d)

1

134.

Fill in the blank to balance the chemical equation.
2KI + ____Cl₂→ 2KCl + I₂

a)

1

b)

2

c)

3

d)

4

135.

What number should go in the blank space to balance the chemical equation?

2Al +____ HCl → 2AlCl₃ + 3H2

a)

2

b)

4

c)

3

d)

6

136.

Which of the following represent chemical equations? Check all that apply.

a)

$2Na\ +\ H_2O\ \rightarrow\ 2NaOH\ +\ H_2$

b)

$2KClO_3\ \ \rightarrow\ 2KCl\ +\ 3O_2$

c)

$2Fe\ +\ 3O_{2\ }\rightarrow\ 2Fe_2O_3$

d)

$2H_2O$

e)

$3O_3\ ,\ H_2O$

137.

How are elements organized in the periodic table ?

a)

Alphabetically

b)

Based on physical and chemical properties

c)

Increasing number of electrons

d)

Most reactive to least reactive

138.

Most elements on the periodic table are classified as ____________.

a)

Gases

b)

Metalloids

c)

Metals

d)

Nonmetals

139.

Groups on the periodic table are arranged...

a)

Vertically

b)

Horizontally

c)

Diagonally from bottom right corner

d)

Diagonally from top right corner

140.

Which accurately describes nonmetals?

a)

Poor conductors of electricity

b)

Often used in computer parts

c)

Both malleable and ductile

d)

Both dull and brittle

141.

Which group on the periodic table is the most reactive?

a)

Group 1

b)

Group 2

c)

Group 13

d)

Group 18

142.

What is the chemical symbol for Sodium?

a)

S

b)

So

c)

Na

d)

Ca

143.

A neutral atom of _____________ has 52 electrons.

a)

Chromium

b)

Tellurium

c)

Manganese

d)

Antimony

144.

Each horizontal row on the periodic table is called a what?

a)

Group

b)

Row

c)

Period

d)

Family

145.

Who arranged the periodic table of elements by the atomic weight ?

a)

Democritus

b)

John Dalton

c)

Henry Moseley

d)

Dmitri Mendeleev

146.

Identify the unknown atom.

a)

Flourine

b)

Beryllium

c)

Boron

d)

Helium

147.

Choose ALL of the alkali metals (group 1) from the list below:

a)

lithium

b)

copper

c)

mercury

d)

potassium

e)

sodium

148.

What ions do Metals form when they react?

a)

Positive Ions

b)

Negative Ions

149.

Select all the properties of a Metal:

a)

Strong

b)

Malleable

c)

Conductive

d)

Brittle

150.

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

151.

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

152.

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

153.

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

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

154.

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

a)

Increases

b)

Decreases

155.

What is formed when sodium reacts with water?

a)

sodium oxide and hydrogen

b)

sodium hydroxide and hydrogen

c)

sodium hydroxide and oxygen

d)

sodium hydroxide and carbon dioxide

156.

What is the symbol equation for the reaction between sodium hydroxide and water?

a)

2Na + 2H₂O → 2NaOH + H₂

b)

Na + H₂O → NaOH + H

c)

Na + H₂0 → NaCl + CO₂

d)

2Na + 2H₂O → 2NaH₂ + O₂

157.

What is another name for the elements in group 7?

a)

The Halogens

b)

The Noble gases

c)

The Oxides

d)

The Alkali Metals

158.

When an alkali metal reacts with water, the hydroxide produced dissolves to form and alkaline solution, True or False?

a)

True

b)

False

159.

At room temperature, chlorine is...

a)

a yellow-green gas

b)

a brown gas

c)

a yellow-green liquid

160.

As you move down the group, halogens' reactivity...

a)

increases

b)

decreases

c)

doesn't change

d)

shows no trend.

161.

Which halogens can displace bromide ions to make bromine?

a)

Fluorine and iodine.

b)

Fluorine and bromine.

c)

Fluorine and chlorine

d)

Chlorine and iodine.

162.

A displacement reaction involves...

a)

a solution turning brown or yellow.

b)

a less reactive element taking the place of a more reactive element.

c)

a dislocated hip.

d)

a more reactive element taking the place of a less reactive element.

163.

What type of ions do the Group 7 elements make?

a)

positive 2 (+2)

b)

positive 1 (+1)

c)

negative 1 (-1)

d)

negative 2 (-2)

164.

Would a displacement reaction occur for Bromine + Potassium Iodide?

a)

Yes

b)

No

c)

Maybe

165.

How many electrons do the halogens all have in their outer shells?

a)

1

b)

2

c)

7

d)

8

166.

Would a displacement reaction occur for Iodine + Potassium Bromide?

a)

Yes

b)

No

c)

Maybe

167.

As you go down the group, how does the boiling point of the halogen elements change?

a)

Increases

b)

Decreases

c)

They're all about the same

168.

Which of these is not a noble gas?

a)

Helium

b)

Argon

c)

Nitrogen

d)

Krypton

169.

6.15: Which of these is not a property of noble gases?

a)

Colourless

b)

Odourless

c)

Flammable

d)

Gas at room temperature

170.

Name the group that contains inert (nonreactive) elements.

a)

noble gases

b)

halogens

c)

alkali metals

d)

alkaline earth metals

171.

Which of the following is a noble gas that is heavier than air?

a)

Hydrogen

b)

Helium

c)

Argon

d)

Sodium

172.

Which of the following has the lowest boiling point?

a)

Argon

b)

Krypton

c)

Xenon

d)

Helium

e)

Neon

173.

All noble gases have 8 electrons in their outer shell.

a)

True

b)

False

174.

What is the trend in boiling point for noble gases?

a)

There is no trend.

b)

Boiling point decreases down the group.

c)

Boiling point increases down the group.

d)

All the boiling points are the same.

175.

Another term for being chemically inactive is...

a)

Inert

b)

Inbert

c)

Insert

d)

Inmert

176.

Group 0 elements are non-metals - true or false?

a)

True

b)

False

Chemistry Paper 1 (Foundation)

Total questions: 176

Worksheet time: 2hrs 29mins

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