Free Printable Stogs GCSE Interleaving Periodic Table L

1.

How are elements arranged in the Periodic Table?

a)

In rows called columns, by increasing mass number.

b)

In rows called periods, by increasing mass number.

c)

In rows called columns, by increasing atomic number.

d)

In rows called periods, by increasing atomic number.

2.

The electronic configuration of oxygen is:

a)

2.4

b)

2.6

c)

1.2.4

d)

2.8

3.

Mendeleev’s Periodic Table was revolutionary because:

a)

He ordered elements by both their properties and their atomic number.

b)

He left gaps for undiscovered elements.

c)

He used his Periodic Table to make predictions about undiscovered elements.

d)

He ordered elements by both their properties and their atomic mass.

4.

What group are the Alkali Metals in?

a)

Group 1

b)

Group 2

c)

Group 7

d)

Group 0

5.

What group are the Alkali Earth Metals in?

a)

Group 1

b)

Group 2

c)

Group 7

d)

Group 0

6.

What group are the Halogens in?

a)

Group 1

b)

Group 2

c)

Group 7

d)

Group 0

7.

What group are the Noble Gases in?

a)

Group 1

b)

Group 2

c)

Group 7

d)

Group 0

8.

Elements in the same group in the Periodic Table have:

a)

Similar reactivity

b)

The same melting and boiling points

c)

The same number of outer shell electrons

d)

The same mass

9.

Select the correct physical properties of the alkali metals from the list below.

a)

Soft

b)

Brittle

c)

Dense

d)

Have relatively low melting points

10.

When lithium reacts with water, the following observations are true:

a)

Melts into a ball.

b)

Effervescence is seen.

c)

Burns with a lilac flame.

d)

Floats on the surface of the water.

11.

When potassium reacts with water, the following observations are true:

a)

Melts into a ball.

b)

Effervescence is seen.

c)

Burns with a lilac flame.

d)

Floats on the surface of the water.

12.

Why do the alkali metals get more reactive down the group?

a)

They have smaller atomic radiI and less electron shielding.

b)

They have greater atomic radii and more electron shielding.

c)

It is easier for them to lose their outer shell electron.

d)

The attraction from the nucleus for the outer shell electron is less.

13.

Select the statements about the appearances of the halogens at room temperature and pressure which are true.

a)

Chlorine is a purple gas.

b)

Iodine is a grey solid.

c)

Fluorine is a green gas.

d)

Bromine is a red-brown liquid.

14.

How should you test for chlorine gas?

a)

Damp blue litmus paper goes red.

b)

Damp red litmus paper goes blue.

c)

Damp blue litmus paper goes red then bleaches white.

d)

Damp red litmus paper goes blue, then bleaches white.

15.

Select the correct equation from the options below:

a)

$Cl\ +H\ \rightarrow\ HCl$

b)

$Cl_{2\ }+H_2\ \rightarrow\ 2HCl$

c)

$Cl_2\ +\ H_2\ \rightarrow\ HCl$

d)

$2Cl\ +H_2\ \rightarrow\ 2HCl$

16.

Reduction is:

a)

Gain of oxygen

b)

Loss of oxygen

c)

Gain of electrons

d)

Loss of electrons.

17.

Oxidation is:

a)

Gain of oxygen

b)

Loss of oxygen

c)

Gain of electrons

d)

Loss of electrons

18.

Select the correct ionic equation from the list below:

a)

$I^-\ +Cl_2\ \rightarrow\ Cl^-\ +I_2$

b)

$I^-\ +Cl\ \rightarrow\ Cl^-\ +I$

c)

$2I^-\ +Cl_2\ \rightarrow\ 2Cl^-\ +I_2$

d)

$2Cl^-\ +I_2\ \rightarrow\ Cl_2\ +2I^-$

19.

Halogens are less reactive down the group because:

a)

It is harder to gain an electron.

b)

They have less shielding and smaller radii.

c)

They have more shielding and larger radii.

d)

The attraction of the nucleus to the electron to be gained is weaker.

20.

Why are the noble gases unreactive?

a)

They are already in molecules.

b)

They have done all their bonding.

c)

They have full outer electron shells.

d)

They are colourless.

21.

Noble gases are useful for different applications because:

a)

They are inert.

b)

They are very reactive.

c)

They have a low density.

d)

They are not flammable.

22.

Select the correct properties of transition metals from the list below:

a)

They tend to form coloured compounds.

b)

They are good catalysts.

c)

They have a high melting point.

d)

They have a high density.

23.

What is magnalium an alloy of?

a)

Magnesium and manganese.

b)

Magnesium and aluminium.

c)

Magnesium and silver.

d)

Magnesium and gold.

24.

Aluminium is often used for plane body parts as it is:

a)

Malleable

b)

Low density

c)

Has a high melting point

d)

Is brittle

25.

An alloy tends to be harder than a pure metal as:

a)

Particles are different sizes.

b)

Carbon gives this property.

c)

Layers are disrupted.

d)

Layers of particles cannot slide over one another.

26.

Which pair of values is most likely to be the melting point and the boiling point of sodium? Use the table below to help you.

a)

59 and 910

b)

113 and 735

c)

98 and 890

d)

134 and 1498

27.

The following diagram shows an outline of the periodic table. Give the letter of an element which is found in group 0 and period 2.

a)

A

b)

B

c)

C

d)

D

28.

Group 7 elements react with iron. Select the symbol equation that shows the reaction of iron and fluorine.

a)

$Fe\ +F\ \rightarrow FeF$

b)

$Fe\ +F_2\ \rightarrow\ FeF_3$

c)

$2Fe\ +\ 3F_2\ \rightarrow\ 2FeF_3$

d)

$2Fe\ +F_2\ \rightarrow\ FeF_3$

29.

The reaction of sodium and chlorine produces a white solid.

Choose from the list below a solution that could be used to show that the white solid contains chloride ions.

a)

Limewater

b)

Silver nitrate

c)

Sodium hydroxide

d)

Sulphuric acid

30.

Give the correct equation for the reaction of sodium with water.

a)

$Na\ +H_2O\ \rightarrow\ NaOH\ +H$

b)

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

c)

$Na\ +OH^-\ \rightarrow NaOH$

d)

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

Stogs GCSE Interleaving Periodic Table L

Total questions: 30

Worksheet time: 15mins

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