15 questions · 97 marks · ≈ 2 hours
A metallic lattice structure is shown in the diagram.
What are the missing labels, X & Y?
Choose your answer
X:positively charged metal ionsY:negatively charged ions
X:positively charged protonsY:negatively charged non-metal ions
X:positively charged metal ionsY:delocalised electrons
X:positively charged protonsY:negatively charged electrons
Metals exists in giant metallic structures which have many strong metallic bonds.
Which of these properties of metals can be explained by this feature of their structure?
Choose your answer
Good conductors of electricity
Malleable and ductile
High melting point
High density
This question is about magnesium.
Magnesium can be shaped easily. Place ticks in boxes by the two statements which explain why metals can be shaped.
| The atoms are all joined by ionic bonds. | |
|---|---|
| The atoms can slide over each other. | |
| The atoms are small. | |
| The atoms are in layers. | |
| The atoms are different sizes |
The boxes give two properties of metallic compounds and possible explanations for these properties.
Draw one straight line from each property to the correct explanation.
What is meant by an alloy?
Magnesium can be mixed with other elements to form an alloy to make it harder. The structure of an alloy is shown.
Complete the sentence to explain why an alloy is harder than a pure metal:
The atoms in an alloy are different ____________________ so the layers are unable to ____________________ over each other when pressure is applied.
Why is it incorrect to describe an alloy as a compound?
Welding involves joining two pieces of metal together.
Copper and iron are two metals that this can occur with.
Give two properties typical of these metals.
Metals have a lattice structure? What does this lattice consist of?
Choose your answer
anions and cations
anions
cations in a sea of delocalised electrons
molecules in a sea of electrons
To join two pieces of metal by welding, they must be melted together.
State why a high temperature has to be used.
An atmosphere of argon is used when the pieces of metal are welded together. Why is an atmosphere of argon used?
Choose your answer
to speed up the process of welding
to prevent the metal reacting with oxygen
to increase the melting point of the materials
to save energy
Aluminium is an element found in Group 3 of the Periodic Table.
Use your Periodic Table to deduce the number of protons, neutrons and electrons found in an atom of aluminium.
| protons | neutrons | electrons | ||
|---|---|---|---|---|
| ☐ | A | 13 | 27 | 13 |
| ☐ | B | 13 | 27 | 14 |
| ☐ | C | 27 | 14 | 14 |
| ☐ | D | 13 | 14 | 13 |
Choose your answer
Give two physical properties of aluminium.
Duralumin is an alloy of aluminium and copper. What type of substance is an alloy?
Choose your answer
Atom
Element
Compound
Mixture
Aluminium is extracted from bauxite, a mixture containing aluminium oxide.
One sample of bauxite contains 17% aluminium. Calculate the percentage of substances other than aluminium found in bauxite.
The table below shows the properties of four substances, W,X, Y and Z.
| Substance | Melting point | Boiling point | Conducts electricity when | |
|---|---|---|---|---|
| /oC | /oC | solid | liquid | |
| W | 3410 | 5930 | yes | yes |
| X | 801 | 1413 | no | yes |
| Y | 3550 | 4830 | no | no |
| Z | -91 | 98 | no | no |
Use the information in the table to identify the substance that is a metal.
Choose your answer
Substance W
Substance X
Substance Y
Substance Z
The diagram shows the arrangement of ions in copper metal.
Which statement explains a physical property of copper?
Choose your answer
Copper can conduct electricity as its ions are able to carry charge around its structure
Copper has a high melting point as the metal ions are strongly attracted to each other
Copper is malleable as the layers of ions can slide over each other
Copper is malleable as the metallic bonds between the layers of ions break easily
Zinc is a typical metal.
Describe the structure and bonding in zinc.
Explain how zinc is able to conduct electricity.
The surface of some metals, such as iron and copper, corrode when exposed to the air which reduces their electrical conductivity.
Suggest why their conductivity is reduced.
Magnesium ribbon is used in many school laboratories for carrying out reactions involving metals and acids. It can be cut and folded easily.
Explain why metals can be bent and shaped.
This question is about potassium.
Potassium is located in Group 1 of the Periodic Table.
i) State the electronic configuration for a potassium atom.
(1 mark)
ii) State the formula of a potassium ion.
(1 mark)
One physical property of potassium is that it is soft.
i) Give two other physical properties of potassium.
(2 marks)
ii) Give one chemical property of potassium.
(1 mark)
Potassium can react with chlorine to form potassium chloride.
Compare the structure and bonding of potassium with potassium chloride.
Explain the conditions in which potassium oxide can conduct electricity.
Gallium is a metallic element in Group 3. It has similar properties to aluminium.
i) Describe the structure and bonding in a metallic element. You should include a labelled diagram in your answer.
(3 marks)
ii) Explain why metallic elements such as gallium are good conductors of electricity.
(2 marks)
Gallium exists as two stable isotopes, gallium-69 and gallium-71.
Complete the following table to show the number of protons, electrons and neutrons in each particle.
| particle | number of protons | number of electrons | number of neutrons |
|---|---|---|---|
Give the formulae of
Gallium(III) chloride ......................................
Gallium(III) sulfate ........................................
Alloys of gallium and other elements are often more useful than the metallic element itself.
Suggest two reasons why alloys of gallium are more useful than the metallic element.
Which statement describes metallic bonding?
Choose your answer
Electrostatic attraction between atoms
Electrostatic attraction between positively charged particles and delocalised electrons
Electrostatic attraction between oppositely charged ions
Electrostatic attraction between the nuclei of two atoms and a shared pair of electrons
This question is about metals.
Which statement describes metallic bonding?
Choose your answer
electrostatic attraction between oppositely charged ions
electrostatic attraction between the nuclei of two atoms and a pair of electrons shared between them
electrostatic attraction between positively charged particles and delocalised electrons
electrostatic attraction between atoms
Aluminium is malleable and can be easily shaped to make saucepans used for cooking food.
State two other properties of aluminium that make it suitable for saucepans used for cooking food.
1.......................................................................
2.......................................................................
Magnalium is an alloy of aluminium and magnesium.
i) State what is meant by the term alloy.
(1 mark)
ii) Explain why magnalium is harder than aluminium.
(3 marks)
Copper is a typical metal.
Explain how the particles in copper are held together and why the metal is malleable.
You may use a diagram in your answer.
Metals are good conductors of electricity.
Electrical conductivity increases across Period 3, from sodium to aluminium.
Explain why.
Copper can react with oxygen to form copper (II) oxide. Explain the charge on the oxide ion.
Write a half equation for the process that copper undergoes when it reacts with oxygen.
Stainless steel is an alloy of iron, chromium and nickel.
Iron is a typical metal.
Explain why it has a high melting point.
Explain why stainless steel is harder than the iron it is made from.
Early hip replacement joints were made from stainless steel. Apart from being harder, suggest one other property of stainless steel that made them useful as hip replacement joints.
Explain why nickel and chromium are both good thermal conductors.
Both lithium and lithium chloride contain ions of lithium. However, the structure bonding and properties of these substances are very different.
State how the ions are held together in solid lithium and in solid lithium chloride.
Table 4.1 below shows the melting and boiling points of lithium and lithium chloride.
Table 4.1
| Melting point (oC) | Boiling point (oC) | |
|---|---|---|
| Lithium | 180.5 | 1342 |
| Lithium chloride | 605.0 | 1382 |
Explain what can be deduced from the information in Table 4.1.
Two students, A and B, are comparing the properties of lithium and lithium chloride. Student A states that both lithium and lithium chloride will conduct electricity, but Student B states that only lithium will conduct electricity.
State whether Student A, Student B, or neither student is correct. Explain your answer.
Student A and B then went on to discuss the bonding in another substance, CaF2.
Explain, in terms of electrons, how CaF2 is formed from its atoms.