Topic questions Bonding, structure and the properties of matter Giant covalent structures
7 questions · 66 marks · about 1 hour
Diamond and graphite are two naturally‑occurring forms of carbon.
They both have giant covalent structures.
Explain, with reference to its bonding, why diamond has a high melting point.
Explain why graphite is soft and is a conductor of electricity.
Refer to structure and bonding in your answer.
Diamond and graphite are made of carbon atoms, joined together by covalent bonds.
The diagram shows their structures.
State, in terms of electrostatic attractions, what is meant by a covalent bond.
Explain why diamond has a high melting point.
Explain why graphite is a good conductor of electricity.
C60 fullerene is a molecule made of 60 carbon atoms.
The diagram shows the structure of C60 fullerene.
One mole of atoms contains 6.0
1023 atoms.
Determine the number of atoms in one mole of C60 fullerene.
Give your answer in standard form.
This question is about the oxides of some elements in Group 4 of the Periodic Table.
When 5.34 g of lead(II) carbonate are heated, lead(II) oxide and carbon dioxide are formed.
This is the equation for the reaction.
Give the name for this type of reaction.
Calculate the maximum mass of lead(II) oxide that can be formed from 5.34 g of lead(II) carbonate.
[for PbCO3, Mr = 267 for PbO, Mr = 223]
The diagram shows apparatus used to heat lead(II) carbonate.
Complete the diagram to show what needs to be added to the apparatus to test that the gas released is carbon dioxide.
Give the result of the test.
Silicon dioxide (SiO2) and carbon dioxide both contain covalent bonds.
Silicon dioxide is a solid with a high melting point. Carbon dioxide is a gas at room temperature.
Explain why silicon dioxide has a much higher melting point than carbon dioxide.
Refer to structure and bonding in your answer.
The table shows properties of four substances, A, B, C and D.
| Substance | Melting point in °C | Boiling point in °C | Conducts electricity when solid | Conducts electricity when molten |
| A | 800 | 1465 | no | yes |
| B | 327 | 1749 | yes | yes |
| C | 232 | 573 | no | no |
| D | 3550 | 4830 | no | no |
Use information from the table to identify these substances.
Which substance could be a metal?
Which substance could be diamond?
Which substance is a gas at 600 °C?
One of the substances in the table is a compound with the formula C10H16N2O3S
Give the number of different elements in C10H16N2O3S
Determine the number of atoms in a molecule of C10H16N2O3S
Silicon hydride (SiH4) and silicon dioxide (SiO2) both contain covalent bonds but they have different structures.
Describe the forces of attraction in a covalent bond.
Complete the diagram to show the outer shell electrons in a molecule of silicon hydride (SiH4).
The diagram represents part of the structure of silicon dioxide (SiO2).
State how the diagram shows that the atom labelled A is oxygen, not silicon.
Silicon hydride has a simple molecular structure.
Silicon dioxide has the same type of structure as diamond.
Explain why silicon dioxide has a much higher melting point than silicon hydride.
Refer to structure and bonding in your answer.
Silicon hydride reacts with oxygen to form silicon dioxide and water.
Write a chemical equation for the reaction between silicon hydride and oxygen.
This question is about some compounds of the elements in Group 4 of the Periodic Table.
When carbon dioxide dissolves in water, a weak acid forms.
Which of these could be the pH of this weak acid?
Which of these is a correct statement about acids?
When lead(II) carbonate is heated, lead(II) oxide and carbon dioxide form.
Give the name of this type of reaction.
Complete the equation for this reaction.
Silicon dioxide, SiO2, and silicon(IV) chloride, SiCl4, are both covalently bonded compounds.
The table shows the melting and boiling points of these two compounds, and the physical state of silicon dioxide at room temperature.
| Compound | Melting point in °C | Boiling point in °C | Physical state at room temperature |
| SiO2 | 1710 | 2230 | solid |
| SiCl4 | −69 | 58 |
Complete the table by giving the physical state of silicon(IV) chloride at room temperature.
Explain, in terms of structure and bonding, why silicon dioxide has a much higher melting point than silicon(IV) chloride.
This question is about carbon and its compounds.
Draw a dot-and-cross diagram to show the outer shell electrons in a molecule
The atoms in carbon dioxide are held together by covalent bonds.
Describe the forces of attraction in a covalent bond.
The diagram shows three different structures of carbon.
Explain why graphite conducts electricity.
Explain why diamond has a much higher melting point than C60 fullerene.
Refer to structure and bonding in your answer.
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