Bonding, Structure and Properties of Matter - Worksheets, Questions and Revision

22 original exam-style questions - 17 pages of questions with a full mark scheme - free printable PDF.

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GCSE · Chemistry

C2 Bonding, Structure and Properties of Matter

AQA 8462 / 8464 (Chemistry topic 4.2 / Combined Science Trilogy C2) · Calculator allowed · about 95 minutes
Total Marks
Name: _______________________________    Date: ____ / ____ / ______
Answer ALL questions. Show all your working.
1
Figure 1 shows the arrangement of particles in three samples of the same substance: Sample X, Sample Y and Sample Z.
Figure 1 Sample X Sample Y Sample Z
(a)Identify the state of matter shown in Sample Z.(1)
(b)Describe one difference between the arrangement of particles in Sample X and the arrangement of particles in Sample Y.(2)
(c)Explain, in terms of the particle model, why a gas can be compressed (squashed into a smaller volume) much more easily than a liquid.(2)
(Total for Question 1 is 5 marks)
2
The simple particle model represents all particles as small, solid, inelastic spheres with no forces acting between them.
(Total for Question 2 is 3 marks)
3
Sodium reacts with chlorine to form the ionic compound sodium chloride, NaCl.
Na Cl sodium atom chlorine atom Complete the diagram to show the transfer of the electron and the resulting ions
(a)Describe what happens to a sodium atom when it reacts with a chlorine atom.(2)
(b)Describe, in terms of electron transfer, how the ionic bond in sodium chloride is formed, including the charges on the ions produced.(3)
(c)Explain why the ionic bond between sodium and chloride ions is strong.(2)
(Total for Question 3 is 7 marks)
4
This question is about ionic charges and formulae. Higher tier only.
(a)State the charge on a magnesium ion and on an oxide ion.(2)
(b)Explain why the formula of calcium chloride is CaCl2, not CaCl.(2)
(Total for Question 4 is 4 marks)
5
Sodium chloride is a typical ionic compound.
(a)State two properties of ionic compounds such as sodium chloride.(2)
(b)Explain why ionic compounds have high melting points.(2)
(c)Explain why sodium chloride conducts electricity when molten or dissolved in water, but not when solid.(3)
(Total for Question 5 is 7 marks)
6
A student investigates the electrical conductivity of the ionic compound lead bromide (PbBr2) in three different states: solid at room temperature, molten (melted), and dissolved in water to form a solution. Figure 2 shows the circuit used, with two carbon electrodes dipped into the sample and connected to a power pack via a bulb.
Figure 2: circuit to test conductivity of lead bromide bulb power pack carbon electrode carbon electrode sample of lead bromide (solid, molten, or in solution)
(a)Identify the independent variable in this investigation.(1)
(b)Identify the dependent variable in this investigation.(1)
(c)State one variable that should be controlled for a fair test, and explain why it should be controlled.(2)
(d)Give one hazard associated with this practical and a precaution that should be taken to reduce the risk.(2)
(e)The table shows the student's results.
State of lead bromideDoes the bulb light?
SolidNo
MoltenYes, brightly
Dissolved in waterYes, brightly
Use the results and your knowledge of ionic bonding to explain why solid lead bromide does not conduct electricity, but molten and dissolved lead bromide do.(3)
(f)Suggest one improvement to this investigation that would increase confidence in the conclusion.(2)
(Total for Question 6 is 11 marks)
7
Water, H2O, is a simple covalent molecule.
O H H • = oxygen electron × = hydrogen electron (outline only - shared pairs not yet completed)
(a)State the number of covalent bonds in one molecule of water.(1)
(b)Describe how the atoms in a water molecule are held together, in terms of shared electrons.(2)
(c)State why a water molecule has no overall electrical charge.(1)
(Total for Question 7 is 4 marks)
8
Chlorine, Cl2, exists as small (simple) covalent molecules.
(a)Explain why substances made of small covalent molecules, such as chlorine, have low melting and boiling points.(3)
(b)Explain why substances made of small covalent molecules do not conduct electricity.(2)
(Total for Question 8 is 5 marks)
9
Bromine (Br2) has a higher boiling point than chlorine (Cl2). Higher tier only.
(Total for Question 9 is 3 marks)
10
Diamond is a giant covalent structure made entirely of carbon atoms.
Diamond: giant covalent lattice (part shown) each carbon atom bonded to 4 others C-C covalent bond = carbon (C) atom Lattice continues in all directions - only part of the giant structure is shown
(a)Describe the bonding and structure of diamond.(2)
(b)Explain why diamond has a very high melting point.(2)
(c)State the number of covalent bonds formed by each carbon atom in diamond.(1)
(Total for Question 10 is 5 marks)
11
Graphite is another giant covalent structure made of carbon atoms, but its properties are very different from diamond.
Layer 1 Layer 2 Layer 3 Small gap: atoms in same layer (strong covalent bonds) Large gap: between layers (only weak forces act here) each dot = C atom Cross-section of graphite: hexagonal layers of carbon atoms Gap between layers is much larger than the gap between atoms within a layer
(a)Describe the structure of graphite.(2)
(b)Explain why graphite is able to conduct electricity, even though it is a form of carbon like diamond, which does not conduct.(2)
(c)Explain why graphite is soft and slippery.(2)
(Total for Question 11 is 6 marks)
12
Graphene and fullerenes are other allotropes (forms) of carbon.
(a)State what graphene is.(1)
(b)Buckminsterfullerene (C60) is a hollow, cage-like molecule that can be used to deliver drugs into the body. Suggest why this structure makes fullerenes suitable for this use.(2)
(c)Which property makes graphene especially useful in electronics?
A) It is a giant ionic lattice
B) It is a good electrical insulator
C) It conducts electricity and is extremely thin and strong
D) It has a very low melting point(1)
  • A) It is a giant ionic lattice
  • B) It is a good electrical insulator
  • C) It conducts electricity and is extremely thin and strong
  • D) It has a very low melting point
(Total for Question 12 is 4 marks)
13
Poly(ethene) is an example of a polymer made from many small monomer units joined together.
(a)Describe the difference between the bonding within a polymer chain and the forces between separate, neighbouring polymer chains.(3)
(b)Use this to explain why many polymers are solid at room temperature.(2)
(Total for Question 13 is 5 marks)
14
Copper is a typical metal.
Structure of a typical metal (e.g. copper) + + + + + + + + + + + + + + + + + + + + Positive metal ion (fixed in position) Sea of delocalised electrons - free to move between ions + = positive metal ion (fixed in a layer) • = delocalised electron (free to move)
(a)Describe the structure of a typical metal such as copper.(2)
(b)Explain why metals such as copper are malleable (can be hammered or bent into shape).(2)
(c)Explain why metals such as copper are good conductors of electricity.(2)
(Total for Question 14 is 6 marks)
15
Bronze is an alloy of copper and tin. Higher tier only.
(Total for Question 15 is 3 marks)
16
Nanoparticles are particles with dimensions between about 1 nm and 100 nm.
(a)A cube-shaped nanoparticle has sides of length 5 nm. Calculate the surface area to volume ratio of the nanoparticle.(3)
(b)A larger, bulk sample of the same substance is cube-shaped with sides of length 2 cm. Calculate the surface area to volume ratio of this larger cube.(3)
(c)Show that the surface area to volume ratio of the nanoparticle in part (a) is about 4 x 106 times greater than the surface area to volume ratio of the larger cube in part (b). (1 cm = 1 x 107 nm)(2)
(Total for Question 16 is 8 marks)
17
Nanoparticles have a wide range of everyday and industrial uses.
(a)Give two uses of nanoparticles.(2)
(b)Evaluate the possible risks of using nanoparticles in everyday products.(3)
(Total for Question 17 is 5 marks)
18
Sodium chloride, carbon dioxide and diamond are three substances with very different structures. Compare the structure and bonding in these three substances, and use this to explain the differences in their melting points and ability to conduct electricity.
(Total for Question 18 is 6 marks)
19
Scientists use different models to represent bonding and structure, including dot-and-cross diagrams, ball-and-stick models, and 2D displayed formulae.
(Total for Question 19 is 4 marks)
20
For each question, identify the correct answer.
(a)Which type of bonding involves a 'sea' of delocalised electrons surrounding positive ions?
A) Ionic
B) Covalent
C) Metallic
D) Hydrogen bonding(1)
  • A) Ionic
  • B) Covalent
  • C) Metallic
  • D) Hydrogen bonding
(b)Which property is typical of a simple covalent molecular substance?
A) High melting point
B) Conducts electricity when solid
C) Low melting and boiling point
D) Extremely hard(1)
  • A) High melting point
  • B) Conducts electricity when solid
  • C) Low melting and boiling point
  • D) Extremely hard
(c)A solid conducts electricity, has a very high melting point, and is malleable rather than brittle. What type of structure/bonding does it most likely have?
A) Ionic compound
B) Simple molecular substance
C) Metallic
D) Giant covalent (diamond-type)(1)
  • A) Ionic compound
  • B) Simple molecular substance
  • C) Metallic
  • D) Giant covalent (diamond-type)
(d)A white crystalline solid melts at 801 degrees C, conducts electricity only when dissolved in water, and is brittle. What type of bonding does it have?
A) Metallic
B) Ionic
C) Simple covalent (molecular)
D) Giant covalent(1)
  • A) Metallic
  • B) Ionic
  • C) Simple covalent (molecular)
  • D) Giant covalent
(Total for Question 20 is 4 marks)
21
A student heats a beaker of ice until it melts, then continues heating the water until it boils.
(Total for Question 21 is 4 marks)
22
A student measures the melting points of four unknown white solids, A, B, C and D, using melting point apparatus. Figure 3 shows the apparatus used.
Figure 3 — melting point apparatus oil stand clamp capillary tube sample thermometer oil bath gauze tripod Bunsen burner
(a)Name one piece of apparatus, other than a thermometer, used to measure a melting point in this way.(1)
(b)State one variable that should be kept the same for each solid to make this a fair comparison.(1)
(c)The table shows the student's results.
SolidMelting point (degrees C)
A1085
B-78 (sublimes; does not have a true liquid melting point at normal pressure)
C3550
D1538
Using the melting points, suggest which solid, A, B, C or D, is most likely to be: (i) an ionic compound, (ii) a simple molecular substance, (iii) a giant covalent substance such as diamond.(3)
(d)Explain why the student should repeat each melting point measurement and calculate a mean.(2)
(e)One repeat reading for solid A is much lower than the other readings taken. Suggest how the student should treat this reading.(1)
(Total for Question 22 is 8 marks)
Mark scheme · C2 Bonding, Structure and Properties of Matter

Question 1

Question 2

Question 3

Question 4

Question 5

Question 6

Question 7

Question 8

Question 9

Question 10

Question 11

Question 12

Question 13

Question 14

Question 15

Question 16

Question 17

Question 18

Question 19

Question 20

Question 21

Question 22