Bo01 Ionic BondingBo02 Giant Ionic StructuresBo03 Covalent BondingBo04 Simple and Giant Covalent StructuresBo05 Fullerenes and GrapheneBo06 Bonding in MetalsBo07 Nanoparticles and their Applications
Bo01
Ionic Bonding R A G How atoms can form either positive or negative ions.
How to explain chemical bonding in terms of electrostatic forces and the transfer of electrons.
How the charges on ions are related to group numbers in the Periodic table.
Read the Bo01 sections on your knowledge organisers before you begin.
Comprehension Task1. Complete the boxes with the key information about ionic bonding.
2. Are the statements true? If not, then write a correct version of the statement.
Statement True or false? Correct Statement.Metal ions lose electrons to become negatively charged atoms.In ionic bonding, the atoms share electrons.In an ionic structure, the ions are held in place by electrostatic forces of attraction.
Examples
Diagram
Non-examples
Definition
Ionic Bonding
Bo 01 Ionic Bonding Exam Question Practise
Q1. The diagram shows how magnesium and iodine atoms form magnesium iodide.
Only the outer electrons are shown.
The dots (●) and crosses (×) are used to represent electrons.
Use the diagram to help you to answer this question.
Describe, as fully as you can, what happens when magnesium reacts with iodine to make magnesium iodide.
To gain full marks you should use the words atom, electron and ion in your answer.
(4)
Q2. Figure 1 shows the outer electrons in an atom of the Group 1 element potassium and in an atom of the Group 6 element sulfur.
Figure 1
Potassium forms an ionic compound with sulfur.
Describe what happens when two atoms of potassium react with one atom of sulfur.
Give your answer in terms of electron transfer.
Give the formulae of the ions formed.
(5)
Bo02
Giant Ionic Structures R A G Why ionic compounds have high melting points. Why ionic compounds conduct electricity. How the ions are arranged in giant ionic lattices.
Read the Bo02 sections on your knowledge organisers before you begin.
Comprehension Task 1. Complete the following sentences using key facts about ionic structures.
Ionic compounds have high melting and boiling points because
Ionic compounds have high melting and boiling points but
Ionic compounds have high melting and boiling points so
2. Draw two labelled diagrams to explain why an ionic compound cannot conduct electricity as a solid but can when molten or in solution.
Q1. Figure 3 represents the structure of manganese oxide.
Manganese oxide is an ionic compound.
(a) Determine the empirical formula of manganese oxide.
Use Figure 3.
Empirical formula = ______________________
(1)
(b) Why does manganese oxide conduct electricity as a liquid?
Tick (✔) one box.
Atoms move around in the liquid
Electrons move around in the liquid
Ions move around in the liquid
Molecules move around in the liquid
(1)
Q2. The diagram shows the structure of potassium iodide.
Explain why a high temperature is needed to melt potassium iodide.
(3)
Q3.A student was investigating a magnesium salt, X.
The student found that X:• has a high melting point• does not conduct electricity• dissolves in water and the solution conducts electricity.
(a) (i) What is the type of bonding in magnesium salt X?
______________________________________
(1)
(ii) Explain why solid X does not conduct electricity but a solution of X does conduct electricity.
(2)
(b) The student dissolved X in water.
The student added dilute nitric acid and silver nitrate solution to the solution of X.
A white precipitate was formed.
Salt X contains chloride ions.
Explain why a white precipitate was formed.
(2)
Bo03
Covalent Bonding R A G How covalent bonds are formed. How covalent bonds are represented. How to explain chemical bonding in terms of the sharing of
electrons. The type of substances that contain covalent bonds.
Examples
Diagram
Read the Bo03 sections on your knowledge organisers before you begin.
Comprehension Task 1. Complete the boxes with the key information about covalent bonding.
2. Are the statements true? If not, then write a correct version of the statement.
Statement True or false? Correct Statement.Covalent bonds occur between metals and non-metals.In covalent bonding, electrons become delocalised.Covalent molecules can be simple, such are water, or complex, such as silicon dioxide.
Covalent Bonding
Non-examples
Definition
Bo 03 Covalent Bonding Exam Question Practise
Q1. Figure 2 shows the bonding in substance C.
(a) What is the formula of substance C?
Draw a ring around the correct answer.
SO2 SO2 S2O
(1)
(b) Use the correct answer from the box to complete the sentence.
delocalised shared transferred
When a sulfur atom and an oxygen atom bond to produce substance C,
electrons are _____________________________________________
(1)
(c) What is the type of bonding in substance C?
Draw a ring around the correct answer.
covalent ionic metallic
(1)
Q2. Sulfur can also form covalent bonds.
Complete the dot and cross diagram to show the covalent bonding in a molecule of hydrogen sulfide.
Show the outer shell electrons only.
(2)
Q3. Complete the dot and cross diagram to show the covalent bonding in a nitrogen molecule, N2
Show only the electrons in the outer shell.
(2)
Q4. Complete the dot and cross diagram in Figure 3 to show the bonding in ethanol.
Show the outer shell electrons only.
(2)
Bo04
Simple and Giant Covalent Structures R A G The limitations of using models such as ball and stick and
dot and cross. Why simple molecules have low melting and boiling points. Why covalent substances do not conduct electricity. The general properties of giant covalent structures.
Read the Bo04 sections on your knowledge organisers before you begin.
Comprehension Task For each diagram representing the bonding in ammonia, give a positive and a negative about the representation:
Positive:
Negative:
Positive:
Negative:
Positive:
Negative:
Positive:
Negative:
1
4
3
2
Bo04 Simple and Giant Covalent Structures Exam Question Practise
Q1. a) Complete the diagram below to show the bonding in iodine.
Show the outer electrons only.
(2)
b) Explain why iodine has a low melting point.
(3)
c) Explain, in terms of particles, why liquid iodine does not conduct electricity.
(2)
Q2. Explain why diamond is hard.
(2)
Q3. Graphite and fullerenes are forms of carbon.
Graphite is soft and is a good conductor of electricity.
Explain why graphite has these properties.
Answer in terms of structure and bonding.
(4)
Bo05
Fullerenes and graphene R A G The structure of fullerenes and graphene. The uses of fullerenes and graphene.
Read the Bo05 sections on your knowledge organisers before you begin.
Comprehension Task 1. Complete the Venn Diagram to compare the similarities and differences of fullerenes
and graphene.
2. Match each structure to a use for that structure:
Graphene Electrical chips
Fullerene Delivering drugs
Nanotube lubricants
graphenefullerene
As05 Fullerenes and Graphene Exam Questions
Q1. Figure 1 shows a model of a Buckminsterfullerene molecule.
A lubricant is a substance that allows materials to move over each other easily.
Suggest why Buckminsterfullerene is a good lubricant.
Use Figure 1.
(2)
Q2.The article gives some information about graphene.
Nanotunes!
Carbon can be made into nano-thin, strong sheets called graphene.
A graphene sheet is a single layer of graphite.
Graphene conducts electricity and is used in loudspeakers.
(a) Use the picture and your knowledge of bonding in graphite to:
(i) explain why graphene is strong;
(3)
(ii) explain why graphene can conduct electricity.
(2)
(b) Graphite is made up of layers of graphene.
Explain why graphite is a lubricant.
(2)
Bo06
Bonding in metals R A G How the atoms in metals are arranged. How the atoms in metals are bonded together. Why metals can be bent and shaped without breaking. Why alloys are harder than pure metals. Why metals conduct electricity and thermal energy.
Read the Bo06 sections on your knowledge organisers before you begin.
Comprehension Task1. Complete the following sentences using key facts about bonding in metals:
The ions in pure metals are arranged in layers because…
The ions in pure metals are arranged in layers but…
The ions in metals are arranged in layers so…
2. Complete the boxes with the key information about metallic bonding.
Metallic Bonding
Definition
Non-examplesExamples
Diagram
Bo06 Bonding in Metals Exam Question Practise
Q1. Figure 1 shows the structure of five substances.
(a) Which diagram shows a gas?
Tick (✔) one box.
A B C D E
(1)
(b) Which diagram shows the structure of diamond?
Tick (✔) one box.
A B C D E
(1)
(c) Which diagram shows a metallic structure?
Tick (✔) one box.
A B C D E
(1)
(d) Which diagram shows a polymer?
Tick (✔) one box.
A B C D E
(1)
Q2. Copper metal is used in electrical appliances.
Describe the bonding in a metal, and explain why metals conduct electricity.
(4)
Q3. Magnesium is a metal.
Explain why metals can be bent and shaped.
(2)
Q4. (a) Describe how the structure of an alloy is different from the structure of a pure metal.
(2)
(b) Alloys are used to make dental braces and coins.
(i) Nitinol is an alloy used in dental braces.
Why is Nitinol used in dental braces?
(1)
Bo07
Nanoparticles and their applications [Chemistry only] R A G How to compare ‘nano’ dimensions to typical dimensions of
atoms and molecules. Some uses and benefits of nanoparticles. Some possible risks associated with nanoparticulate
materials.
Read the Bo07 sections on your knowledge organisers before you begin.
Comprehension TaskQ1. Complete the boxes below detailing information about nanoparticles.
Q2. Define the following:
Nanoscience
Coarse particles
Q3. Explain why nanoparticles may have properties that are different from the properties in bulk.
Definition Uses
Example Non-example
Nanoparticles
As07 Nanoparticles and their Applications Exam Question Practise (Chemistry Only)
Q1. Silver can form cubic nanocrystals.
Figure 2 represents a silver nanocrystal.
(a) A silver nanocrystal is a cube of side 20 nm
Calculate the surface area to volume ratio of the nanocrystal.
Surface area to volume ratio = ____________________
(3)
(b) Silver nanoparticles are sometimes used in socks to prevent foot odour.
Suggest why it is cheaper to use nanoparticles of silver rather than coarse particles of silver.
(2)
Q2. Nanoparticles of cobalt oxide can be used as catalysts in the production of hydrogen from water.
(a) How does the size of a nanoparticle compare with the size of an atom?
(1)
(b) Suggest one reason why 1 g of cobalt oxide nanoparticles is a better catalyst than 1g of cobalt oxide powder.
(1)
Q3. (a) Give one advantage of using nanoparticles in sun creams.
(1)
(b) Give one disadvantage of using nanoparticles in sun creams.
(1)
(c) A coarse particle has a diameter of 1 × 10−6 m.
A nanoparticle has a diameter of 1.6 × 10−9 m.
Calculate how many times bigger the diameter of the coarse particle is than the diameter of the nanoparticle.
