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Question 1
Magneisum and fluorine react together to form the ionic compound, magnesium fluoride. |
a) | Write the equation, including state symbols, for the reaction between magnesium and fluorine to produce magnesium fluoride.
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b) | Draw a dot-and-cross diagram to show the bonding in magnesium fluoride. Include the outer-shell electrons only.
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c) | State what is meant by the term ionic bond.
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Question 2
Hydrazine is a colourless liquid at room temperature. It has the formula N2H4 in which two nitrogen atoms are covalently bonded together. |
a) | State what is meant by the term covalent bond.
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b) | Complete the dot and cross diagram for a molecule of hydrazine showing the outer electrons only. Use crosses (x) to represent the electrons from nitrogen and dots (⸱) to represent the electrons from hydrogen.
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Question 3
a) | Define the term bond energy.
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b) | Define the term bond length.
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c) | The table show shows the bond lengths and bond energies of some hydrogen halides. |
Using information in the table above, explain which hydrogen halide (from HF to HI) is the most reactive.
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Question 4
Graphene is an extremely strong and thin material used in electronics. It is an excellent conductor of electricity and it has a very high melting point. Graphene is made from carbon atoms. The diagram below shows part of the structure of graphene. |
a) | Deduce the type of crystal structure shown by graphene.
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b) | Explain why graphene is an excellent conductor of electricity.
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c) | Explain why graphene has a high melting point.
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d) | Carbon atoms can also bond to each other to produce a range of other structures, including graphite, diamond and nanotubes. |
Describe two features of the structure and bonding in graphite that are similar to diamond.
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e) | Describe two features of the structure and bonding in graphite that are different to diamond.
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Question 5
This question is about the element copper. |
a) | Describe the metallic bonding in copper.
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b) | Explain why copper can conduct electricity.
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c) | The melting points of some copper halides are shown in the table below. |
Suggest why the melting point of copper(I) chloride is higher than that of copper(I) iodide.
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Question 6
Calcium nitride has a giant ionic lattice structure. |
a) | Describe what is meant by the term giant ionic lattice, in terms of the type and arrangement of particles present.
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b) | Write the equation, including state symbols, for the reaction between calcium and nitrogen to form calcium nitride.
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c) | State all the conditions under which calcium nitride conducts electricity. Explain your answer in terms of the particles involved.
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Question 7
Ammonia reacts with aluminium chloride as shown by the equation: NH3 + AlCl3 ➔ H3NAlCl3 |
a) | Name the type of bond formed between N and Al in H3NAlCl3. Explain how this bond is formed.
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b) | Draw the structure of H3NAlCl3. Show each covalent bond as a line and each co-ordinate bond as an arrow.
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Question 8
This question is about the structure and bonding of alkenes. Alkenes contain a C=C double bond that consists of a σ bond and a π bond. |
a) | Complete the diagram below to show the areas of electron density for each bond. Label the σ bond and the π bond.
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b) | Describe, using the concept of hybridisation, the orbitals involved in the formation of the σ bond of the alkene C=C double bond.
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c) | The table shows below shows some average bond enthalpies. Compare the relative bond strength of the C-C single and C=C double bonds. Explain your answer.
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