Ionic, Metallic and Covalent Bonding - exam practice
Ionic, Metallic and Covalent Bonding
Question 1 of 8
Magneisum and fluorine react together to form the ionic compound, magnesium fluoride.
Write the equation, including state symbols, for the reaction between magnesium and fluorine to produce magnesium fluoride.
Draw a dot-and-cross diagram to show the bonding in magnesium fluoride.
Include the outer-shell electrons only.
State what is meant by the term ionic bond.
The table shows the ionic radius and charge of six ions.
| Ion | Ionic radius (nm) |
|---|---|
| A^+^ | 0.14 |
| B^+^ | 0.18 |
| C^2+^ | 0.15 |
| X^-^ | 0.14 |
| Y^-^ | 0.18 |
| Z^2-^ | 0.15 |
The ionic solids AX, BY and CZ have the same lattice structure.
Deduce the order of magnitude of their lattice energies, giving the most exothermic first.
Explain your answer.
Hydrazine is a colourless liquid at room temperature. It has the formula N2H4 in which two nitrogen atoms are covalently bonded together.
State what is meant by the term covalent bond.
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.
Define the term bond energy.
Define the term bond length.
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.
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.
Deduce the type of crystal structure shown by graphene.
Explain why graphene is an excellent conductor of electricity.
Explain why graphene has a high melting point.
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.
Describe two features of the structure and bonding in graphite that are different to diamond.
This question is about the element copper.
Describe the metallic bonding in copper.
Explain why copper can conduct electricity.
The melting points of some copper halides are shown in the table below.
| Substance | Melting point (°C) |
|---|---|
| CuF_2_ | 836 |
| CuCl_2_ | 630 |
| CuBr_2_ | 498 |
Suggest why the melting point of copper(II) fluoride is higher than that of copper(II) bromide.
Calcium nitride has a giant ionic lattice structure.
Describe what is meant by the term giant ionic lattice, in terms of the type and arrangement of particles present.
Write the equation, including state symbols, for the reaction between calcium and nitrogen to form calcium nitride.
State all the conditions under which calcium nitride conducts electricity.
Explain your answer in terms of the particles involved.
Ammonia reacts with aluminium chloride as shown by the equation:
NH3 + AlCl3 ➔ H3NAlCl3
Name the type of bond formed between N and Al in H3NAlCl3.
Explain how this bond is formed.
Draw the structure of H3NAlCl3.
Show each covalent bond as a line and each co-ordinate bond as an arrow.
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.
Complete the diagram below to show the areas of electron density for each bond.
Label the σ bond and the π bond.
Describe, using the concept of hybridisation, the orbitals involved in the formation of the σ bond of the alkene C=C double bond.
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.