Practice S2.1 The ionic model with authentic IB Chemistry exam questions for both SL and HL students. This question bank mirrors Paper 1A, 1B, 2 structure, covering key topics like atomic structure, chemical reactions, and organic chemistry. Get instant solutions, detailed explanations, and build exam confidence with questions in the style of IB examiners.
Paper
Level
Question 1
SLPaper 2
Sodium chloride is an example of an ionic compound.
1.[1]
State the type of bonding in sodium chloride.
2.[2]
Identify the ions formed when sodium reacts with chlorine.
3.[2]
Describe the electrostatic interaction that holds the lattice together.
Question 2
SLPaper 2
Magnesium oxide () is an ionic compound used as a refractory material in furnaces.
1.[2]
Write the electron configurations of magnesium and oxide ions.
2.[2]
Explain how magnesium forms an ion and why it achieves a noble gas configuration.
3.[1]
Deduce the formula of magnesium oxide based on the charges of its ions.
4.[2]
Describe the structure of solid magnesium oxide.
5.[2]
Explain why magnesium oxide has a high melting point and is a good electrical insulator when solid.
Question 3
SLPaper 2
The diagram below shows a simple apparatus used to investigate the properties of sodium chloride and carbon tetrachloride in both solid and molten states.
1.[2]
State the type of bonding present in sodium chloride and in carbon tetrachloride.
2.[2]
Explain why sodium chloride does not conduct electricity in the solid state but does when molten.
3.[1]
Suggest why carbon tetrachloride does not conduct electricity in any state.
4.[1]
Use the diagram and your knowledge of structure and bonding to deduce which substance(s) contain delocalized ions.
5.[2]
State and explain the difference in melting point between sodium chloride and carbon tetrachloride.
6.[2]
Predict the state of carbon tetrachloride at room temperature. Justify your answer based on its intermolecular forces.
7.[2]
Draw the Lewis (electron dot) structure for the ion and a molecule
Question 4
SLPaper 2
A materials scientist studies the properties of two ionic compounds: sodium chloride () and aluminum oxide (). These compounds have very different melting points and electrical conductivities.
1.[2]
Compare the charges and sizes of the ions in and .
2.[2]
Explain how the differences in ionic charge and radius affect the strength of the ionic bonds in these compounds.
3.[2]
Predict which compound has the higher melting point and justify your answer using ionic bonding theory.
4.[2]
Explain why solid does not conduct electricity but molten does.
Question 5
SLPaper 1A
Which substance has the greatest volatility under the same conditions?
Question 6
HLPaper 1A
Which compound has the largest value of lattice enthalpy?
Question 7
HLPaper 1A
Which of the following statements correctly explains the conductivity of ionic compounds?
Question 8
HLPaper 1A
Which combination would create the strongest ionic bond?
| Answer | Ionic radius | Charges on ions |
|---|---|---|
| A | Large | High |
| B | Large | Low |
| C | Small | High |
| D | Small | Low |
Question 9
HLPaper 1A
Which ions are listed in order of decreasing ionic radius (highest first)?
Question 10
HLPaper 1A
Which statement correctly explains why sodium chloride has a high melting point?