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.
Sodium chloride is an example of an ionic compound.
State the type of bonding in sodium chloride.
Identify the ions formed when sodium reacts with chlorine.
Describe the electrostatic interaction that holds the lattice together.
Magnesium oxide () is an ionic compound used as a refractory material in furnaces.
Write the electron configurations of magnesium and oxide ions.
Explain how magnesium forms an ion and why it achieves a noble gas configuration.
Deduce the formula of magnesium oxide based on the charges of its ions.
Describe the structure of solid magnesium oxide.
Explain why magnesium oxide has a high melting point and is a good electrical insulator when solid.
The diagram below shows a simple apparatus used to investigate the properties of sodium chloride and carbon tetrachloride in both solid and molten states.
State the type of bonding present in sodium chloride and in carbon tetrachloride.
Explain why sodium chloride does not conduct electricity in the solid state but does when molten.
Suggest why carbon tetrachloride does not conduct electricity in any state.
Use the diagram and your knowledge of structure and bonding to deduce which substance(s) contain delocalized ions.
State and explain the difference in melting point between sodium chloride and carbon tetrachloride.
Predict the state of carbon tetrachloride at room temperature. Justify your answer based on its intermolecular forces.
Draw the Lewis (electron dot) structure for the ion and a molecule
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.
Compare the charges and sizes of the ions in and .
Explain how the differences in ionic charge and radius affect the strength of the ionic bonds in these compounds.
Predict which compound has the higher melting point and justify your answer using ionic bonding theory.
Explain why solid does not conduct electricity but molten does.
A student investigates the properties of sodium oxide () and magnesium oxide (), both ionic compounds used in industrial processes.
Write the electron configuration of a neutral sodium atom and a sodium ion.
Explain how sodium forms a positive ion and why it is stable.
Write the formula of sodium oxide based on the charges of the ions formed.
Compare the bonding and structure of sodium oxide and magnesium oxide.
Explain why magnesium oxide has a higher melting point than sodium oxide.
State one electrical property of these oxides in the solid state and explain the reason for this property.
Calcium chloride is a salt commonly used for de-icing roads in winter.
State the number of electrons transferred when calcium reacts with chlorine.
Write the formula of calcium chloride.
Describe the structure and bonding in solid calcium chloride.
Sodium oxide is used in glass manufacturing and consists of sodium and oxygen ions.
State the electron configurations of a sodium atom and a sodium ion.
Explain why sodium forms a positive ion.
Deduce the formula of the ionic compound formed between sodium and oxygen.
Describe the structure and bonding in sodium oxide.
Magnesium oxide is a white crystalline solid formed in high-temperature reactions.
State the charge on the magnesium and oxide ions in .
Write the formula of the compound formed between magnesium and oxygen.
Describe why magnesium oxide has a high melting point.
Which substance has the greatest volatility under the same conditions?
Which compound has the largest value of lattice enthalpy?