Practice S2.3 The metallic 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.
Which of the following is a good explanation for why metals are malleable?
Lithium, sodium, and potassium are Group 1 metals.
State the trend in melting point down Group 1.
Suggest how the number of delocalized electrons compares in these metals.
Explain the trend in melting point based on bonding.
Sodium is a good conductor of electricity.
State the type of bonding present in metallic sodium.
Identify the particles responsible for electrical conductivity.
Explain how this bonding allows metals to conduct electricity.
Which of the following best explains why metals are good conductors of electricity?
Electrical and thermal conductivity depend on the mobility of electrons in metals.
Explain why aluminium is a better electrical conductor than sodium.
Compare the electrical conductivity of sodium (), magnesium (), and aluminium (), and justify your order.
Suggest one use of copper based on its high electrical conductivity.
Iron and potassium are both metallic elements, but their physical properties differ greatly.
State the type of bonding present in metallic elements.
Compare the number of delocalized electrons per atom in Fe and K.
Explain why iron has a higher melting point than potassium.
Which best describes the bonding in iron?
Why does magnesium have a higher melting point than sodium?
Which of the following factors most significantly contributes to the high melting point of chromium () compared to potassium ()?
Which of the following metals is expected to have the strongest metallic bonding based on its ion charge and atomic radius?
Practice S2.3 The metallic 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.
Which of the following is a good explanation for why metals are malleable?
Lithium, sodium, and potassium are Group 1 metals.
State the trend in melting point down Group 1.
Suggest how the number of delocalized electrons compares in these metals.
Explain the trend in melting point based on bonding.
Sodium is a good conductor of electricity.
State the type of bonding present in metallic sodium.
Identify the particles responsible for electrical conductivity.
Explain how this bonding allows metals to conduct electricity.
Which of the following best explains why metals are good conductors of electricity?
Electrical and thermal conductivity depend on the mobility of electrons in metals.
Explain why aluminium is a better electrical conductor than sodium.
Compare the electrical conductivity of sodium (), magnesium (), and aluminium (), and justify your order.
Suggest one use of copper based on its high electrical conductivity.
Iron and potassium are both metallic elements, but their physical properties differ greatly.
State the type of bonding present in metallic elements.
Compare the number of delocalized electrons per atom in Fe and K.
Explain why iron has a higher melting point than potassium.
Which best describes the bonding in iron?
Why does magnesium have a higher melting point than sodium?
Which of the following factors most significantly contributes to the high melting point of chromium () compared to potassium ()?
Which of the following metals is expected to have the strongest metallic bonding based on its ion charge and atomic radius?