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.
Electrical and thermal conductivity depend on the mobility of electrons in metals.
Explain why transition metals are generally better conductors than alkali metals.
Compare the electrical conductivity of , , and , and justify your order.
Suggest one use of a highly conductive transition metal and explain why it is suitable.
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.
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.
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.
Metals like copper can be drawn into wires.
Define the term ductility.
Explain why metallic bonding allows ductility.
Identify one additional property important for wire applications. Justify your choice.
Group 2 metals such as beryllium, magnesium, and calcium are used in structural alloys and electronics. Their physical properties, such as melting point, depend on the strength of their metallic bonding.
State the trend in atomic radius as you move down Group 2 from beryllium to calcium.
Describe how ionic charge and atomic radius affect the strength of metallic bonding in Group 2 elements.
Predict the correct order of melting points for beryllium, magnesium, and calcium.
Explain your prediction in terms of metallic bond strength and periodic trends.
Which metal has the strongest metallic bond?
Which best describes the bonding in iron?
Which combination causes the strength of metallic bonding to increase?
| Answer | Charge on Cations | Ionic Radius |
|---|---|---|
| A | Smaller | Smaller |
| B | Larger | Larger |
| C | Smaller | Larger |
| D | Larger | Smaller |
Which of the following statements best describes the bonding in metals according to the metallic model?