Practice IB Chemistry Topic S2.4 from Models to Materials with authentic exam-style questions for both SL and HL students. This question bank focuses on the exact syllabus content for S2.4 from Models to Materials and mirrors Paper 1A, 1B, 2 style where relevant.
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What is the primary reason why alloys are generally stronger than pure metals?
Which of the following best explains why stainless steel is more resistant to corrosion than pure iron?
Why does graphite conduct electricity along its layers (but not between layers), whereas diamond does not conduct?
Which of the following is a property of giant covalent structures like diamond?
The degradation of condensation polymers, such as proteins and polyesters, is an important process for sustainability and environmental impact.
(a) the type of reaction responsible for breaking down condensation polymers.
(b) in detail how this reaction occurs in both proteins and polyesters, including the specific bonds affected and products formed.
(c) and one environmental factor that accelerates the degradation of condensation polymers in nature.
(d) the role of enzymes in polymer degradation and how they influence the reaction rate.
Alloys have higher melting points than pure metals.
Alloys contain atoms of different sizes that disrupt the metal lattice, making it harder for layers to slide over each other.
Alloys allow electrons to move freely, increasing conductivity.
Alloys are less dense than pure metals.
Stainless steel contains carbon atoms that prevent rusting.
Stainless steel contains chromium, which forms a protective oxide layer on the surface.
Stainless steel has a lower density than pure iron.
Stainless steel is an insulator.
(e) how entropy changes during the hydrolysis of condensation polymers and why this is important for spontaneity.
Diamond has delocalized electrons throughout a 3D structure; graphite has none
Diamond has strong metallic bonding; graphite does not
Graphite has delocalized electrons between the layers, allowing conduction perpendicular to the layers; diamond has none
Graphite has delocalized electrons within layers; diamond has only localized bonds
Low melting point
Electrical conductivity in solid state
Hard and brittle
Poor thermal conductivity
