Practice IB Chemistry Topic S2.3 the Metallic Model with authentic exam-style questions for both SL and HL students. This question bank focuses on the exact syllabus content for S2.3 the Metallic Model and mirrors Paper 1A, 1B, 2 style where relevant.
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Which of the following is a good explanation for why metals are malleable?
Which of the following best explains why metals are good conductors of electricity?
What is the term for the bond formed by the electrostatic attraction between positive metal ions and delocalized electrons?
Which factor increases the strength of metallic bonding across Period 3 from sodium to aluminum?
Aluminium is widely used in kitchen foil and drink cans.
(a) malleability.
(b) why metallic bonding allows malleability.
(c) one property of aluminium, besides malleability, that makes it useful in packaging.
Metal atoms are bonded with directional covalent bonds
Layers of ions can slide over each other without breaking the metallic bond
Metals contain molecules that are loosely packed
Metallic bonds are weak and easy to break
They contain mobile protons
They contain free-moving ions
They contain delocalized electrons that move freely throughout the lattice
Their atoms are strongly bound in fixed positions
Ionic bond
Covalent bond
Metallic bond
Hydrogen bond
Increasing atomic radius
Increasing number of delocalized electrons
Decreasing charge on the metal ion
Increasing number of energy levels
