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2.3.1Additional lessons

Properties of Metals and Their Uses — IB Chemistry HL Revision Notes & Topical Questions

5 min read 5 parts Lesson 42 of 172

📚 IB Chemistry HL Hub / Topical Revision
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Curriculum Equation Key قوانين الرقم الهيدروجيني والاتزان الأيوني - pH & Acid-Base Equilibrium FormulasFast Exam Solution
pH = -log[H⁺] | pOH = -log[OH⁻] | pH + pOH = 14 | [H⁺][OH⁻] = 10⁻¹⁴
Word Equation & Conditions: الرقم الهيدروجيني = -لوغاريتم تركيز أيون الهيدروجين | pH + pOH = 14
Location & Specifications: الاتزان الأيوني، كيمياء 3 ثانوي، التحصيلي، و AP Chemistry.
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Part 1 of 5Metallic Bonding

Metals are held together by attraction between positive ions and a sea of mobile electrons.

Cations
  • Cations Metal atoms lose their outer electrons and form a regular lattice of positive ions.
Delocalised electrons
  • Delocalised electrons The outer electrons are free to move throughout the structure.
The bond
  • The bond Metallic bonding is the electrostatic attraction between the cations and the delocalised electrons.
Non-directional
  • Non-directional The attraction acts in all directions, so metal atoms can pack closely in layers.

Part 2 of 5Explaining the Properties

Explaining the Properties
Electrical conductivity
  • Electrical conductivity Delocalised electrons move through the lattice when a potential difference is applied.
Thermal conductivity
  • Thermal conductivity Mobile electrons and vibrating ions pass energy rapidly through the metal.
Malleable and ductile
  • Malleable and ductile Layers of ions slide over one another while the electron sea keeps them bonded.
Lustre
  • Lustre The free electrons reflect light, giving metals their shiny surface.

Part 3 of 5Melting Point Trends

1
Strength of metallic bonding increases with greater ionic charge, more delocalised electrons and a smaller ionic radius.
2
Sodium, magnesium and aluminium have 1, 2 and 3 delocalised electrons per atom, and their melting points rise from 98 to 650 to 660 °C.
3
Going down group 1 the ions become larger and the attraction weaker, so melting points fall from lithium at 181 °C to potassium at 63 °C.
4
Mercury is a liquid at room temperature because its metallic bonding is unusually weak.
MetalDelocalised electronsMelting point / °C
Na198
Mg2650
Al3660

Part 4 of 5Uses Linked to Properties

Copper
  • Copper Used for electrical wiring because it is an excellent conductor and ductile.
Aluminium
  • Aluminium Used in aircraft and overhead cables because it has low density and conducts well.
Iron and steel
  • Iron and steel Used in construction because of their strength and low cost.
Gold
  • Gold Used in electronics because it conducts well and resists corrosion.

Part 5 of 5Exam Checklist & Tips

2.3.1 – Key Points for the Exam

  • Metallic bond The electrostatic attraction between metal cations and delocalised electrons.
  • Delocalised electrons Electrons that are free to move throughout the metal lattice.
  • Malleable Able to be hammered or pressed into shape without breaking.
  • Ductile Able to be drawn into wires.

Common Mistakes

  • Saying metals contain free atoms or free ions that carry current.
  • Explaining conductivity by electrons passing from atom to atom in covalent bonds.
  • Stating that metallic bonds break when metals bend.
  • Forgetting that ionic charge and radius both affect melting point.

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