Study Notes
Metals are elements known for their shiny appearance, high density, and excellent conductivity of heat and electricity. They form positive ions and react with acids to produce hydrogen gas and a salt.
- Metallic Bonding — a lattice of positive ions in a sea of delocalised electrons Example: Explains why metals are good conductors and malleable.
- Alloys — mixtures of a metal with other elements Example: Brass is an alloy of copper and zinc.
- Reactivity Series — order of metals based on their reactivity with water, acids, and oxygen Example: Potassium is more reactive than copper.
- Malleability — ability of metals to be shaped without breaking Example: Gold can be hammered into thin sheets.
- Conductivity — ability to conduct heat and electricity Example: Copper is used in electrical wiring due to its high conductivity.
Exam Tips
Key Definitions to Remember
- Metallic Bonding
- Alloys
- Reactivity Series
- Malleability
- Conductivity
Common Confusions
- Confusing alloys with compounds
- Misunderstanding why some metals do not react with water
Typical Exam Questions
- What is metallic bonding? A lattice of positive ions in a sea of delocalised electrons
- Why are alloys used instead of pure metals? Alloys are harder and have improved properties
- How does the reactivity series affect reactions with acids? More reactive metals react vigorously, less reactive metals do not
What Examiners Usually Test
- Understanding of metallic bonding and its effects
- Ability to identify and explain the use of alloys
- Knowledge of the reactivity series and its implications