13.4Unit 8: Energy changes and reactions of metals
Reactions of metals with water
5 min read 5 parts Lesson 4 of 5 2 quizzes
Lesson summary
13.4 Reactions of metals with water — CHECKPOINT (CHEMISTRY) notes: Describe how metals react with water and steam.Method — clean the metal with sandpaper so water touches the metal and not the oxide layerTest — place the metal in water; use hot water if nothing happensOrder of r…
- Order of reactivity
- Storage and safety
- Collecting the gas
- Hydrogen test
- Magnesium with steam
- Why steam is faster
Section 1 of 5Reactions with water
- Method
- clean the metal with sandpaper so water touches the metal and not the oxide layer
- Test
- place the metal in water; use hot water if nothing happens
- Order of reactivity
- observations show which metal is most reactive
Section 2 of 5Sodium and potassium
- Reaction
- metal + water → metal hydroxide + hydrogen
- Sodium
- reacts vigorously
- Potassium
- even more reactive; the hydrogen catches fire
- Storage and safety
- stored under oil, only demonstrated by teachers with safety screens
Section 3 of 5Calcium and magnesium
- Calcium
- reacts less vigorously with water to give hydrogen
- Collecting the gas
- invert a funnel over the metal and collect the gas in a test tube by displacement of water
- Equation
- calcium + water → calcium hydroxide + hydrogen
- Hydrogen test
- a lighted splint gives a squeaky pop
Section 4 of 5Steam
- Magnesium with steam
- magnesium + water (g) → magnesium oxide + hydrogen
- The hydrogen can be burnt.
- Why steam is faster
- steam particles have more energy than water particles
- Steam compared with water vapour
- steam is formed by boiling and is very hot; water vapour is in the air at lower temperatures
Section 5 of 5Unreactive metals
- Gold
- does not react with water at all
- Inert
- an element that is inert does not react
Marked practiceQuizzes for this lesson
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