Chemistry Paper 1 - Topic 3 Chemical Changes - Flashcards in GCSE Chemistry

What does a metal + water(l) produce?

Metal + water ----> Metal hydroxide + hydrogen

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What does a metal + steam(g) produce?

Metal + steam ----> Metal oxide + hydrogen

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What does a metal and an acid produce?

Metal + acid ---> Metal salt + hydrogen

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What does an acid and a carbonate produce?

Acid + carbonate ---> Salt + water + carbon dioxide

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What does an acid and a base (metal oxide) produce?

Acid + base ---> Salt + water

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What does an acid and an alkali (metal hydroxides) produce?

Acid + alkali ----> Salt + water

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What is the chemical test for hydrogen?

1) Bubble hydrogen into a container such as a test tube
2) Insert a lit splint into the test tube
3) If hydrogen is present, a squeaky pop will be heard

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What is the chemical test for carbon dioxide?

1) Bubble the gas into a container of limewater.
2) If carbon dioxide is present, it goes from colourless to cloudy

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What is the chemical test for oxygen?

1) Collect the gas into a container such as a boiling tube
2) Insert a glowing splint into the container
3) If oxygen is present, the splint will re-light

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What is the chemical test for chlorine?

1) Damp a piece of blue litmus paper
2) If chlorine is present, the litmus paper turns red and then the chlorine bleaches it white

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Soluble:
All common sodium, potassium and ammonium salts

Insoluble:
-

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Soluble:
Every nitrate salt

Insoluble:
No exceptions

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Soluble:
Most common chlorides

Insoluble:
Silver chloride, lead chloride

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Soluble:
Most common sulphates

Insoluble:
Lead sulphate, Barium sulphate, Calcium sulphate

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Soluble:
Sodium carbonate, potassium carbonate, ammonium carbonate

Insoluble:
Most common carbonates

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Soluble:
Sodium hydroxide, potassium hydroxide, ammonium hydroxide

Insoluble:
Most common hydroxides

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What is electrolysis?

Splitting of an ionic compound back into its elements using a direct electrical current

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How do you form an electrolyte?

You take an ionic compound and either turn it molten (turn it liquid) or put it in solution

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Why can an electrolyte conduct electricity?

Ionic compounds are made up of ions. When in liquid form or in solution, the ions are free to move. The movement of charge is what electricity is.

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In electrolysis of a molten ionic compound, what is formed at the electrodes? (+ where does oxidation and reduction take place?)

At the anode: oxidation, the non-metal element forms

At the cathode: reduction, the metal element forms

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In electrolysis of an ionic compound in solution, how do you determine what becomes discharged at the cathode:
The hydrogen or the metal?

If the metal is more reactive than hydrogen, the hydrogen is discharged and will bubble at the cathode. The metal remains in solution
If hydrogen is less reactive, the metal is discharged and forms at the cathode. Hydrogen stays in solution

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In electrolysis of an ionic compound in solution, how do you determine what is discharged at the anode?
The non-metal element or the hydroxide ions

If a halide (group 7) ion is present, the halogen bubbles at the anode, the hydroxide stays in solution.
If no halogen is present, the hydroxide is discharged and the non-metal stays in solution

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When the hydroxide ions are discharged at the anode, what is the constant half equation?

4OH-(aq) ---> 2H2O(l) + O2(g) + 4(e-)

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Chemistry Paper 1 - Topic 3 Chemical Changes

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