Metals and the reactivity series Flashcards
Whats the order of metals from the reactivity series from most to least reactive
Potassium
Sodium
Calcium
Magnesium
Aluminium
Zinc
Iron
Hydrogen (anything under here doesnt react with water or dilute acids)
Copper
Silver
Gold
(search up reactivity series edexcel to refrence)
Recall that:
most metals are extracted from
unreactive metals are found
ores found in the Earth’s crust .
in the Earth’s crust as the uncombined elements.
In general, the more reactive a metal is:
the more vigorous its reactions are
the more easily it loses electrons in reactions to form positive ions (cations)
Recall that the extraction of metals involves
reduction of ores
Explain how rusting of iron can be prevented by:
exclusion of oxygen
exclusion of water
sacrificial protection
Oxygen can be excluded by storing the metal in an atmosphere of unreactive nitrogen or argon
Water can be excluded by storing the metal with a desiccant (substance which absorbs water vapour) such as calcium chloride
Iron can be protected from rusting if it is in contact with a more reactive metal, such as zinc. The more reactive metal oxidises more readily than iron, so it ‘sacrifices’ itself while the iron does not rust. Once the sacrificial metal has corroded away, it can simply be replaced.
Explain how electroplating can be used to improve the appearance and/or the resistance to corrosion of metal objects
electroplating involves using electrolysis to put a thin layer of a metal on the object
For example, steel cutlery can be electroplated with silver using a silver anode (plating material) and silver nitrate solution. Electroplating improves the corrosion resistance of metal objects. It also improves their appearance and may be used to produce gold-plated jewellery.
Q: What are two core practical methods used to investigate the effects of changing the conditions of a reaction?
Measuring gas production (e.g., hydrochloric acid + marble chips)
Observing a colour change (e.g., sodium thiosulfate + hydrochloric acid)
Q: Suggest practical methods for determining the rate of a given reaction.
Measure volume of gas produced over time
Record mass loss over time
Observe and time colour change
Use a light sensor for opacity/turbidity
Q: How do reactions occur and how can their rates be increased?
A:
Reactions occur when particles collide. Rates increase if collisions are more frequent or have more energy (i.e., successful collisions).
Q: What factors affect the rate of reaction and how?
A:
Temperature: Increases particle energy, more frequent and energetic collisions
Concentration/Pressure: More particles in a given volume → more frequent collisions
Surface area: More area for collisions (e.g., powdered solids react faster than lumps)
Catalyst: Lowers activation energy
Q: What can graphs of mass, volume, or concentration against time tell us?
A:
Steeper line = faster reaction
Flat line = reaction has stopped
Compare rates by slopes of lines
Q: What is a catalyst?
A:
A substance that increases reaction rate without being used up or chemically changed at the end.
Q: How does a catalyst increase the rate of a reaction?
A:
By lowering the activation energy, making it easier for particles to react during collisions.
Q: What are enzymes and what is one use of them in industry?
A:
Enzymes are biological catalysts. They are used in the production of alcoholic drinks (e.g., fermentation).
