Unit 2 Topic 1 Reactivity Series Flashcards
Why do metals reacting with air gain mass?
Because they form an oxide
When heated in air, metals react with the (?) in the air
oxygen
When heated in air, potassium
burns with a lilac flame, forming a white solid
When heated in air, sodium
burns with a golden yellow flame, forming a white solid
When heated in air, calcium
burns with a brick red flame, forming a white solid
When heated in air, magnesium
burns with a bright white light, forming a white solid/ash
Aluminium only burns in air when (?)
finely powdered
When heated in air, aluminium powder
burns with white sparks, forming a white solid
When heated in air, zinc
burns steadily forming a yellow solid, which becomes white on cooling
Which forms of iron burn/do not burn easily?
Sheets of iron do not burn easily, but iron filings do
When heated in air, iron
burns with yellow/orange sparks when in the form of filings, forming a black solid
When heated in air, copper
does not burn, but forms a black solid
After iron and copper are left in air, the oxide layer formed is easily (?)
rubbed off
To heat potassium and sodium in air you would use a (?)
deflagrating spoon
When potassium and sodium are freshly cut,
a shiny surface is exposed, which quickly tarnishes (goes dull)
When calcium, magnesium, aluminium, zinc, iron and copper are left in air, they react ….
slowly with the air, forming an oxide layer on the surface
Metal + oxygen —>
metal oxide
Fe3O4 is a (?)
mixed oxide
Why must sodium, potassium, and calcium be heated in air under very careful supervision and strict safety procedures?
The reactions can be extremely dangerous, because these metals are high up in the reactivity series.
Metals other than sodium, potassium and calcium are heated in air in a (?)
crucible
Which form of the metal is usually heated in air?
Powder form
Why is the crucible lid lifted occasionally when heating a metal in air?
To allow more air into the crucible
Draw the diagram for heating metals in air (with the exception of sodium, potassium and calcium)
Labels:
- crucible containing metal
- crucible lid
- pipeclay triangle
- tripod
- heat/Bunsen burner
- heatproof mat
Describe the safety procedures when reacting sodium or potassium with water. [3]
A small piece of the metal is placed in a trough half-full of water.
The reaction is carried out behind a safety screen.
Tongs/tweezers are used to handle the metal.
Describe the reaction of potassium with water.
Potassium: Floats on the surface Moves around the surface Burns with a lilac flame Fizzes, giving off a gas Heat is released Small explosion/crackles Eventually disappears Forms a colourless solution
Describe the reaction of sodium with water.
Sodium: Floats on the surface Melts and forms a silvery ball Fizzes, giving off a gas Heat is released Eventually disappears Forms a colourless solution
Describe a further test to prove potassium/sodium has fully reacted with the water.
Solution changes universal indicator from green to blue.
Describe the reaction of calcium with water.
Calcium: Fizzes, giving off a gas Sinks, then rises Heat is released Eventually disappears Forms a colourless solution
Aluminium, zinc, iron and copper have (?) with water, however iron will (?) after a few days
no reaction, rust
Describe the reaction of magnesium with water.
Magnesium:
Undergoes a very slow reaction
Gives off a few bubbles of gas
Why are potassium and sodium stored under oil?
To prevent reaction with oxygen and moisture in the air
Metal + water –>
metal hydroxide + hydrogen
Describe how you would react calcium and magnesium with water. [2]
The metal is placed in water inside a beaker and an inverted filter funnel is placed over the metal.
A boiling tube filled with water is used to collect the hydrogen produced.
Draw a diagram of the apparatus used to react non-group 1 metals with cold water
Labels:
- beaker
- water
- filter funnel
- boiling tube
- hydrogen
- calcium/metal
How do you test that hydrogen is produced?
Hydrogen burns with a squeaky pop, when in contact with a glowing splint
Describe the production of bubbles of gas if magnesium is reacted with water.
Only a few bubbles of gas are produced over a period of several days.
Describe the reaction of magnesium with steam.
The heated magnesium ribbon burns with a bright white light, forming a white solid, and heat is released
Describe the reaction of aluminium with steam.
Powdered aluminium burns to form a white solid and heat is released
Which form does aluminium not react in, and why?
Foil form, because the protective layer of aluminium oxide has to be removed by washing with mercury (II) chloride solution
Describe the reaction of zinc with steam.
Powdered zinc glows to form a yellow solid, which changes to white on cooling, and heat is released.
Describe the reaction of iron with steam.
Powdered iron glows at red heat forming a black solid
Which metals in the reactivity series do not react with water or steam?
Copper and metals below it in the reactivity series.
Metal + steam –>
metal oxide + hydrogen
What is the colour of copper, if it is formed as a product in a displacement reaction?
Salmon pink
What is the colour of copper (II) nitrate solution?
Blue
