32 Questions
Which metal burns with a lilac flame when heated in the air?
Potassium
What is the color of the flame observed when magnesium is heated in the air?
Brilliant white
What is the product formed when iron is heated strongly in the air?
Iron oxide
What is the observation when lead is heated strongly in the air?
A yellow powder is formed on the surface
Which metal reacts with oxygen to form a white powder when heated gently in the air?
Sodium
What is the product formed when copper is heated strongly in the air?
Copper oxide
Which of the following is an example of a displacement reaction?
Zn + CuSO4 → ZnSO4 + Cu
Which of the following metals is most likely to displace copper from a copper sulfate solution?
Mg
What is the nature of aluminum oxide?
Amphoteric
Which of the following metals is least reactive, according to the reactivity series?
Au
What is the oxidation state of iron in a reaction where it forms a compound with oxygen?
+3
Which metal can displace copper from a copper(II) sulfate solution according to the reactivity series?
Zinc (Zn)
What is the oxidation state of sodium in a reaction where it forms a compound with chlorine?
+1
What is the outcome of a metal displacement reaction involving a more reactive metal and a less reactive metal?
The more reactive metal loses electrons and becomes a positive ion, while the less reactive metal gains electrons and becomes a neutral atom
What happens when calcium is added to water?
A colourless solution is produced.
What is the product of the reaction between steam and zinc?
Zinc oxide and hydrogen.
What is the observation when potassium is added to water?
It moves around on the surface of water.
What is the product of the reaction between steam and iron?
A black powder is produced.
What happens when sodium is added to cold water?
It dissolves and a colourless solution is produced.
What is the product of the reaction between steam and magnesium?
A white powder is produced.
What happens when very reactive metals like potassium react with dilute acids?
They react vigorously and produce a large amount of hydrogen gas.
What is the reason for the lack of observable change when aluminium reacts with dilute acids at first?
The protective oxide layer on the surface of the aluminium is reacting with the acid.
What happens when the oxide layer on the surface of aluminium is completely reacted with the dilute acid?
The acid reacts with the aluminium to form salt and hydrogen.
Which of the following metals do not react with dilute acids?
Copper and silver
What is the product formed when aluminium oxide reacts with hydrochloric acid?
Aluminium chloride and water
What is the characteristic of the reaction between aluminium and dilute acids?
It is a vigorous reaction.
What is the purpose of heating the metal in the set-up?
To vent with the steam
What happens when calcium is added to water?
Calcium hydroxide and hydrogen are produced
What is the product of the reaction between steam and zinc?
Zinc hydroxide and hydrogen
Why should the mineral wool not be heated?
It might explode
What is the product of the reaction between steam and iron?
A black powder is produced
What is the observation when potassium is added to water?
A colourless gas is evolved and it burns with a lilac flame
Study Notes
Reactivity Series
- A list of metals in order of their reactivity, with the most reactive at the top and the least reactive at the bottom
- The series is based on the metal's ability to lose electrons and form ions
- The reactivity series consists of, in order: potassium (K), sodium (Na), calcium (Ca), magnesium (Mg), aluminium (Al), zinc (Zn), iron (Fe), tin (Sn), lead (Pb), copper (Cu), silver (Ag), and gold (Au)
Oxidation States
- The oxidation state of an element is the number of electrons it has lost or gained to form a bond
- Metals tend to lose electrons to form a positive ion (cation) and have a positive oxidation state
- The oxidation state of a metal can vary depending on the reaction it is involved in
- Examples of oxidation states include:
- Sodium (Na) typically having an oxidation state of +1
- Iron (Fe) having oxidation states of +2 or +3
- Copper (Cu) having oxidation states of +1 or +2
Metal Displacement
- A reaction in which a more reactive metal displaces a less reactive metal from its compound
- The more reactive metal loses electrons and becomes an ion, while the less reactive metal gains electrons and becomes a neutral atom
- The reactivity series can be used to predict the outcome of metal displacement reactions
- Examples of metal displacement reactions include:
- Zinc (Zn) displacing copper (Cu) from copper(II) sulfate solution
- Iron (Fe) not displacing copper (Cu) from copper(II) sulfate solution because iron is less reactive than copper
Test your knowledge of the reactivity series of metals, including potassium, sodium, calcium, and magnesium. Learn how they react with oxygen and observe the different flames produced.
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