Online Test — Metals and Non-metals
18 Questions • 15 min • Chapter MCQ
15:00
Question 1 of 18
Which of the following is the most malleable metal?
Iron
Gold
Zinc
Lead
Explanation: Gold (and silver) are the most malleable metals and can be beaten into very thin sheets.
Question 2 of 18
The only metal that is liquid at room temperature is:
Mercury
Bromine
Sodium
Gallium
Explanation: Mercury is the only metal that is liquid at room temperature (bromine is a liquid non-metal).
Question 3 of 18
An amphoteric oxide among the following is:
Na₂O
Al₂O₃
CO₂
SO₂
Explanation: Al2O3 reacts with both acids and bases, so it is amphoteric.
Question 4 of 18
Aqua regia is a mixture of concentrated HCl and HNO3 in the ratio:
1:1
1:3
3:1
2:3
Explanation: Aqua regia is 3 parts concentrated HCl to 1 part concentrated HNO3 and dissolves gold.
Question 5 of 18
Which gas is produced when a metal reacts with a dilute acid?
Oxygen
Carbon dioxide
Hydrogen
Chlorine
Explanation: Reactive metals displace hydrogen from dilute acids, e.g. Zn + 2HCl -> ZnCl2 + H2.
Question 6 of 18
In the reactivity series, the metal placed just above hydrogen is:
Copper
Lead
Silver
Mercury
Explanation: Lead lies just above hydrogen; copper, mercury, silver and gold are below it.
Question 7 of 18
Which reaction will actually occur?
Cu + ZnSO₄ → CuSO₄ + Zn
Ag + CuSO₄ → Ag₂SO₄ + Cu
Fe + CuSO₄ → FeSO₄ + Cu
Au + FeSO₄ → Au₂(SO₄)₃ + Fe
Explanation: Iron is more reactive than copper, so it displaces copper; the other metals are less reactive than the metal in the salt.
Question 8 of 18
In forming NaCl, sodium:
gains one electron
loses one electron
shares one electron
loses two electrons
Explanation: Sodium (2,8,1) loses one electron to become Na+ (2,8).
Question 9 of 18
Ionic compounds conduct electricity when:
solid
molten or in aqueous solution
powdered
never
Explanation: Free-moving ions exist only in the molten or dissolved state, allowing conduction.
Question 10 of 18
Ionic compounds generally have:
low melting points
high melting points
no melting point
negative melting points
Explanation: Strong electrostatic forces between ions give ionic compounds high melting and boiling points.
Question 11 of 18
A naturally occurring metal compound from which a metal can be profitably extracted is a/an:
mineral
ore
alloy
gangue
Explanation: An ore is a mineral concentrated enough to extract the metal profitably.
Question 12 of 18
The impurities (sand, soil) present in an ore are called:
slag
flux
gangue
matte
Explanation: Gangue is the unwanted earthy material mixed with the ore.
Question 13 of 18
Roasting is the process of heating:
a carbonate ore in limited air
a sulphide ore strongly in air
an oxide ore with carbon
the metal in steam
Explanation: Roasting heats a sulphide ore strongly in excess air to convert it to the oxide.
Question 14 of 18
The reaction ZnO + C → Zn + CO is an example of:
oxidation of zinc
reduction of zinc oxide
calcination
corrosion
Explanation: Carbon reduces zinc oxide to zinc metal, so it is a reduction of the oxide.
Question 15 of 18
During electrolytic refining of copper, the impure copper acts as the:
cathode
anode
electrolyte
salt bridge
Explanation: Impure metal is made the anode and pure metal is deposited on the cathode.
Question 16 of 18
Rusting of iron requires:
only air
only water
both air and water
neither air nor water
Explanation: Both oxygen (air) and water must be present for iron to rust.
Question 17 of 18
Coating iron with a layer of zinc to prevent rusting is called:
tinning
galvanisation
electroplating
annealing
Explanation: Galvanisation is coating iron or steel with zinc.
Question 18 of 18
Stainless steel is an alloy of iron with:
copper and tin
chromium and nickel
zinc and lead
carbon only
Explanation: Stainless steel is iron alloyed with chromium and nickel, which resists rusting.