Metal Reactivity Series Quiz

Which metal does not displace hydrogen gas from dilute acids?

• Copper (Cu)

• Zinc (Zn)

• Iron (Fe)

• Aluminum (Al)

Complete the reaction: 4Fe (s) + 3O2 (g) --> ?

• 2Fe2O3 (s)

• FeO (s)

• Fe3O4 (s)

• Fe2O3 (g)

What is the role of acids in metal reactions?

• Acids can react with metals to produce salts and hydrogen gas.

• Acids neutralize metals to form water and carbon dioxide.

• Acids dissolve metals completely without any reaction.

• Acids prevent metals from corroding in the presence of oxygen.

Complete the reaction: 2Cu (s) + O2 (g) --> ?

• CuO (s)

• Cu2O (s)

• 2CuO (s)

• Cu2 (s)

What is the product of the reaction between magnesium and hydrochloric acid?

• Magnesium sulfate and oxygen gas.

• Magnesium chloride and hydrogen gas.

• Magnesium hydroxide and chlorine gas.

• Magnesium carbonate and water.

Which of the following metals does not react with water?

• Lead (Pb)

• Sodium (Na)

• Potassium (K)

• Calcium (Ca)

What is the result of heating copper(II) oxide with carbon?

• Copper and carbon dioxide are produced.

• Copper and oxygen are produced.

• Carbon monoxide and copper are produced.

• Copper(II) oxide remains unchanged.

What is the reactivity series?

• A list of metals arranged in order of decreasing reactivity.

• A chart showing the atomic mass of elements.

• A sequence of metals based on their melting points.

• A classification of metals based on their electrical conductivity.

What is the reaction of magnesium with water?

• Magnesium reacts rapidly with water to form magnesium oxide and hydrogen.

• Magnesium reacts slowly with water to form magnesium hydroxide and hydrogen.

• Magnesium does not react with water at all.

• Magnesium reacts with water to form magnesium sulfate and oxygen.

What is a displacement reaction?

• A reaction where a more reactive metal displaces a less reactive metal from its compound.

• A reaction that occurs when two compounds exchange ions to form new compounds.

• A reaction that involves the breaking of chemical bonds without any change in the oxidation states.

• A reaction where a substance combines with oxygen to produce heat and light.