25-minute Test : Part III Metals

Which of the following actions should NOT be performed inside a school laboratory?

• A. Heating silver oxide strongly in a Bunsen flame
• B. Heating zinc oxide with carbon powder
• C. Adding sodium metal to hydrochloric acid
• D. Passing steam over hot magnesium ribbon

What is the mass of aluminium in 12.0 g of Al₂O₃?

(Relative atomic masses: O = 16.0, Al = 27.0)

• A. 0.12 g
• B. 3.18 g
• C. 5.65 g
• D. 6.35 g

Calcium is more reactive than magnesium because

• A. calcium atoms have more electrons than magnesium atoms.
• B. calcium has a lower melting point than magnesium.
• C. calcium atoms lose electrons more readily than magnesium atoms.
• D. the metallic bonds between calcium ions are stronger than those between the magnesium ions.

Which of the following solutions would turn blue when a piece of copper is added to it?

• A. Silver nitrate solution
• B. Iron(II) nitrate solution
• C. Calcium nitrate solution
• D. Ammonium nitrate solution

Which of the following combinations about corrosion prevention methods of metal objects is INCORRECT?

• A
• B
• C
• D

Consider the following set-ups. Which of the following shows the iron nails arranged in ascending order of speed of rusting?

• A. (1), (3), (2), (4)
• B. (2), (4), (1), (3)
• C. (3), (1), (4), (2)
• D. (4), (2), (3), (1)

When 11.16 g of lead(II) oxide is heated with 0.36 g of carbon powder, 6.22 g of lead forms. Which of the following combinations is correct?

(Relative atomic masses: C = 12.0, O = 16.0, Pb = 207.2)

• A
• B
• C
• D

What is the mass of carbon required for the complete reduction of 15.9 g of copper(II) oxide?

(Relative atomic masses: C = 12.0, O = 16.0, Cu = 63.5)

• A. 0.60 g
• B. 1.20 g
• C. 2.40 g
• D. 4.80 g

Which of the following ionic equations correctly represents the reaction between magnesium and iron(III) nitrate solution?

• A. Mg(s) + Fe³⁺(aq) → Mg²⁺(aq) + Fe(s)
• B. 2Mg(s) + 3Fe²⁺(aq) → 2Mg³⁺(aq) + 3Fe(s)
• C. 3Mg(s) + 2Fe²⁺(aq) → 3Mg³⁺(aq) + 2Fe(s)
• D. 3Mg(s) + 2Fe³⁺(aq) → 3Mg²⁺(aq) + 2Fe(s)

The following diagram shows a set-up used for determining the empirical formula of an oxide of copper, X. It was found that 5.74 g of X was reduced to 5.10 g of copper. Which of the following is the empirical formula of X?

(Relative atomic masses: O = 16.0, Cu = 63.5)

• A. CuO
• B. CuO₂
• C. Cu₂O
• D. Cu₂O₃