Chemistry 9th Chap 4 : Topic 14 - Maryam Publications

Chemistry Chapter 4 : Topic 14

Halogen Displacement Reactions

1 / 15

A student adds chlorine water to a solution of potassium bromide. A reddish-brown color appears, indicating a chemical reaction has occurred. This observation is best explained by:

A) No displacement reaction occurs between halogens

B) Chlorine is less reactive than bromine and displaces it

C) Bromine displaces chlorine from chloride ions

D) Chlorine is more reactive and displaces bromine from bromide ions

2 / 15

In a displacement reaction, when iodine solution is added to potassium chloride solution, no visible reaction occurs. The most appropriate conclusion is:

A) Iodine is less reactive than chlorine and cannot displace chloride ions

B) Iodine is more reactive than chlorine

C) Chlorine cannot displace iodine

D) Chlorine and iodine form a compound

3 / 15

Which statement correctly describes halogens in displacement reactions?

A) Halogens only react with metals, not halide ions

B) All halogens have equal reactivity

C) A more reactive halogen displaces a less reactive halide ion

D) A less reactive halogen displaces a more reactive halogen

4 / 15

When bromine water is added to potassium iodide solution, iodine is formed. This happens because:

A) Iodine reduces bromine to bromide

B) No reaction occurs

C) Bromine oxidizes iodide ions to iodine

D) Iodine is more reactive than bromine

5 / 15

Which halogen is the strongest oxidizing agent among the following?

A) Bromine

B) Fluorine

C) Iodine

D) Chlorine

6 / 15

A displacement reaction occurs when chlorine is passed through potassium iodide solution. The correct observation is:

A) No change occurs

B) Potassium chloride decomposes

C) Iodine vapors (purple) are formed

D) Chlorine turns purple

7 / 15

Which of the following correctly represents halogens acting as oxidizing agents?

A) They reduce metals only

B) They gain electrons and cause other substances to oxidize

C) They always form basic solutions

D) They lose electrons easily

8 / 15

In the reaction: Cl₂+2KBr → 2KCl+Br₂

A) Neutralization

B) Decomposition

C) Double displacement

D) Single displacement redox reaction

9 / 15

Which halide ion acts as the strongest reducing agent?

A) Br⁻

B) I⁻

C) F⁻

D) Cl⁻

10 / 15

A student observes that chlorine can displace bromine and iodine, but bromine can only displace iodine. This shows that:

A) Iodine is most reactive

B) All halogens have equal strength

C) Reactivity decreases down the group

D) Reactivity increases down the group

11 / 15

Why is chlorine considered a stronger oxidizing agent than bromine?

A) It has a larger atomic size

B) It loses electrons easily

C) It forms ionic bonds only

D) It gains electrons more easily due to higher electronegativity

12 / 15

When iodine is added to potassium bromide solution, no reaction occurs. This is because:

A) Bromine is a stronger oxidizing agent than iodine

B) Iodine converts into bromine

C) Iodine is more reactive than bromine

D) Iodine cannot oxidize bromide ions

13 / 15

Which best explains why halogens undergo displacement reactions?

A) They form covalent bonds with metals only

B) They lose protons in solution

C) They compete to gain electrons from halide ions

D) They form metallic bonds easily

14 / 15

In halogen displacement reactions, the halogen that gets displaced always:

A) Gains electrons

B) Becomes more reactive

C) Forms a precipitate only

D) Is converted into halide ions

15 / 15

Which statement correctly describes iodine in redox reactions?

A) It does not participate in redox reactions

B) It acts as a reducing agent because it loses electrons easily

C) It is a strong oxidizing agent

D) It easily oxidizes other substances

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