p-Block Elements Quiz - ICSE Class 12 Chemistry

Free practice quiz: p-Block Elements (ICSE Class 12 Chemistry). 39 multiple-choice questions with answers and explanations. Play online, no sign-up needed.

Sample questions

1. Which of the following is the strongest oxidizing agent among the halogens?

   1. Chlorine
   2. Bromine
   3. Iodine
   4. Fluorine
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   Answer: D. Fluorine

   Fluorine is the most electronegative element and has the highest electron affinity, making it the strongest oxidizing agent among the halogens. It readily accepts electrons and oxidizes other substances.

2. Which of the following is NOT a property of noble gases?

   1. Monatomic
   2. Highly reactive
   3. Colorless and odorless
   4. Low boiling points
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   Answer: B. Highly reactive

   Noble gases (Group 18) are known for their extremely low reactivity due to their stable electron configuration with a full valence shell. They are monatomic, colorless, odorless, and have very low boiling points.

3. Which element exhibits the maximum number of oxidation states?

   1. Sulfur
   2. Chlorine
   3. Phosphorus
   4. Bromine
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   Answer: A. Sulfur

   Sulfur (atomic number 16) has the electronic configuration [Ne] 3s² 3p⁴. It can exhibit oxidation states from -2 (in sulfides) to +6 (in sulfates and related compounds), including +2, +4, and +0. This wide range is due to the availability of d-orbitals for hybridization.

4. The decreasing order of reducing character of halogens as halide ions is:

   1. I⁻ > Br⁻ > Cl⁻ > F⁻
   2. F⁻ > Cl⁻ > Br⁻ > I⁻
   3. Cl⁻ > Br⁻ > I⁻ > F⁻
   4. I⁻ > Cl⁻ > Br⁻ > F⁻
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   Answer: A. I⁻ > Br⁻ > Cl⁻ > F⁻

   Reducing character as halide ions increases with decreasing ionization energy and increasing atomic size. Iodine is the largest and has the lowest ionization energy, making I⁻ the strongest reducing agent. Fluoride ion (F⁻) is the weakest reducing agent.

5. The acidic strength of the oxides of the third period elements increases in the order:

   1. Na2O < MgO < Al2O3 < SiO2 < P4O10 < SO2 < Cl2O7
   2. Cl2O7 < SO2 < P4O10 < SiO2 < Al2O3 < MgO < Na2O
   3. Na2O < MgO < Al2O3 < SiO2 < SO2 < P4O10 < Cl2O7
   4. Cl2O7 < P4O10 < SO2 < SiO2 < Al2O3 < MgO < Na2O
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   Answer: A. Na2O < MgO < Al2O3 < SiO2 < P4O10 < SO2 < Cl2O7

   Across a period, the acidic strength of oxides increases due to increasing electronegativity and non-metallic character. The order of acidic strength of oxides of third-period elements is: basic oxides (Na2O, MgO) < amphoteric oxide (Al2O3) < acidic oxides (SiO2, P4O10, SO2, Cl2O7). The acidic strength further increases from SiO2 to Cl2O7.

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