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Introduction
Master the key concepts of Anomalous Properties and Periodic Trends in the s-Block Elements with this carefully curated CBSE Class 11 Chemistry MCQ Practice Test. Designed strictly as per the NCERT syllabus, this online test covers the unusual behaviors and exceptions observed in alkali and alkaline earth metals, including lithium (Li) and beryllium (Be) — both of which deviate from their group trends due to small atomic size, high charge density, and polarizing power.
These Class 11 Chemistry MCQs focus on vital exam topics such as diagonal relationships (Li–Mg, Be–Al), ionization enthalpy, hydration energy, polarizing power, and anomalous chemical properties. Each question is followed by an answer and explanation to help students understand the logic behind every concept.
Perfect for CBSE board exam preparation and competitive entrance tests (JEE/NEET), this quiz strengthens conceptual clarity and ensures complete coverage of Chapter 10 from the NCERT textbook. Attempt this timed quiz online to assess your knowledge and track your performance instantly.
Sample MCQs (with Answers and Explanations):
Q1. The anomalous behavior of lithium compared to other alkali metals is due to its:
A) Large atomic size
B) High atomic mass
C) Small size and high polarizing power
D) Metallic bonding
Answer: C) Small size and high polarizing power
Explanation: Lithium’s small ionic size and strong polarizing power cause covalent bonding and distinct behavior from other alkali metals.
Q2. Beryllium differs from other Group 2 elements because:
A) It forms amphoteric oxide
B) It is highly reactive
C) It forms ionic halides
D) It has d-orbitals available
Answer: A) It forms amphoteric oxide
Explanation: BeO shows amphoteric behavior (reacts with both acids and bases) due to the covalent nature of its bonds.
Q3. Which of the following pairs shows diagonal relationship?
A) Li and Na
B) Li and Mg
C) Be and Ca
D) Na and K
Answer: B) Li and Mg
Explanation: Lithium and magnesium show similar properties (covalent compounds, solubility patterns) due to comparable ionic radii and charge densities.
Q4. Hydration enthalpy of alkali metals decreases down the group because:
A) Ionic size increases
B) Nuclear charge increases
C) Solubility increases
D) Ionization energy increases
Answer: A) Ionic size increases
Explanation: As atomic and ionic radii increase down the group, hydration enthalpy decreases due to reduced charge density.
Q5. Which property of Be²⁺ ion explains its covalent character in compounds?
A) Large size
B) High polarizing power due to small ionic radius
C) Presence of d-orbitals
D) Low ionization energy
Answer: B) High polarizing power due to small ionic radius
Explanation: Be²⁺ ion has high charge density and can polarize large anions, leading to covalent character in its compounds.