Are the practice questions for Classification of Elements and Periodicity in Properties free?

Yes. Every chapter includes free practice questions for Class 11 - Science students to get you started.

What types of questions are included?

The practice set for Classification of Elements and Periodicity in Properties mainly includes MCQs and CBSE-style short-answer questions, with instant feedback on each answer. For full-length textbook practice, use the NCERT Solutions page.

Are the practice questions suitable for board exam preparation?

Yes. The questions test the same concepts and depth that CBSE asks in board exams. After finishing, also solve the NCERT and NCERT Exemplar exercises for Classification of Elements and Periodicity in Properties for full coverage.

How many practice questions are there for Classification of Elements and Periodicity in Properties?

The number scales with chapter length and concept density. Each chapter typically has 15-50 practice questions across MCQ and short-answer formats.

Classification of Elements and Periodicity in Properties Class 11 Chemistry Practice Questions with Answers

easy

An element has an atomic number of 34. Apply your knowledge of the periodic table to predict the following: (a) Its group and period. (b) Its block. (c) Its valence shell electronic configuration.

Try solving it in your notebook first, then check the solution.

easy

Explain why the atomic radius generally decreases on moving from left to right across a period in the periodic table.

Try solving it in your notebook first, then check the solution.

easy

State the Modern Periodic Law.

Try solving it in your notebook first, then check the solution.

easy

Justify why the metallic character of elements increases as you move down a group in the periodic table.

Try solving it in your notebook first, then check the solution.

easy

Apply IUPAC systematic nomenclature to determine the name and symbol for the element with atomic number 119.

Try solving it in your notebook first, then check the solution.

easy

Justify why there is an exceptionally large difference between the first and second ionization enthalpies of alkali metals like Sodium.

Try solving it in your notebook first, then check the solution.

easy

Justify why an anion is consistently larger than its neutral parent atom.

Try solving it in your notebook first, then check the solution.

easy

Name the scientist who proposed the Law of Octaves for the classification of elements.

Try solving it in your notebook first, then check the solution.

easy

Define electronegativity.

Try solving it in your notebook first, then check the solution.

medium

An element has the outer electronic configuration

[Kr] 4d^{10} 5s^2 5p^3

. Analyze this configuration to determine its period, group, and block in the periodic table.

Try solving it in your notebook first, then check the solution.

medium

Describe Dobereiner's Law of Triads and illustrate it with the example of the chlorine, bromine, and iodine triad.

Try solving it in your notebook first, then check the solution.

medium

Recall the numerical root and symbol for the digit '9' used in the IUPAC nomenclature for elements with atomic number greater than 100.

Try solving it in your notebook first, then check the solution.

medium

The first (

\u0394_iH_1

) and second (

\u0394_iH_2

) ionization enthalpies (in kJ mol⁻¹) and the electron gain enthalpy (

\u0394_{eg}H

) for three elements X, Y, and Z are given below.

Element	$\u0394_iH_1$	$\u0394_iH_2$	$\u0394_{eg}H$
X	419	3051	-48
Y	1681	3374	-328
Z	738	1451	-40

Formulate an identity for X, Y, and Z from among the elements Na, Mg, K, Cl. Justify your identification by evaluating the given energy values. Propose the formula of the compound formed between Y and Z.

Try solving it in your notebook first, then check the solution.

medium

On the basis of quantum numbers and orbital filling rules, demonstrate why the sixth period of the periodic table should have 32 elements.

Try solving it in your notebook first, then check the solution.

medium

Summarize the periodic trends for the following physical properties and explain the reason for each trend across a period and down a group: (a) Atomic Radius (b) Ionization Enthalpy

Try solving it in your notebook first, then check the solution.

medium

Compare the ionic radii of

K^+

and

Cl^-

. Justify which one is larger.

Try solving it in your notebook first, then check the solution.

medium

Explain why the first ionization enthalpy generally decreases as we move down a group in the periodic table.

Try solving it in your notebook first, then check the solution.

medium

Define isoelectronic species and list one species that is isoelectronic with (i)

Ar

and (ii)

Mg^{2+}

.

Try solving it in your notebook first, then check the solution.

medium

Analyze and explain why the first ionization enthalpy of Sulfur (

Z=16

) is lower than that of Phosphorus (

Z=15

).

Try solving it in your notebook first, then check the solution.

medium

Apply the concept of valence to predict the chemical formula of the stable oxide formed by Gallium (Ga,

Z=31

).

Try solving it in your notebook first, then check the solution.

medium

Justify why the first ionization enthalpy of Beryllium (Be) is greater than that of Boron (B), contradicting the general periodic trend.

Try solving it in your notebook first, then check the solution.

medium

Propose the location (period, group, block) for a hypothetical element with atomic number Z = 119. Formulate the chemical formula of its most likely oxide and justify your reasoning based on periodic trends.

Try solving it in your notebook first, then check the solution.

medium

The following species are isoelectronic:

S^{2-}, Cl^-, Ar, K^+, Ca^{2+}

. Analyze their nuclear charges and arrange them in the order of increasing ionic/atomic radius. Provide a clear justification for the order.

Try solving it in your notebook first, then check the solution.

medium

List three main characteristics of p-block elements.

Try solving it in your notebook first, then check the solution.

medium

Compare the chemical nature (acidic, basic, or amphoteric) of the oxides

Na_2O

,

Al_2O_3

, and

SO_3

. Justify your answer based on their positions in the periodic table.

Try solving it in your notebook first, then check the solution.

medium

Identify the block in the periodic table to which elements of Group 13 to 18 belong.

Try solving it in your notebook first, then check the solution.

medium

An element 'X' is located in the 3rd period and Group 16 of the periodic table. Analyze this information to determine the following: (a) The electronic configuration of X. (b) The atomic number of X. (c) Whether X is a metal or a non-metal. (d) The formula of its binary compound with hydrogen. (e) Compare the atomic radius and electronegativity of X with the element in Group 15 of the same period.

Try solving it in your notebook first, then check the solution.

medium

Describe the classification of elements into s, p, d, and f blocks based on their electronic configurations. State the general outer electronic configuration for each block.

Try solving it in your notebook first, then check the solution.

medium

Arrange the elements Beryllium (Be), Magnesium (Mg), Calcium (Ca), and Boron (B) in order of increasing metallic character. Analyze the periodic trends to justify your arrangement.

Try solving it in your notebook first, then check the solution.

medium

Explain why a cation is smaller than its parent atom, while an anion is larger.

Try solving it in your notebook first, then check the solution.

medium

Propose a method to determine the atomic radius of a non-metal like Chlorine and a metal like Sodium. Justify why the methods must be different.

Try solving it in your notebook first, then check the solution.

medium

Formulate an argument to justify placing Helium (He) in Group 18, even though its valence shell configuration (

1s^2

) technically belongs to the s-block.

Try solving it in your notebook first, then check the solution.

medium

The elements Silicon (Si), Beryllium (Be), Magnesium (Mg), Sodium (Na), and Phosphorus (P) are given. Formulate an arrangement of these elements in increasing order of metallic character and justify your arrangement based on their positions in the periodic table.

Try solving it in your notebook first, then check the solution.

medium

Formulate an explanation for the diagonal relationship observed between Boron (B) and Silicon (Si). Your justification must involve at least two distinct periodic properties.

Try solving it in your notebook first, then check the solution.

hard

Compare the electron gain enthalpies of Oxygen (O) and Sulfur (S). Explain why the value for Sulfur is more negative than that for Oxygen.

Try solving it in your notebook first, then check the solution.

hard

Examine the given data for the elements of the second period and answer the questions that follow.

Element	Be	B	N	O
$"\Delta_i H_1"$ (kJ/mol)	899	801	1402	1314
Atomic Radius (pm)	111	88	74	66

(a) Analyze the general trend for atomic radius from Be to O and provide a reason. (b) Explain why the first ionization enthalpy of B is lower than that of Be, which is an exception to the general trend. (c) Explain why the first ionization enthalpy of O is lower than that of N, another exception. (d) Correlate the atomic radius of these elements with their electronegativity trend.

Try solving it in your notebook first, then check the solution.

hard

Arrange the following elements in order of increasing electronegativity and justify your answer: Carbon (C), Nitrogen (N), Silicon (Si), Phosphorus (P).

Try solving it in your notebook first, then check the solution.

hard

Define electron gain enthalpy. Explain the general trend of this property across a period and down a group. Also, explain why the electron gain enthalpy of fluorine is less negative than that of chlorine.

Try solving it in your notebook first, then check the solution.

hard

Critique the statement: "Electronegativity is an inherent, measurable property of an isolated atom." Justify your critique.

Try solving it in your notebook first, then check the solution.

hard

Imagine a universe where the Pauli Exclusion Principle allows a maximum of three electrons per orbital, each with a different 'spin' quantum number (

m_s = +1/2, -1/2, 0

). Propose a new structure for the first three periods of the periodic table in this universe. Justify the number of elements in each period and predict the atomic numbers of the first two 'noble gases'.

Try solving it in your notebook first, then check the solution.

hard

The first ionization enthalpy (

"\Delta_i H_1

") of Potassium (K) is

419 \text{ kJ mol}^{-1}

and that of Calcium (Ca) is

590 \text{ kJ mol}^{-1}

. However, the second ionization enthalpy (

"\Delta_i H_2

") of K is

3051 \text{ kJ mol}^{-1}

, while that of Ca is only

1145 \text{ kJ mol}^{-1}

. Analyze these values and provide a detailed explanation for this difference based on electronic configurations.

Try solving it in your notebook first, then check the solution.

hard

Evaluate why the first ionization enthalpy shows an anomalous trend for Nitrogen and Oxygen (

\u0394_iH

of N >

\u0394_iH

of O), while the trend for Carbon and Nitrogen (

\u0394_iH

of C <

\u0394_iH

of N) is regular.

Try solving it in your notebook first, then check the solution.

hard

Summarize the main reasons for the anomalous properties of the first element in each group of the s- and p-blocks.

Try solving it in your notebook first, then check the solution.

hard

Critique Mendeleev's decision to place Tellurium (Te, atomic mass

\approx

127.6 u) before Iodine (I, atomic mass

\approx

126.9 u) in his periodic table, an arrangement that violated his own Periodic Law. Justify his choice based on the principles he valued, and evaluate the long-term significance of this decision for the development of the modern periodic table.

Try solving it in your notebook first, then check the solution.

hard

Critique the classification of Zinc (Zn), Cadmium (Cd), and Mercury (Hg) as transition elements. Formulate a balanced argument, presenting a case for why they should be excluded from the transition metals and another case for why their placement in the d-block is justified.

Try solving it in your notebook first, then check the solution.

Classification of Elements and Periodicity in PropertiesClass 11 Chemistry Practice Questions