How to Excel in JEE Main Mock Tests on Classification of Elements & Periodicity
Mastering the classification of elements and periodicity in properties is crucial for excelling in JEE Chemistry, as this chapter forms the base for many advanced concepts. Explore trends in atomic properties, periodic law, and the periodic table through high-quality, exam-styled questions. Take this mock test now to reinforce your understanding and maximize your JEE Main score!
Mock Test Instructions for the Classification Of Elements And Periodicity In Properties Mock Test 1:
- 20 questions from Classification Of Elements And Periodicity In Properties Mock Test 1
- Time limit: 20 minutes
- Single correct answer per question
- Correct answers appear in bold green after submission
How Can JEE Mock Tests Help You Master Classification Of Elements And Periodicity In Properties?
- Identify and avoid frequent mistakes in periodic trends and group behaviors.
- Strengthen foundational knowledge of periodic law and atomic properties through practice.
- Enhance speed and accuracy for JEE by solving time-bound classification questions.
- Receive instant feedback for every question and target revision to weak concepts.
- Refine application of concepts like electronegativity, ionization energy, and atomic size in MCQs.
Boost Your JEE Chemistry Score: Expert Mock Test Practice for Periodicity
- Practice with difficulty-leveled questions to simulate real JEE Main exam pressure.
- Improve recall of exceptions and special cases with targeted quizzes.
- Use expert-designed questions to clarify doubts in group and period trends.
- Develop exam temperament and learn critical time management techniques for Chemistry.
- Utilize detailed answer keys to perfect your exam approach for this chapter.
Subject-Wise Excellence: JEE Main Mock Test Links
| S.No. | Subject-Specific JEE Main Online Mock Tests |
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| 1 | Online FREE Mock Test for JEE Main Chemistry |
| 2 | Online FREE Mock Test for JEE Main Maths |
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FAQs on JEE Main 2025-26 Mock Test Preparation: Classification of Elements and Periodicity in Properties
1. What is the modern periodic law?
Modern periodic law states that the physical and chemical properties of elements are a periodic function of their atomic numbers. This means that when elements are arranged in increasing order of their atomic numbers, elements with similar properties recur at regular intervals.
2. What is periodicity in properties?
Periodicity in properties refers to the repeating pattern of certain chemical and physical properties of elements at regular intervals when the elements are arranged by increasing atomic number in the periodic table. Examples include atomic radius, ionization energy, electronegativity, and valency.
3. Who gave the modern periodic table, and what is its basis?
Henry Moseley proposed the modern periodic table in 1913. He arranged elements based on their atomic number (Z), rather than atomic mass, resolving anomalies found in Mendeleev's arrangement.
4. What is the difference between groups and periods in the periodic table?
Groups are the vertical columns in the periodic table and contain elements with similar valence electron configurations and hence similar chemical properties. Periods are the horizontal rows in the periodic table, where elements have the same number of electron shells but different chemical properties.
5. What are the main features of the long form of the periodic table?
The long form of the periodic table:
- Arranges elements in order of increasing atomic number
- Consists of 7 periods (rows) and 18 groups (columns)
- Distinguishes between main group elements, transition elements, lanthanoids, and actinoids
- Shows trends such as electronegativity and atomic radius
6. Why does atomic radius decrease across a period?
As we move from left to right across a period, the atomic radius decreases. This is because the number of protons and electrons increases, causing a greater nuclear charge and stronger attraction between the nucleus and the electrons, pulling them closer to the nucleus.
7. What are periodic trends in ionization energy and electronegativity?
Ionization energy increases across a period and decreases down a group, since atoms hold their electrons more tightly across a period. Electronegativity also increases across a period and decreases down a group, reflecting an element’s ability to attract shared electrons in a bond.
8. What are s, p, d, and f block elements?
S-block elements include groups 1 and 2, where electrons fill the s orbital. P-block elements are in groups 13-18, with the p orbital being filled. D-block elements, or transition metals, are in groups 3-12, filling the d orbital. F-block elements are lanthanoids and actinoids, where f orbitals are filled.
9. Why are noble gases placed in group 18?
Noble gases are placed in group 18 because they have completely filled valence shells, making them extremely stable and mostly chemically inert. Their unique electronic configuration justifies their distinct grouping.
10. How do valency and atomic size change along a period and down a group?
Valency generally increases from 1 to 4, then decreases from 4 to 0 across a period. Atomic size (radius) decreases across a period and increases down a group due to the addition of more electron shells.
11. What are the applications of periodic classification of elements?
Periodic classification helps in:
- Predicting the chemical properties of elements
- Identifying trends in reactivity
- Selecting suitable elements for industrial and laboratory uses
- Understanding the structure and bonding in compounds
12. What is a Dobereiner’s triad?
Dobereiner’s triads were early attempts to classify elements into groups of three, where the atomic mass of the middle element was approximately the average of the other two. Although limited in scope, it showed evidence for periodic relationships among elements.
