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Index: Classification of Elements & Periodicity in Properties | Chemistry Class 11 - NEET PDF Download

(a) Genesis of Periodic Classification

(b) Modern Periodic Law and the Present form of the Periodic Law

(c) Nomenclature of Elements with Atomic Numbers > 100

(d) Electronic Configurations of Elements and the Periodic Table

(e) Electronic Configurations and Types of Elements: s, p, d, f Blocks

(f) Periodic Trends in Properties of Elements

(g) Past Year Questions

(h) NCERT Textbook and Solution

(i) Tests, Question Doc and Summary

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FAQs on Index: Classification of Elements & Periodicity in Properties - Chemistry Class 11 - NEET

1. What is the periodic table and how is it organized?
Ans. The periodic table is a tabular arrangement of chemical elements, organized based on their atomic number, electron configuration, and recurring chemical properties. It consists of rows called periods and columns called groups. Elements in the same period have the same number of electron shells, while elements in the same group have similar chemical properties.
2. How are elements classified in the periodic table?
Ans. Elements in the periodic table are classified into metals, nonmetals, and metalloids. Metals are usually solid, shiny, and good conductors of heat and electricity. Nonmetals are typically gases or brittle solids and have poor conductivity. Metalloids have properties that are intermediate between metals and nonmetals.
3. What is the trend in atomic radius across a period?
Ans. The atomic radius generally decreases across a period from left to right in the periodic table. This is because as you move across a period, the number of protons in the nucleus increases, resulting in a stronger attraction between the electrons and the nucleus. This causes the electrons to be pulled closer to the nucleus, leading to a decrease in atomic radius.
4. How does electronegativity change as you move down a group in the periodic table?
Ans. Electronegativity generally decreases as you move down a group in the periodic table. This is because the atomic size increases down a group due to the addition of new electron shells. As the atomic size increases, the distance between the nucleus and the outermost electrons also increases, resulting in a weaker attraction between the nucleus and the electrons. Thus, the ability of an atom to attract electrons decreases, leading to a decrease in electronegativity.
5. What is the periodic trend in ionization energy?
Ans. Ionization energy generally increases across a period from left to right in the periodic table. This is because as you move across a period, the atomic size decreases and the nuclear charge increases. The electrons in the outermost shell experience a stronger attraction to the nucleus, making it more difficult to remove an electron. Therefore, the ionization energy increases. However, ionization energy decreases as you move down a group due to the increased atomic size and shielding effect.
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