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Short Tricks: Periodic Trends Video Lecture | Chemistry Class 11 - NEET

FAQs on Short Tricks: Periodic Trends Video Lecture - Chemistry Class 11 - NEET

1. What are periodic trends in chemistry?

Ans. Periodic trends in chemistry refer to the regular patterns observed in the properties of elements as they are arranged in the periodic table. These trends include atomic radius, ionization energy, electronegativity, and electron affinity, among others.

2. How does atomic radius change across a period?

Ans. Atomic radius decreases across a period from left to right in the periodic table. This is primarily due to an increase in the effective nuclear charge, which attracts the electrons more strongly and leads to a contraction of the atomic size.

3. Why does ionization energy increase going up a group?

Ans. Ionization energy increases going up a group in the periodic table because the atomic size decreases and the valence electrons are held more tightly by the nucleus. As a result, more energy is required to remove an electron from an atom.

4. What is electronegativity and how does it vary across the periodic table?

Ans. Electronegativity is the measure of an atom's ability to attract and hold electrons in a chemical bond. It generally increases from left to right across a period and decreases from top to bottom in a group. This trend is influenced by factors such as atomic size and effective nuclear charge.

5. How does electron affinity change across the periodic table?

Ans. Electron affinity refers to the energy change that occurs when an atom gains an electron. Generally, electron affinity increases across a period from left to right due to an increase in effective nuclear charge. However, electron affinity tends to decrease down a group as the atomic size increases and the electrons are further from the nucleus.

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Sep 06, 2025 Last updated

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