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Short Tricks: Periodic Trends Video Lecture | Chemistry Class 11 - NEET
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FAQs on Short Tricks: Periodic Trends Video Lecture - Chemistry Class 11 - NEET
| 1. What are periodic trends in chemistry? |  |
| 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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