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Short Tricks: s-block trends Video Lecture | Chemistry for JEE Main & Advanced
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FAQs on Short Tricks: s-block trends Video Lecture - Chemistry for JEE Main & Advanced
| 1. What are the trends observed in the s-block elements? |  |
Ans. The trends observed in the s-block elements include increasing atomic radius down a group, decreasing ionization energy down a group, and increasing reactivity down a group.
| 2. How does the atomic radius change in the s-block elements? | |
Ans. The atomic radius generally increases down a group in the s-block elements. This is due to the addition of new energy levels as we move down the group.
| 3. What happens to the ionization energy in the s-block elements as we move down a group? | |
Ans. The ionization energy generally decreases down a group in the s-block elements. This is because the outermost electrons are farther away from the nucleus, making them easier to remove.
| 4. How does the reactivity change in the s-block elements? | |
Ans. The reactivity generally increases down a group in the s-block elements. This is because the outermost electrons are farther away from the nucleus, making them more easily lost or shared in chemical reactions.
| 5. Are there any exceptions to the trends observed in the s-block elements? | |
Ans. Yes, there are some exceptions to the trends observed in the s-block elements. For example, the ionization energy of helium is higher than that of hydrogen, even though helium is below hydrogen in the periodic table. This is because helium has a completely filled 1s orbital, which provides extra stability and makes it harder to remove an electron.
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Nov 23, 2024 Last updated |
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