Question

The probability density plots of 1s and 2s orbitals are given in figure. 

 

The density of dots in a region represents the probability density of finding electrons in the region. On the basis of the above diagram, which of the following statements is incorrect?

• A. 1s and 2s orbitals are spherical in shape.
• B. The probability of finding the electron is maximum near the nucleus.
• C. The probability of finding the electron at a given distance is equal in all directions.
• D. The probability density of electrons for 2s orbital decreases uniformly as distance from the nucleus increases.

Hint:

For atomic orbitals: - 1s and 2s orbitals are spherically symmetric. - The 2s orbital has a node where the probability density is zero. - The probability density depends only on the distance from the nucleus, not on the direction.

Answer 1

The Correct Option is D

Step 1: Analyze the given statements based on the properties of 1s and 2s orbitals. 
- Statement A: 1s and 2s orbitals are spherical in shape. This is correct. Both 1s and 2s orbitals are spherically symmetric. 
- Statement B: The probability of finding the electron is maximum near the nucleus. This is correct for the 1s orbital. However, for the 2s orbital, the probability density has a node (a region where the probability density is zero) before increasing again. Thus, the probability is not maximum near the nucleus for the 2s orbital. 
- Statement C: The probability of finding the electron at a given distance is equal in all directions. This is correct. Since both 1s and 2s orbitals are spherically symmetric, the probability density depends only on the distance from the nucleus, not on the direction. 
- Statement D: The probability density of electrons for the 2s orbital decreases uniformly as the distance from the nucleus increases. This is incorrect. The probability density of the 2s orbital does not decrease uniformly. It has a node (a region of zero probability density) and then increases again before eventually decreasing. 
Conclusion: The incorrect statement is (D).