How would the dx2−y2 orbital in the n=5 shell compare to the dx2−y2 orbital in the n=3 subshell?
True or False
1.The contour of the orbital would extend further out along the x and y axes.
2. The value of ℓ would increase by 2.
3.The radial probability function would include two more nodes.
4. The orientation of the orbital would be rotated 45∘ along the xy plane.
5. The mℓ value would be the same.
1,3,5 are true
2 and4 false
1,3,5 are true
2 and 4 false. I just verified this.
You're three years late bro
Yeah A, C, and E are true, B and D are false.
1 3 5 are true 2 and 4 are false, just verified it lovesss
1,3,5 are correct.
1,3,5 are true 2,4 are false.
To compare the dx2−y2 orbital in the n=5 shell to the dx2−y2 orbital in the n=3 subshell, we can use the principles of quantum mechanics. Here's how we can determine the accuracy of each statement:
1. True. The n=5 shell has higher energy levels than the n=3 subshell, which means the dx2−y2 orbital in the n=5 shell would extend further out along the x and y axes than in the n=3 subshell.
2. False. The value of ℓ determines the shape of the orbital and is independent of the principal quantum number (n). The dx2−y2 orbital has ℓ = 2 in both the n=5 shell and the n=3 subshell.
3. True. The radial probability function determines the probability of finding an electron at a particular distance from the nucleus. Higher energy levels have more nodes, which are regions of zero probability. The n=5 shell would have two more nodes than the n=3 subshell, leading to a different radial probability function.
4. False. The orientation of the dx2−y2 orbital along the xy plane remains the same regardless of the energy level or subshell.
5. True. The mℓ value represents the magnetic quantum number and determines the orientation of the orbital within a given subshell. Since we are comparing the dx2−y2 orbital within the same subshell (ℓ = 2), the mℓ value would remain the same.
Therefore, the correct answers are:
1. True
2. False
3. True
4. False
5. True
1,3,5 are true
and
5,4 are false