a. The orbital described by n=3 and l=0 is a 3s orbital.
b. The orbital described by n=4 and l=2 is a 4d orbital.
c. The orbital described by n=5 and l=3 is a 5f orbital.
Name the orbitals described by the stated quantum numbers.
a. n=3, l=0
b. n=4, l=2
c. n=5, l=3
9 answers
2. State the "n" and "l" quantum numbers for the following orbitals?
a. 4d
b. 5f
a. 4d
b. 5f
a. The "n" and "l" quantum numbers for the 4d orbital are n=4 and l=2.
b. The "n" and "l" quantum numbers for the 5f orbital are n=5 and l=3.
b. The "n" and "l" quantum numbers for the 5f orbital are n=5 and l=3.
What are the possible ml values for the âfâ orbital?
The "f" orbital can have a range of possible "ml" values. The "ml" quantum number represents the magnetic quantum number, which specifies the orientation of the orbital in space. For the "f" orbital, the possible ml values range from -3 to +3, including 7 values in total (-3, -2, -1, 0, 1, 2, 3).
4. How many possible orbitals are there for n=10?
The number of possible orbitals for a given value of the principal quantum number "n" can be determined using the formula 2n^2.
For n=10, the number of possible orbitals is:
2(10^2) = 2(100) = 200
Therefore, there are 200 possible orbitals for n=10.
For n=10, the number of possible orbitals is:
2(10^2) = 2(100) = 200
Therefore, there are 200 possible orbitals for n=10.
I thought it was 100 for the last answer
Apologies for the confusion. You are correct. The formula for determining the number of possible orbitals for a given value of the principal quantum number "n" is 2n^2.
So for n=10, the number of possible orbitals is:
2(10^2) = 2(100) = 200.
The previous answer I gave was incorrect. There are indeed 100 possible orbitals for n=10. Thank you for catching that mistake.
So for n=10, the number of possible orbitals is:
2(10^2) = 2(100) = 200.
The previous answer I gave was incorrect. There are indeed 100 possible orbitals for n=10. Thank you for catching that mistake.
1 answer