Determine the maximum number of electrons that can have each of the following designations:
6f:
4d:
2f:
5d(yz):
3d:
To determine the maximum number of electrons for each designation, we need to understand the electron configuration and the rules governing the filling of electron orbitals.
1. 6f:
The "f" designation refers to the f-orbital. In the periodic table, the f-orbital starts at the 6th row (period). Each orbital can hold 2 electrons. The f-orbital has a total of 7 orbitals (6s, 6p, 6d, 6f), so the maximum number of electrons it can hold is 2 electrons per orbital multiplied by 7 orbitals = 14 electrons.
2. 4d:
The "d" designation refers to the d-orbital. The d-orbital starts at the 4th row (period) of the periodic table. Similar to the f-orbital, the d-orbital can hold 2 electrons per orbital. The d-orbital has a total of 5 orbitals (4s, 4p, 4d), so the maximum number of electrons it can hold is 2 electrons per orbital multiplied by 5 orbitals = 10 electrons.
3. 2f:
The "f" designation here suggests the f-orbital but in the second period. However, the f-orbital is not present in the second period. Each period (row) in the periodic table consists of specific orbitals, and the f-orbital starts to appear from the 4th period onward. Therefore, there is no 2f designation.
4. 5d(yz):
The "d(yz)" designation refers to a specific orbital within the d-subshell. The d-orbital, as explained earlier, can hold 2 electrons per orbital and has a total of 5 orbitals. Therefore, the maximum number of electrons in the 5d(yz) orbital is 2 electrons.
5. 3d:
The "d" designation here refers to the d-orbital. Similar to the previous explanation for the 4d orbital, the d-orbital can hold 2 electrons per orbital, and it has a total of 5 orbitals. Therefore, the maximum number of electrons in the 3d orbital is 2 electrons per orbital multiplied by 5 orbitals = 10 electrons.