what is the orbital diagram for Au+, how do you fit the f orbitals in?
[Xe] 4f14 5d10
Always follow this pattern:
1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 4f 5d 6p 7s...
http://www.webelements.com/gold/atoms.html
To determine the orbital diagram for Au+ (gold ion), we need to first determine its electron configuration.
The atomic number of gold (Au) is 79, which means it has 79 electrons in its neutral state. However, Au+ indicates that the ion has lost one electron, so it now has 78 electrons.
To fill the orbitals, we follow the Aufbau principle, which states that lower-energy orbitals are filled before higher-energy ones. The order of filling orbitals is as follows: 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f...
Since we are dealing with Au+ (with 78 electrons), we remove electrons in the reverse order of filling until we reach 78 electrons.
Here is the step-by-step process:
1. The first two electrons go into the 1s orbital:
1s²
2. The next two electrons go into the 2s orbital:
2s²
3. The next six electrons go into the 2p orbital:
2p⁶
4. The next two electrons go into the 3s orbital:
3s²
5. The next six electrons go into the 3p orbital:
3p⁶
6. The next two electrons go into the 4s orbital:
4s²
7. The next ten electrons go into the 3d orbital:
3d¹⁰
8. The next ten electrons go into the 4p orbital:
4p⁶
9. The next two electrons go into the 5s orbital:
5s²
10. The next ten electrons go into the 4d orbital:
4d¹⁰
11. The next six electrons go into the 5p orbital:
5p⁶
12. The next two electrons go into the 6s orbital:
6s²
At this point, the electron configuration is [Xe] 4f¹⁴ 5d¹⁰ 6s².
To fit the f orbitals in, we write the electron configuration for elements that have f orbitals (lanthanides and actinides) and their subsequent positions in the periodic table. In the case of gold (Au), its electron configuration is written after the noble gas xenon (Xe) because it is in period 6. Therefore, we include [Xe] in the electron configuration.
Note that for Au+, the electron configuration would be [Xe] 4f¹⁴ 5d¹⁰, as it lost two electrons from the 6s orbital.
To determine the orbital diagram for Au+, we need to consider the electron configuration of gold (Au) and then remove one electron to account for the +1 charge.
The atomic number of gold is 79, indicating that a neutral gold atom has 79 electrons. The electron configuration of neutral Au is:
1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁶ 5s² 4d¹⁰ 5p⁶ 6s² 4f¹⁴ 5d¹⁰ 6p⁶ 7s²
Now, let's remove one electron to account for the Au+ ion. The removed electron is typically taken from the highest energy orbital, which in this case is the 6s orbital. Therefore, the electron configuration of Au+ becomes:
1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁶ 5s² 4d¹⁰ 5p⁶ 6s¹ 4f¹⁴ 5d¹⁰ 6p⁶ 7s²
Regarding the f orbitals, for Au+, the f orbitals (4f) are completely filled before the 6s orbital is filled. This is due to the Aufbau principle, which states that lower energy levels must be filled before higher energy levels. The f orbitals are filled before the 6s orbital because they have a lower energy level.
So, in the orbital diagram for Au+, you would show the complete filling of the f orbitals (4f) first and then proceed with the remaining electrons as per the electron configuration mentioned above.
Please note that the orbital diagrams are represented by the orbitals as boxes and arrows indicating the spin direction of the electrons within the orbitals.