The value of azimuthal quantum number, L, determines the shape of the orbital:
- L = 0 corresponds to s orbital
- L = 1 corresponds to p orbital
- L = 2 corresponds to d orbital
- L = 3 corresponds to f orbital
Since we are looking for the number of electrons with L = 1 for Cd+2, we need to determine the electron configuration of Cd+2 first.
The atomic number of Cd (Cadmium) is 48, so it has 48 electrons in its neutral state. When Cd loses two electrons to form Cd+2, it will have 46 electrons remaining.
The electron configuration of Cd in its ground state is [Kr]5s^24d^10.
When Cd loses two electrons, the electron configuration of Cd+2 becomes [Kr]4d^10.
The 4d subshell has an azimuthal quantum number L = 2, which means there are 10 electrons in that subshell.
For L = 1 (p orbital), there are three p orbitals: px, py, and pz. Each p orbital can hold a maximum of 2 electrons.
Therefore, the number of electrons with L = 1 for Cd+2 is 3 p orbitals × 2 electrons per p orbital = 6 electrons.
So, the number of electrons with L = 1 for Cd+2 is 6.
find the number of electrons with the value of azimuthal quantum number L=1 for Cd+2
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