What is the set of quantum numbers for the last three electrons in an iodine atom?
ml = -4, -3, -2, -1, 0 1, 2, 3, 4. These arbitrarily correspond to the 5s, 5px, 5py, 5pz, 4dx2-y2, 4dz2, 4dxy, 4dxz, and 4dyz orbitals.
The three quantum numbers (n, l, and m) that describe an orbital are integers: 0, 1, 2, 3, and so on. The principal quantum number (n) cannot be zero. The allowed values of n are therefore 1, 2, 3, 4, and so on. The angular quantum number (l) can be any integer between 0 and n - 1.
"Water. Earth. Fire. Air. Long ago, the four nations lived together in harmony. Then, everything changed when the Fire Nation attacked. Only the Avatar, master of all four elements, could stop them, but when the world needed him most, he vanished. A hundred years passed and my brother and I discovered the new Avatar, an airbender named Aang. And although his airbending skills are great, he has a lot to learn before he's ready to save anyone. But I believe Aang can save the world."
Note to above answers:
Since the last 5 electrons in I are 5p5, the 5px, 5py and 5pz are the only three
orbitals involved; i.e., there are no electrons in those d orbitals shown.
To determine the set of quantum numbers for the last three electrons in an iodine atom, we need to first understand the structure of an iodine atom.
Iodine (I) has an atomic number of 53, which tells us it has 53 electrons. The electronic configuration of iodine is 2-8-18-18-7, indicating that there are 5 electron shells.
To determine the quantum numbers for the last three electrons, we start with the fourth electron shell, which contains 18 electrons. The fourth electron shell can have the quantum numbers (n, l, ml, ms), where:
- n is the principal quantum number and represents the energy level or shell. In this case, it is 4.
- l is the azimuthal quantum number and represents the shape of the orbital. It can have values from 0 to (n-1). For the fourth shell, l can range from 0 to 3, representing the s, p, d, and f orbitals, respectively.
- ml is the magnetic quantum number and represents the orientation of the orbital. It ranges from -l to +l, including zero.
- ms is the spin quantum number and describes the spin orientation of the electron. It can be either +1/2 or -1/2.
Since we are interested in the last three electrons, which are in the fifth electron shell, we need to find their quantum numbers within that shell.
In the fifth shell, there are two subshells: one with l = 0 (s orbital) and one with l = 1 (p orbital). The electrons fill orbitals in a specific order, following the Pauli exclusion principle and Hund's rule.
Based on this information, we can determine the set of quantum numbers for each electron as follows:
1. For the first electron in the fifth shell:
- n = 5
- l = 0
- ml = 0 (only one possible value for s orbital)
- ms = +1/2 or -1/2 (two possible values for spin)
2. For the second electron in the fifth shell:
- n = 5
- l = 1
- ml = -1, 0, or +1 (three possible values for p orbital)
- ms = +1/2 or -1/2
3. For the third electron in the fifth shell:
- n = 5
- l = 1
- ml = -1, 0, or +1 (three possible values for p orbital)
- ms = +1/2 or -1/2
Therefore, the set of quantum numbers for the last three electrons in an iodine atom would depend on the specific arrangement of the electrons among the available orbitals.