The selection rules for quantum numbers allow finding the base state electron configuration of carbon is:
- Base state configuration 1s² 2s²2p²
- The excited state configuration of the sub-level 2s and the three sub-levels 2p forms a hybrid orbital called sp³ where the four orbitals have the same energy.
Atoms have an electronic configuration given by the rules of selection of quantum numbers:
- Principal. It is the fundamental number (n) and has values from 1 to infinity, it represents the periods of the periodic table.
- Secondary or orbital. It is the second number and its symbol is l and it has values from zero to n-1, in general it is written in the form of the letter: s p d f.
- Magnetic. The orbital motion of electrons is given and can have values from -l to l.
There is a fourth quantum number when it is the spin and it can only have two values +1/2 and - ½
Carbon has an atomic number 6, therefore its configuration of the ground state is:
1s² 2s² 2p²
When the atom is excited, an electron jumps from the 2 s² level to the 2p² level, leaving the configuration
2s¹ 3p³
In this configuration it has four unpaired electrons, therefore I could form four chemical bonds, experiential measurements show that these four bonds have the same energy, for this to happen there must be a hybridization between the s and p levels where it forms the sp³ orbitals that have the same Energy.
In conclusion using the selection rules of quantum numbers we can find the base state electron configuration of carbon:
- Base state configuration 1s² 2s²2p²
- The excited state configuration of the sub-level 2s and the three sub-levels 2p forms a hybrid orbital called sp³ where the four orbitals have the same energy.
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