What is the electron configuration for carbon with sp hybridization?
I have no idea. I know carbon has 4 electrons to use (6 electrons total, but 4 to move around for hybridization purposes), I know that the sp orbitals would take up two of the electrons, do the other two electrons go in unhybridized p orbitals? But what would be the written out electron configuration?
See if this helps. Google sp hybridization and there are several sites to read.
https://www.khanacademy.org/science/chemistry/chemical-bonds/copy-of-covalent-bonds/v/sp-hybridization-jay-final
To determine the electron configuration for carbon with sp hybridization, follow these steps:
1. Determine the total number of valence electrons for carbon. Carbon is in Group 14 of the periodic table, so it has 4 valence electrons.
2. Understand that with sp hybridization, one s orbital and one p orbital will combine to form two sp hybrid orbitals. Each sp orbital will contain one electron.
3. Assign the first two electrons to the two sp hybrid orbitals.
4. The remaining two valence electrons will be placed in the unhybridized p orbitals. Since there are three p orbitals available, one of the p orbitals will remain unoccupied.
So, the electron configuration for carbon with sp hybridization would be written as: 1s^2 2s^1 2p^2.
Note: Remember that electron configurations are written in order of increasing energy levels and individual orbital subshells.