Take an example of ion and find the number of hybrid orbitals and pure orbitals

To find the number of hybrid orbitals and pure orbitals for an ion, we need to determine the electron configuration of the ion first. Let's take the example of the chloride ion (Cl-).

Step 1: Determine the electron configuration of the neutral atom. The neutral atom of chlorine (Cl) has an atomic number of 17. Therefore, the electron configuration of Cl is 1s2 2s2 2p6 3s2 3p5.

Step 2: Determine the number of valence electrons. Valence electrons are the electrons in the outermost energy level of an atom. In the case of Cl, the outermost energy level is the 3rd energy level, and it contains 7 electrons (3s2 3p5).

Step 3: Determine the number of hybrid orbitals. The number of hybrid orbitals is equal to the number of valence electrons. In the case of Cl, there are 7 valence electrons, so there will be 7 hybrid orbitals.

Step 4: Determine the number of pure orbitals. Pure orbitals are the orbitals that are not involved in hybridization. In the case of Cl, the 1s, 2s, and 2p orbitals are not involved in hybridization. Therefore, there are 3 pure orbitals.

In summary, for the chloride ion (Cl-), there are 7 hybrid orbitals and 3 pure orbitals.