Accordung to crystal Field theory ,
If splitting energy is higher than the pairing energy (∆s >∆p) in an octahedral complex
Then will the electrons pair up or will they not?
I am confused because
In the video, it was said that they'll pair up if ∆p>∆s
And in my book, it's written that they'll pair up if ∆s>∆p
Accordung to crystal Field theory ,
If splitting energy is higher than the pairing energy (∆s >∆p) in an octahedral complex
Then will the electrons pair up or will they not?
I am confused because
In the video, it was said that they'll pair up if ∆p>∆s
And in my book, it's written that they'll pair up if ∆s>∆p
According to the Aufbau principle, electrons are filled from lower to higher energy orbitals. For the octahedral case, this corresponds to the dxy, dxz, and dyz orbitals. Following Hund's rule electrons are filled in order to have the highest number of unpaired electrons. For example, if one had a d3 complex, there would be three unpaired electrons. If one were to add an electron, however, it has the ability to fill a higher energy orbital ( dz² or dx²-y²) or pair with an electron residing in the dxy, dxz, or dyz orbitals. This pairing of the electrons requires spin pairing energy. If the pairing energy is less than the crystal field splitting energy(∆p<∆s), then the next electron will go into the dxy, dxz, or dyz orbitals due to stability. This situation allows for the least amount of unpaired electrons, and is known as low spin If the pairing energy is greater than ∆p>∆s, then the next electron will go into the dz² or dx²-y²orbitals as an unpaired electron. This situation allows for the most number of unpaired electrons, and is known as high spin.
According to the Aufbau principle, electrons are filled from lower to higher energy orbitals. For the octahedral case, this corresponds to the dxy, dxz, and dyz orbitals. Following Hund's rule electrons are filled in order to have the highest number of unpaired electrons. For example, if one had a d3 complex, there would be three unpaired electrons. If one were to add an electron, however, it has the ability to fill a higher energy orbital ( dz² or dx²-y²) or pair with an electron residing in the dxy, dxz, or dyz orbitals. This pairing of the electrons requires spin pairing energy. If the pairing energy is less than the crystal field splitting energy(∆p<∆s), then the next electron will go into the dxy, dxz, or dyz orbitals due to stability. This situation allows for the least amount of unpaired electrons, and is known as low spin If the pairing energy is greater than ∆p>∆s, then the next electron will go into the dz² or dx²-y²orbitals as an unpaired electron. This situation allows for the most number of unpaired electrons, and is known as high spin.
