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Add acceptor calculated

okay so today we're gonna look at El FSC ligand field stabilization energy and then we'll take that one step further and look at stabilization energy of coordination complexes and we can use this to predict whether a compound is likely to be high spin or low spin so we'll walk through the example of the iron complex with six water ligands so our calculation for lf-- see is that it's negative point four times the number of electrons and the teach of G orbitals plus point six times the number of electrons in the eg orbitals times the Delta zero Delta o which is the energy gap between the t 2 g and the eg so our example the first thing we need to do is determine the number of D electrons so this is iron plus two iron has eight valence so this is six D electrons then we draw the splitting diagrams I have them over here and we can fill them in so for high spin we would fill in one electron in each orbital and then pair one and for the low spin we're gonna put all of them paired in the T 2 G orbitals so we've drawn the diagrams we set up the equation so this is LF se- 0.4 times T 2g so that's times four plus 0.6 times the two in the eg so that's times two so this is negative one point six plus one point two times Delta o and that gives us negative 0.4 times Delta zero and if we assume that Delta zero is 16,000 usually you have to go look that up for the compound or measure it with the UV so that gives us we do the calculation negative 0.4 times 16,000 you get negative 6400 centimeters to the minus one for the low-spin this is going to be zero because I don't have any in the eg and this will be six so this will be negative two point four times oh and if that's 16,000 we'll multiply 16 thousand times negative two point four and we get negative 38 thousand four hundred oops there's 400 there centimeters to the minus one so we've calculated the LF AC for both of them in the next page we're going to talk about calculating the SE just the stabilization energy so this is the LFS e plus then we take into account the cost of pairing electrons so I've taken a brought over the sixty-four net minus 60 400 centimeters to the minus one for the high spin from the previous page and minus thirty eight hundred for the stabilization of the low spin then we have to look at how much pairing energy so in this we have one set of electrons and so that that are paired so it would be plus one pairing energy but in the low spin I have three sets of electrons that are paired so this will be three pairing energies so this the pairing energy has been calculated here is minus eighteen thousand so this will be minus sixty four hundred plus eighteen thousand which gives you eleven thousand 600 centimeters to the minus 1 and this is minus 38 thousand four hundred plus three times eighteen thousand so plus fifty four thousand six hundred we add those together and we get fifteen thousand six hundred and so we have the stabilization energy so now we look at how much energy it costs to put the electrons into the upper orbitals the eg the higher energy plus balancing it with how much it costs to pair of them and when we calculate them together we can look and say oh the high spin is actually more stable it's got a smaller energy than low spin so we would predict that this iron complex is high spin you