![]() Periodic table Chemical element Color Atomic number Worksheet, periodic, angle, text png 3108x2045px 459.09KB. ![]() Electron shell Valence electron Boron Electron configuration, chemical Element, angle png 600圆00px 47.14KB.Electron configuration Germanium Electron shell Bohr model Valence electron, copper shell, chemical Element, electron png 500x500px 60.89KB.Electron shell Sodium Electron configuration Bohr model, valance, chemical Element, label png 1200x1200px 128.83KB.Atomic nucleus Proton Electron Chemistry, Atomo, purple, chemical Element png 978x1024px 679.27KB.Zinc Atom Lewis structure Bohr model Electron configuration, Electron House, chemical Element, label png 1200x1200px 160.51KB.Phosphorus Electron shell Valence electron Atom Chemical element, three-dimensional blocks, angle, electron png 600圆00px 62.14KB.Bohr model Atomic nucleus Atomic theory Iron, atomic, chemical Element, electronics png 500x510px 77.31KB.In the end, for this particular geometry, it doesn't matter whether you assume the bottom four #d# orbitals are in a high spin or low spin configuration amongst each other.Non-commercial use, DMCA Contact Us Relevant png images So, we would expect to fill the lower four #d# orbitals completely, before filling the #d_(z^2)#. Here we see that the energy gap between #d_(xy)# and #d_(x^2 - y^2)# and #d_(z^2)# is large. The crystal field splitting diagram then looks like this: The #d_(xz)# and #d_(yz)# are about equally stabilized amongst each other, but more stabilized than the #d_(xy)# and #d_(x^2-y^2)#, as the best the ligands can do is line up with their nodal planes.The #d_(xy)# and #d_(x^2 - y^2)# are somewhat stabilized by their attraction to the positive metal center.The #d_(z^2)# is directly along the #z# axis, and is highly destabilized by interacting directly with the metal #d# orbital.Here, we treat the #"CN"^(-)# as point charges that repel the metal's #d# orbitals as they come in to form the complex. I won't go too much into the molecular orbital diagram other than the portion of it that comes out of Crystal Field Theory. #underbrace(ul(uarr darr)" "ul(uarr color(white)(darr))" "ul(uarr color(white)(darr))" "ul(uarr color(white)(darr))" "ul(uarr color(white)(darr)))_("3d")#īut this is a complex, and cobalt here has a coordination number of #5#, which denotes a trigonal bipyramidal geometry. So the electron configuration for #"Co"^(3+)# isĪnd we denote complex as containing a #bb(d^6)# electron count. The electron configuration of neutral cobalt is Thus, cobalt is in its #bb(+3)# oxidation state. Since cyanide, #"CN"^(-)# will contribute a #-1# charge, it follows that the total charge contributed by #5# of them is #-5#. If there are any unpaired electrons, we should expect #^(2-)# to be paramagnetic. (We'll work in the realm of crystal field theory and only look at the crystal field splitting diagram that came from the metal's original #d# atomic orbitals.) Well, the first thing you should do is find out the oxidation state of cobalt in this complex ion, so you can find its d-electron count.įrom there, by knowing the electron configuration of cobalt in the complex, one can deduce if any of the electrons are unpaired in the complex's molecular orbital diagram.
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