How to determine the greatest d orbital splitting?












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This question comes specifically from an IB Chemistry HL Paper 1 in May 2018 TZ1, namely question 8.



Which complex has the greatest d orbital splitting?



It gives 4 Complexes $ce{[Fe(H_2O)_6]^{2+}}$, $ce{[Fe(H_2O)_6]^{3+}}$, $ce{[Co(H_2O)_6]^{3+}}$, $ce{[Cr(NH_3)_6]^{3+}}$ and it says that they give the colours green, orange, blue and violet respectively.



Initially I thought that the answer would be $ce{[Cr(NH_3)_6]^{3+}}$ because it gives the highest energy light, being violet. However, the answer is given as $ce{[Fe(H_2O)_6]^{3+}}$, why is this?






ions transition-metals oxidation-state color







share|improve this question











$endgroup$

















    1












    $begingroup$


    This question comes specifically from an IB Chemistry HL Paper 1 in May 2018 TZ1, namely question 8.



    Which complex has the greatest d orbital splitting?



    It gives 4 Complexes $ce{[Fe(H_2O)_6]^{2+}}$, $ce{[Fe(H_2O)_6]^{3+}}$, $ce{[Co(H_2O)_6]^{3+}}$, $ce{[Cr(NH_3)_6]^{3+}}$ and it says that they give the colours green, orange, blue and violet respectively.



    Initially I thought that the answer would be $ce{[Cr(NH_3)_6]^{3+}}$ because it gives the highest energy light, being violet. However, the answer is given as $ce{[Fe(H_2O)_6]^{3+}}$, why is this?






    ions transition-metals oxidation-state color







    share|improve this question











    $endgroup$















      1












      1








      1





      $begingroup$


      This question comes specifically from an IB Chemistry HL Paper 1 in May 2018 TZ1, namely question 8.



      Which complex has the greatest d orbital splitting?



      It gives 4 Complexes $ce{[Fe(H_2O)_6]^{2+}}$, $ce{[Fe(H_2O)_6]^{3+}}$, $ce{[Co(H_2O)_6]^{3+}}$, $ce{[Cr(NH_3)_6]^{3+}}$ and it says that they give the colours green, orange, blue and violet respectively.



      Initially I thought that the answer would be $ce{[Cr(NH_3)_6]^{3+}}$ because it gives the highest energy light, being violet. However, the answer is given as $ce{[Fe(H_2O)_6]^{3+}}$, why is this?






      ions transition-metals oxidation-state color







      share|improve this question











      $endgroup$




      This question comes specifically from an IB Chemistry HL Paper 1 in May 2018 TZ1, namely question 8.



      Which complex has the greatest d orbital splitting?



      It gives 4 Complexes $ce{[Fe(H_2O)_6]^{2+}}$, $ce{[Fe(H_2O)_6]^{3+}}$, $ce{[Co(H_2O)_6]^{3+}}$, $ce{[Cr(NH_3)_6]^{3+}}$ and it says that they give the colours green, orange, blue and violet respectively.



      Initially I thought that the answer would be $ce{[Cr(NH_3)_6]^{3+}}$ because it gives the highest energy light, being violet. However, the answer is given as $ce{[Fe(H_2O)_6]^{3+}}$, why is this?






      ions transition-metals oxidation-state color




      ions transition-metals oxidation-state color






      share|improve this question















      share|improve this question













      share|improve this question




      share|improve this question








      edited 2 hours ago









      Mathew Mahindaratne

      1,44413




      1,44413










      asked 4 hours ago









      Anthony PAnthony P

      71




      71






















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          $begingroup$

          The colour at which the complex absorbs reflects the wavelength of the d–d* electronic transitions. However, this colour is not the same as the transmitted colour (which you see), but is instead complementary to the transmitted colour. Therefore, a complex that appears purple is actually absorbing lower-energy light than a complex that appears red.






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            $begingroup$

            The colour at which the complex absorbs reflects the wavelength of the d–d* electronic transitions. However, this colour is not the same as the transmitted colour (which you see), but is instead complementary to the transmitted colour. Therefore, a complex that appears purple is actually absorbing lower-energy light than a complex that appears red.






            share|improve this answer









            $endgroup$


















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              $begingroup$

              The colour at which the complex absorbs reflects the wavelength of the d–d* electronic transitions. However, this colour is not the same as the transmitted colour (which you see), but is instead complementary to the transmitted colour. Therefore, a complex that appears purple is actually absorbing lower-energy light than a complex that appears red.






              share|improve this answer









              $endgroup$
















                2












                2








                2





                $begingroup$

                The colour at which the complex absorbs reflects the wavelength of the d–d* electronic transitions. However, this colour is not the same as the transmitted colour (which you see), but is instead complementary to the transmitted colour. Therefore, a complex that appears purple is actually absorbing lower-energy light than a complex that appears red.






                share|improve this answer









                $endgroup$



                The colour at which the complex absorbs reflects the wavelength of the d–d* electronic transitions. However, this colour is not the same as the transmitted colour (which you see), but is instead complementary to the transmitted colour. Therefore, a complex that appears purple is actually absorbing lower-energy light than a complex that appears red.







                share|improve this answer












                share|improve this answer



                share|improve this answer










                answered 3 hours ago









                orthocresol♦orthocresol

                39.6k7114242




                39.6k7114242






























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