This might be because of the impurities present in the product As a result it

This might be because of the impurities present in

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This might be because of the impurities present in the product. . As a result, it can be concluded that the sample obtained was not pure. The splitting energy found from the previous experiment 5 is ~22931 which is pretty high, which indicates that the metal complex is a low spin. Table 4 shows the IR of hexamminecobalt(III) [Co(NH 3 ) 6 ] 3+ . There are three medium intensity peaks at ~ 3175.43, ~ 1632 and ~ 1326 which indicates the presence of ammine. The peak at ~1384 corresponds to the N-H stretch. Therefore, the presence of ammine group confirms that the sample prepared was hexamminecobalt(III) [Co(NH 3 ) 6 ] 3+ . Co has an oxidation state of 3+. It has 6 electrons in its d orbital. Since ox -2 is a strong field ligand and thus it has low spin. [Co(NH) 3 ] 3+ has an octahedral structure. . Previous experiments 5 confirm that [Co(NH 3 ) 6 ] 3+ is a high spin(paramagnetic) molecule with electronic configuration (t 2g 6 e g 0 ). Therefore the electronic configuration of [Co(NH 3 ) 6 ] is t 2g 6 e g 0 and structure are shown below: Triglycinatocobalt(III) [Co(gly) 3 ] [Co(gly) 3 ] is a d 6 complex.
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Graph 4 shows the UV-VIS spectra of Triglycinatocobalt(III) [Co(gly) 3 ] produced in this experiment. Co has an oxidation state of 3+. It is a d 6 complex and is octahedral in structrure. Since gly is a strong field ligand and thus it has low spin. Therefore the electronic configuration of [Co(gly) 3 ] is t 2g 6 e g 0 as shown below: The purple color is the result of the absorption of the light which results in the promotion of this t 2g electrons into the e g level. It is purple in color because cobalt absorbs light in the yellow part of the spectrum . When glycine is bonded to the cobalt, it acts as a strong ligand. The extinction coefficient calculated is ~278 as shown in table 2. Since calculated is less than 1000, which means that there is a d- ɛ d transition. Literature values for the extinction coefficient were unable to obtain. So, these values will not be directly commented on. Graph 4 shows the UV-VIS spectra of - [Co(gly) 3 ] produced in this experiment. The λ mzx1 observed are at 531nm corresponds to two e g ←t 2g transitions. The peak at 531 nm corresponds to the 5 T 2 5 E 1 (lower energy) transition and these transitions are spin allowed and laporte forbidden. In Previous experiments 5 , λ mzx1 found for this experiment is 538 which is pretty close to the values obtained. As a result, it can be concluded that the sample obtained was pure. The splitting energy found from the previous experiment 5 is ~20286 which is pretty high, which indicates that the metal complex is a low spin. Trioxalatocobaltate [Co(ox) 3 ] 3- Co has an oxidation state of 3+. It has 6 electrons in its d orbital. Previous experiments 5 confirm that Sox -2 is a weak field ligand and thus it has high spin. [Co(ox) 3 ] 3- has an octahedral structure. Therefore the electronic configuration of [Co(gly) 3 ] is t 2g 4 e g 2 as shown below:
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Graph 6 shows the UV-VIS spectra of Trioxalatocobaltate [Co(ox) 3 ] 3- produced in this experiment.
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