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Cr(VI) should have no unpaired electrons and have no color, but when bound to oxygen, charge transfer occurs from the O 2-. CrO4 (chromate) has four oxygens which all charge transfer to the Chromium giving orange color. In Cr2O7 (dichromate) one oxygen bridges between the two Chromium atoms so each only gets charge transfer from three oxygens. Cr(VI) should have no unpaired electrons and have no color, but when bound to oxygen, charge transfer occurs from the O 2-. CrO4 (chromate) has four oxygens which all charge transfer to the Chromium giving orange color. In Cr2O7 (dichromate) one oxygen bridges between the two Chromium atoms so each only gets charge transfer from three oxygens.

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15y ago
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1w ago

Potassium dichromate appears orange-red due to the presence of two chromium atoms in the +6 oxidation state. On the other hand, potassium chromate appears yellow as it contains only one chromium atom in the +6 oxidation state. The difference in color is due to the different chemical environments and structures of the two compounds.

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Q: In potassium dichromate and potassium chromate the oxidation state of chromium is 6 but both have different colors?
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by the reaction of lead nitrate with potassium chromate or potassium dichromate


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