[cs_content][cs_section parallax=”false” separator_top_type=”none” separator_top_height=”50px” separator_top_angle_point=”50″ separator_bottom_type=”none” separator_bottom_height=”50px” separator_bottom_angle_point=”50″ style=”margin: 0px;padding: 45px 0px;”][cs_row inner_container=”true” marginless_columns=”false” style=”margin: 0px auto;padding: 0px;”][cs_column fade=”false” fade_animation=”in” fade_animation_offset=”45px” fade_duration=”750″ type=”1/1″ style=”padding: 0px;”][cs_text]The Chemistry of Art > 4. The Transition Metals > Colour Changes in Transition Metal Ions >[/cs_text][cs_text style=”color: #800000;font-family: “Oxygen”,sans-serif;”]Account for colour changes in transition metal ions in terms of changing oxidation states[/cs_text][cs_text]
- Colour of transition compounds is due to absorption of specific photons of light by electrons (as outlined above)
- The small energy differences between the d orbitals are similar to the energy of photons within the visible light range of ER
- This absorption of certain components of white light makes a compound appear coloured
- It exhibits the complement of the colours absorbed
- e.g. Absorbing Red = Blue/Green (cyan) appearance
- As each oxidation state has a different arrangement of filled and unfilled d orbitals, the range of energies from visible light it can absorb are also different
- Which d-orbitals are full or empty
- Which d-electrons can gain energy to occupy them
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