How to determine the greatest d orbital splitting?How do I determine the crystal field splitting for an arbitrary point group?How to determine peroxy oxygen?Iron chemistry: acetates for ebonizing woodHow can the intense color of potassium permanganate be explained with molecular orbital theory?How to determine the magnetic character of heteroleptic complexes?Why do better π-acceptor ligands cause smaller Δ(T) d-orbital splitting?How to Determine An Element's ColourWhat exactly is the d-orbital splitting and how does this affect the colors for transition metal compounds?Pattern to determine the maximum ionic charge for transition elements?Effect of oxidation state on d-orbital splitting
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How to determine the greatest d orbital splitting?
How do I determine the crystal field splitting for an arbitrary point group?How to determine peroxy oxygen?Iron chemistry: acetates for ebonizing woodHow can the intense color of potassium permanganate be explained with molecular orbital theory?How to determine the magnetic character of heteroleptic complexes?Why do better π-acceptor ligands cause smaller Δ(T) d-orbital splitting?How to Determine An Element's ColourWhat exactly is the d-orbital splitting and how does this affect the colors for transition metal compounds?Pattern to determine the maximum ionic charge for transition elements?Effect of oxidation state on d-orbital splitting
$begingroup$
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
edited 2 hours ago
Mathew Mahindaratne
1,44413
asked 3 hours ago
Anthony PAnthony P
71
$endgroup$
add a comment |
$begingroup$
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
edited 2 hours ago
Mathew Mahindaratne
1,44413
asked 3 hours ago
Anthony PAnthony P
71
$endgroup$
add a comment |
$begingroup$
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
edited 2 hours ago
Mathew Mahindaratne
1,44413
asked 3 hours ago
Anthony PAnthony P
71
$endgroup$
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
edited 2 hours ago
Mathew Mahindaratne
1,44413
asked 3 hours ago
Anthony PAnthony P
71
edited 2 hours ago
Mathew Mahindaratne
1,44413
asked 3 hours ago
Anthony PAnthony P
71
edited 2 hours ago
Mathew Mahindaratne
1,44413
edited 2 hours ago
Mathew Mahindaratne
1,44413
edited 2 hours ago
Mathew Mahindaratne
1,44413
1,44413
asked 3 hours ago
Anthony PAnthony P
71
asked 3 hours ago
Anthony PAnthony P
71
asked 3 hours ago
Anthony PAnthony P
71
71
add a comment |
add a comment |
1 Answer
1
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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.
answered 3 hours ago
orthocresol♦orthocresol
39.6k7114242
$endgroup$
add a comment |
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1 Answer
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votes
1 Answer
1
active
oldest
votes
active
oldest
votes
active
oldest
votes
$begingroup$
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.
answered 3 hours ago
orthocresol♦orthocresol
39.6k7114242
$endgroup$
add a comment |
$begingroup$
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.
answered 3 hours ago
orthocresol♦orthocresol
39.6k7114242
$endgroup$
add a comment |
$begingroup$
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.
answered 3 hours ago
orthocresol♦orthocresol
39.6k7114242
$endgroup$
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.
answered 3 hours ago
orthocresol♦orthocresol
39.6k7114242
answered 3 hours ago
orthocresol♦orthocresol
39.6k7114242
answered 3 hours ago
orthocresol♦orthocresol
39.6k7114242
answered 3 hours ago
orthocresol♦orthocresol
39.6k7114242
39.6k7114242
add a comment |
add a comment |
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