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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
edited 2 hours ago
Mathew Mahindaratne
1,44413
asked 4 hours ago
Anthony PAnthony P
121
$endgroup$
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 4 hours ago
Anthony PAnthony P
121
$endgroup$
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 4 hours ago
Anthony PAnthony P
121
$endgroup$
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 4 hours ago
Anthony PAnthony P
121
edited 2 hours ago
Mathew Mahindaratne
1,44413
asked 4 hours ago
Anthony PAnthony P
121
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 4 hours ago
Anthony PAnthony P
121
asked 4 hours ago
Anthony PAnthony P
121
asked 4 hours ago
Anthony PAnthony P
121
121
add a comment |
add a comment |
1 Answer
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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 4 hours ago
orthocresol♦orthocresol
39.6k7114242
$endgroup$
add a comment |
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1 Answer
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1 Answer
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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 4 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 4 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 4 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 4 hours ago
orthocresol♦orthocresol
39.6k7114242
answered 4 hours ago
orthocresol♦orthocresol
39.6k7114242
answered 4 hours ago
orthocresol♦orthocresol
39.6k7114242
answered 4 hours ago
orthocresol♦orthocresol
39.6k7114242
39.6k7114242
add a comment |
add a comment |
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