James Mahanyu
Jun 20
Explain clearly?
11. (i) . A complex of a
certain metal ion has a
magnetic moment of
4.90 B.M. Another
complex of the same
metal ion in the same
oxidation state has a
magnetic moment of 0
B.M. Which one
among the following
central metal ions
could produce these
data? (a)Cr3+, (b) Mn3+,
(c) Fe2+ or (d) Co2+
(neatly, show all your
calculations)
(ii) . In question (i) above,
if a metal ion has a com-
plex ion with magnetic
moments 4.90B.M. and 2.
8 B.M, then the central
metal ion is?
certain metal ion has a
magnetic moment of
4.90 B.M. Another
complex of the same
metal ion in the same
oxidation state has a
magnetic moment of 0
B.M. Which one
among the following
central metal ions
could produce these
data? (a)Cr3+, (b) Mn3+,
(c) Fe2+ or (d) Co2+
(neatly, show all your
calculations)
(ii) . In question (i) above,
if a metal ion has a com-
plex ion with magnetic
moments 4.90B.M. and 2.
8 B.M, then the central
metal ion is?
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ChatGPT
Jun 20
(i) To determine which central metal ion could produce the given magnetic moments, we can use the formula:
μ = √n(n+2)
Where μ is the magnetic moment in Bohr magnetons (B.M) and n is the number of unpaired electrons.
For the first complex with a magnetic moment of 4.90 B.M:
4.90 = √n(n+2)
Solving for n, we get n = 2 unpaired electrons.
For the second complex with a magnetic moment of 0 B.M:
0 = √n(n+2)
Solving for n, we get n = 0 unpaired electrons.
Now, we can determine which central metal ion corresponds to 2 unpaired electrons in the d orbital. This corresponds to the d4 configuration, which is found in the Fe2+ ion. Therefore, the central metal ion that could produce these data is (c) Fe2+.
(ii) If a metal ion has a complex ion with magnetic moments of 4.90 B.M. and 2.8 B.M., we can use the same formula to determine the number of unpaired electrons for each complex.
For the complex with a magnetic moment of 4.90 B.M:
4.90 = √n(n+2)
Solving for n, we get n = 2 unpaired electrons.
For the complex with a magnetic moment of 2.8 B.M:
2.8 = √n(n+2)
Solving for n, we get n = 1 unpaired electron.
Therefore, the central metal ion in this case would have a d7 configuration, which corresponds to the Mn3+ ion.
μ = √n(n+2)
Where μ is the magnetic moment in Bohr magnetons (B.M) and n is the number of unpaired electrons.
For the first complex with a magnetic moment of 4.90 B.M:
4.90 = √n(n+2)
Solving for n, we get n = 2 unpaired electrons.
For the second complex with a magnetic moment of 0 B.M:
0 = √n(n+2)
Solving for n, we get n = 0 unpaired electrons.
Now, we can determine which central metal ion corresponds to 2 unpaired electrons in the d orbital. This corresponds to the d4 configuration, which is found in the Fe2+ ion. Therefore, the central metal ion that could produce these data is (c) Fe2+.
(ii) If a metal ion has a complex ion with magnetic moments of 4.90 B.M. and 2.8 B.M., we can use the same formula to determine the number of unpaired electrons for each complex.
For the complex with a magnetic moment of 4.90 B.M:
4.90 = √n(n+2)
Solving for n, we get n = 2 unpaired electrons.
For the complex with a magnetic moment of 2.8 B.M:
2.8 = √n(n+2)
Solving for n, we get n = 1 unpaired electron.
Therefore, the central metal ion in this case would have a d7 configuration, which corresponds to the Mn3+ ion.
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Google Gemini AI
Jun 20
(i)
- The magnetic moment (µ) of a complex ion is given by the formula:
```
µ = √(n(n+2))
```
where n is the number of unpaired electrons.
- For a magnetic moment of 4.90 B.M.,
```
4.90 = √(n(n+2))
```
Squaring both sides,
```
24.01 = n(n+2)
```
Solving for n,
```
n = 5
```
- Therefore, the complex ion with a magnetic moment of 4.90 B.M. has 5 unpaired electrons.
- For a magnetic moment of 0 B.M., n = 0. Therefore, the complex ion with a magnetic moment of 0 B.M. has no unpaired electrons.
- Based on these observations, the central metal ion could be either Cr3+ or Fe2+.
- Cr3+ has 3 unpaired electrons, which is not consistent with the given magnetic moment of 4.90 B.M.
- Fe2+ has 4 unpaired electrons, which is consistent with the given magnetic moment of 4.90 B.M.
- Therefore, the central metal ion that could produce these data is Fe2+.
(ii)
- The central metal ion has a complex ion with magnetic moments 4.90B.M. and 2.8 B.M.
- For a magnetic moment of 4.90 B.M., n = 5.
- For a magnetic moment of 2.8 B.M.,
```
2.8 = √(n(n+2))
```
Squaring both sides,
```
7.84 = n(n+2)
```
Solving for n,
```
n = 3
```
- Therefore, the central metal ion has complex ions with 5 and 3 unpaired electrons.
- The only metal ion that can have complex ions with these numbers of unpaired electrons is Fe2+.
- Therefore, the central metal ion is Fe2+.
- The magnetic moment (µ) of a complex ion is given by the formula:
```
µ = √(n(n+2))
```
where n is the number of unpaired electrons.
- For a magnetic moment of 4.90 B.M.,
```
4.90 = √(n(n+2))
```
Squaring both sides,
```
24.01 = n(n+2)
```
Solving for n,
```
n = 5
```
- Therefore, the complex ion with a magnetic moment of 4.90 B.M. has 5 unpaired electrons.
- For a magnetic moment of 0 B.M., n = 0. Therefore, the complex ion with a magnetic moment of 0 B.M. has no unpaired electrons.
- Based on these observations, the central metal ion could be either Cr3+ or Fe2+.
- Cr3+ has 3 unpaired electrons, which is not consistent with the given magnetic moment of 4.90 B.M.
- Fe2+ has 4 unpaired electrons, which is consistent with the given magnetic moment of 4.90 B.M.
- Therefore, the central metal ion that could produce these data is Fe2+.
(ii)
- The central metal ion has a complex ion with magnetic moments 4.90B.M. and 2.8 B.M.
- For a magnetic moment of 4.90 B.M., n = 5.
- For a magnetic moment of 2.8 B.M.,
```
2.8 = √(n(n+2))
```
Squaring both sides,
```
7.84 = n(n+2)
```
Solving for n,
```
n = 3
```
- Therefore, the central metal ion has complex ions with 5 and 3 unpaired electrons.
- The only metal ion that can have complex ions with these numbers of unpaired electrons is Fe2+.
- Therefore, the central metal ion is Fe2+.
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