What is the oxidation state and coordination number (C.N.) of the metal atom in the following coordination compound: Mn(acac)2(SCN)(OH) A. Mn(II), C.N. = 4 B. Mn(II), C.N. = 6 %3D C. Mn(IV), C.N. = 4 D. Mn(IV), C.N. = 6 %3D
What is the oxidation state and coordination number (C.N.) of the metal atom in the following coordination compound: Mn(acac)2(SCN)(OH) A. Mn(II), C.N. = 4 B. Mn(II), C.N. = 6 %3D C. Mn(IV), C.N. = 4 D. Mn(IV), C.N. = 6 %3D
Chemistry
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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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![**Oxidation State and Coordination Number of the Metal Atom in Coordination Compounds**
Understanding both the oxidation state and the coordination number of the central metal atom in a coordination compound is fundamental to grasping its chemical behavior and structure. Let's explore this through a given example:
**Question:** What is the oxidation state and coordination number (C.N.) of the metal atom in the following coordination compound:
\[ \text{Mn(acac)}_2(\text{SCN})(\text{OH}) \]
**Options:**
A. Mn(II), C.N. = 4
B. Mn(II), C.N. = 6
C. Mn(IV), C.N. = 4
D. Mn(IV), C.N. = 6
### Analysis:
1. **Oxidation State Calculation:**
- Acetylacetonate (\(\text{acac}\)) is a bidentate ligand.
- Thiocyanate (\(\text{SCN}\)) is a monodentate ligand.
- Hydroxide (\(\text{OH}^{-}\)) is a monodentate ligand.
Given the neutral nature of the compound and the individual charges of the ligands, calculating the oxidation state of manganese (\(\text{Mn}\)) is necessary.
- Each \(\text{acac}\) ligand is neutral.
- \(\text{SCN}\) is also neutral.
- \(\text{OH}\) carries a -1 charge.
Therefore, the oxidation state (x) of Mn can be derived from the equation:
\[ x + 2(0) + 0 + (-1) = 0 \]
Solving this, we get \( x = +1 \).
However, as hydroxide (\(-1\)) is present, \( \text{Mn} \) has to balance an additional +2 charge often resulting in a stable +3 state.
2. **Coordination Number:**
- Each \(\text{acac}\) ligand coordinates via two donor atoms.
- \(\text{SCN}\) coordinates via one donor atom.
- \(\text{OH}\) coordinates via one donor atom.
Therefore, the total number of coordinated sites:
\[
2(\text{acac}) + 1(\text{SC](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fc8727b1b-9c58-411e-9891-4fb64e6bc696%2F05efd925-bc76-4d2c-90fe-91dbbc036a4f%2Feue0bo_processed.png&w=3840&q=75)
Transcribed Image Text:**Oxidation State and Coordination Number of the Metal Atom in Coordination Compounds**
Understanding both the oxidation state and the coordination number of the central metal atom in a coordination compound is fundamental to grasping its chemical behavior and structure. Let's explore this through a given example:
**Question:** What is the oxidation state and coordination number (C.N.) of the metal atom in the following coordination compound:
\[ \text{Mn(acac)}_2(\text{SCN})(\text{OH}) \]
**Options:**
A. Mn(II), C.N. = 4
B. Mn(II), C.N. = 6
C. Mn(IV), C.N. = 4
D. Mn(IV), C.N. = 6
### Analysis:
1. **Oxidation State Calculation:**
- Acetylacetonate (\(\text{acac}\)) is a bidentate ligand.
- Thiocyanate (\(\text{SCN}\)) is a monodentate ligand.
- Hydroxide (\(\text{OH}^{-}\)) is a monodentate ligand.
Given the neutral nature of the compound and the individual charges of the ligands, calculating the oxidation state of manganese (\(\text{Mn}\)) is necessary.
- Each \(\text{acac}\) ligand is neutral.
- \(\text{SCN}\) is also neutral.
- \(\text{OH}\) carries a -1 charge.
Therefore, the oxidation state (x) of Mn can be derived from the equation:
\[ x + 2(0) + 0 + (-1) = 0 \]
Solving this, we get \( x = +1 \).
However, as hydroxide (\(-1\)) is present, \( \text{Mn} \) has to balance an additional +2 charge often resulting in a stable +3 state.
2. **Coordination Number:**
- Each \(\text{acac}\) ligand coordinates via two donor atoms.
- \(\text{SCN}\) coordinates via one donor atom.
- \(\text{OH}\) coordinates via one donor atom.
Therefore, the total number of coordinated sites:
\[
2(\text{acac}) + 1(\text{SC
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