Which of the following complex `(s)` is/are having correct name ?

Options

A. `Cs[Pt(NH_(3))I_(5)]` Ceasium amminepentaiodidoplatirate(IV)
B. `[Ag(CN)_(2)]^(Θ)` Dicyanidoargentate(I)ion
C. `[Rb_(3)[Cr(C_(2)O_(4))_(3)]` -Rubidium trioxalatochromate(III)
D. `K_(2)[Ni(EDTA)]` Potassium ethylenediaminetetraacetatonickel(II)

Explanation

To determine which of the given complexes have the correct names, we will analyze each complex step by step, focusing on the oxidation states of the central metal ions and the naming conventions for coordination compounds.

### Step 1: Analyze the First Complex
**Complex:** Cs[Pt(NH3)(I)5]
1. **Identify the ligands:** Amine (NH3) and Iodide (I) ligands.
2. **Determine the charge of the complex:** The overall charge is -1.
3. **Calculate the oxidation state of Platinum (Pt):**
- Let the oxidation state of Pt be \(x\).
- The charge from the ligands: 5 Iodide ligands contribute -5 (since each Iodide is -1).
- The equation becomes: \(x - 5 = -1\) → \(x = +4\).
4. **Name the ligands:**
- NH3 is named as "ammine".
- I5 is named as "penta-iodide".
5. **Name the complex:** Since Pt has a +4 oxidation state, it is named as "platinate".
6. **Final name:** Cs[Pt(NH3)(I)5] = Cesium penta-iodidoammine platinate(IV).

**Conclusion for First Complex:** The name is correct.

### Step 2: Analyze the Second Complex
**Complex:** Ag[CN]2
1. **Identify the ligands:** Cyanide (CN).
2. **Determine the charge of the complex:** The overall charge is -1.
3. **Calculate the oxidation state of Silver (Ag):**
- Let the oxidation state of Ag be \(x\).
- The equation becomes: \(x - 2 = -1\) → \(x = +1\).
4. **Name the ligands:** Cyanide is named as "cyano".
5. **Name the complex:** Since Ag has a +1 oxidation state, it is named as "argentate".
6. **Final name:** Ag[CN]2 = Silver dicyanidoargentate(I).

**Conclusion for Second Complex:** The name is correct.

### Step 3: Analyze the Third Complex
**Complex:** Rb3[Cr(C2O4)3]
1. **Identify the ligands:** Oxalate (C2O4).
2. **Determine the charge of the complex:** The overall charge is -3.
3. **Calculate the oxidation state of Chromium (Cr):**
- Let the oxidation state of Cr be \(x\).
- The equation becomes: \(x - 6 = -3\) → \(x = +3\).
4. **Name the ligands:** Oxalate is named as "oxalato".
5. **Name the complex:** Since Cr has a +3 oxidation state, it is named as "chromate".
6. **Final name:** Rb3[Cr(C2O4)3] = Rubidium trioxalatochromate(III).

**Conclusion for Third Complex:** The name is correct.

### Step 4: Analyze the Fourth Complex
**Complex:** K2[Ni(EDTA)]
1. **Identify the ligands:** Ethylenediaminetetraacetic acid (EDTA).
2. **Determine the charge of the complex:** The overall charge is -2.
3. **Calculate the oxidation state of Nickel (Ni):**
- Let the oxidation state of Ni be \(x\).
- The equation becomes: \(x - 4 = -2\) → \(x = +2\).
4. **Name the ligands:** EDTA is named as "ethylenediaminetetraacetato".
5. **Name the complex:** Since Ni has a +2 oxidation state, it is named as "nickelate".
6. **Final name:** K2[Ni(EDTA)] = Potassium ethylenediaminetetraacetato nickelate(II).

**Conclusion for Fourth Complex:** The name is incorrect (it should be nickelate, not nickel).

### Final Summary of Names
1. **First Complex:** Correct
2. **Second Complex:** Correct
3. **Third Complex:** Correct
4. **Fourth Complex:** Incorrect

### Final Answer
The complexes with correct names are 1, 2, and 3.

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