Which of the following is not correctly matched ?

Options

A. Coordination compound containing cationic complex ion : `[Fe(H_(2)O)_(2)(C_(2)O_(4))_(2)]_(2) SO_(4)`
B. Coordination compound containing anionic complex ion : `[Ag(NH_(3))_(2)] Cl`
C. Non-ionic coordination compound : `[Co(NO_(2))_(3)(NH_(3))_(3)]`
D. Coordination compound containing cationic and anionic complex ion : `[Pt(NH_(3))_(4)] [CuCl_(4)]`

Explanation

To determine which of the following coordination compounds is not correctly matched, let's analyze each option step by step.

### Step 1: Analyze the First Option
**Option 1:** Coordination compound containing cationic complex ion: Fe(H2O)2(C2O4)2(SO4)
- The formula can be interpreted as Fe(H2O)2(C2O4)2(SO4).
- The sulfate ion (SO4) has a charge of -2.
- The oxalate ion (C2O4) has a charge of -2, and there are two of them, contributing -4.
- The total negative charge from the ligands is -6.
- To balance this, the iron (Fe) must have a charge of +6. However, iron typically has oxidation states of +2 or +3.
- Therefore, this complex is indeed a cationic complex ion.
**Conclusion:** This option is correctly matched.

### Step 2: Analyze the Second Option
**Option 2:** Coordination compound containing anionic complex ion: Ag(NH3)2Cl
- The formula can be interpreted as Ag(NH3)2Cl.
- The chloride ion (Cl) has a charge of -1.
- The ammonia (NH3) is a neutral ligand and does not contribute to the charge.
- Therefore, the silver (Ag) must have a charge of +1 to balance the -1 charge from the chloride ion.
- This means that the complex ion is Ag(NH3)2^+.
- Since the complex is positively charged, it is a cationic complex, not an anionic complex.
**Conclusion:** This option is incorrectly matched.

### Step 3: Analyze the Third Option
**Option 3:** Non-ionic coordination compound: Co(NO2)3(NH3)3
- The formula can be interpreted as Co(NO2)3(NH3)3.
- The nitrite ion (NO2) has a charge of -1, and there are three of them, contributing -3.
- The ammonia (NH3) is neutral and does not contribute to the charge.
- Therefore, cobalt (Co) must have a charge of +3 to balance the -3 charge from the nitrite ions.
- Since this complex does not carry an overall charge, it is indeed a non-ionic coordination compound.
**Conclusion:** This option is correctly matched.

### Step 4: Analyze the Fourth Option
**Option 4:** Coordination compound containing cationic and anionic complex ion: Pt(NH3)4CuCl4
- The formula can be interpreted as Pt(NH3)4CuCl4.
- The chloride ions (Cl) have a charge of -1, and there are four of them, contributing -4.
- The ammonia (NH3) is neutral and does not contribute to the charge.
- The platinum (Pt) must have a charge of +2 to balance the -4 charge from the chloride ions.
- The complex ion CuCl4 has a charge of -2, indicating that there are both cationic (Pt(NH3)4^2+) and anionic (CuCl4^2-) complexes present.
**Conclusion:** This option is correctly matched.

### Final Answer
Based on the analysis, the option that is not correctly matched is **Option 2: Ag(NH3)2Cl**, which is incorrectly labeled as containing an anionic complex ion when it is actually a cationic complex.