The chemical formula of Aluminium plumbate is `-`

Answer

To determine the chemical formula of Aluminium plumbate, we can follow these steps:

### Step 1: Identify the oxidation states
- Aluminium typically has an oxidation state of +3.
- Plumbate, which is derived from lead (Pb) and oxygen (O), has an oxidation state of -2. The general formula for plumbate is PbO3, which carries a -2 charge.

### Step 2: Write the formula for the plumbate ion
- The plumbate ion can be represented as \( \text{PbO}_3^{2-} \). This indicates that for every plumbate ion, there are two negative charges.

### Step 3: Determine the ratio of Aluminium to Plumbate
- Since Aluminium has a +3 charge and Plumbate has a -2 charge, we need to balance the charges in the compound.
- To balance the charges, we can use the least common multiple (LCM) of the charges. The LCM of 3 (from Al) and 2 (from plumbate) is 6.

### Step 4: Calculate the number of ions needed
- To achieve a total positive charge of +6, we would need 2 Aluminium ions (2 x +3 = +6).
- To achieve a total negative charge of -6, we would need 3 plumbate ions (3 x -2 = -6).

### Step 5: Write the final formula
- Therefore, the formula for Aluminium plumbate can be written as:
\[ \text{Al}_2(\text{PbO}_3)_3 \]
- This simplifies to:
\[ \text{Al}_2\text{Pb}_3\text{O}_9 \]

### Final Answer:
The chemical formula of Aluminium plumbate is \( \text{Al}_2\text{Pb}_3\text{O}_9 \).

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