2. Which of the following is the correct formula for Ammonium Dichromate. A. $$ \mathrm{NH}_{4} \mathrm{Cr}_{2} \mathrm{O}_{7} $$ B. $$ \mathrm{NH}_{4}\left(\mathrm{Cr}_{2} \mathrm{O}_{7}\right)_{2} $$ C. $$ \left(\mathrm{NH}_{4}\right)_{2} \mathrm{Cr}_{2} \mathrm{O}_{7} $$ D. $$ \left(\mathrm{NH}_{4}\right)_{2} \mathrm{CrO}_{4} $$

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To determine the correct formula for Ammonium Dichromate, we need to analyze the components of the compound:

1. **Ammonium Ion**: The ammonium ion is represented as $$ \mathrm{NH}_{4}^{+} $$.
2. **Dichromate Ion**: The dichromate ion is represented as $$ \mathrm{Cr}_{2}\mathrm{O}_{7}^{2-} $$.

Since the ammonium ion has a charge of $$ +1 $$ and the dichromate ion has a charge of $$ -2 $$, we need two ammonium ions to balance the charge of one dichromate ion. Therefore, the formula for Ammonium Dichromate can be constructed as follows:

- We need 2 ammonium ions: $$ 2 \times \mathrm{NH}_{4}^{+} $$
- We need 1 dichromate ion: $$ \mathrm{Cr}_{2}\mathrm{O}_{7}^{2-} $$

Putting this together, the formula becomes:

$$
\left(\mathrm{NH}_{4}\right)_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}
$$

Now, let's compare this with the options provided:

A. $$ \mathrm{NH}_{4} \mathrm{Cr}_{2} \mathrm{O}_{7} $$  
B. $$ \mathrm{NH}_{4}\left(\mathrm{Cr}_{2} \mathrm{O}_{7}\right)_{2} $$  
C. $$ \left(\mathrm{NH}_{4}\right)_{2} \mathrm{Cr}_{2} \mathrm{O}_{7} $$  
D. $$ \left(\mathrm{NH}_{4}\right)_{2} \mathrm{CrO}_{4} $$

The correct formula for Ammonium Dichromate is:

**C. $$ \left(\mathrm{NH}_{4}\right)_{2} \mathrm{Cr}_{2} \mathrm{O}_{7} $$**.
The correct formula for Ammonium Dichromate is $$ \left(\mathrm{NH}_{4}\right)_{2} \mathrm{Cr}_{2} \mathrm{O}_{7} $$.

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