The number of oxygen atoms present in 2 moles of a compound, which consists of a bivalent metal and a perchorate ion is

Options

A. 4 N
B. 6 N
C. 8 N
D. 16 N

Answer

To solve the problem of finding the number of oxygen atoms present in 2 moles of a compound consisting of a bivalent metal and a perchlorate ion, we will follow these steps:

### Step 1: Identify the components of the compound
The compound consists of a bivalent metal (let's denote it as M) and a perchlorate ion (ClO₄⁻). Since the metal is bivalent, it has a charge of +2 (M²⁺).

### Step 2: Determine the formula of the compound
The perchlorate ion has a charge of -1. To balance the charges of the bivalent metal and the perchlorate ion, we need two perchlorate ions. Therefore, the formula of the compound can be written as:
\[ \text{M(ClO₄)₂} \]

### Step 3: Count the number of oxygen atoms in one formula unit
Each perchlorate ion (ClO₄⁻) contains 4 oxygen atoms. Since there are 2 perchlorate ions in the formula:
\[ \text{Total oxygen atoms in one formula unit} = 2 \times 4 = 8 \text{ oxygen atoms} \]

### Step 4: Calculate the number of oxygen atoms in 2 moles of the compound
Now, we need to find the total number of oxygen atoms in 2 moles of the compound. Since 1 mole of the compound contains 8 oxygen atoms:
\[ \text{Oxygen atoms in 2 moles} = 2 \times 8 = 16 \text{ oxygen atoms} \]

### Step 5: Use Avogadro's number to find the total number of oxygen atoms
Avogadro's number (Na) is approximately \( 6.022 \times 10^{23} \) particles per mole. Therefore, the total number of oxygen atoms in 2 moles of the compound is:
\[ \text{Total oxygen atoms} = 16 \times N_a \]

### Conclusion
Thus, the total number of oxygen atoms present in 2 moles of the compound is:
\[ 16 N_a \]

### Final Answer
The answer is \( 16 N_a \).

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