Difference in `._(17)Cl^(35) and ._(17)Cl^(37)` is of

Options

A. Atomic number
B. Number of protons
C. Number of neutrons
D. Number of electrons

Explanation

To find the difference between the isotopes \( _{17}^{35}\text{Cl} \) and \( _{17}^{37}\text{Cl} \), we can follow these steps:

### Step 1: Identify the Atomic Number
The atomic number of chlorine (Cl) is 17. This means both isotopes have the same number of protons.

### Step 2: Identify the Mass Numbers
The mass numbers for the isotopes are given as follows:
- For \( _{17}^{35}\text{Cl} \), the mass number is 35.
- For \( _{17}^{37}\text{Cl} \), the mass number is 37.

### Step 3: Calculate the Number of Neutrons
The number of neutrons in an isotope can be calculated using the formula:
\[ \text{Number of Neutrons} = \text{Mass Number} - \text{Atomic Number} \]
- For \( _{17}^{35}\text{Cl} \):
\[ \text{Number of Neutrons} = 35 - 17 = 18 \]
- For \( _{17}^{37}\text{Cl} \):
\[ \text{Number of Neutrons} = 37 - 17 = 20 \]

### Step 4: Compare the Number of Neutrons
Now we can compare the number of neutrons in both isotopes:
- \( _{17}^{35}\text{Cl} \) has 18 neutrons.
- \( _{17}^{37}\text{Cl} \) has 20 neutrons.

### Conclusion
The difference between the two isotopes \( _{17}^{35}\text{Cl} \) and \( _{17}^{37}\text{Cl} \) lies in the number of neutrons. Specifically, \( _{17}^{35}\text{Cl} \) has 18 neutrons, while \( _{17}^{37}\text{Cl} \) has 20 neutrons. Therefore, the difference in the number of neutrons is:
\[ 20 - 18 = 2 \]

### Final Answer
The difference in \( _{17}^{35}\text{Cl} \) and \( _{17}^{37}\text{Cl} \) is in the number of neutrons, which is 2.

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