`._(6)^(14)C, ._(6)^(12)C` differ from each other in number of

Options

A. electrons
B. photons
C. protons
D. nucleons

Explanation

To solve the question regarding the differences between the isotopes \(_{6}^{14}C\) and \(_{6}^{12}C\), we need to analyze the provided notation and understand what each part represents.

### Step-by-Step Solution:

1. **Identify the Components of the Isotopes:**
- The notation \(_{6}^{14}C\) indicates a carbon isotope with:
- Atomic number (Z) = 6 (number of protons)
- Mass number (A) = 14 (total number of protons and neutrons)
- The notation \(_{6}^{12}C\) indicates another carbon isotope with:
- Atomic number (Z) = 6 (number of protons)
- Mass number (A) = 12 (total number of protons and neutrons)

2. **Determine the Number of Protons:**
- Both isotopes have the same atomic number (6), which means they both have 6 protons.

3. **Determine the Number of Neutrons:**
- For \(_{6}^{14}C\):
- Number of neutrons = Mass number - Atomic number = 14 - 6 = 8 neutrons
- For \(_{6}^{12}C\):
- Number of neutrons = Mass number - Atomic number = 12 - 6 = 6 neutrons

4. **Compare the Number of Neutrons:**
- \(_{6}^{14}C\) has 8 neutrons.
- \(_{6}^{12}C\) has 6 neutrons.
- Therefore, the two isotopes differ in the number of neutrons.

5. **Conclusion:**
- The isotopes \(_{6}^{14}C\) and \(_{6}^{12}C\) differ from each other in the number of neutrons.

### Final Answer:
The isotopes \(_{6}^{14}C\) and \(_{6}^{12}C\) differ from each other in the number of neutrons.

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