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The image shows part of a table with information about isotopes of chlorine. For one isotope, \(\ce{^{37}Cl}\), the mass is 36.966 amu, and the natural abundance is 23.89%. However, the isotope symbol, mass, and natural abundance for the other isotope are missing.

Given that chlorine has two common isotopes, \(\ce{^{35}Cl}\) and \(\ce{^{37}Cl}\), and knowing the general abundance of these isotopes, we can infer the missing information:

1. The other isotope is likely \(\ce{^{35}Cl}\).
2. Its mass is approximately 34.969 amu.
3. The natural abundance is likely around 76.11% (since \(\ce{^{37}Cl}\) makes up 23.89%, and their percentages must sum to 100%).

Would you like me to calculate the weighted average atomic mass of chlorine based on this data? Let me know if you'd like additional details!

Here are five related questions to expand this topic:
1. What is the definition of isotopes, and how do they differ?
2. How is the atomic mass of an element calculated using isotopic abundances?
3. What are some applications of chlorine isotopes in scientific research?
4. How does the natural abundance of isotopes affect chemical reactions?
5. How can the isotopic composition of an element be determined experimentally?

**Tip**: The atomic mass shown on the periodic table is a weighted average of all naturally occurring isotopes of an element.

The image shows part of a table with information about isotopes of chlorine. The isotope \(\ce{^{37}Cl}\) is shown, but the isotope symbol, mass, and natural abundance for the other isotope are missing. The question is to infer the missing isotope's information.

Learn how to calculate the weighted average atomic mass of chlorine using isotopic abundances. This problem involves key concepts like isotopic abundance and the weighted average formula. Suitable for high school students.

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