Gallium has two naturally occurring isotopes, \[\ce{Ga-69}\] and \[\ce{Ga-71}\]. The average atomic mass of gallium is \[\pu{69.72 u}\].

**Which pie chart best shows the relative abundances of the two isotopes in nature?**

Choose 1 answer:

Choose 1 answer:

(Choice A)   

Ga-69Ga-71

A

Ga-69Ga-71

(Choice B)   

Ga-69Ga-71

B

Ga-69Ga-71

(Choice C)   

Ga-69Ga-71

C

Given that gallium has two naturally occurring isotopes, \(\ce{Ga-69}\) and \(\ce{Ga-71}\), with an average atomic mass of \(\pu{69.72 u}\), we can infer the relative abundances of these isotopes.

Since the average atomic mass (\(\pu{69.72 u}\)) is closer to the atomic mass of \(\ce{Ga-69}\) (around \(\pu{68.93 u}\)) than to \(\ce{Ga-71}\) (around \(\pu{70.92 u}\)), it indicates that \(\ce{Ga-69}\) is more abundant than \(\ce{Ga-71}\).

Therefore, the correct pie chart should show that \(\ce{Ga-69}\) has a larger portion compared to \(\ce{Ga-71}\). The answer corresponds to:

**Choice C** - The pie chart where the segment representing \(\ce{Ga-69}\) is larger than that of \(\ce{Ga-71}\).

Would you like further details or have any other questions?

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Here are 5 related questions you might find interesting:

1. How do isotopic abundances affect the calculation of average atomic mass?
2. Why is the average atomic mass of gallium closer to \(\ce{Ga-69}\) than \(\ce{Ga-71}\)?
3. What are the exact isotopic masses of \(\ce{Ga-69}\) and \(\ce{Ga-71}\)?
4. How can you experimentally determine the relative abundances of isotopes?
5. What is the significance of isotopic abundance in chemistry and material science?

**Tip:** When analyzing average atomic mass, the closer the average is to an isotope's mass, the more abundant that isotope is.

Explore the concept of isotopes in gallium and how average atomic mass is calculated. Learn why the average atomic mass of gallium is closer to Ga-69 than Ga-71, based on their isotopic abundances. Suitable for high school students studying chemistry.

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