Question

The Periodic Table Online Practice
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Question
Suppose that hypothetical element Jovian occurs as three isotopes with mass numbers 44, 46, and 48 respectively. If, in nature, Jovian occurs as Jovian-44 approximately 22.4% of the time, and as Jovian-46 approximately 44.0% of the time, what is the best value to use as the atomic mass of Jovian?(1 point)
Responses

46.0 amu
46.0 amu

30.1 amu
30.1 amu

39.0 amu
39.0 amu

46.2 amu

Answer 1

To find the atomic mass of the hypothetical element Jovian, we need to take a weighted average of its isotopes based on their natural abundances.

The information provided is as follows:
- Jovian-44: 22.4% abundance
- Jovian-46: 44.0% abundance
- Jovian-48: The remaining percentage, which we can calculate as:
\[
100\% - (22.4\% + 44.0\%) = 100\% - 66.4\% = 33.6\%
\]

Now we have:
- Jovian-44: 22.4% or 0.224
- Jovian-46: 44.0% or 0.440
- Jovian-48: 33.6% or 0.336

Next, we calculate the weighted average using the formula:
\[
\text{Atomic mass} = (0.224 \times 44) + (0.440 \times 46) + (0.336 \times 48)
\]

Calculating each term:
1. \(0.224 \times 44 = 9.856\)
2. \(0.440 \times 46 = 20.240\)
3. \(0.336 \times 48 = 16.128\)

Now, summing these values:
\[
\text{Atomic mass} = 9.856 + 20.240 + 16.128 = 46.224 \, \text{amu}
\]

Rounding this value, the best estimation for the atomic mass of Jovian is approximately \(46.2 \, \text{amu}\).

So, the correct answer is:
**46.2 amu**