🤓 Based on our data, we think this question is relevant for Professor Enderle's class at UCD.

**Isotopes** represent atoms of an element that contain the **same atomic number** (same number of protons), but **different mass numbers** (different number of neutrons).

a. ^{35}**Cl is more abundant**

b. The average atomic mass of Cl is 35.45 amu.

Since **35.45 amu is closer to the mass of ^{35}Cl (35 amu)** than

We’re being asked to **percent ^{37}Cl**. We can use the following equation:

$\overline{){\mathbf{Atomic}}{\mathbf{}}{\mathbf{Mass}}{\mathbf{}}{\mathbf{=}}{\mathbf{}}{\left[\mathbf{mass}\mathbf{\times}\mathbf{f}\mathbf{.}\mathbf{a}\mathbf{.}\right]}_{\mathbf{isotope}\mathbf{}\mathbf{1}}{\mathbf{+}}{\left[\mathbf{mass}\mathbf{\times}\mathbf{f}\mathbf{.}\mathbf{a}\mathbf{.}\right]}_{\mathbf{isotope}\mathbf{}\mathbf{2}}}$

where atomic mass = average atomic mass of the element and f.a. = fractional abundance of the isotope.

Chorline exists mainly as two isotopes ^{35}Cl and ^{37}Cl,

a) Which is more abundant?

b) How do you know?

c) Compute the percentage of chlorine that is the ^{37}Cl isotope.

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Isotopes concept. You can view video lessons to learn Isotopes. Or if you need more Isotopes practice, you can also practice Isotopes practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Enderle's class at UCD.