Isotopes are atoms of the same element that have the same number of protons but different numbers of neutrons. They matter because the atoms of an element in nature are often a mixture of several isotopes, not all identical atoms. The mass listed on the periodic table is usually an average based on that mixture.
Understanding isotopes helps explain atomic mass values, mass spectra, radioactive dating, and many medical and chemical applications.
Average atomic mass is calculated by multiplying each isotope mass by its fractional abundance, then adding the results. A mass spectrum helps show which isotopes are present by displaying peaks at different mass-to-charge values, with peak heights related to abundance. The isotope with the largest abundance contributes the most to the average, but every naturally occurring isotope affects the final value.
This is why chlorine has an average atomic mass near 35.45 amu instead of exactly 35 or 37 amu.
Key Facts
- Isotopes have the same atomic number but different mass numbers.
- Atomic number = number of protons.
- Mass number = protons + neutrons.
- Neutrons = mass number - atomic number.
- Average atomic mass = Σ(isotope mass × fractional abundance).
- Percent abundance must be converted to a decimal before calculating, so 75.0% = 0.750.
Vocabulary
- Isotope
- An isotope is an atom of an element with the same number of protons as other atoms of that element but a different number of neutrons.
- Atomic number
- Atomic number is the number of protons in the nucleus of an atom and identifies the element.
- Mass number
- Mass number is the total number of protons and neutrons in an atom's nucleus.
- Average atomic mass
- Average atomic mass is the weighted average mass of all naturally occurring isotopes of an element.
- Mass spectrum
- A mass spectrum is a graph that shows ions separated by mass-to-charge ratio and often reveals isotope masses and relative abundances.
Common Mistakes to Avoid
- Adding isotope masses and dividing by the number of isotopes is wrong because average atomic mass is a weighted average based on abundance.
- Using percent abundances directly in the equation is wrong because percentages must be converted to decimals before multiplying by isotope masses.
- Confusing atomic number with mass number is wrong because atomic number counts only protons, while mass number counts protons plus neutrons.
- Rounding too early during a calculation is wrong because it can shift the final average atomic mass noticeably, especially when several isotopes are involved.
Practice Questions
- 1 An element has two isotopes: 10.0129 amu at 19.9% abundance and 11.0093 amu at 80.1% abundance. Calculate the average atomic mass.
- 2 Chlorine has two major isotopes: Cl-35 with mass 34.969 amu and 75.78% abundance, and Cl-37 with mass 36.966 amu and 24.22% abundance. Calculate the average atomic mass of chlorine.
- 3 A mass spectrum for an unknown element has one very tall peak at mass 28 and two much smaller peaks at masses 29 and 30. Explain why the average atomic mass would be close to 28 but not exactly 28.