What particles determine the mass of an isotope? Do all atoms of the same element have the same mass? Look at the periodic symbol for potassium, which number represents atomic mass... What particles determine the mass of an isotope? Do all atoms of the same element have the same mass? Look at the periodic symbol for potassium, which number represents atomic mass? If atomic mass is just protons + neutrons, how do we get a decimal? What is average atomic mass? What does abundance refer to, and how is relative abundance determined using mass spectrometry?
Understand the Problem
The question is asking about concepts related to average atomic mass and mass spectrometry, including the definition of isotopes, how atomic mass is determined, and the role of mass spectrometry in measuring isotopic abundance. It also implies a need for clarification on specific definitions and functions involved.
Answer
Protons and neutrons determine isotope mass; isotopes cause mass differences; potassium's atomic mass is 39.098; mass is a decimal because it's an average; average atomic mass considers isotopes and abundances, measured by mass spectrometry.
The final answer is: Protons and neutrons determine the mass of an isotope; atoms of the same element can have different masses due to isotopes; on the periodic table for potassium, 39.098 represents atomic mass; atomic mass has a decimal because it's an average; average atomic mass is the weighted average of all isotopes’ masses; abundance refers to how common an isotope is, determined using mass spectrometry.
Answer for screen readers
The final answer is: Protons and neutrons determine the mass of an isotope; atoms of the same element can have different masses due to isotopes; on the periodic table for potassium, 39.098 represents atomic mass; atomic mass has a decimal because it's an average; average atomic mass is the weighted average of all isotopes’ masses; abundance refers to how common an isotope is, determined using mass spectrometry.
More Information
Average atomic mass reflects the naturally occurring distribution of isotopes. Potassium has multiple isotopes contributing to this weighted average.
Tips
A common mistake is confusing atomic mass with mass number (mass number is whole, whereas atomic mass is a weighted average).
Sources
- Atomic number, atomic mass, and isotopes (article) - Khan Academy - khanacademy.org
- 1.7: Isotopes and Atomic Masses - Chemistry LibreTexts - chem.libretexts.org
- Atomic Mass - Chemistry - Socratic - socratic.org
