Discussion Overview
The discussion revolves around calculating the mass of 111 gold atoms and understanding the atomic mass of sulfur (S). It includes questions about the relationship between atomic weight and the number of atoms, as well as the factors contributing to the atomic mass of an element.
Discussion Character
- Technical explanation
- Conceptual clarification
- Debate/contested
Main Points Raised
- One participant suggests multiplying the atomic weight of gold (Au) by 111 to find the mass of 111 gold atoms.
- Another participant counters that the atomic weight is the weight of one mole of gold atoms, indicating that one must first determine how many moles correspond to 111 atoms.
- A participant explains that the atomic mass of sulfur is an average that accounts for different isotopic masses, noting that it includes the mass of protons and neutrons, while the mass of electrons is negligible.
- Several participants emphasize that the atomic mass is an average atomic mass, reiterating its significance in the context of isotopes.
Areas of Agreement / Disagreement
Participants generally agree on the concept that atomic mass is an average and that it includes contributions from isotopes. However, there is some disagreement regarding the method for calculating the mass of 111 gold atoms, with differing interpretations of how to apply atomic weight.
Contextual Notes
There are assumptions regarding the definitions of atomic weight and atomic mass that are not explicitly stated. The discussion also does not resolve the mathematical steps needed to convert between the number of atoms and moles.