1 / 3

Subatomic Particles

Subatomic Particles. Calculating Average Atomic Mass. expressed in atomic mass units (amu) done because actual masses so small and hard to work with based on carbon-12 assigned mass of exactly 12 amu weighted average of all naturally occurring isotopes.

ilandere-wauters
Download Presentation

Subatomic Particles

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Subatomic Particles

  2. Calculating Average Atomic Mass • expressed in atomic mass units (amu) • done because actual masses so small and hard to work with • based on carbon-12 assigned mass of exactly 12 amu • weighted average of all naturally occurring isotopes.

  3. change %abundances to decimals for each isotope Multiply abundance by atomic mass of isotope Add products to get average atomic mass for element for 75.77% = 0.7577 for 24.33% = 0.2433 Example Chlorine has two isotopes. The isotope with a mass of 34.969 amu has a relative abundance of 75.77%. The isotope with a mass of 36.966 amu has a relative abundance of24.33%. Calculate the atomic mass of chlorine. x 34.969 = 26.49 amu x 36.966 = 8.994 amu for Cl atomic mass = 35.484 = 35.48 amu

More Related