1 / 10

ISOTOPES!

ISOTOPES!. What is the average number of fingers on one human hand?. Data: 6,000,000 people have 5 fingers, 240,000 people have 4 fingers and 1,800 people have 6 fingers (*NOTE: Mrs. Baker made this data up: I’m sure there are people with 0, 1 & 2 fingers). Review

kenna
Download Presentation

ISOTOPES!

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. ISOTOPES!

  2. What is the average number of fingers on one human hand? Data: 6,000,000 people have 5 fingers, 240,000 people have 4 fingers and 1,800 people have 6 fingers (*NOTE: Mrs. Baker made this data up: I’m sure there are people with 0, 1 & 2 fingers)

  3. Review • All atoms of an element have the same # of protons (EXAMPLE: EVERY SINGLE CARBON ATOM IN THE WORLD HAD 6 PROTONS) • However, atoms of the same element can have different numbers of neutrons • Since mass = p + n, these atoms have different mass numbers

  4. Isotope: An atom with the same number of protons, but a different number of neutrons. C-12 C-13 C-14 12 13 14 C C C 6 6 6 6 p+, 6 n 6 p+, 7 n 6 p+, 8 n 12.011—average atomic mass

  5. How do we measure the mass of a tiny atom? Atomic mass units (amu): The mass of a single atom is called its atomic mass and units are labeled “amu”. 1 amu is = to 1/12 of a carbon atom with a mass # of 12. (6 protons @ 1 amu each + 6 neutrons @ 1 amu each = 12 amu)

  6. 225,000,000,000,000,000,000,000,000 amu = 1 pound!!!!!!!!!!!!!!!!!!!!!

  7. You’ll often see elements written like this: Mass Number 23 Na 11 Atomic number

  8. Naming Isotopes • Scientists usually name isotopes by their mass #. Example: Cobalt-60 (60 = the mass number) You try: Ex #1: How would you write the name and symbol for a neon atom with 10 protons and 11 neutrons? Ex #2: How would you write the name and symbol for an atom with 15 protons and 17 neutrons?

  9. How do you calculate average atomic mass? (atomic mass)(relative abundancy) + (am)(ra) + … Example: Oxygen Oxygen-16 mass = 16, 99.759% Oxygen-17 mass = 16.995, 0.037% Oxygen-18 mass = 17.995, 0.207% (15.995)(0.99759) + (16.995)(0.00037) + (17.995)(0.00207) = 15.99998985

  10. Let’s do a problem! Unknown Element X has 2 isotopes Mass= 12.00000g, 98.89% 13.00335g, 1.11% What is the mystery element X? (12.0000)(0.9889) + (13.00335)(0.0111) 12.011 Carbon

More Related