A community for students.

Here's the question you clicked on:

55 members online
  • 0 replying
  • 0 viewing

anonymous

  • 4 years ago

Naturally occuring boron is 80.20% boron-11 (atomic mass 11.01 amu) and 19.80% of some other isotope. What must the atomic mass of this second isotope be in order to account for the 10.81 amu average atomic mass of boron? ***NOTE: I will be more than happy if somebody just clarifies the question, I'm not specifically looking for the answer. :)

  • This Question is Closed
  1. Xishem
    • 4 years ago
    Best Response
    You've already chosen the best response.
    Medals 1

    The average atomic mass of an element is found by taking the weighted average of all naturally occurring isotopes. The algorithm will be something like this:\[Avg=(Percent_{} Occurrence)*(Atomic_{}Weight)+(PercentOccurrence)*(AtomicWeight)+...\]Do this for each isotope of the element.

  2. anonymous
    • 4 years ago
    Best Response
    You've already chosen the best response.
    Medals 0

    Okay, thanks for the help, and equation. :)

  3. Not the answer you are looking for?
    Search for more explanations.

    • Attachments:

Ask your own question

Sign Up
Find more explanations on OpenStudy
Privacy Policy

Your question is ready. Sign up for free to start getting answers.

spraguer (Moderator)
5 → View Detailed Profile

is replying to Can someone tell me what button the professor is hitting...

23

  • Teamwork 19 Teammate
  • Problem Solving 19 Hero
  • You have blocked this person.
  • ✔ You're a fan Checking fan status...

Thanks for being so helpful in mathematics. If you are getting quality help, make sure you spread the word about OpenStudy.

This is the testimonial you wrote.
You haven't written a testimonial for Owlfred.