A community for students.
Here's the question you clicked on:
 0 viewing
anonymous
 4 years ago
Naturally occuring boron is 80.20% boron11 (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. :)
anonymous
 4 years ago
Naturally occuring boron is 80.20% boron11 (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

Xishem
 4 years ago
Best ResponseYou've already chosen the best response.1The 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.

anonymous
 4 years ago
Best ResponseYou've already chosen the best response.0Okay, thanks for the help, and equation. :)
Ask your own question
Sign UpFind more explanations on OpenStudy
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
 Engagement 19 Mad Hatter
 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.