Step 3. Add the masses contributed by each isotope. 20.2 amu Atomic mass = 18.1

Question

Step 3. Add the masses contributed by each isotope. 20.2 amu Atomic mass = 18.1 amu + 0.057 amu + 2.04 amu This value is also close to the atomic mass of neon provided on the periodic table, 20.18 amu. Practice Problem 2.3 Calculate the atomic mass of naturally occurring boron if 19.9% of the boron atoms are 1 and 80.1% are 11 B. Helpful Hint: The calculated value of 20.2 amu is slightly greater than the mass of the most abundant isotope. For Further Practice: Question 2.38. 2.2 Development of Atomic Theory LEARNING GOAL Summarize the history of the development of atomic theory beginning with Dalton. With this overview of our current understanding of the structure of t now look at a few of the most important scientific discoveries tha atomic theory 4 or Dalton's Theory The first experimentally based theory of early 1800s by John Dalton, glish sch ing description of atoms: 1. All matter consists 2. An atom cannot be ticles divid o any o type of atom 3. Atoms of a parti 4. Atoms of differe

Explanation / Answer

Problem 2.3 -

This is problem based on average atomic weight.

So, in order to calculate it, each exact atomic mass is multiplied by its % abundance. Then, add the results together to get the your average atomic mass, ie

Average atomic mass = atomic mass of isotope 1 x % abundance + atomic mass of isotope 2 x % abundance

Or, average atomic mass = 10 x (19.9/100) + (11 x 80.1/100)

Average atomic mass = 10.801 amu

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