2. At the end of the lesson, the learners shall be able to:
1. Define atomic mass unit;
2. Calculate the average atomic mass of elements;
3. Determine the average molecular mass of molecules; and
4. Determine the average formula mass of ionic compounds.
Objectives
22. For carbon, the natural abundance of C-12 is 98.90% while that of C-13 is
1.10%. The atomic
mass of C-13 has been determined to be 13.00335 amu while that of C-12 is
exactly 12 amu.
Now, we calculate the average atomic mass of carbon:
= (atomic mass of C-12) (% abundance of C-12) + (atomic mass of C-13) (%
abundance of C-13)
= (12.0000 amu) (.9890) + (13.00335 amu) (.0110)
= 12.01 amu
23. PRACTICE
EXERCISES:
1. From the periodic table, look up the average atomic mass of the following
elements: Co, Be,
Al, Zn.
2. Copper has two stable isotopes with the following masses and % abundances:
Cu-63 (62.93
amu, 69.09% abundance) and Cu-65 (64.9278 amu, 30.91% abundance).
Calculate the
average atomic mass of copper.
24. PRACTICE
EXERCISES:
3. An element consists of an isotope with mass of 10.0129 amu and 19.91%
abundance, and
another isotope with mass of 11.0093 amu and 80.09% abundance. Calculate the
average
atomic mass of this element. Refer to the periodic table and identify the element.