Average Atomic Mass - Evan's Regents Chemistry Corner
Chemistry: Form Ls2.4A
Name ______________________________
ATOMS
Date _________________ Period _____
Average Atomic Mass
Aim
?
to calculate the average mass of an element
Notes
Atomic mass
n The relative mass of an atom is the sum of its protons and neutrons
q Examples
p Carbon 12 has 6 protons and 6 neutrons (6 + 6 = 12)
p Carbon 14 has 6 protons and 8 neutrons (6 + 8 = 14)
q The relative mass of any isotope is an integer
Average atomic mass
n The masses of the elements listed on the Periodic Table are not integers
n The masses of the elements listed on the Periodic Table are the average masses of the isotopes of each element
q The average mass of an element is a weighted average
q Both the mass of the isotopes and the percentage of each effect the average mass
p Procedure
o The percentage, expressed as a decimal, is multiplied by the mass to get the product
o The products are added together to get the total
n
x AVG =
¡Æp
y =1
y
x y = p1 x1 + p2 x 2 + K+ pn x n
p Example
Average Mass of Nitrogen
Isotope
Nitrogen-14
Nitrogen-15
Percentage
0.9963
0.0037
Mass
14
15
Product
13.95
0.06
14.01
Answer the questions below by circling the number of the correct response
1. The common isotopes of hydrogen have masses of 1 amu, 2amu,
and 3 amu. The average atomic mass of hydrogen is 1.00794
amu. This shows that the most common isotope has a mass of
(1) 1 amu, (2) 2 amu, (3) 3 amu, (4) 4 amu
3. A new element, unbiennium, has been synthesized. A typical
sample contains 22.50 percent Ube¨C323 and 77.50 percent
Ube¨C325. What is the average mass? (1) 324.6 amu
(2) 323.4 amu (3) 324.0 amu (4) 325.2 amu
2. Chlorine occurs naturally as two common isotopes, 35Cl and 37Cl.
Which of the following percentages results in the average mass of
about 35.5 amu? (1) 20 percent 35Cl and 80 percent 37Cl (2) 50
percent 35Cl and 50 percent 37Cl (3) 75 percent 35Cl and 25
percent 37Cl (4) 85 percent 35Cl and 15 percent 37Cl
? Evan P. Silberstein, 2002
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