Average Atomic Mass
Dec 26, 2015
Average Atomic Mass
Isotopes• Atoms of the same element with
different numbers of neutrons.
• Isotopes have the same number of protons, so the atomic number is the same. The atomic mass is different because the neutrons are different.
• Different isotopes of the same element are identified by their atomic mass. (IE: Carbon-12, Carbon-14)
Isotopes
• Because of the existence of isotopes, the mass of a collection of atoms has an average value.
• Average mass = ATOMIC WEIGHT
Example
• Boron is 20% B-10 and 80% B-11. • That is, B-11 is 80 percent abundant on
earth.
• For boron atomic weight= 0.20 (10 amu) + 0.80 (11 amu) = 10.8 amu
Average Atomic Mass
• weighted average of all isotopes• on the Periodic Table• round to 2 decimal places
Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem
Avg.AtomicMass
= (mass)(%) + (mass)(%)
100
Average Atomic Mass
• EX: Calculate the avg. atomic mass of oxygen if its abundance in nature is 99.76% 16O, 0.04% 17O, and 0.20% 18O.
Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem
Avg.AtomicMass
= (16)(99.76) + (17)(0.04) + (18)(0.20)
100= 16.00
amu
Average Atomic Mass
• EX: Find chlorine’s average atomic mass if approximately 8 of every 10 atoms are chlorine-35 and 2 are chlorine-37.
Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem
Avg.AtomicMass
= (35)(8) + (37)(2)
100= 35.40 amu
100
90
80
70
60
50
40
30
20
10
034 35 36 37
Ab
un
dan
ce
Mass
Mass spectrum of chlorine. Elemental chlorine (Cl2) contains only two isotopes: 34.97 amu (75.53%) and 36.97 (24.47%)
AAM = (34.97 amu)(0.7553) + (36.97 amu)(0.2447)
AAM = (26.412841 amu) + (9.046559 amu)
AAM = 35.4594 amu
Cl-35
Cl-37
Cl35.4594
17
Mass Spectrum for Mercury
196 197 198 199 200 201 202 203 204
Mass numberMass number
Rel
ativ
e n
umb
er o
f at
oms
Rel
ativ
e n
umb
er o
f at
oms
30
25
20
15
10
5
196 199 201 204
198 200 202
Mass spectrum of mercury vaporMass spectrum of mercury vapor
The percent natural abundances The percent natural abundances for mercury isotopes are:for mercury isotopes are:
Hg-196 0.146%Hg-196 0.146% Hg-198 10.02%Hg-198 10.02% Hg-199 16.84%Hg-199 16.84% Hg-200 23.13%Hg-200 23.13% Hg-201 13.22%Hg-201 13.22% Hg-202 29.80%Hg-202 29.80% Hg-204 6.85%Hg-204 6.85%
(The photographic record has been converted to a scale of relative number of atoms)
The percent natural abundances The percent natural abundances for mercury isotopes are:for mercury isotopes are:
Hg-196 0.146%Hg-196 0.146% Hg-198 10.02%Hg-198 10.02% Hg-199 16.84%Hg-199 16.84% Hg-200 23.13%Hg-200 23.13% Hg-201 13.22%Hg-201 13.22% Hg-202 29.80%Hg-202 29.80% Hg-204 6.85%Hg-204 6.85%
(0.00146)(196) + (0.1002)(198) + (0.1684)(199) + (0.2313)(200) + (0.1322)(201) + (0.2980)(202) + (0.0685)(204) = x
0.28616 + 19.8396 + 33.5116 + 46.2600 + 26.5722 + 60.1960 + 13.974 = x
x = 200.63956 amu
Hg200.59
80
(% "A")(mass "A") + (% "B")(mass "B") + (% "C")(mass "C") + (% "D")(mass "D") + (% "E")(mass "E") + (% F)(mass F) + (% G)(mass G) = AAM
ABCDEFG
Mass spectrums reflect the abundance of naturally occurring isotopes.
Hydrogen
Carbon
Nitrogen
Oxygen
Sulfur
Chlorine
Bromine
1H = 99.985% 2H = 0.015%
12C = 98.90% 13C = 1.10%
14N = 99.63% 15N = 0.37%
16O = 99.762% 17O = 0.038% 18O = 0.200%
32S = 95.02% 33S = 0.75%
34S = 4.21% 36S = 0.02%
35Cl = 75.77% 37Cl = 24.23%
79Br = 50.69% 81Br = 49.31%
Natural Abundance of Common Elements
Atomic Mass
Calculate the atomic mass of copper if copper has two isotopes. 69.1% has a mass of 62.93 amu and the rest has a mass of 64.93 amu.
... )B"" )(massB"" (% )A"" )(massA"" (% (AAM) massatomic Average
Copper for amu 63.548 A.A.M.
amu 20.06337 amu 43.48463 A.A.M.
amu) .93(0.309)(64 amu) .93(0.691)(62 A.A.M.
Cu29
63.548
IsotopeIsotopePercentPercent
AbundanceAbundanceMassMass
Cu-63 69.1 62.93
Cu-65 64.93
43.48463
20.0633730.9
63.548