1 Mr. ShieldsRegents Chemistry U01 L05 2 Atomic Mass Up to now we discussed Atomic mass number in...
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Transcript of 1 Mr. ShieldsRegents Chemistry U01 L05 2 Atomic Mass Up to now we discussed Atomic mass number in...
![Page 1: 1 Mr. ShieldsRegents Chemistry U01 L05 2 Atomic Mass Up to now we discussed Atomic mass number in terms of The Number of Neutrons and Protons Ex. 8p.](https://reader035.fdocuments.us/reader035/viewer/2022062721/56649f1c5503460f94c321ed/html5/thumbnails/1.jpg)
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Mr. Shields Regents Chemistry U01 L05
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Atomic MassAtomic Mass
Up to now we discussed Atomic mass number in terms ofThe Number of Neutrons and Protons
Ex. 8p + 9n = atomic mass number 17
But mass should tell us how much matter is present.
What does “17” really tell us about how much matter(mass) is present?
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Atomic MassAtomic Mass
Remember - Neutrons and Protons DON’T reallyHave the same mass.
Mass of a Proton = 1.6726 x 10-24 gramMass of a Neutron = 1.6749 x 10-24 gram
So a neutron is really a little heavier than a Proton.So what’s the implication?
If I have 19 neutrons and 19 protonsin a nucleus it DOES NOT have exactly the same mass asA nucleus with 21 neutrons and 17 protons even thoughThe stated mass number is the same (38)
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Atomic MassAtomic Mass
Let’s look at the mass of one of the isotopes of Carbon.
Carbon-12: 6 protons + 6 neutrons
6p x (1.6726 x 10-24) + 6 x (1.6749 x 10-24) grams1 atom of carbon-12 = 2.00850 x 10-23 grams
But this is an “awkward” number to work with
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Atomic Mass UnitsAtomic Mass Units
Instead of actual weights in grams Scientist use a unit called an ATOMIC MASS UNIT
- Abbreviated “AMU”
Scientist decide NOT to base theAMU on either the proton or neutron
Instead an arbitrary “Standard” was chosen
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Atomic Mass UnitAtomic Mass UnitThe “Standard” they chose was an isotope of Carbon
- Carbon-12 (REMEMBER THIS!!)
The mass of CARBON-12 wasdefined to be EXACTLY equal to12 AMU’s
In other words 1 AMU EQUALS 1/12 the mass of aCarbon-12 Atom
1 AMU is slightly less than the mass of either aneutron or a proton
- 1 AMU = 1.661 x 10-24 g
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AMU’sAMU’s
For example here’s some examples of AMU’s vs Mass No.
Atomic Mass in AMU’s Mass #Proton 1.007825 1Carbon-12 12.00000 12Oxygen-16 15.994915 16Magnesium-25 24.985837 25Nickel-60 59.930791 60Uranium-235 235.043925 235
EXCEPT for Carbon-12 the MASS of an atom in AMU’s is NEVER EXACTLY the same as it’s MASS NUMBER
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Isotopic Abundance/CompositionIsotopic Abundance/CompositionIn nature an element may have several
isotopes
Isotopes have a specific percentcomposition no matter where thesample is collected on earth.
For example, oxygen in the air we breath has this composition:
% AMUOxygen-16 99.76% 15.994915Oxygen-17 0.038% 16.999132Oxygen-18 0.200% 17.999160
Total: 100.00%
liquid
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Relative AbundanceRelative AbundanceThese %’s are known as The “Relative Abundances” of the isotope.
In our example of Oxygen the Average AMU’s of a sample ofOxygen must be between 15.994915 and 17.999160. Why?
The AVERAGE MASS of all the elements isotopes is calledthe ATOMIC MASS or the ATOMIC WEIGHT
THIS IS DIFFERENT THAN ATOMIC Mass Number
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Isotopic CompositionIsotopic CompositionSo how do we calculate Atomic Mass?
Well it’s simply a weighted average.
Since we’re considering Oxygen ….
Rel Abundance AMUOxygen-16 99.762% 15.994915Oxygen-17 0.038% 16.999132Oxygen-18 0.200% 17.999160
total: 100%
So, What is the Atomic Mass for Oxygen?
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Isotopic CompositionIsotopic Composition
i.e. (Mass x abundance) + (mass x Abundance) etc.
(.9976 x 15.994915) + (.00037 x 16.999132) + (.00204 x 17.999160) =
(15.956527) + (0.006290) + (0.036718) = 15.9995
LOOK AT OXYGEN’S MASS ON THE PERIODIC TABLE.
Is it pretty close to our answer ?
Remember: the Atomic mass is the Avg. Atomic mass of all the elements isotopes & we need to use a weighted avg. to Calculate it.
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Estimating Atomic MassEstimating Atomic MassLook at our Calculated average Atomic Mass of Oxygen(15.9995) and the relative abundance of the isotopesOf Oxygen.
Abundance AMUOxygen-16 99.762% 15.994915Oxygen-17 0.038% 16.999132Oxygen-18 0.200% 17.999160
Could you guess what the Calculated Atomic mass would beClose to?
Which isotope is present in the greatest amount?
Isn’t it’s mass pretty close to the calculated value?
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Estimating Atomic MassEstimating Atomic Mass1. In the following problem which isotope will have a massClosest to the actual atomic mass?
2. Calculate the atomic mass of Chlorine (Assume these values are correct though they are not)
Abundance AMUChlorine-35 70% 35.0Chlorine-37 30% 37.0
1. Chlorine 352. (0.70 x 35) + (0.30 x 37) = 24.5 + 11.1 = 35.6 AMU