Name the subatomic particles, charges, location, and mass. Bellwork 8.
1.3 Understanding Atomic Mass. A Review: Subatomic particles Electron Proton Neutron...
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![Page 1: 1.3 Understanding Atomic Mass. A Review: Subatomic particles Electron Proton Neutron NameSymbolCharge Relative mass Actual mass (g) e-e- p+p+ nono +1.](https://reader036.fdocuments.net/reader036/viewer/2022062322/56649e9f5503460f94ba1db4/html5/thumbnails/1.jpg)
1.3 Understanding Atomic Mass
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A Review: Subatomic particles
Electron
Proton
Neutron
Name Symbol ChargeRelative mass
Actual mass (g)
e-
p+
no
-1
+1
0
1/1840
1
1
9.11 x 10-28
1.67 x 10-24
1.67 x 10-24
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Structure of the Atom
There are two regions:
1. The Nucleus: • With protons and neutrons• Positive charge• Almost all the mass
2. Electron cloud• Most of the volume of an atom• The region where the electrons can be found
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If the atom was the size of a stadium,
the nucleus would be the size of: a marble.
http://www.andrew.cmu.edu/user/jgrao/Manchester%20United/giant%20stadium.jpg
http://www.akronmarbles.com/marble-frag-2.jpg
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Standard Atomic Notation
Includes the symbol of the element, the mass number and the atomic number
X Massnumber
Atomicnumber
# protons
# protons + # neutrons mass number
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• Find the – number of protons– number of neutrons– number of electrons– Atomic number– Mass number
F19 9
= 9
= 10
= 9
= 9
= 19
+
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http://chemistry.beloit.edu/Stars/EMSpectrum/fluorine.gif
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Find the – number of protons– number of neutrons– number of electrons– Atomic number– Mass number Br80
35
= 35
= 45
= 35
= 35
= 80
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Find the – number of protons– number of neutrons– number of electrons– Atomic number– Mass number
Na2311
1+
Sodium ion
= 11
= 12
= 10
= 11
= 23
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http://www.webelements.com/webelements/elements/media/nearingzero/Na.gif
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http://discover.edventures.com/images/termlib/i/isotope/support.gif
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Isotopes• Atoms of the same element can have
different numbers of neutronsThis gives them different mass
numbers.They have the same atomic numbers.They look, act and react the same.
C-12 vs. C-14
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Isotopes of Hydrogen
1 p+ 1 e-1 p+
1 n 1 e-1 p+2 n 1 e-
Protium Deuterium Tritium
(ordinary hydrogen) (heavy hydrogen) (radioactive hydrogen)
H11
H21
H31
Ralph A. Burns, Fundamentals of Chemistry 1999, page 100
H-2 H-3H-1
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Isotopes of Hydrogen
•• ProtiumProtium (H-1)1 proton, 0 neutrons, 1 electronMost abundant isotope
•• DeuteriumDeuterium (H-2)1 proton, 1 neutron, 1 electronUsed in “heavy water”
•• TritiumTritium (H-3)1 proton, 2 neutrons, 1 electronradioactive
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Naming Isotopes
• Put the mass number after the name of the element
• Examples:
• Carbon-12 and Carbon-14
• Uranium-235 and Uranium-238
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Isotopes of Three Common Elements
92.21%
4.70%
3.09%
27.977
28.976
29.974
28
29
30
Si
Si
Si
Silicon
Chlorine
Carbon
Average Atomic Mass
Fractional AbundanceSymbolElement
126
136
3517
3717
2814
2914
3014
12.01
35.45
28.09
1.11%13.00313C
99.89%12 (exactly)12C
Mass (amu)
75.53%
24.47%36.96637Cl
34.96935Cl
Mass
Number
LeMay Jr, Beall, Robblee, Brower, Chemistry Connections to Our Changing World , 1996, page 110
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Which isotopes are represented in this sketch?
http://discover.edventures.com/images/termlib/i/isotope/support.gif
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Calculations of Average Atomic Mass
Why is the mass number on a periodic table never a nice whole
number?
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Mass Number vs AverageAtomic Mass
• The Mass Number is specific to one isotope.
• The Average Atomic Mass is the calculated based on the abundance of each naturally occurring isotope of that element.
• The Average Atomic Mass is shown on Periodic Tables.
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Average Atomic Mass• How heavy is an atom of oxygen?• There are different kinds of oxygen atoms.
oxygen-16, oxygen-17 and oxygen-18
• We are more concerned with average atomic mass, based on the abundance of each element in nature.
• We don’t use grams because the numbers would be too small.
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Atomic Mass Unit (amu or u)
• This unit is used instead of grams.
• It is 1/12 of the mass of a carbon-12 atom.
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Radioactive Isotopes
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• Radioactive: – Capable of spontaneously emitting radiation in
the form of particles and/or gamma rays
• Radioisotope:– A radioactive isotope of an element that occurs
naturally or is produced artificially.
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Radioisotopes• Many elements have one or more isotopes
that are unstable. • Atoms of unstable isotopes decay, emitting
radiation as their nucleus changes.• The changes can happen quickly or slowly,
depending on the isotope.• Radiation emitted can be harmless or very
dangerous to living cells.
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Applications of Nuclear Science
Radiology:Anthropology:
Nuclear Reactors:http://blogs.warwick.ac.uk/images/flingard/2004/11/08/carbon_dating.jpg
http://www.johnharveyphoto.com/RoadTrip/NuclearReactor.jpghttp://mednews.stanford.edu/story_images/radiology-xray-051805.jpg
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Radioisotopes
• Radioactive isotopes• Many uses
– Medical diagnostics– Optimal composition of
fertilizers– Abrasion studies in engines
and tires Radioisotope is injected into the bloodstream toobserve circulation.
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