atomic structure the periodic table, isotopes, and average atomic mass
TRANSCRIPT
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Atomic Structure
The Periodic Table, Isotopes, and Average
Atomic Mass
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Atomic Number
• Number of protons in an atom
• Periodic table is arranged by increasing atomic number
• The number of electrons in a neutral atom equals the number of protons in that atom
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Reading the Periodic Table
H
Hydrogen
1
1.008
Element Name
Atomic Number
Symbol
Atomic Mass (amu)
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Mass Number
• Sum of protons and neutrons in an atom
NOT THE SAME AS ATOMIC MASS!
H
Hydrogen
1
1.008
Cannot be found on periodic table
NO NO NO NO NO!!!!
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6
CCarbon12.011
Atomic Number
ElementSymbol
ElementName
Atomic Massround this off
to get Mass Number
Reading the Periodic Table
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Reading the Periodic Table
Number of:
Protons = Atomic Number
Neutrons = Mass Number – Atomic Number
Electrons = Atomic Number
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Wrap-Up 1
• Which of the following can be found on a periodic table?
1) Atomic number
2) Atomic mass
3) Mass number
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What’s in a cheeseburger?
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Isotope• Atoms with same number of
protons, but different number of neutrons
HYDROGEN - 1 HYDROGEN - 2 HYDROGEN - 3
= neutrons
= protons
= electrons
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3 Different Hydrogen Isotopes
HYDROGEN – 1(protium)
1 proton0 neutrons1 electron
HYDROGEN – 2(deuterium)
HYDROGEN – 3(tritium)
1 proton1 neutron1 electron
1 proton2 neutrons1 electron
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Ways to Write Isotopes
1) Hyphen notation (2 parts)
name of element – # OR symbol – #
ex: carbon-14 OR C-14 chlorine-35OR Cl-35 hydrogen-3 OR H-3
MASSNUMBER
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Ways to Write Isotopes
2) Nuclear symbol (3 parts)
C14
6
elementsymbol
mass number
atomic number
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Ex problem
K
Potassium
19
39.10
# protons
# neutrons
# electrons
Nuclearsymbol
Potassium-39 Potassium-40 Potassium-41
19
19
1919
19
2220 21
19
K KK39
19
41
19
40
19
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Wrap Up 2
• There are three common isotopes of carbon. The most prevalent has a mass of 12 amu. The other two have masses of 13 amu or 14 amu. Write the nuclear symbols for all three of these carbon isotopes.
CCC 146
136
126
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Mass of Individual Atoms
• Atoms have extremely small masses (~1×10-27 kg)
• Instead we use a relative mass – atomic mass unit (amu)
• 1 amu ≈ mass of 1 proton or 1 neutron
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Comparing Subatomic Particles
particle Mass (amu)
e-
p+
n0
0.000549
1.007276
1.008665
0
1
1
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Atomic Mass
• Weighted average mass of all isotopes of an element
• Where can it be found found on periodic table?
K
Potassium
19
39.10
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Example: calculate atomic mass of chlorine
Isotope mass (amu) percent abundance
35Cl 35 75.770%37Cl 37 24.230%
amu
amuamu
amuamu
485.35
965.8520.26
24230.03775770.035
decimal as %isotopeisotope of mass mass Atomic
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Which isotope is most abundant?Ar-38, Ar-40, or Ar-41?
Ar
Argon
18
39.948
Ar-40