ch. 4.2 - atomic structure i. subatomic particles (p.113 - 114)
TRANSCRIPT
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Ch. 4.2 - Atomic Structure
I. Subatomic Particles(p.113 - 114)
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Subatomic Particle Properties
Particle Symbol Location Charge Relative Mass (amu)
Actual Mass (g)
electron
proton
neutron
e-
p+
n0
Electron cloud
nucleus
nucleus
–
+
0
1/1840
1
1
9.11 x 10-28
1.67 x 10-24
1.67 x 10-24
approx 0
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Symbols
Elements are listed by their chemical symbols
Symbols are usually either one capital letter like C for Carbon, or one capital and one lowercase letter like Ne for Neon
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Periodic Table
The periodic table gives much information we need to learn more about the atom of each element
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Atomic Number
Atomic number = # of protons in an atomWhole number shown on periodic tablePeriodic table is arranged by atomic
number
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Atomic Mass
The average atomic mass is the number at the bottom of this square
Found by averaging the natural abundances of its isotopes
Weighted average
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Atom Math
Atomic Number
Symbol
Element Name
Atomic Mass
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Atom Math
Protons Electrons
Protons Neutrons
# n0 = Atomic mass – Atomic number
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Subatomic Particles
POSIT IVECHARG E
PROT ONS
NEUT RALCHARG E
NEUT RONS
NUCLEUS
NEG AT IVE CHARG E
ELECT RONS
AT OM
Most of the atom’s mass.
NUCLEUS ELECTRONS
PROTONS NEUTRONS NEGATIVE CHARGE
POSITIVE CHARGE
NEUTRAL CHARGE
ATOM
QUARKS#n0 = Atomic mass- Atomic #
equal in a neutral atomAtomic Number
equals the # of...
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Subatomic Particles
Quarks component of
protons & neutrons
6 types
3 quarks = 1 proton or 1 neutron
He
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Ch. 4.3 - Atomic Structure
II. How Atoms Differ (p. 114 - 121) Mass Number Isotopes Relative Atomic Mass Average Atomic Mass
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A. Mass Number
mass # = protons + neutrons
always a whole number
NOT on the Periodic Table!
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B. Isotopes
Atoms of the same element with different numbers of neutrons
C126
Mass #
Atomic #
Isotope notation:
Isotope name: carbon-12
Element name Mass #
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B. Isotopes
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B. Isotopes
Chlorine-37 atomic #:
mass #:
# of protons:
# of electrons:
# of neutrons:
17
37
17
17
20
Cl3717
Isotope notation:
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Natural Abundances of Isotopes
Most elements are found as mixtures of isotopes
Relative abundance of each isotope is the same in each source
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C. Relative Atomic Mass
12C atom = 1.992 × 10-23 g
1 p = 1.007276 amu
1 n = 1.008665 amu
1 e- = 0.0005486 amu
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atomic mass unit (amu)
1 amu = 1/12 the mass of a 12C atom
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D. Average Atomic Mass
weighted average of all isotopeson the Periodic Tableround to 2 decimal places
100
(%)(mass(mass)(%) )
Avg.AtomicMass
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Avg.AtomicMass
D. 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.
100
(18)(0.20)(17)(0.04))(16)(99.76 16.00amu
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Avg.AtomicMass
D. 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.
100
(37)(20)(35)(80)35.40 amu