introduction to chemistry for allied health sciences structure of the atom kirk hunter chemical...
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![Page 1: Introduction to Chemistry for Allied Health Sciences Structure of the Atom Kirk Hunter Chemical Technology Department Texas State Technical College Waco](https://reader036.vdocument.in/reader036/viewer/2022082422/56649dbf5503460f94ab36e5/html5/thumbnails/1.jpg)
Introduction to Chemistry
for Allied Health Sciences
Structure of the Atom
Kirk HunterChemical Technology Department
Texas State Technical College Waco
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Structure of the Atom
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Subatomic Particles
Name Relative Relative Mass (amu)
ChargeProton 1 +1Neutron 1 0Electron 0 -1
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ATOMThe protons and
neutrons are located in the
center in the region called the nucleus.
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ATOMElectrons are found around the nucleus in shells or principle energy levels (PEL).
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ATOMIC NUMBER
The number of protons in the nucleus of an atom
Z = #p
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ATOMIC NUMBER
For a neutral atom, the number of protons is equal to the number of electrons.
#p = #e
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MASS NUMBERThe sum of protons and
neutrons in the nucleus of an atom.
A = #p + #n
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MASS NUMBERRound the atomic
weight to the nearest whole numberElement Atomic Mass Mass
Number
Li 6.941
Ca 40.078
B 10.81
Au 196.9665
7
41
11
197
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Isotopic Notation
A = mass number E = symbol of element
Z = atomic number
EA
Z
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Isotopic Notation
Example:Determine the number of protons, electrons and neutrons in 51
23V.
Solution:
# p = 23
# e- = 23
# n = 51 - 23 = 28
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Isotopic NotationExample:Determine the number of protons,
electrons and neutrons for the following:
147
N 23892U 23
11Na 20080Hg
#p#e- #n
777
9292146
111112
8080120
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Isotopes• Around 20 elements have a fixed
number of neutrons.• Atoms of the same element having
a different number of neutrons are called isotopes.
Isotopes have the same number of protons and a
different number of neutrons.
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Isotopes of Hydrogen
11H 2
1H 31H
Protium Deuterium Tritium p+ 1 1 1 n0 0 1 2 e- 1 1 1
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Isotopes of Helium
32He 4
2He
p+ 2 2 n0 1 2 e- 2 2
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Isotopes of Oxygen
168O 17
8O 188O
p+ 8 8 8 n0 8 9 10 e- 8 8 8
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ATOMIC MASS UNIT• Carbon-12 used as the reference
standard.• All atoms are compared to C-12.
1 amu = 1/12 the mass of a C-12 atom.
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ATOMIC MASS The average mass of all isotopes of the element.
–exact mass of each isotope
–percent abundance of each isotope in nature
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ATOMIC MASSExample:
Determine atomic mass of vanadium.
Isotope exact mass % abundance51V 50.9876 amu 35.64%52V 51.9346 amu 64.36%
At.wt.=(50.9876 *0.3564) + (51.9346 * 0.6436)
= 18.17+33.43
= 51.60 amu
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ATOMIC MASSExample:
Determine atomic mass of silicon.
Isotope exact mass % abundance
26Si 25.9854 amu 5.435%28Si 27.9721 amu 76.42%29Si 28.9632 amu 18.15%
At.wt. = (25.9854*0.05435)+(27.9721*0.7642) +(28.9632*0.1815) = 28.05 amu