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8/14/2019 Dev Elopement of Atomic Theory
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TheThe
DevelopmenDevelopmen
t of Atomict of Atomic
TheoryTheory
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TheoryTheory
Unit 1 ExamUnit 1 Exam
ResultsResults
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Remember our Atomic HistoryRemember our Atomic History
Time LineTime Line
450 BCE - Democritus
First posed idea that
matter is made of
indivisible particles called
atoms
Started with the Greeksthen
nothing for a long
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long,
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long time
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until
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1780s Antoine
Lavoisier
proposed the law of
conservation of mass:
matter is neither
created nor destroyed
1790s Joseph Louis
Proustfound that a compound
always has the same
composition regardless of
where it is found
1770s Ben
FranklinExperimented with
electricity and
labeled the charges
+ and -
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1800s John Dalton
Combined Democritus,
Lavoisier and Prousts
theories into a unified
atomic theory of matter
1890s Henri Becquerel, Marie
and Pierre Curie
Discovered radioactivity and
proved that the atom is not the
smallest unit of matter
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1910s Robert Millikan
Measured the charge on the
electron using the oil can
experiment.
1890s JJ Thomson
Discovered that cathoderays were actually
electrons, the negative
particles Franklin saw
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1910s Henry Moseley
Found that each element hasa unique number of positive
charges (protons) and
therefore atomic number
1900s Ernest Rutherford
shot a particles at a thin goldfoil to discover that most of
the mass of an atom (the
nucleus) takes up very little
space
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Law of Conservation ofLaw of Conservation of
MassMass
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Law of DefiniteLaw of Definite
ProportionsProportions Discovered by a Frenchman, Joseph Proust (1754 1826). Sometimes known as Prousts Law. Each compound has a specific ratio of elements
It is a ratio by mass. Water is always 8 grams of oxygen for each 1 gram
of hydrogen
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The Law of Multiple ProportionsThe Law of Multiple Proportions
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Say What?Say What?
Water is 8 grams of oxygen per 1 gram ofhydrogen.
Hydrogen Peroxide is 16 grams of oxygen per
gram of 1 hydrogen. The ratio of Oxygen to hydrogen is 16 to 8 or
a 2 to 1 ratio
True because you have to add a whole atom,
you cant add a piece of an atom.
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Daltons AtomicDaltons Atomic
TheoryTheory
Thus, armed with the Law of Conservation of Mass,
The Law of Definite & Multiple ProportionsDaltonoutlined five fundamental postulates about atoms:
1. All matter consists of tiny, indivisible particles,
which Dalton called atoms that cannot be broken downor destroyed.
2. All atoms of a particular element are exactly alike,
but atoms of different elements are different.3. All atoms of different elements are unchangeable and
have different physical and chemical properties.
l iD lt At i
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4. Atoms of elements combine to form"compound atoms" (i.e., molecules) of
compounds in simple whole-number ratios.
5. In chemical reactions, atoms are neither
created nor destroyed, but are only
rearranged.
Daltons AtomicDaltons Atomic
TheoryTheory
Hurray!
Were Saved!
Oh, thank
youDalton!
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Random ThoughtsRandom Thoughts
Using similar reasoning techniques for othercompounds, Dalton prepared the first table of
atomic masses (sometimes called atomic weights
by chemists since masses are obtained by
weighing).
His work paved the way for other scientists such
as Joseph Gay-Lussac (1778 1850) and Amadeo
Avogadro (1776 1856) to continue research thatwill be presented in class when we reach the Gas
Laws Unit.
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Percent CompositionPercent Composition
The percentage by mass of each element in
a compound.
If a sample of water contains 2 grams ofhydrogen to 16 grams of oxygen, the
percent composition of oxygen will always
be approximately 89%, or 16 gramsoxygen/18 grams total. Hydrogen would
account for about 11%.
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The End!The End!