Download Uncovering the atom

Atoms: discovering the
stuff that stuff is made of
We know all matter is made from elements
What makes each element unique?
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A component unique to each element?
A common component but assembled in a different
way?
Learning Objectives
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Describe what is meant by “atom”
Describe Law of Conservation of Mass and
Definite Proportions
Identify main features of Dalton’s atomic
theory
Describe Avogadro’s Hypothesis
Glimpse into the interior
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What we “see” now
with scanning tunneling
microscope could only
be speculated on 2,000
years ago
The scale of things
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From a distance sand looks smooth and continuous
Up close it’s made of particles
Each particle looks smooth
Up closer it is made of particles - atoms
400 BC
Beginnings of the atom
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Democritus posed the question: could matter be
subdivided forever? He answered no: there is a limit
to the extent to which matter can be subdivided, and
he coined the term atom from the Greek for
uncuttable a-tomos.
Democritus’ idea is not much different from the
modern atom with some modifications...
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Atoms are not uncuttable
Atoms are all very small
Atoms are themselves made of particles
Stop forward movement:
Science in the dark ages
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The decline of Greek civilization saw concomitant decline of
intellectual activity in Europe
Science and maths continued in Persian Empire (golden age)
The major “scientific” activity was alchemy, largely the
pursuit of the transformation of matter into gold and the elixir
of life
Uncritical acceptance of Greek thinking about matter lingered
until the Age of Enlightenmen
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Matter is made of the four elements (earth, wind and fire...and water)
The modern scientific era began in the 17th century, pioneered
by a few inspired individuals who broke free from longestablished conventions
Models for nature were based on observation and experiment
1780
Re-emergence of the atom:
Daniel Bernoulli’s kinetic theory of gases
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Atoms were assumed to be hard round
spheres which behaved much like billiard
balls.
Success of kinetic theory in describing gases
lends support to atomic description of matter.
It is still used, with scarcely any
modification
1790 Order out of chaos
Antoine Lavoisier and the elements
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Beginning of the periodic
table and the concept of
elements
Introduced concept of
compounds – elements
combined
Demonstrated Law of
Conservation of Mass
No additional insights into the
atom at this stage.
Chemical laws and the case for an
atomic world
Law of Conservation of Mass:
Matter is neither created nor destroyed in the course of a
chemical reaction.
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Does not apply to nuclear changes
Law of Definite Proportions:
In forming compounds, elements combine together in
definite mass ratios
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No knowledge of actual atom ratios at this stage, but how
else to explain fixed quantities unless the elements were
present as discrete bodies
Strong indication for combination of the atoms in simple
ratios
1803
John Dalton’s atomic musings
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Sample of any element contains
tiny particles called atoms
Atoms cannot be subdivided,
created or destroyed
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Law of Conservation of Matter
All atoms of the same element are
the same
All atoms of different elements are
different
Atoms combine together in simple
whole number ratios
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Law of Multiple Proportions: The ratio of
the masses of one element combined with
the same mass of another element is a
simple whole number
Significance of the Law of Multiple
Proportions
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With benefit of knowledge of chemical
composition, consider example of carbon
dioxide (CO2) and carbon monoxide (CO)
MassOCO2
MassOCO
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2
Combination of finite components (atoms) of
C and O in simple number ratios is the most
sensible explanation of the Law
1808
Gay-Lussac law of combining
volumes
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Gases react with other gases to give products, in
volumes which have simple whole number ratios.
“Mystery” of the reaction of hydrogen and oxygen to
provide water.
2 vols of hydrogen + 1 vol of oxygen gives 2 vols of
water (Why not 1 vol?)
The ratio of 2:1 was inconsistent with Dalton’s
unproven belief that the formula of water was HO
Mystery of the gas volumes
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Combining H and O in 1:1 ratio (Dalton’s
proposed ratio) does not satisfy Conservation
of Matter…
Needs another box of O atoms
H:O = 2:1
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However, the 2:1 ratio (as suggested by
volume ratio of reactants) predicts only 1 vol
of H2O, not 2 vols as observed…?
Enter Avogadro:
What if they are diatomic molecules?
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Matter conserved, and each volume contains
same number of particles
1811
Amadeo Avogadro’s hypothesis
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Solved riddle of gas volumes by positing
that the molecules in the gas contained
two atoms.
Most elemental gases are diatomic
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The same volumes of all gases contain the
same number of particles.
Results conflicted with Dalton’s views and were
not recognized for nearly 50 years
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Key result: Able to calculate the relative
atomic masses of the elements:
development of a scale of atomic weight.
1815
William Prout: weights of atoms appear to be
simple multiples of hydrogen
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Coincidence or significance?
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Proposed that atoms of heavier elements are made of
hydrogen atoms
Implies that larger atoms comprise smaller units
Partial truth: there are common factors between atoms
of different elements…
but not H atoms…
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Unanswered questions
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What features of the atoms are responsible for
the differences in element properties?
How can atoms actually bind together in
compounds to give substances of different
properties if the atoms cannot be modified
what would the attractive forces be?
What about those other experimental
observations accumulating…?