Atomic Structure. The Atoms Family Atom: the smallest part of an element. Name means “indivisible”
Early Ideas about Matter. atom u The smallest piece of the element with all the chemical properties...
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Early Ideas about Matter
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atom
The smallest piece of the element with all the chemical properties of the element
an old and new idea
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GreeksDiscontinuists
–DemocritusContinuists
–Aristotle
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Discontinuists Democritus Believed there was a smallest
piece “atomos” = indivisible
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Continuists Continuists thought there
was no “smallest piece” they believed a bar of gold,
for example, could be cut into smaller pieces forever
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Aristotle’s ideas
There are four elements–earth, air, fire, and water
all matter is composed of these four elements in different proportions
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The Alchemists Tried to turn lead into gold
–put more fire into it–the “medicine stone” would
“cure” the Pb developed many lab techniques
and apparatus
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The Renaissance A new approach to science experiment to test if the
hypothesis is true many of Aristotle’s ideas were
shown to be wrong
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Law of Conservation of Mass
Lavoisier> France, 1790’s Matter (or mass) is neither created
nor destroyed in an ordinary chemical reaction
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Lavoisier did three important things:1. brought in an entire new language for chemistry
2. established the correct identity of the elements and distinguished them from compounds, showing that those are combinations of elements
3. introduced the art of precise measurements. He turned chemistry into a physical science and
can properly regarded as the father of modern chemistry.
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Law of Definite Proportions
In a given compound, elements are always combined in the same proportion by mass.
Ex: H2O is always 11% H, 89% O by mass.
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Dalton’s Atomic Theory All matter is composed of atoms
– atoms are indestructible
– “billiard ball” model In a chemical reaction,
atoms are rearranged– conservation of mass
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All atoms of the same element are identical
Atoms of one element are different from the atoms of any other element–elements could be identified and
distinguished from each other
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Atoms combine to form compounds in small whole number ratios.–Ex: could be XY, X2Y, XY2, etc, but never X11/2Y
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What came next? 49 new elements were discovered
between 1801 - 1900 new particles were discovered
– alpha, beta, gamma - radiation
– particles smaller than atoms
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1897: JJ Thomson discovered electrons– smaller than atoms
– negatively chargedRobert Millikan
– problem with Dalton’s model
1914 Rutherford’s Gold Foil Experiment– nuclear model of atom
http://www.shsu.edu/~chm_tgc/sounds/pushmovies/
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Gold Foil experiment setup
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Gold Foil Experiment - results
http://www.chemsoc.org/timeline/pages/1911.html
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• The repulsive force between the positively charged nucleus and positive alpha particles caused the deflections.
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Modern atom Nucleus
– in geometric center of the atom
– very small and dense
– nearly all of the atom’s mass
– gives the atom its identity
– protons (+) and neutrons
– Nucleus held together by the “strong force”
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Electron cloud–gives the atom its size
–mostly empty space
–electrons
–electrons do not “orbit” like planets; more like bees/beehive
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Summary of the subatomic particlesName Abbr Where Charge mass Who?
Proton P+ Nucleus +1 1.007u Rutherford
Neutron
No Nucleus 0 1.008u Chadwick
Electron
e- Electroncloud
-1 0.00055u
Thomsom
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Summary of the subatomic particles particle where? Mass who?Proton p+ Nucleus 1.007amu Rutherford
Neutron no Nucleus 1.008amu Chadwick
Electron e- Electron cloud
0.00055 amu
Thomson
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Atomic Number
the number of protons in the nucleus of an atom
gives the atom it’s identity also, equal to the number of
electrons in a neutral atom
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Mass Number
Equal to the number of protons plus the number of neutrons in the nucleus of an atom
#no = mass # - atomic #
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Important note! The atomic number of an element
is on the periodic table, but the mass number is usually not!
The location of the numbers on the periodic table is at the printer’s discretion
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The good news: –all atoms of the same element
have the same atomic number The bad news:
–not all atoms of the same element have the same mass number
What is different?–The number of neutrons
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isotopes Atoms of the same element with
different mass numbers– different numbers of neutrons
different versions of the same element no difference in chemical properties only fundamental difference is in mass
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Isotope symbols
The elements symbol, plus... the mass number is written in
the upper left corner the atomic number is written in
the lower left corner
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When writing out the name of an isotope, the number following the element name is the mass number of the isotope
Compare carbon-12, carbon-13, and carbon-14
each have the same number of protons, but a different number of neutrons
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Examples of isotope symbols12C 6p+6no
6
13C 6p+7no
6
14C 6p+8no
6
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Isotopes and Mass Number
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Ions An atom that is no longer neutral
– #p+ ≠ #e-
No change in the nucleus, so the same element, but now with a + or - charge
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How does an atom become an ion? The atom either gains or loses
electrons The nucleus is not directly involved
in ionization– The term used when a neutral atom becomes
an ion The number of protons does not change
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How does an atom become an ion? If the atom gains electrons, it
becomes negatively charged Ex: If a sulfur atom, with it’s 16
protons and 16 electrons gains two electrons…
It now has a charge of (+16) + (-18) = -2
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How does an atom become an ion? If the atom loses electrons, it
becomes positively charged Ex: If an aluminum atom, with it’s 13
protons and 13 electrons loses three electrons…
It now has a charge of (+13) + (-10) = +3
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anionsAtoms that have gained
one or more electronsBecome negative (-) ionsUsually nonmetals
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cations
Atoms that have lost one or more electrons
Become positive (+) ionsUsually the metals