Download Atomic Theory

Bellwork 08/20/2012
How long have people been interested in
understanding matter and its structure?
A. Thousands of years
B. Hundreds of years
C. A few years
D. Never
History of Atomic
Structure
Ancient Philosophy
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Who: Aristotle, Democritus
When: More than 2000 years ago
Where: Greece
What: Aristotle believed in 4 elements: Earth,
Air, Fire, and Water. Democritus believed
that matter was made of small particles he
named “atoms”.
• Why: Aristotle and Democritus used
observation and inference to explain the
existence of everything.
Democritus
• Matter is composed of empty space through which
atoms move.
• Atoms are solid, homogeneous, indestructible, and
indivisible.
• Different kinds of atoms have different sizes and
shapes.
• The differing properties of matter are due to the
size, shape, and movement of atoms.
• Apparent changes in matter result from changes in
the groupings of atoms and not from changes in the
atoms themselves.
Democritus
Aristotle
Alchemists
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Who: European Scientists
When: 800 – 900 years ago
Where: Europe
What: Their work developed into what is now
modern chemistry.
• Why: Trying to change ordinary materials
into gold.
Alchemic Symbols
Particle Theory
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Who: John Dalton
When: 1808
Where: England
What: Described atoms as tiny particles that
could not be divided. Thought each element
was made of its own kind of atom.
• Why: Building on the ideas of Democritus in
ancient Greece.
Dalton
• Atoms of an element are not changed into
atoms of a different element by chemical
reactions; atoms are neither created nor
destroyed in chemical reactions.
• Compounds are formed when atoms of
more than one element combine; a given
compound always has the same relative
number and kind of atoms.
• BILLIARD BALL MODEL
John Dalton
Discovery of Electrons
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Who: J. J. Thompson
When: 1897
Where: England
What: Thompson discovered that electrons
were smaller particles of an atom and were
negatively charged.
• Why: Thompson knew atoms were neutrally
charged, but couldn’t find the positive
particle.
The Atom, circa 1900:
PLUM PUDDING MODEL
• “Plum pudding” model, put
forward by Thompson.
• Positive sphere of matter with
negative electrons imbedded
in it.
J. J. Thompson
Atomic Structure I
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Who: Ernest Rutherford
When: 1911
Where: England
What: Conducted an experiment to isolate
the positive particles in an atom. Decided
that the atoms were mostly empty space, but
had a dense central core.
• Why: He knew that atoms had positive and
negative particles, but could not decide how
they were arranged.
Discovery of the Nucleus
Ernest Rutherford shot
 particles at a thin
sheet of gold foil and
observed the pattern of
scatter of the particles.
The Nuclear Atom
Since some particles
were deflected at
large angles,
Thompson’s model
could not be correct.
THE NUCLEAR MODEL
According to Rutherford,
most of the atom
consists of electrons
moving rapidly through
empty space and a
very dense, positively
charged nucleus.
Ernest Rutherford
Other Subatomic Particles
• By 1920 , Rutherford had refined his
concept of the nucleus: He concluded
that the very dense nucleus contained
positively particles called protons.
• James Chadwick, a coworker, showed
that the nucleus also contained a
neutral particle in 1932. This was the
neutron – a particle with nearly equal
mass as a proton.
Atomic Structure II
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Who: Niels Bohr
When: 1913
Where: England
What: Proposed that electrons traveled in
fixed paths around the nucleus. Scientists
still use the Bohr model to show the number
of electrons in each orbit around the nucleus.
• Why: Bohr was trying to show why the
negative electrons were not sucked into the
nucleus of the atom.
Niels Bohr
Electron Cloud Model
• Electrons travel around the nucleus in
random orbits.
• Scientists cannot predict where they will be
at any given moment.
• Electrons travel so fast, they appear to form
a “cloud” around the nucleus.
Electron Cloud Model
Atomic Structure Timeline
Requirements:
• Must include a title.
• Must include a spot for each of the 7 items.
• Must include at least the Who, When, and
What.
• Must have a picture (color is preferred) for
each item.
Options:
1. Comic book format
2. Standard timeline
Properties of Subatomic Particles
Symbol Location Charge
Relative
mass
Actual mass
(g)
Electron
e-
Around
nucleus
1–
1
1840
9.11×10-28
Proton
p+
Nucleus
1+
1
1.673×10-24
Neutron
n0
nucleus
0
1
1.675×10-24
Particle
Atomic Structure and the
Periodic Table
Symbol
14
Si
28.086
Silicon
Atomic number = # protons
Name
Atomic Mass: Round to a whole #:
28 = Relative mass of nucleus
-14 = # protons
14 = # neutrons
Practice From the Periodic
Table
Complete the following chart:
Name
Relative
Symbol
mass
#
#
#
protons neutrons electrons
Lithium
Mg
26
16