1. Today in Science
You will Need:
1)Pencil, Colored Pencils, Highlighters or
Markers
2)Atom Booklet Directions– 1 page 2 sides-
Bookshelf
3)4 pieces of white unlined paper–
Bookshelf

2. Reminder
1)Update Log #3
2)End of Quarter is this Wednesday– if you
have missing assignments you want to turn
in they must be turned in by Wed.
3)Test #2 Corrections + Parent Signature –
Due Wednesday

3. 1) Materials Managers – Pick up a
stapler from front table.
2) Folding and Stapling the Book
3) Label pages according to Sample
Booklet
4) Page six Element = DO NOT
CHOOSE Platinum
5) Page six and seven need CHARTS
– can be done as “T” Tables

4. Topic:
Atom Booklet Information
Do we understand
everything????

5. Democritus 400 BC • 1st idea of “atoms”
Greece - stated that
all matter is made up
• Believed all matter is made
of atoms. He also
stated that atoms are up of tiny particles separated
eternal and invisible
and so small that
they can’t be divided,
by space
and they entirely fill
up the space they’re
• Named particles “atomos”
in
which means indivisible.
Lavoisier 1789 • Founder of modern
chemistry
France - provided the
formula for the
conservation of matter
• 1st carefully controlled
in chemical reactions,
and also distinguished experiments providing
between an element
and a compound evidence to the Law of
Conservation of Mass

6. Dalton 1766-1844 1st MODERN Atomic Theory
(pg 165) 1.All matter made up of tiny
England - formed the 1st atomic theory,
which states that all matter is composed of indivisible particles called atoms
tiny, indestructible particles called atoms
that are all alike and have the same atomic
weight.
2.Atoms of the same element
have identical properties
3.Atoms of different elements
have different properties
4.Atoms combine in a specific
ratio to form compounds
5.A specific compound is always
made up of atoms in a specific
proportion.

7. Thomson 1897 Plum Pudding Model
(pg 166) 1.Negative particles scrambled
into the “dough” of the positive
particles.
England - discovered
the electron and
developed the plum-
pudding model of the
atom.
Rutherford 1898 Gold Foil Experiment
(pg 167) England - used the
results of his gold-foil
experiment to state that
1.Atoms are mostly empty space
all the mass of an
atom was in a small
2.All the Mass of an atom is in the
positively-charged
ball at the center of positively charged ball in the
the atom.
center of the structure.

8. Bohr 1922 Denmark - stated that
“Planetary” atom model
(pg 169)
the electrons moved 1.Believed the atom structure was like our
around the nucleus in
successively large solar system: nucleus in the middle like
orbits. He also
presented the Bohr
the sun and the electrons orbiting like the
atomic model which planets.
stated that atoms
absorb or emit radiation
only when the electrons
abruptly jump between
allowed, or stationary,
states.
Schrödinger (Schroedinger ) Wave Mechanic Model
1930
Austria - introduced the
Shroedinger Equation, a 1.Planetary model was too specific
wave equation that
describes the form of the
2.Rather: electrons vibrate around the
probability waves that
govern the motion of
outside of the nucleus- can only
small particles and how
these waves are altered
predict where they are most like to be
by external influences. 3.QUARKS – protons, neutrons and
electrons made up of some of these
smaller particles.
4.http://library.thinkquest.org/05aug/01087/quarks.html

9. Basic Atomic Structure Today scientists agree on the
three basic subatomic particles
that make up all atoms.
Bohr Model for Lithium
(not to scale) Electron = 3
(pg 172)
P= 3 +
N = 3 0
Where is most of the mass in the
NUCLEUS
Atom?
Where is most of the volume in the Outside the Nucleus; Electron
Atom?
Cloud

10. Nucleus • Contains protons(+) and
Neutrons (0)
• Holds most of the mass of
the atom
• Very small compared to the
entire size of the atom
• Most dense part of the atom
Electron • Negatively charged
subatomic particle
• Found outside the nucleus in
the electron cloud
• Smallest particle; mass =
1/1836th of the atom

11. Proton • Positively charged subatomic particle
• Found in the nucleus
• Mass = 1 amu (atomic mass unit)
• # of protons in an atom IDENTIFIES the
atom (which element)
• # of protons in the nucleus of an atom
called the atomic number
Neutron • Zero charge
• Mass = 1 amu
• Do NOT affect the identity of the atom
• Found in the nucleus
• Same atom of an element can have
varying amounts of neutrons (isotope)
• Adding the total number of protons &
neutrons = Atomic Mass Number
http://www.sawyerscience.com/Units/unit2/atoms_compounds.html

12. All atoms found on the • Neutral – same # of protons(+) and
Periodic Table are # of electrons(-)
Isotope • Atoms of the same element with
(pg 176) same number of protons and
different number of neutrons.
nucleus nucleus
Proton
Hydrogen has 3 natural
occurring ISOTOPES: Protiu nucleus Deuteriu
Protium, Deuterium and m m
Tritium
are Neutro
All ROGEN have n
l
HYD use al Tritium
a
bec oton.
r
1p

13. Atomic MASS • On the Periodic Table represents a
weighted average of the mass of all
naturally occurring isotopes of each
element. (based on mass and
abundance of each isotope).
• When atoms gain or lose electrons
IONS
they become charged. (number of
protons (+) and electrons (-)
particles are NOT EQUAL)

14. How do we know if an
element is a metal, 1. Metalloids – are in green boxes
nonmetal or metalloid? 2. Nonmetals – are in yellow boxes
3. Metals – are in blue boxes
Look on pg. 196-197
Go to the Hyperlink in Learning
How can I find the Bohr Point for this week.
Model for my Element? It should read BOHR MODEL and
have a picture of a globe next to it.

15. Homework
1)Atom Booklet– Due by Thursday at
the end of class
2)Test #2 Corrected & Signed by
Parents on the Front – Due Wednesday
Have you noticed HOW the periodic
table and the Atomic Structure are
RELATED?