Let’s Review
CHAPTER 4
Videos
 Song about the Dudes of chemistry

http://www.youtube.com/watch?v=07yDiELe83Y&fea
ture=related
 Lewis Dot

http://www.youtube.com/watch?v=ulyopnxjAZ8
Vocab
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Dissociation (3)
Spectroscope (4)
Spectra (4)
Energy (4)
Ion (3)
Ionization Energy
(3)
 Nucleus (3)
 Proton (3)
 Electron (3)
 Alpha Particle (4)
 Physical Model (4)
 Conceptual Model
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(4)
Inference (2)
Evidence (2)
Cathode Ray (4)
Molecule (3)
Compound (3)
Quantum (4)
Valence Electron (3)
Where are the following
located?
 Alkali Metals
Group 1
 Alkaline Earth
Metals Group 2
 Transition
Groups 3-10
Metals
 Halogens Group 17
 Noble Gases Group 18
Structure of an Atom
 What are atoms made up of?

Protons (+) in nucleus

Electrons (-) outside nucleus
in shells

Neutrons (no charge) nucleus
 Can you draw a Bohr Diagram of an element?
Don’t forget to label the charges.
 What are the three types of bonds? How are
they similar how are they different?

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Ionic- taken not shared
complete shell
Covalent- shared equally
complete shell

Polar- unequal sharing
complete shell
Trends in the Periodic Table
 What are three trends we discussed in the
periodic table?
Left to right- IE. EN increase AR decrease
Top to bottom- IE. EN decrease AR increase
 What are families (groups) and periods? What
can they tell you about trends. Groups/Family- columns
Periods - rows
 What group is the stable group? How do you
know? Group 18 also known as Noble Gas, full valence shell
 Which group do you find the highest/lowest I.E
and E.N?
Group 17 Highest IE and EN, Group 1 Lowest IE, EN
Important dudes discussed
 The following individuals contributed to the
modern idea of the atom. How? Name the
model, and what ideas they brought in.
 Democritus Matter is made up of atoms
 Dalton Atoms are indivisible spheres
 Thompson Atoms contain negative charges called electrons, Model “Plum
Pudding” Used Cathode Ray Tube
 Rutherford Gold Foil Experiment showed: nucleus, and empty space.
Model is called the Nuclear Model
 Bohr Used Spectra scope to add to the idea that electrons orbit in shells
and each shell is an energy level
PLANETARY MODEL
Spectroscope
 What is it what does it do?
An instrument that separates light into its
principal wavelengths
 What do you see when looking at sun,
incandescent, or a fire?
A continuous spectra. All wavelengths are present in the light that
is emitted
 What do you see if burning metal ions or
when looking at a specific elemental tube?
That element’s specific spectral lines. Each element has its own
“finger print” or lines specific to only that element. Elements emit
light (photons) when decreasing in energy levels.
Rutherford
 Tell me about his experiment. What was his
experiment? What did he do? What did it
explain to him?
He shot alpha particles through gold foil and observed the amount of
deflection. It proved that there was a high concentration of positive charges in
the middle (nucleus) and that the rest of the atom was consisting of mostly
empty space.
 How did his discoveries help our current level
of understanding of the atom.
Our current model still uses the nucleus and we still believe that most of the
atom consists of empty space
 What two things did he discover?
Nucleus
Empty space
Super Model – Study this well
for the Test tomorrow!
 Ernest
Rutherford
– 1871- 1937
 His famous
experiment
is known as
the Gold
Foil
Experiment
.
Super Model _ Study this well
for the Test tomorrow!
 Ernest Rutherford– 1871- 1937
What he saw (evidence)
What he concluded (Inference)
Most of the alpha particles went straight
through the foil (undeflected)
The atom is mostly empty space
Very few alpha particles bounced straight
back (or at a large angle)
The atom has a very small, very dense
center (nucleus)
Some alpha particles were deflected at a
an angle.
The nucleus must have a positive charge,
since the positive alpha particles that
came close to the nucleus were deflected
at a small angle.
Bohr
 How is Bohr Model different from
Rutherford?
Bohr believed that the electrons orbit the nucleus in different shells (energy
levels)
 What evidence did he have to support his
theories?
The spectral lines viewed through the spectra scope and comparing different
wavelengths
 How does a quantum relate to the light
spectrum?
A quantum of energy is the amount of energy required to move an electron
from one energy level to another
Physical and Conceptual
Models
 Make a T-chart/Venn Diagram/ or Table
 Similarities and Differences
 Give an example of each
Physical Model
Conceptual model
An object on a different
Describes a system, not a thing
scale
Example: using analogies to describe
Example: Model of airplane,
how photosynthesis works
schools.
Similarities: Both help represent the concept or item trying to describe
without using the idea or concept directly
Lewis Dot/Electron Dot
 Sulfur
 Carbon
 Phosphorus
 Boron
 Magnesium
 Argon