This document provides class notes on atomic structure that include: 1) An overview of the basic particles that make up atoms - protons, neutrons, and electrons. It defines their properties like charge and location within the atom. 2) Details on atomic number and mass, and how they relate to the number of protons, neutrons, and electrons in an atom. 3) Explanations of isotopes and how atoms of the same element can have different numbers of neutrons. Hydrogen isotopes are illustrated as an example.

1. You Will Need:
1) Pencil, Colored Pencils
2) Log #3 – Update on-line
3) Power Notes – Atomic Structure
– Book shelf 3 pages 6 sidesPlease Staple.
4) Oral Presenters – Log-in

2. Class Notes
Power Notes –
Topic: ________________________
Atomic
Name ________________________________________
Class ________________________________________
Period ________________________________________
Date _____________________________________
Notes:
Structure
Questions/Main Ideas:
1. All Matter
2. What are
Atoms?
•
Is made up of tiny particles
called atoms.
•
Smallest particle into which
an element can be divided
and still keep its properties.
•
EX: one atom of gold still has
all the properties of
gold….but if you split the
atom it is no longer gold.

3. 3. How do we
know what we
know about
atoms?
•
Most of what we know was
discovered throughout
history from indirect
observations. (without ever seeing an
image)….remember the “Whatzit?”
4. How big is the
atom?
•
The diameter is about one
hundred-millionth of a
centimeter (0.00000001 cm)

4. 5. What are the
basic particles of
an atom?
There are three different types of
particles; protons, neutrons and
electrons
They are called subatomic particles
•
6. What is a
proton?
7. What is a
neutron?
•
•
•
•
•
Found in the nucleus (center)
of the atom
Positively charged
Mass of 1 amu (atomic mass
unit)
Found in the nucleus (center) of the
atom
No charge
Mass of 1 amu

5. 8. What is an
electron?
Draw
this pic
•
•
•
•
•
9. What charge
does the nucleus
have? Why?
•
•
•
Found orbiting outside the
nucleus of the atom
Negative charge
Mass of 1/1840 amu
This particle determines how
the element will bond
This particle also determines
the charge of the atom
Positive
Only protons (+) and neutrons
(no charge) in the nucleus
No other particles to cancel
out the + particles in this space

6. 10. What part of
the atom take up
the most space?
(volume)
11. Which part of
the atom has the
most mass?
12. What does
a model of the
atom look like?
•
•
•
•
•
•
•
•
The electron cloud
EX: If the center of an atom was the
size of a bee, the atom would be as
big as a football stadium
The nucleus (contains protons
and neutrons)
Both subatomic particles have
1 amu
Pg. 174 in your text.
Label: proton, neutron, electron &
nucleus.
Label their charges.
Color each particle a different color

7. 13. If all elements
are made up of
atoms, how do we
know which element
we are looking at?
•
•
•
•
14. What charge do
the atoms have?
•
•
15. Are there atoms
that are charged?
•
•
•
Each element has their own unique amount
of protons
No two elements have the same amount of
protons
Count the protons in the nucleus and you
can identify what element you are looking
at
Atoms found on the Periodic Table are
electronically neutral.
They have the same # of protons (+) and
electrons (-),.
Their charges cancel each other out.
Yes, they are called IONS
Ions will have more or less electrons than
protons
PLASMAS contain IONS

8. 16. Periodic Table
Connection
•
Each element box contains all the
information for finding the number
of subatomic particles
•
Label the CARBON box using the key on
pg. 196
•
•
# of Protons
# of Electrons if the atom is neutral (has
not charge)
17. How do you read
the Periodic Table
box? (pg. 196)
18. The atomic
number tell you the
number of?

9. 19. The atomic mass
tells you the number
of?
•
20. How do you find
the # of neutrons
•
•
•
•
21. How do you
know which is the
most common
ISOTOPE of an
element?
Protons added to the number of
Neutrons
In other words: the mass of the
nucleus
Round the atomic mass to the nearest
whole #
Subtract the Atomic Number from the
Atomic Mass
Your answer represents the # of
neutrons in the most common isotope of
an element
•
Round the atomic mass
•
•
EX: Li 6.9 Most common Isotope = Li 7
Cu 63.5 Most common Isotope = Cu 64

10. 22. What is an
ISOTOPE?
•
Same element with a different # of
neutrons
23. What is an
example of an
ISOTOPE?
•
Hydrogen 1, 2 & 3 or Protium, Deutirium
and Tritium
All have 1 proton
Different # of neutrons in the nucleus
24. Illustrate, Label &
Color the 3 different
forms of Hydrogen
(pg. 175)
*Clue: Tritium has
one electron & 1
proton….how many
neutrons?
•
•

11. 25. How are the
ISOTOPES similar?
•
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Same # of protons
Same element
Review:
Use your notes to help answer the Review
questions.

12. 1.
2.
Power Notes – Due by
Oct. 23rd
No Homework over the
weekend