1) Atoms are the smallest particle into which an element can be divided and still retain its properties. Atoms are made up of even smaller particles called subatomic particles - protons, neutrons, and electrons. 2) Protons are positively charged and found in the nucleus. Neutrons have no charge and are also found in the nucleus. Electrons are negatively charged and orbit the nucleus. 3) The number of protons determines which element an atom is. All atoms of the same element have the same number of protons. The number of neutrons can vary forming different isotopes of an element.

1. You Will Need:
1)Pencil, Colored Pencils
2)Power Notes – Atomic
Structure – Book shelf 3
pages 6 sides- Please Staple.

2. Reminders :
1.Binder Check #2 – Due at the beginning
of class on Thur.
1.Table of Contents on-line
2.Edit out my notes
3.Number your pages starting with Log
#2
2. ½ page of notes for Test #2 – Thur-
Computer, Fri-Written portion
Front side only – Done by hand

3. Class Notes
Power Notes –
Topic: ________________________ Atomic Name ________________________________________
Class ________________________________________
Structure
Questions/Main Ideas: Period ________________________________________
Date _____________________________________
Notes:
• Is made up of tiny particles
1. All Matter
called atoms.
2. What are • Smallest particle into which
Atoms? 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.

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

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

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

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

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

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

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

11. 22. What is an • Same element with a different # of
ISOTOPE? neutrons
23. What is an • Hydrogen 1, 2 & 3 or Protium, Deutirium
example of an and Tritium
ISOTOPE? • 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?

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

13. 1. Power Notes – Due by the end
of the period Tomorrow
2. Binder Check #2 - Due
Thursday
3. Test #2-1/2 page of notes –
Due Thursday