Download Unit 2, Day 25

Changes Matter
Unit 2, Day 25
10/29/14
Period 1
Period 4
Period 5
Period 6
Changes Matter
WEEK 9  10/29/14
CATALYST
What do you think an
atom is?
Have out on
your desk:
 Binder
 Notes
*Answer in complete
sentences!
Homework:
None!
(front)
 TURN IN write-ups
if you didn’t
yesterday
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End
Changes Matter
10/29/14
Learning Intention:
We will demonstrate
knowledge of the elements
that compose the
periodic table.
Success Criteria:
We will be successful when we
can calculate the number of
electrons, protons, and neutrons
an element has based on the
atomic number & mass number.
Today’s Agenda
 Turn
in write-ups
 Intro to Unit 3: The Atom
 Notes
 Review
 Clip
(if done early)
NEW Unit = THE ATOM
 AKA
 TAKE
the building blocks of matter
OUT UNIT 3 NOTES!
Lets be COLLEGIATE
Remember…
 Elements
are:
_________________________________________
__________________________________________
The Atom
Although elements are the
purest form of anything, they
can be broken down into
their smallest form: the atom
Everything that is a pure
element is made of the
exact same atoms.
The Atom
Each atom is made of 3 parts: the
proton, the neutron and the
electron
Proton: subatomic particle that is
found in the nucleus that carries
a positive charge, and has a
mass of 1 amu
(AMU = Atomic Mass Units)
The Atom
Each atom is made of 3
parts: the proton, the neutron
and the electron
Neutron: subatomic particle
found in the nucleus that has no
charge and a mass of 1 amu
The Atom
Each atom is made of 3
parts: the proton, the neutron
and the electron
Electron: subatomic particle
found flying around the nucleus
that carries a negative charge
All atoms have the same general
structure
The protons and neutrons are
found in the center, or the
nucleus
Electrons surround the nucleus
in orbitals
We identify each
element by how many protons it has
…This is the atomic number
 Each
element has a unique atomic number
 This number increases as you move from left to right
on the periodic table
In order for an element to not carry a charge, the
number of protons and the number of electrons
must be exactly the same.
Example: The atomic number of carbon is 6. How
many protons and electrons does it have?
Atomic number =
Number of protons =
Number electrons
6=6=6
→ 6 protons & 6 electrons
Practice: Determine the number
of protons and electrons each
of the following elements has.
1. Br
2. Xe
3. Sb
4. H
Practice: Determine the number
of protons and electrons each
of the following elements has.
1. Br  35 protons, 35 electrons
2. Xe  54 protons, 54 electrons
3. Sb  51 protons, 51 electrons
4. H  1 proton, 1 electron
Each individual atom
has a mass, measured in atomic mass units
 amu
is used because the mass of each subatomic
particle is too small to measure in grams
 The mass of each atom is equal to the number of
protons plus the number of neutrons.
(Electrons are ignored, because their mass is so
small that they don’t affect the mass enough)
Example: Determine how many protons,
neutrons and electrons helium has.
1.
Find the chemical symbol
1.
Identify the atomic number (#
protons)
2.
Identify the atomic mass
3.
Take atomic mass – atomic number
to find number of neutrons
4.
Round to nearest whole number
Practice: Complete the table.
Element
Name
Element
Symbol
Carbon
Atomic Mass
12.01
N
Protons
6
7
17
Xe
Potassium
Neutrons
7
Electrons
Practice: Complete the table.
Element
Name
Carbon
Nitrogen
Element
Symbol
C
N
Atomic Mass
12.01
Protons
Neutrons
6
6
7
7
17
Xe
Potassium
Electrons
6
Using your periodic table,
what element has 8
neutrons and an atomic
mass of 16?
*Complete Sentences!
Have a good day 
Success Criteria
Question
Changes Matter
10/29/14