Unit 2 Matter
Chem 1
Be Seated
CHEMISTRY
Agenda 10/4
1.
2.
3.
4.
5.
Panther Drill 4
Notes (Properties and States of Matter)
PD Redux, If I knew then what I know now
WS Sci Notebook Sec 3.1
Close/Exit Ticket
Panther Drill 4
Identify the state of matter of the following:
(IE is it Liquid ect)
O2 Gas
Water Liquid
Solid
Ice
Water Vapor Gas
Inside Florescent Lights Plasma
Liquid
Blood
Solid
Jell-O
The Sun Mostly Plasma, Some Gas
Substances
A substance is matter that has definite composition
and properties.
i.e. Table salt (NaCl) always has the same make-up
and properties no matter if you put it on your
popcorn in Lake City, Murrells Inlet, or Lake City
Colorado.
Whereas salt water found in the pacific ocean is
different than salt water found in the arctic ocean.
What is MATTER?
Anything that Takes up Space and Has Mass.
What are the States of Matter?
Solid, Liquid, Gas, Plasma
1) Solid:
Definite volume and definite shape
(Glass)
2) Liquid:
Definite volume indefinite shape (Water)
Solids and Liquid
In a solid. all molecules vibrate
and forces of attraction hold
them in place.
In a liquid the molecules have
partially overcome the forces
of attraction and still partially
in contact
Gas:
Indefinite volume, indefinite shape.
IE Car Exhaust
Plasma:
High temperature physical state, made up
of free electrons and ions of the element
IE Florescent Lights, Mushroom Cloud, the
northern lights, and Plasma TVs.
Gas and Plasma
Molecules have completely
over come attractive
forces, any contact is
random.
Movement is extremely fast
and electrons are striped
away from the molecules.
Characteristics of States of Matter
http://www.nasa.gov/images/content/147515main_phases_large.jpg
Properties
Extensive properties: properties that depend
on how much of matter is present.
i.e. Volume and Mass
Intensive properties: does not depend on how
much matter is present
i.e.: density and boiling point
Physical Properties
Physical Properties: something that can
be changed in a substance w/o
changing its identity.
i.e.: Melting Ice
Cutting a 2x4 in half
Boiling
Chemical Properties: changes that result in a
substance being changed into new substances.
i.e.: Burning charcoal = carbon ash and O2 & CO2
Iron Rusting
** A physical or chemical change requires energy to
be added to what ever is changing (aka the system)
Energy can be heat or light other forms
Shoulder Partners Answer and check ea. other answers
Mushroom Cloud
Shampoo
Jell-o
S,L,G,P
S,L,G,P
S,L,G,P
Burning Gas
Baking Cookies
Maxing Salt water
Physical or Chemical
Physical or Chemical
Physical or Chemical
Odor
Weight
Color
Extensive or Intensive
Extensive or Intensive
Extensive or Intensive
Before you pack up
Compare and Contrast Extensive
and Intensive properties
Show it to me before you leave
10/5
1.
2.
3.
4.
5.
PD 5
Notes
Example Conservation of Mass
Do practice problems w/ partners
Exit Problem
Modified Seats 3rd Period
Go to your seats and Panther Drill will start at bell
Justice
Porchea
Spud
Yessie
Galloway
Gaskins
Pace
Stukes
Ashley
Belinda
Amber
Cordrick
Wade
Josh
Kyianna
Terrance
Breanna
Modified Seating 6th Period
Sade’ Jasmine
Kayla
Nasia
Jaron
Justin
Tykosha
Shekia
Whitney
Demond
Terica
Willie
Quay
Keshon
Reggie
Diamond
Steve
Tyiesha
Rayneesha
Jamika
Dominque
Panther Drill #5
Think about what you know about
nature, tell me about how the
physical phase change of water,
effects the natural world.
Kinds Physical Changes
Freezing is the change of state from a liquid to a
solid.
Melting is the change of state from a solid to a liquid.
Vaporization is the change of state from a liquid to a
gas.
Condensation is the change of state from a gas to a
liquid.
Sublimation is the change of state from a solid
directly into a gas.
Deposition is the change of state from a gas directly
into a solid.
Example
More
energy
in the
system
Less
energy in
the
system
State Changes and the Environment
Chemical Reactions
In a chemical reaction there are the reactants and
the products.
Reactants: what you start with
Products: what you end with
99.08g Fe + 55.92 g O2
 155g Fe2O3(Rust)
Reactants
Products
What is the mass of the Fe and the O? 99.08g + 55.92g
What is the mass of the Fe2O3? 155g
Law of Conservation of Mass
“Matter can’t be created or destroyed in a
chemical reaction, it is conserved”
That means the mass of the reactants = the
mass of the products.
Mass reactants = Mass products
Get in your pairings and work on problems
Partners 1st Period
Brad & LaTonya
Mary & Qualisha
Quanisha & Howard
Hank & Brenton
Jess & Abria
Raven & Cody
Sam and Devonte
Cassidy and Devonta
Trevon’ & Drequan
Partners 3rd Period
Josh & Cordrick
Kyiana & Belinda
Breanna & Terrance
Justice & Yessie
Galloway & Cadejah
Gaskins and Spud
Brandon and Porschea
Ashley, Amber, & Clarence
Partners 6th Period
Jaron & Willie
Jamika & Dominique
Keshon &Shekia
Nasia & Tykosha
Justin & Quay
Sade’ & Whitney
Jasmine & Demond
Rayneesha & Terica
Steve & Diamond
Tiesha,
Reggie, & Kayla
Partner A show partner B how to
do Problem #1 Then Reverse roles
1. When 245 grams of KClO3 are heated, the KClO3
breaks down into 78 grams of potassium, 71
grams of chlorine and some oxygen gas. What is
the mass of oxygen gas formed?
2. You have 729 g of NaOH (Sodium Hydroxide) is
broken down into its parts. What resulted was
459 g of Na, 127 g of Oxygen, and how many
grams of Hydrogen?
Do number 6,7&8 from pp
78 in your text by
yourselves, and show it to
me, before you pack-up
Agenda 10/6
1. PD #6
2. Notes/Discussion (Mixtures/Pure
Substances/Separation)
3. PD Redux
4. Exit Assignment
5. Lab Thurs. Reminder
Panther Drill #6
Identify the following items (NOT as solid liquid
or gas) but as mixtures or pure substances.
Aluminum Pure
Table Salt Mixture
Water Pure
Stainless Steel Mixture
Kool Aid Mixture
Carbon Pure
DRESS FOR LAB TOMORROW
THURSDAY 10/7
Classification of Matter
Matter is classified as either a MIXTURE or a PURE
SUBSTANCE.
1) Pure Substances: is homogeneous and has a fixed
composition.
Every sample has the exact same properties
IE all pure water boils at 100C and freezes at 0C
Every sample has the exact same composition
IE all pure water has 11.2% H and 88.8% O2
Classification of Matter
2 kinds of pure substances:
Compounds and Elements
Elements: a pure substances that can not be
broken down into simpler parts IE Carbon
Compound: a substance that can be broken in
to simpler substances. IE WATER - H and O
Classification of Matter
2) Mixture: blend of 2 or more kinds of matter,
where each different type of matter keeps its
own identity or properties. Mixtures can be
broken down into their original parts.
2 kinds of mixtures:
Homogeneous: these have uniform
composition always in a single phase,
blended uniformly.
oSteel (a mix of carbon and iron)
oMilk
oMayonnaise
oSolutions
Classification of Matter
Mixtures Cont.
Heterogeneous: these are not uniform, their
composition changes from sample to sample, they
are not blended smoothly.
• Buttermilk
• Fresh squeezed orange juice
• Homemade mashed potatoes
• Pond water
Classification of Matter
Separating Mixtures
Filtration: using a filter to separate the a
heterogeneous mixture of solid and liquid
Distillation: using different boiling points of
substances in a homogeneous mixture to separate
it
Separating Mixtures
Crystallization: when pure solid forms from a
liquid solution containing as much solid as can
be held be the liquid (super saturated). Solid is
then formed as the liquid evaporates (Think
making rock candy.)
Sublimation: separation of solids and gas w/o
going through liquid state
Separating Mixtures
Chromatography: separate the
components of a mixture
(liquid or gas) by allowing it to
move across another material
(i.e. paper). The components
separate because the move
across the paper at different
rates.
If I only knew then what I know now…
Identify the following items as mixtures ore
pure substances.
Pure
Oxygen
Sugar
Mixture
Sugar Pure
Gator Aid Mixture
Pizza
Mixture
Water
Pure
Text assignment pp 83
#16,18
Due before you leave
Get into you lab Groups
Start Pre-Lab questions and assign jobs to
members.
1.
2.
3.
4.
5.
Equipment Person
Experimenter
Recorder
Leader/Clean up
If 5 in group then divide leader and cleanup
Thursday 10/7
Agenda
1. Panther Drill 7
2. Lab “”
3. Closure
Panther Drill #7
Get into your lab groups
and see who in your group
is in violation of Lab Safety
Rules.
Friday 10/8 Early Dismissal
Agenda
1. Panther Drill 8 Turn in for quiz
2. Finish Analysis and Conclusions for lab from
10/7
MONDAY Agenda 10/11
1. PD 8 quiz
2. Notes/Discussion
(Elements/Compounds/Periodic Table basics)
(10 min)
3. WS 3.4 (10 min)
4. Trading Card Game Elements/Compounds
(10 Min)
5. Exit Ticket 5 min
1
Panther Drill #8
Write out 2 sample quiz
questions based on last weeks
material that start with:
Can you explain in your
own words….?
How many...?
Can you distinguish
between ….?
Can you name the...?
Can you tell why...?
Find the meaning of...?
2
Write out 1 sample quiz
questions based on last weeks
material that start with:
Can you design a ... to
...?
Compare and
contrast….?
Explain the differences
between…?
Rank the following
based on…..
QUIZ
CHOOSE 4 TO ANSWER
1. Compare and contrast a physical and
chemical change.
2. Explain the best way to separate the pulp
from fresh squeezed OJ, and the best way to
separate salt water into its components.
3. Explain the law of conservation of mass.
4. Compare the molecule structure of the all 4
states of matter.
5. List and explain 5 of the 6 physical changes
of matter.
Elements
Elements are pure substances that can not be broken
down into simpler substances by physical or
chemical means. Oxygen, Carbon, Boron ect.
Abbreviated by 1,2,or 3 letter abbreviation 1st letter
always capitalized. O, Al, Zn, Uus (Ununseptium)
91 NATURALLY occurring elements on the earth.
Compounds
Compounds are a combination of 2 or more different
elements that have combined or bonded
chemically.
Most of the matter in the universe is compounds.
There are approx 10 million known compounds with
more discovered or created all the time.
List some compounds that you
encounter every day life:
Gasoline
C8H18
Baking soda
CHNa03
Milk of magnesium (Medicine)
Mg(OH )
Cream of tartar (Used in cooking)
KC4H5O6
2
Periodic Table
The periodic table is table that organizes all known
elements into horizontal rows and vertical columns
based on their properties.
The modern periodic table is based mainly on the
work of Russian Scientist Dmitri Mendeleev.
Mendeleev’s predictions of blank yet to be
discovered elements and where they would fit in
the table were pretty much right on.
We will do much more work with the periodic table
later in the semester.
Mendeleev’s Periodic Table
Modern Periodic Table
Tuesday Agenda
1. PD 8 How do compounds made of the same
elements differ, and what does that mean to their
properties. (5min)
2. WS 3.4 (Notebook) 10 (min)
3. Notes/Discussion Law of Definite proportions (10
min)
4. Modeling Example Law of Definite proportion
problems (10 min)
5. Independent practice problems (20 Min) pp78 #s 2023
6. Exit ticket (5 min)
Panther Drill 9
Answer the following question:
How do compounds, made of the same
elements differ, and what does that mean to
their properties?
IE H O and
2
HO
2
2
WS 3.4
Take the first 10-12 min to start WS # 3.4, us
section 3.4 in the Chem Text to complete it
and then put it in the Classwork Section of
your notebook.
Law of Definite Proportion
Individual Compounds are named and defined by the
number and ratio of the elements they are made
of.
WHAT IS A RATIO?
Relationship between two of the same kind
of numbers. The relationships in this case of
the subscripts or small #s below each
elements, which is the # of atoms of that
element in the compound.
Law of Definite Proportion 2
This is so important that it is stated in a law of
moderns Chemistry, The Law of Definite
Proportion.
This law says that in a compound the elements are
always present in the same proportion.
IE: H 0
2
There are always 2 Hs for every 1 O in
water.
Formula you need to know how to use
Percent mass or mass percent =
Mass of the element
Mass of the compound
x100
…
Mass Percent
A 25 gram sample of water contains 2.80 grams
of hydrogen.
What is the mass % of hydrogen?
2.80g/25g X 100 =
11.2%
Panther Drill 9 A
1. Think about the law of conservation of matter. If a 13
gram sample of element X combines with a 34.7 gram
sample of element Y, to form compound XY, what will
the mass of compound XY be?
2. A 25.3 sample of an unknown compound contains .0.8
grams of oxygen. What is the mass percent of the
oxygen in the unknown compound?
3. When mercury oxide is heated it breaks down into its
components of mercury and oxygen. 28.4 grams
completely breaks down it yields 2.0 grams of oxygen.
What is the mass percent of mercury in mercury
oxide?
`
Panther Drill 10
In your own words, define the law of
conservation of mass and the law of
definite proportion.
Prentice Hall © 2003
Chapter 1
Law of Multiple Proportion
States: when different compounds are formed by
the combination of the elements X and Y, then the
ratios between elements change, one element is
usually consistent in its subscript while the other
usually changes.
ie. H2O and H202
The H stays consistent and the Oxygen subscript
changes
Law of Multiple Proportion
EXAMPLE
Lets compare 2 different compounds a containing
copper and chlorine.
Compound 1 contains 64.2% copper and 35.8 %
Chlorine.
Compound 2 contains 47.27 % Copper and 52.73 %
Chlorine.
Law of Multiple Proportion
Now we have to determine the RATIO of copper to
Chlorine in each Compound. To do that we divide
the Mass % of the copper by the mass % of the
chlorine in each compound
Formula: Mass % element 1
Mass % Element 2
= Ratio of g Element 1 per g Element 2
Law of Multiple Proportion
Compound 1:
64.2 % Cu
35.8 % Cl
= 1.796 g Cu : 1 g Cl
Law of Multiple Proportion
Compound 2:
47.27% Cu
52.73 % Cl
= .8964 g Cu : 1 g Cl
Law of Multiple Proportion
Now we find the ratio of copper between
compound 1 and compound 2
1.796 g Cu/1 g Cl
8.964g Cu /1 g Cl
= 2.00
SO
The ratio is 2: 1
Compound 1 : Compound 2
Law of Multiple Proportion
This is important because there are only about
116 elements n the world and multiple
proportion allows for exponentially more
compounds
Try This 1
Draw table and fill in the information
Compound
Total Mass
Compound
Mass
Iron
Mass Mass %
Oxygen Iron
A
75.00 g
52.46 g 22.54 g
B
56.00 g
43.53 g 12.47 g
Mass % = Mass Element
Mass Compound
x 100
Mass %
Oxygen
Compound
Total Mass
Compound
Mass
Iron
Mass Mass %
Oxygen Iron
A
75.00 g
52.46 g 22.54 g 70 %
30 %
B
56.00 g
43.53 g 12.47 g 77.7 %
22.3 %
Mass %
Oxygen
Mass % Compound A= Fe: 52.46/75.00 x 100 = about 70 %
O: 100 % - 70% = 30 %
Mass % Compound B= Fe: 43.53/56 x 100 = about 77.75 %
O: 100 % - 76% = 22.25%
Use the Law of Multiple proportion to
find the ratio between Compound A
and Compound B from the table.
Mass Ratio Formula For a Compound:
Mass of Element 1 (Fe)
Mass Element 2 (O)
52.46 g Fe
22.54 g O
Compound A Ratio= 2.33 g Fe/ 1 g O
You Do Compound B
43.53 g Fe
12.47 g O
= 3.5 g Fe/g O in Compound B
Now compare compound A to Compound B
3.49 g Fe Comp B/ 2.33 g Fe Comp A =
3.5 g Fe Comp B: 2.33 g Fe Comp. A
Chapter 4
Friday: 4.1
TSWBAT:
Define and atom
Create a time line citing the key milestones
leading to the modern atomic theory.
Panther Drill # 11
Brainstorm Quick Write:
Just “stream of consciousness” write and put
down as many facts that you can think of
about the atom!!!
Early Theories of matter and atoms
•
•
•
•
•
Greek Philosopher Democritus about 400 BC
1st to suggest atoms
1st to suggest matter is empty space that atoms
move through
Atoms were solid and could not be divided into
any thing smaller.
Atoms were of different sizes and shapes
Properties depended on shape, size and
movement of atoms
Early Theories of matter
Greek Philosopher Aristotle about 350 BC
• He was the “Rock Star” of his time
• He rejected Democritus’s Ideas because the were
opposite of his.
Early Theories of matter
Not much new progress made for
about 2100 years or so
Early Theories of matter
John Dalton 1766-1844
• All elements are made up of atoms. It is
impossible to divide or destroy an atom.
• All atoms of the same elements are alike.
• Atoms of different elements are different.
• Atoms of different elements combine to form
a compound.
Early Theories of matter
Thompso
n’s Plum
Pudding
Model
J.J. Thompson Late 1800’s
• English scientist.
• He discovered the electron when he was
experimenting with gas discharge tubes.
• He saw that they moved to the positive end of the
gas tube and figured out that they had a – charge.
Early Theories of matter
Lord Ernest Rutherford 1871-1937
• Famous for gold foil experiment that showed that
some + charged particles could pass through a thin
layer of gold foil and some bounced back proving
that matter contained empty space and atoms had
a + charged nucleus that made some particles
“bounce back”.
Early Theories of matter
Niels Bohr Early 1900’s
• He proposed a model of the atom that is
similar to the model of the solar system.
• There are different energy levels or electron
orbits around the nucleus, like the different
planets orbit the sun at different distances.
Bohr
Model
Nitrogen
Your Assignment:
Use the notes you have plus the book if you have it to create
a time line the tells the story of the development of the
atomic theory.
Use color and try to make it as neat as you can the best will
be put up on the wall of fame.
The Assignment is due Monday 10/18 and is worth 15 points it will be
graded as follows:
6-7 Entries 12 points
5 entries 11 points
2-4 entries 8 points
1 entry 5 points
Neatness, and Creativity can get you up to 3 points
EXAMPLE OF A TIME LINE
http://www.bing.com/images/search?q=Example+of+timeline&FORM=SSIR&adlt=strict#focal=407f79a01ce488aee10015bab6c14733&furl=http%3A%2F%2Fwww.studentsfriend.com%2Fsfcimage%2Feras.jpg
Monday 10-18
1. PD 12
2. Demo Rutherford experiment
3. Work on project
Panther Drill 12
In your opinion who do you think is the most
important person in the development of the
modern atomic theory. Use your notes and
your own research to decide.
Panther Drill #13 Period 1
Write down 2 possible test questions
about atomic theory, on the paper on
your desk. One can be a basic question,
one needs to be a harder extended
response type question using question
stems for analyzing and applying for the
second question. PLEASE WRITE IN THE
½ SHEETS YOU HAVE AND NOT THE FULL
SHEETS.
Panther Drill #13
Particle
Location
Charge
Size
Electron
Proton
Neutron
Create and fill in the blanks in the table, for
size rank the particles 1 2 or 3 for size
Atoms
The Atom:
Smallest particle of matter that will retain its
properties.
Size: A single copper atom is .000000000128 or
1.28 x 10 -10 meters in diameter.
The only way it is possible to see an atom is to
use a scanning tunneling microscope STM, a
very fine sharp point is moved over a sample
and it interacts w/ the superficial or surface
atoms and this interaction is recorded by a
computer.
STM images
Silicon
Nickel
STMs
Informational Only
STMs are allowing science to
start to develop
“nanotechnology” meaning
they are able to build
machines the size of a
molecule, 1 atom at a time.
Here is an example of a
scientist w/ too much time
on their hands!!!!!!
Electrons
Formally discovered to have a negative charge and a
definitive mass, by JJ Thompson in 1897, use a
cathode ray tube.
The strength of the – charge was determined by
Millikan and the oil drop experiment.
The electron was found to have a mass of 1/1840 of
1 Hydrogen atom or 9.1 x 10 -28 grams.
Electron Cloud
Electrons are not really in
defined orbitals, but
are found in a cloud.
The cloud shows where
the electrons are likely
to be at any given time.
Heisenberg uncertainty principle
A math equation that states position and
momentum, cannot be simultaneously
known to high precision.
Means that we can either know what way an
electron is moving or where it is but not both
at the same time.
Schrödinger's cat
Schrödinger's cat is a thought experiment, often
described as a paradox, devised by Austrian
physicist Erwin Schrödinger in 1935. It illustrates
what he saw as the problem of the Copenhagen
interpretation of quantum mechanics applied to
everyday objects. The thought experiment
presents a cat that might be alive or dead,
depending on an earlier random event. In the
course of developing this experiment, he coined
the term quantum entanglement.
Quarks
There are six quarks, these are the particles that
make up protons and neutrons for our purposes
we will deal with up and down quarks.
Up quarks have a + 2/3 charge
Down quarks have a -1/3 charge
Protons, Neutron and the Nucleus
Protons:
Found by Rutherford
Charge of +1
Mass 1.673 x 10 -28
Protons, Neutron and the Nucleus
Neutron:
Confirmed by James Chadwick in 1932
Charge : Neutral or 0
Mass 1.673 x 10 -28
To Sum it Up
a.m.u. = atomic mass unit, about 1 proton or neutron of
a Hydrogen atom.
Panther Drill # 14
1. Sketch an atom.
2. How many Protons, Neutrons and
Electrons are in the following element.
Different Elements
We know protons and neutrons are in the nucleus
and electrons are outside but how do atoms for
different elements vary? I mean how is Hydrogen
different from Helium?
See the atomic # on the periodic table
H=1 and He = 2 ect
This means that H has 1 proton and 1 electron
And Helium has 2 protons and 2 electrons
***REMEMBER # OF ELECTRONS = # PROTONS
IN A NORMAL ATOM***
Reading the Periodic Table
Atomic Number
Elements Symbol
Chemical Name
Average Atomic
Mass
Reading the Periodic Table
No need to write this
Remember not all
periodic tables are
as detailed as
others some have
more information
than the basics like
this one.
Neutrons
Lets look at Hydrogen and Helium on the
periodic table
We see the atomic #, but what is the number
underneath the symbol?
THAT IS THE ATOMIC MASS
To find the # of Neutrons all we do is round the
atomic mass to the nearest whole number. This is
called the mass number Try it w/ H and He
H= 1
He = 4
Then we subtract the # of protons from the MASS NUMBER
NEUTRONS = MASS NUMBER - #PROTONS
H: 1-1 =0 (no neutrons in Hydrogen)
He 4 – 2 = 2 (2 neutrons in Helium)
Lets Try Some
Get w/ a Partner
How Many protons neutrons and electrons in
MASS NUMBER = 6.941 = 7 Atomic # = 3
Lithium?
Protons = atomic # = 3
Electrons = protons = 3
Neutrons = MASS NUMBER - # protons = 7 - 3
4 Neutrons
In Carbon?
MASS NUMBER = 12.011 = 12 Atomic # = 6
Protons = atomic # = 6
Electrons = protons = 6
Neutrons = MASS NUMBER - # protons = 12 - 6
In Zinc (Zn)?
6 Neutrons
MASS NUMBER = 65.39 = 65 Atomic # = 30
Protons = atomic # = 30
Electrons = protons = 30
Neutrons = MASS NUMBER - # protons = 65 -30 35 Neutrons
Run it back
What element has 5 neutrons and 4 protons.
Atomic # = # Protons = 4 = Beryllium
What is the name of the element with 31 neutrons
and 28 ELECTRONS? What is the element?
# of electrons = # protons = atomic # = 28
Nickel = 58.69 (atm mass)
=
Try Some on Your
Element Sheet
Panther Drill 15
1. How many protons, neutrons and electron
does Gold have?
2. What is a isotope?
3. How do you explain hydrogen with 2
protons?
Isotope Video Clip
Isotopes LCHS Laptop
Isotopes Flash Drive
Isotopes
Atoms that have the same number of
protons but different numbers of
neutrons. Most atoms have isotopes.
Hydrogen has 3 different isotopes.
http://education.jlab.org/glossary/isotope.html
Isotopes
Remember
# Neutrons = Mass # - Atomic #
SO
Mass # = atomic # (aka # protons) +
# neutrons.
http://education.jlab.org/glossary/isotope.html
Isotope
Carbon has 2 isotopes
Carbon-12
&
Carbon-14
Isotopes
Find out the number of neutrons in an isotope the
same way as in a normal element.
NEUTRONS = MASS NUMBER - ATOMIC # OR PROTONS
Isotope Notation
How do I write and isotope?
Mass #
ATM #
Sym
How would you write the isotopes of copper:
a) 1 w/ a mass number of 63
b) 1 w/ a mass # of 65
How would you write the isotopes of copper:
a) 1 w/ a mass number of 63
b) 1 w/ a mass # of 65
a)
63 Mass #
Cu
29 # protons
65 Mass #
b)
Cu
29 # protons
Why not whole # atomic mass
Elements have isotopes
so we don’t whole #
atomic masses.
Atomic mass = Atomic #
Elements and their
isotopes occur in
different natural
abundances
To find the atomic
mass we use a
weighted average
Weighted Average
If a 75% of the apples in a box have a mass of
149 grams and 25 % of the apples a mass of
153 grams. What is the average mass of an
apple in the box?
Formula: [mass (item1) + (% item1 x .01)] X
[mass (item2)x (% item2 x .01)]
Weighted Average
[mass (item1)x (% item1 x .01)] + [mass (item2)x (% item2 x .01)]
Item 1 = Apple 1 = mass 149g and 75% abundance
Item 2 = Apple 2 = mass 153g and 25% abundance
Avg. mass of apple =
[149 g x (75% x .01)] + [ 153 g x (25% x .01)
111.75g + 38.25g = 150 g
The average apple has a mass of 150 grams
Class Work
Do Problems 18 and 24 on page 121 in
your book
on handout
Let me see at least 18 before you leave!!!
Panther Drill 16
1. Silver has 2 isotopes 107
Ag
47
& 109
Ag
47
Based on Silvers atomic mass from the
periodic table, which isotope is more
abundant??
Agenda 10/25
1. Panther Drill 17 (3 Q’s 1 review from last
week and 2 to assess pre-knowledge of
today’s topic)
2. Notes and Discussion (Teacher will explain
Nuclear rxns, Radioactive decay (Unstable
Nuclei), alpha, beta, and gamma radiation).
3. WS 4.4 From Text.
4. Thumbs up or Down Review.
Panther Drill 17
1. Why do elements have on the periodic table
have decimals in their atomic masses
instead of whole numbers.
2. What is radiation?
3. What is a nuclear reaction?
Radioactivity
• Discovered in 1890s when scientists noticed
energy constantly being emitted they called this
radioactivity.
• This energy was called radiation.
• Atoms that emit radiation are called radioactive
atoms.
• The energy emitted was in the form of particles
and rays of energy.
Nuclear reactions
• It was found the radioactive atoms were not
undergoing a chemical reaction but what is called
a nuclear reaction.
• Nuclear reactions are changes in the nucleus of an
atom where energy is released.
• Atomic nuclei that emit energy through nuclear
reactions are called unstable.
• After the unstable nuclei release energy and
become stable, they become new isotopes or even
other elements. This is called radioactive decay.
Radioactive decay
Positive charged plate
Negative charged plate
In an experiment shows the 3 types of radiation
Alpha Radiation
Alpha particles are the form of radiation that is
drawn to the neagative charged plate in the
experiment.
An alpha particle contains 2 protons and 2 neutrons
so it is the same as a helium atom.
Alpha particle is shown as
4HE
2
or a
Beta Radiation
Beta particles were drawn to the + charged plat in
the experiment.
A beta particle is really and – charged electron and is
shown as an electron or b particle
This release allows the neutron to change to proton
b
Gamma Radiation
• Gamma radiation or g is
the only of the 3 types
to be an energy ray
instead of a particle
• It is not influenced by
the + or – charged plate.
• It has no mass whereas
the other 2 do.
Agenda 10/27
1. PD # 18 (3 Q’s, 1 review and 2 to assess prior
knowledge.) (7 min)
2. Notes/Discussion (Students will be re-introduced to
electron configuration models, Including Bohr Models)
(15 min)
3. Guided Practice (Instructor will model for students
creating Bohr models) (5-10 min)
4. Students will illustrate electron configurations using
Bohr models, of simple atoms in pairs. Instructor will
observe and assist struggling students. (15 min)
5. Some groups will show their models on the Prom
Board.
Panther Drill 18
1. What are the differnece between alpha and beta
radiation.
2. How many electrons are in a Carbon atom?
3. How do you show them in a Bohr Model?
Electron distribution
We will talk a lot more about electrons in a month or
so but lets look at how to create models of the
atoms showing electrons, protons, and neutrons.
Now in reality we know that the electrons exist in
electron clouds around the nucleus, but we will
use MODELS that show them in orbitals like the a
solar system. These are called BOHR MODELS.
Electron Cloud vs Bohr Model
CHLORINE
Electron Cloud
Bohr Model
Electron Orbitals
n=5
n=4
n=3
n=2
Orbitals are
abbreviated
as n.
n=1
Nucleus
There are
more than
can be as
many as 7
orbitals or
energy
levels.
Electron Orbitals
N=5
N=4
N=3
N=2
N=1
Level1 2 e32 eLevel2: 8e50 e18 eLevel3 18eLevel 4 32eLevel 5 50e-
8 e-
Nucleus
2 e-
Max
Electrons
for each n
level.
Lets try some
Atom with 3 protons
and 3 neutrons
Atom with 7 protons
and 6 neutrons.
Panther Drill # 19
1. What is the difference between the Bohr
model and the “more realistic” electron
cloud model?
2. What are valance electrons?
3. Is this Bohr model correct, if not why?
e-
e-
e-
5P
4N
e-
e-
e-
Valence Electrons
• The electrons in the outermost shell are the
valence electrons
• The valance electrons are the electrons on an
atom that can be gained or lost in a chemical
What element is
reaction.
this?
e-
How do you
know?
ee-
e-
ee-
Where are the
valence
electrons?
Volunteer or Victim
Circle the valence electrons
ee-
ee-
e-
e13 P
14N
e-
e-
ee-
eee-
e-
e-
Review of Bohr
n=5
n=4
n=3
n=2
n=1
Level1 2 e32 eLevel2: 8e50 e18 eLevel3 18eLevel 4 32eLevel 5 50e-
8 e-
Nucleus
2 e-
Max
Electrons
for each n
level.
Project
You will be assigned your choice of a poster project of
an atom or creating a 3-D Bohr model of an atom.
It is your choice the assignments can be seen in full
on the assignment sheet handout. When you have
decided then get a full handout that includes the
rubric, real quick let’s look at some examples of real
creative 3-D models from other students.
3D EXAMPLES
The basics of the projects can also be seen on the
front bulletin board if you can need them.
3-D Model Due Friday 11/5
• Your 3‐D model of your atom is DUE ON Friday 11/5.
• In addition to your 3-D model, you should include a short write up
that includes al of the following list:
• Element Name
• Atomic number
• Chemical symbol
• Metal/non‐metal/metalloid?
• State or phase at room temp.
• Uses
• Any interesting facts
• Characteristics or properties
• Number of electrons, neutrons, and protons
• The elements you have to choose from for the 3-D model are
Hydrogen through Argon on the periodic table. If you need to see
examples again go to website (Power Point Note section) and look
at the 3-D model Power Point.
Poster Due Wednesday 11/3
• Along with a Bohr model drawing of your atom your poster must
display the following information on the front so it can be seen:
• Element Name
• Atomic number
• Chemical symbol
• Metal/non‐metal/metalloid?
• State or phase at room temp.
• Uses
• Any interesting facts
• Characteristics or properties
• Number of electrons, neutrons, and protons
• Your choices for your Bohr Model atom posters are any atom from
sodium and higher in atomic number on the periodic table.
Exit Ticket
Name________________________________
ee-
ee-
e-
e13 P
14N
e-
e-
e-
e-
1. Circle the valence
electrons. What is their
function.
2. On the back sketch and
label a Bohr model of
Silicon or Magnesium
e-
ee-
Drop in basket before you
leave.
HAVE A GREAT DAY!!
Exit Ticket
Name________________________________
ee-
ee-
e-
e13 P
14N
e-
e-
e-
e-
1. Circle the valence
electrons. What is their
function.
2. On the back sketch and
label a Bohr model of
Silicon or Magnesium
e-
ee-
Drop in basket before you
leave.
HAVE A GREAT DAY!!
Panther Drill 20
Define valence electrons and state
their main job in the atom.
Heisenberg Uncertainty Principle
(review)
• The Heisenberg Uncertainty Principle says loosely - that you can't know with certainty
both where an electron is and where it's
going next.
• What it actually says is that it is impossible to
define with absolute precision, at the same
time, both the position and the momentum
of an electron.
Purpose
Electron configuration notation is a written and
visual and written method of noting every
thing we can about 1 given electron in an
atom’s ground state.
Ground state: the atom’s lowest most stable
energy state or condition. This the condition
represented on the periodic table.
Orbitals and principal quantum numbers
As we learned with Bohr models, n = the electron
energy levels or orbitals.
n is also referred to as the principal quantum level.
Trends
• As n increases, the orbital becomes larger and the
electron becomes farther from the nucleus.
• As n increases the amount of energy of the
electrons increase.
ADD THIS: The higher the quantum levels are less
stable than the lower levels.
In the Bohr Model
Principal Quantum Level 3
Sublevels
Principal energy levels contain energy
sublevels or orbitals.
(n=1) Principal energy level 1 contains 1
sublevel
(n=2) Principal energy level 2 contains 2
sublevels
(n=3) Principal energy level 3 contains 3
sublevels
Sub-levels
Sublevels are labeled s, p, d, or f
depending on their shape
S orbitals
s orbitals are spherically and symmetric
around the nucleus
P orbitals
A p orbital is rather like 2 identical
balloons tied together at the
nucleus.
P orbitals
At any energy level (or
n level) it is possible
to have 3 p orbitals
or sub-levels at right
angles to each other
P sub shell can have a
total of 6 e- (2 in
each orbital)
D sub level
“d” sub level has 5 orbital and can hold 10
electrons.
“d” does not start to get filled untill after 4s is filled.
F sub level
“f” orbital has 7 orbitals, and the first ‘”f”
orbital is seen in the 4th energy level.
4f does not begin to fill until after level 6s is
full.
Aufbau Principle
The Aufbau principle states that
each electron occupies the lowest
energy level available.
Start here and follow the
arrow
This is the
order they
fill up in.
Just follow
the arrow.
Hund's Rule
Within a subshell, the electrons will
occupy the orbitals by themselves
first, and will only pair up when
there are no longer any empty
orbitals available in that subshell.
Would you want to
share a room with
someone if you
didn’t have to?
The Pauli Exclusion Principle
This principle says that an orbital is filled when
it contains 2 electrons. After that, you have
to put the electrons in a different orbital.
Each type of subshell (sublevel) contains a
different number of orbitals. And, each
orbital can hold ONLY 2 electrons.
The Pauli Exclusion Principle
Subshell Type
# of Orbitals
Maximum # of
Electrons
s
1
2
p
3
6
d
5
10
f
7
14
1s
Write the notation this way
Carbon= 6 electrons
It fills like this
2s
2p
3s
3p
4s
The arrows point in
opposite directions in
each box because
they spin in opposite
directions because the
– charges repel each
other
3d
1s
2s
Write the notation this way
Why do the
fill each box
w/ one arrow
1st
2p
3s
The arrows point in
opposite directions
in each box
because they spin
in opposite
directions because
the – charges repel
each other
3p
4s
3d
Lets try some
1s
2s
2p
3s
3p
4s
3d
Panther Drill 21
1.How many electrons can be in each
ORBITAL ?
2.Complete the electron configuration for
Fluorine.
1s
2s
2p
Panther Drill #22
1. In what order do the following sublevels fill
up with electrons? 4s 3s 2p 3d 2s 3p 1s
2. How many valence electrons are in N and in
Mg?
Written Electron Configuration
After the standard orbital notation (boxes and
arrows), we need to know how use written
electron notation.
This is much simpler!
All you do is look at the boxes and write out
what is in them.
Written Electron Configuration
1s
2s
Write this as
follows:
1s22s22p3
2p
2p3
n or quantum
level
Sub
Level
Number
of
electrons
in the sub
level.
1s2 2s2 2p6 3s2 3p4
Write the
correct
electron
notation
and identify
the
element.
1s
2s
Atomic # 16
2p
S
Sulfur
3s
3p
4s
3d
4p
Write the
correct
electron
notation
and identify
the
element.
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p4
1s
2s
Atomic # 34
2p
Se
Selenium
3s
3p
4s
3d
4p
Panther Drill 23
In electron notation (not box and arrow
diagrams), write the notation for the
following elements:
a) Oxygen 1s22s22p4
1s22s22p6
b) Neon
c) Argon 1s22s22p63s23p6 4s23d104p6
Still a lot of writing?
We can use the Noble Gas Notation. Noble
gases come from group 18 on the periodic
table
Put the noble gas symbol in brackets [Ne] to
show that the all levels in it are full and
stable.
Then use notation to show the electrons in the
outermost orbital.
Try Magnesium in your notes
Mg = [Ne] 3s2
In your notes
Write the noble gas notation for:
Nitrogen
Calcium
Copper
Orbital Filling Periodic Table
1s
2s
2p
3s
4s
3p
4p
3d
5s
5p
4d
6s
6p
5d
7s
6d
7p when more discovered
4f
5f
Orbital Filling Periodic Table
Fill-in
GO TO ACTIVE INSPIRE
ELECTRON DOT
DIAGRAM
Electron Dot Diagrams
Because valence electrons are the ones that are
involved in CHEMICAL BONDING, we often
represent them in a visual short-hand called
electron dot diagrams or Lewis diagrams.
These are simple to do, they only show the valence
electrons. So for the simplest atoms like we will
look at
Lewis or electron Dot Diagrams
Here is an example:
Phosphorus has how many valence electrons? 5
Fill in the Electrons in this order.
4th e3rd
e-
7th
8th
He
2nd
e-
6th
1st
5th
e-
Panther Drill
Take a few minutes to either study or add
to your cheat sheets. If you can do this
reasonably quietly, you can have up to
10 min. As soon as it becomes too loud,
you will not have any more time and we
will start the test.
Notebooks for unit 2 will be checked after
you turn your test in.