Download Electron

Matter
Make a “Matter” title page in toolkit:
•Properties of Matter-Physical and Chemical
•Phases of Matter
•Atoms
•Elements, Molecules, and Compounds
•Periodic Table of Elements
Priority Standards
Learning Targets
Proficiencies
Matter Pre/Post Assessment
Complete the pretest quietly on your own,
trying your best!
Sit quietly until everyone is finished.
Correct pretest as a class using a different
colored writing utensil.
Matter
Open thin, blue textbook titled “Matter” to
Chapter 1. Read the introduction page
silently to yourself.
Next look at ALL pictures/diagrams in the
chapter READING ALL captions.
Title next page in toolkit “Basics of Matter”
Basics of Matter (Toolkit Entry)
Define each of the following words (4 flipper or this chart):
Matter
anything that has ______ and takes up
space (_______)
Law of
Conservation _____ cannot be created nor destroyed
of Matter
Chemistry
the study of _______
Phases
a change in ____ or condition of _____
Make a “ Matter” keeper pocket for this
unit, and glue in on the next page.
Matter
Open thin, blue textbook titled “Matter” to
Chapter 2. Read the introduction page
silently to yourself.
Next look at ALL pictures/diagrams in the
chapter READING ALL captions.
Return to the Section 1 and quietly read
the whole text to yourself.
Title the next page in your toolkit “Laws of
Gases”
Matter
Open thin, blue textbook titled “Matter” to
Chapter 2. Read the introduction page
silently to yourself.
Next look at ALL pictures/diagrams in the
chapter READING ALL captions.
Return to the Section 2 and quietly read
the whole text to yourself.
Title the next page in your toolkit “Phase
Changes Vocab”
3 Common
States of Matter
on Earth
Gas
•No definite _______
•No definite _______
•Molecules move _______
•Molecules are _______ ____
•Steam (draw picture)
Liquid
•No definite _______
•Has a definite _______
•Molecules move _______
•Molecules are a little _______ ____
•Water (draw picture)
Solid
•Definite _______
•Definite _______
•Molecules move _____ ________(vibrate)
•Molecules are _____ ________
•Ice (draw picture)
4th Phase of Matter
Plasma
•No definite _______
•No definite _______
•Atoms move very _______
•Atoms are very _____ ________
•The most common form of matter in the universe
•EXTREMELY HOT!!!!
Laws of Gases
Boyle’s Law
Describe this law
Draw a diagram.
Charles’s Law
Describe this law
Draw a diagram.
Phase Change Lab
You will be working with your shoulder partner.
Half of the team will complete the lab, while the
other half complete notes in toolkit.
Teams will switch roles half way through class.
Phase Changes Vocab
Term
Freezing
Freezing
Point
Melting
What’s Happening
Energy-Remove or Add
(Solid/Liquid/Gas/Temperature) Temperature- Change or Not
_______ changing to _____
Energy _________
the specific ____________
each type of matter changes
from a _______ to a ______
Energy _________ BUT NO
______________ CHANGE
_____ changing to _______
Energy _________
the specific __________ each
Melting Point type of matter changes from
______ to _________
Boiling
________ changes to _____
throughout the liquid
the specific ____________
Boiling Point each type of matter changes
from ________ to ______
Energy _________ BUT NO
______________ CHANGE
Energy _________
Energy _________ BUT NO
______________ CHANGE
Phase Changes Vocab (Con’t)
Term
Evaporation
Vaporization
Condensation
Sublimation
Frost Formation
What’s Happening?
Energy
______ changes to ___ Energy _________
at the surface at any
temperature
______ changes to ___ Energy _________
at boiling point
___ changes to a ____
Energy _________
______ changes
straight to a ____
Energy _________
____ changes straight
to ______
Energy _________
Phases of Matter Graphic Representation
Plasma
Gas
Liquid
Solid
Particle Movement
Particle Movement
Particle Movement
Phases or States of Matter
 Discuss what the molecules or atoms are doing
in each of the 3 phases of matter.
Phase Change Worksheet
Complete the Phase Change Worksheet.
It will be turned in for a grade at the
beginning of the next class (Lunch
Academy Assignment).
Properties of Matter
(2 Long Flippers)
Properties are the characteristics to
describe matter.
2 Types of Properties
Physical
Chemical
Physical Properties
 Color, Texture, Mass, Volume, Weight, Temperature
 Density- d=m/v amount of ______ in a ______
 Buoyancy- how well an object ________
 Viscosity- how fast matter will _______
 Solubility- how well matter _________
 Elasticity- how well matter _________
 Brittleness- how easily matter _________
 Hardness- how well matter does not _________
 Ductile- how well can it be made to a thin ______
 Luster- ________
 Malleability- how well can it be made to a thin ______
Chemical Properties
Corrosive- matter that gradually wears away
_________
Flammable- how well matter ________
Combustible- how easily matter ______ to burn
Reaction rate- how fast matter _______ with
other matter
Ease or not of bonding- how easily matter
______ together
Conductivity- how well matter lets _______
and/or _________ flow through it
Physical Changes
No new substance made- still same
substances with same properties.
Can be separated by physical means
Sorted
Filtered
Magnetism
Spinning
Phase change
Gravity (separates over time)
Evidence of Chemical Change
New substance made
Color Change
Heat given off or removed from
environment
Light given off
Change in odor
Gas given off
Precipitate made (solid made)
Physical or Chemical Change Lab
Travel with your team to each station
Read the directions at each station
Record observations BEFORE completing
the task
Record observations AFTER completing the
task
Decide if the task resulted in a Physical
change or a Chemical change.
Return each station to it’s ordered state.
Assessment
Physical and Chemical Changes:
Properties of Matter (worksheet)
Classifying Matter
Six Flipper or Chart
Atom
 Basic unit of all matter.
Molecules
Elements
Matter that can not be broken down into
anything simpler, by simple means.
A pure substance or the same through out.
All are on the Periodic Table of Elements-all
the types of atoms.
Compounds
Matter that is made of 2 or more elements
that are chemically bound. Ex: NaCl
A pure substance or the same through out.
Ex: NaCl (Table Salt)
Mixtures
Matter made of 2 or more other types of matter that is NOT
chemically bound.
Can be separated by physical means.
May or may not be the same through out
-Homogeneous- same through out Ex: Salt water
-Heterogeneous- different through out Ex: Milk
Types of mixtures
Suspensions-large particles and settles out (Italian Dressing)
Colloid-Medium particle and settles out (Jello, paint, milk)
Solution-minute particles don’t settle out (Salt water)
Alloy-metals mixed together (Brass)
Solutions
Homogeneous mixture, usually in liquid
form
-Solvent- the substance that
dissolves the solute Ex: Water
-Solute- the substance that is
dissolved Ex: Salt
Review Sheets
Heterogeneous vs. Homogeneous Mixtures
Solutions, Compounds, Mixtures
Review of Classifying Matter
Matter
Is it uniform throughout?
No
Yes
Homogeneous
mixture
Can it be separated by physical means?
No
Yes
Heterogeneous
mixture
Pure Substance
Can it be decomposed into other
substance by a chemical process?
No
Element
Yes
Compound
Homogeneous
Mixture (solution)
Review Classification of Matter Activity
 Find the 3 title strips-Element, Compound, and
Mixture
 Make 3 columns with the title strips.
 Deal out the strips of paper with examples to
each team member evenly.
 WithOUT team input, each member places their
examples under the appropriate title.
 Once all examples are out, then team mates can
start to discuss and support their thoughts with
evidence.
 Key will be revealed, make corrections and copy.
Classifying Activity Key
Compounds
Elements










Gold
Copper
Helium
Sodium
Barium
Francium
Lithium
Sulfur
Carbon
Argon
o
o
o
o
o
o
o
o
o
o
Water
Ammonia
Carbon dioxide
Sugar
Table salt
Carbon monoxide
Ozone
Cholesterol
Glucose
Copper sulfate
Mixtures
o Milk
o Coffee
o Air
o Ink
o Blood
o Sand
o Soil
o Aluminum foil
o Chocolate Chip Ice
Cream
o Paint
History of the Atomic Model
History of the Atomic Model
Timeline foldable:
Fold the strip of paper in half, then “burrito” fold it
into three equal sections. (total of 6 sections)
Label the first section “The Atomic Model”
Each of the remaining 5 sections should then include
the information on each screen:
Name
Year
Diagram of the model
Major facts
History of the Atomic Model
All elements are made of
atoms, which cannot be
divided or destroyed.
 “Billiard Ball” theory –
atoms are tiny particles
Atoms of the same elements
are alike, and different from
John Dalton
other element’s atoms.
(1766-1844)
(1856-1940)
J.J. Thomson
Atoms had even
smaller, “subatomic”
particles.
Subatomic particles
had a charge (+ or -).
Plum Pudding = Atoms
as a positively-charged
“pudding” with
electrons (-) scattered in
it.
Ernest
Atoms have lots of empty
Rutherford space!
(1871-1937) 1st model to show a nucleus.
Positively-charged particles
are in the nucleus (center) of
an atom.
Negatively-charged particles
are around the atom’s edge.
Neils Bohr Added to Rutherford’s
(1885-1962) model.
“Planetary Orbit” model Electrons orbit around an
atom’s nucleus, like the
planets around the Sun.
Wave Model Atoms have a nucleus with
(Current) protons (+) and neutrons
(neutral)
The nucleus is surrounded
by electrons (-).
Electrons don’t follow a set
orbit. We can only predict
their locations.
Subatomic Particles:
Parts of atoms!
3 Sided Pyramid Foldable
 Fold a top corner down to the side to make a triangle
 Unfold and repeat opposite direction.
 Before unfolding fold bottom section for anchor.
 Unfold and cut 1 angle fold to the center.
 Mark 1 triangle with the word “glue”
 Write the title on the anchor and complete the notes
for each side.
 Spread a small amount of glue on the triangle marked
“glue” and tuck it inside the pyramid and stick
together.
 Finally, glue the anchor down into your toolkit.
Additional vocab
Subatomic particles- particles that make up an
atom
Electron
Proton
Neutron
*Protons + Neutrons = Atomic Mass
Proton
A positive (+) particle within the
nucleus (center) of an atom.
Electron
A negative (-) particle that orbits
the nucleus (outside of the
nucleus) of an atom in what’s
called an electron cloud.
Neutron
A neutral (no charge or +/-)
particle in the nucleus (center) of
an atom.
Subatomic Particles
A positive (+) particle within
the nucleus (center) of an
atom.
Neutrons A neutral (no charge or +/-)
particle in the nucleus (center)
of an atom.
Electrons A negative (-) particle that
orbits the nucleus (outside of
the nucleus) of an atom in
what’s called an electron
cloud.
Protons
Isotopes
Isotope- atoms of the same element that
have different numbers of neutrons in the
nucleus.
C12 and C14
Forces Within the Atom
(Toolkit page title)
Multiple shutter fold
Hold your paper horizontally and burrito
fold (2 folds/make 3 equal sections)
Unfold the burrito and turn upside down,
so the folds make 2 “mountains”.
Fold the 2 end sections in half
Fill in your notes using the 4 sides
Glue down the back middle section.
Electromagnetic Force
Repels particles of the same force.
Attracts particles of the opposite force.
+
N
+
-
N
Strong Force
Attracts particles of the same charge when
they are close together. This keeps
protons together in the nucleus of the
atom.
+
N
+
N
Weak Force
The force responsible for radioactive
decay, where a neutron turns into one
electron and one proton.
N
+
-
Gravity
Force of attraction between all objects in
nature
The Periodic Table of Elements
https://www.youtube.com/watch?v=zUDDiWtFtEM
http://www.search.ask.com/search?o=100000031cr&gct=kwd&q=periodic+table+elemen
ts+songs&tpr=10&ctype=videos
Vertical columns: Groups or Families (# of valence electrons)
Dimitri Mendeleev: Creator of the
6
Atomic Number:# of Protons or Electrons
C
Carbon
12.011
Element Symbol: 1st Capital 2nd Lower Case
Element Name
Atomic Mass: # Protons + # Neutrons
Key
Metals
Metalloids
Non-Metals
Horizontal rows: Periods (# of shells of electrons)
Classifying the Periodic Table
Metals
Metalloids
Non-Metals
Metals
Cu
Cr
Metals
Ag
Au
Metals
Physical Properties
•Luster or shine
• Conduct heat and
electricity
• Ductile (can spread
thin)
• Malleable (can be
shaped)
Chemical Properties
• Lose electrons
• Corrode, or wear
away
Metals
Na
W
http://www.youtube.com/watch?v=sXanNFGY1kA&feature=related
Non-metals
Ne
He
Non-metals
Physical Properties
No shine or luster,
dull in appearance
Chemical Properties
Gain electrons when
bonding
Not good conductors Noble Gases are nonof heat or electricity. reactive
Brittle and break
easily
Non-metals
Nitrogen
http://www.youtube.com/watch?v=MaxZwsqs
tFs
Hydrogen
http://www.youtube.com/watch?v=DbmV5lM4
z74&feature=related
Metalloids
As
Si
Metalloids
Physical Properties
Chemical Properties
•Solids that are shiny or
dull
•Ductile and malleable
•Semiconductors
•Properties of both
metals and non-metals
Reading the Periodic
Table
Reading the Periodic Table of Elements
6
C
Atomic Number:# of Protons or electrons
Element Symbol: 1st Capital 2nd+ Lower Case
Carbon Element Name
12.011 Atomic Mass: # Protons + # Neutrons
Putting it all together
6
C
12.011
Atomic Number:
Atomic Mass:
Element Symbol:
Number of Protons:
Number of Neutrons:
Number of Electrons:
Putting it all together
8
O
15.999
Atomic Number:
Atomic Mass:
Element Symbol:
Number of Protons:
Number of Neutrons:
Number of Electrons:
Putting it all together
26
Fe
55.847
Atomic Number:
Atomic Mass:
Element Symbol:
Number of Protons:
Number of Neutrons:
Number of Electrons:
Periodic Table Vocabulary
Atomic Number
Number of
_________ in
each atom of an
element
Number of
_________=
Number of
_________
Atomic
Mass
The number
of ________
and
__________
_ together
in the
nucleus
Atomic Symbol
1-3 __________
abbreviation for
an element.
The first letter is
___________ and
the next letter(s) is
__________
Chemical Bonding
The combining of atoms to create a new substance.
Electron Mapping
 Electrons orbit the nucleus of an atom in an electron
cloud.
 The electron cloud is made of energy levels,
depending on how many electrons.
 Each energy level can only hold a certain number of
electrons, energy levels start around the nucleus.
1st Energy Level can only hold up to 2 electrons
2nd Energy Level can only hold up to 8 electrons
3rd through unlimited energy levels can only hold up
to 18 electrons
 The outer most level of electrons that are used for
bonding are called valence electrons.
How to fill the energy levels
 Start with the 1st (inner) level and
work your way outward.
 Let’s map N (Nitrogen), Ni (Nickel),
and then Si (Silicon)
1st Energy Level:
2 electrons
2nd Energy Level:
8 electrons
4th and more
Energy Levels:
18 electrons
Valence electrons: ______
http://www.brooklyn.cuny.edu/bc/ahp/SDP
S/SD.PS.electrons.html
M&M Electrons
N
How to fill the energy levels
 Let’s do this on paper! Ex: Ti
(Titanium)
 1. Map Nitrogen
 2. Map Nickel
1st Energy Level:
2 electrons
2nd Energy Level:
8 electrons
4th and more
Energy Levels:
18 electrons
Valence electrons: ______
Chemical Bonds
Foldable: 3 sided pyramid
Anchor title: 3 Types of Chemical Bonds
Ionic (Giving/Taking) Bonds
 One atom loses an electron to make it positively
charged.
 The other atom gains an electron to make it
negatively charged.
 The positive and negative charges attract,
forming an ionic bond.
Covalent (Sharing) Bonds
 Two or more nonmetal atoms are in
need of electrons to
fill their outer energy
levels.
 The atoms decide to
share electrons.
 This “sharing of
electrons” is the
definition of a
covalent bond
Metallic (free-moving) Bonds
The electrons become property of all the
atoms.
Electrons are not tied to their nucleus alone.
Ions
Electron Affinity- Tendency (or desire) to attract
electrons
Ion-An atom or atoms that have lost or gained
electrons, thus having a charge.
+cation -anion
Ionization Energy- The energy it takes to form
an ion.
Chemical Bonding Vocabulary (6 Flipper)
Chemical Bonding
Combination of ______to form new
__________
Valence Electrons
Electrons in the ___________ energy level
of an ________
Ionization Energy
The energy it takes to ______ an ion.
Electron Affinity
Tendency (or desire) to _________ electrons
Ion
An atom or atoms that have _______ or
_______ electrons, thus having a charge.
+_____ -_____
Oxidation Number
The number of __________ an atom gains,
loses, or shares when it forms ______ bonds
Chemical Formulas and Equations
Chemical Formulas and Equations
Chemical Formula- symbols and numbers to
represent atoms and/or molecules. Ex: H2O
Chemical Equation- represents chemical reactions.
Ex:
2 H2 + O2  2 H2O
Co-efficient
2 H2 + O2  2 H2O
Subscripts
Reactant:
What goes in.
2 H2 + O2  2 H2O
Hydrogen + Oxygen  Water
Product:
What comes out
Equation Examples
Fruit Salad:
Strawberries + Apples + Grapes  Fruit Salad
Tuxedo:
Jacket + Shirt + Bowtie  Tuxedo
ABC’s where A and B bond together:
A + B + C  AB + C
Salt:
Sodium + Chlorine  Salt
Photosynthesis:
6CO2 + 6H2O + Energy  C6H12O6 + 6O2
Cellular Respiration:
C6H12O6 + 6O2  6CO2 + 6H2O + Energy
Oxidation Numbers
and
Chemical Bonding
Reminders about chemical bonds:
Covalent bonds: Occur between
non-metals, where atoms share
electrons
Ionic bonds: Occur between metals
and non-metals, where one atom
gives up electrons and another atom
takes electrons
How chemical bonding works
Atoms either share or give/take
electrons.
Atoms work together to become stable
and fill their energy shells.
Example: Covalent bond – HCl
Oxidation numbers: H= +1
Cl = -1
Cl
H
How chemical bonding works
Example: Ionic bond – KCl
Oxidation numbers: K= +1
+
Cl = -1
-
Oxidation Numbers
Oxidation Number: The number of
electron(s) an atom gains, loses or
shares when it forms chemical bonds
Examples:
O -2
Oxygen’s oxidation number is -2
because it wants to take two electrons
Chemical Reactions
Chemical Reaction Vocab
Chemical Reaction
Process where substances undergo
______ and chemical
_______ changes, resulting
physical
in a newsubstances
________ with new _________.
properties
Catalyst
Substance that _______
speeds up chemical
reactions ______
without being used up itself
Exothermic
Chemical reaction where heat energy
is _________
released (Heat _____
exits the
reaction so it feels _____).
warm
Endothermic
Chemical reaction where heat energy
is _________
_____ the
absorbed (Heat enters
reaction so it feels _____).
cool
Chemical Reaction Labs
Hot or Not
Ice Ice Baby
Understanding a Catalyst
 Catalytic Oxidation Demonstrations
Catalytic oxidation
 Demonstration:
A penny is heated to glow red-hot and hung over acetone.
https://www.youtube.com/watch?v=TWF0-jIdU-0
 Observations:
The penny glows until all of the acetone is consumed.
 Explanation:
The copper penny catalyzes the oxidation of the acetone to its combustion
products of CO2 and H2O. However, although the combustion products are
being formed, keep in mind that combustion itself is not taking place. The
copper is simply providing a catalytic surface for the acetone to react upon.
 The copper, being a catalyst, is not expended during the reaction.
What Happened – Hot or not?
Calcium Chloride + Sodium Bicarbonate =
Sodium Chloride + Calcium Carbonate +
Carbonic Acid
Carbonic Acid breaks down to water and
CO2
 Phenol Red turns yellow in acids and red in
bases
What happened – Ice Ice Baby
The reaction feels cold because the
energy (heat) is absorbed by the
reactant (sodium bicarbonate).
Acids and Bases
Acids vs. Bases
Acids
(Acidic)
Bases
(Alkaline)
Form an _________
hydrogen ion
(___)
H+ in water
- Ex. HCl and H3PO4
hydroxide ion
Form a ___________
(___)
OH- in water
- Ex. NaOH and NH4OH
sour in foods
Taste _______
bitter
-Taste _________
in foods
slippery
-Feels _________
donor
Called a “proton _______”
acceptor
Called a “proton ________”
The pH Scale
pH Measures
the acidity of a
solution
Neutral
pH Scale
Less than 7 = Acid
Water = 7 = Neutral
More than 7 = Base
Acid or Base?
HCl
H3BO3
HC2H3O2
Ca(OH)2
NaOH
NH4OH
KOH
H2SO4
H2CO3
HNO3
H 3 C 6H 5O 7
Mg(OH)2
H3PO4
Al(OH)3
What does salt and water have to
do with acids and bases?
Can you figure it out?????
HCl + NaOH  (H+) + (Cl-) + (Na+) + (OH-)
HCl + NaOH  H2O + NaCl
Acid + Base  Water + Salt
Acid/Base Lab
Acid/Base Lab Review
1. If a solution has a pH of 14, is it an acid
or base?
2. If a solution has a pH of 3, is it an acid or
base?
3. Is HCl an acid or a base?
4. Is NaOH an acid or base?
5. Why are acids called “proton donors”?
Ticket to Lab
You must have the
Acid/Base Lab notes
complete before you
begin the lab!
Materials List:
 1 tube of pH stripes with key
 1 apple slices
 1 orange slices











1 small cup of baking soda solution
1 small cup of water
1 small cup of milk
1 small cup of dishwashing detergent
1 small cup of ammonia
1 small cup of salt solution
1 small cup of sugar solution
1 small cup of apple cider vinegar
1 small cup of vinegar
1 small cup laundry starch
12 small cups
Testing pH Procedure
1. Write down the name of the solution you are
testing in the first column.
2. Dip one end of your litmus paper into the
solution.
3. Record observations and any changes in
color of the litmus paper under
“Observations”.
4. Write the pH that matches the color of the
litmus paper.
5. Record if the solution is an acid or base.
Solution Samples
Apples
Orange
Baking Soda
Tap Water
Milk
Dishwasher Detergent
Ammonia
Salt Water
Sugar water
Apple Cider Vinegar
Vinegar
Starch
Clorox Bleach
Saliva
Acids and Bases Videohttp://app.discoveryeducation.com/player/view/assetGuid/410F287B-55FA4A7A-BE2A-14E9B813F994