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Pre-read Chapter 16 Section 1
 Write 3 important facts, in complete sentences,
about each state of matter that would help you
answer the lesson essential question.
 Number each fact!
 Write 2 Questions that you still have over the
reading.
 This will count as your reflection tonight!
Grab your folder!!!!
Have out reflections/notes from yesterday to be
stamped!
 Look at the display in front of the room…
 Describe, in complete sentences, what you see
in each box.
 Ask the people at your table your 2 questions
and see if they can answer them.
Work on Test corrections when you are
finished!!!
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Bell Ringer 09/06/2012
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Write Question and Answer
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What is capillary action?
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Bell Ringer 09/07/2012
Describe and illustrate the physical
differences among solids, liquids, and gases
in terms of their mass, volume, density,
shape, and particle arrangement.
UEQ: How does the structure of matter influence its physical and chemical
behavior?
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Choose 1: How to do
Vocabulary:
 Write word and definition.
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Underline and highlight
vocabulary word.
Write word on front and
definition on back of index
cards.
Create a poem or rap of
vocabulary words and
definitions.
Create foldable with words
and definitions.
Create a crossword puzzle.
Also make answer key!!!
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Kinetic theory
Property
Density
Physical property
Chemical property
Matter
Volume
Physical change
Chemical change
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What are the 3 assumptions to kinetic theory?
All matter composed of small particles
(atoms, molecules, ions)
Particles are in constant random motion
Particles are colliding with each other and the
walls of their containers
Overall, kinetic energy is how fast the
molecules are moving and will do so at all
temperatures.
Solids
Holds shape! Why?
Definite shape and Definite volume
Not compressible (naturally) because packed tightly
Usually most dense phase of a substance because
packed tightly
 Exception: water
 Definite melting points. Least amount of energy.
Movement of particles is slow and around fixed
points; but, increases with increase in temperature.
 Low rate of diffusion b/c low mobility of particles
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Two types of Solids
Crystalline solid
 Particles are in an orderly, geometric, repeating
pattern
 Have definite melting points
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Amorphous solid (plastics and glass)
 Particles are arranged randomly
 No definite melting points
Liquids
Definite volume but no definite shape
Take shape of container
Particles free to move/slide past one another;
but, still held together by intermolecular forces
 Cannot be compressed under common pressure
 Can transmit pressure equally in all directions
 Usually less dense than solids; but, more dense
than gases
 Diffuses at average speed
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Bell Ringer 09/07/2012
Write Question and answer in a complete
sentence.
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Explain what happens in surface tension.
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Surface Tension
 Drawing molecules together to decrease surface area
 Predict: How many drops of water do you think will fit
on a penny? Was your prediction correct?
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Capillary Action
 When surface of a liquid and solid meet, surface of
liquid molecules are pulled upward, against the pull of
gravity, along surface of solid
 Meniscus
 Observation: What is reading on the graduated
cylinder?
Gases
No fixed shape, no fixed volume
Too much energy to remain attached. Particles
vibrate at high speeds.
 Gas takes shape of container by expanding
 Less dense than solids and liquids
 Still considered a fluid
 Can be compressed easily with very little
pressure. However, once it is contained, it want
to escape the container.
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Diffusion
Spontaneous mixing of particles of two
substances caused by random motion
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Plasmas
Once molecule is superheated, electrons
leave the atoms in the molecules
+/- charged particles
Stars, lightening bolts, neon/fluorescent
bulbs, auroras
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Exit slip
State of matter with indefinite volume and
indefinite shape
State of mater with definite volume and
definite shape
State of matter with definite volume and
indefinite shape
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Homework:
 Continue to work on Vocabulary. Due Tuesday!
 Write Questions and Answers
▪ Pg. 483 #’s 1, 2
▪ Pg. 500-501 #’s 5, 8, 12, 16
▪ Pg. 502 #s 1, 4, 6, 19
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Bell Work 09/11/2012
First, write LEQ above.
Write Questions and Answer
What are the appropriate units for mass,
volume, and density?
How do you calculate density?
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Mass = kg, g
Volume = cm³, m³
Density = g/cm³, g/L, g/mL, kg/L, kg/m³
D = M/V
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Writing a lab report.
Follow the template
Keep template in reference section of
notebook.
Use water displacement to obtain Volume
-or- calculate mathematically
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 Remember that 1 cm³ = 1 mL
 To calculate volume of cylinder:
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Use triple balance beam/electronic balance to
measure the mass of object
You should have out your lab papers,
the reference sheet on how to write
a lab report and a separate sheet of
paper to write out your lab report!
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Bell Work 09-17-2012
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Write Question and Answer
What do you think a density column is?
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Some liquids are denser than others
When you layer them, the denser liquids will
sink to bottom
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Some liquids are denser than others
When you layer them, the denser liquids will
sink to bottom
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Write the following
information and
calculate the density:
Water
 volume: 1.5 mL
mass: 1.5g
 Vegetable oil
 volume: 1.5 mL
mass: 1.38 g
 Dish soap
 volume: 1.5 mL
mass: 1.59 g
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Rubbing alcohol
 volume: 1.5 mL
mass: 1.22 g
 Lamp oil
 volume: 1.5 mL
mass: 1.20 g
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Bell Work 09-18-2012
Write Question and Answer
Observe the magnesium strip.
What are some physical properties of
magnesium? What are some chemical
properties?
Propose a way you could physically change
the magnesium strip and one way you
could chemically change the magnesium
strip.
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What is a property?
A unique characteristic that categorizes
(groups or identifies) objects/substances
together
PHYSICAL PROPERTIES
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Characteristic observed
or measured without
changing substance
Melting point, boiling
point, color, size,
ductility, malleable,
density, ability to
conduct heat or
electricity
CHEMICAL PROPERTIES
Ability to change from
one substance to a
new substance
 Ability to produce a
gas, burn, rust
 Example: Copper w/
moist air
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PHYSICAL CHANGES
CHEMICAL CHANGES
does not change the
identity or chemical
makeup of the
substance
 Cutting, melting,
drawing into wire,
crushing, temperature
and pressure changes
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Substance changes into
new substance b/c
chemical bonds have
been broken or made
Occurs on molecular
level
Noticed by temperature
change, smell/odor,
bubbles (gas), rust
formation
Reactants products
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PREDICT:
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Write down a prediction of what you think
will occur upon mixing lead nitrate and
potassium iodide.
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Extra Credit: (3 points to test grade)
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Search the internet for important uses of
Potassium Iodide. Write down any important
uses and turn in tomorrow.
Also, while you are searching the internet,
see if you can find why Potassium Iodide
should be stored in a closed amber colored
bottle.
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Bell Work 09-19-2012
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Write question and answer.
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Explain how you could you prove the Law of
Conservation of Mass.
Law of Conservation of Mass
Mass cannot be created or destroyed
in ordinary chemical and physical
changes
 Therefore, the mass before the
reaction will be equal to the mass after
the reaction
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Homework Assignment:
Pg. 465 #’s 1-5
Pg. 470-471 #’s 4, 8, 10, 13-16
 Pg. 472 #’s 4, 6, 7
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LEQ: When temperature changes, how are
the 4 states of matter affected?
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Vocabulary
 Write word and definition.




Underline and highlight
vocabulary word.
Write word on front and
definition on back of index
cards.
Create a poem or rap of
vocabulary words and
definitions.
Create foldable with words
and definitions.
Create a crossword puzzle
using words and definitions.
Also make answer key!!!
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Kelvin
Celsius
Fahrenheit
Boyles Law
Charles’ Law
Bernoulli’s Principle
Archimedes Principle
Pascal’s Principle
Fluid
Freezing point
Boiling point
Melting point
Phase diagram
Law of conservation of
energy/mass
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Bell Work 09-20-2012
Write question and answer.
Explain the difference between evaporation
and vaporization.
Evaporation is liquid leaving the surface
without reaching boiling point. Vaporization
is liquid becoming vapor due to boiling.
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Energy is required to change the states of
matter!
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Phase Changes of Matter
Sublimation (dry ice, iodine)
Melting (heat of fusion)
Vaporization (“boiling” heat of vaporization)
Condensation (dew)
Solidification (freezing, crystallization)
Deposition (fire extinguisher)
GAS
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Matter exists in
gaseous state at room
temp
VAPOR
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Matter is in gaseous
state; but, normally in
liquid state at room
temp
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Avg KE doesn’t change at plateau, this is
potential energy where atoms/molecules are
rearranging
Lower plateaus should be shorter because it
takes less energy to change state
Slopes – kinetic energy
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What is equilibrium?
2 opposing changes occur at equal rates in a
closed system.
Occurs at plateaus
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Boiling point
 Temp at which vaporized pressure = atmospheric
pressure
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Freezing point
 Temp at which solid and liquid are in equilibrium
at 1 atmospheric pressure
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Exit slip:

Sum up today’s lesson in 6 words!!!
Bell Work 09/21/2012
Write Question and Answer
Explain the relationship between heat of fusion of
a solid and the attraction between the particles.
The greater the attraction between the molecules
results in greater amount of energy needed to
overcome the attraction -or- higher heat of
fusion
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Phase Diagram
A graph of the relationship b/t the physical
state of a substance and the temperature and
pressure of the substance
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What is triple point?
Temperature and pressure conditions where
all 3 states of matter exists together at
equilibrium
What is critical point?
The temperature and pressure at which the
gas and liquid states of a substance become
identical and form one phase
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Particle of liquid cannot escape due to air
pressure pushing down on surface of liquid
When liquid particles gain enough KE (from
heat) to break through the surface, the liquid
boils. This can also occur by decreasing the
amount of pressure.
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Buoyancy-ability of a fluid to exert an
upward force on an object that is immersed in
it
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1. float if weight is less than the buoyant
force from the fluid
2. sink if its weight is more than the buoyant
force from the fluid
3. Archimedes’ principle – buoyant force on
an object is equal to the weight of the fluid
displaced by the object
4. float if its density is less than the density of
the fluid it is placed in
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Pascal’s principle: Pressure applied to a fluid
is transmitted throughout the fluid
 Pressure is force exerted/unit area (P= F/A)
 Force = Newtons
Area = m
 Hydraulic machines use this principle to lift heavy
loads (this is because more force is available to lift
a heavy load by increasing the surface area)
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Bernoulli’s principle- as velocity of a fluid
increases, the pressure exerted by the fluid
decreases; airplanes use this principle to fly
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Viscosity – a liquid’s resistance to flow
 1. molecular structure determines a fluid’s
viscosity
 2. increased temperature will lower viscosity
 Low viscosity – thin
 High viscosity - thick
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Pressure
 Is measured in units called pascal (Pa)
 1. collisions of particles in air result in atmospheric
pressure.
 2. Moving particles colliding with the inside walls
of a container result in gas pressure and push the
walls of the container outward
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Boyle’s Law-relates pressure and volume
 Volume decreases as pressure increases
 Pressure decreases as volume increases
 Pressure multiplied by volume is always equal to a
constant if the temperature is constant
 Pg. 493 practice problem
 Pg. 841 numbers 174 and 176
 http://www.grc.nasa.gov/WWW/k-
12/airplane/boyle.html
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Charles’s Law-relates volume and
temperature
 At constant pressure, volume increases as
temperature increases
 At constant pressure volume decreases as
temperature decreases
 http://www.grc.nasa.gov/WWW/k12/airplane/glussac.html
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Either an element or a compound
A type of matter with a fixed composition
Element
 All the atoms in a substance are alike
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Compound
 A substance with 2 or more elements combined in
a fixed proportion
▪ Example: water, chalk
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Two or more substances that can be easily
separated by physical means
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Heterogeneous
 Mixture of different and easily distinguishable
materials
▪ Colloid-large particles that never settle (ex. Milk, paint)
▪ Tyndall effect-scatter light
▪ Suspension- containing a liquid in which visible particles
settle (ex. Pond water)
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Homogeneous
 Contains two or more gaseous, liquid, or solid
substances blended (also called a solution)
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Physical Properties
 Characteristics of a material which can be
observed without changing the identity of the
substances in the material
 Ex: color, shape, size, melting point, and boiling
point
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Appearance
 Physical description of a substance
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Behavior
 How the substance acts; for example magnetism,
viscosity, ductility
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Physical properties such as size and
magnetism could be used to separate
mixtures
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Changes in a substance’s size, shape, or state
of matter
Substance does not change identity
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Distillation
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 A process for separating a mixture by evaporating
a liquid and condensing its vapor
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Chemical Property
 Characteristics of a substance indicating that it
can change chemically
▪ Example: flammability or light sensitivity of a substance
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When a substance changes to another
substance, a chemical change has occurred.
 Indicated by temperature change, smell, or
bubble formation
 Rust
 Chemical changes can be used to separate
substances such as metals from ores
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Weathering of Earth’s surface involves
physical and chemical changes
 Physical – big rocks split into smaller ones, erosion
 Chemical – in rocks when calcium carbonate in
limestone changes to calcium hydrogen
carbonate due to acid rain
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Mass of all substances present before a
chemical change equals the mass of all
substances after the change