Instructions:
• You will work through the presentation
and answer any questions posed, and
filling out any missing material in your
itinerary
• Just click through the presentation
using the arrows.
Lab 1
Lab 2
WOODY, YOUR GUIDE:
“Hi, I’M YOUR GUIDE.
MY NAME IS WOODY. WE’RE
GOING TO EXPLORE ENERGY
AND MATTER TOGETHER.”
“AS WE EMBARK ON THIS
ADVENTURE YOU NEED TO READ
ALL THE INFORMATION PRESENTED,
FOLLOW ALL THE DIRECTIONS GIVEN,
THINK ABOUT THE QUESTIONS
POSED, AND FILL OUT YOUR
TRIP PLANNER.”
“LET’S GET STARTED!”
“What is this energy thing?”
“ENERGY IS THE
CAPACITY TO DO WORK,
OR TO PRODUCE HEAT.”
“Energy …”
“MAYBE YOU HAVEN’T
THOUGHT MUCH ABOUT IT,
BUT EVERYTHING WE DO,
AND EVERYTHING WE
HAVE REQUIRES ENERGY.”
“WITHOUT ENERGY WE COULD
NOT ACCOMPLISH ANY OF THE
COUNTLESS TASKS THAT MAKE UP
OUR DAYS.” “YIKES!!!”
“There are 3 forms of energy
important for this class.”
“KINETIC ENERGY IS
ENERGY IN MOTION.”
“YEEEHAAWWW!”
“There are 3 forms of energy
important for this class.”
Potential energy is very
important to Chemistry,
since every molecule or
atom wants to reach their
lowest potential energy
possible. This leads to
chemical bonding.
“POTENTIAL ENERGY
IS STORED ENERGY,
OR ENERGY AT REST.”
“OUCH!”
“There are 3 forms of energy
important for this class.”
“RADIANT ENERGY
IS HEAT ENERGY,
LIKE THE SUN.”
“THIS HAMMER CAN
BE DESCRIBED AS
POTENTIAL ENERGY.”
“YEEAAAHHHH!!
IF I SWING IT LIKE THIS
IT’S KINETIC ENERGY!!!”
“NOW ANSWER
THE QUESTION ON
THE ITINERARY.”
“How do we measure energy?”
“ONE WAY IS WITH
THE UNIT,
CALORIE.”
“Measuring energy...”
“A CALORIE IS THE AMOUNT
OF HEAT NEEDED TO RAISE
THE TEMPERATURE
OF 1 GRAM OF WATER
BY 1 CELSIUS DEGREE.”
“SHEESH THIS IS HOT!”
“Measuring energy...”
“THE SI BASE UNIT OF
ENERGY IS THE JOULE,
WHICH IS NAMED AFTER
ME, JAMES JOULE.”
“IN MY OPINION…NO MATTER
WHAT FORM OF ENERGY YOU
USE IT ALWAYS TAKES THE
SAME AMOUNT OF ENERGY
TO HEAT WATER UP 1 DEGREE
CELSIUS. AS IF YOU CARE!!”
“HERE’S A QUESTION FOR YOU,
CAN I MAKE THIS STEW BOIL
BY JUST STIRRING IT?”
“NOW ANSWER
THE QUESTION ON
THE ITINERARY.”
“YES, ACCORDING TO JOULE
IF I CAN STIR IT HARD ENOUGH
AND FAST ENOUGH AND
PUT AS MUCH ENERGY INTO
THE STEW AS FIRE DOES…
I CAN BOIL THIS STEW BY
STIRRING IT.”
“REMEMBER OUR CONVERSION
FACTORS? THE MODERN
EXPRESSION OF JOULE’S WORK
IS: 1 CAL = 4.184 JOULES.
SO A CALORIE IS 4 TIMES
BIGGER THAN A JOULE.”
“NOW ANSWER
THE QUESTION ON
THE ITINERARY.”
“ONE WONDERFUL
THING ABOUT
ENERGY IS THAT
IT IS ETERNAL”
“ENERGY IS NEITHER
CREATED NOR
DESTROYED…
IT IS ONLY CHANGED
FROM ONE FORM
TO ANOTHER.”
“THIS IS CALLED ENERGY
TRANSFORMATION,
WHEN ENERGY IS
TRANSFERRED FROM
KINETIC TO POTENTIAL
AND BACK .”
“KINETIC ENERGY FROM
THE BAT IS TRANSFERRED
TO THE BALL, WHICH HAD
POTENTIAL ENERGY.”
THE BALL NOW
HAS KINETIC
ENERGY
“NOW ANSWER
THE QUESTION ON
THE ITINERARY.”
“THE NEXT STOP
ON OUR JOURNEY
IS TEMPERATURE .”
“We know when we feel something hot.”
“We know when we feel
something cold.”
Temperature is how
we measure hot or cold
“We use a thermometer to measure
temperature.”
A THERMOMETER IS A BULB
CONNECTED TO A SEALED TUBE.
THE BULB IS FILLED WITH A LIQUID
THAT EXPANDS OR CONTRACTS
WHEN HEATED OR COOLED.
THE STEM IS MARKED WITH
A SCALE SO THAT THE LEVEL OF
THE LIQUID CAN BE READ.
A thermometer reads how fast the
molecules of the substance are vibrating
(Kinetic Energy). The faster they vibrate
the higher the temperature, and vice versa.
“THE SCALE USED TO
MEASURE TEMPERATURE
IS TOTALLY ARBITRARY.
THE FIRST ONE THAT WORKED
WELL WAS FAHRENHEIT,
BUT LATER CAME CELSIUS .”
“CELSIUS FOLLOWS THE SPIRIT
OF THE METRIC SYSTEM.
IT ALSO IS BASED ON 10’S .”
“THE CELSIUS SCALE WAS
DERIVED FROM TWO
SPECIFIC PHENOMENA.
“Water freezing...”
set at 0
0
“And water boiling...”
1
0
0
0
SET AT 100
1
0
0
“The marks are then evenly
divided...”
“MAKES YOU
WONDER WHY
IT TOOK SO LONG
TO INVENT .”
0
“NOW ANSWER
THE QUESTION ON
THE ITINERARY.”
COMPARISON OF CELSIUS AND
FAHRENHEIT TEMPS
EXAMPLE
TEMPERATURE
LOWEST OFFICIAL TEMP RECORDED
IN THE US (PROSPECT CREEK, AK
JANUARY 23, 1971)
-62°C
-80° F
MELTING ICE
0°C
32°F
TYPICAL ROOM TEMP
21°C
70°F
“NORMAL” BODY TEMP
37.0°C 98.6°F
HIGHEST OFFICIAL TEMP RECORDED
IN THE US (DEATH VALLEY, CA,
JULY 10, 1913)
57°C
134°F
BOILING WATER
100°C
212°F
TYPICAL OVEN TEMP FOR BAKING
163°C
325°F
SURFACE OF THE SUN
6000°C 10,000°F
“However, the SI base unit for
temperature is Kelvin”
“ACCORDING TO MY
NOTES…KELVIN &
CELSIUS SCALES RUN
PARALLEL .”
373 K
100°C
WATER
BOILS
ROOM
TEMPERATURE
294 K
273 K
100 K
21°C
WATER
FREEZES
0°C
-173°C
AIR LIQUIFIES
0K
-273°C
ABSOLUTE
ZERO
ALL
MOTION
STIOPS
“HOW ARE THEY
CONNECTED?”
373 K
100°C
WATER
BOILS
ROOM
TEMPERATURE
294 K
273 K
100 K
21°C
WATER
FREEZES
0°C
-173°C
AIR LIQUIFIES
0K
-273°C
ABSOLUTE
ZERO
ALL
MOTION
STIOPS
“WRITE AN EQUATION
THAT WILL CONVERT
BETWEEN THEM.”
“To convert between Celsius
and Kelvin…”
°
C = K ????
OR
K = C ????
°
“To convert between Celsius
and Kelvin…”
°
C = K - 273
OR
K = C + 273

“THE DIFFERENCE WITH
KELVIN IS THE LOCATION
OF THE ZERO POINT.”
“THE ZERO POINT FOR KELVIN
IS CALLED, ABSOLUTE ZERO.
ABSOLUTE ZERO
•
CORRESPONDS TO -273 C.”
“ABSOLUTE ZERO IS THE POINT
AT WHICH THE MOTION OF
PARTICLES OF MATTER - THEIR
KINETIC ENERGY - CEASES.”
“CLICK ON ME AND
GO TO THIS WEBSITE AND
EXPLORE THIS ELUSIVE
CONCEPT… ABSOLUTE
TEMPERATURE
“LOOKS LIKE THE NEXT
STOP IS TO LEARN
ABOUT THE CONCEPT
OF MATTER.”
To get an sneak peek at
how matter is organized,
check out the last page
of your itinerary!
“Matter is anything that has mass
and volume.”
&
“That seems like just about
everything right?”
MATTER
ENERGY
That is because it is everything
in the universe…that isn’t energy.
“There are four states of
matter.”
CLICK ON EACH
STATE AND READ
ABOUT THEM.
CLICK ON EACH
AND VIEW AN ANALOGY
OF EACH STATE
“The states of matter can change
from one state to another...”
“BY ADDING OR
REMOVING ENERGY
TO A SAMPLE
OF MATTER, WE CAN
CHANGE MATTER
FROM ONE STATE
TO ANOTHER.”
TRANSITIONS
FROM A SOLID TO
A LIQUID OR FROM
A LIQUID TO A GAS
ARE CALLED CHANGES
IN STATE.
ADDING ENERGY TO A
SAMPLE OF MATTER WILL
FOLLOW THIS DISTINCT
PATTERN, THROUGH ALL
FOUR STATES OF MATTER.
THIS IS CALLED A
HEATING CURVE
PHASE CHANGE
THIS DIAGRAM SHOWS
WHAT WE CALL THE PHASE
CHANGES BETWEEN ALL OF
THE PHASES, ARE THERE ANY
THAT YOU DIDN’T KNOW?
WHEN YOU PLAY
WHERE’S WALDO
YOU LOOK FOR
CHARACTERISTICS
OF THE TITLE
CHARACTER.
YOU CAN ALSO
DISTINGUISH
BETWEEN
MATTER BASED
ON ITS
CHARACTERISTICS
OR PROPERTIES.
“What are properties of matter?”
THE CHARACTERISTICS
OF A SUBSTANCE THAT
DISTINGUISH IT FROM OTHER
SUBSTANCES ARE THE
PHYSICAL PROPERTIES &
CHEMICAL PROPERTIES
OF THAT SUBSTANCE.
“Physical properties…”
“CHARACTERISTICS OF A
SUBSTANCE THAT CAN
BE OBSERVED WITHOUT
ALTERING THE IDENTITY
OF THE SUBSTANCE .”
“Chemical properties…”
“CHARACTERISTICS OF
A SUBSTANCE THAT
CANNOT BE OBSERVED
WITHOUT ALTERING
THE IDENTITY OF THE
SUBSTANCE .”
“There are two ways to change
matter…”
PHYSICAL
CLICK ON EACH AND EXPLORE
CHEMICAL
“CLICK ON ME TO READ MORE
ABOUT CHEMICAL AND PHYSICAL
PROPERTIES AND CHANGES.
MAKE SURE YOU WRITE DOWN
WHAT INTENSIVE AND EXTENSIVE
PROPERTIES.”
“Conservation of Matter…”
“THEN ALONG COMES
THIS DUDE,
ANTOINE LAVOISIER,
AND HE REALLY SHOOK
UP THE WORLD.”
“Conservation of Matter…”
“HE WROTE THAT IN
EVERY REACTION
THERE IS AN EQUAL
QUANTITY OF MATTER
BEFORE AND AFTER.”
“Conservation of Matter…”
“WHAT DID HE MEAN?
DID HE MEAN THAT
MATTER LIKE
ENERGY IS ETERNAL
AND CONSERVED?”
“The Law of Conservation of Matter…”
MATTER, LIKE ENERGY,
IS NEITHER CREATED
NOR DESTROYED IN
ANY PROCESS.
Click on the rectangle above and read the article on
the importance of Lavoisier’s work and life on earth.
“Conservation of matter…”
What that means...is that all
the matter in the universe is a fixed
amount. It is constant.
The amount of matter currently
present has always been here
since the dawn of time
and will always be here.
“SO THE MATTER IN
THAT PENCIL YOU ARE
HOLDING HAS ALWAYS
BEEN HERE IN SOME
FORM OR ANOTHER.”
“NOW YOU AND YOUR
PARTNERS WILL
INVESTIGATE THE
LAW OF CONSERVATION
OF MATTER TOGETHER.”
CLICK ON THE COUPLE
AND PROCEED WITH
YOUR INVESTIGATION
“WELCOME, I HOPE YOU
FIND THE NEXT STOP ON
YOUR JOURNEY
PLEASANT. LET’S LOOK AT
ELEMENTS AND
COMPOUNDS.”
“Elements and compounds…”
“HERE’S ANOTHER AMAZING
THING… EVERYTHING AROUND
US…EVERYTHING…
IS MADE FROM DIFFERENT
COMBINATIONS OF ABOUT 100
OR SO ELEMENTS.”
“Elements and compounds…”
“IT’S A LOT LIKE THE ALPHABET.
EVERY WORD YOU CAN THINK OF
IN THE ENGLISH LANGUAGE IS
MADE UP OF A COMBINATION OF
THE SAME 26 LETTERS.
EVERY SUBSTANCE IN THE
UNIVERSE IS COMPOSED OF THE
SAME 100 ELEMENTS.
“Elements…”
“AN ELEMENT IS A
SUBSTANCE THAT
CANNOT BE SEPARATED
INTO SIMPLER
SUBSTANCES
BY CHEMICAL CHANGE.”
“Elements…”
“THEY ARE KIND OF LIKE THE
LEGO BLOCKS THAT ARE USED
TO BUILD ALL OF MATTER”
“Elements…”
THEY ARE IN FACT ATOMS.
IF YOU BROKE AN ELEMENT
UP ANYMORE THAN YOU
WOULD END UP WITH
SUBATOMIC PARTICLES LIKE
ELECTRONS AND PROTONS.”
“Elements…”
HAVE YOU EVER WONDERED
HOW SMALL ATOMS ARE?
THE LEGO BLOCKS THAT MAKE UP
EVERYTHING YOU CAN SEE,
TASTE, TOUCH, OR SMELL ARE
EXTREMELY SMALL. CHECK OUT
THIS WEBSITE.”
“Elements…”
“I’VE EVEN GOT MY OWN
ELEMENT. LOOK AT A
PERIODIC TABLE AND WRITE
DOWN THE NAME AND
NUMBER OF MY ELEMENT.”
“WHAZZZ
ZZZUUUP?’
“Elements…”
• FOR CONVENIENCE ELEMENTS HAVE
ABBREVIATIONS CALLED THE
ELEMENT SYMBOL(S)
• ELEMENT SYMBOLS CONSIST OF ONE
OR TWO LETTERS
– THE FIRST LETTER OF A SYMBOL
IS ALWAYS CAPITALIZED
– AND THE SECOND IF PRESENT
IS NEVER CAPITALIZED
THE ELEMENTS ARE ARRANGED
IN A TABLE THAT IS CALLED THE
PERIODIC TABLE
THE PERIODIC TABLE IS
ORGANIZED BY THE ELEMENTS’
BEING GROUPED TOGETHER BY
THEIR CHEMICAL PROPERTIES
IN COLUMNS CALLED FAMILIES
OR GROUPS
“Periodic Table…”
“THERE ARE 18 COLUMNS
ACROSS THE PERIODIC TABLE.
NUMBERED 1-18, AND MOST
OF THEM HAVE NAMES TO HELP
IDENTIFY THEM,
SO LET’S MEET THE FAM.”
Click Here and Check Out Some Videos
“Periodic Table…”
“THERE ARE 7 ROWS IN THE
MODERN PERIODIC TABLE, WHICH
ARE CALLED PERIODS.
THE PROPERTIES OF THE
ELEMENTS CHANGE PREDICTABLY
AS WE GO ACROSS EACH ROW.”
“Periodic Table…”
“YOU MIGHT SAY WAIT A MINUTE AL,
WHAT ABOUT THE TWO ROWS AT
THE BOTTOM, DON’T THEY MAKE
IT 9 ROWS DOWN? ACTUALLY NO,
THOSE TWO ROWS REALLY BELONG
WITH 6 & 7, LIKE THIS”
“Periodic Table…”
“THE ELEMENTS CAN BE CLASSIFIED
AS METALLIC, NONMETALLIC, OR
SEMI-METALLIC. AND WE CAN TELL
WHICH CATEGORY AN ELEMENT
FITS INTO BASED ON ITS POSITION
ON THE PERIODIC TABLE”
“Metals…”
“DID YOU EVER WONDER WHAT
MAKES A METAL A METAL?
WELL I HAVE, I WONDER A LOT.
ALL METALS CONDUCT ELECTRICITY,
ALL METALS ARE BENDABLE AND
SHAPEABLE, AND ALL METALS ARE
ABLE TO BE STRETCHED OUT.”
“Metals…”
THESE ARE THE METALLIC
ELEMENTS, THEY ARE ALL SOLIDS
AT ROOM TEMPERATURE
EXCEPT FOR 1, MERCURY.
“Nonmetals…”
“NONMETALS, WHAT MAKES THEM
UNIQUE? WELL THEIR MAJOR
DISTINGUISHING CHARACTERISTIC
IS THAT THEY ARE NOT METALS.
THEY DON’T CONDUCT ELECTRICITY,
THEY CAN’T BE BENT AND SHAPED.”
“Nonmetals…”
THE SOLIDS ARE BRITTLE
AND NONCONDUCTIVE,
AND THERE ARE SEVERAL
LIQUIDS AND GASES.
“Semi-metals…”
“SEMI-METALS/METALLOIDS ARE
THE GRAY AREA IN BETWEEN. THEY
ARE PART METAL AND PART
NONMETALS, AND DON’T FIT WELL
IN EITHER CATEGORY. THEY ARE
BRITTLE SOLIDS LIKE THE
NONMETALS, BUT ARE SLIGHTLY
CONDUCTIVE LIKE METALS.”
“Semi-metals…”
THESE ELEMENTS ARE
POSITIONED BETWEEN THE
METALS AND THE NONMETALS
ON THE PERIODIC TABLE
AND MAKE A CHARACTERISTIC
STAIR STEP PATTERN.
“Compounds…”
“WHEN DIFFERENT
ELEMENTS ARE GROUPED
TOGETHER WE CALL
IT A COMPOUND.”
“Compounds…”
“TO WRITE CHEMICAL
COMPOUNDS WE WILL
USE ELEMENTAL SYMBOLS
MORE OFTEN THAN NOT,
AND USE THEM TO WRITE
FORMULAS.”
“Compounds…”
“FORMULAS ARE
COMBINATIONS OF THE
ELEMENT SYMBOLS THAT
MAKE UP THE COMPOUND.”
“Types of Compounds…”
“METALLIC ELEMENTS
CAN COMBINE WITH
NONMETALLIC ELEMENTS
TO MAKE COMPOUNDS
KNOWN AS IONIC.”
“NONMETALLIC ELEMENTS
CAN COMBINE WITH OTHER
NONMETALLIC ELEMENTS TO
MAKE COMPOUNDS KNOWN
AS COVALENT.”
“Elements and compounds…”
“ELEMENTS &
COMPOUNDS ARE
CONSIDERED PURE
SUBSTANCES, BUT AN
ELEMENT CAN NOT BE
BROKEN INTO SMALLER
PIECES WHILE A
COMPOUND CAN.”
“JUST ONE MORE
VACATION SPOT LEFT.
LET’S CHECK OUT
MIXTURES.”
“Mixtures”
“A MIXTURE IS SIMPLY
A BLEND OF TWO OR
SUBSTANCES,
JUST LIKE THIS
SHAVING CREAM
I’M USING.”
“Types of mixtures”
“THERE ARE 2
DIFFERENT TYPES
OF MIXTURES,
HOMOGENEOUS &
HETEROGENEOUS.”
“Homogeneous Mixtures”
“A HOMOGENEOUS
MIXTURE CONTAINS NO
VISIBLY DIFFERENT
PARTS. PARTS THAT
AREN’T EASILY SEPARATED.
“Homogeneous Mixtures”
EXAMPLES OF
HOMOGENEOUS
MIXTURES.
“Heterogeneous Mixtures”
“A HETEROGENEOUS
MIXTURE HAS VISIBLY
DIFFERENT PARTS.
IT CAN EASILY BE
SEPARATED.”
“Homogeneous Mixtures”
EXAMPLES OF
HETEROGENEOUS
MIXTURES.
“Separating Mixtures”
IN THE CHEMISTRY LAB, SPECIAL
EQUIPMENT AND TECHNIQUES HAVE
BEEN DEVELOPED FOR THE SOLE
PURPOSE OF SEPARATING MIXTURES.
“Filtration”
“HETEROGENEOUS
MIXTURES CAN OFTEN
BE SEPARATED WITH
THE SIMPLE TECHNIQUE
OF FILTERING.”
“Filtration”
“THE MIXTURE IS POURED
THROUGH A PIECE OF
PAPER, WHICH CATCHES
THE SOLID, BUT ALLOWS
THE LIQUID TO PASS
THROUGH.”
“Filtration”
“THIS IS A USELESS
METHOD FOR TRYING
TO SEPARATE
HOMOGENEOUS
MIXTURES THOUGH.”
“Distillation”
“THIS IS A METHOD
OF SEPARATING HOMOGENEOUS MIXTURES,
WHICH SEPARATES
LIQUIDS.”
“Distillation”
2.
“IT TAKES ADVANTAGE
OF DIFFERENCES
IN BOILING POINTS
OF THE LIQUIDS.”
THE LOWER
BOILING LIQUID
BECOMES A GAS
AND TRAVELS UP
THE COLUMN.
3.
THE GAS
CONDENSES IN
THIS TUB.
4.
1.
STARTS WITH
BOILING THE
LIQUID
HERE IN THIS
CHAMBER.
PURE LIQUID IS
COLLECTED IN
THIS FLASK.
“Crystallization”
“THIS IS A METHOD
OF SEPARATING
HOMOGENEOUS MIXTURES,
WHICH SEPARATES A SOLID
DISSOLVED IN A LIQUID.”
“Crystallization”
“PARTIALLY EVAPORATING
A LIQUID THAT CONTAINS
DISSOLVED PARTICLES MAY
ALLOW SOLIDS TO FORM
AS PURE CRYSTALS.”
“Crystallization”
“THIS IS A METHOD
OF SEPARATING
HOMOGENEOUS MIXTURES,
WHICH SEPARATES LIQUIDS.”
“Chromatography”
“THE COMPONENTS
ARE SEPARATED BY THEIR
ABILITY TO BE STICKY
ON THE STATIONARY
SUBSTANCE, THOSE LESS
STICKY COME OUT FIRST.”
“Chromatography”
“THERE IS A STATIONARY PHASE
AND A MOBILE PHASE IN
CHROMATOGRAPHY. THE MIXTURE
TO BE SEPARATED IS DRAWN
ACROSS THE STATIONARY PHASE
WITH THE MOBILE PHASE AND IT
GETS SLOWLY SEPARATED.”
“Chromatography”
THESE 3 TYPES OF CHROMATOGRAPHY ALL SHARE COMMON
MECHANISMS, THE MIXTURE IS
DRAWN ACROSS THE STATIONARY PHASE AND THE MIXTURE
IS SLOWLY SEPARATED.
“Chromatography”
“NOW YOUR GROUP
WILL INVESTIGATE A
MINIATURE VERSION
OF CHROMATOGRAPHY
JUST CLICK ON ME AND
FOLLOW THE DIRECTIONS.”
“Liquids...”
A LIQUID DOES NOT HOLD ITS OWN
SHAPE, BUT IT DOES OCCUPY
A DEFININTE VOLUME.
“Liquids...”
A LIQUID FLOWS FREELY AND TAKES
THE SHAPE OF ITS CONTAINER.
THE MOLECULES STICK TOGETHER
TIGHTLY ENOUGH THAT THEY ARE
BOUND, BUT NOT SO TIGHT THAT THEY
ARE LOCKED INTO POSITION.
“Solids...”
A SOLID IS ANY MATTER THAT HAS A
DEFINITE SHAPE AND DEFINITE VOLUME.
“Solids...”
WHEN A SOLID IS BROKEN INTO SMALLER
PIECES IT IS NOT CHANGED CHEMICALLY.
THE MOLECULES ARE SO STUCK TOGETHER
THAT THEY BECOME LOCKED IN POSITION.
“Gases...”
A GAS HAS NO DEFINITE
SHAPE OR VOLUME.
“Gases...”
GASES EXPAND TO FILL THE AVAILABLE
VOLUME. THE MOLECULES ARE NOT STUCK
TOGETHER AT ALL AND ARE COMPLETELY
INDEPENDENT OF EACH OTHER.
“PLASMA...”
HIGH
ENERGY
IONS FOUND
INSIDE
STARS.
“PLASMA...”
WE’RE NOT
GOING TO
TALK ABOUT
PLASMA MUCH.
Before you rush off, there is
evidence of a 5th state of
matter. Check it out by
clicking on the picture of the
sun to the left.
LIKE A CROWD A LIQUID IS PACKED
TOGETHER BUT THE PARTICLES CAN
MOVE OVER AND AROUND EACH OTHER
FREELY. THEY ONLY HAVE SO MUCH
SPACE TO MOVE AROUND IN SO THERE
IS A CONSTANT VOLUME.
LIKE A FOOTBALL GAME A GAS IS CONSTANTLY SHIFTING
AND HAS NO DEFINITE PATTERN OR SHAPE...
LIKE A MARCHING BAND A SOLID IS HIGHLY
STRUCTURED AND HOLDS A DEFINITE SHAPE...
“Physical Change…”
ANY CHANGE IN A PROPERTY OF MATTER
THAT DOES NOT CHANGE ITS IDENTITY
THE BAT IS STILL
WOOD EVEN IF IT
LOOKS DIFFERENT
“Other Physical Changes…”
PHYSICAL CHANGES IN MATTER
CAN INVOLVE STARTLING ALTERATIONS
IN FORM, BUT THE MATTER ITSELF
IS NOT ALTERED.
“Chemical Change…”
ANY CHANGE IN WHICH ONE OR MORE
SUBSTANCES ARE CONVERTED INTO
DIFFERENT SUBSTANCES WITH DIFFERENT
PROPERTIES.
“Other Chemical Changes…”
CHEMICAL CHANGES IN MATTER INVOLVE A
COMPLETE CHANGE. A CHANGE THAT MAKES
THE SAMPLE A DIFFERENT MATERIAL WITH
TOTALLY DIFFERENT PROPERTIES.
“Endothermic/Exothermic…”
CHEMICAL CHANGES EITHER PRODUCE
ENERGY AND GIVE OFF HEAT OR ABSORB
ENERGY AND DRAW IN ENERGY.
EXO =
ENERGY OUT
ENDO =
ENERGY IN
“Evidence of chemical reactions or
changes…”
• BUBBLES OF GAS APPEARS
• FORMATION OF AN INSOLUBLE SOLID
• A COLOR CHANGE FORMS
• TEMPERATURE CHANGE
• LIGHT EMITTED
• CHANGE IN VOLUME
“EVIDENCE OF CHEMICAL CHANGES…”
• CHANGE IN ELECTRICAL CONDUCTIVITY
• CHANGE IN MELTING POINT OR BOILING
POINT.
• CHANGE IN SMELL OR TASTE
• A CHANGE IN ANY DISTINCTIVE CHEMICAL
PROPERTIES OR PHYSICAL PROPERTIES
CONSERVATION OF MATTER
This is an investigation in the lab where
you will be working through a problem
and trying to illustrate the Law of
Conservation of Matter.
I. You need a clean sheet of paper,
and you need to go to the back and
put on a pair of safety goggles.
CONSERVATION OF MATTER
II. Now on your paper, make a data table with
four columns and three rows.
– Label the boxes in row 1: column 2:
Initial mass(g), column 3: Final mass(g),
and column 4: Change in mass(g)
– Label the boxes of row 2, column 1 “Part
1” & row 3, column 1 “Part 2”.
Initial Mass
Part 1
Part 2
Final Mass
Change
in Mass
1) Place a plastic cup on the laboratory
balance and zero out the mass of the cup.
– Place about 2g of baking soda in the cup.
2) Using the 100ml graduated cylinder,
measure about 30ml of vinegar.
– Remember to read the bottom of the
meniscus and to 1 decimal place
3) Pour the vinegar into a second plastic cup.
4) Place both cups on the balance pan of a
laboratory balance, and determine the
starting mass of the entire system.
– Record this mass in your data table as
“initial mass”.
5) Take the cups off the balance. Carefully
pour the vinegar into the cup that contains
the baking soda.
6) Gently swirl the cup to make sure
everything is well mixed.
7) When the reaction is finished, place both
cups back on the balance to determine
the “final mass” of the system.
– Record the mass in your data table in the
“final mass” column.
– Subtract the final and the starting masses
to get the “change in mass”.
1. Examine the materials you have on
the table
• Develop a procedure that will test the
law of conservation of mass more
accurately than Part 1 did.
2. When you and your partner have a
plan, get my approval.
3. Afterwards, implement it using the same
materials and quantities from Part1.
– Use the baggies instead or in addition
to the cups from Part 1.
4. If you show that mass is conserved
effectively, then answer the following
questions on your lab sheet.
1. Describe all evidence that a chemical
change occurred in this experiment.
2. Did your first set of data agree with the
law of conservation of mass? Explain.
3. Why are the results from Part 2 different
from those for Part 1?
PAPER CHROMATOGRAPHY
This is an investigation in the lab
where you will be working through
a problem and will illustrate
separation of liquids.
I. You need a clean sheet of paper, and
you need to go to the back and put on
a pair of safety goggles and an apron.
MATERIALS
• You need to find three different colored
ink pens
• You need to pick up 3 strips of filter paper
from the back table
• You need to pick up a 300ml or 400ml
beaker from the back table
PROCEDURE
1. Take each strip of filter paper and using
the ink pens make one small dark spot
3cm from the base of the strip (one
color per strip)
3cm
PROCEDURE
2. Using a graduated cylinder obtain
about 2.0ml of rubbing alcohol from
the table
3. Pour the rubbing alcohol into the
beaker and then add enough water
until the solution is about 2 cm deep.
PROCEDURE
4. Tape the strip to a pencil so that the ink
spots hang down, and hang the strip on
the beaker so that the tip of the strip
dips into the solution. Note: make
sure that the ink isn’t submerged.
INK SPOTS
ALCOHOL
PROCEDURE
5. Watch the solvent travel up the strip
of paper
6. Write down observations.
7. When the solvent reaches the top
of the strip, remove the strip from
the tank and allow to dry.
8. Repeat each step for the other
two colors.
ANALYSIS
i. Draw what you see on each strip.
ii. Is chromatography a good method of
separating mixtures? Think about the
quantity of mixture you had.
iii. What are the limitations of this
method of separation?
CHOOSE THE STOP YOU WERE
CLOSEST TO…TO BEGIN
“Energy”
“Matter”
“Mixtures”
“Elements
and
Compounds”
“Temperature”