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Do-Now Title: “Bill Nye Clip” 1. Write down today’s FLT
1atm=760mmHg=760torr=101,325Pa=101.325kPa
2. What is “STP”? Include what it stands for as well as the actual values.
3. Convert 54.7 kPa to atm. Show all work and units.
4. Convert 7.1 torr to mmHg. Show all work and units. Finished? Take out your planner and table of
contents.
Announcements • Didn’tturninyourlab?
– Seemetopickupamissingassignmentform-required
• Checkyourgradesregularly– Missingassignmentsturnintozeroes!
L
• StudyCh.13+notesforupcomingquiz
• Bringyourcalculators
Planner: • Study for Ch. 13 Quiz • Get stamps through #13 by the end of
the week Table of Contents #1:
11. Bill Nye Clip WS 12. Ch. 13 CN Part B 13. States of Matter WS
Video Clip • Watch the video clip • Answer questions as you watch • Noise level 0 • Wait until after the clip is finished to
ask your partner(s) questions
FLT • I will be able to describe the properties
of liquids and solids by completing Ch. 13 Notes B
Standard HS-PS1-4:Developamodeltoillustratethatthe
releaseorabsorpQonofenergyfromachemical
reacQonsystemdependsuponthechangesintotal
bondenergy.
Notes Protocol • Title your notes & add assignment # • Complete Cornell-style • Copy down all bolded ideas • Noise level 0 • Raise hand to question/comment • Be prepared to pair-share-respond
The Nature of Liquids • Liquids have an indefinite shape and a definite
volume • The molecules in liquids are always moving, so they
have kinetic energy • This allows them to take the shape of their
container just like gases
Gas Particles vs. Liquid Particles • Gas particles are different than liquid particles: 1. Liquid particles attract each other, but gas
particles do not.
Gas Particles vs. Liquid Particles • Gas particles are different than liquid particles: 2. Because of their attraction, liquid particles
move but are closer together. – Liquids have a definite volume
Gas Particles vs. Liquid Particles • Gas particles are different than liquid particles: 3. Liquids are more dense than gases.
– Liquid molecules are more closely packed together.
Evaporation • Liquidsevaporatefasterwhenheatedbecausehea(ngincreasestheaveragekine(cenergyoftheparQclesintheliquid.
Vapor Pressure • VaporPressure=pressureexertedbyavaporoveraliquid
• Watervaporcollectsabovetheliquidandexerts
pressureduetocollisions
Boiling Point • Remember: liquids are attracted to each other.
They LIKE being close together. • Adding heat adds energy so that particles can
overcome the attractive forces and enter the gaseous state.
Boiling Point • Boiling Point (bp) =
temperature at which the vapor pressure is equal to the pressure of the gas above it
• The vapor has enough pressure to keep the gas bubbles from collapsing
• Molecules even at the bottom of the liquid have enough energy to vaporize, so they rise to the surface
Pair-Share-Respond 1. Identify two ways that liquids differ from
gases 2. Distinguish between the terms
“vaporization” and “evaporation” 3. Why does heating increase the rate of
evaporation? 4. Define the term “vapor pressure”
The Nature of Solids • Solids have a definite shape and volume • Solids à orderly arrangement, vibrate in
fixed positions, and do not flow
Melting Point • Melting point (mp) = temp at which solid à
liquid = the same temp as the freezing point (liquid à solid)
• At the melting point, the vibrations are strong enough to overcome the attractions holding them in fixed positions.
Crystalline Structure • Solid structures = Most are crystalline • In a crystal the particles are arranged in an orderly,
repeating, three-dimensional pattern called a crystal lattice.
Allotropes • Allotropes = Some solid substances can exist
in more than one form • Ex. Allotropes of carbon (diamonds and graphite) • Different structures give allotropes different
properties
Pair-Share-Respond 1. Describe solids at the particulate level 2. What is an allotrope? 3. Most solids have a crystalline structure,
but some are “amorphous”. What do you think amorphous might mean?
CW 1. Use your textbook and/or notes to
complete the states of matter WS 2. Any work that needs to be stamped
should be on the corner of your desk/table with your stamp sheet
3. Study Ch. 13 à quiz next class
Do-Now Title: “Ch. 13 Notes C” 1. Write down today’s FLT 2. List the three states of matter and list an
example 3. Describe one property of each state underneath 4. _________ is the change of a liquid into a vapor 5. Explain why changing the temperature can help
speed up the process of evaporation. 6. We will take notes under our do-now. Draw or
fold your column for cornell notes. Finished? Take out your planner and table of
contents.
Announcements • Clearmissingassignments• Bringclassmaterialsdaily
• Reminder:DojoPoints
– 5points:• Treat,pen/pencil,calculatoruse(one-Qme)
– 10points:• Newperiodictable/referencesheet
– 15points:• ToCstamp
Planner: • Turn in Inquiry Activity • Elements WS • Read 3.2-3.3
Table of Contents #1: 14. Ch. 13 CN Part C 15. Elements WS
FLT • I will be able to identify the temperature
and pressure conditions for states of matter by completing Ch. 13 Notes C
Standard HS-PS1-4:Developamodeltoillustratethatthe
releaseorabsorpQonofenergyfromachemical
reacQonsystemdependsuponthechangesintotal
bondenergy.
Notes Protocol • Title your notes & add assignment # • Complete Cornell-style • Copy down all bolded ideas • Noise level 0 • Raise hand to question/comment • Be prepared to pair-share-respond
Changes of State • Sublimation can occur because solids and liquids
have vapor pressure • Sublimation occurs in solids with vapor pressures
that exceed atmospheric pressure at or near room temperature.
Phase Diagrams • Phase Diagram = Diagram that shows the
relationships among solid, liquid, and vapor states of a substance
Phase Diagrams • Shows the temperature and pressure at which
substances exist at each state • You can locate the normal melting point, normal
boiling point, triple point, and critical point on the diagram
Phase Diagrams • Triple Point = Set of conditions at which the
three phases exist in equilibrium • At the critical point, the physical properties of the
liquid and gaseous states are identical
Problem • Through a variety of different procedures,
determine whether the unknown substance and water solution that the beaker contains is a solid or a liquid.
Pre-Lab Questions • We will work in groups of 2-3. • It is important that we exhibit good
laboratory safety behaviors and measurement skills.
• Answer questions 1-4 with your lab partner. Answer in complete sentences. When finished, get the front page stamped off.
Reminders • Observations:
– Can be qualitative or quantitative – Be detailed – Observation: The solution looks blue – Better: The solution is a transparent sky blue color
with a few particles settled at the bottom of the beaker
Procedure 1. Useweighboatstoobtain15gramsofthe
mysterysubstanceintoaplasQccup/beaker.
– WritedetailedobservaQonsofwhatyouseeand
statewhethertheyaresolidsorliquidsinstep#2.
2. Useagraduatedcylindertomeasure12mLof
waterandplaceintothebeaker.DONOTMIX.
àObserve,andthenuseyourhandtomix
together.MakedetailedobservaQonsabout
textureandconsistencyindatatable(step#4)
àNowfollowsteps#5-9tofinishyourlab
Procedure 3.Tapthesurfaceoftheunknownsubstancewith
yourfingerFIRMLY.Filloutdatatablestep#5.
4.SLOWLYsubmergeyourfingerintothesoluQon.
Filloutdatatablestep#6.
5.TrygrabbingabouthalfofthesoluQonwithyour
handandseehowitreactsinyourpalm.Fillout
datatable#7.