Do Now: Find new seats
melanie 1
zacharia
9
jacob
17
andretta 2
ian
10
arianna
18
jennifer
joy
11
gabrielle
19
3
elias
4
Shajra
12
Jose
20
mariah
5
de'andre
13
Nailah
21
hector
14
syndey
22
julianna
15
emily
23
isabella
16
Se'jean
24
casandra 6
shaquom 7
augustin 8
angelica 25
daniel
26
jairo
27
christina 28
kayla
29
Do Now: Find New Seats
egar
1
alexandra
2
damien
3
kiara
4
lorena
5
denzell
6
olivia
7
emma
8
jordan
elijah
yasheema
joshua
mina
christopher
kevin
bruno
9
10
11
12
13
14
15
16
joseph
seth
johanan
lindsey
itzel
Jessica
jonathan
vernon
17
18
19
20
21
22
23
24
parker
25
megan
26
sara
27
nazjai
28
WELCOME BACK!
• WELCOME BACK!
• Bellringer:
– Read the first page of the notes packet and fill in
the particle diagrams based on the reading
• Remember about gravity…
Homework:
• Make sure you finish and turn in types of
reactions lab by tomorrow…
This unit
• All about phases, their properties and phase
changes
– Are there different types of solids?
– What happens when things go from slg?
– How much energy is needed in order to go
through those changes
Today’s objective
• Describe the properties of solids
• Design a lab to determine the type of solid for
an unknown
Solids
• High, Medium, or Low attraction between
each particle?
• How do they move?
Liquids
• High Medium or Low
attraction
• How do they move?
• Proof that liquid molecules
are attracted to each other:
• http://www.youtube.com/wa
tch?v=r7fEHYkGxd0
Gas
• High Medium or Low
attraction?
• How do they move?
Solids!
• We are going to focus on Different types of solids.
• Focus: You are going to design a lab to determine
what type of solid two different solids are
• Read along with your neighbor and fill in the venn
diagram on the next page
– Maybe split it: 2 types per neighbor?
• Things all Solids have in common goes in the
center
• Overlap is for things in common
Do Now
• Pick up a copy of the lab
• RETURN ANY EXTRA COPIES OF THE NOTES
THAT YOU MAY HAVE TAKEN
• Make sure the following are described in the
venn diagram:
– Melting point (very high, high, variable, low)
– Solubility
– Conductivity (if so, under what conditions)
– How the particles are arranged
Types of solids lab
• 2 different solids
• You have:
• Distilled water (may have CO2 Dissolved in it…)
– This would make it slightly conductive…need to
account for that
•
•
•
•
Conductivity testers
cups
stirring rods
other miscellaneous lab equip (NOT
BUNSEN BURNERS)
Procedure
• Get it approved before beginning
•
It would be unfortunate to get all the way
done and then find an error with the
procedure and need to do it all over
• Something to think about: When CO2 dissolves
into water, it makes the water
conductive…going to need to account for that
Do now
•
•
•
•
•
•
Take out your Types of Solids Lab
Refresh your memory
Ionic
Molecular
Network
Sol.
Cond.
M.p.
Metallic
• Make sure you get your procedure approved and
finish the lab (and turn it in)
Absent?
• Then you need to play a little catch up
• Read the notes about the types of solids and
fill in the 4 box ven diagram on the next page
• Use this information to figure out how you
could test these 2 unknown solids to
determine what type of solid they are
Homework:
• Finish the lab
Do now
• Bellringer Quiz:
• Pick up, do independently and turn in
• Also turn in Types of Solids lab
Homework
• Phases and phase change diagrams
• Heat of phase changes
(front and back of 1st page)
And now…
• Read page 4 and fill in the graphic organizer
on page 5 and 6
A nice simulator
• http://phet.colorado.edu/en/simulation/state
s-of-matter-basics
Phase Changes:
Label the phase changes (1-6), identify each side as either exothermic or endothermic, fill in
the phase change diagrams and particle diagrams for each phase.
Temp. (K)
_____thermic
+ or - ΔH
Temp. (K)
_____thermic
+ or - ΔH
Gas
Time
5.___________
Time
(particle diagram)
1.___________
6.___________
2.___________
Liquid
(particle diagram)
3.___________
4.___________
Solid
(particle diagram)
Sublimation and Deposition
• http://www.youtube.com/watch?v=4E0syFN2M8
• 1) Label the phases present at each line segment above using
(s), (l), and (g).
• 2) What is the boiling point of this substance? ________
• 3) What is the melting point of this substance? ________
c. Heat of phase change
• In previous units we have calculated the amount of
energy needed to change the temperature of water
using the formula: q=mCΔT (remember that catchy
song?). During a phase change, however, there is no
change in temperature so this formula cannot be used
to solve for the heat needed for a phase change.
Instead, there are different formulas used for phase
changes; q=mHf and q=mHv. Hf is the heat of fusion, the
amount of energy required to melt or freeze a gram of
water (334 J/g). Hv is the heat of vaporization of water;
the amount of energy required to boil or condense
water (2260 J/g).. ‘m’ is the mass of water involved in
the phase change.
How much energy is required to melt
50.0g of water at 0oC?
• q = m Hf
– Why Hf?
• q = 50.0 g x 334J/g
• q =16700 J
Practice Problems
• _____1) Which of the following phase changes
requires heat of fusion to accomplish?
• a) H2O (s)  H2O (g)
b) H2O (g)  H2O (l)
• c) H2O (l)  H2O (g)
d) H2O (s)  H2O (l)
•
• _____2) Which of the following phase changes is
endothermic?
• a) H2O (s)  H2O (l)
b) H2O (g)  H2O (l)
• c) H2O (l)  H2O (s)
d) H2O (g)  H2O (s)
Calculate the number of joules required to
(show correct numerical setup):
•
•
•
•
•
•
•
a) melt 20.0 g of H2O (s) at 0oC
b) boil 30.0 g of H2O (l) at 100oC
c) freeze 200.0 g of H2O (l) at 0oC
d) boil 50.0 g of H2O (g) at 100oC
Ice cubes at –12.0oC are placed in a
saucepan and heated at a constant rate
over a stove to 115.0oC.
• Sketch a phase change diagram for the phase
changes that occur between -12.0 oC and
115.0oC. Label the temperatures at which the
phase changes occur. Then label each line
segment with a letter (A, B, C, D, E, etc.).
Label where P.E. increases/stays same
Do the same for K.E.
Do Now:
• Pick up a copy of the lab
• Read over the procedure to the lab
Questions?
• _____1) Which of the following phase changes requires heat of fusion to
accomplish?
• a) H2O (s)  H2O (g) b) H2O (g)  H2O (l)
c) H2O (l)  H2O (g)
d) H2O
(s)  H2O (l)
•
• _____2) Which of the following phase changes is endothermic?
• a) H2O (s)  H2O (l) b) H2O (g)  H2O (l)
c) H2O (l)  H2O (s)
d) H2O (g)  H2O (s)
•
• Calculate the number of joules required to (show correct numerical setup):
• a) melt 20.0 g of H2O (s) at 0oC
•
• b) boil 30.0 g of H2O (l) at 100oC
•
• c)
freeze 200.0 g of H2O (l) at 0oC
•
• d) boil 50.0 g of H2O (g) at 100oC
• Ice cubes at –12.0oC are placed in a saucepan and heated
at a constant rate over a stove to 115.0oC.
• Sketch a phase change diagram for the phase changes that
occur between -12.0 oC and 115.0oC. Label the
temperatures at which the phase changes occur. Then label
each line segment with a letter (A, B, C, D, E, etc.).
Safety
•
•
•
•
Goggles
Be careful of HOT WATER
Don’t drop the thermometers…
Do not poke a whole in the bottom of the
calorimeters!
• Don’t eat the ice…
Big Idea
• Starting with hot water and Ice
• Going to calculate how much energy was lost
by the water (q=mCΔT)
• That energy was used to melt the ice
• Calculate the Hf based on that
– q/(g of ice melted)
• Follow the procedure!
Do Now
• Take out The Heat of Fusion Lab from
yesterday and begin working on it
• Plan on the Test being on Thursday
• Quiz on THIS FRIDAY (covering phase changes)
This period’s agenda
• Finish the lab
• Finish the ‘H.W.’, front and back of the first
page
• Start reading the 4. Gases and Pressure
Do now
• Turn in Heat of Fusion Lab
• Turn in first page (front and back) from
homework packet
• Read over topic 4: Gases and Pressure (a+b)
• Start brainstorming on how you could visualize
each of these concepts
Kinetic molecular theory (KMT) for
gases and ideal gas laws
• Before we can discuss what an ‘Ideal’ gas is,
we must first discuss what is true for all gases,
ideal and real. The following is true for all
gases:
•
•
•
•
•
•
Gas particles have no definite volume
Gas particles have no definite shape
Gases are highly compressible
Gases take the volume and shape of the container
Gas molecules are relatively far apart from one another
Gases form homogeneous mixtures with each other
• Real gases will act like Ideal gases at low
pressure and high temperature. Smaller gases
(H2 and He) also behave more ideally than
larger gases (CO2, CH4).
• The concept of the ‘Ideal gas’ is to explain the
behavior of real gases. There is a list of things that
we assume about gases to be true to explain their
behavior. For example, we assume that ‘ideal’ gas
particles have no attraction for each other, which is
why the take on the volume of their container.
‘Real’ gas particles do have some attraction to each
other. The reason we make these assumptions is
because they are mostly true, and in doing so we
can calculate a lot of information about gases. The
following are the Ideal Gas Laws:
• Gas molecules are so small that the combined size
is insignificant compared to the volume occupied by
the gas.
• Gas molecules move in straight line motion until
they collide with the container wall or another gas
molecule
• Any collisions between gas molecules are elastic
with NO energy lost from the collisions.
• No attractive or repulsive forces exist between gas
molecules.
• The Average velocity (speed with direction) of the
gas is directly proportional to the KELVIN
temperature (the higher the temperature, the faster
they move).
b. Avagadros hypothesis
• Simply put, Avogadro’s Hypothesis states that
equal volumes of ALL gases, at the same
temperature and pressure, have the same
number of molecules. If you were to double
the number of molecules, you would double
the volume.
Poster Project (14 minutes)
• Illustrations are excellent for visualizing some
abstract concepts. You will use your creativity
to create a visual for one of these concepts
• It can be a literal representation, an example
from real life or a metaphor.
• Example: The atom is mostly empty space
– Draw an atom with mostly empty space
– A club named ‘Atom’, which is almost completely
empty
Poster Project (14 minutes)
• Be prepared to explain your illustrations to the
class…
Poster presentations
Quickly Sketch your favorites into your
notes packet
Do Now (Test Thursday)
• Take out Homework Packet and put everything
else away
• Homework check time!
• Finished?
• Read:
– Pressure, vapor pressure and boiling points
–  through ‘Using the reference tables’
• Try some of the practice
c.
Pressure, vapor pressure and
boiling point
• Pressure is defined as a force exerted on an area. You may
be familiar with the term psi, which stands for pounds per
square inch. This is what you see on your gas gauge when
you check the pressure in your tires of your car or bicycle
and measures how much force is being exerted on every
square inch of your tire’s surface. The force itself is a result
of the gas particles colliding with the surface of the
container. There are other units to measure pressure and in
chemistry we will either use atmospheres (1 atmosphere of
pressure is the amount of force exerted by the atmosphere
above use, about 14.7 psi), or kilopascal named after a
French mathematician and physicist (1 atmosphere = 101.3
kPa).
Pressure
Pressure simulator
• Web
• File
• Particles in the liquid phase, in a closed
container, may evaporate (go into the gas
phase while below the boiling point) and exert
a pressure. We call this vapor pressure, as it is
the pressure caused by the vapor and it does
not depend on how much liquid is in the
container.
Vapor Pressure
i.
Normal boiling point
• Particles in the liquid phase, in a closed container, may
evaporate (go into the gas phase while below the
boiling point) and exert a pressure. We call this vapor
pressure, as it is the pressure caused by the vapor and
it does not depend on how much liquid is in the
container. A substance will boil when it is heated to the
point that its vapor pressure is equal to that of its
environment. The normal boiling point is the
temperature at which the vapor pressure is equal to
standard pressure. Standard pressure has been defined
as 1 atmosphere (101.3 kPa) and can be found in your
reference tables under the Table A titled ‘Standard
Temperature and Pressure’.
i.
Normal boiling point
• If you change the pressure of the system a liquid is in,
you also change its boiling point. This is how you can
get LP (liquid propane) gas tanks for your grill. Propane,
at standard temperature, will be in its gas phase. In
order to store it in its more condensed liquid phase,
the pressure needs to be increased. This is why they
are stored in pressurized tanks. When you open the
tank, you let some of the propane out, which is then
exposed to a much lower pressure in the grill, becomes
a gas which is then ignited to cook some hot dogs,
hamburgers, chicken, maybe some corn…whatever
your little heart desires! It’s really up to you.
Don’t believe me?
• Let me show you!
Normal Boiling Point
• Pressure cookers also make use of the impact
of pressure on boiling points. A pressure
cooker doesn’t allow for gas to escape as
you’re cooking your meal. This causes the
pressure inside to build up, which increases
the temperature at which the water will boil.
This higher temperature allows the food to
cook faster!
Pressure Cooker
Using the reference tables
• Reference Table H is titles Vapor Pressure of
Four Liquids and can be used to determine the
boiling points of these liquids at different
temperatures. Remember, the boiling point is
the temperature at which the vapor pressure
equals the pressure of the system.
Using R.T. H
•
•
•
•
•
•
What are the normal boiling points for:
Propanone:____________
Ethanol:_____________
H2O:________________
Ethanoic Acid:_____________
What would the boiling point of water be at a
pressure of 200 kPa?__________
• What would the vapor pressure be for propanone at
50 degrees celcius?____________
• Which of these 4 liquids has the strongest attractive
force?_________________________
Do Now (Test Thursday)
•
•
•
•
Turn in Heat of Fusion Lab
Pick up a copy of the lab
Read over the procedures
(Next homework due tomorrow)
Safety
• Bunsen burner safety
– Not using it, turn it off!
• Beaker tongs to handle hot things
• Be careful when flipping your hot can, don’t let
the water escape
• Be careful in general
• Balloon + water: need about an inch of water
• Finished the lab?
– Finish the HW’s
Do Now
• Take out the lab from yesterday and your
homework packet
Reviewing the lab
• As Temperature increased, volume___________
• As Temperature decreased, pressure__________
• As the pressure increased, volume___________
– Neat demo…
And now
• Gases and pressure Practice in the ‘HW’
packet
• H.W. for tonight:
– Read the rest of the notes packet and attempt the
practice
– Short summary next class and then jumping right
into practice
Do Now:
• Take out homework #3 (gases and pressure)
• Read topic 5: Gas laws: Pressure, temperature
and volume
• Try the practice problems on the next page
Homework Review
•
•
•
•
•
C
A
B
D
D
•
•
•
•
•
•
•
•
•
202.6
19.25
~102
~25
~80
~70
~45
~123
~57
Gas laws: Pressure, temperature and
volume
• The Gas Laws are relationships between
temperature, pressure and volume of a gas.
Gas law equations are used to determine what
effect changing one of those variables will
have on any of the others. There are three gas
laws that combine to give us our ‘combined
gas law’, and they are:
Boyles Law:
• Boyles Law: P1V1=P2V2: As pressure on a gas
increases, the volume of the gas decreases.
The product of the initial pressure (P1) and
volume (V1) will be equal to the product of the
final pressure and volume (P2V2)
• Which experiment?
Charles Law
• Charles Law: V1/T1 = V2/T2: As temperature of
the gas increases, the volume of the gas must
also increase. The quotient of the initial
volume and temperature (V1/T1) is equal to
the quotient of the final volume and
temperature (V2/T2).
• TEMPERATURE NEEDS
TO BE IN KELVIN
• Which experiment?
Gay-Lussac’s Law
• Gay-Lussac’s Law: P1/T1 = P2/T2: As the
temperature of a gas increases, so does its
pressure. The quotient of the initial pressure
and temperature (in kelvin) (P1/T1) is equal to
the quotient of the final pressure and
temperature (P2/T2).
• Which experiment?
‘PT Cruiser’ Cards
• A neat way to remember how these three factors are
related is by what has been trademarked as a ‘PT Cruiser’
card. Simply take an index card and write across it the
letters P T V. To see how one factor will be affected by
changing one of the other two, simply grasp the card with
your finger covering the letter for the factor being kept
constant, push the variable that is being changed in the
direction in which it is changing (up for increasing, down for
decreasing) and see how the other variable responds. For
example: increasing pressure while temperature is kept the
same. You would cover grab the card at the temperature
letter, push the ‘P’ up, and see how the volume would
decrease!
Pt Cruiser Card
P T V
Combined Gas Law
• The three individual gas laws combine to give us
the combined gas law, which allows us to
examine how all three variables respond to a
change in a system without needing to have one
of the variables kept constant (seen on the right).
You can also get the other three gas laws from
this combined formula. If one of the variables is
kept constant, it simply drops out of the
equation. For example: If temperature was kept
the same, T would drop out and you would be
left with: P1V1=P2V2.
Solving for when something is held
constant
• A sealed can with an initial
pressure of #p1 is heated from
#t1 kelvin to #t2 kelvin. What is
the new pressure?
Solving for when something is held
constant
• A balloon with an initial
pressure of #p1 is heated from
#t1 kelvin to #t2 kelvin at a
constant pressure. What is the
new volume?
Practice: (remember temperature
needs to be in kelvin).
• What volume will 500.mL of a gas occupy if
the pressure is changed from 1.00 atmosphere
to 2.00 atmosphere at constant temperature?
P1 =
P2=
V1=
V2=
T1 =
T2=
• A tube of hydrogen gas at a room temperature of
22.4ºC has a pressure of 88.0 KPa. What was the
new temperature of the hydrogen gas when the
pressure in the tube is at 101.3 KPa? (Volume is
constant!)
P1 =
P2=
V1=
V2=
T1 =
T2=
• A gas has a volume of 700.mL at a temperature of
10.0ºC at constant pressure. What volume will the
gas occupy if the temperature is raised to 50.0ºC?
(Remember: change °C to K!!)
P1 =
P2=
V1=
V2=
T1 =
T2=
• 4 .) A sample of gas occupies a volume of 500. mL at
a pressure of 0.500 atm and a temperature of
298K. At what temperature will the gas occupy a
volume of 250. mL and have a pressure of 2.50
atm?
P1 =
P2=
V1=
V2=
T1 =
T2=
Homework:
• Finish the homework packet
• Start studying for the test/quarterly (heavy on
the periodic table)
Do Now
• Read the final topic: Gas laws; pV=nRT
Honors: Gas laws; pv=nRT
• The pressure and volume of a gas are
proportional to the number of moles of gas and
the Kelvin temperature. The equation can be
derived as follows:
• From the Combined Gas Law, we have
• PV/T = K,
• K = nR (n is number of moles, R is a
proportionality constant)
• (increase the number of moles, it affects
everything else…)
R
• Since one mole of gas exerts a pressure of
1.00 atm and occupies a volume of 22.4 L at
273 K, R (the proportionality constant) can be
derived as follows:
• (1 atm)(22.4 L)/(1 mole)(273 K) = R
• R = 0.0821 atm-L/mol-K
Ideal Gas Law
• This yields the IDEAL GAS LAW, which can be
used to determine the pressure, volume,
temperature or number of moles of gas if all of
the other conditions are known, and none of the
conditions have changed.
• PV = nRT
• P= Pressure (atm) V = Volume (L)
• n = moles
R = 0.0821 atm-L/mol-K
• T = Temp (K)
Practice with ideal gas law
• What is the pressure exerted by 3.00 moles of
gas at a temperature of 300. K in a 4.00 L
container?
• PV = nRT
What is the volume of a sample of gas
if 5.00 moles if it exerts a pressure of
0.500 atm at 200. K?
• PV = nRT
A sample of gas contained in a cylinder
of 5.00 L exerts a pressure of 3.00 atm
at 300. K. How many moles of gas are
trapped in the cylinder?
• PV = nRT
• A hydrogen gas thermometer is found to have
a volume of 100.0 cm3 when placed in an icewater bath at 0°C. When the same
thermometer is immersed in boiling liquid
chlorine, the volume of hydrogen at the same
pressure is found to be 87.2 cm3. What is the
temperature of the boiling point of chlorine?
• When filling a weather balloon with gas you have to
consider that the gas will expand greatly as it rises
and the pressure decreases. Let’s say you put about
10.0 moles of He gas into a balloon that can inflate
to hold 5000.0L. Currently, the balloon is not full
because of the high pressure on the ground. What
is the pressure when the balloon rises to a point
where the temperature is -10.0°C and the balloon
has completely filled with the gas.
Do Now
• Turn in any owed work (last day to turn in is
Friday of next week)
• Take out a sheet of paper and something to
write with
Topics on the test
• Properties of phases (solid vs liquid vs gas)
– Phase diagrams and describing how they behave
– Types of solids and their properties
• Conductivity, melting points, solubility, how they are ‘held
together’
•
•
•
•
Phase changes and heat of phase changes
Properties of gases (ideal vs real)
Gas law problems
Really, re-do the homework, read and re-do the
practice in the notes packet…as always, no real
surprises
Combined Gas Law Partner Practice
• As we have done in the past;
– 1st person writes the givens and rearranges the formula to
solve for what is missing
– 2nd person plugs and chugs, then rounds final answer
correctly to sig figs and gives units
– Switch for the next problem
• 1 sheet of paper per partnership
• Answers are on the back to ensure you are doing it
correctly
• Cant see what your’re doing wrong?
– Ask a neighbor, then ask me!
• A bag of potato chips is packaged at sea level (1.00
atm) and has a volume of 315 mL. If this bag of
chips is transported to Denver (0.775 atm), what
will the new volume of the bag be?
• 2) A Los Angeles class nuclear submarine has an
internal volume of eleven million liters at a pressure
of 1.250 atm. If a crewman were to open one of
the hatches to the outside ocean while it was
underwater (pressure = 15.75 atm), what be would
the new volume of the air inside the submarine?
• 3) A child has a toy balloon with a volume of 1.80
liters. The temperature of the balloon when it was
filled was 200 C and the pressure was 1.00 atm. If
the child were to let go of the balloon and it rose 3
kilometers into the sky where the pressure is 0.667
atm and the temperature is -100 C, what would the
new volume of the balloon be?
• 4) A commercial airliner has an internal pressure of
1.00 atm and temperature of 250 C at takeoff. If the
temperature of the airliner drops to 170 C during
the flight, what is the new cabin pressure?
•
• 5) If divers rise too quickly from a deep dive, they
get a condition called “the bends” which is caused
by the expansion of very small nitrogen bubbles in
the blood due to decreased pressure. If the initial
volume of the bubbles in a diver’s blood is 15 mL
and the initial pressure is 12.75 atm, what is the
volume of the bubbles when the diver has surfaced
to 1.00 atm pressure?
• GET READY FOR JEOPARDY!
TEST DAY!
•
•
•
•
•
•
Turn in Homework packet
Pick up:
Quarterly Review
New unit packet
HOMEWORK Read/highlight pages 1-4
Monday: Start the first day of the new unit,
then review for the quarterly
Take out the review from yesterday
• Any questions on it?
• Anything you would like me to go over?