Do Now: Find new seats

Do Now: Find new seatsmelanie 1

andretta 2

jennifer 3

elias 4

mariah 5

casandra 6

shaquom 7

augustin 8

zacharia 9

ian 10

joy 11

Shajra 12

de'andre 13

hector 14

julianna 15

isabella 16

jacob 17

arianna 18

gabrielle 19

Jose 20

Nailah 21

syndey 22

emily 23

Se'jean 24

angelica 25

daniel 26

jairo 27

christina 28

kayla 29

Do Now: Find New Seats

egar 1alexandra 2damien 3kiara 4lorena 5denzell 6olivia 7emma 8

jordan 9elijah 10yasheema 11joshua 12mina 13christopher 14kevin 15bruno 16

joseph 17seth 18johanan 19lindsey 20itzel 21Jessica 22jonathan 23vernon 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 slg?– 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 Metallic• Sol.• Cond.• M.p.

• 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/states-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.

Gas(particle diagram)

Liquid(particle diagram)

Solid(particle diagram)

_____thermic _____thermic+ or - ΔH + or - ΔH

1.___________

2.___________

3.___________

4.___________

5.___________6.___________

Time

Tem

p. (K

)

Time

Tem

p. (K

)

Sublimation and Deposition

• http://www.youtube.com/watch?v=4E0sy-FN2M8

• 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 sameDo 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 ice-water 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?