Unit 1, Properties of Matter

Warm Up
• An experiment requires the use of a lab apron, goggles, and insulated mitts or beaker tongs. The purpose of these safety items is primarily to protect against a. release of hazardous gases b. hot materials and spills of harmful liquids c. contamination of chemicals and glassware d. staining of lab clothing

Today’s Learning Objective
Today you will. . .
• Differentiate between the states of matter based on their properties

Today’s Agenda
• Warm Up
• States of Matter Video
• States of Matter Notes
• States of Matter Puzzles
• Ice Cube Melting Activity
• Review Video
• Critical Safety Questionnaire
• Exit Slip

• How are the physical properties of solids, liquids, and gases explained?
• States of Matter Video

Matter Defined
• Matter is anything that has mass and takes up space.
• Mass is the amount of matter in an object.
 Is air an example of matter? Why or why not?

States of matter
• Matter is made up of particles that are in constant motion.
• This constant motion gives the particles kinetic energy
(energy of movement)
• The temperature of a substance is a measure of the average kinetic energy of all the particles of the substance.
• As these particles move, they attract, or pull, other particles towards themselves.
• The state of matter is determined by how fast the particles move and how strongly attracted they are to one another.
 Which state of matter has the most kinetic energy?

• Particles have low kinetic energy
• Particles cannot flow (particles flow when they move past one another)
• Solids have a definite shape and volume and are not compressible.
• A solid maintains its volume and shape because the particles in it are packed tightly and are held together by strong attractive forces.
• Particles vibrate in relatively fixed positions
 Why are solids not compressible?

• Particles are relatively close together, but have enough energy to move past one another (flow)
• Therefore, liquids take the shape of their container
• However, liquid still have a definite volume and are not compressible.
• Particles have more kinetic energy than those of solids, but less than those of gases
 Are attractive forces greater in solids or in liquids?

• Particles have high kinetic energy—they move rapidly in all directions and are far apart
• A gas expands to fill its container, taking on the volume and the shape of the container
• Gases expand with an increase in temperature.
• Gases are compressible
 How could you shrink an inflated balloon?
• Shrinking balloon video


Which state of matter is shown in each picture? How do you know?
Liquid Gas Solid

Solid
Definite
Volume?
Definite
Shape?
Temp. increase
Compressible?
YES
YES
Small
Expans.
NO
Liquid
YES
NO
Small
Expans.
NO
Gas NO NO
Large
Expans.
YES

Ice Cube Melting Activity
• Obtain an ice cube, zip top bag, and timer from a teacher.
• Your task is to melt the ice cube in the shortest time possible.
 What did you have to add to the ice cube to get it to melt faster? Write your thoughts on your warm up sheet.

States of Matter Review Video
• YouTube Review Video

Exit Slip
1. As the temperature of a gas is increased, what happens to the kinetic energy of its molecules?
2. Which state of matter has defined volume and shape and is not compressible?
3. Which state of matter is compressible? Why is this?

Warm Up
The same amount of hydrogen gas is in both containers. The pressure in container B is a. ¼ the pressure in container A b. ½ the pressure in container A c. 2 times the pressure in container A d. 4 times the pressure in container B

Today’s Learning Objective
Today you will. . .
Describe the changes in energy and the arrangement of particles that take place during a change of state (phase change).

Today’s Agenda
• Warm Up
• States of Matter Venn Diagram
• Review for Quiz
• Quiz 1.1
• Dry Ice Sublimation Demonstration
• Changes of State Notes
• Exit Slip

• How does the arrangement of particles change during changes of state?
• How does energy transfer during changes of state?

• Particles of matter have kinetic energy. The more kinetic energy a particle has, the faster and farther it moves.
• When matter changes state, energy is either absorbed or released, but chemical composition of the substance does not change.
• The temperature of a substance is the average kinetic energy of all the particles of the substance.
 Is energy absorbed or released as a liquid changes to a gas?

Melting
• Solid changes to liquid.
• An increase in KE allows the particles to vibrate so intensely that attractive forces are overcome and the particles can begin to move past one another (flow).
• Melting point: the temperature at which solid changes to liquid
 When you melted the ice cube at the beginning of class, how did you get it to melt?

Freezing
• Liquid changes to solid
• As a liquid substance cools and loses energy, the particles slow down and get closer together.
• Eventually, the attraction between the particles overcomes their motion, and the substance becomes a solid.
• Freezing point: the temperature at which liquid changes to solid
 Why don’t solids flow?

Vaporization
• Liquid changes to gas
• The particles of a liquid gain energy, the motion of the particles increases, and temperature rises.
• When the particles of the liquid have enough energy to overcome attractive forces, the particles become free to spread apart.
• Boiling point: the temperature at which vaporization occurs throughout the liquid
 How does vaporization differ from boiling?

Condensation
• Gas changes to liquid
• Occurs as a gas cools, releasing thermal energy.
• The particles slow down and when the attractive forces pull them together, the gas becomes a liquid.
• The condensation point is the same as the boiling point of the substance.
• Example: clouds form from condensation
 Why does a cold glass of water
“sweat”?

Sublimation
• Solid changes to gas
• The particles of the solid absorb enough energy to go from being very tightly packed to being very far apart.
• Example: As a comet approaches the sun, some of the solids inside it change to gases, resulting in the visible “tail” of the comet.
 What is another example of sublimation?

Changes of State Summary
Freeze
Melt
Condense
Evaporate
Solid Liquid Gas

Sublimation
Solid
Definite Shape
Cannot flow
Particles tighly packed
Freezing
Melting
Liquid
Small expansion with temp. increase
Not compressible
Definite volume Particles slide past each other
Atoms
Matter
Particles can flow
No definite shape
Large expansion with temp. increase Compressible
Vaporization
Boiling
Evaporation
No definite volume
Condensation
Particles move quickly
Gas

Exit Slip
• Does water melt and freeze at the same temperature? How do you know?

Warm Up
• We demonstrated dry ice changing state from solid to gas. The term for this type of change is a. vaporization b. sublimation c. melting d. evaporating
• Does water melt and freeze at the same temperature? How do you know?

Today’s Learning Objective
Today you will:
• Analyze the phase change of water

Today’s Agenda
• Warm Up
• Go over Quiz 1.1
• Definitions
• Pre-lab Questions
• Phase Change of Water Lab
• Notes on Heating Curve of Water
• Exit Slip

Heating Curve of Water Lab
• Variable
– factors that affect the results of an experiment
• Dependent Variable
– the variable in an experiment that changes in response to choices made by the experimenter
– this variable is plotted on the y-axis of a graph
• Independent Variable
– the variable in an experiment that is manipulated by the experimenter
– causes changes in the dependent variable in the experiment
– this variable is plotted on the x-axis of a graph

Heating Curve of Water
Temperature does not change during changes of state. That is why the line is horizontal at those points on the curve.

Exit Slip
1. Why do you see a horizontal line (plateau) on your heating curve graphs when water is changing state?
2. Which state of water has the largest amount of kinetic energy?
a. liquid b. solid c. gas d. they all have the same amount

Warm Up
• Explain why temperature does not change during a change of state.

Today’s Learning Objective
Today you will…
• Analyze physical and chemical properties of matter

Today’s Agenda
• Warm Up
• Review for Quiz
• Quiz 1.2
• Properties of Matter Notes
• Properties of Matter Whiteboard Activity
• Pre-lab Questions
• Properties of Matter Lab
• Exit Slips

Properties of Matter
 All matter can be described through a combination of characteristics called properties
 There are two categories of properties
 Physical
 Chemical

 Can be observed without changing the substance itself
 Describe the size, shape, appearance, amount, and physical attributes of the matter
 Examples:
 Color, mass, volume, shape, texture
 State of matter, melting point, boiling point, density, conductivity, malleability, ductility
 Explain why melting point is a physical property.

• Chemical properties can only be observed by changing the matter itself
• Examples
– Reactivity (iron reacts with oxygen to form rust)
– Combustibility (hydrogen gas burns easily)
– Corrosiveness (sulfuric acid burns skin)

• Flammability
– Chemical
Physical or Chemical?
• Malleability
– Physical
• Melting point
– Physical (change of state)
• Ability to rust
– Chemical
• Ability to tarnish
– Chemical

Exit Slip
1. One chemical property of matter is a. boiling point b. reactivity c. texture d. density

Warm Up
1. A physical property may be investigated by a. melting ice b. allowing silver to tarnish c. letting milk turn sour d. burning wood
2. Rust is formed on iron pipes after prolonged exposure to humid air. What type of change does this illustrate?

Today’s Learning Objective
Today you will…
• Analyze the physical properties density and viscosity, and determine density for substances

Today’s Agenda
• Warm Up
• Go over Quiz 1.2
• Notes on Viscosity and Density
• Notes on Density Calculations
• Density Calculations Practice
• Exit Slip

• Viscosity is defined as the resistance of a fluid to flow
• A substance that pours more slowly has a higher viscosity.
 Give an example of a liquid that is more viscous than water.

 Physical property that measures how tightly packed matter is
 Density is a comparison of how much matter there is in a certain amount of space.
 Directly related to the mass of matter and inversely related to the volume

• If you pour together liquids that don’t mix and have different densities, they will form layers in the order of their densities.
 Imagine that the liquids have the following densities:
– 10g/cm 3 .
3g/cm 3 .
– 6g/cm 3 .
5g/cm 3 .
Which density value goes with each layer?
3 g/cm 3
5 g/cm 3
6 g/cm 3
10 g/cm 3

Try this problem:
 Densities of common substances at room temperature (g/cm 3 )
Water 1.00
Aluminum 2.70
Gold 19.3
Wood 0.6
Mercury is a liquid at room temperature with a density of 13.6g/cm 3 .
Would a bar of aluminum float or sink in a pool of liquid mercury?
Float, because the density of aluminum is less than that of mercury.

Calculating Density
• Density = Mass
Volume
• Units: g/mL or g/cm 3
 A block of wood has a mass of 400 g and a volume of 650 cm 3 . What is the density of the wood in g/cm 3 ?
m = 400 g v = 650 cm 3
D = m/v
D = 400 g
650 cm 3
D = 0.6 g/cm 3

Calculating Density
 Lead has a density of 11.34 g/cm 3.
If a sample of lead has a mass of 5.67 g, what is the volume of the sample?
d = 11.34 g/cm3 m = 5.67 g
D = m/v
11.34 g/cm 3 = 5.67 g
V
V = 5.67 g / 11.34 g/cm 3
V = 0.5 cm 3

Exit Slip
• The picture shows the results of pouring a blue liquid into a clear liquid and allowing the mixture to settle for 25 minutes. Compared to the clear liquid, the blue liquid is more a. massive b. dense c. viscous d. soluble

Warm Up
1. What is the density of 12 mL of a liquid that has a mass of
4.05 grams?
a. 0.338 g/mL b. 2.96 g/mL c. 16.1 g/mL d. 48.6 g/mL
2. What is the mass of a 500.00 mL sample of seawater with a density of 1.025 g/mL?
a. 487.8 g b. 500.0 g c. 512.5 g d. 625.0 g

Today’s Agenda
• Warm Up
• Finish Density Practice
• Review for Quiz
• Quiz 1.3 (“Pre-Test”)
• Density Column Lab
• Exit Slip

Exit Slip
• What liquid was the bottom layer in your density column? Why was it the bottom layer?

Today’s Learning Objective
Today you will…
• Analyze the physical property buoyancy

Exit Slip
• How do objects that are more dense than water float?

Warm Up
1. Students in a chemistry lab measure the time it takes four different 100 mL solutions to pass through a hole in the bottom of the cup. Which of the following properties of the solutions is most likely being measured?
a. Buoyancy b. Mass c. Viscosity d. Volume
2. How are density and viscosity related?

Today’s Learning Objective
Today you will…
• Analyze the physical property buoyancy
• Solidify your understanding of Unit 1 concepts

Today’s Agenda
• Warm Up
• Go over Quiz 1.3
• Review for Unit 1 Test
• Exit Slip

• Buoyancy is the upward force fluids exert on objects.
• Archimedes Principle-
The buoyant force is equal to the weight of the fluid the object displaces or takes the place of.
• An object will float if the water it displaces has a greater mass than the object's mass.

Exit Slip
• Which of the following objects will float on water? Why?
a. b. c. d.

Warm Up
• A block of maple wood with a volume of 405 cubic centimeters and a density of 0.67 g/cm 3 is sawed in half. The density of the two smaller blocks is now a. ¼ the original density b. ½ the original density c. 2 times the original density d. the same as the original density

Solid
Definite
Volume?
Definite
Shape?
Temp. increase
Compressible?
YES
YES
Small
Expans.
NO
Liquid
YES
NO
Small
Expans.
NO
Gas NO NO
Large
Expans.
YES

Changes of State Summary
Freeze
Melt
Condense
Evaporate
Solid Liquid Gas

Heating Curve of Water
Temperature does not change during changes of state. That is why the line is horizontal at those points on the curve.

• Flammability
– Chemical
Physical or Chemical?
• Malleability
– Physical
• Melting point
– Physical (change of state)
• Ability to rust
– Chemical
• Ability to tarnish
– Chemical

• If you pour together liquids that don’t mix and have different densities, they will form layers in the order of their densities.
 Imagine that the liquids have the following densities:
– 10g/cm 3 .
3g/cm 3 .
– 6g/cm 3 .
5g/cm 3 .
Which density value goes with each layer?
3 g/cm 3
5 g/cm 3
6 g/cm 3
10 g/cm 3

Calculating Density
• Density = Mass
Volume
• Units: g/mL or g/cm 3
 A block of wood has a mass of 400 g and a volume of 650 cm 3 . What is the density of the wood in g/cm 3 ?
m = 400 g v = 650 cm 3
D = m/v
D = 400 g
650 cm 3
D = 0.6 g/cm 3

Today’s Learning Objective
Today you will…
• Demonstrate level of mastery of Unit 1 material

Today’s Agenda
• Warm Up
• Review for Test
• Unit 1 Test
• Fill out Unit 2 Key Terms
• Start Notes for Unit 2
• Exit Slip

Exit Slip
• What was the design of the boat that held the most pennies? Why did this boat win?

Unit 1 Key Terms
• Compressibility-the property of being able to occupy less space; capable of being more compact
• Fluidity-the property of flowing easily; the state of being fluid rather than viscous
• Kinetic Energy-the energy of an object due to its motion
• Sublimation-a change directly from the solid to gaseous state without becoming liquid
• Temperature-a measurement of the average kinetic energy of the particles in a system
• Vaporization-gasify; to turn into a gas; evaporate
• Viscosity-the state of being thick, sticky, and semifluid in consistency; having a high resistance to flow

Unit 1 Key Terms
• Boiling point-the temperature at which a liquid boils and turns to vapor.
• Buoyancy-the ability or tendency to float in water or air or some other fluid
• Chemical change-a change in the chemical composition of a substance to produce a new material with new properties
• Chemical property-any of a material's properties that becomes evident during a chemical reaction; any quality that can be established only by changing a substance's chemical identity
• Condensation-the conversion of a vapor or gas to a liquid
• Conductivity-the degree to which a specified material conducts electricity

Unit 1 Key Terms
• Density-the degree of compactness of a substance; measured by the quantity of mass per unit volume
• Ductility-capable of being pulled or stretched into thin wire by mechanical force without breaking; molded easily into a new form
• Freezing-the withdrawal of heat to change something from a liquid to a solid
• Gas-an airlike fluid substance which expands freely to fill any space available
• Liquid-having a consistency like that of water or oil; flowing freely but of constant volume
• Malleability-the property of something that can be worked or hammered or shaped without breaking

Unit 1 Key Terms
• Mass-quantity or amount of something
• Melting-change something to a liquid condition by heating it
• Phase change-a change from one state (solid or liquid or gas) to another without a change in chemical composition
• Physical change-a process in which the basic chemical identity of the substances in unchanged; a good example is heating water to its boiling point; the water changes from liquid to gas, but is still water
• Physical property-a property which can be determined without changing something chemically
• Reactivity-the state or power of being reactive or the degree to which a thing is reactive
• Solid-of definite shape and volume; firm; neither liquid nor gaseous; "ice is water in the solid state"
• Volume-the amount of space that a substance or object occupies, or that is enclosed within a container

Phase Change Videos
• Joe Genius Video
• Discovery Education Types of Phase Change