Name: Period: _______Date: ___________

Pre-assessment SheetUnit 2

Classification of MatterDefine the following termsElement –

Compound –

Homogeneous mixture –

Heterogeneous mixture –

Give some examples of the followingPhysical change –

Chemical change –

How do particles move in the following?Solid –

Liquid –

Gas -

What makes an object float?

Name: Period: _______Date: ___________

What causes air or water pressure?

What happens when a gas is heated?

What happens when air is pressurized?

Summative AssessmentUnit 2

Classification of Matter TestDensity – malleability – solubility – viscosity – melting point – boiling point exothermic - ductility – state of matter - reactivity – flammability

Name: Period: _______Date: ___________

– size conductivity – compound - Pure substance - homogeneous - mass - mixtures heterogeneous – volume - endothermic – element - solubility - temperature

volume The amount of space that an object takes up. It is often measured in cm3, or ml.

Density The amount of matter in a space. It plays a role in the ability of a substance to float.

ductility A measure of how much strain a material can take before breaking. A material with this can be drawn into long thin wires.

exothermic A reaction in which energy is lost to the surroundings. This type of reaction/change will cause the noticeable heat and or light.

compound A pure substance made up of two or more elements. They cannot be separated by physically, but can be separated chemically

solubility a chemical property referring to the ability for a given substance, the solute, to dissolve in a solvent.

elements The simplest form of matter. They cannot be separated into physically or chemically. They are made of only one type of atom.

endothermic A reaction/change in which energy is taken from the surroundings often causing the temperature of the surroundings to decrease.

conductivity the degree to which a specified material conducts electricity orthe rate at which heat passes through a specified material

melting point The temperature at which a solid changes state be become a liquid. Water's for example is 0oC

viscosity A quantity that describes a fluid's resistance to flow. It describes the thickness of a fluid. It may change with temperature.

boiling point The temperature at which a liquid changes state be become a gas. Water's for example is 100oC

mixtures Matter that does not have a definite composition. They are physical blends of different substances that are easily separated.

homogeneous A type of mixture with uniform composition formed when substances are soluble. The particles are dissolved and not visible.

reactivity The rate at which a chemical substance tends to undergo a chemical reaction.

heterogeneous

A mixture with different composition formed when substances are not soluble. The different particles are clearly visible.

Pure substance

A type of matter that has a definite composition. Elements and compounds are examples.

The words in the word box may be used more than once - element, compound, homogeneous, heterogeneous, Chemical change, and physical change.

Copper SugarBurning log in a Salad

Name: Period: _______Date: ___________

bonfireWater Cutting with

scissorsOrange juice with pulp Gatorade

Boiling water Dissolving with strong acid

Iron Salt waterAnswer the questions below using the graph

What is the state of matter between A and B?What is the state of matter between C and D?What is the state of matter after E?What is happening to the kinetic energy between B and C?What is happening to the kinetic energy between C and D?What is happening to the potential energy between D and E?What is the melting point of this substance?What is the boiling point of this substance?Does this graph show an endothermic or an exothermic change?

Answer the questions below using the graph

Name: Period: _______Date: ___________

What is the mass of 4.8 mL of this substance?What is the volume of 85 g of this substance?What is the density of this substance?What is the name of this substance?What is on the X- axis of this graph?What is the dependant variable?

Pascal's Principle - P1/A1 = P2/A2

Boyle’s Law - P1V1 = P2V2

Charles’s Law - V1/T1 = V2/T2

A sample of neon gas has a volume of 837mL at 25OC what would the volume be at 100OC if the pressure remains constant?

A small balloon is inflated with helium at 102 kPa to a volume of 2.12 L. According to the balloon's manufacturer, if the balloon is stretched to a volume of 4.25 L, the balloon will pop. If the balloon were released, at what pressure would the balloon pop?

Assume constant temperature throughout. In changing a tire, a hydraulic jack lifts 7,468 N on its large piston, which has an area of 28.27 cm2. How much force must be exerted on the small piston if it has an area of 1.325 cm2?

Explain the following laws and principles in the space providedThe Law of Conservation

Name: Period: _______Date: ___________

of Matter

Kinetic Molecular Theory

Archimedes’ principle

Bernoulli’s Principle

Pascal’s Principle

Boyle’s law

Charles’ Law

Unit 2 Test

Name: Period: _______Date: ___________

Instructor: Mr. Benken

Instructions –There is to be no talking during the quiz. Clearly fill in the letter of the correct answer on the Scantron sheet. Draw a hot air balloon on the green lined space on the back of the Scantron sheet. Read over the questions carefully.

1. Describe how the particles in a gas move. a. Quickly in all directionsb. Stay in one place and vibratec. Do not move d. Medium speed and they roll

over each other

2. What is the term for a solid becoming a liquid?a. Evaporationb. Condensationc. Melting d. Sublimation

3. What is the term for a liquid becoming a solid? a. Evaporationb. Condensationc. Sublimation d. Freezing

4. What is the term for a solid becoming a gas?a. Evaporationb. Melting c. Sublimation d. Freezing

5. What is the term for a gas becoming a liquid? a. Evaporationb. Condensationc. Melting d. Freezing

6. If a block of wood has a volume of 10 cm3 and a mass of 5 grams what is the density of the wood?

a. 15 g/cm3

b. 0.5 g/cm3

c. 2 g/cm3

d. 50 g/cm3

7. If a bar of gold has a density of 20g/cm3 and weighs 2000g what is the volume of the gold bar

a. 100 cm3

b. 10 cm3

c. 20 cm3

d. 200 cm3

8. Describe how the particles in a solid move. a. Quickly in all directionsb. Stay in one place and vibratec. Do not move d. Medium speed and they roll

over each other

9. Describe how the particles in a liquid move.a. Quickly in all directionsb. Stay in one place and vibratec. Do not move d. Medium speed and they roll

over each other

10. If you increase the temperature the volume will increase. Whose law is this? a. Bernoulli’sb. Charles’c. Boyle’sd. Archimedes

Name: Period: _______Date: ___________

11. What will happen to the pressure inside of the container if its volume cannot be changed and you increase the temperature? a. Increasesb. Decreasesc. Does not changed. All of the above

12. If an object displaces more mass of fluid than the object’s mass the object will float in the fluid. Whose principle is this? a. Bernoulli’sb. Charles’c. Archimedes d. Pascal’s

13. If an object is more dense than water it willa. Sink to the bottomb. Float to the topc. Stay in the middled. None of the above

14. If an balloon is less dense than the air on the ground but more dense than the air in the upper atmosphere it willa. Sink to the bottomb. Float to the topc. Stay in the middled. None of the above

15. What is the term for a liquid becoming a gas? a. Evaporationb. Condensationc. Melting d. Sublimation

16. What happens to the speed of the particles if you heat them? a. Increasesb. Decreasesc. Does not changed. Stops completely

17. What happens to the speed of the particles if you cool them? a. Increasesb. Decreasesc. Does not changed. Stops completely

18. If you decrease the volume of a container the pressure will increase. Whose law is this?a. Bernoulli’sb. Charles’c. Boyle’sd. Archimedes

19. What will happen to the volume of the container if you increase the pressure inside of it? a. Increasesb. Decreasesc. Does not changed. All of the above

20. What will happen to the pressure if you increase the volume of a container a. Increasesb. Decreasesc. Does not changed. All of the above

21. If water goes from a big pipe into a small pipe it will move a. Faster b. Slower

22. The color of sulfur is aa. Chemical change

Name: Period: _______Date: ___________

b. Physical changec. Chemical propertyd. Physical property

23. Which of the following is another name for a homogeneous mixture?

a. Colloidb. Solution c. Suspensiond. Element

24. All phase changes (ie. solid to liquid or liquid to gas) are considered

a. Physical changesb. chemical propertiesc. matterd. solutions

25. The Law of Conservation of Mass holds true for

a. chemical changesb. physical changesc. Both A & B

26. Pepsi is an example of aa. Colloidb. Suspensionc. Solutiond. Substance

27. Which of the following is made of only one type of atom?

a. Mixtureb. Solution c. Carbond. Pizza

28. If you heat a gas what happens to the density? a. Increasesb. Decreasesc. Does not changed. All of the above

29. If you increase the pressure on a gas what happens to the density?a. Increasesb. Decreasesc. Does not changed. All of the above

30. When a fluid is moving there is a decrease in pressure that leads to an increase in velocity. Whose principle is this? a. Bernoulli’sb. Boyle’sc. Archimedes d. Pascal’s

31. If water moves quickly over the right side of a surface and not at all on the left side of a surface which direction will it move? a. Leftb. Rightc. Up d. Down

32. If air moves quickly over the top of a wing and slowly on the bottom of a wing which direction will the plane move? a. Leftb. Rightc. Up d. Down

Name: ______ Period: _______Date: ___________

The black and white circles above represent a different kind of atom. Match each box with its description below, write the letter of the correct box on the space provided. Each picture is used only one time.

33. Pure element ____________

34. Mixture of two elements ____________

35. Pure compound ____________

36. Mixture of two compounds ____________

37. Mixture of a compound and an element ____________

Station 1: What is Viscosity?Read the passage provided and investigate the materials.  

Name: ______ Period: _______Date: ___________

ViscosityFrom Wikipedia, the free encyclopedia

The viscosity of a fluid is a measure of its resistance to gradual deformation by shear stress or tensile stress. For liquids, it corresponds to the informal concept of "thickness". For example, honey has a much higher viscosity than water.[1]

Viscosity is a property arising from friction between neighboring particles in a fluid that are moving at different velocities. When the fluid is forced through a tube, the particles which comprise the fluid generally move faster near the tube's axis and more slowly near its walls: therefore some stress, (such as a pressure difference between the two ends of the tube), is needed to overcome the friction between particle layers and keep the fluid moving. For the same velocity pattern, the stress required is proportional to the fluid's viscosity.

A fluid that has no resistance to shear stress is known as an ideal fluid or inviscid fluid. Zero viscosity is observed only at very low temperatures, in superfluids. Otherwise, all fluids have positive viscosity, and are technically said to be viscous orviscid. In common parlance, however, a liquid is said to be viscous if its viscosity is substantially greater than water's, and may be described as mobile if the viscosity is noticeably less than water's. If the viscosity is very high, for instance in pitch, the fluid will appear to be a solid in the short term.

1. What is viscosity?

2. If you have a piece of a machine that needs to remain coated in a fluid, would you use a high or a low viscosity fluid?  Why?

3. If you are cooling a machine with a fluid and need a lot of fluid to move through it quickly, would you use a fluid with high or low viscosity?  Why?  

Changing Temperature and Viscosity1. Hold one of the room temperature corn syrup vials (labeled C) with the cap down so that

the metal sphere sinks in the fluid and touches the cap.

2. Prepare a stop watch to time the period of falling from the top of the vial to the bottom.

3. Invert the tube and start the timer

4. Record the time on the data table

5. Repeat these steps with the corn syrup vial that is resting the ice bath.

6. Repeat with the vials containing room temperature and ice cold polyvinyl alcohol solution (labeled A)

Station 2: ConductivityRead the passage provided and investigate the materials.  Use the multi-meter provided to investigate the conductivity of the various materials.  

Name: ______ Period: _______Date: ___________

1. What does it mean to be conductive?  

2. What are the 3 classifications of materials according to conduction?  

3. According to the reading, what are some examples of good conductors?  What are good insulators?  

4. According to the chart provided, what kinds of materials are good conductors?  

5. Touch the wood block and one of the metal pieces.  They are both the same temperature.  Which one feels cooler?  Why is this?  

6. Examine the materials provided.  List ones that are conductive and ones that are not.  What are some common traits about the conductive ones?  The non-conductive ones?  

7. If you are selecting a material to carry electricity.  What material would you select and why?  

8. You are selecting a material to block heat or electricity.  What material would you select and why?  

 

Conductivity is the measure of the ease at which an electric charge or heat can pass through a material. A conductor is a material which gives very little resistance to the flow of an electric current or thermal energy. Materials are classified as metals, semiconductors, and insulators. Metals are the most conductive

Name: ______ Period: _______Date: ___________

and insulators (ceramics, wood, plastics) the least conductive.

Electrical conductivity tells us how well a material will allow electricity to travel through it. Many people think of copper wires as something that has great electrical conductivity.

Thermal conductivity tells us the ease upon which thermal energy (heat for most purposes) can move through a material. Some materials like metals allow heat to travel through them quite quickly. Imagine that with one hand you are touching a piece of metal and with the other, a piece of wood. Which material would feel colder? If you said, "metal," you would be correct. But, in fact, both materials are in fact the same temperature. This is relative thermal conductivity. Metal has a higher heat transferability, or thermal conductivity, than wood, letting the heat from your hand leave faster. If you want to keep something cold the best idea is to wrap it in something that does not have a high heat transferability, or high thermal conductivity, this would be an insulator. Ceramics, and polymers are usually good insulators, but you have to remember that polymers usually have a very low melting temperature. That means if you are designing something that will get very hot the polymer might melt, depending on its melting temperature.

Electrical and thermal conductivity are closely related. For the most part good electrical conductors are also good thermal conductors.

Many products will contain both conductors and insulators- the conductors take the electricity or thermal energy where it is wanted and the insulators prevent it from getting where it isn't wanted.

Silver has the highest electrical conductivity of all metals. In fact, silver defines conductivity - all other metals are compared against it. On a scale of 0 to 100, silver ranks 100, with copper at 97 and gold at 76. Because of this property, and because it doesn't spark easily, silver is commonly used in electrical circuits and contacts. Silver is also utilized in batteries where dependability is mandatory and weight restrictions apply, such as those for portable surgical tools, hearing aids, pacemakers and space travel.

LINKShttp://www.physics4kids.com/files/elec_conduct.htmlLesson plan for teachers about conductivity- http://www.infinitepower.org/pdf/09-Lesson-Plan.pdf

Name: ______ Period: _______Date: ___________

Station 3: Boiling/Evaporation Point

Name: ______ Period: _______Date: ___________

Read the passages and examine the graphic provided.  Then follow the instructions below and answer the questions provided.

At this station are two small beakers. One has water in it, the other rubbing alcohol. Both have an eyedropper.

Using the eyedropper drop a drop of water on the back of your partners hand. As quickly as you can using the other eyedropper place a drop of rubbing alcohol on the back of your partners other hand.

1. Which liquid feels colder?  

2. Spread the liquids out a little.  Which one dries first? (you may need to wait a few minutes to answer this.)

3. What happens to a liquid to make it boil or evaporate?  

4. What is the difference between boiling and evaporating?  

5. What is the boiling point of water?  What is the boiling point of rubbing alcohol?

6. Does a lower boiling point mean it requires more or less energy to boil?  

7. What is happening to the rubbing alcohol at a faster rate than to water?  

8. Can you think of a way to separate rubbing alcohol from water without losing any water?  What is it?  Why will this work?  

9. Why does your skin feel colder from the rubbing alcohol than from the

EvaporationFrom Wikipedia, the free encyclopedia

Evaporation is a type of vaporization of a liquid that occurs from the surface of a liquid into a gaseous phase that is not saturated with the evaporating substance. The other type of vaporization is boiling, which is

Name: ______ Period: _______Date: ___________

characterized by bubbles of saturated vapor forming in the liquid phase. Steam produced in a boiler is another example of evaporation occurring in a saturated vapor phase. Evaporation that occurs directly from the solid phase below the melting point, as commonly observed with ice at or below freezing or moth crystals (napthalene or paradichlorobenzine), is called sublimation.

On average, a fraction of the molecules in a glass of water have enough heat energy to escape from the liquid. Water molecules from the air enter the water in the glass, but as long as the relative humidity of the air in contact is less than 100% (saturation), the net transfer of water molecules will be to the air. The water in the glass will be cooled by the evaporation until an equilibrium is reached where the air supplies the amount of heat removed by the evaporating water. In an enclosed environment the water would evaporate until the air is saturated.

With sufficient temperature, the liquid would turn into vapor quickly (see boiling point). When the molecules collide, they transfer energy to each other in varying degrees, based on how they collide. Sometimes the transfer is so one-sided for a molecule near the surface that it ends up with enough energy to 'escape'.

Evaporation is an essential part of the water cycle. The sun (solar energy) drives evaporation of water from oceans, lakes, moisture in the soil, and other sources of water. In hydrology, evaporation and transpiration (which involves evaporation within plant stomata) are collectively termed evapotranspiration. Evaporation of water occurs when the surface of the liquid is exposed, allowing molecules to escape and form water vapor; this vapor can then rise up and form clouds.

Station 4: Malleability/DuctilityRead the passage provided and examine the materials provided.

1. What is Malleability?  

Name: ______ Period: _______Date: ___________

2. How does the clay demonstrate Malleability?

3. What are some malleable materials?  

4. What is Ductility?  

5. How does the clay demonstrate Ductility?  

6. What are some ductile materials?  

7. What generally happens to the malleability of materials as their temperature increases?  

8. Describe a process to follow to shape a piece of metal if you need in a very specific shape?  Can you think of the name of this nearly – ancient job?  

What is malleability?Malleability is a physical property of metals that defines the ability to be hammered, pressed or rolled into thin sheets without breaking. In other words, it is the property of a metal to deform under compression. A metal's malleability can be measured by how much pressure (compressive stress) it can withstand without breaking. Differences in malleability amongst metals are due to variances in their crystal structures. Compression stress forces atoms to roll over each other into new positions without breaking their metallic bond. When a large amount of stress is put on a malleable metal, the atoms roll over each other, permanently staying in their new position.

Name: ______ Period: _______Date: ___________

Examples of malleable metals are:

Gold silver iron

aluminum copper tin

indium lithium

Examples of products demonstrating malleability include gold leaf, lithium foil and indium shot.

Malleability and Hardness:The crystal structure of harder metals, such as antimony and bismuth, makes it more difficult to press atoms into new positions without breaking. This is because the rows of atoms in the metal don't line-up, that is, more grain boundaries exist. Metals tend to fracture at grain boundaries - areas where atoms are not as strongly connected. So the more grain boundaries a metal has, the harder, more brittle and, therefore, less malleable it will be.

Malleability vs. Ductility:While malleability is the property of a metal deforming under compression, ductilityis the property of a metal allowing it to stretch without damage.Copper has both good ductility - it can be stretched into wires - and good malleability - it can also be rolled into sheets. Most malleable metals are also ductile, but the two properties can be exclusive. Lead and tin, for example, are malleable and ductile while cold, but become increasingly brittle as temperatures rise towards their melting points. Most metals, however, become more malleable when heated. This is due to the effect of temperature on the crystal grains within metals.

Controlling Crystal Grains:Temperature has a direct affect on the behavior of atoms, and in most metals heat results in atoms having a more regular arrangement. This reduces the number of grain boundaries, thereby, making the metal softer or more malleable. An example of temperature's affect on metals can be seen with zinc, which is a brittle metal below 300°F (149°C). Yet when heated above this temperature, zinc can become so malleable that it can be rolled into sheets. In contrast to the affect of heat treatment, cold working - a process that involves working (rolling, drawing or pressing causing plastic deformation) a cold metal - tends to result in smaller grains, making the metal harder. Alloying is another common method of controlling grain sizes to make metals more workable. Brass, an alloy of copper and zinc, is harder than both individual metals because its grain structure is more resistant to compression stress attempting to forces the rows of atoms from shifting into new positions.

Station 5:  Melting / Freezing PointRead the Passage provided.  Then observe the two objects in the tray before you.  

Melting Point and Freezing Point

Pure, crystalline solids have a characteristic melting point, the temperature at which the solid melts to become a liquid. The transition between the solid and the liquid is so sharp for small samples of a pure substance that melting points can be measured to 0.1oC. The melting point of solid oxygen, for example, is -218.4oC.

Name: ______ Period: _______Date: ___________

Liquids have a characteristic temperature at which they turn into solids, known as their freezing point. In theory, the melting point of a solid should be the same as the freezing point of the liquid. In practice, small differences between these quantities can be observed.It is difficult, if not impossible, to heat a solid above its melting point because the heat that enters the solid at its melting point is used to convert the solid into a liquid. It is possible, however, to cool some liquids to temperatures below their freezing points without forming a solid. When this is done, the liquid is said to be supercooled.A liquid can become supercooled because the particles in a solid are packed in a regular structure that is characteristic of that particular substance. Some of these solids form very easily; others do not. Some need a particle of dust, or a seed crystal, to act as a site on which the crystal can grow. Because it is difficult to heat solids to temperatures above their melting points, and because pure solids tend to melt over a very small temperature range, melting points are often used to help identify compounds. We can distinguish between the three sugars known as glucose (MP= 150oC), fructose (MP = 103-105oC), and sucrose (MP = 185-186oC), for example, by determining the melting point of a small sample.Measurements of the melting point of a solid can also provide information about the purity of the substance. Pure, crystalline solids melt over a very narrow range of temperatures, whereas mixtures melt over a broad temperature range. Mixtures also tend to melt at temperatures below the melting points of the pure solids.

1. What does it mean for a substance to melt?  Freeze?

2. How does the freezing point of a substance generally compare to the melting point of the same substance?  

3. Are all melting points the same?  

4. Consider the metal block and the glass of water.  What can you tell me about the temperature of the items in comparison to their melting points?  

5. Is it possible to separate out different materials using the understanding of the freezing and melting points?  If so describe a way to do so.  

Station 6:  HardnessMohs Hardness Scale

Name: ______ Period: _______Date: ___________

Different methods are the base for hardness tests of minerals. Commonly used and internationally known is the Mohs (mineralogist, 1773-1839) hardness scale. It depends on the discovery that softer substances scratch harder ones. So Mohs created his scale, arranging 10 minerals according to their scratching hardness from the softest material (talcum) with hardness 1 up to the hardest material (diamond) with hardness 10. The Mohs scale is a relative scale. Later other scales were developed which show the absolute hardness: The Rosiwal scale e.g. shows the expenditure during the cutting ("cutting hardness"), the Vickers (airplane factory) scale shows the denting depth of a material. Regarding gemstones the Mohs hardness is always meant when dealers and buyers meet. 

1. What does the hardness of a material refer to?  

2. If a material is harder than another material, what could it do it it?

3. What do we use Mohs Scale to identify?

4. What is the softest mineral known?  

5. What is the hardest mineral known?  

6. Use the materials in the scratch test kit.  Attempt to determine the approximate hardness of the materials provided. Create a chart that names the materials and the hardness of each.

Station 7:  Buoyancy

Name: ______ Period: _______Date: ___________

Archimedes' principleFrom Wikipedia, the free encyclopedia

Archimedes' principle indicates that the upward buoyant force that is exerted on a body immersed in a fluid, whether fully or partially submerged, is equal to the weight of the fluid that the body displaces. Archimedes' principle is a law of physics fundamental to fluid mechanics. Archimedes of Syracuse [1]  formulated this principle, which bears his name.

In On Floating Bodies, Archimedes stated (c. 250 BC):

Any object, wholly or partially immersed in a fluid, is buoyed up by a force equal to the weight of the fluid displaced by the object.

—  Archimedes of Syracuse

Practically, the Archimedes principle allows the buoyancy of an object partially or wholly immersed in a liquid to be calculated. The downward force on the object is simply its weight. The upward, or buoyant, force on the object is that stated by Archimedes' principle, above. Thus the net upward force on the object is the difference between the buoyant force and its weight. If this net force is positive, the object rises; if negative, the object sinks; and if zero, the object is neutrally buoyant - that is, it remains in place without either rising or sinking. In simple words, Archimedes' principle states that when a body is partially or completely immersed in a fluid, it experiences an apparent loss in weight which is equal to the weight of the fluid displaced by the immersed part of the body.

FormulaConsider a cube immersed in a fluid, with its sides parallel to the direction of gravity. The fluid will exert a normal force on each face, and therefore only the forces on the top and bottom faces will contribute to buoyancy. The pressure difference between the bottom and the top face is directly proportional to the height (difference in depth). Multiplying the pressure difference by the area of a face gives the net force on the cube – the buoyancy, or the weight of the fluid displaced. By extending this reasoning to irregular shapes, we can see that, whatever the shape of the submerged body, the buoyant force is equal to the weight of the fluid displaced.

The weight of the displaced fluid is directly proportional to the volume of the displaced fluid (if the surrounding fluid is of uniform density). The weight of the object in the fluid is reduced, because of the force acting on it, which is called upthrust. In simple terms, the principle states that the buoyant force on an object is equal to the weight of the fluid displaced by the object, or the density of the fluid multiplied by the submerged volume times the gravitational constant, g. Thus, among completely submerged objects with equal masses, objects with greater volume have greater buoyancy.

Suppose a rock's weight is measured as 10 newtons when suspended by a string in a vacuum with gravity acting on it. Suppose that when the rock is lowered into water, it displaces water of weight 3 newtons. The force it then exerts on the string from which it hangs would be 10 newtons minus the 3 newtons of buoyant force: 10 − 3 = 7 newtons. Buoyancy reduces the apparent weight of objects that have sunk completely to the sea floor. It is generally easier to lift an object up through the water than it is to pull it out of the water.

Name: ______ Period: _______Date: ___________

Material Density (g/cm3)Gold 19.3

Mercury 13.6Lead 11.3Silver 10.5

Aluminum 2.7Glass 2.58

Rubber 1.1Cork 0.24Air 0.0013

1) What is the density of water?

2) For an object to float in water, what must it’s density be?

3) The diver in the bottle is made of a glass eyedropper. List the three parts of the diver and the densities of each of the parts

4) Two of the three parts are denser than water. How is it that the diver is floating right now?

5) Squeeze the bottle until you observe a change. Then release the bottle. Describe what happens to the diver in both conditions?

6) Explain what is causing the change when you squeeze the bottle and when you release the bottle.

7) Apply your observations to a Navy submarine. How can a boat at certain times sink without sinking and at other times float just like any other boat?

Classification of Matter Test

Name: ______ Period: _______Date: ___________

Density – malleability – solubility – viscosity – melting point – boiling point exothermic - ductility – state of matter - reactivity – flammability – size conductivity – compound - Pure substance - homogeneous - mass - mixtures heterogeneous – volume - endothermic – element - solubility - temperature

The amount of space that an object takes up. It is often measured in cm3, or ml.The amount of matter that is in a space. It play a role in the ability of a substance to float.A measure of how much strain a material can take before breaking. A material with this can be drawn into long thin wires.A reaction in which energy is lost to the surroundings. This type of reaction/change will cause the noticeable heat and or light.A pure substance made up of two or more elements. They cannot be separated by physically, but can be separated chemicallya chemical property referring to the ability for a given substance, the solute, to dissolve in a solvent.The simplest form of matter. They cannot be separated into physically or chemically. They are made of only one type of atom.A reaction/change in which energy is taken from the surroundings often causing the temperature of the surroundings to decrease.the degree to which a specified material conducts electricity orthe rate at which heat passes through a specified materialThe temperature at which a solid changes state be become a liquid. Water's for example is 0oCA quantity that describes a fluid's resistance to flow. It describes the thickness of a fluid. It may change with temperature.The temperature at which a liquid changes state be become a gas. Water's for example is 100oCMatter that does not have a definite composition. They are physical blends of different substances that are easily separated.A type of mixture with the same composition formed when substances are soluble. The particles are dissolved and not visible.The rate at which a chemical substance tends to undergo a chemical reaction.A mixture with different composition formed when substances are not soluble. The different particles are clearly visible.A type of matter that has a definite composition. Elements and compounds are examples.

The words in the word box may be used more than once - element, compound, homogeneous, heterogeneous, Chemical change, physical change.

Name: ______ Period: _______Date: ___________

Copper SugarBurning log in a bonfire Salad

Water Cutting with scissors

Orange juice with pulp Gatorade

Boiling water Dissolving with strong acid

Iron Salt waterAnswer the questions below using the graph

What is the state of matter at A?What is the state of matter at D?What is the state of matter at H?What is happening to the kinetic energy between B and C?What is happening to the kinetic energy between D and E?What is happening to the potential energy between A and B?What is happening to the potential energy between F and G?What is the melting point of this substance?What is the boiling point of this substance?Is this a graph of an endothermic or an exothermic change?Find the mass of 250.0 mL of benzene. The density of benzene is 0.8786 g/mL.m = Show your work Final answer

Name: ______ Period: _______Date: ___________

v =

d =

A block of aluminum with a volume of 15.0 mL weighs 40.5 g, what is its density?m =

v =

d =

Show your work

Final answer

Explain the kinetic theory of matter -

Explain the law of conservation of matter -

Answer the

questions below using the graph

What is the mass of 4.8 mL of this substance?What is the volume of 85 g of this substance?What is the density of this substance?What is the name of this substance?What is on the X- axis of this graph?What is the dependant variable?

Pascal's Principle - P1/A1 = P2/A2 Boyle’s Law - P1V1 = P2V2

Charles’s Law - V1/T1 = V2/T2

A sample of neon gas has a volume of 837mL at 25OC what would the volume be at

Name: ______ Period: _______Date: ___________

100OC if the pressure remains constant?

A small balloon is inflated with helium at 102 kPa to a volume of 2.12 L. According to the balloon's manufacturer, if the balloon is stretched to a volume of 4.25 L, the balloon will pop. If the balloon were released, at what pressure would the balloon pop?

Assume constant temperature throughout. In changing a tire, a hydraulic jack lifts 7,468 N on its large piston, which has an area of 28.27 cm2. How much force must be exerted on the small piston if it has an area of 1.325 cm2?

Explain the following laws and principles in the space provided

Kinetic Molecular Theory

Archimedes’ principle

Bernoulli’s Principle

Pascal’s Principle

Boyle’s law

Charles’ Law

Name: ______ Period: _______Date: ___________