UNIT 2: PHYSICAL BEHAVIOR OF MATTER DO NOW: Answer the following questions: 1. What is matter? 2. What are the different states of matter and list one example of each?

Aim # 1: What kinds of matter are there? What is matter? Has mass Takes up space Made up of atoms

AIM # 1: What kinds of matter are there? Classification of matter SUBSTANCES Elements and Compounds: are all HOMOGENEOUS containing the same composition of material throughout the sample Elements: substances that cannot be broken down by chemical change Symbols are on Periodic Table Ex. N (nitrogen) Ni (nickel)

Two or more element symbols combined Ex. NaCl, H2O Compounds: substances that are made up of elements chemically bonded together, can be decomposed by chemical means. Two or more element symbols combined Ex. NaCl, H2O constant composition MIXTURES: combination of substances that are not chemically combined together, and can be broken down by physical means ratio will vary

AIM # 2: How can you turn one form of matter into another form?

Ex: salt water Ex: sand water AIM # 2: How can you turn one form of matter into another form? Types of mixtures MIXTURES Homogeneous Mixture: solution of uniform composition (aq) Ex: salt water Heterogeneous Mixture: non uniform composition Ex: sand water

AIM # 2: How can you turn one form of matter into another form? Soluble- the ability to be dissolved, produces a solution (aq) Water is the universal solvent Insoluble- unable to dissolve in a liquid, can remain a solid, or separate from the solution (s) Miscible- “mixable”, the ability to form a homogenous mixture, the ability to dissolve within one another Seltzer and orange juice Immiscible- incapable of being mixed with one another Oil and water (Italian salad dressing)

AIM # 2: How can you turn one form of matter into another form AIM # 2: How can you turn one form of matter into another form? Law of Conservation MATTER CANNOT BE CREATED NOR DESTROYED, BUT CAN CHANGE FROM ONE FORM TO ANOTHER

Law of Conservation Examples: If 40 grams of substance A are reacted with 20 grams of substance B to form substance C, what will the mass of substance C be? 35 grams of liquid water are evaporated off in a closed container. How many grams of water vapor will there be when the process is done? Magnesium metal is reacted with oxygen to form magnesium oxide. How will the mass of the magnesium oxide be compared to the combined masses of the magnesium metal and the oxygen that formed it?

Particle Diagrams

Particle Diagrams

Aim # 3: What are the specific properties of matter? Intensive property- a property of matter that is independent of the amount, does not need a specific quantity Color, melting point, boiling point, density Extensive property- a property of matter that is dependent on the amount Mass, Volume, length, shape

AIM # 3: What are the specific properties of matter AIM # 3: What are the specific properties of matter? Physical Properties and Changes Physical Changes: changes that change only the appearance of the substance, not its chemical identity Physical Properties: properties that can be observed though physical change

AIM #3 : What are the specific properties of matter?

Chemical Properties and Changes Chemical Changes: changes that result in changing the chemical composition of a substance, can be reversed by another chemical change – results in a new substances being formed Chemical Properties: properties that can only be observed through a chemical change

AIM # 4 : How does the proximity of atoms or molecules to each other affect properties they exhibit? States of Matter

SOLIDS Particles tightly packed together Particle Movement type: vibrate Has definite shape Has definite volume If you put a sneaker in a box its volume doesn’t change

LIQUIDS Particles are moderately packed together Particle movement: Vibrate and Rotate No definite shape, Takes the shape of its container Has Definite Volume

GAS (vapor) Particles are loosely packed Particle movement: Vibrate, Rotate & bounce off container Has No Definite Shape Has No Definite Volume

Phases of Matter

Aim # 5: How can we explain phase changes in terms of energy? Temperature: Measure of average kinetic energy of the particles of a substance Heat : The flow of energy due to a temperature difference. Heat always flows from high temp to low temp Exothermic- heat is released Endothermic- heat is absorbed Kelvin Temperature: scale that is directly proportional to average KE (See Table T )

Melting change from SOLID to LIQUID Heat is absorbed -ENDOTHERMIC Molecules spread out Fusion -no temp change even though energy is added Average KE of particles remains the same Particles absorb heat as Potential Energy

FREEZING change from LIQUID to SOLID Heat is removed -EXOTHERMIC Molecules get closer Solidification no temp change, P.E. decreases

EVAPORATION LIQUID to GAS Heat is absorbed Molecules spread out Vaporization No change in temp gain P.E.

CONDENSATION GAS to LIQUID Heat is removed Molecules get closer

SUBLIMATION/ DEPOSITION Sublimation: SOLID to GAS Molecules spread out Deposition: GAS to SOLID Molecules get closer

Heating and Cooling Curves Graph of temperature vs. time Showing the phase changes of a substance Time increases but temperature stays constant represent phase changes with no slope Places with a slope indicate temperature changes

What caused the water to change phases during this experiment? What is happening at the two plateaus on the graph?   Why doesn’t the temperature change at these spots? The melting point of water occurs at the same temperature as the point of water. What other phase changes happen at the same temperature? Heating the water, increasing the temperature Phase change Kinetic energy doesn’t change Freezing Condensation and evaporation