Objectives:

1. I can classify matter into substances and mixtures.2. I can identify and distinguish between physical and

chemical properties. 3. I can identify and distinguish between the two types of

forces that affect the nature of molecules. 4. I can understand and distinguish between physical and

chemical changes. 5. I can identify techniques used to separate mixtures.

Daily Objective

• I can define matter. • I can identify and distinguish between the

classes of matter.

What is Matter?

What does all matter have in common?

What does all matter have in common?Atoms!

What is Matter?

• One or more atoms that take up space and has mass.

• Emphasized that all matter’s properties and changes are due to the chemical make-up and interactions on the atomic level.

Classification of Matter

What are some terms associated with the classification of matter?

Classification of MatterSubstance Mixture

Element Homogenous Mixture

Compound Heterogenous Mixture

Classification of MatterTerms: element, compound, mixture,

substance, homogenous mixture, and heterogenous mixture.

1. Define/illustrate each term above.

2. Use a graphic organizer to show how these terms are connected to matter and each other.

Infinite Campus Update

• Density Lab• Scientific Measurement Exam

Classification of MatterSubstance Mixture

Element Homogenous Mixture

Compound Heterogenous Mixture

Classification of Matter

Elements• Smallest type of matter that maintains it properties.• Each element represents a different atom (natural

or synthetic)A symbol is used to represent each element.

Elements

Compound• Chemical Combination of substances in a fixed

amount.

• Each compound has a unique chemical formula.Ex. Sodium chloride = NaCl

• The chemical combination of substances produces new properties.

Sodium (Na) + Chlorine (Cl) = Salt (NaCl)

Mixture

• Physically mixed together, so each matter’s properties are preserved.

• Use matter’s individual properties to physically separate from one another.

• Mixture’s composition can vary.

Heterogenous MixuresObserve multiple phases (parts) because the substances do not mix well.

Homogenous MixturesSubstances mix so well it looks like one phase.

Homongenous Mixtures• Also called solutions.

• Solutions:

-Solute: what is dissolved

-Solvent: what dissolves

Solubility= the ability of the solute to dissolve in the solvent.

.

NaCl + H2O

Classification of Matter

Exit Slip• Classify the following examples two ways:

a. Substance or Mixture?

b. Element, Compound, Heterogenous mixture or Homogenous mixture?

1. gasoline at the pump

(C8H18 + other hydrocarbons)

2. glucose (C12H22O11)

3. aluminum foil

4. sand

Classifying Matter:Substances vs. Mixtures

Substances•Definite chemical make-up•Elements or compounds•Ex. Silicon chip or H2O

Mixtures•Varied chemical make-up• 2 or more substances physically combined•Homo or Hetero Mixtures• Pizza and salt water

Classifying Matter:Substances vs. Mixtures

Element•Pure and simplest substance•One type of atom•Periodic table•Symbol, (He= Helium)

Homogenous Mixture•2 or more substances physically combined.•Substances are very soluble in one another-mix well – one phase•Substances in mix properties are preserved•Separated by physical processes.•Also called a solution•Ex. salt water, kool-aid

Compound• 2 or more substances chemically combined•Definite composition•Break-down only thru chemical processes•Substances making up cmpd gain new properties.•Chemical Formula, H2OEx. iron rust

Heterogenous Mixture•2 or more substances physically combined.•Substances are not soluble in one another-do not mix well-multiple phases•Substances in mixture properties are preserved.•Separated by physical processes•Ex. Oil and water, pizza, soil

Classification of Matter

Exit Slip• Classify the following examples two ways:

a. Substance or Mixture?

b. Element, Compound, Heterogenous mixture or Homogenous mixture?

1. gasoline at the pump

2. salt you garnish fries with

3. aluminum foil

4. sand

Infinite Campus Update

• Density Lab• Scientific Measurement Exam

Classifying Matter

• O2

Classifying Matter• represents an atom• physical combination of substances• multiple phases• one phase• chemical combination of substances• same composition from sample to sample• individual properties are preserved when substances

combine• varied composition from sample to sample• individual properties are lost and new properties are

gained when substances combine• chemical formula • solution• atom’s symbol• substances dissolve in one another.

SubstancesElement Compound

Substance

Mixtures

Homogenous Mix Heterogenous MixMixtures

Scientific Measurement Exam

Objectives:

1. I can classify matter into substances and mixtures.2. I can identify and distinguish between physical and

chemical properties. 3. I can identify and distinguish between the two types of

forces that affect the nature of molecules. 4. I can understand and distinguish between physical and

chemical changes. 5. I can identify techniques used to separate mixtures.

Infinite Campus Update

• Density Lab• Scientific Measurement Exam

Classification of Matter

Classification of Matter LabMatter’s Name

One or more phases(parts)

Abbreviation of matter(Symbol/Formula)

# of substance(s)

Element,Compound,Hetro Mix, Homo Mix

1 tap water

2 Deionized water

Classification of Matter Lab Questions

Matter’s Name

One or more phases(parts)

Abbreviation of matter(Symbol/Formula)

# of substance(s)

Element,Compound,Hetro Mix, Homo Mix

1

2

3

4

5

6.

Conclusion:Classification of Matter Lab

• What was most beneficial about this lab?

• What was most challenging about this lab?

• How has this lab helped you make important connections and distinctions between the classes of matter?

Classifying Matter Lab

• Students with peers observe various samples of matter and classify them as an element, compound, homo mixture, or hetero mixture.

Scientific Measurement Exam

Classifying Matter1. Classify each as either an element, compound,

homo mixture, or hetero mixture

a. soil

b. orange juice with no pulp

c. copper wire

d. car gasoline (C8H18)

2. What is the difference between a compound and a mixture?

Bell Ringer: Matter

• What is the difference between:

a. substances and mixtures

b. compounds and mixtures

2. Classify each of the following examples:

c. sugar

d. sugar water

e. gold ring

f. Iron rust (FeO)

g. Italian dressing

Classification of Matter

Classifying Matter Lab

• Students re-assess their classification of matter lab examples.

Classifying Matter Lab

• O2 = compound

Why?• Because the subscript number

represents atoms that are chemically bonded.

• In this example, two atoms of oxygen are chemically bonded together.

Chemical vs. Physical ChangeChemical Change:• Matter’s chemical make-up changes.• New matter is produced with new properties• Ex. Iron Rust (FeO)

Physical Change:• Matter’s chemical make-up stays the same.• Matter is the same, so most properties are the

same.• Ex. Lemonade

Intramolecular Forces

H2O compound

Forces within a compound that holds the atoms together. Also called chemical bonds.

Types of Chemical Changes• Combustion• Decaying• Digesting• Baking• Neutralization (acidic and basic chemicals)• Growing• Spoiled

Physical Changes • Physical process

• Substance(s) chemical make-up is preserved so no new substance is produced.

• Properties are preserved

Ex. Making Lemonade

Intermolecular Forces

Forces between compounds in a sample of matter. (group forces)

Types of Physical Changes

• Most states of matter • Breaks• Dissolves• Crushes• Cuts• Absorbs

Infinite Campus 9/10/12

• Classifying Matter Lab• Classification of Matter Quiz

What kind of forces are affected ?

.

Classification of Matter Quiz

Mixture Separation Lab• Students work in groups to determine what

physical processes they can use to separate out each substance in a given mixture.

• They will design and carry out their experiment to successfully separate out each substance in the mixture.

• Reiterate the concept that substances in a mixture maintain their physical properties because their chemical make-up is preserved.

Mixture Separation Lab (9/11)

Purpose: To design and carry-out an experiment that will separate substances from a mixture.

Mixture Separation Lab

Due: Today

Physical vs. Chemical Changes

What kind of forces are affected ?

.

What type of matter is a solution?

Homogenous Mixtures• Also called solutions.

• Solutions are composed of:

1. Solute: what is dissolved

2. Solvent: what dissolves the

solute

.

Physical Separation TechniquesSeparation Technique

HeterogenousMixture

HomogenousMixture

What physical properties are used?

Filtration

Extraction

Distillation

Chromotography

Physical Separation of Mixtures:Extraction

1. Extraction- separating substances from one another based on their unique physical properties.

2. Based on these examples what type of mixture is best separated using extraction?

Solubility allows us to separateoil from water.

What property did you useto separate iron filings from sand and salt.?

Physical Separation of Mixtures:Filtration

• Used to separate a solid from a liquid in the mixture.• What type of mixture would use filtration?• What physical properties are used during filtration?

Physical Separation of MixturesDistillation

• Separation of liquids or a solid and liquid in a mixture by their differences in boiling points.

• What type of mixture would use distillation?

• Ex. Ethanol (78 0C) and Water (1000C)

Chromotography• Separates homogenous mixtures based on solubility.

• Chromotography has two phases:

-Stationary Phase: solid

Mobile Phase: liquid or gas

• Substances in mixture will separatebased on their degree of solubility toward the mobile phase.

What type of mixture is best for chromotography?

Bell Ringer Identify as a chemical or physical change

a. moldy cheese

b. dew in the morning

c. leaves turning colors in the fall

d. sublimation of dry ice.

e. recycling aluminum

f. combustion of fossil fuels

Changes in Matter and Forces

.

Phase Changes

Mixture Separation Lab:

• Is considered incomplete until ALL sections of the lab report are filled out.

Matter and Energy

I can….• Establish a relationship between changes

in matter, the forces involved, and the flow of energy.

Phases of Matter

Phase Changes

Thermochemistry

• Study of energy changes when matter undergoes a physical or chemical change.

Bell Ringer1. Using your states of matter table what is the

relationship between the following: • intermolecular forces and kinetic energy?

2. Complete the table below using the states of matter table and phases of matter diagram

Changes in state of matter

Kinetic Energy:Absorbed or Released

Intermolecular Forces:Strengthened orWeakened

evaporation of water

condensationof alcohol

deposition of copper

melting of ice cream

Molecular Kinetic Theory:Establishes a relationship between energy flow, speed of particles, and intermolecular forces during physical changes.

Particles in Matter• The particles that make-up matter are in

constant motion.• The particles speed of motion depends upon?

Heat Energy Heat Energy (q) = • Energy that is transferred between matter of

different temperatures. • Unit for Energy: Joules (J) or calories (cal)

1 J = 0.2390 cal

• Energy does not have mass or volume, therefore it is NOT classified as matter.

• How does heat energy flow between objects?

Heat Energy Flow

Heat energy flowing between objects:• System:

The matter you are studying/measuring.• Surrounding :

The matter (environment) around the system.• Endothermic Process:

When heat is absorbed by the system.• Exothermic Process:

When heat is released by the system.

Heat Energy What does heat energy affect?

Heat Energy

Heat Energy• Heat energy affects the:

-speed of particles

-strength of the intermolecular forces

Heat Energy

Temperature Scales

Visionlearning.com

Temperature only measures the heat energy that alters the speed of particles.• Scientist prefer the Kelvin (K) and Celsius (oC)

scales

Temperature and Heat Energy

Heat Energy

OC

Conservation of Matter and Energy

Matter:Matter undergoes changes, but the atoms are conserved as a whole or as parts.

Energy:Energy is also conserved during changes that matter undergoes. If energy increases for a system, then its surroundings must decrease in energy by the same amount.

General Chemistry stops here.

Heat Capacity

Heat Capacity:

The amount of heat needed to raise the temperature of a substance 1.0 oC.

What does heat capacity depend upon?

Specific Heat CapacitySpecific Heat Capcity:

The amount of heat it takes to raise 1g of a substance 1 0C.

Specific Heat Capacity Problems:1. 6,000 cal (1 sig. fig)

2. 100,000 J (1 sig. fig)

3. 120,000 J (2 sig fig)

4. 8.0x102 J (2 sig figs)

5. 0.07 cal/goC (1 sig. fig)

6. 390J/kgoC (2 sig. figs)

7. 140J/kgK (2 sig figs)

8. 840 J/kgK (2 sig figs)

9. 1 g (1 sig fig)

10. 20 g (1 sig. fig)

Specific Heat Calculations

Specific Heat Capacity Problems:

Specific Heats of Common SubstancesSubstances Specific Heat

J/g* 0CSpecific HeatCal/g*0c

water 4.18 1.00

Grain alcohol 2.4 0.58

ice 2.1 0.50

steam 1.7 .40

aluminum 0.90 0.21

silver 0.24 0.057

mercury 0.14 0.033

Specific Heat Calculations

• The temperature of a 95.4 g piece of copper increases from 25.0oC to 48.0oC when the copper absorbs 849 Joules of heat. What is the specific heat of copper?

Specific Heat Calculations

• How much heat is required to raise the temperature of 250.0g of mercury to 52oC?

Conservation of Matter and Energy

Matter:Matter undergoes changes, but the atoms are conserved as a whole or as parts.

Energy:Energy is also conserved during changes that matter undergoes. If energy increases for a system, then its surroundings must decrease in energy by the same amount.

Physical Change: Energy Diagrams

catalog.flatworldknowledge.com

Enthalpy (H):The heat content of a system at constant pressure.

H: change in heat content before and after a change H = heat energy (q)

Physical Change: Energy Diagrams

catalog.flatworldknowledge.com

Exothermic:• heat content before change< heat content after change• heat energy (change in heat content) is negative, q-Endothermic: • heat content before change> heat content after change• heat energy (change in heat content) is positive, q+

Bell Ringer1. What is the difference between heat energy (q) and

specific heat energy (C)?

2. When 150.0 J of energy is absorbed by a 42.1 g sample of silver the temperature increases by 15.0oC. What is the specific heat of silver?

3. If an 8.8 gram sample of aluminum increases in temperature from 25oC to 55oC how much heat was absorbed by the aluminum sample?

Specific Heats of Common Substances

Substances Specific HeatJ/g* 0C

Specific HeatCal/g*0c

water 4.18 1.00

Grain alcohol 2.4 0.58

ice 2.1 0.50

steam 1.7 .40

aluminum 0.90 0.21

iron 0.46 0.11

silver 0.24 0.057

mercury 0.14 0.033

Infinite Campus Update:

• Mixture Separation Techniques Worksheet• Mixture Separation Lab• Matter and Change Review (optional)• Scientific Measurement and Matter Exam

Online Textbook Registration

• Due on Tuesday, September 21st for an extra point on last exam!

Ice Cream LabI can predict and apply the following during a

phase change:• The relationship between energy flow,

speed of particles, and strength of intermolecular forces .

• The difference between an exothermic and endothermic process.

Exit Slip

• Identify with evidence the energy process that occurred when making your ice cream?

• How did this energy process affect the speed of particles and strength of the intermolecular forces within the system.

• Why is adding salt to the ice important in making ice cream?

Infinite Campus Updated:

• Heating Curve Diagram Worksheet• Specific Heat Capacity Problems• Scientific Measurement and Matter Exam

Online Textbook Registration

• Due on Tuesday, September 21st for an extra point on last exam!

Bell Ringer: Assessment• What is your goal(s) for this class?

• What can you do to meet your goals?

• What can I do to help you reach your goals?

Ice Cream LabI can predict and apply the following during a

phase change:• The relationship between energy flow,

speed of particles, and strength of intermolecular forces .

• The difference between an exothermic and endothermic process.

Ice Cream Lab: Post Lab Qts.

• What was the system and what was the surroundings in this experiment?

• Which direction does heat always flow?

• Was this endothermic or exothermic process?

Ice Cream Post Lab Qts.

Ice Cream: Post Lab Qts.

H2O Sugar/Salt Solution

Ice Cream Lab: Post Questions

Exit Slip

• Identify with evidence the energy process that occurred when making your ice cream?

• How did this energy process affect the speed of particles and strength of the intermolecular forces within the system.

• Why is adding salt to the ice important in making ice cream?

Atomic Structure1. What is an atom composed of?

2. What subparticle(s) are responsible for an atom’s charge?

3. What subparticle(s) are responsible for an atom’s mass?

4. Illustrate an atom, identifying the subparticles and their location within the atom.