Matter and Change

Chapter 3

TN Ch 2.1, 2.3 Date

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EQ:

NOTES:

Write out the notes from my website.

Use different types of note-taking

methods to help you recall info (different

color pens/highlighters, bullets, etc)

When I lecture we will add more info, so

leave spaces in your notes

Summary Questions:

2-3 sentences… What did you learn

today from the notes?

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NOTES

Right Side – NOTES ONLY

Reflect

Question:

Reflect on

the

material by

asking a

question

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suppose to

be

answered

from

notes)

TN Ch 2.1, 2.3

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DRAW ANY PICTURES, FIGURES,

AND WRITE OUT ANY PRACTICE

PROBLEMS/QUESTIONS.

WE WILL ANSWER THEM TOGETHER.

LEAVE SPACES SO WE CAN ANSWER

QUES.

LEFT Side – PICTURES, PRACTICE PROBLEMS, ETC

TN CH 3.1-3.2Topic: Matter

EQ: What is Matter and what is not Matter?

READ Ch 3.1-3.2 (pg. 55-56) first then take notes

TN Ch 3.1 & 3.2: Chemistry & Matter Relevance of Matter to us

• Almost everything is made of matter – you, me, the chair you sit on, the air you breathe, the food you eat, clothes you wear, your technology, etc….

• The physical universe basically contains only 2 things: MATTER & ENERGY!

• We begin our study of chemistry by defining and classifying these 2 building blocks of the universe.

TN Ch 3.1 & 3.2: Chemistry & Matter

Chemistry is the study of matter and the changes that it undergoes.

- Central Science!!!

Matter is anything that has mass and takes up space.

Almost everything is MATTER…..so what isn’t matter?

• Matter is composed of atoms, submicroscopic particles that are the fundamental building blocks of matter.

• Atoms are bonded together to form molecules, two or more atoms joined to one another.

Can you think of things that are matter and things that are not matter?

Matter (15 lines down) Not Matter (15 lines down)

Left side

Summary:Let’s reflect….

What did you learn today from the notes? (2-3 sentences)

RIGHT side - THESE ARE AT THE VERY END OF NOTES

TN CH 3.3Topic: States of Matter

EQ: What are the 3 States of Matter and how are their

properties different from each other?

READ Ch 3.3 (pg. 57-58) first then take notes

States of Matter

• All matter that exists on Earth can be classified as one of these physical forms (s, l, g) called states of matter.

• States of matter – Physical property

Solids

• Examples: Wood, paper, iron, and sugar.

• The particles of a solid:

– Very tightly packed

– When heated, a solid expands

– Definite shape and volume – does not change to the shape of the container

– Incompressible - cannot be pressed into a smaller volume.

Draw with

notes

2 Types of Solids• Crystalline solid: Atoms or

molecules arranged in well-

ordered geometric patterns with

long-range, repeating order.

o Examples include salt and

diamond.

• Amorphous solid: Atoms or

molecules do not have long-range

order.

o Examples include glass,

rubber, and plastic.

Draw with

notes

• Which type of solid would it be?

Liquids

• Examples: Water, blood, soda, and mercury

• The particles in a liquid:

– Not held in place

– Less closely packed than solids

– Able to move past each other = FLOWS

– Takes the shape of the container

– The volume is constant no matter what container it is in

– Liquids are incompressible

Draw with

notes

Gases

• Example: Neon, methane, carbon dioxide, and air

• flows to conform to the shape of its container

• fills the entire volume of its container

• Far apart

• Easily compressed – What does this mean??Draw with

notes

Gases are compressible.Since the atoms or molecules that compose gases are not in contact with one another, gases can be compressed.

Example – pushing on a balloon!! Bring gas particles closer together

Draw with

notes

Vapor vs. Gas• Gas and vapor are similar, but not the same

• Water is called a ______ when it is in the gaseous form?

• Carbon dioxide is called a _____ , not vapor.

• What’s the difference?

vapor

gas

A gas is something that is gaseous at room temperature while a vapor is something that was either a solid or liquid when at room temperature.

• Solid

• Liquid

• Gas

SHAPE

• definite shape

• of container

• indefinite shape

VOLUME

• definite volume

• definite volume

• indefinite volume

COMPRESSIBLE

• NO

• NO

• YES

Summary of States of Matter Chart

Solid, Liquid, or Gas?

What two phase changes are occurring at the same time?

Practice Problem #1

Identify each of thefollowing as aproperty of a solid, liquid,or gas. Some answers willinclude more that one state of matter.

Left side

Practice Problem #1

A. flows and takes the shape of a container

B. compressible

C. made of particles held in a specific arrangement

D. has definite volume

E. always occupies the entire space of its container

F. has a definite volume but flows

Left side

Summary:

Let’s reflect….

What did you learn today from the notes? (2-3 sentences)

RIGHT side - THESE ARE AT THE VERY END OF NOTES

TN CH 3.4

Topic: Classifying Matter

EQ: What is the difference between

elements, compounds, and mixtures?

READ Ch 3.4 (pg. 58-61) first then take notes

Classification of Matter

Left side

2 catergories of Matter:

1. Pure Substance:

2 types: Elements and Compounds (and molecules)

2. Mixtures:

2 types: Homogeneous or Heterogeneous

Pure Substance:Elements or Compounds

• Pure Substance - Matter that has a uniform and unchanging composition.

– 2 types: Elements and Compounds (and molecules)

element

compound

structural formula

chemical formula

space filling modelmolecular model

Elements (118 elements known)

• Also called “atoms”• Made of a single type of atom

Elements vs. Compounds

• An element cannot be ___________ down or _____________ into

simpler substances by chemical means.

• Elements are the _________ forms of matter that can exists.

Examples: _______, Helium, __________

• A compound is made up of ____ or ________ elements

______________ bonded together.

• Compounds can only be broken down into simpler substances by

____________ ____________.

Examples: _______, Sand, _______________

broken changed

simplest

MercuryGold

2 morechemically

chemical changes

Water NaCl (table salt)

Mixtures

• A mixture is composed of two or more different types of atoms or molecules combined in variable proportions.

onot chemically united, but simply mixed together.

o2 types: Homogeneous and Heterogeneous

Mixtures

Mixtures are a physical blend of two or more substances

mixed together.” Can be separated by _________ means.

Chicken Noodle Soup Whole Blood Salt Water

Homogeneous mixture (always called SOLUTIONS) –uniform composition.

Heterogeneous mixture – NOT uniform composition.

4 Separation methods: physically!! (distillation, filtration, crystalization, chromatography)

physical

Heterogeneous Mixtures

Don’t draw them – Just list names of pics

Homogeneous Mixtures

Don’t draw them – Just list name of pics

Practice Problem #1

Which of the following are homogeneous and

heterogeneous mixtures?

Gasoline

Tea

Italian salad dressing

White wine

Vinegar

Beach sand

Dirt

Left side

Practice Problem #2

Identify each of the following as an example of a homogeneous mixture or a heterogeneous mixture.

A. 70% isopropyl rubbing alcohol

B. Pile of rusty iron filings

C. Concrete

D. Saltwater

E. Vegetable Oil

F. Bread

Left side

Practice Problem #3: Make this chart

Pure Substances vs. Mixtures

Elements Compounds Homogeneous Mixture

Heterogeneous Mixture

Left side

Mixture - Homogeneous or Heterogeneous OR Pure Substance (Element or Compound)?

Will do these in class

Smog

This marble

Ocean Water Liquid hand soap

“Pure” water

“Pure” gold

Soil

Carbon

“Pure” ammonium

Chloride

RockApple Juice

Apple

Propane

GlassCleaner

Gasoline

“Pure” Copper

Will do these in class

1. 2 categories of Matter – Pure Substances (Element/Compounds) and Mixtures (Homo/Heter)

2. All elements are made of atoms

3. All compounds are made from elements (chemically boundin a fixed ratio)

4. All Mixtures are made from combinationsof elements and/or compounds (not chemically bound)

C12H22O11

NaHCO3

So, In conclusion….

Summary:

Let’s reflect….

What did you learn today from the notes? (2-3 sentences)

RIGHT side - THESE ARE AT THE VERY END OF NOTES

TN CH 3.5-3.6Topic: Physical vs. Chemical

Properties & Changes

EQ: What is the difference between

Physical & Chemical Properties and

Changes?READ Ch 3.5-3.6 (pg. 61-65) first then take notes

Ch 3.5:Physical & Chemical Properties

Observing properties of matter

• Every substance has its own physical and chemical properties.

• Chemical and physical properties depend on temperature and pressure.– At room temp. water is a liquid with a density of

1.00 g/mL

LEFT SIDE of Spiral NB – Physical

RIGHT SIDE of Spiral NB - Chemical

**The next 3 slides**

Physical Properties(Left side)

Chemical Properties(Right side)

Physical Properties (add to chart)• physical property – a characteristic that can be

observed or measured without changing the identity of the substance. Examples are….. (write these example words)

melting pointstate of matter

masscolor

Boiling pointdensity

odortaste

hardness

Chemical Properties (add to chart)• chemical property – a characteristic that can

be observed or measured with a change in the identity of the substanceExamples are….. (write these example words)

flammability

reacts with oxygen

reacts with an acid

rust

Ch 3.6 - Physical and Chemical Changes

*The next 9 slides of notes *

Physical Changes(Left side)

Chemical Changes(Right Side)

Ch 3.6 - Physical Changes(add to chart)

• In a physical change, matter changes its appearance but not its composition.

• When ice melts, it looks different but its composition is the same. Solid ice and liquid water are both composed of water molecules, so melting is a physical change.

Physical Changes (in chart)• physical change – a change in a substance that

does NOT involve a change in the identity of the substance. (write these example words & DRAW SOME PICS to represent these words)

cutting breaking

tearingdissolving

boiling

Physical changes (in chart)• More Examples:

bending

crushing spliting

Mash/grind crumpling

All phase changes are physical changes.

(Draw in chart also)

Chemical Changes (in chart)

• chemical change – a change in a substance that DOES involve a change in the identity of the substance. (write these example words & DRAW SOME PICS to represent these words)

color change

…four good indications of a chemical change.

(HINT: Homework & Test Question!!)

gas released (often with an

odor)

energy change (light,

heat, …)

precipitate formed

Chemical changes ( in chart)

• Examples: explode, rust, oxidize, corrode, tarnish, ferment, burn, rot, dissolving metal in acid, spoilage of food.

• Rusting is a chemical change.

(it turns from iron to iron oxide)

1) ________ is produced: (________)

2) ________ is produced: (_____________ bugs/_____________)

3) ______________ is produced:

(______________)

Indications of Chemical Reactions

lightning fireflies

matchesHeat

Light

Electricity

batteries

(HINT: Homework & Test Question!!)

Indications of Chemical Reactions4) ___________________ forms: (_______ ________)

5) gas/smoke/odor/bubbles produced:

(_____________ ______)

Two liquids chemically

react to form a solid.

soap scumPrecipitate (solid)

baking soda and vinegar

Physical and Chemical Changes

• So……..The difference between chemical and physical changes are

A physical change results in a different form of the same substance.

A chemical change results in a completely new substance.

Which of the following processes physical & chemical

changes?

Iron rusting

Reaction of sodium metal with water

Leaves changing color

Dissolving sugar in water

Filtration of a solid from a liquid

Conductivity of gold

Burning of gasoline

Practice Problem #1 Left side

Summary:

Let’s reflect….

What did you learn today from the notes? (2-3 sentences)

RIGHT side - THESE ARE AT THE VERY END OF NOTES

TN CH 3.7

Topic: 4 methods of Physically Separating

Mixtures and Law of Conservation of Matter

EQ: How do mixtures separate physically

and why is matter conserved?

READ Ch 3.7 (pg. 65-66) first then take notes

Video: All 4 Methods of Separation

Ch 3.7 Separating Mixtures (4 types)

• Mixtures are physically combined & separated using the difference in physical properties of the substances.

Filtration (Lab)

Separates heterogeneous

mixtures composed

of solids and liquids.

Separating

Mixtures

through

Physical

Changes by

Filtration

(Draw with

notes)

Video: Filtration

Distillation (draw with notes)• Distillation is a separation technique that is based on differences in

the boiling points.

Step 1: _________ the solution.

Step 2: ________________ the vapor as is escapes and collect it.

www.edumedia-sciences.com/a438_l2-distillation.html

Boil

Condense

Video: Distillation

Crystallization

• Crystallization is a separation technique that results in the formation of pure solid particles from a solution containing the dissolved substance.

• Rock candy, pop rocks, suckers

Video: Crystallization

Chromatography

• Chromatography separates the components of a mixture on the basis of how they travel or drawn across the surface of another material.

• The separation occurs because the various components of the ink spread through the paper at different rates.

Video: Chromatography

How Matter Changes: Chemical Reactions

• Matter undergoes a chemical change when it undergoes a chemical reaction.

• In a chemical reaction, the substances present before the chemical change are called reactants.

• The substances present after the change are called products.

Law of Conservation of Mass:

There Is No New Matter

• Matter is neither created nor destroyed in a

chemical reaction.

• The total mass involved in the reaction remained constant.

• The law of conservation of mass states that mass is neither created nor destroyed during a chemical reaction—it is rearranged. (Also called the “Law of Conservation of Matter”)

What's the relevance of Conservation of Matter to us?

• The conservation of matter is relevant to, for example, pollution. We often think that humans create pollution, but, actually, we are powerless to create anything. Matter cannot be created. So, pollution is simply misplaced matter-matter that has been put into places where it does not belong.

Verifying the Law of Conservation of Matter

• 1st step : Need to write chemical

equation of reactants & products

• 2nd step :Solve & Verify if the Law of Conservation is vaild.

Suppose that we burn 58g of

butane in a lighter. It will react

with 208g of oxygen to form

176g of carbon dioxide and 90g

of water.

Left side: Leave 5 lines of space to solve in class

Practice Problem #1

Practice Problem #2

2 H2O2 → 2 H2O + O2

If 72 grams of water and 64 grams of oxygen are produced, what mass of H2O2 decomposed?

Left side: Leave 5 lines of space to solve in class

Summary:

Let’s reflect….

What did you learn today from the notes? (2-3 sentences)

RIGHT side - THESE ARE AT THE VERY END OF NOTES

TN CH 3.8Topic: Matter vs Energy

EQ: What is the difference between matter

and energy?

READ Ch 3.8 (pg. 66-68) first and then take notes

Ch 3.8 Energy

• Energy is a major component of our

universe.

• Energy is the capacity to do work.

• Work is defined as a force acting on a

distance.

• The behavior of matter is driven by energy.

• Like matter, energy is conserved.

• The law of conservation of energy states that energy is neither created nor destroyed….The total amount of energy is constant.

• Energy can be changed and transferred from one object to another.

• Energy cannot be created out of nothing, and it does not vanish into nothing.

There are different forms of

energy. • The total energy of a sample of matter is the

sum of its kinetic energy, the energy of motion, and its potential energy, the energy of position (at rest).

There are different forms of

energy.

• Electrical energy: The energy from the flow of electrical charge.

• Thermal energy: The energy from random motions of atoms and molecules in matter.

• Chemical energy: energy associated with the particles from a chemical reaction.

There are different forms of

energy.

What's the relevance of Energy to us?

• Our society’s energy sources will not last forever because as we burn fossil fuels-our primary energy source-we convert chemical energy, stored in molecules, to kinetic and thermal energy. The kinetic and thermal energy is not readily available to be used again. Consequently, our energy sources are dwindling, and the conservation of energy implies that we will not be able simply create new energy-it must come form somewhere else. All of the chemical reactions that we use for energy are exothermic

Units of Energy

• The SI unit of energy is the Joule (J), named after the English scientist James Joule (1818–1889).

• A second unit of energy is the calorie (cal), the amount of energy required to raise the temperature of 1g of water by 1 oC.

• A calorie is a larger unit than a Joule.

• BE careful…… The nutritional or capital C Calorie (Cal), equivalent to 1000 little c calories (cal).

• kilowatt-hour (kWh) – this unit used mostly with electricity in homes/business.

Energy units and their conversion factors. Left side

Conversion Energy map:

calories(cal)

Calories(Cal)

Joules(J)

Kilowatt hour(kWh)

Left side

Practice Problem #1

• A candy bar contains 225 Cal of nutritional energy. How many joules does it contain?

Left side: Leave 5 lines of space to solve in class

Practice Problem #2

• The complete combustion of a wooden match produces 512 cal of heat. How many joules and kilojoules are produced.

Left side: Leave 5 lines of space to solve in class

How many kWh of energy are in a fast food

hamburger containing 560. Calories?

Practice Problem #3

Left side: Leave 5 lines of space to solve in class

Summary:

Let’s reflect….

What did you learn today from the notes? (2-3 sentences)

RIGHT side - THESE ARE AT THE VERY END OF NOTES

TN CH 3.9

Topic: Endothermic and Exothermic

EQ: How does energy flow in a chemical

reaction?

READ Ch 3.9 (pg. 69-70) first then take notes

Ch 3.9 Endothermic and

Exothermic Reactions• Systems that absorb energy from

their surroundings – endothermicreactions

–Example: cold pack.

• Systems that release energy to their surroundings – exothermic reactions

–Example: holding a cup of coffee.

• Energy Diagrams – show how the energy changes between the reactants and products.

Left side

Left side

Practice Problem #1

• Identify each change as exothermic or endothermic:

A. wood burning in a fire

B. ice melting

C. Water freezing into ice

D. Gas burning

Left side

Summary:

Let’s reflect….

What did you learn today from the notes? (2-3 sentences)

RIGHT side - THESE ARE AT THE VERY END OF NOTES

TN CH 3.10

Topic: Temperature Scales

EQ: What is the difference between

Celsius, Fahrenheit, and Kelvin scales?

READ Ch 3.10 (pg. 70-74) first then take notes

What's the relevance of Temperature to us?

• Humans are understandably interested in weather, and air temperature is a fundamental part of weather. We use body temperature as one measure of human health and global temperature as one measure of the planet’s health.

Temperature: Random Motion of

Molecules and Atoms

• The atoms and molecules that compose matter

are in constant random motion—they contain

thermal energy.

• The temperature of a substance is a measure

of its thermal energy.

• The hotter an object,

the greater the

random motion

of the atoms and the

higher its temperature.

We must be careful to not confuse

temperature with heat. Heat - is the transfer or exchange of

thermal energy caused by a

temperature difference.

• indicates that heat ALWAYS flows from HOT objects to COLDER objects.

We must be careful to not confuse

temperature with heat. Temperature - is a measure of how hot

or cold an object is.

• measured using a thermometer.

FIGURE 3.17 Comparison of the

Fahrenheit, Celsius, and Kelvin

temperature scales

Left side

a. 1001 K

b. 1001 °C

c. 1 K

d. –401 °C

e. –401 °F

Which of the following temperatures is not

possible?

Left side

3 Temperature scales:

• Fahrenheit (°F) scale, used mostly for weather (uses thermometer to measure heat in air).

• Celsius (°C) scale – uses thermometer

– water freezes at 0 °C

– boils at 100 °C.

– Room temperature is ~ 25 °C.

3 Temperature scales:

• The Kelvin (K) scale – no thermometer!!

– It’s a calculation to avoid negative temperatures.

• Absolute zero

• 0 K is the coldest temperature possible

• is the temperature at which molecular motion virtually stops.

Temperature Conversions:(Box these equations)

oF = 9/5 oC + 32oC = 5/9 (oF – 32)K = oC + 273Remember there are no negative values for Kelvin.

108

A pepperoni pizza is baked at 455°F. What temperature is needed on the Celsius scale?

Practice Problem #1

--References--Temperature Conversions:Units: Celsius, Fahrenheit and KelvinK = oC + 273

oF = 9/5 oC + 32oC = 5/9 (oF – 32)

Left side: Leave 5 lines of space to solve in class

109

On a cold winter day, the temperature is –15°C. What is that temperature in °F and

Kelvins?

Practice Problem #2

--References--Temperature Conversions:Units: Celsius, Fahrenheit and KelvinK = oC + 273

oF = 9/5 oC + 32oC = 5/9 (oF – 32)

Left side: Leave 5 lines of space to solve in class

Question: The “surface” temperature on the planet Neptune is 133K, whereas on the planet Venus it is 737K. Convert these temperatures to Fahrenheit.

--References--Temperature Conversions:Units: Celsius, Fahrenheit and KelvinK = oC + 273

oF = 9/5 oC + 32oC = 5/9 (oF – 32)

Practice Problem #3

Left side: Leave 5 lines of space to solve in class

Summary:

Let’s reflect….

What did you learn today from the notes? (2-3 sentences)

RIGHT side - THESE ARE AT THE VERY END OF NOTES

CH 3.11-3.12Topic: Specific Heat Capacity

EQ: How much heat can any substance

hold?

READ Ch 3.11-3.12 (pg. 74-76) first then take notes

What's the relevance of Heat Capacity to us?

• The heat capacity for water explains why it is cooler in coastal areas, which are near large bodies of high-heat-capacity water, than in inland areas, which are surrounded by low-heat-capacity land. It also explains why it takes longer to cool a refrigerator filled with liquids than an empty one.

Specific Heat Capacity

• Specific heat capacity - The quantity of heat (in J) required to change the temperature of a given amount of the substance by 1 °C (also in Kelvin).

– Has the symbol C

– units are J/g °C (also in Kelvin).

• What’s the point of Specific Heat Capacity?

• It can be thought of as how much heat energy is needed to warm the substance up.

• THINK: Ever noticed that it is easier to warm up a pan full of oil than it is to warm up one full of water.

Lists of specific heat capacity for

several substances.This table is useful when solving homework problems.

Write table left side)

• Water has the highest

specific heat capacity

on the list. Why??

• Make NOTE: The smallvalues show that not a lot of energy is needed to produce a temperature change, whereas the largevalues indicate a lot more energy is needed.

Left side

Energy and Heat Capacity

Calculations

• q = heat in joules.

• m = mass in grams.

• C = specific heat capacity in (J/g °C).

• T = temperature in Celsius.

• The symbol Δ means the change in, so ΔTmeans the change in temperature

ΔT = (T final – T initial).

The equation that relates these quantities is

Practice Problem #1

• If you hold gallium in your

hand, it melts from your

body heat.

• How much heat must 2.5 g

of gallium absorb from

your hand to raise its

temperature from 25.0 °C

to 29.9 °C?

• The specific heat capacity

of gallium is 0.372 J/g °C.

Left side: Leave 5 lines of space to solve in class

5.0 g of copper was heated from 20.C to 80.C.

How much heat was used melt Cu?

Practice Problem #2

Left side: Leave 5 lines of space to solve in class

Practice Problem #3

If a 3.1 g ring is heated using 10.0 J, it’s temp.

rises by 17.9C. Calculate the specific heat

capacity of the ring. Is the ring pure gold?

Left side: Leave 5 lines of space to solve in class

Summary:

Let’s reflect….

What did you learn today from the notes? (2-3 sentences)

RIGHT side - THESE ARE AT THE VERY END OF NOTES