Matter and Change

Chapter 3

TN CH 3.1-3.2

Topic: Matter

EQ: What is Matter and what is not Matter?

READ Ch 3.1-3.2 (pg. 55-56)

Write Questions & Answer Questions #1-2 (notes

side) Highlight answer

TN Ch 3.1-3.2 Date

Title and

Highlight

Topic:

EQ:

Questions:

Write Question out and answer it (in

another color or HIghlight) based on

from what you read.

NOTES:

Now write out the notes from my

website. You may use different color

pens.

Number notes as you go.

Space out your notes so you can add

anything I say to them.

BUT NO HIGHLIGTING,

UNDERLINING, etc

WE WILL DO OUR FOCUS NOTES

TOGETHER

Right Side – NOTES ONLY

TN Ch 3.1-3.2

Title and

Highlight

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 & 3.2: 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.

(left side)Can you think of things that are matter

and things that are not matter?

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

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)

Write Questions & Answer Questions #3-8 (notes

side) Highlight answer

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.

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.

• 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

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??

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

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

(left side) Summary of States of Matter Chart

Solid, Liquid, or Gas?

What two phase changes are occurring at the same time?

Let’s Practice #1 (left side)

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

Let’s Practice #1(left side)

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

TN CH 3.4

Topic: Classifying Matter

EQ: What is the difference between

elements, compounds, and mixtures?

READ Ch 3.4 (pg. 58-61)

Write Questions & Answer Questions #9-13 (notes

side) Highlight answer

Classification of Matter(Draw on left side)

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

• Since ancient times, humans have tried to understand matter and harness it for their purposes. The earliest humans shaped matter into tools and used the transformations of matter-especially fire-to keep warm and to cook food. To manipulate matter, we must understand it. Fundamental to this understanding is the connection between the properties of matter and the molecules and atoms that compose it

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

Homogeneous Mixtures

Lets Practice #1 (Left Side)

Which of the following are homogeneous and

heterogeneous mixtures?

Gasoline

Tea

Italian salad dressing

White wine

Vinegar

Beach sand

Dirt

Practice Problem #2(Left side)

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

Practice Problem #3: Make this chart (left side)

Pure Substances vs. Mixtures

Elements Compounds Homogeneous Mixture

Heterogeneous Mixture

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

Classify the following: Element, Compound, Homo or

Heter Mixture?

Distilled water

Steel

Milk

Air

Sugar

Aspirin tablets

Smog

This marble

Ocean Water Liquid hand soap

“Pure” water

“Pure” gold

Soil

Carbon

“Pure” ammonium

Chloride

RockApple Juice

Apple

Classify the following: Element, Compound, Homo or Heter

Mixture?

Propane

GlassCleaner

Gasoline

“Pure” Copper

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….

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)

Write Questions & Answer Questions #14-15 (notes

side) Highlight answer

What's the relevance of Properties & Changes of Matter to us?

• The physical and chemical properties of mater make the world around us the way it is. For example, a physical property of water is its boiling point at sea level-100° C. The physical property of water of water-and all matter-are determined by the atoms and molecules that compose it. If water molecules were different-even slightly different-water would boil at a different temperature. Imagine a world where water boiled at room temperature.

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

Physical vs Chemical Properties

( Make this chart – RIGHT NOTES SIDE)

Physical Properties

Chemical Properties

Physical Properties (add to chart)

• physical property – a characteristic that can be observed or measured without changing the identity of the substance. Examples are…..

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 substance

flammability

reacts with oxygen

reacts with an acid

rust

Ch 3.6 - Physical and Chemical Changes (Make chart – Right side)

Physical Changes Chemical Changes

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

cutting breaking

tearingdissolving

boiling

Physical changes (in chart)• More Examples:

bending

crushing spliting

Mash/grind crumpling

All phase changes are physical changes.

(Draw left side)

Chemical Changes (in chart)

• chemical change – a change in a substance that DOES involve a change in the identity of the substance

color change

…four good indications of a chemical change.

(HINT: Homework 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 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

Let’s Practice

Which of the following processes physical & chemical

changes?

Boiling point

Color changes

Reaction with oxygen

Conductivity of gold

Burning of gasoline

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)

Write Questions & Answer Questions #16 (notes side)

Highlight answer

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 left

side)

Distillation (draw left side)• 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

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

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.

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.

Let’s Practice #1

(left side – leave space to solve

it in class)

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.

Let’s Practice #2 (left side – leave space to solve it in class)

2 H2O2 2 H2O + O2

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

TN CH 3.8

Topic: Matter vs Energy

EQ: What is the difference between matter

and energy?

READ Ch 3.8 (pg. 66-68)

Write Questions & Answer Questions #17-21 (notes

side) Highlight answer

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).

• 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.

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 chemicalreactions 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:

(left side)

calories(cal)

Calories(Cal)

Joules(J)

Kilowatt hour(kWh)

Let’s Practice #1(left side – leave space to solve it in class)

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

Let’s Practice #2(left side)

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

How many kJ of energy are in a fast food

hamburger containing 560. Calories?

Let’s Practice #3(left side – leave space to solve it in class)

TN CH 3.9

Topic: Endothermic and Exothermic

EQ: How does energy flow in a chemical

reaction?

READ Ch 3.9 (pg. 69-70)

Write Questions & Answer Questions #22-23 (notes

side) Highlight answer

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.

Draw left side

Draw left side

Let’s Practice #1(left side)

• Identify each change as exothermic or endothermic:

A. wood burning in a fire

B. ice melting

C. Water freezing into ice

D. Gas burning

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)

Write Questions & Answer Questions #24-26 (notes

side) Highlight answer

What's the relevance of Temperature to us?

• The temperature of matter and its measurement are relevant to many everyday phenomena. 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.

Ch 3.10 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.

Temperature - is a measure of how hot or cold an object is.

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

• measured using a thermometer.

FIGURE 3.17 Comparison of the

Fahrenheit, Celsius, and Kelvin

temperature scales

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.

98

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

Let’s Practice #1(left side – leave space to solve it in class)

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

oF = 9/5 oC + 32oC = 5/9 (oF – 32)

99

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

Kelvins?

Let’s Practice #2(left side – leave space to solve it in class)

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

oF = 9/5 oC + 32oC = 5/9 (oF – 32)

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)

Let’s Practice #3(left side – leave space to solve it in class)

CH 3.11-3.12

Topic: Specific Heat Capacity

EQ: How much heat can any substance

hold?

READ Ch 3.11-3.12 (pg. 74-76)

Write Questions & Answer Questions #27-30 (notes

side) Highlight answer

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.

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

Let’s Practice #1(left side – leave space to solve it in class)

• 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.

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

How much heat was used melt Cu?

Let’s Practice #2(left side – leave space to solve it in class)

Let’s practice #3(left side – leave space to solve it in class)

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?