Part 1 Topic: Matter &

Changes

EQ: What is Matter and

how does it change?

Title:Chem Review 1

Date

Title and

Highlight

Topic:

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

• DRAW ANY PICTURES, FIGURES, AND

WRITE OUT ANY PRACTICE

PROBLEMS/QUESTIONS.

• WE WILL ANSWER THEM TOGETHER.

So…LEAVE SPACES SO WE CAN

ANSWER QUES.

Summary (end of notes) :

1-2 Sentences of what you learned

Reflect

Question:

Reflect on

the

material by

asking a

question

(its not

suppose to

be

answered

from

notes)

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.

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.

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

Summary of States of Matter Chart

Solid, Liquid, or Gas?

Classification of Matter

Draw

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 model molecular 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

Mercury Gold

2 more chemically

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

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 bound in a fixed ratio)

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

C12H22O11

NaHCO3

So, In conclusion….

Part 2 Topic: Physical vs

Chemical

EQ: What is the

difference between a

property and a change?

Title:Chem Review 1

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

Make this chart

**The next 3 slides of notes put in the chart**

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….. (write example words)

melting point state of matter

mass color

Boiling point density

odor taste

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 example words)

flammability

reacts with oxygen

reacts with an acid

rust

Physical and Chemical Changes (Make chart – next 9 slides of

notes put in the chart) Physical Changes Chemical Changes

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. Examples are….. (write example words)

cutting breaking

tearing dissolving

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. Examples are….. (write example 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

matches Heat

Light

Electricity

batteries

(HINT: Homework & Test Question!!)

Indications of Chemical Reactions 4) ___________________ forms: (_______ ________)

5) gas/smoke/odor/bubbles produced:

(_____________ ______)

Two liquids chemically

react to form a solid.

soap scum Precipitate (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.

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)

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

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.

Part 3 Topic: Law of

Conservation Mass and

Energy

EQ: How can a reaction

not lose or gain

mass/energy during a

chem rxn?

Title:Chem Review 1

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”)

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.

Endothermic and Exothermic

Reactions • Systems that absorb energy from

their surroundings – endothermic reactions

–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.

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.

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