Properties of Matter

Essential QuestionsHow does the state of matter define its properties?What are the real-life examples of molecules, atoms & ions?How are atoms, molecules & ions alike and how are they different?How can matter be classified?What are the essential components of solutions?Why is water the universal solvent?In what ways can matter be quantified?What units should be used to quantify matter?What are the chemical & physical properties of pure substances?How can chemical and physical changes be determined in a laboratory setting?

The Breakdown of Matter

Matter

Anything with MASS & VOLUME

(solid, liquid, gas)

Pure Substanc

esMixtures

EQ: How can matter be classified?

MIXTURES

Mixtures = two or more substances PHYSICALLY combined.

Can be PHYSICALLY separated

Heterogeneous Mixtures

Hetero = different Geneous = origin or beginning has separations and/or boundaries can see to different parts Are ALL mixtures

Heterogeneous MixturesHeterogeneou

sMixtures

MixturesPhysically combined

substances

HomogeneousMixtures

Homeo = same Geneous = origin or beginning matter of the SAME make-up (no boundaries)

Homogeneous Mixtures

Homogeneous

Mixtures

SolutionsOthers alloys,

colloids, etc.

Homogeneous Mixtures

Homogeneous

Mixtures

Solutions

Solute Solvent

SolutionsEQ: What are the essential components

of solutions?

Homogeneous mixtures Physically NOT chemical

combined Solute = the substance BEING

dissolved Solvent = the substance DOING

the dissolving

Examples of Solutions Alloys = solid mixture or solution

(brass, 14K gold, steel) Air = gas mixture or solution Liquid solutions = sweet tea,

coffee, milk, tap water

EQ: Why is water the universal solvent?

Solution Properties

Soluble = the solute is able to dissolve in the solvent

Insoluble = the solute is NOT able to dissolve in the solvent

Descriptions of a Solution

Diluted Solutions = small amount of solute and/or a large amount of solvent

Concentrated Solutions = large amount of solute and/or a small amount of solvent

Saturated Solution = a solution that will NOT dissolve any more solute

An increase in temperature will allow more solute to dissolve in a solvent. The molecules of the solvent move faster and further apart allowing more room for more solute molecules.

3

21

Name three properties of solutions:

1. __________________________________

2. __________________________________

3. __________________________________

Name two types of mixtures & two types of pure substances.

1. ____________________________________

2. ____________________________________

What is the one key in distinguishing between homogeneous and heterogeneous mixtures

1. _____________________________________

Pure Substances

Pure Substance

s

ElementsCompoun

ds

Pure Substances

chemically pure substances only one part or one kind of

matter Elements = found on the

periodic table Compounds = 2 or more

elements that have combined CHEMICALLY EQ: How are atoms, molecules & ions alike

and how are they different?

Elements EQ: What are the real-life examples of

molecules, atoms & ions? 90 natural occurring elements found on the periodic table Atoms = smallest part of an

element represented by symbols

Compounds

2 or more elements that have combined CHEMICALLY

Molecules = smallest part of a compound

represented by formulas

Elements & Compounds

Pure Substance

s

Elements

Atoms

Symbols

Compounds

Molecules

Formulas

States of Matter Also called Phases of Matter Solids Liquids Vapors (gases)

Solids

Have a definite shape Have a definite volume Particles VIBRATE in place

Liquids

Have NO definite shape

Have definite volume particles SLIDE freely

Gases (vapor)

Have NO definite shape Have NO definite volume particles fill the volume of

the container

Solids, Liquids & Gases Solids = can form

crystals = solid where the particle are arranged into repeating patterns.

Liquids = physical property of Viscosity = “thickness” – the resistance to flow.

Gases = volume of gases depend greatly on pressure and temperature.EQ: How does the state of matter define its properties?

Phase Changes

Melting Freezing Vaporization Condensatio

n Sublimation physical

changes

Melting

the process of changing from a solid to a liquid

energy is being put into the substance

melting point = the temperature at which melting occurs – physical property

the melting point of water is 0ºC

Freezing

the process of changing from a liquid to a solid

energy is being pulled out of the substance

freezing point = same temperature as the melting point

(used mainly in weather)

Vaporization

the process of changing from a liquid to a gas

energy is being put into the substance

evaporation boiling

Evaporation

vaporization that occurs at the surface of the liquid

Boiling vaporization that occurs

throughout the liquid boiling point = the temperature

at which boiling occurs the boiling point of water is

100ºC

Condensation

the process of changing from a gas to a liquid

energy is being pulled out of the substance

Sublimation

the process of changing from a solid to a gas

energy is being put into the substance

ex: dry ice (CO2)

3

21

Name three phases of matter:

1. __________________________________

2. __________________________________

3. __________________________________

Name two types of vaporization.

1. ____________________________________

2. ____________________________________

What is the so different about sublimation?

1. _____________________________________

Properties of Matter

characteristics that can identify and describe matter.

Physical Properties Chemical Properties

EQ: What are the chemical & physical properties of pure

substances?

Physical Properties

observable properties physical change = changes that

occur while the substance remains the same.

ex: phase change

Examples of Physical Properties

density (d=m/v) color melting point & boiling

point hardness phase of matter malleable ductile taste conductivity luster texture solubility

Chemical Properties

properties that describes how the substance interacts with other substances or will act chemically

chemical change = an actual chemical reaction takes place and a NEW substance is formed

ex: combustion

Examples of Chemical Properties

flammability reactivity combustion oxidation reacts with _____ endothermic exothermic forms a

precipitate

Chemical ChangeEQ: How can chemical and physical changes be

determined in a laboratory setting?

Color change Temperature change = reaction is

either endothermic or exothermic Gas given off Precipitate formed = solid formed in

the reaction of two liquids

Energy (temperature) Changes in Reactions

Endothermic reactions– Energy is put into the

reaction– Reaction stops as soon

as energy is no longer put into the reaction

– Ex: cooking Exothermic reactions

– Energy is given off in the reactions

– Ex: burning

Exothermic Reactions

May require energy to be put into to the reaction in order to start or activate the reaction

Activation Energy = energy required to start an exothermic reaction

Reducing Activation Energy

Catalysts are often used to reduce the activation energy required to start an exothermic reaction

Chemical change vs. Physical change

ask the question, “Has a new substance been formed?”

“yes” = chemical change

“no” = physical change

Examples of Problems

ex: 2H2 + O2 2H2O hydrogen gas combines with

oxygen gas to form water a new substance is formed a chemical reaction occurs

EQ: How can chemical and physical changes be

determined in a laboratory setting?

Examples of Problems

: N2 + O2 + CO2 = air nitrogen gas combines with

oxygen gas and carbon dioxide gas and a few other gases mix

NO chemical reaction takes place physical change has taken place

in the gases

Examples of Problems

Ice melting Phases change Solid Liquid No new substance is

formed…it is still water Physical change

Malleable

A physical property that describes being able to be flatten or pounded onto sheets

This property is associated with metals.

Ductile

A physical property that describes being able to be drawn into a wire.

This property is associated with metals.

Luster

A physical property that describes how a substance reflects light

This property is often associated with minerals, gem stones, metals and nonmetals.

Oxidation

A chemical property describing a substance reaction with oxygen

slow oxidation = rusting, tarnish, corrosion

fast oxidation = burning, exploding, combustion

Density The amount of matter in a

given amount of space Density = mass ÷ volume D = m/v D = ?

Mass = m = 96.5 gramsVolume = v = 5 cm3

D = 96.5 g / 5 cm3 = 19.3 g/cm3

19.3 g/cm3 is the density of gold

The density of water = 1.0 g/mL

BUOYANCEThe ability of a fluid (liquid or gas) to exert an upward force on an object immersed in it.If buoyant force = object’s weightthe object will float

GAS LAWS

Boyle’s Law: pressure and volume

Volume decreases as Pressure increases

Pressure decreases as Volume increases

Gas Laws

Charles’s Law: temperature & volume

Volume increases as Temperature increases

Volume decreases as Temperature decreases