Properties of Matter

Essential Questions How 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 Substances Mixtures

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 Mixtures

Heterogeneous Mixtures Mixtures

Physically combined substances

   

Homogeneous Mixtures

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

Homogeneous Mixtures

Homogeneous Mixtures Solutions Others  alloys, colloids, etc.

Homogeneous Mixtures

Homogeneous Mixtures Solutions Solute Solvent

Solutions

EQ: 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 Name three properties of solutions

:

1. __________________________________ 2. __________________________________ 3. __________________________________ 2 Name two types of mixtures & two types of pure substances.

1. ____________________________________ 2. ____________________________________ 1 What is the one key in distinguishing between homogeneous and heterogeneous mixtures 1. _____________________________________

Pure Substances Pure Substances Elements Compounds

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 Substances Elements Compounds Atoms Molecules Symbols 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 Condensation 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 (CO 2 )

3 Name three phases of matter

:

1. __________________________________ 2. __________________________________ 3. __________________________________ 2 Name two types of vaporization.

1. ____________________________________ 2. ____________________________________ 1 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 Change

EQ: 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: 2H 2 + O 2  2H 2 O 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

    : N 2 + O 2 + CO 2 = 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

  

The amount of matter in a given amount of space

Density = mass ÷ volume D = m/v D = ?

Density

Mass = m = 96.5 grams Volume = v = 5 cm 3 D = 96.5 g / 5 cm 3

19.3 g/cm 3

=

19.3 g/cm 3

is the density of gold

The density of water = 1.0

g/mL

BUOYANCE

The ability of a fluid (liquid or gas) to exert an upward force on an object immersed in it.

If

buoyant force = object’s weight

the 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