Topic: Properties of Matter
Objective: will students identify the
properties of matter and recognize chemical
and physical properties using practical
examples?
Global context: scientific and technical
innovation
MATTER
• Matter: everything that occupies a space in the universe
• Every kind of matter is made of one or more elements
• What is an atom?
Atoms are the smallest particle of matter,
and of an element.
• What is an element?
An element is a substance consisting of
atoms which all have the same number of
protons.
• What is a molecule?
Two or more atoms chemically combined.
How can matter be classified?
• Matter is made up of basic “ingredients” known as
atoms.
• An atom is the smallest unit of an element that
maintains the properties of that element.
• Substances are classified as elements, compounds,
and mixtures.
Basic ingredients
of all “stuff”
Substances are
classified as:
Matter
Elements
Compounds
Mixtures
How can matter be classified?
• An atom is a building block of
matter
• An element is made of only one
kind of atom.
•A compound is made up of different kinds of atoms that are
chemically combined.
•A mixture contains a variety of elements and compounds
that are not chemically combined.
The Organization of Matter
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Pure Substances
•
Always have the same composition and
are formed by chemical processes.
• Either elements or compounds.
• Examples:
 Pure water (H2O), carbon dioxide (CO2), hydrogen
(H2), gold (Au)
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Element
•
A substance that cannot be broken down into other
substances by chemical methods.
• Examples:
 Iron (Fe), aluminum (Al), oxygen (O2), and
hydrogen (H2)
• All of the matter in the world around us contains
elements.
Compound
•
A substance composed of a given combination of
elements that can be broken down into those
elements by chemical methods.
• Examples:
 Water (H2O), carbon dioxide (CO2), table sugar
(C12H22O11)
• A compound always contains atoms of different
elements.
• A compound always has the same composition
(same combination of atoms).
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Mixtures
• A mixture is a combination of two or more
substances that are combined physically
but not chemically.
• Mixtures are not pure substances and do
not have definite properties.
• Substances within a mixture keep their
identities and individual properties.
• Mixtures can be separated by physical
changes, although some mixtures are
difficult to separate.
•Magnets, centrifuges, filters, and other materials
can be used to separate mixtures.
Mixtures
•
•
Have variable composition.
Examples
 Wood, wine, coffee, granite
• Can be separated into pure substances: elements
and/or compounds using physical processes.
Homogeneous Mixture
•
•
•
•
Same throughout.
Having visibly indistinguishable parts.
A solution.
Does not vary in composition from one region to
another.
Apple Juice
Cranberry Juice
Orange Juice
Homogeneous Mixture – Examples
•
•
•
Air around you
Brass
Table salt stirred into water
Heterogeneous Mixture
•
•
Having visibly distinguishable parts.
Contains regions that have different properties
from those of other regions.
Heterogeneous Mixture – Examples
•
•
Oil and vinegar dressing
Sand stirred into water
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•
Mixtures can be separated based on different physical properties of
the components.
Different Physical Property
Technique
Boiling point
Distillation
State of matter
(solid/liquid/gas)
Adherence to a surface
Chromatography
Volatility
Evaporation
Filtration
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Distillation of a Solution Consisting of Salt Dissolved in Water
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•
No chemical change occurs when salt water is
distilled.
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How can elements be classified?
• Elements are classified as metals, nonmetals, or metalloids.
• Metals: shiny, conduct
electricity, malleable, ductile
• Nonmetals: not shiny, do
not conduct electricity or
heat.
• Metalloids: have properties
of both
• Classifying elements helps scientists predict the properties of
elements.
• The periodic table is a tool used to classify and identify elements
that have similar properties.
How can compounds be classified?
• Compounds can be classified as acidic, basic, or neutral by
measuring pH.
• Pure water (Neutral) has a pH of 7
• Acids have a pH below 7.
• Blue litmus paper turns red in the presence of an acid.
• Bases have a pH above 7.
• Red litmus paper turns blue in the presence of a base.
How can compounds be classified?
• Compounds can be organic or inorganic.
•Organic compounds are those that contain only carbon,
oxygen and hydrogen.
•Organic compounds made by living things are called
biochemical molecules or bio-molecules.
•Carbohydrates, lipids, proteins, and nucleic acids
are bio-molecules
Topic: Solutions
Objective: will students be able to define solution and each type of
solution through the use of charts and practical examples?
Global context: scientific and technical innovation
Solution
• a mixture of two or more substances that is
homogeneous
Salt water is
considered a
• can be physically separated
solution. How
can it be
physically
• composed of solutes and solvents
separated?
the substance in the smallest
amount and the one that
dissolves in the solvent
Iced Tea Mix
(solute)
the substance in the larger
amount that dissolves the
solute
Iced Tea
(solution)
Water
(solvent)
• A solution is a homogeneous mixture of ions or molecules of two or
more substances.
• Two parts
• Solvent is the component that is in the largest quantity
• Solute is the component that is dissolved in the solvent.
• If one of the components of a solution is a liquid it is usually the
solvent.
• If the solvent is water then the solution is identified as an
aqueous solution.
Solutes Change Solvents
• The amount of solute in a solution determines how
much the physical properties of the solvent are
changed
• Examples:
Lowering the Freezing Point
The freezing point of a liquid solvent
decreases when a solute is dissolved in it.
Ex. Pure water freezes at 320F (00C), but when salt is
dissolved in it, the freezing point is lowered.
This is why people use salt to melt ice.
Raising the Boiling Point
The boiling point of a solution is higher
than the boiling point of the solvent.
Therefore, a solution can remain a liquid at
a higher temperature than its pure solvent.
Ex. The boiling point of pure water is 2120F (1000C),
but when salt is dissolved in it, the boiling
point is higher. This is why it takes salt water
longer to boil than fresh water.
Concentration
• the amount of solute dissolved in a solvent at a given
temperature
•described as dilute if it has
a low concentration of
solute
•described as saturated if it
has a high concentration of
solute
•described as supersaturated if
contains more solute
than normally possible
Solubility
• the amount of solute that dissolves in a
certain amount of a solvent at a given
temperature and pressure to produce a
saturated solution
What do we call things
that are not soluble?
• influenced by:
Temperature
Pressure
Solids increased temperature causes
them to be more soluble and vice versa
Solids increased pressure has no
effect on solubility
Gases increased temperature causes
them to be less soluble and vice versa
Gases increased pressure causes them
to be more soluble and vice versa
Ex. Iced Coffee
Ex. Soda, “The Bends”
HOMEWORK
We are working on a lab that will be developed on your kitchen, please
make sure you have a grown up to help you with the cooking
procedure.
Each student should bring:
• 2 plastic/ glasses
• 2 cups of sugar
• 1/2 cups of water
• 2 wood sticks
• 4 clothes peg/gripper
• food coloring
• essences or sweet flavors
• 1 old newspaper
• 1 small pot
• 1 plastic or wooden spoon
Topic: Properties of Matter
Objective: will students identify the
properties of matter and recognize chemical
and physical properties using practical
examples?
Global context: scientific and technical
innovation
PROPERTIES OF MATTER
Matter has different qualities that
characterize it.
We can distinguish two types of properties:
•Physical
•Chemical
PHYSICAL PROPERTIES
The physical properties are those that can be observed with our
senses, without changing the structure of matter, and are used to
identify, describe and classify matter. For example:
• Mass
• Weight
• Volume
• Porosity
• Color
• Shape
• State (solid, liquid or gas)
Mass
•A measure of how much
matter is in an object.
Weight
•A measure of the force of
gravity on an object.
Volume
•The amount of space that
matter occupies.
MATTER
• Matter: everything that occupies a space in the universe
• Every kind of matter is made of one or more elements
States of Matter
• There are different “states” of matter. States of
matter are also known as phases (a physical state
of matter). Elements and compounds can move
from one phase to another phase when special
physical forces are present.
• Solid
• Liquid
• Gas
The striking blue walls in this photo are actually the sheer ice walls of a massive glacier. The
glacier in the picture is in Argentina, and the bluish water in the foreground is Lake
Argentina. The photo represents an important concept in physical science. Can you guess
what it is?
• The photo represents water in three common states of
matter. States of matter are different phases in which any
given type of matter can exist. There are actually four wellknown states of matter: solid, liquid, gas, and plasma.
Plasma isn’t represented in the iceberg photo, but the other
three states of matter are. The iceberg itself consists of
water in the solid state, and the lake consists of water in the
liquid state.
• Q: Where is water in the gaseous state in the above photo?
• A: You can’t see the gaseous water, but it’s there. It exists as
water vapor in the air.
Solids
• A solid has its own
shape.
• A solid does not change
unless you cut, bend, or
break it.
• Solids have a define
volume defined shape
and have a defined mass.
• Particles are very close together
Liquids
• Liquids do not have their
own shape.
• Liquids take the shape of
their container.
• Liquids have an
undefined shape,
defined volume and
defined mass.
• Particles are not very close
Gases
• Gases have no defined size or
shape.
• Gases take the shape of its
container.
• A gas will fill all the space
inside a container.
• Gases have undefined shape,
undefined volume and
defined mass
Particles are far away
and move freely
CHEMICAL PROPERTIES
The chemical properties are those that tell us how matter change
when combined with other substances , for example:
• Conductivity
• Dissolved oxygen
• Hardness
• pH (Page 54-55 Science Works 1/1-14) (Page 56 1-10)
What does it mean for a solution to be acidic or
basic (alkaline)?
An acid is a substance that donates hydrogen ions.
A base is a substance that accepts hydrogen ions.
Acidity and alkalinity are measured with a logarithmic scale
called pH. Here is why: a strongly acidic solution can have one
hundred million million (100,000,000,000,000) times more
hydrogen ions than a strongly basic solution! The flip side, of
course, is that a strongly basic solution can have
100,000,000,000,000 times more hydroxide ions than a
strongly acidic solution.
Acids
from the Latin word acere  “sharp” or “sour”
taste sour (but you wouldn’t taste an acid to see)
change litmus paper red
corrosive to some metals (reacts to create hydrogen gas – H2)
a substance that can donate a hydrogen ion (H+) to another
substance
• create a hydrogen ion (H+) or hydronium ion (H3O+) when dissolved
in water
•
•
•
•
•
HCl
Hydrochloric
Acid
H 2O

H+
Hydrogen
ion
+
ClChloride
ion
Notice how
the hydrogen
ion is released
when the acid
is in water
Examples: hydrochloric acid, vinegar, lemon juice, rainwater
Bases (Alkalis)
taste bitter (but you wouldn’t taste a base to see)
feel slippery or soapy
change litmus paper blue
react with oils and grease
a substance that can accept a hydrogen ion (H+) from another
substance
• create a hydroxide ion (OH-) when dissolved in water
•
•
•
•
•
Notice how
the hydroxide
ion is released
when the base
is in water; this
ion can accept a
hydrogen ion
(H+)
NaOH
Sodium
Hydroxide
H 2O
 Na+ + OHSodium
ion
Hydroxide
ion
Examples: sodium hydroxide, Drano, Tums, baking soda
Neutralization Reaction
• occurs when acids and bases react with each
other to produce water and salt
• acids release a hydrogen ion (H+) and bases release a
hydroxide ion (OH-)  water (H2O)
• the negative ion from the acid joins with the positive
ion of a base  salt
HCl + NaOH  H2O + NaCl
Hydrochloric
Acid
(acid)
Sodium
Hydroxide
(base)
Water
Sodium
Chloride
(salt)
Both the salt and water are neutral substances; therefore, that
is why this is referred to as a neutralization reaction.
Acid, Base, or Neutralization?
Zn + 2H+ Zn2+ + H2
Acid – because H2 gas was given off
NH3 + H2O  NH4+ + OHBase – because OH- is present in the products
HClO + LiOH  LiClO + H2O
Neutralization – because of the salt and water in the products
Review:
1. Define state of matter.
2. Which states of matter are most common on Earth?
3. Make a table comparing and contrasting solids, liquids, and gases.
QUESTIONNAIRE
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
Define matter
Define atom
Define element
Define molecule
Name the subatomic particles
What makes one element different from other element?
What is the periodic table of elements?
Create a graphic organizer with the classification of
matter
Define pure substance, and give 5 examples
Define compound and give 5 examples
QUESTIONNAIRE
11.
12.
13.
14.
15.
16.
17.
18.
19.
20.
21.
Define mixture and give 5 examples
Define homogeneous mixture and give 5 examples
Define heterogeneous mixture and give 5 examples
How can elements be classified?
How can compounds be classified?
Define solution
How can a solution be classified based on its concentration?
Define diluted solution
Define concentrated solution
Define saturated solution
Define supersaturated solution