Unit 2 - Stevens 2014
Unit 2: Classification and Properties of Matter
Vocabulary
Term
Matter
Substance
Compound
Element
Mixture
Homogeneous
mixture
Heterogeneous
mixture
Solution
Solute
Solvent
Definition
Example
Unit 2 - Stevens 2014
Suspension
Colloid
Physical Property
Physical Change
Chemical Property
Chemical Change
Law of Conversation
of mass
Water cycle
Carbon cycle
Polar
Cohesion
Unit 2 - Stevens 2014
Adhesion
Surface tension
Specific heat
Section 1: Classifying Matter
Key Ideas
1. How can matter be classified?
2. What is the difference between elements and compounds? Give examples.
3. What is the difference between substances and mixtures?
4. How can you determine what type of mixture something is?
5. How can mixtures and compounds be broken down?
6. What is the difference between heterogeneous and homogeneous mixtures?
7. Why is water called the universal solvent?
8. Why do substances dissolve?
Vocab
– Matter
- Compound - Solute
- Solution
-Solvent
– Substance
- Mixture
- Suspension
- Colloid
– Element
- Homogeneous Mixture
- Heterogeneous Mixture
What is matter?
• ________________________________________________________________________
– Examples:
• A brick has mass and takes up space
• A desk has mass and takes up space
• A pencil has mass and takes up space
• ____________________________________________________________
Can you think of anything that would not be considered matter? _________________________
______________________________________________________________________________
Unit 2 - Stevens 2014
How do we classify matter?
- ______________________________________________________________________
Two ‘types’ of Composition of Matter
1. _______________________________________________________
2. _______________________________________________________
Draw Chart.
2 types of Pure Substances
Elements
-
Compounds
-
-
-
-
-
Examples:
-
Examples:
-
How do I identify compounds and elements?
• Elements
– ____________________________________________________
– Has only one type of atom
– _____________________________________________________
• Compounds
– _____________________________________________________
– Often has names that end in “ide”
Unit 2 - Stevens 2014
–
Broken down only by a chemical reaction
• How would you break down water? ______________________________
______________________________________________________________________________
Mixtures:
• Two or more substances are ____________________, not chemically combined
• The substances in a mixture retain (keep) the identities that they originally had.
• _________________________________________________________________
• You determine what type of mixture something is by ______________________
2 Main Types of Mixtures
Heterogeneous Mixture
• _______________________________
• Does not appear the same throughout,
uneven distribution of components
• __________________________________
_____________________________________
_____________________________________
Suspension
• A type of heterogeneous mixture
• _______________________
• _______________________
__________________________
__________________________
• EX: lemonade or orange juice with
pulp, pond water
Homogeneous mixture or solution
• _________________________________
• A mixture of two or more substances that
appears the same (uniform) throughout
• _________________________________
• _________________________________
• Can be solid, liquid, or gas
• Examples: salt water, blood, __________
_________________________________!
Colloid
• A type of homogeneous solution
• _________________________________
• Tyndall effect - particles scatter light (looks
cloudy)
• __________________________________
• EX: milk, fog, gelatin, paint,
Solute: the substance in the smallest amount and the one that dissolves in the solvent
Solvent:______________________________________________________________________________
Salt water is considered a solution. How can it be physically separated? _________________________
____________________________________________________________________________________
Solutes change solvents.
• The amount of solute in a solution determines how much the physical properties of the solvent
are changed
• Examples:
•
__________________________________________________________
•
___________________________________________________________
Unit 2 - Stevens 2014
Concentration
• the amount of solute dissolved in a solvent at a given temperature
• described as _________________if it has a low concentration of solute
• described as __________________if it has a high concentration of solute
• described as _____________________if contains more dissolved solute than normally possible
The Universal Solvent
• ______________________________________________________________________________
______________________________________________________________________________
• No one substance can dissolve all substances
• In general, “like dissolves like”
– _____________________________________________________________________
– Non-polar dissolves non-polar
– ______________________________________________________________________
• We will learn more about water’s special properties later.
How can I separate mixtures?
Let’s Recap: Matter
Draw chart.
Practice:
What are two types of Pure Substances?
1. Element
Definition:
2.Compound
Definition:
Unit 2 - Stevens 2014
Example:
Example:
3. Can an element or compound be separated by physical means?
What are two types of Mixtures?
4. Heterogeneous
Definition:
5. Homogeneous/Solution
Definition:
Example:
Example:
6. What kind of mixture is a solution? ______________________________________________________
7. What kind of mixture is a suspension and give an example. ___________________________________
_____________________________________________________________________________________
8. What kind of mixture is a colloid and give an example. ______________________________________
_____________________________________________________________________________________
9. Can mixtures be separated by physical means? What are some physical means of separation? ______
_____________________________________________________________________________________
_____________________________________________________________________________________
10. What is a solvent? __________________________________________________________________
11. What is a solute? ___________________________________________________________________
12. What is the universal solvent? _________________________________________________________
Section 2: Properties of Matter
Key Ideas
1. Why are color, volume, and density classified as physical properties?
2. Why are flammability and reactivity classified as chemical properties?
3. When water evaporates, is that a physical change of chemical change? Why?
4. What is the law of conservation of mass?
Vocab
– Physical property
- physical change
– Chemical property
- chemical change
– Law of conservation of mass
- reactivity
Physical Properties of Matter
• any property of matter that can be observed or measured without changing the identity of the
matter
Unit 2 - Stevens 2014
•
Examples:
•
•
•
•
•
•
•
•
•
Chemical Properties of Matter
• any property of matter that describes a substance based on _____________________________
______________________________________________________________________________
• Examples
•
•
•
•
flammability
reactivity with vinegar
reactivity with oxygen
Equation: _______________________________________________________
Chemical or Physical Property?
1. Paper is white. _________________________
2. Boiling point of H2O is 100oC. ________________________________
3. Zinc reacts with hydrochloric acid and creates hydrogen gas. ___________________________
4. Nitrogen does not burn. _____________________________________
5. Sulfur smells like rotten eggs. ___________________________________
Comparing Physical and Chemical Properties
Substance/Matter
Physical Property
Helium
Wood
Baking Soda
Powdered Sugar
Rubbing alcohol
Red food coloring
Iron
Chemical Property
Physical Change
• ______________________________________________________________________________
• a change without a change in chemical composition
• a change that keeps the original substance
• Examples
•
•
•
tearing paper
cutting your hair
change in state (solid, liquid, gas)
Chemical Change
• a change in which a substance becomes another substance having different properties
• ___________________________________________________________________
Unit 2 - Stevens 2014
• Changes that usually cause heat, sound, light, odor, fizzing/foaming, color changes
***You usually need more than one of the above characteristics to be considered a chemical change!
• Examples
•
•
•
combining sulfuric acid and sugar
burning a piece of wood
soured milk
Chemical or Physical Change?
1. Bending a Paper Clip. ______________________________
2. Baking a cake. ________________________________________
3. The sublimation of carbon dioxide. ____________________________
4. Crushing an aluminum can. _________________________________
5. Vinegar and baking soda combining to create salt and water. ______________________
Review:
Physical and Chemical Properties
Physical Property (a characteristic of a material that
you can observe without changing the identity of the
substances that make up the material)
Chemical Property (characteristic of a
substance that indicates whether it can
undergo a certain chemical change)
Physical and Chemical Changes
Physical Change (no changes occur in the structure
of the atoms or molecules composing the matter.
The substance is still the same substance as it was
before the physical change occurred)
Rip/ tear/ cut
Change in state (from liquid,
gas or solid)
Chemical Change (rearrangement of bonds
between the atoms occurs. This results in
new substances with new properties).
Unit 2 - Stevens 2014
Color change
Boiling
Stretching / folding
Freezing
Mix
Melt
**Some indicators of a chemical change are
smell, burning, bubbles….but the only way to
be sure a chemical change has occurred is if a
new substance is formed.
Temperature and chemical changes (reactions)
• How does temperature affect chemical changes?
– Increasing the temperature will cause chemical changes to occur _________________.
– Decreasing the temperature will cause chemical changes to occur _________________.
Law of Conservation of Mass
• Matter: has mass, and takes up space
• Mass: amount of matter in an object
• Law of conservation of mass: _____________________________________________________
_____________________________________________________________________________
• ***Remember mass is not the same as weight, so weight may change depending on gravity, but
mass won’t.
Section 3 – Biogeochemical cycles and properties of water
Key ideas
• What is the water cycle?
• What properties of water make it so important to sustain life?
• What is the Carbon cycle?
Vocab
• Water cycle
- adhesion
• Carbon cycle
- surface tension
• Polar
- specific heat
• Cohesion
Biogeochemical Cycles
• The Earth contains fixed amounts of each stable chemical element
• These elements move among reservoirs in the solid earth, oceans, atmosphere and living
organisms as part of biogeochemical cycles (i.e., nitrogen, water, carbon, oxygen and
phosphorus), which are driven by energy from within the Earth and from the Sun.
Water Cycle
• Law of conservation of mass states that matter is not created or destroyed….so is there always
the same amount of water on the Earth? ________________________________________
• Is it always the same water? ___________________________________________________
Unit 2 - Stevens 2014
•
•
•
•
Is it always in the same form (solid, liquid, or gas)? __________________________________
How does it change forms? ____________________________________________________
Where does it travel to/ from? _________________________________________________
Water foldable.
Properties of Water
1. Polar: slight positive and negative charge – can dissolve substances
2. High specific heat: water resists changes in temperature, therefore water must absorb more
heat energy to increase temperature.
- Very important with cells because our cells release a lot of heat and water absorbs that heat
which allows us to regulate cell temperatures. Very important in oceans and ocean life.
3. Cohesion: ____________________________________________________________
- Makes water molecules stick together.
- Ex- beads on a car when it is washed
- Spider walking on top of the water (surface tension).
4. Adhesion: __________________________________________________________________
– ____________________________________________________________
– Ex- upward curve of the surface of the water-> graduated cylinder
– Ex- plants transport water up their roots to their leaves.
Carbon Cycle
1. What is carbon?
– _____________________________________________________________________
2. Why is it important?
– _______________________________________________________________________
– _______________________________________________________________________
3. Where do we get the carbon we use from?
– ________________________________________________________________________
4. Why should we care about the carbon cycle?
–
__________________________________________________________________