12/15/14
Morning Review
Please pull out study guide and a piece of
paper to take notes. We’ll start at 7:05. You
may grab a treat if you’d like one
Finals
• 100 ?’s scan tron
• 85 minutes to take test
Chemistry Review Concepts
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Matter
Measuring
Changes
States
Solutions
pH
2.1 Describing Matter
1. Classify matter in terms of elements,
compounds and mixtures
Element = a pure substance that cannot be
broken down into any other substance
Elements
2.1 Describing Matter
1. Classify matter in terms of elements,
compounds and mixtures
6. What are elements, and how do they relate to
compounds?
Element = a pure substance that cannot be broken
down into any other substance
Compound = a pure substance made of 2+ elements
chemically combined (can’t physically separate)
Mixtures = 2+ substances are combined physically
Element Check
• Are the following elements?
– Aluminum (Al)
– Copper (Cu)
– Oxygen (O2)
– Water (H2O)
REVIEW ELEMENT vs COMPOUNDS
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Nickel (Ni)
Silver (Ag)
Glass (SiO)
Neon (Ne)
Hydrogen (H2)
2.1 Describing Matter
1. Classify matter in terms of elements,
compounds and mixtures
7. What are the properties of a mixture?
Element = a pure substance that cannot be
broken down into any other substance
Compound = a pure substance made of 2+ elements
chemically combined (can’t physically separate)
Mixtures = 2+ substances are combined
physically
2.1 Describing Matter
2. Classify matter as being homogeneous or
heterogeneous
8. What is the difference between a heterogeneous
and homogeneous mixture?
Homogeneous = evenly mixed, can’t see parts
Ex: salt water
Heterogeneous = unevenly mixed, can pick out
pieces
Ex: Chex Mix
E, C or Mixture (He or Ho)
9. What is the difference between an element,
compound and mixture? Give examples:
• Copper (Cu)
• Water (H2O)
• Mixed Salad
• Salt (NaCl)
• Carbon (C )
• Air
• Kool aid
• Sugar
E, C or Mixture (He or Ho)
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Copper (Cu) - ELEMENT
Water (H2O) - COMPOUND
Mixed Salad - HETEROGENEOUS
Salt (NaCl) - COMPOUND
Carbon (C ) - ELEMENT
Air - HOMOGENEOUS
Kool aid - HOMOGENEOUS
Sugar - COMPOUND
2.1 Describing Matter
4. Determine physical and chemical properties of
matter
5. What kinds of properties are used to describe
matter
• PHYSICAL PROPERTY = Can change its
appearance physically
• CHEMICAL PROPERTY = Can change what it is
made up of (can change the atoms to make a new
thing); can react
WARM UP 8.14, answer if the
examples are physical or chemical
properties
Write the property and then write PP or CP
• Tear-able paper Physical property
• Flammable
Chemical property
• Breakable Physical property
• Boiling point Physical property
• Ability to dissolve Physical property
• Ability to rust Chemical property
Put the following properties under the
correct description: (24 properties)
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Volume
Flammable
Can rust
Density
Malleability
Flexible
Floats
Mass
Magnetic
Boiling point
Freezing point
Bouncy
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Can tarnish
• Conducts
electricity
Corrosive
• Smell
Melting point
State of matter • Viscosity
Color
Reactive
Soluble
pH
Evaporates
Reacts w/ water
Conducts heat
Put the following properties under the
correct description: (24 properties)
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Volume
Flammable
Can rust
Density
Malleability
Flexible
Floats
Mass
Magnetic
Boiling point
Freezing point
Bouncy
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Can tarnish
• Conducts
electricity
Corrosive
• Smell
Melting point
State of matter • Viscosity
Color
Reactive
Soluble
pH
Evaporates
Reacts w/ water
Conducts heat
2.2 Measuring Matter
1. Units for measurements
2. Scientific tools used to determine measurements
Mass
Volume
Density
Length
Temperature
2.2 Measuring Matter
• 1. Units for measurements
Mass = grams, mg, kg (scale or triple beam balance)
Volume = cm3 (LxWxH); mL (beaker, graduated
cylinder); cm3 water displacement
Density = g/mL or g/cm3
Length = meters, km, cm (ruler)
Temperature = °C (thermometer)
2.2 Measuring Matter
3. Volume
Cube
Liquid
Irregular shape
2.2 Measuring Matter
4. Density
Density = amount of matter per space occupied
D = M/V
Density
1. Mass of an object is 400 g and the volume is
100 mL, what is the density?
2. Mass of the object is 400 g and the density is
10 g/mL, what is the volume?
3. Volume of the object is 10 cm3 and the
density is 10 g/cm3, what is the mass?
2.3 Changes in Matter
1. & 2. What is a PC & CC?
PHYSICAL CHANGE = an actual change to an object
that does not change the chemical make up
(arrangement of atoms)
EX: state of matter change
size change
shape change
CHEMICAL CHANGE = a new substance has formed
EX: OCPGT
What are the 5 evidences of a CC?
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OCPGT
Osos Can Produce Grande Turds
Odor
Color Change
Precipitate
Gas Produced
Temperature Change
2.3 Changes in Matter
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Cutting wood
Breaking glass
Burnt smell produced
Boiling water
The bag got hotter when mixed
Food coloring was added
A solid formed when the acid was mixed
2.3 Changes in Matter
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Cutting wood - PHYSICAL
Breaking glass - PHYSICAL
Burnt smell produced - CHEMICAL
Boiling water - PHYSICAL
The bag got hotter when mixed - CHEMICAL
Food coloring was added - PHYSICAL
A solid formed when the acid was mixed - CHEMICAL
3.2 Changes of State
3.2 Changes of State
1. 2. 3. Substance during phase changes
3.2 Changes of State
4. Are changes in state a physical or chemical
property?
Does it change into a new substance?
Ice  liquid water  steam
7.1 Understanding Solutions
1. What are the two parts of a solution?
Solution = a well mixed mixture containing a solvent
and at least one solute that has the same properties
throughout
Solvent = the part of the solution that is present in
the largest amount; dissolves
Solute = The part of the solution in the lesser
amount; Gets dissolved
What’s a solvent & solute?
Water
SOLVENT
Sugar & lemon
SOLUTE
Examples
SOLVENT
• Water
• Air
• Water
SOLUTE
Salt
Oxygen and other gases
Carbon Dioxide
You SOLUTE the SOLVENT
7.2 Concentration and Solubility
1. Why is solubility useful in identifying substances?
Solubility = a measure of how much solute can dissolve in
a given solvent at a given temperature
So if I keep adding sugar to my kool aid mix, will it ever
get to a point where it stops dissolving?
Each substance has it’s own point where it reaches
maximum ability to dissolved and becomes saturated
7.2 Concentration and Solubility
2. What factors affect solubility?
Concentration of solvent
Concentration of solute
Temperature
Rate of stirring
Catalyst
7.3 & .4 Describing Acids and Bases
1. What are the properties of acids & bases?
Acids = range from 0-6; taste sour; turn litmus
paper red; react with certain metals
Ex: citrus, battery acid
Bases = range from 8-14; taste bitter; turn litmus
paper blue; slippery feel
Ex: Ammonia, bleach
7.3 Acids and Bases
2. & 3. & 4. What does the pH of a solution tell
you?
7.3 Acids and Bases
3. How are the strengths of acids and bases
determined?
Scales?
• pH
• Litmus paper
• Indicators (bromo blue, phenol red & cabbage
juice)
Questions?