12/15/14

Morning ReviewPlease 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

• 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 substanceCompound = 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

• 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 substanceCompound = 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 heterogeneous8. What is the difference between a heterogeneous and homogeneous mixture?

Homogeneous = evenly mixed, can’t see partsEx: salt water

Heterogeneous = unevenly mixed, can pick out piecesEx: 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)

• 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 matter5. 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• Flammable• Breakable• Boiling point• Ability to dissolve• Ability to rust

Physical property

Physical property

Chemical property

Chemical property

Physical property

Physical property

Put the following properties under the correct description: (24 properties)

• Volume• Flammable• Can rust• Density• Malleability• Flexible• Floats• Mass• Magnetic• Boiling point

• Freezing point• Bouncy• Can tarnish• Corrosive• Melting point• State of matter• Color• Reactive• Soluble• pH

• Evaporates• Reacts w/ water• Conducts heat

• Conducts electricity

• Smell• Viscosity

Put the following properties under the correct description: (24 properties)

• Volume• Flammable• Can rust• Density• Malleability• Flexible• Floats• Mass• Magnetic• Boiling point

• Freezing point• Bouncy• Can tarnish• Corrosive• Melting point• State of matter• Color• Reactive• Soluble• pH

• Evaporates• Reacts w/ water• Conducts heat

• Conducts electricity

• Smell• Viscosity

2.2 Measuring Matter

1. Units for measurements2. Scientific tools used to determine measurements

MassVolumeDensityLengthTemperature

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 displacementDensity = g/mL or g/cm3

Length = meters, km, cm (ruler)Temperature = °C (thermometer)

2.2 Measuring Matter

3. Volume

CubeLiquidIrregular 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 formedEX: OCPGT

What are the 5 evidences of a CC?

• O C P G T• Osos Can Produce Grande Turds• Odor• Color Change• Precipitate• Gas Produced• Temperature Change

2.3 Changes in Matter

• 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

• 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 throughoutSolvent = the part of the solution that is present in the largest amount; dissolvesSolute = The part of the solution in the lesser amount; Gets dissolved

What’s a solvent & solute?

Water Sugar & lemonSOLVENT SOLUTE

Examples

• Water Salt• Air

Oxygen and other gases• Water Carbon

Dioxide

SOLVENT SOLUTE

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 solventConcentration of soluteTemperatureRate of stirringCatalyst

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 metalsEx: citrus, battery acid

Bases = range from 8-14; taste bitter; turn litmus paper blue; slippery feelEx: 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?