Warm-up: 1. What is an element? 2. What is a compound?

1. Hydrogen 2. Helium 3. Lithium 4. Boron 5. Carbon 6. Nitrogen 7 1. Hydrogen 2. Helium 3. Lithium 4. Boron 5. Carbon 6. Nitrogen 7. Oxygen 8.Neon 9. Sodium 10. Aluminum 11. Silicon 12. Sulfur 13. Chlorine 14. Potassium 15. Calcium 16. Titanium 17. Iron 18. Nickel 19. Copper 20. Tin 21. Iodine 22. Tungsten 23. Gold 24. Mercury Lead Radon

Notes: Properties of Matter

Matter is anything that has mass and takes up space.

Matter is divided into TWO main categories for purposes of classification. All matter is either a PURE SUBSTANCE or a MIXTURE

Elements and Compounds are PURE SUBSTANCES

A mixture is when two or more substances are mixed together but not combined chemically

A mixture retains properties of all original ingredients.

MIXTURE OR PURE SUBSTANCE?

MIXTURE OR PURE SUBSTANCE? NaHCO3 - Sodium Bicarbonate

MIXTURE OR PURE SUBSTANCE? Soil

MIXTURE OR PURE SUBSTANCE? Milk

MIXTURE OR PURE SUBSTANCE? Sugar: C12H22O11

MIXTURE OR PURE SUBSTANCE? Air

MIXTURE OR PURE SUBSTANCE? Oxygen

Homogeneous Mixtures are the same throughout.

Warm-Up: 1. Is H2O a _____________. a. Element b. Compound c. Mixture d. All of the Above 2. Why is tap water considered a mixture?

Steel is a homogeneous mixture.

Heterogeneous Mixtures are not the same throughout.

Targets 9/10/14 Identify the following as pure substances or mixtures. Oxygen Milk Vegetable oil Coffee Aluminum Nitrogen Water Carbon dioxide

Density is a physical property

Density = Mass Volume Practice: A material has a mass of 100g and a volume of 10 cm3. Calculate the density.

Warm-Up. Density = Mass. Volume 1 Warm-Up Density = Mass Volume 1. A material has a mass of 500g and a volume of 10 cm3. Calculate the density. 2. A sample of water has a volume of 50mL and a mass of 50g. What is the density? 3. Which type of substance cant be separated into a simpler substance?

Matter Density Element Compound Pure substance Mixture Homogeneous Illustrated Dictionary On each square, complete the following: Write the word and provide a paraphrased definition.(left) Use the word in a complete sentence (left) Provide an illustration of the word on the right. Matter Density Element Compound Pure substance Mixture Homogeneous Heterogeneous

4 States of Matter: -Solid -Liquid -Gas -Plasma

In a gas, molecules are very far apart

In a liquid, molecules are closer together but still move around

In a solid, molecules vibrate in place and do not move around

Plasmas are gases that are so energized that some of their electrons have been stripped away

Gasses and liquids take the shape of their containers, solids do not.

Energy must be added to change a solid to a liquid;

More energy must be added to change a liquid to a gas

Warm-Up: 1. In which state of matter are the molecules moving the fastest? 2. In which state of matter are the molecules not moving around, just vibrating in place? 3. Matter in which two states takes the shape of its container? 4. To make matter change from a solid to a liquid, what must happen to the molecules?

WARM-UP: 1. Matter in which two states takes the shape of its container? 2. To make matter change from a solid to a liquid, what must happen to the molecules?

WARM-UP: 1. Which state of matter is the most dense. 2 WARM-UP: 1. Which state of matter is the most dense? 2. When a substance changes from a solid to a liquid what is this called? 3. When a substance changes from a liquid to a gas what is this called? 4. When a substance changes from a gas to a liquid, what is this called?

WARM-UP: 1. What is volume WARM-UP: 1. What is volume? Give two examples of two things that have different volumes. 2. What makes each element different from one another? 3. What is atomic number?

1. What are the types of pure substances. 2 1. What are the types of pure substances? 2. What are the types of mixtures? 3. What is density? Describe two things that have different densities. 4. What combination of substances retains the properties of its components?

5. Give an example of a homogeneous mixture. 6 5. Give an example of a homogeneous mixture. 6. Give an example of a heterogeneous mixture. 7. List the phases of matter in ascending order of density. 8. What must be done to change a gas to a liquid?

9. What is the phase change called when a solid changes directly to a gas? 10. Is density a physical or chemical property of matter? 11. Nitrogen boils at -196oC. Is this a physical or chemical property? 12. List these items in order of ascending density: -a bowling ball –a beach ball – a penny – a hot air balloon in the air

Physical Properties of matter describe the matter’s physical characteristics

Boiling/Melting Points H2O = 1000C (2120F) CO2 = -570C (-700F)

Density is a physical property

Density = Mass Volume Practice: A material has a mass of 100g and a volume of 10 cm3. Calculate the density.

Others include: -Thermal Conductivity

-Malleability (ability to be pounded into thin sheets)

-Ductility (ability to be drawn into a thin wire)

Chemical Properties describe how a substance reacts chemically with another substance

In a chemical reaction, you always get a new substance.

Law of Conservation of Matter/Mass: Matter can never be created or destroyed

Warm-Up: 1. Find the density of an object with a mass of 40g and a volume of 5 cubic cm. 2. Find the mass of a sample of a substance with a density of 5 g/ml and a volume of 2 ml 3. List three physical properties of H2O

Solutions: S o l u t i o n s - A homogeneous mixture composed of only one phase

Solutions: S o l v e n t - the most abundant substance in a solution. The solvent dissolves the solute. S o l u t e - the least abundant substance in a solution. The solute dissolves into the solvent. In a sugar water solution, water is the solvent & sugar is the solute. In steel (a solution which becomes a solid) iron is the solvent and carbon is the solute Air is a solution

Solutions Homogeneous mixture Mixed molecule by molecule Can occur between any state of matter. Solid in liquid- Kool-aid Liquid in liquid- antifreeze Gas in gas- air Solid in solid - brass Liquid in gas- water vapor

Concentration of Solution Shows level of solute in the solvent Can be Expressed in several ways Relative Concentrations Dilute – small amounts of solute compared to solvent Concentrated – large amounts of solute compared to solvent Levels of Concentration Unsaturated solution – is able to dissolve more solute Saturated solution – has dissolved the maximum amount of solute Supersaturated solution – has dissolved excess solute (at a higher temperature). Solid crystals generally form when this solution is cooled.

Percent Composition (by mass) We can consider percent by mass (or weight percent, as it is sometimes called) in two ways: The parts of solute per 100 parts of solution. The fraction of a solute in a solution multiplied by 100. We need two pieces of information to calculate the percent by mass of a solute in a solution: The mass of the solute in the solution. The mass of the solution. Use the following equation to calculate percent by mass: (Write the equation)

Rate of Dissolving

Factors Affecting How Fast a Solute Dissolves

Hotter = Dissolve Faster 1. Temperature If we heat particles they will move faster The solvent will carry the solute particles away faster Hotter = Dissolve Faster

2. Agitating Stirring or shaking a solution moves the solute particles around so that they are closer to the solvent. The solvent particles can then attract them easily and carry them away! Stir or Shake = Dissolve Faster

3. Crushing (More Surface Area) When a solute is broken into small pieces, the individual particles can get closer to solvent particles so they can be easily dissolved So smaller pieces= dissolves faster

Dissolving happens on the surface of particles When solute is broken up, there is more surface area where dissolving can occur broken up

More pressure = Dissolve Faster Pressure forces solute particles into the spaces between the solvent particles More pressure = Dissolve Faster gas

Warm-Up: 1. What does CO2 (dry ice) do at room temperature. 2 Warm-Up: 1. What does CO2 (dry ice) do at room temperature? 2. Name a physical property of charcoal. 3. Name a chemical property of charcoal.

Warm-Up: 1. What is the difference between a physical change and a chemical change? 2. What are some clues that a chemical change/reaction has taken place?

Warm-Up: 1. What is volume? 2. What is density?