Matter and Change Monday Tuesday Wednesday Thursday Friday SEPTEMBER 1 2 3 4 5 NO SCHOOL Matter & Change Classifying Matter Textbook Activity Meet in B122 Physical and Chemical Properties and Changes Indiana Jones Lab Hw: pg 7 Hw: pg 4 8 9 10 11 12 Intensive and Extensive Properties Quiz Matter Hw: pg 10 States of Matter HW: pg 13 and Finish Study Guide (pg 14-16) Matter Review Study guide due for +5 points on the test Test Matter and Change Name: Period: Page1
Day 1: Textbook Pages 15-18, 388-390 Classification of Matter Matter is. Matter: Pure Substances: Mixtures: Elements Compounds Heterogeneous Mix. Homogeneous Mix. Summary Defn. Examples Separation Special Terms/ Examples Types of Mixtures Suspensions Colloid Solution Stay mixed as long as Looks like Examples Light will Page2
Separating Mixtures Method How does it work? What is it used to separate? Examples Magnetic Attraction Sieving Evaporation Filtration Decanting Centrifugation Distillation Chromatography Crystallization Final Thoughts: Page3
Homework: Classifying Matter Directions: Label the following as an element, compound, heterogeneous mixture, or homogeneous mixture. 1. Flat soda pop 2. Salad dressing 3. Sugar 4. Soil 5. Aluminum foil 6. Black coffee 7. Sugar water 8. Pure water 9. Paint 10. Milk 11. Iron 12. Pure Air 13. Spaghetti Sauce Match the following vocabulary words to the appropriate definition. 1. 2. 3. 4. 5. 6. 7. Page4
Day 2: Textbook Pages 13-15 Properties of Matter Property What is It? How is it measured? Earth vs. Moon: Compare mass and weight Write a single sentence explaining the difference between the two Physical Property Chemical Property What is it? What is it? Examples Examples Changes Physical Chemical What is it? What does it include? What is made? Examples Page5
4 Indicators of a chemical change Exothermic Endothermic Rock Cycle Physical Changes in Rock Cycle Chemical Changes in Rock Cycle Page6
Digestion Physical Changes in Digestion Chemical Changes in Digestion Homework: Physical and Chemical Properties and Changes Directions: Label the following as Physical Properties or Chemical Properties. 1. Red Color 2. Density 3. Flammability 4. Solubility 5. Will react with acid to form hydrogen 6. Supports Combustion 7. Bitter Taste 8. Melting Point 9. Will react with water to form a gas 10. Will react with a base to form water 11. Hardness 12. Boiling point 13. Can neutralize a base 14. Luster 15. Odor Directions: Label the following as Physical Changes or Chemical Changes. 16. Sodium Hydroxide dissolves in water 17. Hydrochloric acid reacts with sodium hydroxide to produce a salt, water, and heat. 18. A pellet of sodium is sliced in two 19. Water is heated and change to steam 20. Potassium chlorate decomposes to potassium chloride and oxygen gas 21. Iron rusts 22. Ice melts 23. Acid on limestone produces carbon dioxide gas 24. Milk Sours 25. Wood Rots Page7
Day 3: Textbook Pages 11, 42-43 Intensive and Extensive Properties Physical Properties Extensive Intensive length, volume, mass and weight density, freezing point, color, melting point, reactivity, luster, malleability, and conductivity. Circle if the following are Intensive or Extensive. The volume of coffee in a mug INTENSIVE EXTENSIVE % of sugar in a COKE INTENSIVE EXTENSIVE The number of calories of energy you derive from eating a banana INTENSIVE EXTENSIVE The number of calories of energy made available to your body INTENSIVE EXTENSIVE when you consume 10.0 g of sugar The mass of iron present in your blood INTENSIVE EXTENSIVE The mass of iron present in 5 ml of your blood INTENSIVE EXTENSIVE The electrical resistance of a piece of 22-gauge copper wire INTENSIVE EXTENSIVE The electrical resistance of a 1-km length of 22-gauge copper wire INTENSIVE EXTENSIVE Density (An Intensive Property) Density depends on: 1. 2. If the black dots are atoms, which box represents the substance with the greatest density? Page8
Useful Density Information Density of water = Objects with a density than 1 g/ml in water Objects with a density than 1 g/ml in water TEACHER DEMO ANALYSIS QUESTIONS: 1. When your teacher cut the piece of paper in half, what happened to the mass of the paper? 2. When your teacher cut the piece of paper in half, what happened to the volume of the paper? 3. If the original mass of the paper was 8.0 g and the original volume was 2.5 cm 3, what was the original density of the paper? (Show your work) 4. Assuming the information given above is correct, what would the NEW density be for just one half of the original piece of paper? (Show your work) 5. When your teacher doubled the amount of water in the beaker, what happened to its mass? 6. When your teacher doubled the amount of water in the beaker, what happened to its volume 7. If the original mass of the water was 150.0 g and the original volume was 150 ml, what was the original density of the water? (Show your work) 8. Assuming the information given above is correct, what would the NEW density be for double the original amount of water? (Show your work) Density is calculated with the formula: Density = or D = Guess Method Given- Unknown Equation Substitue Solve Page9
Let s Practice! 1. What is the density of a piece of wood that has a mass of 35.99 g and a volume of 45.68 cm 3? 2. A metal cylinder is placed into a graduated cylinder with 24.0 ml of water. After the cylinder is added, the volume of water rises to 30.4 ml. The density of the cylinder is known to be 8.9 g/ml. What is the mass of the cylinder? Homework Density 1. A sample of gas has a mass of 0.0707 grams and has a volume of 48.9 milliliters. What is the density of this gas? 2. A rock has a mass of 30.5 grams and, when placed in a beaker of water that has 20.0 ml in it, the volume increases to 22.9 ml. What is the density of the rock in grams per centimeter cubed? 3. Ammonium magnesium chromate has a density of 1.84 g/cm 3. What is the mass of 6.96 cm 3 of this substance? 4. Iron has a density of 7.87 g/cm 3. What volume would 12.5 grams of iron occupy? Page10
NOTES T1 Phases of Matter Kinetic Molecular Theory Atoms and molecules are constantly and we measure the energy of these movements as the of the substance. The more a substance has, the more molecular there will be, and the the perceived temperature will be. States of Matter - There are three states (also called phases) of matter. Phase Definite shape? Definite volume? Particle spacing Particle movement Draw how particles would appear Solid Liquid Gas Density Comparison If you consider the solid, liquid, and gas state of one particular substance, this rule holds true in most cases: Most dense Least dense Water is Weird Most dense Least dense Page11
Transitions between the 3 states of matter: Page12
Matter Homework 1. Which phase(s) of matter has(have) definite volume? 2. Which phase(s) of matter has(have) definite shape? 3. Which phase of matter is the most compressible? 4. Which phase of matter has the particles which move the least? 5. Rank the phases of matter in order of increasing attractive forces between their particles. Hint: If you have strong attractive forces, this means that the particles are very attracted to each other. If you are attracted to something or some-one, do you want to be close to them or far apart from them?,, Using the class Notes, complete the following table: Initial Phase Final Phase Name of Phase Change Endothermic or Exothermic? solid liquid solid gas gas solid liquid gas liquid gas gas liquid Page13
Matter and Change STUDY GUIDE Due Wednesday, Sept 10 th, for 5 pts on your test! 1. Which phase of matter has the greatest attractive forces? 2. Which phase of matter has the least attractive forces? 3. Which phase of matter has the fastest moving particles? 4. Rank the three phases in order of increasing distance between their particles. < < 5. Which phase changes are endothermic? 6. Which phase changes are exothermic? 7. Complete the chart below about the six possible phase changes. Initial Phase Final Phase Name of Phase Change Endothermic or Exothermic? Equation for Water Solid Liquid Ex: melting Endothermic H 2 O (s) H 2 O (l) Gas Gas Liquid Solid Liquid Liquid Solid Solid Gas Gas Page14
8. Classify each of the following as either physical or chemical properties by checking the appropriate box. Property Physical Chemical Blue color Density Flammability Solubility Reacts with acid to form H 2 Combustion Melting point Reacts with water to form a gas Reacts with a base to form water Hardness Boiling point Can neutralize an acid Luster Odor 9. Classify each of the following as either a physical (P) or chemical (C) change. a. Sodium hydroxide dissolves in water b. Chlorine and hydrogen react to produce hydrochloric acid. c. A pellet of sodium is sliced in two. d. Water vaporizes into steam. e. Iron rusts. f. Evaporation. g. Milk sours. h. Ice melting. i. Sugar dissolves in water. j. Wood rotting. k. Food digesting in the stomach. l. Water is absorbed by a paper towel. m. Pancakes cooking on a griddle. n. Sugar is ground into a powder. o. A mirror cracks. p. Phase changes are ALWAYS changes! 10. What are the four signs of a chemical change? a. b. c. d. Page15
11. Classify each of the following as homogeneous or heterogeneous mixtures. a. Blood b. Chocolate-chip ice cream c. Brass (a blend of copper and zinc) d. Motor oil e. Black coffee 12. Classify each of the following as pure substances or mixtures. a. Silver h. Candle wax b. Pine tree i. Fog c. Orange juice d. Oxygen j. Ink k. Egg e. Iced tea l. Ice f. Air g. Soda m. Gasoline n. Blood 13. Circle the extensive properties. Highlight the intensive properties. a. Melting point d. length b. Hardness e. freezing point c. Color f. hardness g. boiling point h. volume i. density 14. Calculate the density of an object with a mass of 45.0g and a volume of 25.0mL. 15. Calculate the volume of an object with a mass of 45.0g and a density of 1.5g/mL. 16. Calculate the mass of an object with a density of 2.0g/mL and a volume of 15.0mL. 17. In the lab, you gather the following data: Mass Volume #1 Volume #2 11.8g 50.0mL 70.0mL Calculate the density of this object. Page16