1. What defines the matter around us? Unit Three: Matter and Change UEQ

2. LEQ: Why is it said that ALL things are made of matter?

3. Lecture Notes Chapter 3 Matter-Properties and Changes A. Properties of Matter: 1. Substance: matter with a uniform and unchanging composition. a. Physical property: characteristic of matter that can be observed or measures without change in composition. hard, soft, shiny, dull, flexible, density, brittle, malleability (to be shaped), ductility (to be drawn), conductivity (transfer of heat and energy), melting point and boiling point.

4. 2. Chemical property: interaction that result in the change in the composition of matter. Combines into one or more different substances. Indicators of a Chemical Change 1. heat production (energy change) 2. gas production (bubbles), odor 3. change in color 4. precipitation 5. reacts with or inability to react

5.  Silver tarnishes in the air.  Gold remains untarnished after 100 years under seawater.  Sliver hammered into the shape of a ring.  Barium boils at 725 o C.  Argon is an inert gas and will not react with other gases.  Lead is easier to bend than iron.  Potassium metal is spontaneous in water and oxygen.  Graphite and diamonds are both carbon but a diamond will not write.  Two clear liquids are mixed and an orange color is produced.  Digestion Questions: Identify each of the following as a physical or chemical property:

6. LEQ: What form does matter take?

7. **The form matter take under ordinary conditions.. States of Matter:

8. 1. Solid: Define shape and volume. Particles vibrate about a fixed point. NOT compressible. Particles packed in regular patterns (crystalline) or random (amorphous). 2. Liquid: Define volume with NO defined shape. Particle slid about each other. Incompressible. Particles are viscous (able to flow) Four states of matter:

9. 3. Gases: NO defined shape or volume. Particles are random and free flowing. Large spaces between particles. Collisions are elastic (no transfer or loss of energy). Very compressible. a. Vapor: Gaseous form of a substance that is a liquid or solid at room temperature. 4. Plasma: High-energy gas.

10.  Identify each of the following to its state of matter. 1. Random motion and fills the container. 2. Very compressible. 3. Amorphous 4. Defined volume but takes the shape of the container. 5. Defined volume and flows. 6. Defined shape and volume. 7. Not compressible. 8. Elastic collisions. 9. Viscous. 10. Crystalline Questions:

11.  Physical changes: NO change in composition of matter.  Chemical changes: Changes in the composition of matter. Changes in Matter:

12. LEQ: How is matter combined to form the world around us?

13. B. Mixture: a combination of two or more substances. 1.Heterogenous mixture: a mixture where the individual substances maintain the integrity of the substance. NOT uniform composition throughout. 2. Homogeneous mixture: a mixture where the substance are a uniformly composition. Mixtures of Matter

14.  An alloy (a solid solution of several metals and non-metals).  70% isopropyl alcohol  gasoline  bread  latex paint  beef stew  air  seawater  a pile of rusty iron filings  concrete Identify the following as heterogeneous or homogeneous:

15. 1. Compounds: Combination of two or more elements. 2. Elements: simplest form of matter represented in symbols. 3. Symbols: a. First letter of the name b. First two letters of the name c. Places and names d. Latin and Greek Compounds and Elements: Category of substances.

16. NOTE: You are responsible for the material in Chapter 3 that pertains to ‘Mixture of Matter’, Section 3-3 Homework : page95 #56-64 all Independent Study

17. LEQ: How is matter expressed in chemistry?

18.  expression of the interaction between substances. To yield 2NaCl (s) + H 2 SO 4(aq)  Na 2 SO 4 (l) + 2HCl (g) Reactants Products Coefficient: the # of compounds present. Subscript: the # of atoms present in the compound. Physical states: (s) solid; (l) liquid; (g) gas and (aq) aqueous dissolved in water Chemical Equation

19.  The number of compounds or molecule present  The number of each atom in the compound.  Physical state (solubility rules)  Examples:  How many copper atoms in Cu 2 SO 4 ? ans: 2  How many copper atoms in 3Cu 2 SO 4 ? ans: 6 What Does an Equation Tell Us

20. 1. How many oxygen in Fe(NO 3 ) 3 ? ans: 9 2. How many oxygen in 2Fe(NO 3 ) 3 ? ans: 18 3. What is the physical state of: MnCrO 4 (s) ? ans: (s), solid 4. How many sulfates are in 3Cu 2 SO 4 ? ans: 3 5. How many hydroxides are present in Mg(OH) 2 ? ans: 2

21. The amount of mass that occupies a defined volume. D = m/v Units: Triangle Graph: Density

22. % Mass is the total mass of the part divided by the total mass. If you are given three different colors of marbles with each marble having a mass of 5 g. You count 3 red, 7 green and 5 blue marbles. Then % by mass of red is: 3(5 g red) / (15 x 5 g total) x 100 = % by mass red % by Mass

23.  Sum of all the mass in the reactant MUST EQUAL the sum of the mass in the product. Mass reactant = Mass product Law of the Conservation of Mass:

24. A strip of iron with a mass of 15.72 g is placed in a solution containing 21.12 g of copper (II) sulfate. After the reaction, the iron strip has a mass of 8.33 g. The mass of the copper formed in 8.41. What mass of the iron (II) sulfate has been formed in the reaction? Questions:

25. Chemical reaction: Fe + CuSO 4  Cu + FeSO 4 Mass expression: Mass iron + Mass copper sulfate = Mass copper + Mass iron sulfate To find: Mass iron + Mass copper sulfate - Mass copper = Mass iron sulfate (15.72g – 8.33g) + 21.12 - 8.41 = 20.10 g

26. 1. Suppose 5 g of calcium hydroxide and 10 g of ammonium chloride are mixed in a test tube then heated until no more ammonia is given off. The remaining material in the test tube has a mass of 10.27 g. What is the total mass of ammonium and water vapor was produced in the reaction? The reaction is: Ca(OH) 2 + 2NH 4 Cl  2NH 3 + 2H 2 O + CaCl 2 Practice Problems:

27. 2. A reaction of 22.85g of sodium hydroxide with 20.82 g of hydrogen chloride gives off 10.29g of water. What mass of sodium chloride is formed in the reaction? The reaction is: NaOH + HCl  NaCl + H 2 O

28. 3. A sealed glass tube contains 2.25g of copper and 3.32g of sulfur. The mass of the tube and the contents is 18.48g. When the sealed glass tube is heated, a reaction between the copper and the sulfur forms copper (II) sulfide (CuS). All of the copper reacted and there is 1.14 g of sulfur remaining. Predict the mass of the sealed glass tube and its contents after the reaction.

29. A expression of the regular repeating properties to elements.  Dmitri Mendeleev: first table arranged by atomic mass.  Robert Mosley: arranged the periodic table according to the atomic number (the number of protons in the nucleus).  Periods: horizontal row  Groups or Family: vertical columns Periodic Table

30. Category of substances:  Chemical combination of two or more elements.  Specific arrangement of elements  Law of Definite Proportion: compounds are always composed of the same element in the same proportions by mass. H 2 ONaClC 6 H 12 O 6 2:1 1:1 6:12:6 Compounds

31. Elements are always combined in the same elements and in the same proportions. What is the proportional ratio of elements in: NaCl C 6 H 14 O 7 Ca(OH) 2 Law of Definite Proportions

32. By mass: 100 g of H 2 O will always be combined by mass with 11.19 g of hydrogen and 88.81 g of oxygen. 2(1.00797g) / 18g = 11.19 15.9994g / 18g = 88.81g Sampler

33. Percent by mass = mass of element/mass of compound x 100 % = part/whole x 100 Calculated by percent by mass:

34. 1. Given 25 g of a compound that is composed of 6.77 g of tin and 18.23 g of bromine. What is the percent be mass of each element in the compound? % by mass of Sn = mass of Sn/ mass of cpd X100 % = 6.77 g / 25g x 100 % = 27.1 % Sn % by mass of Br = mass of Br/ mass of cpd x 100 % = 18.23 g / 25 g x 100 % = 72.9 % Br

35. 1. A 134.5 g sample of aspirin is made up of 6.03 g of hydrogen, 80.70 g of carbon, and 47.77 g oxygen. What is the percent by mass of each element in aspirin? 2. A 2.89 g sample of sulfur reacts with 5.72 g of copper to form a black compound. What is the percentage composition of the compound? 3. Aluminum oxide has a composition of 52.9% aluminum and 47.1% oxygen by mass. If 16.4 g of aluminum reacts with oxygen to form aluminum oxide, what mass of oxygen reacts? Finish for HW along with 19-23 page 88 Examples:

36. Mass Compound = the sum of all the parts! What is the Mass of a Compound?

37. When the same elements combined in different ratio by mass, more than one compound is formed from those same elements. H 2 O v. H 2 O 2 Copper (I) chloride v. Copper (II) chloride Law of Multiple Proportions

38. You measure the mass of two compounds made-up of phosphorous and chlorine. Compound one contains 3.88g P to 13.28g Cl. Compound two contains 1.32g P to 7.56g Cl. Cpd 1: Cpd 2: Multiple Proportions Sampler

39. Two compounds. Compound one has 0.853g F to 1.47g Xe. Compound two has 0.624g F to 2.16g Xe. Are two compounds formed? Cpd 1 : Cpd 2: Complete #28-29 p 90, #67,72,74-76, 79-80, p95 Multiple Proportion Sampler