1. What defines the matter around us?

2. LEQ: What forms does matter take?

4. ** **Solid: maintains a fixed volume and shape. Amorphous or crystalline. Not compressible. **Liquid: maintains a fixed volume but takes the shape of the container. Viscous flow **Gas: occupies the entire volume available, random motion. Flows with elastic collisions. Compressible **Plasma: occurs at high temperatures

7.  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

8.  LEQ: Why do we say that ALL things are made of matter?

9.  Physical Properties: examples: texture, shape, size, color, odor, volume, mass, weight, malleability, ductility, conductivity, temperature and density `Chemical Properties:  example: color change, energy given off or absorbed, gas given off, odor change, light, solid produced from solution

10. Physical Change: when objects undergo a change that does not change their chemical nature. Involves a change in physical properties. NO change in composition. Chemical Change: substances are changed into different substances. The composition of the substance changes.

11. 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

12.  Intensive Properties: Properties that do not depend on how much of the substance you have. Independent on amount.  Examples: Temperature, pressure, density, boiling point, solubility, color  Extensive Properties: Depend on the amount of the substance.  Examples: Mass and volume

13.  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

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

15. Element:  a pure chemical substance composed of atoms with the same number of protons  not easily broken down into it’s smaller parts  very distinctive properties  properties are different from the compounds they make up Gold Mercury Sodium Chlorine Gas

16. COMPOUND:  has a constant composition with fixed ratios of elements  physical properties such as boiling point or melting point of pure substances are invariant (unchanging).  Example: pure water boils at 100 °C Table salt: NaCl Pure Water: H 2 O Carbon Dioxide: CO 2

17. MIXTURE : a combination of two or more substances that are not chemically united do not exist in fixed proportions most natural substances are mixtures

18. MIXTURES  can be physically separated into pure compounds or elements.  just about everything that you can think of is probably a mixture.  may exhibit a changing set of physical properties. Concrete Sea Water Vegetable soup

19. Heterogeneous:  indicates difference  consists of visibly different substances or phases  the four phases are gas, liquid, solid, and plasma  Example: beach sand, vinegar and oil salad dressing, air with clouds Italian Salad Dressing Jello with Fruit Air with Clouds

20.  "Dancing Raisins" shows liquid, solid, and gas substances in a heterogeneous mixture. Vinegar + Baking Soda – forms a heterogeneous solution: there are liquids and gases present.

21. Homogeneous:  indicates sameness  has the same uniform appearance and composition throughout.  are commonly referred to as solutions.  Examples: corn oil, white vinegar, sugar solution, air (with no clouds) Kool-Aid Swimming Pool Water Air with no Clouds

22.  Are distinguished by particle size.  Homogeneous solutions have particles which are the size of atoms or molecules - too small to be seen.  Homogeneous solutions are two or more substances in a single phase.  The concentrations may be expressed using a variety of measures.

23.  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

24.  Density= Mass/Volume  Describes the degree of compactness of a substance – ( how closely packed together the atoms of an element, molecule or compound are.)

25. LEQ: How is matter expressed in chemistry?

26.  expression of the interaction between substances. To yield 2NaCl (aq) + H 2 SO 4 (aq)  Na 2 SO 4 (aq) + 2HCl (aq) Reactants Products Subscripts: # of atoms in the compound SubscCoeffiecents: the # of compounds or molecules present. Called ‘a Mole’ Physical States: (aq) dissolved in water, aqueous, (s) solid, (l) liquid, and (g) gas

27.  The number of compounds or molecule present  This is the coefficient or ‘the Mole’  The number of each atom in the compound.  This is the subscripts  Physical state (solubility rules)  Examples:  How many copper atoms in Cu 2 SO 4 ? 22  How many copper atoms in 3Cu 2 SO 4 ? 66

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

29.  Fundamental principle that states that matter cannot be created or destroyed.  In a chemical reaction the sum of all the masses of the substances involved in the reaction (reactants) is equal to the sum of all of the masses of the substances produced by the reaction (products).  No matter is gained or lost.

30. 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 8.41g. What mass of the iron (II) sulfate has been formed in the reaction?

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

32. 1. 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

33. 2. 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 calcium chloride in the test tube has a mass of 10.27 g. What is the total mass of ammonium and water vapor produced in the reaction? The reaction is: Ca(OH) 2 + 2NH 4 Cl  2NH 3 + 2H 2 O + CaCl 2 NOTE: The number of Moles of each species!!!!

34. 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. Cu + S  CuS.

35.  The mass of the part (in grams) divided by the mass of the whole (in grams) times 100. % mass = mass of part / mass of whole X 100  Example: Hot Chocolate with Marsh Mellows mass of marsh mellows: 2.5 grams mass of hot chocolate with marsh mellows: 105.26 grams   % Mass of Marsh mellow:  (2.5 g / 105.26 g) X (100)  = 2.38 %

36.  Compounds are formed in exact proportion to the mass of the compound.  Law of Definite Proportions = % Mass

37.  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. Given the mass of one molecule of H 2 O is 18g. Given the mass of one mole hydrogen is 1.00797g Given the mass of one mole of oxygen is 15.9994 g Then one mole of H 2 O is: 2(1.00797g) / 18g = 11.19 g 15.9994g / 18g = 88.81g 100g

38. 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

39. 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?

40.  When the same elements are involved in the formation of more than one compound, each MUST combined in the relationship of a small whole number. Cpd 1: Mass X / Mass Y = Mass 1 Cpd 2: Mass Y / Mass X = Mass 2 Mass 1 / Mass 2 = Whole # Then the combination of elements X and Y can form more than compound.

41.  It is believed that phosphorous and chlorine combine to form two different compounds. In one compound, 3.88 g of P combines with 13.28 g Cl. In the other compound, 1.32 g P combines with 7.56 g Cl. Use the law of Multiple Proportion to support the formation of these two compounds.

42. 1. Elements: simplest form of matter represented in symbols. 2. Symbols: a. First letter of the name b. First two letters of the name c. Places and names d. Latin and Greek

43. 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

44. 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