1. MATTER 1.2 TURN CHAPTER 1 OUTLINES IN TO THE BOX - NOW!

2. 1.Matter is anything that has mass and takes up space. Matter is identified and classified by its properties. There are two types of properties - physical properties and chemical properties.

3. a.Physical properties can be observed or measured without considering the chemical makeup of the sample of matter. For example, this piece of paper you are holding is white and the ink is black. There are two types of physical properties - extensive and intensive.

4. i.Extensive physical properties will change depending on the amount of the sample. Mass, length, and volume are examples of extensive physical properties.

5. ii.Intensive physical properties will never change, regardless of the amount of the sample. Density, luster, and conductivity are examples of intensive physical properties.

6. b.Chemical properties consider the internal chemical structure of the sample of matter. For example, this piece of paper is mostly cellulose, C 6 H 10 O 6, which is able to burn.

8. Classify each of the following as physical or chemical properties. If it is a physical property, then classify it as extensive or intensive. Area Boiling Point Color Concentration Corrosive Density Flammable Hardness Liquid Toxic Viscosity

9. 2.One physical property of matter is its phase. Although there are five phases of matter, three will be focused on: solid, liquid, gas. The physical properties of the phases come from the closeness and connectedness of the particles that comprise it.

10. a.Solids have particles that are very close and strongly bonded to each other. The particles of a solid cannot move; they can only vibrate. This gives solids definite shape and volume, and they are incompressible.

11. b.Liquids have particles that are close together, but they are weakly bonded. The particles in a liquid are free to move around each other, so liquids are fluids (able to flow). Liquids also do not have a definite shape, but still have a definite volume, and are still incompressible.

12. c.Gases have particles that are far apart from each other with no bonds between them. The particles of a gas very easily move around each other, so gases are also fluids. Gases to do not have definite shape nor volume, and are very compressible as there is large amounts of empty space between the particles.

13. d.Plasmas and Bose-Einstein Condensates are the other two phases of matter.

15. SolidLiquidGas Structure (closeness of the particles) Shape Volume Fluid Compressible

16. SolidLiquidGas Structure (closeness of the particles) close Shape Volume Fluid Compressible

17. SolidLiquidGas Structure (closeness of the particles) close Shape definite Volume Fluid Compressible

18. SolidLiquidGas Structure (closeness of the particles) close Shape definite Volumedefinite Fluid Compressible

19. SolidLiquidGas Structure (closeness of the particles) close Shape definite Volumedefinite Fluid no Compressible

20. SolidLiquidGas Structure (closeness of the particles) close Shape definite Volumedefinite Fluid no Compressible no

21. SolidLiquidGas Structure (closeness of the particles) close Shape definite Volumedefinite Fluid no Compressible no

22. SolidLiquidGas Structure (closeness of the particles) close Shape definiteNot definite Volumedefinite Fluid no Compressible no

23. SolidLiquidGas Structure (closeness of the particles) close Shape definiteNot definite Volumedefinite Fluid no Compressible no

24. SolidLiquidGas Structure (closeness of the particles) close Shape definiteNot definite Volumedefinite Fluid no yes Compressible no

25. SolidLiquidGas Structure (closeness of the particles) close Shape definiteNot definite Volumedefinite Fluid no yes Compressible no

26. SolidLiquidGas Structure (closeness of the particles) close Far apart Shape definiteNot definite Volumedefinite Fluid no yes Compressible no

27. SolidLiquidGas Structure (closeness of the particles) close Far apart Shape definiteNot definite Volumedefinite Fluid no yes Compressible no

28. SolidLiquidGas Structure (closeness of the particles) close Far apart Shape definiteNot definite Volumedefinite Not definite Fluid no yes Compressible no

29. SolidLiquidGas Structure (closeness of the particles) close Far apart Shape definiteNot definite Volumedefinite Not definite Fluid no yes Compressible no

30. SolidLiquidGas Structure (closeness of the particles) close Far apart Shape definiteNot definite Volumedefinite Not definite Fluid no yes Compressible no yes

31. 3.Matter can undergo changes, and there are two types of changes - physical and chemical.

32. a.Physical changes only change the spacing between the particles that make up the sample of matter. Examples are melting, condensing, and dissolving. All phase changes are physical changes!

33. b.Chemical changes change the bonding between the particles that make up. Examples are combustion, decomposition, and ionization. (When salts dissolve, they also ionize, so dissolving a salt is both a physical and chemical change.)

34. i. Chemical changes involve chemical reactions. Chemical reactions occur when one or more substances are converted into different substances. These are written as chemical equations.

35. ii. The substances that react in a chemical reaction are called reactants

36. iii. The different substances that are formed are called products

37. ii. The substances that react in a chemical reaction are called reactants iii. The different substances that are formed are called products iv. During a chemical reaction, the laws of conservation of mass and energy, definite proportion, and multiple proportions hold true

38. c.Both types of changes can change the physical properties of the sample of matter, so it can be really tricky to tell the difference between physical and chemical changes.

39. c.Also reversibility gives no indication. Ice can be melted into water; a reversible physical change, and paper can be ripped apart; an irreversible physical change.

40. c.Iron will rust; a reversible chemical change (with aluminum or other reducing agent)

42. c.Iron will rust; a reversible chemical change (with aluminum or other reducing agent), and cake will bake in a hot oven; an irreversible chemical change. The only way to know is to figure out if you’ve changed the distance or the bonds between the particles.

43. Classify each of the following as a physical or chemical change. Rusting (oxidation) of iron Fermentation of grape juice Freezing of yogurt Boiling of water Evaporation of alcohol Glowing of a firefly Battery charging Dissolving sugar in ice tea Grilling a steak Dissolving salt in ice tea

44. d.Regardless of the type of change, all physical and chemical changes must obey the law of conservation of mass and energy. New matter cannot be made from nothing, and matter cannot be made to disappear into nothing. The masses before a physical or chemical change must be equal to the masses after the change.

45. When burning a log in a fireplace, a large, heavy log become a few lightweight ashes. What happened to the rest of the mass if the law of conservation of mass is true?

46. 4.Matter is classified based on its composition. If the matter is uniform (unchanging) in composition, then it is called a substance. If the matter is not uniform (can change) in composition, then it is called a mixture. Uniform Not Uniform

47. Explain why salt (NaCl) and water (H 2 O) are both substances, but ocean water (salty water) is a mixture.

48. a.Substances contain matter that is uniform in composition, which are then separated based on the identity of the atoms in the substance. Substances include elements and compounds.

49. i.If all the atoms are the same, then it is called an element. There are 91 naturally occurring elements, and scientists have created many more. The best way to know if something is an element is to find it on the periodic table of elements. All the matter in the universe is made up of these elements (as far as we can tell).

50. ii.If the substance is made up of two or more types of atoms, but always in the same ratio, then it is called a compound.

51. ii.Elements that form into compounds typically do not retain their old properties. For example, sodium is a silver metal that explodes in water and chlorine is a poisonous yellow gas, but together they form the compound sodium chloride, which is a white solid that your body cannot live without.

52. iii.Chemical formulas can be written for compounds. Two laws apply to compounds:

53. 1.The law of multiple proportions states that the atoms in a compound can make multiple ratios, but they will always form whole-number ratios. For example, nitrogen and oxygen can make NO, NO 2, N 2 O, N 4 O, NO 3, N 2 O 3, and N 2 O 5.

54. 2.The law of definite proportions states that for one particular compound, the ratio of atoms is always definite. Finding the mass percent of each element in the compound can prove this. For example: Total MassMass of N% of NMass of O% of O NO3014471653 NO 2 4614303270 N2ON2O4428641636 N4ON4O7256781622 NO 3 6214234877 N2O3N2O3 7628374863 N2O5N2O5 10828268074

55. Classify the following as elements or compounds. Iron Carbon Potassium Chloride Sodium Nitrate Nitrous Oxide Helium Neon Californium Acetic Acid Dihydrogen Monoxide

56. b.Mixtures contain matter that is not uniform in composition. The two or more substance mixed together retains their individual properties. The composition is variable because there are many ways to mix substances together. Mixtures are further classified into two types - homogeneous and heterogeneous.

57. i.Homogeneous mixtures look like they have “same make-up”. There is an even spreading of all the substances. Homogeneous mixtures can be solutions or colloids.

58. 1.Solutions are made up of a solvent (thing doing the dissolving) and the solute (thing being dissolved). Solutions can be in solid, liquid, and gas phases. The solute has particles < 1 nm.

60. 2.Colloids have medium particles (between 1 nm and 1000 nm) so they are big enough to be noticed and reflect light in the Tyndall Effect, but not big enough to settle. Smoke and fog are examples.  Tyndall Effect

61. Aerosols: Man-made: Aerosol sprays, insecticide spray, smog. Natural: Fog, clouds. Solid aerosol: Natural: Smoke, dust. Foam: Man-made: Shaving lather, whipped cream. Emulsions: Man-made: Mayonnaise, cosmetic lotion, lubricants, milk. Sols: Man-made: Paint, ink, detergents, rubber. Solid foams: Man-made: Marshmallow, styrofoam, insulation, cushioning. Gels: Man-made: Butter, jelly. Solid sols: Man-made: Certain alloys. Natural: Pearl, opal.

62. ii.Heterogeneous mixtures look like they have “different make- up”. They do not have an even spreading of the substances and eventually will settle, so distinct parts can be identified. There is one type of heterogeneous mixtures - suspension.

63. 1.Suspensions have large solute particles (over 1000 nm) so they will settle if left alone. Anything that tells you to “shake well before using” is a suspension.

64. Classify the following as homogeneous or heterogeneous. Milk Sweet tea Muddy water Grape juice Blood Pepsi Whipped cream in a tub Pancake Syrup Bronze (copper and tin) Kool-Aid

67. 5.There are ways to separate mixtures and substances. Mixtures can be separated into substances with physical separations. Substances can be separated into elements with chemical separations.

68. a.Physical separations use physical means to separate the parts of a mixture, into the substances (elements and compounds) that comprise them. This can be as easy as separating the marshmallows from Lucky Charms using your fingers or iron from sand using a magnet.

69. a.Chemists have four typical physical separation techniques that are commonly used – filtration, distillation, crystallization, and chromatography. Sometimes combining several of these together is necessary to fully separate the substances in a mixture.

70. i.Filtration separates a heterogeneous mixture. A porous barrier (filter) is used that catches the undissolved particles from a liquid mixture while the liquid and any dissolved particles pass through.

71. ii.Distillation separates a homogeneous mixture of liquids with different boiling points. The mixture is heated, and the one with the lower boiling point boils out leaving he other one(s) behind. The one that vaporizes can be caught and condensed back into a liquid if desired.

73. iii.Crystallization separates a homogeneous mixture of a solid solute and liquid solvent. Heat is usually applied and the liquid evaporates leaving the solid behind as crystals.

74. iv.Chromatography separates a homogeneous mixture of many solutes of different molecular size or polarity. There are many types of chromatography, like paper, thin-layer, and gel electrophoresis.

76. b.Chemical separations can separate compounds into the elements that comprise it, but the method used depends on the characteristics of the elements. Water can be separated into hydrogen and oxygen by electricity.

77. c.Elements cannot be separated anymore by physical or chemical means (it takes nuclear reactions to separate an element into protons, neutrons, and electrons).

78. Matter Not uniformuniform

79. Matter MixturesSubstances Not uniformuniform looks different looks same

80. Matter MixturesSubstances HomogeneousHeterogeneous looks different looks same Not uniformuniform

81. Matter MixturesSubstances HomogeneousHeterogeneous Colloids Suspensions Solutions Not uniformuniform looks different looks same

82. Matter MixturesSubstances HomogeneousHeterogeneous Colloids Suspensions Solutions Not uniformuniform looks different looks same Elements Compounds

84. The Periodic Table 1.3

85. 1)The periodic table is a complex way to organize all the existing elements and can take many, many different forms 2) The typical periodic table organizes the elements by columns and rows

87. a) Elements are arranged into vertical columns called groups or families, and all the elements within have similar chemical properties.

88. b) The horizontal rows of elements are called periods, and are arranged in order of increasing atomic number (and usually also increasing atomic mass)

89. 3) The elements of the periodic table are arranged into three general categories – metals, nonmetals, and metalloids

90. a) Metals are elements that are good conductors of heat and electricity, and are malleable, ductile, have a high tensile strength, and are usually lustrous. Metals are found to the left of the stair-step line on the periodic table

91. i)Malleability is the ability to be shaped by being struck (with a hammer)

92. ii) Ductility is the ability to be stretched into wire

93. i)Malleability is the ability to be shaped by being struck (with a hammer) ii) Ductility is the ability to be stretched into wire iii) A high tensile strength causes metals to resist breaking when they are pulled

94. i)Malleability is the ability to be shaped by being struck (with a hammer) ii) Ductility is the ability to be stretched into wire iii) A high tensile strength causes metals to resist breaking when they are pulled iv) Most metals have luster and a silver color, but there are exceptions

95. b) Nonmetals are elements that are not good conductors, usually brittle, dull, and colorful in appearance. More than half of the nonmetals are gases at room temperature. Nonmetals are located to the right of the stair-step line, with the exception of hydrogen

96. c) Metalloids are elements that have some properties of metals and some of nonmetals. They are found touching the stair-step line, with the exception of aluminum.

97. d) A special group of elements on the periodic table are the Noble Gases. These are elements in group 8A or 18 and have extremely low reactivity with other elements. In 1962 xenon was forced to react with fluorine to form xenon tetrafluoride.