1. Unit 1. Matter and Change

2. Do Now:  What are the State of Matter?

3. Objectives:  Define the term “chemistry”  Describe the difference branches of Chemistry.  Describe the difference between a physical change and a chemical change and give several examples of each.  Describe different characteristics of the three states matter.  Classify a mixture as homogeneous or heterogeneous.  Classify a pure substance as an element or a compound.

4. Chapter 1 Section 1 Chemistry is a Physical Science

5.  Chemistry is the study of matter and the changes that it undergoes. Biological Science Physical Sciences Chemistry Chemistry is central to all sciences. Both living and non living matter have a chemical structure.

6. Chemistry deals with: 1.What is material made of? 2.What is the makeup and internal arrangement of the atoms? 3.How does it behave when heated, cooled or mixed with other materials?

7. Branches of Chemistry Organic chemistry – the study of carbon containing compounds. Inorganic chemistry – the study of substances that do not contain carbon (metals and gases). Physical chemistry – the study of the properties and changes of matter and their relation to energy. Introduction Video

8. Analytical chemistry –the identification of the components and composition of materials. Biochemistry – the study of the processes occurring in living systems.

9. Let’s try some examples  1.

10. Types of Research  Basic Research - carried out for the sake of increasing knowledge.  Most basic research is carried out in universities.  Research is normally published in scientific journals.

11. Types of Research  Applied Research - carried out to solve a problem.  Research is carried out by companies to make a profit.  Usually short term goals set by the company.

12. Summary 1)Define the word chemistry. 2) Name the five branches of chemistry. 3) Define basic and applied research.

13. STATE OF MATTER

14. States of Matter  There are Four state of matter  A. Solid  B. Liquid  C. Gas  D. Plasma  State of matter depends on Kinetic Energy between the particles

15. A. Kinetic Molecular Theory  KMT  Particles of matter are always in motion.  The kinetic energy (speed) of these particles increases as temperature increases.

16. Four States of Matter  A. Solids  very low KE - particles vibrate but can’t move around  fixed shape  fixed volume

17. Four States of Matter  B. Liquids  low KE - particles can move around but are still close together  variable shape  fixed volume

18. Four States of Matter  C. Gases  high KE - particles can separate and move throughout container  variable shape  variable volume

19. Matter and its Properties  It’s Classified!

20. Objective  Distinguish between:  intensive and extensive properties  Physical & chemical changes/properties  Classify matter

21. Properties & Changes in Matter  Extensive vs. Intensive  Physical vs. Chemical

22. A. Extensive vs. Intensive  Extensive Property  depends on the amount of matter present  ex,.-  Intensive Property  depends on the identity of substance, not the amount  Ex.-

23. A. Extensive vs. Intensive  Extensive Property  depends on the amount of matter present  ex,.- Volume, mass, Energy  Intensive Property  depends on the identity of substance, not the amount  Ex.- melting point, boiling point, conduct electricity or heat  WHAT ABOUT DENSITY??

24. A. Extensive vs. Intensive  Examples:  boiling point  volume  mass  density  conductivity

25. A. Extensive vs. Intensive  Examples:  boiling point…… intensive  Volume …. extensive  Mass ….. extensive  Density ….. intensive  Conductivity ….. intensive

26. PROPERTY B. Physical vs. Chemical  Physical Property  can be observed without changing the identity of the substance  Chemical Property  describes the ability of a substance to undergo changes in identity

27. B. Physical vs. Chemical  Examples:  melting point  flammable  density  magnetic  tarnishes in air physical chemical physical chemical

28. B. Physical vs. Chemical  Examples:  melting point  flammable  density  magnetic  tarnishes in air physical chemical physical chemical

29. CHANGE C. Physical vs. Chemical  Physical Change  changes the form of a substance without changing its identity  properties remain the same  Chemical Change  changes the identity of a substance  products have different properties

30. B. Physical vs. Chemical  Signs of a Chemical Change  change in color or odor  formation of a gas  formation of a precipitate (solid)  change in light or heat

31. In the example of burning of charcoal, carbon and oxygen are the reactants in the combustion reaction. Carbon dioxide is the product. carbon + oxygen carbon dioxide C + O2 CO2 (reactants) (product) Properties and Changes in Matter

32. B. Physical vs. Chemical  Examples:  rusting iron  dissolving in water  burning a log  melting ice  grinding spices

33. B. Physical vs. Chemical  Examples:  rusting iron  dissolving in water  burning a log or charcoal  melting ice  grinding spices chemical physical chemical physical

34. Four States of Matter  D. Plasma  very high KE - particles collide with enough energy to break into charged particles (+/-)  gas-like, variable shape & volume  stars, fluorescent light bulbs, CRTs

35. SOLUTIONS AND MIXTURES

36. Objective:  Classification of Matter  DO NOW:  What is a solution?  Describe the difference between a heterogeneous and homogenous mixture

37. A. Pure Substances  Element  composed of identical atoms  EX: copper wire, aluminum foil

38. A. Pure Substances  Compound  composed of 2 or more elements in a fixed ratio  properties differ from those of individual elements  EX: table salt (NaCl)

39. A. Pure Substances  Law of Definite Composition  A given compound always contains the same, fixed ratio of elements.  Law of Multiple Proportions  Elements can combine in different ratios to form different compounds.

40. A. Pure Substances  For example… Two different compounds, each has a definite composition.

42. Pure Substances (constant composition)  Elements  Listed on the Periodic Table  Cannot be broken down into unique components  Na, Cl, Al, O 2, S 8  Compounds  Made of elements that are chemically joined  Can be broken down  NaCl, H 2 O, AlCl 3, H 2 SO 4

43. B. Mixtures  Variable combination of 2 or more pure substances. HeterogeneousHomogeneous

44. B. Mixtures (variable composition)  Homogeneous – Solutions  evenly distributed  Heterogeneous  not evenly distributed

45. B. Mixtures  Solution  homogeneous  very small particles  no Tyndall effect Tyndall Effect

46. B. Mixtures  Colloid  heterogeneous  medium-sized particles  Tyndall effect  particles don’t settle  EX: milk

47. B. Mixtures  Suspension  heterogeneous  large particles  Tyndall effect  particles settle  EX: fresh-squeezed lemonade

48. C. Mixtures  Examples:  mayonnaise  muddy water  fog  saltwater  Italian salad dressing

49. C. Mixtures  Examples:  mayonnaise  muddy water  fog  saltwater  Italian salad dressing colloid suspension colloid solution suspension

51. A. Matter Flowchart MATTER Can it be physically separated? Homogeneous Mixture (solution) Heterogeneous MixtureCompoundElement MIXTUREPURE SUBSTANCE yesno Can it be chemically decomposed? noyes Is the composition uniform? noyes ColloidsSuspensions

52. A. Matter Flowchart  Examples:  graphite  pepper  sugar (sucrose)  paint  soda

53. A. Matter Flowchart  Examples:  graphite  pepper  sugar (sucrose)  paint  soda element hetero. mixture compound hetero. mixture solution

54. Tea – Homogeneous Mixture

55. Air – Homogeneous Mixture

56. Alloys – Homogeneous Mixtures

57. Cereal – Heterogeneous Mixture

58. Sand – Heterogeneous Mixture

59. Separating Mixtures  Only a physical change- no new matter  Filtration - separate solids from liquids with a barrier (filter paper)  Distillation - separate liquids because of different boiling points  Heat mixture  Catch vapor in cooled area  Chromatography - different substances are attracted to paper or gel, so move at different speeds

61. The Periodic Table

62. A. Mendeleev  Dmitri Mendeleev (1869, Russian)  Organized elements by increasing atomic mass.  Elements with similar properties were grouped together.  There were some discrepancies. C. Johannesson

63. A. Mendeleev  Dmitri Mendeleev (1869, Russian)  Predicted properties of undiscovered elements. C. Johannesson

64. B. Moseley  Henry Moseley (1913, British)  Organized elements by increasing atomic number.  Resolved discrepancies in Mendeleev’s arrangement. C. Johannesson

65. II. Organization of the Elements

66. A. Metallic Character  Metals  Nonmetals  Metalloids C. Johannesson

68. B. Blocks  Main Group Elements  Transition Metals  Inner Transition Metals C. Johannesson

69. Do Now:  Classify the following as either a METAL, NON-METAL or METALLOID: a. Au b. Si c. Br d. An element that is brittle and conducts electricity e. An element that is malleable f. An element that has tendency to become an anion

70. Periods and Families  Periods: horizontal rows on the periodic table  physical and chemical properties change somewhat regularly across a row.  Elements closer to each other in the same period tend to be similar than those that are farther apart.  Families: vertical rows of elements, aka groups  Each group contains similar chemical properties

71. Types of Elements  METALS:  Shiny  Conductors of heat and electricity  Most metals are malleable (can be pounded into thin sheets; a sugar cube sized chunk of gold can be pounded into a thin sheet which will cover a football field),  Most metals are ductile (can be drawn out into a thin wire).

72. Metals cont…..  All are solids at room temp (except Mercury, which is a liquid)  Metals tend to have low ionization energies, and typically lose electrons (i.e. are oxidized) when they undergo chemical reactions  Alkali metals are always 1+ (lose the electron in s subshell)  Alkaline earth metals are always 2+ (lose both electrons in s subshell)  Compounds of metals with non-metals tend to be ionic in nature.

73. Types of Elements  NON- METALS:  Vary greatly in appearance  Non-lustrous  Poor conductors of heat and electricity  The melting points of non-metals are generally lower than metals  Seven non-metals exist under standard conditions as diatomic molecules: H 2 (g) N 2 (g) O 2 (g) F 2 (g) Cl 2 (g) Br 2 (l) I 2 (l) (volatile liquid - evaporates readily)

74. Non-Metals cont……..  Nonmetals, when reacting with metals, tend to gain electrons (typically attaining noble gas electron configuration) and become anions: Nonmetal + Metal -> Salt  Compounds composed entirely of nonmetals are molecular substances (not ionic)

75. Types of Elements  Metalloids:  Elements may share properties of metals and non-metals.  A stair-step line separates the metals from the nonmetals on the periodic table.

76. Metalloids cont……  Properties:  All metalloids are solids at room temperature.  Less malleable than metals but not as brittle as nonmetals.  Metalloids tend to be semiconductors of electricity. (intermediate between metals and nonmetals).

77. Metalloids cont……  Properties:  Metalloids are used in semiconducting materials found in computers, calculators, televisions and radios.  Elements include: boron, silicon, germanium, antimony

78. Noble Gases  Noble Gases - the elements in Group 18 of the periodic table.  They are considered nonmetals.  These elements are generally unreactive.  All are gases at room temperature.  Examples: neon, argon, krypton, xenon (all used in lighting) and helium.