Introductory Chemistry CHEM 107

1. Introductory Chemistry CHEM 107 • Spring 2007 • John Alexander Ph.D. • Email - jalexander@fullcoll.edu • Web site: http://staffwww.fullcoll.edu/jalexander/ • VoiceMail:(714)992-7000 Dial 0 then ask for extension – 28873 • Office hours - By appointment • Lecture - Tuesday and Thursday 8:30-10:20 Am

2. Introductory Chemistry CHEM 107 • CRN-10233 • Lecture 8:30-10:20A Tu ThRoom 411 • Problem Solving 11:00- 11:50A Tu Room 412 • Lab 1:30- 4:20P Tu Room 412 • CRN-10234 • Lecture 8:30-10:20A Tu ThRoom 411 • Problem Solving 11:00- 11:50A Th Room 412 • Lab 1:30- 4:20P Th Room 412

3. Required Material • Text: Foundations of College Chemistry Hein & Arena 12th ed. • Lab manual • Goggles • Safety Packet • Calculator • Fullerton College Computer Account

4. Key Help for Chemistry • Read syllabus carefully • You should have already read chapter 1 • Read ahead, stay ahead • College chemistry before? • I suggest becoming familiar with tutoring services.

5. Tutoring Center • First floor of the Library/Learning Resource Center - Building 800 • Hours: Mon.-Thur. 9:00 A.M. - 7:00 P.M. Fri. 10:00 A.M. - 2:00 P.M.Sat.* 10:00 A.M.-2:00 P.M. • *Only Math, Chemistry, English, Physics and Accounting on Saturday • Phone: 714-992-7000 x 25386 for appointment

6. Absences • AVOID Absences – this is college so it’s up to you!!! • However no make up Exam or quiz is offered so you must be here for exam and quiz. • I you want to maintain a good grade you need to avoid all absences.

7. Why are you HERE? • Chemistry is all around us. Medicines, plastics, energy, etc… • What do you get? Problem solving skills, strategic tool box to allow you to solve complex problems. • Confidence? Chemistry should build confidence in you as you develop the skills to tackle the complex problems.

8. Chemistry? • Chemistry is the science of the composition, structure, properties, and reaction of matter, especially of atomic and molecular systems. • Chemistry is the science dealing with the composition of matter and the changes in composition that matter undergoes.

9. Chemistry? • Chemistry is a fundamental science: an understanding of chemistry help one to understand the complex chemical processes of biological systems. • Chemistry’s scope is broad and touches many of the other area which include engineering of new materials and many other areas.

10. Process of Chemistry • How are discoveries made? Many times it just luck? Or is it good observation!!! • If one pay attention in a chemistry lab you just may make a discovery!!!

11. Process of Chemistry William Buehler was working on a material for the nose cone of missle launcher. He found a titanium/nickel mixture had good impact resistance. While working with this material he accidentally dropped a bar of this material, cool ones made a thud sound, hot gave a bell tone. Why was this observation important? It signals a change of atomic structure!!! He rolled out strips to observe fatigue resistance, the strips were bent, but if heated the strips went back to straight!!! He had basically developed memory metal!!!

12. Scientific Method • 1. Observations – Collect facts & data •  quantitative •  qualitative • 2. Formulating hypotheses •  possible explanation for the observation • 3. Performing experiments •  gathering new information to decide whether the hypothesis is valid • 4. Modify hypothesis •  compatible with all pertinent data

13. Scientific Method • Hypothesis  A tentative explanation of certain facts • Theory (Model) •  A set of tested hypotheses that give an overall explanation of some natural phenomenon. • Natural Law or Scientific Law •  The same observation applies to many different systems, with no know exceptions under a certain set of conditions •  Example – • Law of Conservation of Mass

14. Relationship to Other Sciences • Science on its own • Chemistry & Physics are overlapping both based on properties and nature of materials • Biological processes are chemical in nature. • Food – Agriculture – Preservation • Medicines (pharmaceuticals)

15. Risk and Benefits • Science is relied on for many answers of today's problems • Aids vaccine • Use of herbicides and pesticides • Analysis of DNA – Genetic Disease – Crime Scene • Asbestos, Lead, and Radon • Global warming and Ozone hole • Coffee, Alcohol, Fats, and Tobacco • Global ecology

16. The Particulate Nature of Matter • Matter can be invisible. • Air is matter, but it cannot be seen. • Matter appears to be continuous and unbroken. • Matter is actually discontinuous. It is made up of tiny particles call atoms. • Matter is anything that has mass and occupies space.

17. An apparently empty test tube is submerged, mouth downward in water. Only a small volume of water rises into the tube, which is actually filled with invisible matter–air. 1.3

18. Physical Statesof Matter

19. SOLIDS Shape • Definite - does not change. It is independent of its container. Volume • Definite Particles • Particles are close together. Theycling rigidly to each other. Compressibility • Very slight–less than liquidsand gases.

20. A solid can be either crystalline or amorphous. Which one it is depends on the internal arrangement of the particles that constitute the solid.

21. LIQUIDS • Not definite - assumes the shape of its container. Shape Volume • Definite • Particles are close together. • Particles are held together by strong attractive forces. They stick firmly but not rigidly to each other. • They can move freely throughout the volume of the liquid. Particles Compressibility • Very slight–greater than solids,less than gases.

22. GASES Shape • No fixed shape. Volume • Indefinite. Particles • Particles are far apart compared to liquids and solids. • Particles move independently of each other.

23. GASES Compressibility • The actual volume of the gas particles is small compared to the volume of space occupied by the gas. • Because of this a gas can be compressed into a very small volume or expanded almost indefinitely.

24. ATTRACTIVE FORCES • Attractive forces are strongest in a solid. • These give a solid rigidity. Solid Liquid • Attractive forces are weaker in liquids than in solids. • They are sufficiently strong so that a liquid has a definite volume.

25. ATTRACTIVE FORCES Gas • Attractive forces in a gas are extremely weak. • Particles in the gaseous state have enough energy to overcome the weak attractive forces that hold them together in liquids or solids. • Because of this the gas particles move almost independently of each other.

28. Classifying Matter Matter refers to all of the materials that make up the universe.

29. Substance A particular kind of matter that has a fixed composition and distinct properties. Examples ammonia, water, and oxygen.

30. Homogeneous Matter Matter that is uniform in appearance and with uniform properties throughout. Examples ice, soda, pure gold

31. Heterogeneous Matter Matter with two or more physically distinct phases present. Examples ice and water, wood, blood

32. Homogeneous Heterogeneous

33. Phase A homogenous part of a system separated from other parts by physical boundaries. Examples In an ice water mixture, ice is the solid phase and water is the liquid phase.

34. Mixture Matter containing 2 or more substances that are present in variable amounts. Mixtures are variable in composition. They can be homogeneous or heterogeneous.

35. Homogeneous Mixture (Solution) A homogeneous mixture of 2 or more substances. It has one phase. Example Sugar and water. Before the sugar and water are mixed, each is a separate phase. After mixing the sugar is evenly dispersed throughout the volume of the water.

36. Heterogeneous Mixture A heterogeneous mixture consists of 2 or more phases. Example Sugar and fine white sand. The amount of sugar relative to sand can be varied. The sugar and sand each retain their own properties.

37. Heterogeneous Mixture A heterogeneous mixture consists of 2 or more phases. Example • Iron (II) sulfide (FeS) is 63.5% Fe and 36.5% S by mass. • Mixing iron and sulfur in these proportions does not form iron (II) sulfide. Two phases are present: a sulfur phase and an iron phase. • If the mixture is heated strongly a chemical reaction occurs and iron (II) sulfide is formed. • FeS is a compound of iron and sulfur and has none of the properties of iron or sulfur.

38. solid phase1 solid phase2 Heterogeneous Mixture liquid phase

40. Heterogeneous Mixture of One Substance A pure substance can exist as different phases in a heterogeneous system. Example Ice floating in water consists of two phases and one substance. Ice is one phase, and water is the other phase. The substance in both cases is the same.

41. System The body of matter under consideration. Examples In an ice water mixture, ice is the solid phase and water is the liquid phase. The system is the ice and water together.

42. Classification of matter: A pure substance is always homogeneous in composition, whereas a mixture always contains two or more substances and may be either homogeneous or heterogeneous. 1.6

43. Chapter 1 – An Introduction to Chemistry • Why Study Chemistry • Nature of Chemistry • Thinking like a Chemisty • Scientific Method – Hypothesis, Laws, Method, Theory • Relationship to Other Sciences and Industry • Risk and Benefits • Nature of Matter • Physical States of Matter • Classifying Matter