1. An Introduction to Chemistry Chapter 1 Hein and Arena Eugene Passer Chemistry Department Bronx Community College © John Wiley and Sons, Inc Version 2.0 12 th Edition

2. Chapter Outline 1.1 Why Study Chemistry? 1.2 The Nature of Chemistry 1.3 Thinking Like A Chemist 1.4 A Scientific Approach to Problem SolvingA Scientific Approach toProblem Solving 1.5 The Scientific Method 1.6 The Particulate Nature of MatterThe Particulate Nature ofMatter 1.7 The Physical States of MatterThe Physical States of Matter 1.8 Classifying MatterClassifying Matter

3. What is a Science? The observation, identification, description, experimental investigation, and theoretical explanation of natural phenomena.

4. Natural Phenomena experimentally investigate theoretically explain observe describeidentify

5. Chemistry The science of the composition, structure, properties and reactions of matter, especially of atomic and molecular systems.

6. Matter compositionstructure propertiesreactions

7. 1.4 A Scientific Approach to Problem Solving

8. Problem Solving 1.Define the problem by recognizing it and stating it clearly. In science this is called an observation. 2. Propose solutions to the problem. In science this is called a hypothesis. 3. Decide the best way to solve the problem. In science we perform an experiment.

9. 1.5 The Scientific Method

10. Definitions

11. Law: Statement of natural phenomena to which no exceptions are known under the given conditions. A law is not an explanation. Hypothesis: A tentative explanation of certain facts that provide a basis for further experimentation. Theory: Well- established hypothesis. An explanation of the general principles of certain phenomena with considerable evidence or facts to support it.

12. Outline

14. Steps

15. 2. Analyze the data to find trends (regularities). 3. Formulate a hypothesis that will account for the data and that can be tested by further experimentation. 1. Collect facts or data that are relevant to the problem or question at hand. This is usually done by experimentation.

16. 5. Modify the hypothesis to ensure compatibility with the experimental data. 4. Plan and do additional experiments to test the hypothesis.

17. EXPLANATIONS

19. 1.6 The Particulate Nature of Matter

20. 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.

21. 1.3 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.

22. 1.7 Physical States of Matter

23. Shape Definite - does not change. It is independent of its container. Volume Definite ParticlesParticles are close together. They cling rigidly to each other. SOLIDS CompressibilityVery slight–less than liquids and gases.

24. Solid Amorphous Solid Particles lack a regular internal arrangement Glass, plastics, gels Crystalline Solid Particles exist in regular, repeating three-dimensional geometric patterns. Diamond, metals, salts A solid can be either crystalline or amorphous. Which one it is depends on the internal arrangement of the particles that constitute the solid.amorphous

25. Amorphous: without shape or form.

26. Shape Not definite - assumes the shape of its container. Volume Definite Particles 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. LIQUIDS CompressibilityVery slight–greater than solids, less than gases.

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

28. 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.

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

30. 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.

33. 1.8 Classifying Matter

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

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

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

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

38. Homogeneous Heterogeneous

39. 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.

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

41. 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.

42. 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. Heterogeneous Mixture A heterogeneous mixture consists of 2 or more phases.

43. 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. Heterogeneous Mixture A heterogeneous mixture consists of 2 or more phases.

44. solid phase 2 liquid phase solid phase 1 Heterogeneous Mixture

45. Mixture of iron and sulfur Compound of iron and sulfur FormulaHas no definite formula: consists of Fe and S. FeS CompositionContains Fe and S in any proportion by mass. 63.5% Fe and 36.5% S by mass. SeparationFe and S can be separated by physical means. Fe and S can be separated only by chemical change.

46. 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.

47. 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.

48. 1.6 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.