1. Chapter 1: Chemical Foundations The Scientific Method Units of Measurement Uncertainty in Measurement Significant Figures Dimensional Analysis Temperature Density Classification of Matter

2. Why Study Chemistry Every aspect of our lives are based on chemistry.Every aspect of our lives are based on chemistry. Microscopically (vs. macroscopically), everything is composed of atoms.Microscopically (vs. macroscopically), everything is composed of atoms. Is a tool to help understand and the world around you.Is a tool to help understand and the world around you.

3. Scientific Method A systematic approach to solving problems.

4. General Definitions Chemistry – study of the properties of materials and the changes that the material undergoes.Chemistry – study of the properties of materials and the changes that the material undergoes. Matter – The physical material of the universe; anything that has mass and takes up space.Matter – The physical material of the universe; anything that has mass and takes up space. Elements – A substance that cannot be separated into simpler substances by chemical means.Elements – A substance that cannot be separated into simpler substances by chemical means. Atoms – Building blocks of matter, the smallest representative particle of an element.Atoms – Building blocks of matter, the smallest representative particle of an element. Molecules – Atoms that are held together in specific shapes.Molecules – Atoms that are held together in specific shapes.

5. Chemistry The study of matter and the changes it undergoes.

6. Chemistry Solid – both a definite shape and definite volume Liquid – distinct volume independent of it’s container, so specific shape Gas – no fixed volume or shape

7. Chemistry Solid – molecules held together tightly; only “wiggling” slightly Liquid – molecules are packed more closely together than gas, less tightly than solid; allows for molecules to slide over each other Gas – Molecules are far apart, colliding only briefly with each other and with the wall of the container

8. States of Matter

9. Matter Anything that has mass and takes up space.

10. Matter Atoms are the building blocks of matter.Atoms are the building blocks of matter. Each element is made of the same kind of atom.Each element is made of the same kind of atom.

11. Matter Atoms are the building blocks of matter.Atoms are the building blocks of matter. Each element is made of the same kind of atom.Each element is made of the same kind of atom. A compound is made of two or more different kinds of elements.A compound is made of two or more different kinds of elements.

12. Classification of Matter

22. Uncertainty in Measurement

23. Significant Figures The term significant figures refers to digits that were measured.The term significant figures refers to digits that were measured. When rounding calculated numbers, we pay attention to significant figures so we do not over/understate the accuracy of our answers.When rounding calculated numbers, we pay attention to significant figures so we do not over/understate the accuracy of our answers.

24. Significant Figures 1.All nonzero digits are significant. 2.Zeroes between two significant figures are themselves significant. 3.Zeroes at the beginning of a number are never significant. 4.Zeroes at the end of a number are significant if a decimal point is written in the number.

25. Significant Figures Examples: #Sig FigRule(s) Applied 0.02110640.300714.2324300.000.05082

26. Significant Figures When addition or subtraction is performed, answers are rounded to the least significant decimal place.When addition or subtraction is performed, answers are rounded to the least significant decimal place. When multiplication or division is performed, answers are rounded to the number of digits that corresponds to the least number of significant figures in any of the numbers used in the calculation.When multiplication or division is performed, answers are rounded to the number of digits that corresponds to the least number of significant figures in any of the numbers used in the calculation.

27. Accuracy versus Precision Accuracy refers to the proximity of a measurement to the true value of a quantity. Accuracy refers to the proximity of a measurement to the true value of a quantity. Precision refers to the proximity of several measurements to each other. Precision refers to the proximity of several measurements to each other.

28. Dimensional Analysis Metric System Unit = label “What do you have?” “I have 3.” “How much coffee do you want?” “I want four.” Metric based off UnitUS Metric Weight/MassLengthVolume

29. Dimensional Analysis Conversion Factor - “ratio that converts a measure expressed in one unit to a measure expressed in another unit”.Conversion Factor - “ratio that converts a measure expressed in one unit to a measure expressed in another unit”. Always equal to “1”Always equal to “1”

30. Dimensional Analysis Example A vitamin C tablet is found to contain 0.500 g of vitamin C. How many milligrams of vitamin C does this table contain? GivenKnownQuestion

31. Dimensional Analysis Example A piece of copper metal has a mass of 17.6 lb. What is the copper mass in kilograms? GivenKnownQuestion

32. Dimensional Analysis Example The estimated amount of recoverable oil from the field at Prudhoe Bay in Alaska is 4.0 x 10 11 gal. What is the amount in fluid ounces (fl. Oz)? GivenKnownQuestion

33. Units of Measurement

34. SI Units Système International d’UnitésSystème International d’Unités Uses a different base unit for each quantityUses a different base unit for each quantity

35. Metric System Prefixes convert the base units into units that are appropriate for the item being measured.

36. Volume The most commonly used metric units for volume are the liter (L) and the milliliter (mL).The most commonly used metric units for volume are the liter (L) and the milliliter (mL). □ A liter is a cube 1 dm long on each side. □ A milliliter is a cube 1 cm long on each side.

37. Uncertainty in Measurements Different measuring devices have different uses and different degrees of accuracy.

38. Temperature A measure of the average kinetic energy of the particles in a sample.

39. Temperature In scientific measurements, the Celsius and Kelvin scales are most often used.In scientific measurements, the Celsius and Kelvin scales are most often used. The Celsius scale is based on the properties of water.The Celsius scale is based on the properties of water. □ 0  C is the freezing point of water. □ 100  C is the boiling point of water.

40. Temperature The Kelvin is the SI unit of temperature.The Kelvin is the SI unit of temperature. It is based on the properties of gases.It is based on the properties of gases. There are no negative Kelvin temperatures.There are no negative Kelvin temperatures. K =  C + 273.15K =  C + 273.15

41. Temperature The Fahrenheit scale is not used in scientific measurements.The Fahrenheit scale is not used in scientific measurements.  F = 9/5(  C) + 32  F = 9/5(  C) + 32  C = 5/9(  F − 32)  C = 5/9(  F − 32)

42. Density Physical property of a substance d = mV

43. Properties and Changes of Matter

44. Properties of Matter Physical Properties:Physical Properties: □ Can be observed without changing a substance into another substance. Boiling point, density, mass, volume, etc.Boiling point, density, mass, volume, etc. Chemical Properties:Chemical Properties: □ Can only be observed when a substance is changed into another substance. Flammability, corrosiveness, reactivity with acid, etc.Flammability, corrosiveness, reactivity with acid, etc.

45. Properties of Matter Intensive Properties:Intensive Properties: □ Independent of the amount of the substance that is present. Density, boiling point, color, etc.Density, boiling point, color, etc. Extensive Properties:Extensive Properties: □ Dependent upon the amount of the substance present. Mass, volume, energy, etc.Mass, volume, energy, etc.

46. Changes of Matter Physical Changes:Physical Changes: □ Changes in matter that do not change the composition of a substance. Changes of state, temperature, volume, etc.Changes of state, temperature, volume, etc. Chemical Changes:Chemical Changes: □ Changes that result in new substances. Combustion, oxidation, decomposition, etc.Combustion, oxidation, decomposition, etc.

47. Chemical Reactions In the course of a chemical reaction, the reacting substances are converted to new substances.

48. Compounds Compounds can be broken down into more elemental particles.

49. Electrolysis of Water

50. Separation of Mixtures

51. Distillation Separates homogeneous mixture on the basis of differences in boiling point.

52. Distillation

53. Filtration Separates solid substances from liquids and solutions.

54. Chromatography Separates substances on the basis of differences in solubility in a solvent.

55. Chapter 1: Chemical Foundations The Scientific Method Units of Measurement Uncertainty in Measurement Significant Figures Dimensional Analysis Temperature Density Classification of Matter