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CHAPTER 1 Matter & Measurement General, Organic, & Biological Chemistry Janice Gorzynski Smith

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CHAPTER 1: Matter & Measurement 2 Smith. General Organic & Biolocial Chemistry 2nd Ed. Learning Objectives: Definition of matter Solids, liquids, and gases Physical vs chemical properties and changes Pure substances: Elements & Compounds Mixtures: Heterogeneous vs Homogeneous Units of the metric system & common prefixes Measured vs exact numbers Significant figures: identify & use in calculations Scientific Notation Conversion factors for calculations to cancel units The three temperature scales Density and Specific Gravity

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Matter Definition 3 Smith. General Organic & Biolocial Chemistry 2nd Ed. Matter is anything that has mass and takes up volume. Naturally occurring: cotton sand digoxin, a cardiac drug Synthetic (human-made): nylon Styrofoam ibuprofen

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Matter Solids, Liquids, Gases 4 Smith. General Organic & Biolocial Chemistry 2nd Ed. The Solid State: A solid has a definite volume. It maintains its shape regardless of its container. Solid particles lie close together in a regular pattern. The Liquid State: A liquid has a definite volume. It takes the shape of its container. Liquid particles are close together but can move past one another. The Gas State: A gas has no definite shape; it assumes the shape of its container. It has no definite volume; it assumes the volume of its container. Gas particles are very far apart and move around randomly.

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Matter Physical Properties 5 Smith. General Organic & Biolocial Chemistry 2nd Ed. Physical properties can be observed or measured without changing the composition of the material. boiling point melting point solubility color odor state of matter

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Matter Chemical Properties 6 Smith. General Organic & Biolocial Chemistry 2nd Ed. Chemical properties determine how a substance can be converted into another substance. Chemical change is the chemical reaction that converts one substance into another (Chapters 5 and 6).

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Matter Pure Substances: Elements 7 Smith. General Organic & Biolocial Chemistry 2nd Ed. A pure substance is composed of only a single component (atom or molecule). It has a constant composition, regardless of sample size or origin of sample. It cannot be broken down to other pure substances by a physical change. Pure Substances An element is a pure substance that cannot be broken down by a chemical change. aluminum metal (Al)

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Matter Pure Substances: Compounds 8 Smith. General Organic & Biolocial Chemistry 2nd Ed. A compound is a pure substance formed by chemically joining two or more elements. table salt (NaCl)

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Matter Mixtures 9 Smith. General Organic & Biolocial Chemistry 2nd Ed. Mixtures Mixtures are composed of more than one component. They can have varying composition (any combination of solid, liquid, and gas). Mixtures can be separated into their components by a physical process. All matter can be classified as either a pure substance or a mixture.

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Matter Mixtures: Heterogeneous & Homogeneous 10 Smith. General Organic & Biolocial Chemistry 2nd Ed. Homogeneous Mixture Example: simple syrup Heterogeneous Mixture Example: vinaigrette

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11 Matter Definition http://ridenourmhs.wikispaces.com/ESUnit2

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Measurements Metric System 12 Smith. General Organic & Biolocial Chemistry 2nd Ed. Each type of measurement has a base unit in the metric system.

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Measurements Common Prefixes 13 Smith. General Organic & Biolocial Chemistry 2nd Ed. The prefix of the unit name indicates if the unit is larger or smaller than the base unit.

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Measurements Common Prefixes 14 Smith. General Organic & Biolocial Chemistry 2nd Ed. 1 kilometer (km) = 1,000 meters (m) 1 km = 1,000 m 1 millimeter (mm) = 0.001 meters (m) 1 mm = 0.001 m 1 centimeter (cm) = 0.01 meters (m) 1 cm = 0.01 m The base unit of length is the meter (m).

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Measurements Common Prefixes 15 Smith. General Organic & Biolocial Chemistry 2nd Ed. Mass is a measure of the amount of matter in an object. Weight is the force that matter feels due to gravity. 1 kilogram (kg) = 1,000 grams (g) 1 kg = 1,000 g 1 milligram (mg) = 0.001 grams (g) 1 mg = 0.001 g The base unit of mass is the gram (g).

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Measurements Common Prefixes 16 Smith. General Organic & Biolocial Chemistry 2nd Ed. 1 kiloliter (kL) = 1,000 liters (L) 1 kL = 1,000 L 1 milliliter (mL) = 0.001 liters (L) 1 mL = 0.001 L Volume = Length x Width x Height = cm x cm x cm = cm 3 1 mL = 1 cm 3 = 1 cc The base unit of volume is the liter (L).

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Measurements Units 17 Smith. General Organic & Biolocial Chemistry 2nd Ed.

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Measurements Exact Numbers 18 Smith. General Organic & Biolocial Chemistry 2nd Ed. An exact number results from counting objects or is part of a definition. 10 fingers 10 toes 1 meter = 100 centimeters An inexact number results from a measurement or observation and contains some uncertainty. 15.3 cm 1000.8 g 0.0034 mL

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Measurements Significant Figures 19 Smith. General Organic & Biolocial Chemistry 2nd Ed. Significant figures are all the digits in a measured number including one estimated digit. All nonzero digits are always significant. 3 sig. figures6 sig. figures 65.2 g 255.345 g 65.2 g 255.345 g

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Measurements Significant Figures 20 Smith. General Organic & Biolocial Chemistry 2nd Ed. 3 sig. figures Rule 1: A zero counts as a significant figure when it occurs: between two nonzero digits 5 sig. figures at the end of a number with a decimal place 29.05 g 4 sig. figures 1.0087 mL29.05 g1.0087 mL 3.7500 cm 5 sig. figures 620. lb 3.7500 cm 620. lb

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Measurements Significant Figures 21 Smith. General Organic & Biolocial Chemistry 2nd Ed. Rule 2: A zero does not count as a significant figure when it occurs: 5 sig. figures at the beginning of a number 1 sig. figure at the end of a number that does not have a decimal 0.00245 mg0.008 mL 3 sig. figures 0.00245 mg0.008 mL 2570 m1245500 m 3 sig. figures 2570 m1245500 m

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Measurements Significant Figures: Multiplication & Division 22 Smith. General Organic & Biolocial Chemistry 2nd Ed. 351.2 miles 5.5 hour = 63.854545 miles hour 351.2 miles 5.5 hour 4 sig. figures 2 sig. figures Answer must have 2 sig. figures. Multiplication/Division Rules: The answer has the same number of significant figures as the original number with the fewest significant figures.

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Measurements Significant Figures: Multiplication & Division 23 Smith. General Organic & Biolocial Chemistry 2nd Ed. 63.854545 miles to be retainedto be dropped first digit to be dropped hour 63.854545 If the first digit to be dropped is: Then: between 0 and 4drop it and all remaining digits between 5 and 9 round up the last digit to be retained by adding 1 = 2 sig. figures Answer 64 miles hour

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Measurements Significant Figures: Addition & Subtraction 24 Smith. General Organic & Biolocial Chemistry 2nd Ed. Addition/Subtraction Rules: The answer has the same number of decimal places as the original number with the fewest decimal places. 10.11 kg 3.6 kg 6.51 kg 10.11 kg 3.6 kg 2 decimal places 1 decimal place answer must have 1 decimal place = 6.5 kg final answer 1 decimal place

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Measurements Scientific Notation 25 Smith. General Organic & Biolocial Chemistry 2nd Ed. Coefficient: A number between 1 and 10. y x 10 x Exponent: Any positive or negative whole number. In scientific notation, a number is written as:

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Measurements Scientific Notation 26 Smith. General Organic & Biolocial Chemistry 2nd Ed. When the exponent x is positive, move the decimal point x places to the right. 2.80 x 10 2 = 2.800 x 10 2 = When the exponent x is negative, move the decimal point x places to the left. 280.0 0.0280

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Measurements Conversion Factors 27 Smith. General Organic & Biolocial Chemistry 2nd Ed. Conversion factor: A term that converts a quantity in one unit to a quantity in another unit. Conversion factors are usually written as equalities. 2.21 lb = 1 kg To use them, they must be written as fractions. original quantity original quantity conversion factor desired quantity desired quantity x = 2.21 lb 1 kg or 1 kg 2.21 lb

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Measurements Conversion Factors 28 Smith. General Organic & Biolocial Chemistry 2nd Ed. make sure all unwanted units cancel Factor-label method: Using conversion factors to convert a quantity in one unit to a quantity in another unit. units are treated like numbers To convert 130 lb into kilograms: 130 lbx conversion factor = ? kg original quantity desired quantity

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Measurements Conversion Factors 29 Smith. General Organic & Biolocial Chemistry 2nd Ed. or 2.21 lb 1 kg 2.21 lb 1 kg 2.21 lb 1 kg 2.21 lb 130 lbx =59 kg Answer 2 sig. figures The bottom conversion factor has the original unit in the denominator. The unwanted unit lb cancels. The desired unit kg does not cancel.

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Measurements Temperature 30 Smith. General Organic & Biolocial Chemistry 2nd Ed. Temperature is a measure of how hot or cold an object is. 1.Degrees Fahrenheit ( o F) 2.Degrees Celsius ( o C) 3.Kelvin (K) Three temperature scales are used: To convert from o C to o F: To convert from o F to o C: o F = 1.8( o C) + 32 o C = o F 32 1.8 o C = o F 32 1.8 To convert from o C to K: K = o C + 273 o C = K 273 To convert from K to o C:

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Measurements Temperature 31 Smith. General Organic & Biolocial Chemistry 2nd Ed.

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Measurements Density 32 Smith. General Organic & Biolocial Chemistry 2nd Ed. density= mass (g) volume (mL or cc) Density: A physical property that relates the mass of a substance to its volume. To convert volume (mL) to mass (g): To convert mass (g) to volume (mL): mLx g =g gx g = density inverse of density

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Measurements Specific Gravity 33 Smith. General Organic & Biolocial Chemistry 2nd Ed. Specific gravity: A quantity that compares the density of a substance with the density of water at the same temperature. specific gravity= density of a substance (g/mL) density of water (g/mL) The units of the numerator (g/mL) cancel the units of the denominator (g/mL). The specific gravity of a substance is equal to its density, but contains no units.