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Matter

BIO. Medicine. Physics. CHEM. Engr. GEO. Law. Matter. What is Chemistry Study of the “Physical” Properties Matter (Form and Function) Study of How Matter Changes (Reactivity) Benefits of Chemistry Pharmaceuticals Enhanced food production (fertilizers, herbicides, etc...)

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Matter

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  1. BIO Medicine Physics CHEM Engr GEO Law Matter • What is Chemistry • Study of the “Physical” Properties Matter (Form and Function) • Study of How Matter Changes (Reactivity) • Benefits of Chemistry • Pharmaceuticals • Enhanced food production (fertilizers, herbicides, etc...) • Plastics and Polymers • Why Study Chemistry • Core requirement (?) • Central Science • Employment • Many fields also: environmental economics electronics agriculture politics etc... S.U. B.S. Chapt. 1.1

  2. Matter; A Review • Definition of Matter • anything that occupies space and has mass • States • gas (vapor); no fixed volume or shape, compressable • liquid; fixed volume no fixed shape, mostly incompressable • solid; fixed volume and shape, incompressable • Forms • Substances (pure or single); has a fixed composition and distinct properties. Most things encountered are mixtures of substances. • Properties • Physical Properties; can be measured without changing the substance, i.e., color, density, melting point, etc... • Chemical Properties; the way a substance changes (reacts), i.e., combustion Chapt. 1.1

  3. Matter; A Review • Changes • Physical - Changes in appearance but not identity, i.e., evaporation, melting (all changes of state) • Chemical - transformation into a different substance Chemical Changes Physical Changes burning melting C6H12O6 + 6O2 6CO2 + 6H2O H2O(s) H2O(l) chemical reactions sublimation NaOH + HCl H2O + NaCl H2O(s) H2O(g) corrosion dissolution 4Fe + 3O2 2 Fe2O3 H2O(l ) + NaCl(s) NaCl(aq) Chapt. 1.1

  4. Matter; A Review • Mixtures; combinations of substances • Mixture- • Homogeneous – • Heterogeneous - Chapt. 1.1

  5. Filter Matter; A Review • Filtration • Sand from Salt • Separating Mixtures using Physical Properties • How would you separate; Flow Everyday Examples; Auto Oil Filter Auto Air Filter Aquarium Water Filter Spaghetti Strainer Window Screens Registrar Chapt. 1.1

  6. Matter; A Review • Distillation • Water from Salt Water • Separating Mixtures using Physical Properties • How would you separate; NaCl(s) + H2O(l) NaCl(aq) Chapt. 1.1

  7. Matter; A Review • Chromatograpgy • Dyes from M&M’s • Separating Mixtures using Physical Properties • How would you separate; Before After Dyes Chapt. 1.1

  8. Matter; A Review • Salt and Sand Mixture Ink from Cabbage Juice • solubility and filtration chromatography • Water from Salt Water Iron and Gold Mixture • distillation magnetic properties • melting point differences • chem. reactivity (acids) • Iodine from Copper Chloride • solubility and filtration • Separating Mixtures using Physical Properties • How would you separate; Chapt. 1.1

  9. Matter; Elements and Compounds • Substances • Elements - substances which cannot be decomposed into simpler substances (see periodic table) • Compounds- substances which can be separated into two or more elements • Elements • 110 Known (periodic table to be revisited) • make up all matter and composed of “subatomic particles” • symbols used for abbreviations (from older or common names) • Compounds • Elements combined in a definite proportion by mass (law of definite proportion) • properties different than consititutent elements Water; example of mixtures, compound and elements? Chapt. 1.2

  10. Matter Matter No Yes Uniform ? Heterogeneous Mixture Homogeneous Can be separated by physical methods No Pure Substance Yes Decomposed ? Homogeneous Mixture (solution) No Yes Element Compound

  11. Matter; Measurement • Systems • Metric - base 10 • SI- international scientific system • mass Kilogram • length Meter • time Second • electric current Ampere • temperature Kelvin • light Candela • Amount Mole • Factor label method for conversions Chapt. 1.3

  12. Matter; Measurement • Prefixes Mega M 106 Kilo k 103 Deci d 10-1 Centi c 10-2 Milli m 10-3 Micro  10-6 Nano n 10-9 Chapt. 1.3

  13. Matter; Measurement Common Units: • Length and Mass • Length - unit of distance measured in meters • Mass - measures the amount of matter in an object in grams • Temperature • Kelvin • Celsius °C = 5/9 (°F -32) K = °C + 273.15 Chapt. 1.3

  14. Matter; Measurement Sample exercise: Ethylene glycol, the major ingredient in antifreeze, freezes at -11.5°C. What is the freezing point in a) K b) °F Chapt. 1.3

  15. Matter; Measurement Derived Units: • Volume • Length x length x length • measured in cm3, which is equal to mL Chapt. 1.3

  16. Matter; Measurement Derived Units: • Density • amount of mass per unit volume • measured in g/cm3, or g/mL Chapt. 1.3

  17. Matter; Measurement Sample exercise: A student needs 15.0 g of ethanol (ethyl alcohol) for an experiment. If the density of the alcohol is 0.789 g/mL, how many milliliters of alcohol are needed? Chapt. 1.3

  18. Matter; Uncertainty in Measurement • Precision and Accuracy • Precision - how closely individual measurements agree • Accuracy- how closely the measurements agree with the true value • Significant Figures • All measurements are inaccurate intrinsically • measured quantities are reported such that the last figure is uncertain Chapt. 1.4

  19. Matter; Uncertainty in Measurement Good Precision Poor Accuracy Good Precision Good Accuracy Poor Precision Poor Accuracy

  20. Matter; Uncertainty in Measurement • Determining Significant Figures • all non zero digits are significant • zeros between nonzero digits are significant • zeros to the left of first nonzero digit are not significant • zeros at the end of a number and to the right of a decimal point are significant • when a number ends in a zero but with no decimal point, the zero may or may not be signigicant (use scientific notation) Chapt. 1.4

  21. Matter; Uncertainty in Measurement • Determining Significant Figures 3.573 has 4 significant figures 0.073 has 2 significant figures 3.070 has 4 significant figures 0.003 has 1 significant figures - multiplication and division; result can have no more than the figure with the fewest significant figures - addition and subtraction; result can have the same number of decimal places as the term with the least number of decimal places Chapt. 1.4

  22. Matter; Uncertainty in Measurement Sample exercise: How many significant figures are in each of the following measurements? A) 3.549 g B) 2.3 x 104 cm C) 0.00134 m3 Chapt. 1.3

  23. Matter; Uncertainty in Measurement Sample exercise: How many significant figures are in each of the following measurements? A) 3.549 g 4 sig figs B) 2.3 x 104 cm C) 0.00134 m3 Chapt. 1.3

  24. Matter; Uncertainty in Measurement Sample exercise: How many significant figures are in each of the following measurements? A) 3.549 g 4 sig figs B) 2.3 x 104 cm 2 sig figs C) 0.00134 m3 Chapt. 1.3

  25. Matter; Uncertainty in Measurement Sample exercise: How many significant figures are in each of the following measurements? A) 3.549 g 4 sig figs B) 2.3 x 104 cm 2 sig figs C) 0.00134 m3 3 sig figs Chapt. 1.3

  26. Matter; Uncertainty in Measurement Sample exercise: There are exactly 1609.344 m in a mile. How many meters are in a distance of 1.35 mi? Chapt. 1.3

  27. Matter; Uncertainty in Measurement Sample exercise: There are exactly 1609.344 m in a mile. How many meters are in a distance of 1.35 mi? 1.35 mi = 1 mi x 1609.344 m Chapt. 1.3

  28. Matter; Uncertainty in Measurement Sample exercise: There are exactly 1609.344 m in a mile. How many meters are in a distance of 1.35 mi? 1.35 mi = 1 mi x 1609.344 m x = 2172.6144 m Chapt. 1.3

  29. Matter; Uncertainty in Measurement Sample exercise: There are exactly 1609.344 m in a mile. How many meters are in a distance of 1.35 mi? 1.35 mi = 1 mi x 1609.344 m 1.35 has 3 sig figs x = 2172.6144 m 1609.344 has 7 sig figs 1 is infinitely significant Chapt. 1.3

  30. Matter; Uncertainty in Measurement Sample exercise: There are exactly 1609.344 m in a mile. How many meters are in a distance of 1.35 mi? 1.35 mi = 1 mi x 1609.344 m 1.35 has 3 sig figs x = 2172.6144 m 1609.344 has 7 sig figs x = 2170 m 1 is infinitely significant Chapt. 1.3

  31. Dimensional Analysis • Use Units throughout the calculation (helps “guide” calculation. • Should always yield the proper units • Uses conversion factors • Example; How fast is 50 mph in in/sec.? 50 mi. 1 hour 5280 ft 12 in. = in 1 hour 3600 sec. 1 mi. 1 ft sec.

  32. Dimensional Analysis Sample exercise: By using a conversion factor from the back inside cover, determine the length in kilometers of a 500.0 mi automobile race. Chapt. 1.3

  33. Dimensional Analysis Sample exercise: By using a conversion factor from the back inside cover, determine the length in kilometers of a 500.0 mi automobile race. 500.0 mi Chapt. 1.3

  34. Dimensional Analysis Sample exercise: By using a conversion factor from the back inside cover, determine the length in kilometers of a 500.0 mi automobile race. 500.0 mi 1 km 0.62137 mi Chapt. 1.3

  35. Dimensional Analysis Sample exercise: By using a conversion factor from the back inside cover, determine the length in kilometers of a 500.0 mi automobile race. 500.0 mi 1 km = 804.674 km 0.62137 mi Chapt. 1.3

  36. Dimensional Analysis Sample exercise: By using a conversion factor from the back inside cover, determine the length in kilometers of a 500.0 mi automobile race. 500.0 mi 1 km = 804.674 km 0.62137 mi * answer can only have 4 sig figs; 804.7 km Chapt. 1.3

  37. Chapter One; Review • Matter: Chemical and Physical Changes • Elements and Compounds • Units of Measurement • Uncertainty and Significant Figures • Precision and Accuracy • “Factor Label” Method (Dimensional Analysis)

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