2. Inorganic Chemistry. 1. Organic Chemistry. General and Analytical Chemistry. Page 1. Lecture 1. Chemistry is a branch of physical science that

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1 Lecture 1 General and Analytical Chemistry Chemistry is a branch of physical science that studies the composition, structure, properties and change of matter. It is chiefly concerned with atoms and molecules and their interactions and transformations. 1. Organic Chemistry It investigates matter that contains organic carbon. Organic chemists study the structure, function, synthesis, and identity of organic carbon compounds Useful in petroleum industry, pharmaceuticals, polymers industry 2. Inorganic Chemistry It is involved in studying of matter that does NOT contain organic carbon. Inorganic chemists study the structure, function, synthesis, and identity of various compounds Polymers, Metallurgy Page 1

2 Biochemistry is the study of chemistry in living things Cross between biology and chemistry Pharmaceuticals and genetics 3. Biochemistry 4. Physical Chemistry Physical HONK if you passed p-chem chemistry is the physics of chemistry the forces of matter Much of p-chem is computational It develops theoretical ideas for new compounds 5. Analytical Chemistry Analytical chemistry is the study of high precision measurement Find composition and identity of chemicals Forensics, quality control, medical tests Chemistry uses in communication of ideas and concepts its own language known as chemical nomenclature. International body that sets down the accepted conventions, terms and notation International Union of Pure and Applied Chemistry (IUPAC). Page 2

3 The Language of Chemistry CHEMICAL - pure substances that cannot be decomposed by ordinary means to other substances. The Language of Chemistry CHEMICAL - is an entity consisting of two or more different atoms which associate via chemical bonds Aluminum Sodium Bromine The Language of Chemistry The elements, their names, and symbols are given on the PERIODIC TABLE How many elements are there? 118 elements have been identified 82 elements occur naturally on Earth Examples: gold, aluminum, lead, oxygen, carbon 36 elements have been created by scientists Examples: technetium, americium, seaborgium The Periodic Table Dmitri Mendeleev ( ) Page 3

4 Maria Skłodowska-Curie ( ) Discovered two new elements polonium and radium. She shared the 1903 Nobel Prize in Physics with her husband Pierre Curie and with physicist Henri Becquerel. She won the 1911 Nobel Prize in Chemistry. She is the only person who won this Prize in two different sciences. Glenn Seaborg ( ) Discovered 8 new elements. Only living person for whom an element was named. Nobel prize in Chemistry in 1951 Names of chemical elements originate from: A) country names B) continents C) names of Gods Chemical analysis can be distinguished in two areas qualitative and quantitative. Both types are based on the observations. Page 4

5 Types of Observations and Measurements We collect QUALITATIVE data making observations of reactions changes in color or physical state of investigated solute. We make QUANTITATIVE MEASUREMENTS, which involve comparing a quantity with a standard unit. This procedure is connecting with numbers. Table. 1. Qualitative vs. Quantitative observation Number Observation 1 The temperature of this room is 25 C. 2 It is comfortably warm in this room. 3 Most people have removed their coats. 4 The building is 25 stories high. 5 It is a very tall building. Qualitative or Quantitative Qualitative observations Quantitative measurement Fog caused by dry ice Soda Oxidation state Page 5

6 Some Tools for Measurement Which tool(s) would you use to measure: A. temperature B. volume C. time D. weight Match L) length M) mass V) volume M A. A bag of tomatoes is 4.6 kg. L B. A person is 2.0 m tall. M C. A medication contains 0.50 g Aspirin. V D. A bottle contains 1.5 L of water. Stating a Measurement In every measurement (variable) there is a Number followed by a Unit from a measuring device Standards of Measurement When we measure, we use a measuring tool to compare some dimension of an object to a standard. For example, at one time the standard for length was the king s foot or his elbow. What are some problems with this standard? The number should be as precise as the measurement! Page 6

7 UNITS OF MEASUREMENT units based on the metric system Length Mass Volume Time Temperature Meter, m Kilogram, kg m 3, Liter, L Seconds, s kelvins, K Celsius degrees, C Metric Prefixes Kilo- means 1000 of that unit 1 kilometer (km) = 1000 meters (m) Centi- means 1/100 of that unit 1 meter (m) = 100 centimeters (cm) 1 dollar = 100 cents Milli- means 1/1000 of that unit 1 Liter (L) = 1000 milliliters (ml) Page 7

8 Metric Prefixes 1 attogram = mass of 1 molecule of polystyrene 1 femto gram = mass of 1 DNA molecule 1 pico gram = mass of phosphorus used to dope 1 g of silicon 1 ng = mass of single ferrite particle for use in a computer floppy disc 1 g = mass of ink in a full stop 1 mg= mass of ink on a banknote 1 cg = mass of nicotine absorbed from single cigarette 1 dg = mass of the active component within 1 aspirin tablet 1g = mass of a single lentil 1 Mg = mass of a baby elephant 1 Gg = mass of a large crane 1 Tg = mass of a mountain Metric Prefixes m = 1 a) mm b) km c) dm g = 1 a) mg b) kg c) dg L = 1 a) ml b) cl c) dl m = 1 a) mm b) cm c) dm Page 8

9 Units of Length? kilometer (km) = 500 meters (m) 2.5 meter (m) =? centimeters (cm) 1 centimeter (cm) =? millimeter (mm) 1 nanometer (nm) = 1.0 x 10-9 meter O H distance = 9.4 x m 9.4 x 10-9 cm nm Select the unit you would use to measure 1. Your height a) millimeters b) meters c) kilometers 2. Your mass a) milligrams b) grams c) kilograms 3. The distance between two cities a) millimeters b) meters c) kilometers 4. The width of an artery a) millimeters b) meters c) kilometers How to convert various units. Steps to Problem Solving 1. Write down the given amount. Don t forget the units! 2. Multiply by a fraction. 3. Use the fraction as a conversion factor. Determine if the top or the bottom should be the same unit as the given so that it will cancel. 4. Put a unit on the opposite side that will be the new unit. If you don t know a conversion between those units directly, use one that you do know that is a step toward the one you want at the end. 5. Insert the numbers on the conversion so that the top and the bottom amounts are EQUAL, but in different units. 6. Multiply and divide the units (Cancel). 7. If the units are not the ones you want for your answer, make more conversions until you reach that point. 8. Multiply and divide the numbers. Don t forget Please Excuse My Dear Aunt Sally! (order of operations) Write conversion factors that relate each of the following pairs of units: 1. Liters and ml 2. Hours and minutes 3. Meters and kilometers Page 9

10 How many minutes are in 2.5 hours? Conversion factor 2.5 hr x 60 min = 150 min 1 hr cancel By using dimensional analysis / factor-label method, the UNITS ensure that you have the conversion right side up, and the UNITS are calculated as well as the numbers! A rattlesnake is 2.44 m long. How long is the snake in cm? a) 2440 cm b) 244 cm c) 24.4 cm Solution A rattlesnake is 2.44 m long. How long is the snake in cm? b) 244 cm 2.44 m x 100 cm = 244 cm 1 m Wait a minute! What is wrong with the following setup? 2.44 m x 1m 100cm Page 10

11 How many seconds are in 1.4 days? Unit plan: days hr min seconds 24 hr 1.4 days.??? 1 day Wait a minute! What is wrong with the following setup? 1.4 day x 1 day x 60 min x 60 sec 24 hr 1 hr 1 min Equalities Customary and Metric Systems State the same measurement in two different units length 10.0 in cm Page 11

12 Common tools for volume determination one tablespoon is approximately 15 ml, teaspoon has the volume of 5 ml Glass volume Volume in ml No of spoons 1/4 62 ml 4 1/2 125 ml 8 2/3 166 ml 10 spoons & 2 tea spoons 3/4 187 ml ml 16 What are some U.S. units that are used to measure each of the following? A. length B. volume C. weight D. temperature English and Metric Conversions Conversion factors for different systems of units If you know ONE conversion factor for each type of measurement, you can convert anything! Page 12

13 Conversion Factors Fractions in which the numerator and denominator are EQUAL quantities expressed in different units Example: 1 in. = 2.54 cm Factors: 1 in. and 2.54 cm 2.54 cm 1 in. Conversion factors 2 Mass: 454 grams = 1 pound Factors: 1 lb. and 454 lb 454 g 1 g Length: cm = 1 yd Factors: 1 yd and cm cm 1 yd Length: cm = 1 ft Factors: 1 ft and cm 30.48cm 1 ft Volume: Conversion factors L = 1 quart Factors: 1 qt. and L L 1 qt. Volume: L = 1 gal Factors: 1 gal and L L 1 gal. Sample Problem You have $7.25 in your pocket in quarters. How many quarters do you have? 7.25 dollars 4 quarters X 1 dollar = 29 quarters An introduction to chemistry by Mark Bishop, Chiral Publishing Company Page 13

14 You Try This One! If Jacob stands on Spencer s shoulders, they are two and a half yards high. How many m is that? An adult human has 4.65 L of blood. How many gallons of blood is that? Unit plan: L qt gal Equalities: 1 quart = L 1 gallon = 4 quarts Your Setup: Dealing with Two Units Dealing with Two Units If your pace on a treadmill is 65 meters per minute, how many seconds will it take for you to walk a distance of 8450 feet? If your pace on a treadmill is 65 meters per minute, how many seconds will it take for you to walk a distance of 8450 feet? m 1 ft = 8450 ft x m = m 65 m = m = 2374 s 60 s x s Page 14

15 What about Square and Cubic units? Use the conversion factors you already know, but when you square or cube the unit, don t forget to square or cube the number also! Best way: Square or cube the ENITRE conversion factor Example: Convert 4.3 cm 3 to mm 3 ( ) = 4.3 cm mm cm 3 10 mm 3 1 cm 1 3 cm 3 A Nalgene water bottle holds 1000 cm 3 of dihydrogen monoxide (DHMO). How many cubic decimeters is that? = 4300 mm 3 Solution 1000 cm 3 1 dm 3 ( ) = 1 dm 3 10 cm Temperature Scales Fahrenheit Celsius Kelvin So, a dm 3 is the same as a Liter! A cm 3 is the same as a milliliter. Gabriel Fahrenheit Lord Kelvin (William Thomson) Anders Celsius Page 15

16 Boiling point of water Temperature Scales Freezing point of water Fahrenheit 212 F 180 F 32 F Celsius 100 C 100 C 0 C Notice that 1 kelvin = 1 degree of Celsius Kelvin 373 K 100 K 273 K Calculations Using Temperature Generally require temp s in kelvins T (K) = t ( C) Body temp = 37 C = 310 K Liquid nitrogen = -196 C = 77 K Fahrenheit Formula Honors Only Celsius Formula Honors Only 180 F = 9 F = 1.8 F 100 C 5 C 1 C Zero point: 0 C = 32 F F = 9/5 C + 32 Rearrange to find T C F = 9/5 C + 32 F - 32 = 9/5 C ( ) F - 32 = 9/5 C 9/5 9/5 ( F - 32) * 5/9 = C Page 16

17 Temperature Conversions Honors Only A person with hypothermia has a body temperature of 29.1 C. What is the body temperature in F? F = 9/5 (29.1 C) + 32 = = 84.4 F Honors Only The normal temperature of a chickadee is F. What is that temperature in C? 1) 73.8 C 2) 58.8 C 3) 41.0 C Honors Only Pizza is baked at 455 F. What is that in C? 1) 437 C 2) 235 C 3) 221 C Scientific approach 1. Observations gathering information and collecting data 2. Experiments checking the observations 3. Hypothesis tentative explanation of observation 4. Theory explains why observations, hypothesis apply. 5. Laws describe how nature works Page 17

18 Scientific Method 1. State the problem clearly. 2. Gather information. 3. Form a. 4. Test the hypothesis. 5. Evaluate the data to form a conclusion. If the conclusion is valid, then it becomes a theory. If the theory is found to be true over along period of time (usually 20+ years) with no counter examples, it may be considered a law. 6. Share the results. Example of scientific approach Observations: The colour intensity of solution changes when the concentration of the solute in the solution varies Hypothesis: The concentration of the solute affects its intensity (absorbance) Experiment: Checking the influence of the solute concentration on the colour intensity (MEASUREMENT) Thesis: There are relationships between solute concentration and its absorbance Law: Lambert Beer Scientific approach to test 1. Observations not all compounds dissolve in water 2.Experiments How to present experiment results 3. Hypothesis 4. Theories Page 18

19 What is Scientific Notation? Scientific notation is a way of expressing really big numbers or really small numbers. For very large and very small numbers, scientific notation is more concise. Scientific notation consists of two parts: A number between 1 and 10 A power of 10 N x 10 m To change standard form to scientific notation Place the decimal point so that there is one non-zero digit to the left of the decimal point. Count the number of decimal places the decimal point has moved from the original number. This will be the exponent on the 10. If the original number was less than 1, then the exponent is negative. If the original number was greater than 1, then the exponent is positive. Examples Given: 300, Use: 3.0 (moved 8 places) Answer: 3 x 10 8 Given: Use: 7 (moved 4 places) Answer: 7.0 x 10-4 Page 19

20 Given: Answer: Given: To change scientific notation to standard form Simply move the decimal point to the right for positive exponent 10. Move the decimal point to the left for negative exponent 10. (Use zeros to fill in places.) Answer:. Example Given: x 10 6 Answer: (moved 6 places to the right) Given: x 10-4 Answer: (moved 4 places Express these numbers in standard form: 1) 2.40 x ) 3.89 x ) 4.18 x ) 1 x 10-3 to the left) Page 20

21 Presenting data Acid volume = 52,9 ml or 52,90 ml or 52,900 ml Significant Figures The numbers reported in a measurement are limited by the measuring tool Significant figures in a measurement include the known digits plus one estimated digit Reading a Meterstick. l I.... I 3....I.... I 4.. cm First digit (known) = 2 2.?? cm Second digit (known) = ? cm Third digit (estimated) between Length reported = 2.75 cm or 2.76 cm or 2.77 cm Known + Estimated Digits In 2.76 cm Known digits 2 and 7 are 100% certain The third digit 6 is estimated (uncertain) In the reported length, all three digits (2.76 cm) are significant including the estimated one Page 21

22 Zero as a Measured Number. l I.... I 9....I.... I 10.. cm. l I.... I I.... I 5.. cm What is the length of the green line? 1) 9.6 cm 2) 9.62 cm 3) 9.63 cm How does your answer compare with your neighbor s answer? Why or why not? What is the length of the line? First digit Second digit Last (estimated) digit is 5.?? cm 5.0? cm 5.00 cm Always estimate ONE place past the smallest mark!? Page 22

23 DENSITY - an important and useful physical property Density mass (g) volume (cm3) Mercury Platinum 13.6 g/cm g/cm 3 Aluminum 2.7 g/cm 3 Density is an INTENSIVE property of matter. does NOT depend on quantity of matter. But depends on temperature and pressure Contrast with EXTENSIVE depends on quantity of matter. mass and volume. DENSITY Styrofoam Brick Problem A piece of copper has a mass of g. It is 9.36 cm long, 7.23 cm wide, and 0.95 mm thick. Calculate density (g/cm 3 ). Density mass (g) volume (cm3) Strategy 1. Get dimensions in common units. 2. Calculate volume in cubic centimeters. 3. Calculate the density. Page 23

24 SOLUTION 1. Get dimensions in common units mm 1cm 10 mm = cm 2. Calculate volume in cubic centimeters. PROBLEM: Mercury (Hg) has a density of 13.6 g/cm 3. What is the mass of 95 ml of Hg in grams? In pounds? (9.36 cm)(7.23 cm)(0.095 cm) = 6.4 cm 3 Note only 2 significant figures in the answer! 3. Calculate the density g = 9.0 g / cm3 6.4 cm 3 PROBLEM: Mercury (Hg) has a density of 13.6 g/cm 3. What is the mass of 95 ml of Hg? PROBLEM: Mercury (Hg) has a density of 13.6 g/cm 3. What is the mass of 95 ml of Hg? First, note that 1 cm 3 = 1 ml 1. Convert volume to mass Strategy 1. Use density to calc. mass (g) from volume. 2. Convert mass (g) to mass (lb) Need to know conversion factor = 454 g / 1 lb 95 cm g cm 3 = 1.3 x 10 3 g 2. Convert mass (g) to mass (lb) 1.3 x 10 3 g 1 lb 454 g = 2.8 lb Page 24

25 Solution Osmium is a very dense metal. What is its density in g/cm 3 if g of the metal occupies a volume of 2.22cm 3? 1) 2.25 g/cm 3 2) 22.5 g/cm 3 3) 111 g/cm 3 2) Placing the mass and volume of the osmium metal into the density setup, we obtain ρ = mass volume = g 2.22 cm 3 = = g/cm 3 = 22.5 g/cm 3 Volume Displacement A solid displaces a matching volume of water when the solid is placed in water. What is the density (g/cm 3 ) of 48 g of a metal if the metal raises the level of water in a graduated cylinder from 25 ml to 33 ml? 1) 0.2 g/ cm 3 2) 6 g/cm 3 3) 252 g/cm 3 25 ml 33 ml 25 ml 33 ml Page 25

26 Which diagram represents the liquid layers in the cylinder? (K) Karo syrup (ρ = 1.4 g/ml), (V) vegetable oil (ρ = 0.91 g/ml,) (W) water (ρ= 1.0 g/ml) 1) 2) 3) The density of octane, a component of gasoline, is g/ml. What is the mass, in kg, of 875 ml of octane? 1) kg V W K W K V K V W 2) 614 kg 3) 1.25 kg If blood has a density of 1.05 g/ml, how many liters of blood are donated if 575 g of blood are given? 1) L 2) 1.25 L 3) 1.83 L A group of students collected 125 empty aluminum cans to take to the recycling center. If 21 cans make 1.0 pound of aluminum, how many liters of aluminum (ρ =2.70 g/cm 3 ) are obtained from the cans? 1) 1.0 L 2) 2.0 L 3) 4.0 L Page 26

27 Book to be used during General and Analytical Chemistry course 1. J.E. Brady, F. Senese: Chemistry Matter and its Changes, 4th ed. Wiley J. Brady, N. Jespersen, A. Hyslop Chemistry, 7 ed., International student version. Wiley, D. A. Skoog, F. J. Holler, S. R. Crouch - Principles of instrumental analysis. - 6th ed., Thomson, Brooks/Cole, J. Crowe. T. Bradshaw, P. Monk, Chemistry for the Biosciences. The essential concepts., Oxford University Press, D. A. Skoog, D. M. West, F. J. Holler, S. R. Crouch; Analytical Chemistry. An Introduction, 7 th ed., J. A. Beran; Laboratory Manual for Principles of General Chemistry 7. P. Monk, Physical Chemistry, Wiley 2004 Page 27