Lecture 2: Finish Ch. 1; Appendices 1&2.
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1 Lecture 2: Finish Ch. 1; Appendices 1&2. Before Today: Read syllabus, Appendix 1 & 2 (see details) & Ch. 1 Do the Initial Assessment on ALEKS by 11 PM. For Monday: Get your Clicker and register its ID on Catalyst. (same clicker can be used for all your courses). Work examples from Ch. 1 notes (web) on your own. Read Ch. 2 (see Reading schedule in Syllabus) Start working toward Objective 1 on ALEKS, due next Friday at 9 PM (8:55 to allow clock error). and work Ch. 1 example problems Drs. Phil Reid and Andrea Carroll will lecture on Monday.
2 Oceanography Chemistry as the Central Science Atmospheric Sciences Physics Medicine Economics Governments Chemistry Engineering Geology Anthropology Biology Astronomy Politics People
3 The next BIG THING in 1997: Nanotechnology The next BIG THING now: Molecular Engineering
4 Poly(Vinyl Chloride) (PVC) and Teflon H H H H H H H H H H C C C C C C C C C C H Cl Vinyl chloride H Cl H Cl H Cl H Cl n PVC F F F F F F F F F F C C C C C C C C C C F F F F F F F F F F n Tetrafluoroethylene Teflon
5 Figure 1.2 Paper: A Polymer called Cellulose The Polymer cellulose, which consists of B-D-glucose monomers. Proteins, DNAs and RNAs are other biological polymers.
6 The Scientific Method Information or data is gathered by careful observation of the phenomenon being studied. On the basis of that information a preliminary hypothesis is formed. A series of experiments is devised to test the predictive power of the hypothesis.
7 K (s) + H 2 O (l) KOH (aq) + H 2(g) Na (s) + H 2 O (l) NaOH (aq) + H 2(g) etc.
8 The Periodic Table of the Elements Most Probable Oxidation State +1 0 H _ He Li Be B C N O F Ne Na Mg Al Si P S Cl Ar K Ca Sc Ti V CrMn Fe Co Ni Cu Zn Ga Ge As Se Br Kr Rb Cs Sr Ba Y La Zr Hf Nb Ta Mo Tc W Re Ru Os Rh Ir Pd Pt Ag Au Cd Hg In Tl Sn Pb Sb Bi Te Po I At Xe Rn Fr Ra Ac Rf Db Sg Bh Hs Mt Ds Ce Th Pr Nd PmSmEu Gd Tb Dy Ho Er TmYb Lu Pa U Np Pu AmCmBk Cf Es FmMd No Lr
9 The Scientific Method (cont.) On the basis of the experimental tests, the hypothesis may be (a) Accepted as scientific law or theory. (b) Modified so that all results are adequately explained. (c) Discarded. When accepted, we also often devise/test new hypotheses to explain why it is true. Laws sometimes later found to apply only in specified cases.
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11 STATES OF MATTER - and The World around US SOLID - The Earth LIQUID - Water GAS - The Atmosphere
12 Energy Involved in Phase Changes Gas Liberates Energy Boiling Condensation Liquid Melting Freezing Requires Energy Solid
13 Definitions Energy - The capacity to do work! Potential Energy - The energy due to the position of the object(s) and the forces acting on it by other objects (gravity, Coulomb s law, chemical bonding forces, etc.) Kinetic Energy - The energy due to the motion of the object(s): ½ mass x velocity 2
14 All Measured Quantities Consist of a Number and a Unit
15 . Table A2.1
16 Derived SI Units Quantity Definition of Quantity SI unit Area Length squared m 2 Volume Length cubed m 3 Density Mass per unit volume kg/m 3 Speed Distance traveled per unit time m/s Acceleration Speed changed per unit time m/s 2 Force Mass times acceleration of object kg * m/s 2 ( = Newton, N) Pressure Force per unit area N/(m 2 ) ( = pascal, Pa) Energy Force times distance traveled kg * m 2 /s 2 ( = N*m = joule, J)
17 Units Used in Calculations Length : A car is 12 feet long, not 12 or 12 long! A person is 6 feet tall, not 6 or 6 tall! Area : A carpet measuring 3 feet (ft) by 4 ft has an area of: (3 ft)x(4 ft) = ( 3 x 4 )( ft x ft ) = 12 ft 2 Speed and Distance : A car traveling 350 miles (mi) in 7 hours (hr) has a speed of: 350 mi / 7 hr = 50 mi / hr In 3 hours the car travels: 3 hr x 50 mi / hr = 150 mi
18 (this is Table A2.2 in your book.)
19 (The back cover of your book has a similar table. Use it for HW.)
20 Conversion Factors : Unity Factors - I Equivalent factors can be turned into conversion factors by dividing one side into the other! (See Table back cover) 1 mile = 5280 ft or 1 = 1 mile / 5280 ft = 5280 ft / 1 mi 1 in = 2.54 cm or 1 = 1 in / 2.54 cm = 2.54 cm / 1 in In converting one set of units for another, the one desired is on top in the conversion factor, and the old one is canceled out! Example: Convert 29,141 ft into miles! 29,141 ft x = mi 1 mi 5280 ft
21 Conversion Factors - II 1.61 km = 1 mi or 1 = Convert miles into kilometers: Conversions in the metric system are easy, as 1 km = 1000 m and 1 meter (m) = 100 centimeters (cm) and 1 cm = 10 millimeters (mm). Ex.: Convert 8.89 km into m and cm:
22 Conversion Factors - II 1.61 km = 1 mi or 1 = 1.61 km / 1 mi Convert miles into kilometers: mi x (1.61 km / mi) = 8.89 km Conversions in the metric system are easy, as 1 km = 1000 m and 1 meter (m) = 100 centimeters(cm) and 1 cm = 10 millimeters(mm) Ex.: Convert 8.89 km into m and cm! 8.89 km x (1000 m / 1 km) = 8,890 m 8,890 m x (100 cm / m) = 889,000 cm
23 Conversion Factors - III Multiple conversion factors! Convert 3.56 lbs/hr into units of milligrams/sec!
24 Conversion Factors - III Multiple conversion factors! Convert 3.56 lbs/hr into units of milligrams/sec lbs 1 kg 1000g 1000mg 1 hr 1 min hr x x x x x lbs 1 kg 1 g 60 min 60 sec = = 448 mg/ sec
25 Conversion Factors - III Multiple conversion factors! Convert 3.56 lbs/hr into units of milligrams/sec lbs 1 kg 1000g 1000mg 1 hr 1 min hr x x x x x lbs 1 kg 1 g 60 min 60 sec = = 448 mg/ sec
26 Conversion Factors - IV metric volume to liters 1.35 x 10 9 km 3 = volume of world s oceans. 1 Liter = 1 L = 1 dm 3 How many liters of water are in the oceans? conversion factors: 1 km = 1000 m 1 L = 1 dm 3 = 10-3 m 3 or 1000 L = 1 m 3
27 Conversion Factors - IV metric volume to liters 1.35 x 10 9 km 3 = volume of world s oceans. 1 Liter = 1 L = 1 dm 3 How many liters of water are in the oceans? conversion factors: 1 km = 1000 m 1 L = 1 dm 3 = 10-3 m 3 or 1000 L = 1 m x 10 9 km 3 x (10 3 m/1 km ) 3 x ( 10 3 L/m 3 ) = 1.35 x liters
28 Density Density is defined as mass per unit volume: mass Density = = ρ volume You can use it like a conversion factor ratio: Since density of lead =11.4 g/ cm 3, then 11.4 g lead = 1.00 cm 3 lead 11.4 g lead / (1.00 cm 3 lead) = 1
29 Conversion Factors - V Calculate the mass of 1.00 ft 3 of lead (density of lead =11.4g /ml = 11.4 g/ cm 3 )
30 Conversion Factors - Calculate the mass of 1.00 ft 3 V of lead (density of lead =11.4g /ml = 11.4 g / cm 3 ) 1.00 ft 3 x (12 in/ft) 3 x (2.54 cm/in) 3 = 28,300 cm x 10 4 cm 3 Pb x (11.4 g Pb /cm 3 Pb ) = 323,000 g Pb Ans. = 3.23 x 10 5 g = 323 kg
31 Conversion Factors - chemical 2H 2 (g) + O 2 (g) 2 H 2 O (g) + Energy 2 O atoms 1 O 2 molecule reacts 1 O 2 molecule 2 H 2 O molecules produced
32 How to Solve Chemistry Problems 1) Problem: State all of the information needed to solve the problem. Write down the knowns and unknowns. Include as known any definitions or laws (Both give equations!) that might mathematically relate the values. 2) Plan: What steps are needed to find the solution? Develop a roadmap by working backwards. Look for additional information / laws as needed. 3) Solution: Do the algebraic manipulations & calculations in the order planned. Keep units! 4) Check: Is the result what you expect or at least in the same order of magnitude! Does it have the right units?
33 An Example Problem! The Volume of an irregularly shaped solid can be determined from the volume of water it displaces. A graduated cylinder contains ml water. When a small piece of Pyrite, an ore of iron, is submerged in the water, the volume increases to ml. What is the volume of the piece of Pyrite in cm 3 and in liters.
34 An Example Problem! The Volume of an irregularly shaped solid can be determined from the volume of water it displaces. A graduated cylinder contains ml water. When a small piece of Pyrite, an ore of iron, is submerged in the water, the volume increases to ml. What is the volume of the piece of Pyrite in cm 3 and in liters. Vol (ml) = ml ml = 70.8 ml Vol (cm 3 ) = 70.8 ml x (1 cm 3 / 1 ml) = 70.8 cm 3 Vol (liters) = 70.8 ml x (10-3 liters / ml) = 7.08 x 10-2 liters
35 Archimedes Principle Problem Problem: Calculate the density of an irregularly shaped metal object that has a mass of g if when it is placed into a 2.00 liter graduated cylinder containing ml of water, the final volume of the water in the cylinder is 1, ml? Plan: Calculate the volume from the different volume readings, and calculate the density using this with the mass that was given, and definition: density = mass / volume. Solution: Volume = Density = } ΔV
36 Archimedes Principle Problem Problem: Calculate the density of an irregularly shaped metal object that has a mass of g if when it is placed into a 2.00 liter graduated cylinder containing ml of water, the final volume of the water in the cylinder is 1, ml? Plan: Calculate the volume from the different volume readings, and calculate the density using this with the mass that was given, and definition: density = mass / volume. Solution: Volume = 1, ml ml = ml Density = = = g / ml mass g volume ml
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38 A Sample Problem - I International computer communications will soon be carried by optical fibers in cables laid along the ocean floor. If one strand of optical fiber weighs 1.19 x 10-3 lbs/m, what is the total mass (in kg) of a cable made of six strands of optical fiber, each long enough to link New York and Paris? (8.85 x 10 3 km). Mass (kg) of Cable Length (km) of Fiber 1 km = 10 3 m Length (m) of Fiber lb = 1 kg 1m = 1.19 x 10-3 lb 6 fibers = 1 cable Mass (lb) of Fiber Mass (lb) of Cable
39 Sample Problem - II Length (m) of Fiber = 8.85 x 10 3 km Mass (lb) of Fiber = Mass (lb) of cable = Mass (kg) of cable =
40 Sample Problem - II Length (m) of Fiber = 8.85 x 10 3 km x 10 3 m / km = 8.85 x 10 6 m Mass (lb) of Fiber = 8.85 x 10 6 m x (1.19 x 10-3 lb /m) = 1.05 x 10 4 lb Mass (lb) of cable = 1.05 x 10 4 lb / fiber x (6 fibers/cable) = 6.30 x 10 4 lb / cable Mass (kg) of cable = 6.30 x 10 4 lb /cable x (1kg / lb) = 2.86 x 10 4 kg / cable
41 A Problem on Density - I Lithium (Li) is a soft, gray solid that has the lowest density of any metal. If a slab of Li weighs 1.49 x 10 3 mg and has sides that measure 20.9 mm by 11.1 mm by 12.0 mm, what is the density of Li in g/ cm 3? Lengths (mm) of sides Mass (mg) of Li Mass (g) of Li Volume (cm 3 ) Lengths (cm) of sides Density (g/cm 3 ) of Li
42 Density Problem - II Mass (g) of Li = 1.49 x 10 3 mg Length (cm) of one side = Similarly, the other side lengths are 1.11 cm and 1.20 cm Volume (cm 3 ) = mass Density of Li = = volume
43 Density Problem - II Mass (g) of Li = 1.49 x g mg x = 1.49 g 10 3 mg Length (cm) of one side = 20.9 mm x 1cm / 10 mm = 2.09 cm Similarly, the other side lengths are 1.11 cm and 1.20 cm Volume (cm 3 ) = 2.09 cm x 1.11 cm x 1.20 cm = 2.78 cm g Density of Li = = g/cm cm 3
44 Difference between Mass & Weight (except on earth): Mass - The quantity of matter an object contains kilogram - ( kg ) - the SI base unit of mass, is a platinum - iridium cylinder kept in Paris as a standard! Weight - depends upon an object s mass and the strength of the gravitational field pulling on it.
45 Temperature Scales and Interconversions Kelvin ( K ) - The Absolute temperature scale begins at absolute zero and only has positive values. Celsius ( o C) -The temperature scale used by science, formally called centigrade and most commonly used scale around the world, water freezes at 0 o C, and boils at 100 o C. Fahrenheit ( o F) -Commonly used scale in America for our weather reports, water freezes at 32 o F, and boils at 212 o F.
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47 Temperature Conversions T (in K) = T (in 0 C) T (in 0 C) = T (in K) T (in 0 F) = 9/5 T (in 0 C) + 32 T (in 0 C) = [ T (in 0 F) - 32] 5/9
48 Temperature Conversions - I The boiling point of Liquid Nitrogen is C. What is the temperature in Kelvin and degrees Fahrenheit? T (in K) = T (in 0 C) T (in K) = T (in 0 F) = 9/5 T (in 0 C) + 32 T (in 0 F) =
49 Temperature Conversions - I The boiling point of Liquid Nitrogen is C, what is the temperature in Kelvin and degrees Fahrenheit? T (in K) = T (in 0 C) T (in K) = C = K = 77 K T (in 0 F) = 9/5 T (in 0 C) + 32 T (in 0 F) = 9/5 ( C) + 32 = F
50 Temperature Conversions - II The normal body temperature is F, what is it in degrees Celsius and Kelvin? T (in 0 C) = [ T (in 0 F) - 32] 5/9 T (in 0 C) = T (in K) = T (in 0 C) T (in K) =
51 Temperature Conversions - II The normal body temperature is F, what is it in degrees Celsius and Kelvin? T (in 0 C) = [ T (in 0 F) - 32] 5/9 T (in 0 C) = [ F - 32] 5/9 = C T (in K) = T (in 0 C) T (in K) = C = K
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53 What is the boiling point of Pure water? A F B F C F D F E. None of the Above A B C D E
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55 Rules for Determining Which Digits Are Significant All digits are significant, except zeros that are used only to position the decimal point. 1. Make sure that the measured quantity has a decimal point. 2. Start at the left of the number and move right until you reach the first nonzero digit. 3. Count that digit and every digit to it s right as significant. Zeros that end a number and lie either after or before the decimal point are significant; thus ml has four significant figures, and L has four significant figures also. Numbers such as 5300 L are assumed to only have 2 significant figures. A terminal decimal point is often used to clarify the situation, but scientific notation is the best!
56 Examples of Significant Digits in Numbers Number - Sig digits Number - Sig digits L two x 10 7 nm six g four 5600 ng two kg two 87,000 L two L six 78,002.3 ng six g four g four 875,000 oz three x 10-6 L four 30,000 kg one oz five m 3 five kg six 23, lbs seven ml nine g three kg eight 1,470,000 L three 1,000,000,000 g one
57 Rules for Significant Figures in Answers 1. For multiplication and division. The number with the least certainty limits the certainty of the result. therefore, the answer contains the same number of significant figures as there are in the measurement with the fewest significant figures. Multiply the following numbers: 9.2 cm x 6.8 cm x cm = cm 3 = 23 cm 3 2. For addition and subtraction. The answer has the same number of decimal places as there are in the measurement with the fewest decimal places. Example, adding two volumes 83.5 ml ml = ml = ml Example subtracting two volumes: ml ml = ml = ml
58 Rules for Rounding off Numbers: 1. If the digit removed is more than 5, the preceding number increases by 1 : rounds to 5.38 if three significant figures are retained and to 5.4 if two significant figures are retained. 2. If the digit removed is less than 5, the preceding number is unchanged : rounds to if three significant figures are retained and to 0.24 if two significant figures are retained. 3.If the digit removed is 5, the preceding number increases by 1 if it is odd and remains unchanged if it is even: rounds to 17.8, but rounds to If the 5 is followed only by zeros, rule 3 is followed; if the 5 is followed by nonzeros, rule 1 is followed: rounds to 17.6, but rounds to Be sure to carry two or more additional significant figures through a multistep calculation and round off only the final answer. (In sample problems and follow-up problems, we round off intermediate steps of a calculation to show the correct number of significant figures.)
59 How many significant digits does the number have? A. 3 B. 4 C. 6 D. 7 E. None of the Above
60 Precision and Accuracy Errors in Scientific Measurements Precision - Refers to reproducibility or How close the measurements are to each other! Accuracy - Refers to how close a measurement is to the real value! Systematic error - produces values that are either all higher or all lower than the actual value. Random Error - in the absence of systematic error, produces some values that are higher and some that are lower than the actual value.
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62 SUMMARY 1. Chemistry, the central science! 2. Real-world chemistry problems are difficult but very, very important, and fun!! 4. Units conversions 5. Density 6. Problem solving approach 7. Sig. figs. and rounding 8. Accuracy vs. precision
63 Presentation about labs and lab safety by Dr. Andrea Carroll Lab Instructor (15 minutes)
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