Keys to the castle copy these to your notes

1. Keys to the castle (copy these to your notes)

2. No Talking when Mr. B. is talking. (safer, saves time, just plain rude) Cell phones to off or at least vibrate. (no checking phones during class. I have calculators to lend and there is a clock on the wall.)

3. Items to frame a decision � People first (you are my priority) do no harm don't limit anyone�s options perception is reality in the end, only kindness matters

4. Pass out books and info sheets Intro activity - Write on the back of the info sheet two true things about you and one thing that you might wish to be true that isn�t. We will share these and try to guess which one isn�t true NB - Mistruths involving numbers are not fair. You can�t say that you have 4 cats when you only have three

5. I have been weightless I have been faster than the speed of sound I have been on the front page of the Boston Globe skiing off a cliff

6. Goals � What are you goals for the course (beyond just getting through it :-) When your goals are in line with the goals of the course we are working toward the same success.

7. Pass out intro letter and syllabus Collect info sheets

8. Chapter 1 guide

9. Safety in the Lab Review the safety items and their locations in the lab.

10. What is Chemistry? How does chemistry effect our lives?

11. What evidence suggests that climate change is happening?

12. Greenhouse effect / Ozone hole

13. Energy in the atmosphere converts O2 to O3 (still oxygen but does different things)

14. Make ozone here Tesla coil used as an energy source

15. And then humans came along�

16. This is a mechanism for how CFC�s break down ozone. The chlorine monoxide is further cycled back into raw chlorine when it gives up its oxygen to another chlorine monoxide to make two chlorines and one oxygen molecule. This is called a catalytic reaction.

17. Know, be able to answer the following -

19. What is Chemistry? If biology is the study of life, what is chemistry?

23. Where is chemistry relevant here?

25. Know, be able to answer the following -

26. Know the relevant overlapping vocabulary from this chapter for a brief vocab quiz at the start of tomorrow�s class. Don�t forget about the safety contract too.

27. How do we investigate Chemistry? What is the scientific method?

28. What could we investigate right now? Can you design an experiment that uses what we have on hand to perform a well supported investigation of? Water boiling temp? Magnet polarity? Relationship between mass and volume? Salt�s effect on water and vice versa?

29. Experimental Design What is a variable?

30. Lab Investigation Determine the relationship between the volume of a substance and its mass. Are they related? Directly, randomly? What happens to their organization when we plot the two variables against each other? Skills Measuring volume Measuring mass and scale operation Graphing

31. Lab investigation Water, NaCl, Lead, Tin. Volume vs. Mass Wearing the appropriate safety aprons, measure out 10 different volumes of a chemical and then take the mass of each volume. Record each data pair in a table that you can use to make a graph from. Switch to the next chemical and repeat

32. Lab investigation Water, NaCl, Lead, Tin. Mass vs. Volume Wearing the appropriate safety aprons, measure out 10 different masses of a chemical and then take the volume of each mass. Record each data pair in a table that you can use to make a graph from. Switch to the next chemical and repeat

33. HW for tomorrow Cover your book and have all paperwork signed to turn in

34. Journal How do you identify something and know that it is real? What can you do to make sure it is made of what it says it is? Have you ever been fooled, how and why?

35. Variability in Data What does it mean to be accurate?

36. Confidence, reproducibility and estimation Simply representing an observation as a number does not always tell the whole story behind it. Reporting an answer to many decimal places just because the calculator says so is not scientifically responsible Does it really matter if you say that it is 76.34532226 degrees out� Or that you are 14 and 245/365ths years old? Answers can not be more accurate than the numbers used to calculate them Stopped here for cp2Stopped here for cp2

37. Significant Figures (sig figs) The number of digits used in a measurement is called the number of significant figures (sig figs) in the measurement. The answer to a problem that is derived from two numbers is always expressed with the number of sig figs in the least accurate measurement

38. The base units of most variables

39. Scientific Notation

41. What is it? Why do we use it? How do you add and subtract in SN? How do you multiply and divide in SN? Scientific Notation

44. Units of measure Nan, until mom calls Dad, don�t heat kettle much

45. Unit Conversion � Converting from one unit or size to another Factor conversion method � uses a conversion factor (ratio of equivalent units = 1) to change from one unit system to another. Based on the following method Unit given | units wanted | units wanted --------------+-------------------+------------------ | units given |

46. Unit Conversion � Converting from one unit or size to another Also called dimensional analysis because it coverts one dimension into another. Cups to gallons, feet to miles, miles to kilometers. How about kilometers to feet? How many cups are in 6 gallons (set it up) If you live 2.75 miles from school how many feet away do you live? How many kilometers do you live away?

47. Factor conversion method

48. Factor conversion method

49. Additional problems Hw Hw

50. Sig figs and rounding to keep errors and numbers from getting inflated hwhw

51. Remember these? the base units of most variables

52. THE MOLE (holy moley) The craziest and hardest unit of them all! But once you get it, you�ll never understand how hard it once was. You need to remember a couple of things

53. The Mole Remember how to add and subtract numbers in scientific notation Remember how to multiply and divide numbers in scientific notation And how to use a calculator. GET ONE, while you�re at it, get one that does the Log (short for logarithm not a piece of wood) function.

54. Let�s review fractions What fraction is 6 of 8 slices of a pizza? What part is 6 of 8 slices of a pizza? What percentage is 6 of 8 slices of a pizza? Remember that �parts� always goes over the �whole�. More parts than the whole = bigger number, less parts than the whole = smaller

55. Keep fractions in mind, but consider what a mole is. A mole is a counting unit much like ream of paper Eggs = Donuts= Gum = Firewood= Soda cans= x 4 = 12 x 12 = Chemicals are measured in moles

56. Avogadro�s Number The mole is the number of atoms in 12 grams of carbon. (painstakingly determined in the lab) Since the most common form of carbon has 12 subatomic particles, this number was used to establish the conversion factor from atomic mass units to grams If 1 mole of carbon 12 has 12 subatomic parts and weighs 12 grams, and 1 of those 12 particles is a proton, then there are Avogadro�s number of protons in 1 gram

57. Yeah, so what�s a Mole? Simply, a mole of any chemical (or anything for that matter) is 6.02 x10^23 molecules or atoms that type of chemical 10^23 of anything is a huge number, let alone 6.02 times that number. 602,000,000,000,000,000,000,000.00 HexPent Qua Tril Bill MillThou

58. Mole 1 mole of paper = 1 mole of sand over Los Angeles = 1 mole of marshmallows = 1/sec for 5 billion people= But 1 mole of carbon = 1 mole of sodium chloride (table salt, NaCl)=

59. What are all those things in the Periodic table? Mass, Atomic #, Symbol, Name

61. 1 mole of anything is 6.02 x1023 pieces of what ever you are dealing with. Know this!!

62. Moles, molar mass, and molecular formulae (do each, resist the urge to follow the other answers in the class. It�s your BRAIN ? 1 mole of carbon (C) = 12 grams � mole of carbon = 1 mole of water (H2O) = � mole of water = 1 mole of carbon dioxide (CO2) = 2 moles of carbon dioxide (CO2) = 2.25 moles of carbon dioxide (CO2) =

63. Molecular formula Molecular formula is not only the ratio of elements in the molecule, but also the ratio of moles of each element in one mole of a compound. Glucose = C6H12O6 1 mole has: moles C = g moles H = g moles O = g

64. Grams to moles 12 g of C = 16 g of O = 8 g of O = 1 g of H = 2 g of H = 18 g of water (H2O) = 27 g of water (H2O) =

65. More grams to moles 100 g of water = 100 g of glucose = 100 g of table salt (NaCl) = 100 g of carbon dioxide = 100 g of oxygen = 100 g of hydrogen peroxide (H2O2)= 100 g of lithium fluoride =

66. How much of 100g� (in moles) of water is hydrogen= of glucose is hydrogen = of table salt (NaCl) is chlorine = of table salt (NaCl) is sodium = of table salt (NaCl) is hydrogen = of carbon dioxide is carbon = of hydrogen peroxide (H2O2)= of lithium fluoride is lithium =

67. Moles to grams 12 moles of C = 16 moles of O = 8 moles of O = 1 mole of H = 2 mole of H = 18 moles of water (H2O) = 27 moles of water (H2O) =

68. How much of 100g� (in grams) of water is hydrogen= of glucose is hydrogen = of table salt (NaCl) is chlorine = of table salt (NaCl) is sodium = of table salt (NaCl) is hydrogen = of carbon dioxide is carbon = of hydrogen peroxide (H2O2) is oxygen= of lithium fluoride is lithium =

69. Moles to parts (remember sci.not. and sig. figs.) Atoms of H in 1g Atoms of Na in 11.5g Atoms of C in 48g Atoms of C in 28 g of CO Atoms of C in 36 g of CO2 Atoms of H in 180 g of glucose Atoms of O in 90 g of glucose

70. Percent composition by mass Of the molar mass, how many grams are each part? Then convert this mass ratio to a percentage. H20 %H= %O= CO2 %C= %O= C6H12O6 %C= %H= %O= H2O2 %H= %O=

71. Density Density can be used to discriminate between two substances because it is a property of each. Compare two liquids here

72. What variables are used to calculate and object�s density? What is density in terms of matter?

73. Use the displacement method and the scales to determine the densities of the elements from Mr. B. be careful to report your densities with the correct number of sig figs.

74. Graph the period (row) number of elements on one axis and density on the other What does the graph of an element�s atomic number vs. its density look like?

75. Units Density is a derived quantity based on the combination of two measurements, each with their own unit. Volume is measured as a cube function of distance with a base unit of meters, and the amount of matter (mass) is measured in kilograms. Note that grams are often used instead of kilograms though. The units for density are grams per cubic centimeter (g/cm3)

76. What variables are used to calculate and object�s density? What is density in terms of matter?

77. The base units of most variables

78. More with density Density is a physical property of all substances and can be used to identify them. Do liquids have different densities?

79. Let�s find out� Mineral oil Water Alcohol Hexane

80. How about gasses? Qualitative determination of density Quantitative determination of density

81. The big bang � electrolysis of water Remember what the test for hydrogen gas was?

82. What is the density of water?

83. Each bench has a different chemical on it and a set of weigh boats. Your job is to have each person in your lab group mass out the molar amount stated on the weigh boat.

84. More than a mole?... Less than a mole?...

85. More than a mole?... Less than a mole?...

86. If the thickness of aluminum foil was .0015 cm, how thick would a mole of sheets be?

87. Moles and formulas teach us about how much stuff something is made out of. Remember that a fraction (A/B) is a part divided by the whole. To determine the percent of a compound that and element makes up you need to know the mass of the part AND the mass of the compound.

88. Percent Composition Would the same amount of sugar and sulfuric acid always produce the same amount of carbon? Make sure that you have done the carbon souffl� demo now or before this.Make sure that you have done the carbon souffl� demo now or before this.

89. Percent Composition If two compounds have the same elements, then they might be the same compound! Note that they might have the same elements but still have different proportions� Think H2O and H2O2.

90. First let�s try to calculate the percentages of single compounds Potassium Iodide - KI Lead Nitrate - Pb(NO3)2

91. First let�s try to calculate the percentages of single compounds Hydrochloric Acid - HCl Sodium Hydroxide - NaOH

92. An interesting reaction� �Where did that come from?....� HCl and NaOH are interesting chemicals in and of themselves, but when they are mixed they do something interesting.

93. An interesting reaction� First we need to make solutions of each chemical and we need to know the concentrations of each so that we can mix the right amounts. We need two molar sodium hydroxide. What amount would I need to make 500ml of this solution (500ml of 2M NaOH)?

94. An interesting reaction� Next, we need two molar hydrochloric acid. The dilution of this is tricky and a skill/calculation that we will learn later when we learn about acids. Can you guess what amount of a 12 molar solution I would I need to make 500ml of a 2 molar solution (500ml of 2M HCl)?

95. Write balanced equations for the following:

96. Write balanced equations for the following:

97. So, what can we do with this balanced reaction stuff?

98. So, what can we do with this balanced reaction stuff?

99. So, what can we do with this balanced reaction stuff?

100. So, what can we do with this balanced reaction stuff?

101. So, what can we do with this balanced reaction stuff?

102. Isotopes Isotopes are atoms of an element with the same number of protons (that�s what defines and atom of a certain element) but with different numbers of neutrons. As elements are �built or �assembled� in the craziness of the stars, some atomic combinations of subatomic particles get the same number of protons but different numbers of neutrons. Those combinations that are stable enough to last the test of time exists as isotopes of each other.

103. ELEMENTS AND ISOTOPES

104. Isotopes There are two ways to write or refer to isotopes of an element : Isotope name - name of the element plus a hyphen followed by the number of protons and neutrons in the nucleus. This number is called the mass number (i.e. carbon-14) Symbolic notation - symbol for the element with the mass number and the atomic number written before it as a superscript and subscript. 14 C (hard to do on PowerPoint� sorry ?) 6

105. An example to do parallel to the Penny lab I owe you $80,000 and you want me to pay you in pennies. Say I give you a truckload of pennies and I know how much the truck weighs? How can I calculate how many pennies are in the truck? How many dollars? How accurate am I�.?

106. Truck with pennies weighs 40 tons Truck alone weighs 15 tons 25 tons of pennies = 25tons x 2000lbs/ton = 50,000 pounds of pennies 28.35 grams in an ounce so 1 pound = 16oz x 28.35 grams/oz =454 grams per pound 1 penny = 3.0 grams 50,000 x 454 = 22,700,000 grams 22,700,000/3.0 = 7,570,000 pennies = $75,700 I HAVE UNDER PAID AND AM IN TROUBLE!

107. Two isotopes of penny There are actually two different types of pennies�. Now, how could I calculate the number of pennies in the truck? Truck with pennies weighs 40 tons Truck alone weighs 15 tons 25 tons of pennies = 25tons x 2000lbs/ton = 50,000 pounds of pennies 28.35 grams in an ounce so 1 pound = 16oz x 28.35 grams/oz =454 grams per pound penny type 1 = 3.0 grams penny type 2 = 2.5 average of the 2 types of penny = 2.75 grams 50,000 x 454 = 22,700,000 grams 22,700,000/ 2.75 = ? pennies = 8254545 /100= $82,545 ($75,700 = old value) how much money were we off by..? (if we used the truck as payment we overpaid!!!)

108. So, why aren�t there infinite numbers of isotopes? Because the combinations of protons and neutrons that are too unstable to last the test of time break down or decompose into other elements until they become stable If we know the masses of the subatomic particles

109. Complete the following chart

112. We know the Subatomic parts! Why don�t the masses of the elements on the periodic table not agree with the sum of the masses of the part? How many electrons would iodine need to have its mass equal to the mass reported? Illustrate the difference between the two types of pennies.

115. How does this relate to real life other than chemistry?... Tom, Mary, and Ralph all contribute to a shared checking account. Tom has contributed $145.56, Mary has given $768.42, and Ralph put in $4356.56. If the account earns 7% interest and this gain is then taxed at 30%, how much does each owe the government? Think percent composition and yield.

116. Tom, Mary, and Ralph all contribute to a shared checking account. Tom has contributed $145.56, Mary has given $768.42, and Ralph put in $4356.56. Total $145.56 + $768.42 + $4356.56 =$5270.54 Gain = $5270.54* 0.07 = $368.94

117. Gain = $5270.54 * 0.07 = $368.94 So, how much of this does each have to pay? Tom Mary Ralph $145.56 + $768.42 + $4356.56 =$5270.54 $145.56 $768.42 $4356.56 $5270.54 $5270.54 $5270.54 2.8% 14.7% 83.3%

118. Gain = $5270.54 * 0.07 = $368.94 So, how much of this does each have to pay? Tom Mary Ralph 2.8% 14.7% 83.3% Tax due is $368.94 * 0.30 =$110.68 $3.10 $16.20 $92.20

119. Do you know how your grade is calculated? It�s the same way as a weighted average for the elements Like isotopes of an element, there are different types of grades (HW, labs, quiz, and tests) each with different percentages. Calculating your grade is like calculating the average atomic mass of an element.

120. For example: HW Labs Quizzes Tests

121. What happens when there are to many neutrons for a nucleus to hold? There is a critical ratio of protons to neutrons that elements �like� to have and makes them stable. If elements don�t have the right amounts they will shed the amount of energy and particles needed to become stable.

122. Go over home work now. Make sure labs are collected

123. Do types of radiation mad lib Remind students about what they should have seen in the cloud chamber Reiterate what CO2 is and why it �wants� to be a gas at room temperature.

124. So, what can we do with this balanced reaction stuff?

125. Lets put it all together.

126. Percent yield problems � 1.� �90% 2. 37.2% 3. 93.8% 4. 3.70g 5. 99%� 1.� �90% 2. 37.2% 3. 93.8% 4. 3.70g 5. 99%

128. % yield possible lab or demo A common reaction in chemistry is the precipitation of calcium carbonate from the addition of a calcium chloride solution to a solution of sodium carbonate.� Assume we started with 16.78 g of calcium chloride and 32.14 g of sodium carbonate.� After filtration and drying the mass of calcium carbonate produced was 12.68 g CaCO3.�� Calculate the percent yield

129. Time permitting, try the experimental determination of H20 boiling point in large beakers with lab summary. Percent error is similar to percent yield only that the error represents a number rather than a quantity. Try the percent yield (stoichiometry) worksheet�

130. Working with gasses 1 volume of gas contains half as much gas as twice the volume. So volume is proportional to the amount of a gas. Twice the volume equals twice the gas� makes sense?

131. Avagodro�s Principle Avagadro, the same guy who thought up the torture of the mole noticed that there was another curiosity around the power of the mole. He noticed that no matter which gas was picked (small molecule H2O or some large 100 atom hydorcarbon), that one mole of it occupied the same volume as one mole of any other gas.

132. Because of this, he postulated that all gasses must have the same behavior and could be all described by a simple set of parameters and that there must be a way of converting the values of these parameter to one constant. Since the pressure, volume, and temperature can all be predicted for a known sample of any gas, there should be a way to set these parameters up to have them all equal a constant value.

133. For any amount of gas (n) if you multiply this value by the experimentally derived pressure and volume then divided by the temp in kelvin, you get the same value for each gas! This value has the abbreviation R, so� P�V� = R and P�V� = the same value R n�T� n�T�

134. P�V� = R and P�V� = the same value R n�T� n�T� From this you can prove that PV=nRT is applicable to any gas situation with only a few exceptions where the atoms themselves get in the way. Since atoms are so very small and their interaction so weak, these considerations are negligible.

135. Picking the R with the correct value is crucial!! You can tell the correct R from its units. If PV=nRT, then R=PV with units of atm x Li nT mol x K or mmHg x Li mol x K in order to establish the equality in situations

136. These are conversion factors so that you can move from any gas situation to another R= in atm with units of atm x Li = 0.0821 mol x K in Mercury mmHg x Li = 62.4 mol x K in kilopascals kPa x Li = 8.31 mol x K

137. Atoms and gasses and R�s, oh my!! MAKE SURE YOU PICK THE RIGHT ONE!! VERIFY IT WITH THE UNITS OF PRESSURE!!!! The temp, amount of matter, and volume units don�t change between the different R�s, although you must convert to kelvin, moles, and liters in the problem to get the right value for the final answer.

138. IDEAL GAS LAW Brings together gas properties. Can be derived from experiment and theory. BE SURE YOU KNOW THIS EQUATION!

139. Using PV = nRT P = Pressure V = Volume T = Temperature N = number of moles

140. Using PV = nRT R is a constant, called the Ideal Gas Constant Instead of learning or looking up a different value for R for all the possible unit combinations, we can just memorize one value and convert the units to match R if you know the conversion factors for the set points of pressure and that in atmospheres R = 0.0821 in atms

141. Pressure Column height measures Pressure of atmosphere 1 standard atmosphere (atm) * = 760 mm Hg (or torr) * = 29.92 inches = 14.7 pounds/in2 (psi) = 101.3 kPa (SI unit is PASCAL) * = about 34 feet of water! * Memorize these!

142. Learning Check Dinitrogen monoxide (N2O), laughing gas, is used by dentists as an anesthetic. If 2.86 mol of gas occupies a 20.0 L tank at 23�C, what is the pressure (mm Hg) in the tank in the dentist office? 2641 mmHg or 3.48 atm or 51 psi2641 mmHg or 3.48 atm or 51 psi

143. Learning Check A 5.0 L cylinder contains oxygen gas at 20.0�C and 735 mm Hg. How many grams of oxygen are in the cylinder?

144. Deviations from Ideal Gas Law Real molecules have volume. The ideal gas consumes the entire amount of available volume. It does not account for the volume of the molecules themselves. There are intermolecular forces. An ideal gas assumes there are no attractions between molecules. Attractions slow down the molecules and reduce the amount of collisions. Otherwise a gas could not condense to become a liquid.

145. Go over the gas stoichiometry sheet here to model the calculations and last nights hw before trying the following examples. Demonstrate Charles law and relate it to how a barometer works

152. 0.357 grams 533 liters0.357 grams 533 liters

153. 0.541 moles methane 15.6 li 58.4 ml or 5.84x10-3 0.541 moles methane 15.6 li 58.4 ml or 5.84x10-3

154. How much oxygen is in the air? What percent of each liter is O2? How many moles and molecules of O2 are in each liter of air? (do candle consumption under water here)

155. Introduce microscale gas production here and have students calculate the amount of sodium bicarbonate needed to fill one syringe full of gas when reacted with acetic acid. Next: Unit two - Atoms and why they react