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# Study Guide Lessons 1-9 CHMY 141N - 00

UM

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This 19 page Study Guide was uploaded by Isabella Sturgeon on Sunday September 20, 2015. The Study Guide belongs to CHMY 141N - 00 at University of Montana taught by Mark Cracolice (P) in Fall 2015. Since its upload, it has received 186 views. For similar materials see College Chemistry I in Chemistry at University of Montana.

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Date Created: 09/20/15

Study Guide Lesson 19 Lesson 1 Main points Understand the difference between a direct proportionality an inverse proportionality and multiply proportionalities Understand and be able to use quantitative algebra to solve problems Know how to separate the quantity from the unit Know how to use conversion factors to go from a given unit to the desired unit This also requires the use of quantity algebra Know that a proportionality constant is needed to turn a proportionality into an equa on Practice Problems Basic 1 An 897 kg block of iron magnetite is found If the block is 270 Iron oxide how what is the mass of Iron oxide 2 A car can drive an average of 65 miles per hour How many minutes will it take to travel will it take the car to travel 178913 feet 3 Heat fusion is when a pure substance melts q is proportional to the mass of the given sample m Create a proportionality and then find the units for the constant if the heat is measured in kilocalories and the mass is measured in grams If it takes 891 calories to melt 86 grams of ice Calculate the heat of fusion of water in calories per gram Intermediate 1 What mass of an 976 by mass sodium solution must be measured to obtain 709 grams of sodium 2 The number of miles a car is driven is proportional to the gallons of gasoline burned Write a proportionality statement Write an equation with k as the constant Calculate the value of k if the car has driven 1752 miles and burned 35 gallons of gas 3 Calculate how many minutes are in a year What about seconds Lesson 2 Main points Understand that fractions can be converted to decimals Know what a ratio is and how to change it to a percent Know how to convert a percent to parts per million parts per trillion and parts per billion Memorize that 1cm cubed is equal to 1 mL Know what temperature absolute zero is Know how to convert Celsius to Kelvin Understand metric conversions and have the highlighted ones memorized Understand that on Earth weight and mass are used interchangeably Always make sure to use quantitative algebra Practice Problems Basic 1 If a gold ore is 0078 by mass gold and a company wants 200 troy ounces of pure gold what is the mass in grams or gold ore needed a troy ounce is 3110348 grams 2 An ore contains 1245 milligrams of silver What is the percent by mass parts per billion and part per million if the sample is 273 grams 3 Convert the following 259 L to mL 134 cm cubed to mL 19876 mL to L 00875 m to picometers 45678 grams to decagrams Intermediate 1 A sucrose solution is made by dissolving 3 grams of sucrose in 345 grams of water What is the percentage by mass parts per million and parts per billions of sucrose in the solution 2 A sample of blood is shown to have a concentration of 11 ppm of lead If the sample of blood is 154 grams what is the mass of lead in milligrams 3 If a student pays 7985 for a book and sales tax is 67 what is the original cost of the book If the bookstore gave the book a 13 markup what price did the bookstore pay 4 Convert the following 917 L to cm cubed 876 cm to mm 00076 kg to ng ChaHenge 1 How many minutes are in 45 of the day How many minutes are in 3 of the day when a person is awake if they are awake for 18 hours 2 If 521 grams of sugar are added to 16 fluid ounces of hot tea that is 85 degrees Celsius what is the percentage by mass of sugar in the solution We will assume that that the plain tea has a mass of 0876 grams for 1mL and that 1 fluid ounces is equal to 295735 mL Lesson 3 Know what an experiment is Know what a hypothesis is Understand and know the relationship between pressure and volume Know Boyle s Law Know what a law is Know the formula for a directly proportional relationship Know the formula for an indirectly proportional relationship Know how the Kinetic molecular hypothesis explains Boyle s Law Know and understand what a molecule is Understand and know Charles s Law Know what temperature is Know what a theory is Know and understand the combined gas law Practice Problems Basics 1 What is science 2 What is a law 3 What is pressure 4 A balloon is filled with 725 L of helium is at 23 degrees Celsius and 1 atm What will the volume be if the balloon is moved to an area with a temperature of 0 degrees Celsius at a pressure of 451 torr Intermediate 1 How does the J tube experiment show the pressure of the atmosphere versus the pressure of the contents of the contents of the tube 2 What is the pressure if the force is 376 pounds on an area that is 2 inches by 7 inches 3 If you have a fixed amount of gas what will the volume be if the temperature is doubled and the pressure is tripled 4 Gas being released from a factory is discharged at 125 degrees Celsius and 676 torr Every 2 L of gas shrinks to 087 L and is the temperature outside is 35 degrees Celsius What is the atmospheric pressure outside in torr ChaHenge 1 Why does a filled flexible container spring back to its original form after being compressed 2 A fixed amount of gas has a volume of 345 L at 75 degrees Celsius and 657 torr What will the volume be in mL if the pressure is reduced to 025 atm and the temperature is changed to 45 degrees F What will the temperature be if the pressure is increase to 785 torr and the volume remains the same at 345 L Lesson 4 Main Points Understand what accuracy is Know the precision of the instrument of measurement Know how to use significant figure convention and where the uncertain digit is Know the significant figure rule for subtraction and addition Know the significant figure rule for multiplication and division Know what the formula for density is Know conversions within the United States Customary System Practice Problems Basic 1 How many significant figures are in the following 8765 102 10 11x10 912345672 2 A graduated cylinder weighs 9785 grams and contains 56 mL of water A solid cylinder of aluminum is placed into the water and the level rises to 1356 mL and the mass of the water increased to 19776 grams What is the density of the cylinder 3 Convert 175 pound per cubic foot to grams per mm cubed 4 If the density is 3475 grams per cubic inch what is the weight in lbs of 3 quarts of liquid gold Intermediate 1 Determine the density of a block that is 45 inches by 76 inches by 3 inches that weighs 97531 lbs The density should be in grams per cubic centimeter 2 If a solution is 7 ammonia by mass and has a density of 1006 gmL What is the mass of ammonia dissolved in 65 gallons of ammonia solution 3 If the density of gasoline is 756 grams per cubic foot what is the mass of gasoline if the volume is 6778 L 4 How many pounds of aluminum are needed for 300 100foot rolls of wire that has a diameter of 17th of an inch The density of aluminum is 985 grams per centimeter cubed and the volume of a cylindrical solid isV nrzl ChaHenge 1 If the density is 683610339gmm2 what is the density in pounds per cubic foot What is the weight of a block that is 5 feet by 7 feet by 7 feet 2 If you are painting a room that has one window that is 2 feet by 45 feet that does not need to be painted and the paint has a density of 124 grams per mL and the room has four walls that are 135 feet by 25 feet which need 25 mm of paint how many pounds of paint are needed Lesson 5 Main Points Know what a chemical change is Know what a chemical property is Know what a physical change is Know what a physical property is Know how to classify matter Know what a compound is Know what an element is Understand the process of distillation Know what a gas is Know what a heterogeneous mixture is Know what a homogeneous mixture is Know what matter is Know what a mixture is Know what a pure substance is Know what a solution is Know what vapor is Practice problems 1 Define the list of main points 2 Classify the following as pure substance or mixture sugar salt water smoke coffee with milk coffee water oxygen 3 Classify the following as homogeneous or heterogeneous muffins gold ring coffee with milk coffee 4 Classify the following as elements or compounds mercury iron oxide helium zinc calcium carbonate Intermediate 1 Classify the following as a physical or chemical change ice melting to water paper burning dissolving salt in water rusting of iron 2 If after distilling a liquid the new liquid has a lower freezing point than the original liquid was the substance pure or a mixture 3 Can there be different compounds made from the same two elements If so list examples 4 If you have to separate salt from water would you use physical or chemical changes ChaHenge 1 If a substance is burned and looks the same before and after but tastes different is the substance and element or compound 2 If after distillation the liquid looks the same as the original liquid and has the same freezing point was the original liquid a pure substance or mixture 3 Name some things that are not the result of a chemical change made by humans that are used in everyday life Lesson 6 Main Points Understand and know the Law of Conservation of Mass Understand and know the Law of Definite Proportions Understand and know the Law of Multiple Proportions Know what an atom is Know what the atomic hypothesis is Know what the atomic theory is Know the symbols and names for all of the elements highlighted in the book Know the atomic mass unit Know the Dalton Understand relative atomic mass Practice Problems Basic 1 Define the three laws listed above How do they give evidence that supports Dalton s atomic model 2 If a solution of 13 oz is mixed with a solution that has a mass of 67 g They combine and produce a gas leaving the new solution to have a mass of 38 g What was the weight of the gas in pounds 3 Write the name of the following atomic symbols Ar H He Zn Mg Mn 0 P K Li N Ne Be Ba 4 Write the symbol for the following elements Silver Silicon Mercury Cobalt Calcium Intermediate 1 Oxygen and carbon combine to form three different compounds that are 4749 3112 and 1843 percent carbon by mass What law do these confirm and how 2 How can an atom and a molecule of an element be identical but the atom and molecule of a compound cannot be identical 3 A gas has a volume of 57 gallons when at 56 degrees F and a pressure of 76 mmHg If the volume is increased to 67 gallons and the temperature is decreased to 13 degrees C what will the pressure be ChaHenge 1 Which law of the three Laws does not have enough information to be the basis for a hypothesis when looking at by itself Lesson 7 Main Points Know Avogadro s Hypothesis Know the Law of Combining Volumes Understand how the charge of an electron was discovered Understand the plum pudding model of an atom Understand the nuclear model of the atom Understand the Rutherford scattering experiment and how that changed the idea of the structure of an atom Practice Problems Basic 1 Why did they think of the atomic structure as being planetary 2 What is significant about Rutherford s experiment and the alpha particles passing through the gold without being deflected 3 If 1 volume of element A combines with 2 volumes of element B to form 2 volumes of compound AB are the elements diatomic or monatomic Intermediate 1 Compare the volumes of 200 hydrogen molecules with 200 oxygen molecules and 400 molecules of helium all at the same temperature and pressure 2 If a nucleus is 5 inches in diameter what would the diameter of an atom be 3 What is the volume in fl oz of a spherical drop with a radius of 12 inch if the formula is 4 TT 3 3 ChaHenge 1 Why does Avogadro s Hypothesis work for only gasses 2 Explain the connection between Dalton s atomic theory and the Law of Definite Composition Lesson 8 Main Points Know what a neuron is Know what a proton is Know what the atomic number means Know what an isotope is Know what atomic mass is Know what nuclear symbol is Know chemical family and group Know metals vs non metals Know what a transition metal is Practice Problems Basic 1 What are the three major subatomic particles Compare their mass and charge 2 Why can isotopes of different elements have the same mass number but not isotopes of the same element 3 Can two elements have the same atomic number Why or why not 4 Why is the atomic mass unit good 5 Identify the group number and period of the following elements atomic number s 20 14 8 30 Intermediate 1 What was the first part of Dalton s atomic theory that was proven wrong 2 If there are two isotopes of an element why isn t the average of the two sometimes listed 3 Find the average mass of a boron atom if the isotopes are 1100931 u and 2001 have a mass of 100129 u 4 Write the symbols for the elements in Period 3 and the atomic numbers for the elements in group 2A2 ChaHenge 1 The element of oxygen is found in two isotopes one form has a density of 175 g per cm cubed and the other has a density of 318 g per cm cubed The volume of an oxygen atom is 15x10 22cm3 Calculate the density Propose a reason for the difference in isotope density from the actual density If the radius of the atom is 10000 times bigger than the nucleus what is the volume of the nucleus What is the density of the nucleus Lesson 9 Main Points Know what a chemical formula is Know what a chemical nomenclature is Know what IUPAC is Know what a molecule is Know what a state symbol is Know what a binary molecular compound is Know what a metalloid is Know what an anion and cation is Know what an ion is Know what an ionic compound is Know what a monoatomic ion is Know what oxidation state is Know what an acid is Know what an oxoacid is Practice Problems Basic 1 What are monatomic cations and how are they formed from atoms 2 Write the formulas of the elements of Group 8A18 3 Write the names for C12 02 Ba Fe Ar 4 Write the formulas for Carbon lead potassium nickel and iron 5 Write the name for 02 I Cu H Intermediate 1 How are monatomic anions formed from atoms 2 What is an element How about a compound 3 Does the Law of Definite Composition relate to the chemical formula of a compound

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