Honors Pre-AP Chemistry Summer Assignment

Transcription

1 Honors Pre-AP Chemistry Summer Assignment I hope you are excited about enrolling in Honors Pre-AP Chemistry for next year. As you probably know, this course is weighted and will be more rigorous and demanding than regular chemistry. This course is designed to prepare you for AP Chemistry. If you are ready for the demands of the course, you are expected to complete the following summer assignment. I look forward to seeing you in the Fall! Thank you, Mr.Thomas thomasje@wsd3.org Summer Assignment Overview: In this summer assignment, you will be reviewing math skills vital to your success in the class, as well as introduce you to the element names and symbols we will use daily in chemistry. You will complete both an Element Quiz on the first day of school and Math Skills Quiz the first week of school. In addition, you will be required to use the course website to support your learning throughout the summer. Moodle Website Access: 1. Go to (UserName is your Student Number and use your password that contains your initials-four digit code-initials!) 2. You will be enrolled into the course once the final schedules have been finalized in June. Assume you have chemistry the first day of school, do not wait to find out your schedule! Bring your assignments to school! Assignments: 1. Make flash cards for memorization. Located at: In this packet! a. Use index cards, not cut strips of paper to produce your flash cards. You will need flash cards of the following: i. Element Names and Symbols (quiz on the 1 st day of school) You will see a list of what needs to be on the flash cards in this packet. For elements, put the symbol on one side and the name on the other. Have only one element per card. You can use the same strategy for the list of fractions. You will be given a grade for these flash cards on your return from summer and be tested on them throughout the year. You can visit the summer assignment webpage to learn these elements and from quizlet.com, an online resource for playing games to memorize content. You can even use your ipod to play games for memorization! 2. Summer Unit Packet. Located at: 1. In this packet! 2. a. If you need assistance, view each of the video lectures (vodcasts) for the Summer Unit objectives on the course website. Complete each of the required assignments for the objectives in the packet. All of the assignments need to be completed by the first day of class. Resources for completing the assignments: Following this page is the list of elements that are required to be memorized! You will need to access the course webpage for the Summer Unit Packet resources and complete that assignment over the summer. If you have any technical problems over the summer with the website, Mr.Thomas with your question. Again, I hope you are looking forward to the challenge this course has to offer and I ll see you in August! Mr.Thomas Pre-AP and AP Chemistry Teacher Mesa Ridge High School thomasje@wsd3.org

2 Mesa Ridge High School Chemistry Element List You will need to MEMORIZE the following elements (both their symbols and name) for quiz on the 1 st day of class. Write the element symbol on one side of you flash card and the name on the other. Example Flashcard: Sulfur S Element Name Element Symbol Element Name Element Symbol Element Name Element Symbol Hydrogen H Sulfur S Rubidium Rb Helium He Chlorine Cl Strontium Sr Lithium Li Argon Ar Molybdenum Mo Beryllium Be Potassium K Silver Ag Boron B Calcium Ca Tin Sn Carbon C Chromium Cr Iodine I Nitrogen N Manganese Mn Xenon Xe Oxygen O Iron Fe Cesium Cs Fluorine F Cobalt Co Barium Ba Neon Ne Nickel Ni Gold Au Sodium Na Copper Cu Mercury Hg Magnesium Mg Zinc Zn Lead Pb Aluminum Al Arsenic As Radon Rn Silicon Si Bromine Br Uranium U Phosphorus P Krypton Kr Plutonium Pu

3 LT # Learning Targets Assignments Math- 1 Convert between scientific notation and regular number form WS 1.1 Scientific Notation Math- 2 Math- 3 Math- 4 Use the Order of Operations and solve basic algebra problems Manipulate equations algebraically to solve for an unknown variable Convert between units using dimensional analysis (1- Dimensional) WS 1.2 Order of Operations PEMDAS WS 1.3 Algebraic Manipulation WS Dimensional Analysis Math- 5 Math- 6 Math- 7 Convert between units using dimensional analysis for multi dimensional, squared and cubic dimensional problems Calculate the density of a substance Calculate percent error WS 1.5 Multi Dimensional Analysis Dimensional Analysis Graphing Exercise Graph the given data and find the slope of a best- fit line WS Density WS 1.7 Percent Error

4 Worksheet 1.1: Scientific Notation 1. Write the following numbers in scientific notation In Scientific Notation meters grams L moles 2. Write the following numbers in regular notation. In Regular Notation ml mg M m/s 3. Rank each of the following in order from smallest to largest. 2.2x x x x 10-3 Convert the following: (Sci. Notation à Number or Number à Sci. Notation) 1. a) 2 x 10 4 b) x 10 2 c) 5 x 10-6 d) 3.41 x 10 1 e) 5.5 x a) - 8 x b) x 10-2 c) - 1 x 10 1 d) x 10-8 e) x a) 3.45 x 10 6 b) 4 x 10-1 c) 1.8 x 10 1 d) 7.2 x 10-3 e) 7.65 x a) 400,000 b) 4,000,000,000 c) d) e) 100

5 Perform the following calculations, giving all answers in the scientific notation version AND numerical version: 1. (5.61 x 10 4 ) * (3.20 x 10 3 ) 2. (2.12 x 10-3 ) + (9.41 x 10-4 ) 3. (7.02 x 10 6 ) - ( x 10 6 ) 4. (1.08 x ) / (4.66 x 10 5 ) 5. (5.85 x 10 4 ) * ( x 10-6 ) 6. (6.51 x 10-4 ) / (4.19 x 10-9 ) 7. (3.75 x 10 3 ) - (8.05 x 10 9 ) 8. (5.66 x 10 3 ) + ( x 10 8 )

6 Worksheet 1.2 Order of Operations PEMDAS Rules Evaluate the problem in the following order: 1) P - Parentheses 2) E - Exponents (Powers and Square Roots) 3) MD - Multiplication and Division (Left to Right) 4) AS - Addition and Subtraction (Left to Right) PLEASE EXCUSE MY DEAR AUNT SALLY

7 Algebraic Manipulation The key to solving simple algebraic equations containing a single unknown (e.g. x + 6 = 10) is to realize that the equation is an equality. As long as you do the same mathematical operation (e.g. add a constant, subtract a constant, multiply by a constant, and divide by a constant) to both sides of the equation, the equality is still an equality. This includes squaring both sides of the equation or taking the square root of both sides of the equation. Fundamental Laws: Distributive Law: 3(x + 2) = 3x + (3)(2) = 3x + 6 Associative Law: 4x - 7x = x(4-7) = -3x Example 1 To solve for x, it is necessary to subtract 6 from both sides of the equation Example 2 To solve for x, you need to add 6 to both sides of the equation and then divide both sides by 2. Example 3 To isolate x, you need to (1) multiply through by 6, (2) subtract 2 from both sides, and (3) divide both sides by 5. Example 4 To solve for x this time, you need to Example 4 alternative) (1) multiply both sides of the equation by 4 and 3 to cancel out the denominator in line 2, (2) use the distributive law, (3) by adding and subtracting, move the x terms to one side, and the non-x terms to the other side in line 5, (4) use the associative law to simplify to get line 7, and (5) divide both sides by 2. This process is called "cross-multiplying." This entails multiplying the numerator of one side of the equality by the denominator of the other side of the equality. When this is done, the very same line 3 results. The rest of the problem is done identically. Example 5 This problem could be very complicated and become a quadratic equation. However, because it has a perfect square on both sides, if you simply take the square root of both sides of the equality, you are left in line 3 with a straightforward algebra problem as you solve for the positive root, which I did here. In Chemistry, when we use this technique to solve equilibrium problems, only one of the roots is meaningful. Of course, the square root of 49 can be -7 as well as +7. You can then go ahead and solve for the second root, x = -0.8 = -4/5.

8 Worksheet 1.3 Algebraic Manipulation Solve for x in the equations below! 1.) x / 6 = 7 12.) 3x x = 113/8 2.) 2 + x = 9 13.) 2x x = 35 3.) 1 + x = 10 4.) x + 9 = ) 3x x = 60 5.) 9 = x ) 3x + 9 = 6x ) 6x + 9 = ) x + 9 = 4/7x + 81/7 7.) 7 + 2x = ) 7(1/2 + 5x) = 287/2 8.) 7x + 3 = ) 6(7x + 8) = ) 6x + 9 = ) 7x + 6 = ) 3(1x + 10) = ) x x = ) 3(5x + 7) = 21

9 Worksheet 1.4: Dimensional Analysis (Single Dimensions) How do you set- up a dimensional analysis problem? Example: If 1 inch is the same as 2.54 cm, how many inches are equal to 4.5 cm? Step 1: Identify the given value and write it down. 4.5 cm Step 2: Determine which unit you want the answer expressed in. 4.5 cm x =? inches Step 3: Choose your conversion factor. Your conversion factor should get you from the units you start with to the units you want to end with. The units you started with should go on the bottom of the conversion factor. The units you want to end with should go at the top of your conversion factor. 1 inch 4.5 cm =? inches 2.54 cm Step 4: Do the math by either multiplying or dividing, depending on the problem. 1 inch 4.5 cm = cm Step 5: Cancel units where possible and write the remaining unit behind your answer. 1 inch 4.5 cm = 1.77 inches 2.54 cm Here are some conversion factors that you are expected to know: 1000 milliliter = 1 Liter; 1000 millimeters = 1 meter 100 centimeters = 1 meter 1000 meters = 1 kilometer; 1000 grams = 1 kilogram You must show your dimensional analysis set- up to receive credit for these problems yard is equal to 3 feet. How many feet are in a football field (100 yards)? 2. 1 gallon is equal to 4 quarts. How many gallons do you have if you have 18 quarts? 3. How many milliliters are in 5.7 Liters? 4. The average age of a high school junior is How many days old is the average high school junior?

10 grams of food contain 130 calories. How many grams of food would you need in order to consume 2150 calories? 6. How many kilometers are in 2500 meters? 7. There are 16 ounces in a pound. How many pounds are in 52 ounces? 8. How many grams are in 30,000 kilograms? Express your answer in scientific notation. 9. Texas is 790 miles from East to West. How many feet is that if 1 mile is equal to 5,280 feet? 10. How many centimeters are in 0.05 meters? Express your answer in scientific notation. 11. Each large pizza can feed three teenage boys. How many pizzas would be needed to feed that Atascocita football team? (56 teenage boys). 12. Main Street is approximately 0.25 miles long. How many yards long is Main Street if 1 mile is equal to 1760 yards? 13. You spend 242 minutes in chemistry class each week. How many minutes will you spend in chemistry at the end of the school year (36 weeks)?

11 Worksheet 1.5: Dimensional Analysis (Multi- Dimensional) km/hr =? miles/hr (mph) 2. Convert a speed of 35.8 mi/hr to m/s mph =? mi/s mph =? m/s km/hr =? mi/hr m/s =? cm/s 7. Convert a speed of 73.5 km/hr to m/s 8. Convert a speed of 88 m/s to cm/s km/hr =? m/s 10. Convert a density of 4.52 g/ml to kg/l.

12 Worksheet 1.6: Density For each problem below, write the equation and show your work. Always use units and box in your final answer. 1. The density of silver (Ag) is 10.5 g/cm 3. Find the mass of Ag that occupies 965 cm 3 of space. 2. A 2.75 kg sample of a substance occupies a volume of cm 3. Find its density in g/cm Under certain conditions, oxygen gas (O 2 ) has a density of g/ml. Find the volume occupied by g of O 2 under the same conditions. 4. Find the volume that 35.2 g of carbon tetrachloride (CCl 4 ) will occupy if it has a density of 1.60 g/ml. 5. The density of ethanol is g/ml at 20 o C. Find the mass of a sample of ethanol that has a volume of ml at this temperature g of each of the following acids are needed. Find the volume of each that must be measured out in a graduated cylinder. A. hydrochloric acid (HCl), density = g/ml B. sulfuric acid (H 2 SO 4 ), density = g/ml C. nitric acid (HNO 3 ), density = g/ml

13 7. A rectangular block of lead (Pb) measures 20.0 mm X 30.0 mm X 45.0 mm. If the density of Pb is g/cm 3, calculate the mass of the block. 8. A cube of gold (Au) has a side length of 1.55 cm. If the sample is found to have a mass of 71.9 g, find the density of Au. 9. An irregularly-shaped sample of aluminum (Al) is put on a balance and found to have a mass of 43.6 g. The student decides to use the water-displacement method to find the volume. The initial volume reading is 25.5 ml and, after the Al sample is added, the water level has risen to 41.7 ml. Find the density of the Al sample in g/cm 3. (Remember: 1 ml = 1 cm 3.) 10. If you are sure that a sample of material is aluminum but have no measuring instruments AND are not allowed to handle the sample, how would you determine the sample s density? 11. A gas has a mass of 3175 g and takes up enough space to fill a room that is 2.00 m X 2.00 m X 5.00 m. Use the table below, which lists densities in units of g/ml to help you determine what the gas is. (Hint: Change the units on the size of the room.) Densities of Common Gases at 20 o C under Normal Atmospheric Pressure Gas Density (g/ml) Hydrogen Helium Nitrogen Oxygen

14 Worksheet 1.7 Percent Error Percent Error = Your Answer Accepted Value x100 Accepted Value 1. Joshua uses his thermometer and finds the boiling point of ethyl alcohol to be 75 o C. He looks in a reference book and finds that the actual boiling point of ethyl alcohol is 80 o C. What is his percent error? 2. Ariel weighed an object on her balance and recorded a mass of 24.3 grams. Her teacher told her that there was obviously something wrong with her balance because it was giving her a reading, which was 30.0% too high. What was the actual mass of the object? 3. Chase got a lab report back with -5.0% error written in red on it. He had determined the boiling point of an unknown liquid to be 45 o C. What is the correct boiling point of his unknown liquid? 4. The density of water at 4 o C is known to be 1.00 g/ml. Kayla experimentally found the density of water to be g/ml. What is her percent error? 5. The Handbook of Chemistry and Physics lists the density of a certain liquid to be g/ml. Taylor experimentally finds this liquid to have a density of g/ml. The teacher allows up to +/ % error to make an A on the lab. Did Fred make an A? Prove your answer. 6. An object has a mass of 35.0 grams. On Anthony s balance, it weighs grams. What is the percent error of his balance?

15 7. Shelby measured the volume of a cylinder and determined it to be 54.5 cm 3. The teacher told her that she was 4.25% too high in her determination of the volume. What is the actual volume of the cylinder? 8. Walter gets a paper back in lab with -2.75% error written on it. He had found the mass of an object to be grams. What should he have found as the mass of the object? 9. After lab, all of Darrel s friends looked at his data and laughed and laughed. They told him that he was 30.8% too low in the boiling point he had just recorded. He had recorded a boiling point of 50 o C on his data sheet. What is the correct boiling point of the liquid he was working with in lab?