Introduction to Chemistry
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1 Introduction to Chemistry Regents Chemistry: Unit 1 Essential Questions: What is chemistry? How do we know a study is valid? What are the most accurate and precise ways to work with numbers? 1
2 (I) What is Chemistry? Chemistry: studies how reactions! Reactants break and/or form new to form products Atoms or combine in different ways to form new substances Also Includes studies of: of materials How change how a reaction occurs 2
3 (II) Scientific Method: The steps to doing good science! Step 1: Ask a Ex- Step 2: and Observation: Interpretations: Step 3: Draw a Ex- Step 4: Develop an Experiment Valid experiments need to have these components/variables: (1) (2) (3) (4) Other Ideas: Step 5: Perform the Experiment Step 6: Analyze the results of the experiments Question: What are good ways to analyze data? Step 7: Draw a - this should lead to more questions! 3
4 (III.) Measurement Precision single measurement decimal places more precise Ex: cm more precise than cm Ex: Rewrite the following measurements from least to most precise 30.4 cm 30 cm 30. cm cm m Precision -- multiple measurements -- how close measurements agree Accuracy how close measurement is to (requires ) Ex: a one foot board is made and then checked with a ruler, inches is more accurate than inches. 4
5 Rule for measuring 1. Write down the value of lines on either side of measurement 2. Add a dotted zero (in the next decimal place) to each shows this is an estimated place 3. To the lower value, replace the dotted zero with an estimate of the measurement cm a. d. b. c. a Value of line to left (with dotted zero added) Value of line to right (with dotted zero added) Measurement b c d Ex: In the following measurements, underline the estimated number cm 64.3 g 74 L miles in 4.46 x 10 5 calories In all measurements, there is/are estimated number(s) 5
6 Reading liquid volume Meniscus: the shape at the top of a liquid like water *** measure from the (IV.) Significant Figures and Scientific Notation Definition: Atlantic-Pacific rule can be used to determine which digits are significant. Pacific Rule If the decimal point is start from the Pacific side of the number and move right to the first nonzero digit. Underline this digit and every number to the right. All underlined digits are significant. Atlantic Rule If the decimal point is, start from the Atlantic side of the number and move left to the first nonzero digit. Underline this digit and every number to the left. All underlined digits are significant 6
7 Determine the number of significant figures in the measurements below: A. ) 2000 B.) C. ) D.) E.) F.) G.) H.) I.) Rules for Adding & Subtracting with Significant Figures Perform the following calculations, solving to the correct number of significant figures: A.) 10.6cm 3.45cm = B.) 1.234mL mL = C.) 5m + 7.3m = D.) nm 1.03nm = 7
8 Rules for Multiplication & Division with Significant Figures Perform the following calculations, solving to the correct number of significant figures: A.) 47.9/3.2 = B.) x 1200 = Mixed Math Practice: A.) = B.) = C.) 7.16 x = D.) 104.6/75 = E.) x 2.7 x = Scientific Notation and Significant Figures Determine the number of significant figures in each measurement below: A.) 3.0 x 10 2 B.) 1.00 x 10 5 C.) x
9 Scientific & Decimal Notation Convert the following into scientific notation: A.) B.) C.) D.) Convert the following into decimal notation: A.) 4.5 x 10 3 B.) 1.7 x 10-4 C.) 2.05 x 10-6 D.) 8.6 x 10 7 Rules for Multiplying a Diving when numbers are in scientific notation: 9
10 Perform the following calculations and write your answer in scientific notation to the correct number of significant figures: A.) 1.9 x x 3.8 x 10 6 = B.) 5.0 x 10-4 x x 10-3 = C.) x x = D.) 4.84 x x 10 9 = (V.) Metric System and Unit Conversions *** Table D includes the units that you will need to be comfortable with*** 1. kilogram A. Unit of length 2. millimeter B. defined to be 1 ml 3. liter C. Unit of volume 4. density D. Unit of mass 5. cm 3 E. mass of 1 cm 3 of a substance Fill in the blanks (Hint: Use Table C in the Chemistry Reference Tables) Prefix Kilo Hecto Abbreviation K d Value /1000 Exponential Form 1 x x 10-2 King Henry 10
11 Conversion by moving decimal place: Write down metric in order Move decimal place same number of and as prefixes. Use Table C in your Reference Table to help you with the following conversions. Record your answer to the correct number of significant figures. A.) 15m to km B.) 1.5m to nm C.) 350g to mg D.) 100kg to g E.) 0.19 cm to m F.) 0.026mg to g (VI.) Dimensional Analysis Also called Label Method Can solve more problems than by moving decimal place Requires conversions with numbers and. You must multiply and units to convert to new unit! You must multiply and units to convert to new unit! Step 1: Write down conversions with units Step 2: Arrange conversions to proceed from old unit to new unit Step 3: Plug in the numbers and do the math to convert to a new unit 11
12 (VII.) Density measures how closely matter is materials are denser because: either they are packed or because the atoms are. (or both)! Challenge Question: Given equal masses of Copper, Aluminum, Iron, and Magnesium, which will have the greatest volume? How do you know? The Density Triangle : 12
13 Density Word Problems: Pre-Question.) What is the formula for density? Which table on the Reference Tables gives you this formula? 1.) Find the density of an object to the correct number of significant figures if the volume is 3.00 ml and the mass is 15g. M = V = D = 2.) A piece of aluminum has a mass of 8.1g and a volume of 3.23mL. Find the density of aluminum and record your answer to the correct number of significant figures. M = V = D = 3.) The density of an unknown liquid is g/ml. What is the mass of 15mL sample of the substance? M = V = D = 4.) The density of gold is g/ml. What is the volume of 10.5g of gold? M = V = D = 5.) Which element has a high density, yttrium or manganese? 6.) Which element on Table S has the highest density? What is the chemical symbol for this element? 13
14 (VIII.) Percent Error Percent Error: Percent Error Word Problems: A.) What table on the reference tables gives you the formula for percent error? B.) When solving a percent error question does it matter if you get a positive or negative answer? C.) A student determines the density of a piece of iron to be 7.59 g/ml. What is the student s percent error? (Hint: you will need Table S) D.) In an experiment, the density of copper is determined to be 9.45 g/ml. The accepted value for the density of copper is g/ml. Find the percent error. 14
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