Honors Chemistry Summer Packet. Dear Honors Chemistry Student,

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1 Dear Honors Chemistry Student, This packet is designed to provide students entering Honors Chemistry with important chemistry-based mathematical skills and chemistry content before the start of the school year in order to ensure success throughout the academic year. A written assessment of the topics will be conducted during the second class block of the school year in September. The packet is broken up into two different portions. The chemistry content portion of this packet will require an outline creation. Each outline topic requires a hand-written summary sheet that will act as a study guide for the written assessment. Each summary sheet should be a single standard page (8.5" x 11") using both-sides of the paper. Only the originals (not copies) of these sheets will be collected and graded. The mathematical portion of this packet provides students with an opportunity to learn and practice mathematical skills specific to chemistry and its related topics. BOTH portions will be assessed on the written assessment in September. In order to help students prepare, both video tutorials and guiding questions are provided in this packet. These are not all-encompassing resources, though. You will also need to make use of the Internet and your local library to help ensure completion of this packet. All Honors Chemistry students are expected to complete this assignment, regardless of the date of enrollment in the course. Do not hesitate to reach out if there are any questions regarding this packet. We look forward to your enrollment in Honors Chemistry for the academic school year! Sincerely, The Honors Chemistry Teachers Monroe Township High School

2 Resources Video Tutorials Go to Bozeman Science website at Watch the following videos: Unit 1: Introduction Factor-Label Method Unit 1: Introduction Scientific Method Unit 1: Introduction Significant Digits Unit 2: Matter & Atomic Theory History of the Atom Unit 2: Matter & Atomic Theory Matter Unit 2: Matter & Atomic Theory Properties of Matter Go to Kahn Academy website at the following YouTube links. Significant Figures: Calculations with Significant Figures -- o Multiplying and Dividing: o Adding and Subtracting: Scientific Notation: p5rw8 Metric Conversions:

3 Part 1: Chemistry Content Guiding Questions These general topics and subsequent guiding questions will be used to create your outline. Each general topic requires the complete of an outline sheet. The requirements for the sheets are given on the previous page. 1. Topic #1: Introduction to Chemistry What is a chemical? How is matter measured? Describe the difference between mass and volume. Describe what each term is and what it is made of o Atom o Element o Compound For the following properties, define the property, and describe how the property can be measured or observed, and give 3 examples for each. o Extensive o Intensive o Physical o Chemical Describe the atoms in the following states of matter o Solid o Liquid o Gas o Plasma Explain the differences between a physical and chemical change. Why is a phase change a physical change and not chemical change? Describe a chemical reaction in terms of reactants and products. Explain how the law of conservation of energy and the law of conservation of mass can hold true during a chemical reaction. Describe the two types of mixtures, how are the two mixtures identified. Compare and contrast homogeneous mixtures and compound. Define pure substance. On the periodic table below identify the location of o groups / families o periods o metals o nonmetals o metalloids o noble gases Compare and contrast the characteristics of metals and nonmetals. 2. Topic #2: Quantitative Chemistry

4 What is the difference between a quantitative observation and a qualitative measurement? What are the advantages to the metric or SI system? Make a chart of the seven base units of the SI system. In the chart include what each unit measures, the unit name, the quantity symbol and the unit abbreviation. How is a derived unit different from and base unit? Make a chart of the seven derived SI units; include the quantity measured, the quantity symbol, the unit name, the unit abbreviation and the equation used to derive the unit. Explain density as it relates to chemistry. 3. Topic #3: Atomic Theory Democritus (date) o initial view of the atom o image/example of what the Democritus Atom would look like (based on the description) Dalton (date) o Dalton s atomic theory o explain Dalton s model of the atom o image of Dalton s model J.J. Thomson (date) o particle found by J.J. Thomson o explanation of the experiment used to find the particle o image of the experiment o the model J.J. Thomson developed, description and image Rutherford (date) o explain the experiment performed by Rutherford o image of the experiment o development made towards the atom based on the experiment o Image of the Rutherford atomic model Millikan (date) o experiment used by Millikan o development made based on the experiment o image of the experiment o inferences that could be made about the atom Bohr (date) o Describe how Bohr s model of the atom is different than Rutherford s o image of the Bohr s Atomic Model Quantum Model o Describe how the Quantum model is different that the Bohr Model What information about element does the atomic number give? How is the mass number found? Why is it important when discussing isotopes?

5 Describe how protium, deutritium and tritium are similar and how are they different. Describe the difference between relative atomic mass and average atomic mass. 4. Topic #4: Descriptive Chemistry List the Names, symbols, atomic number, mass number, and atomic mass of the first twenty elements. Chemical Nomenclature of Ionically and Covalently bonded materials List the rules and identify a compound s name from its formula and the formula from its name

6 Part 2: Chemistry-related Mathematical Concepts Significant figures The last digit of a measurement expression is uncertain. That is because the last digit is estimation. Significant figures in a measurement expression comprise all digits that known with certainty, plus one digit that is uncertain. PLACEHOLDERS ARE NOT SIGNFICANT. Rules for determining the number of significant figures in a given value: 1. All non-zero digits are significant. 2. All zeros between two nonzero digits are significant. (aka: sandwich rule). PRACTICE: Determine the number of significant figures in each of the measurements below L L g g 5. 3,400,008 ml 3. Trailing zeros are significant only if there is a decimal point or a bar drawn over the zero PRACTICE: determine the number of significant figures in each of the measurements below: ,00 g _ , 000 cm L mg 4. Zeros in the beginning of a number whose only function is to place the decimal point are not significant. Ex: has 2 significant figures. 5. Zeros following a decimal significant figure are significant Ex: has 3 significant figures PRACTICE: determine the number of significant figures in each of the measurements below: ml kg g L g cm

7 Significant figures - Determine the number of significant figures in the following measurements ml L L ,876, mm g ,008 g ,000 cm g ,000 cm cm ,000 ml cm g cm ,008 ml cm L x ,000 g x g x ,010g Rule for Multiplying and Dividing Limit and round to the least number of significant figures of any of the factors. Example: 23.0 cm x 432 cm x 19 cm = 188,784 cm 3 = 190,000 cm 3 since 19 cm has only two significant figures Rule for Adding and Subtracting Limit and round your answer to the least number of decimal places Example: ml ml ml = ml = ml since 46.0 ml has only one decimal place Perform the following operations expressing the answer in the correct number of significant figures m x m = 2. 1,035 m 2 / 42 m = ml Ml + 6 ml = g 28.9 g = cm cm cm =

8 Scientific Notation Scientist very often deal with very small and very large numbers, whichcan lead to confusion when counting zeros. We have learned to express these numbers as powers. Scientific notation takes the form of M x 10 n where 1 M < 10 and n represents the number of decimal places to be moved. Positive n indicates the standard form is a large number. Negative n indicates a number between zero and one. Example: Convert 1,400,000 to scientific notation. We move the decimal point so that there is only one digit to its left, a total of 6 places. 1.4 x 10 6 Example: Convert to scientific notation. For this we move the decimal place 5 places to the right = 2.5 x 10-5 Practice Part 1 Convert the following to scientific notation = = 2. 5,050 = = = = 4. 1,000 = = 5. 1,000,000 = 10. 5,000 = Part 2 Convert the following to standard decimal notation x 10 3 = x 10-1 = x 10-3 = x 10-4 = x 10-2 = 8. 1 x 10 4 = x 10 2 = 9. 1 x 10-1 = x 10 5 = x 10 0 =

9 Metric Conversions Facts you need to know Length Mass Volume Volume of a solid 10 mm = 1 cm 100 cm = 1 m 1000 mm = 1 m 1000 m = 1 km 10 mg = 1 cg 100 cg = 1 g 1000 mg = 1g 1000 g = 1 kg 10 ml = 1 cl 100 cl = 1 L 1000 ml = 1 L 1000 L = 1 kl 1 cm 3 = 1mL Worked Example 500 ml =?? L Calculations: 500 ml 1 L 1000 ml = 0.5 L 35 kg =?? mg Calculations: 35 kg 35,000,000 mg 1000 g 1 kg 1000 mg 1 g = Practice Problems g = kg cm = mm 3. 5 L = ml km = mm (Hint: this is a two step process) ml = kl (Hint: this is a two step process) 6. 3 m = cm ml = L g = kg mm = cm m = km