School District of Hillsborough County Middle School Science Physical Science Honors Semester 1 Exam Review

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1 School District of Hillsborough County Middle School Science IPS Chapter 1 Volume and Mass - (Safety) 1. Review all required reading sections and chapter questions for all sections. 2. Be familiar with all safety procedures. List a minimum of List the steps of the Scientific Method and apply these to various experiments. 4. Demonstrate mathematical skills in the use of scientific notation and significant digits. 5. Be able to read and interpret data from graphs. 6. Discuss why a professional scientist would repeat an experiment many times. 7. Exp. 1.1 Baking Soda: know the purpose for the apparatus and describe in full detail the results/observations of this experiment. What observations were made in the test tube when the baking soda was heated? What is the purpose of the water in the inverted bottle in lab? Where did the gas come from? What is the purpose of the tea test? 8. Explain water displacement. 9. How do you find the volume of the following? a. Regular solid b. Irregular solid c. A liquid 10. Read scales accurately when measuring length, mass, and volume. Redo CQC s 9,10, and 11 (pp 11,12) 11. List the steps to calculate the percent of air in sand & its applications. (Exp. 1.4) 12. Discuss whether volume can or cannot be conserved? 13. Explain the outcome of Lab 1.8 The Sensitivity of a Balance

2 IPS Chapter 2 Mass Changes in a Closed System 1. What is the sensitivity of a balance? 2. Why is it important to display data using a Histogram? 3. When doing the ice lab in chapter 2, the student finds the mass before melting to be 20.2g. A lid is not used. After the ice melts, the student finds the mass to be 18.2g. What happened? 4. Why should you wipe the condensation off the container in the melting ice lab? 5. Liquid A has a mass of 120g and a volume of 40 cm3. Liquid B has a mass of 30g and a volume of 50 cm3. You pour the two liquids together. What can be said about the mass? About the volume? 6. When doing the Copper and Sulfur Lab: The test tube and cover had a mass of 20.2g. The tube, cover, copper and sulfur before the reaction had a mass of 23.2g. The tube, cover, copper and sulfur after the reaction had a mass of 23.1g. A. What is the mass of the copper and sulfur only before the reaction? B. What is the change in mass? 7. When doing the alka-seltzer lab, the mass before mixing was 51.0g and the mass after mixing was 49.02g. Explain the decrease in mass. 8. When is the Law of Conservation of Mass valid? 9. Define the Law of Nature and give 3 examples 10. Be able to determine the mass of a gas when given data. 11. Determine the best explanation for a gain or loss in mass; when salt is dissolved, ice melts, copper combines with sulfur, or a gas is produced. 12. Describe and interpret data from a histogram. 13. Restate and apply the Law of Conservation of Mass. 14. Demonstrate your knowledge of the difference between mass and volume; be able to apply this concept in a variety of situations.

3 IPS Chapter 3 Characteristic Properties 1. Identify which properties are considered characteristic properties. 2. Sketch a graph of each freezing point, melting point, and boiling point. Label x and y axis, room temperature, and title. Determine what state of matter (solid, liquid, or both solid & liquid) a substance is in from a cooling curve. Compare and contrast the freezing point and melting point of a substance. Compare and contrast the boiling point and condensation point of a substance. 3. Explain what affect different volumes of a substance will have on a temperature vs. time graph. 4. Identify and use the formula to calculate density for solids, liquids, and gases. A block has a mass of 10.0g. Its length is 6cm, width is 1cm and height is 2 cm. What is the density of the block? A balloon has a volume of cm 3 and the gas inside the balloon has a mass of 0.5g. What is the density of the gas? A liquid has a volume of 10.7 cm 3 and a mass of 10.0g. What is the density of the liquid? 5. List the common range of densities for solids, liquids, and gases 6. Determine whether an object will sink or float based on density. List specific examples from Table What is the density of water? Of alcohol? 8. What is the boiling point of water? Freezing point? 9. Find the average of the following numbers and write the answer with proper significant digits. A cm, cm and 12.30cm B g, g and 17.0g C. 3.9mm, 3.92 mm and mm 10. Know how to identify a substance based on its characteristic properties. 11. Distinguish between a physical property and a chemical property.

4 12. Define a physical change and a chemical change; list examples of each. 13. Why is a beaker of cold water used in some experiments when collecting a gas? 14. What are boiling chips used for? IPS Chapter 4 Solubility 1. What is the difference between qualitative and quantitative observations? 2. Define solute, solvent, solubility, concentration, saturated, unsaturated solution, and precipitate. List examples of each. 3. Determine the difference between concentration and density 4. Sketch a solubility curve (Exp. 4.4). 5. Explain how solubility varies with different solvents and /or different temperatures. 6. How can you change the solubility of most solids in water? 7. When testing the solubility of a gas, how does the temperature and the motion affect the outcome (Exp 4.7) 8. What effect does the burning of gasoline and coal have on the environment? 9. What is the difference between a weak (dilute) and a strong (concentrated) solution? 10. List the factors that affect the dissolving rate of a solute in a solvent. IPS Chapter 6 Compounds & Elements 1. Explain the difference between an element, a mixture, and a compound. 2. Define decomposition and synthesis reactions. Give an example of each. 3. Describe how a catalyst is used in a reaction. (Exp. 6.2) 4. Identify factors that affect the ratio when substances combine to for compounds 5. Discuss what happens to the ratio when an excess quantity of a reactant exists. 6. Analyze graphical data for the synthesis of a product. (Exp. 6.4) 7. Define and apply the Law of Constant Proportions and Conservation of Mass.

5 8. Describe the difference between an endothermic and an exothermic reaction. 9. Differentiate between a complete and an incomplete reaction. IPS Chapter 7 Radioactivity; IPS Chapter 8 The Atomic Model of Matter (8.9,8.10) 1. Review all the required reading sections and chapter questions for all sections. 2. Summarize Henri Becquerel s Experiment (7.1) 3. Explain Radioactivity in terms of alpha decay, beta decay, and gamma rays. 4. Describe how the decaying dice activity was used to model radioactivity. (Exp. 8.9) 5. Calculate half - life problems. (Exp. 8.10) 6. What factors could possibly affect the counting rate of a Geiger counter? This document has been compiled from the Hillsborough County School District Middle School Science Curriculum Guide for, to meet the requirements for the Sunshine State Standards.

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