Unit 1: States of Matter/Physical and Chemical Changes Learning objectives; to understand three states of matter to distinguish the properties of three states of matter to identify physical and chemical properties of substances to distinguish characteristics of physical and chemical changes Unit 1: Worksheet 1. Define Matter. 2. Identify three states of matter. i) ii) iii) 3. The box at left represents the atoms of aluminum (.) in the solid state. Represent the same atoms in the liquid state in the box at right. solid state liquid state 4. Draw the diagram of CO 2 in gaseous state below. CO 2 =
5. Identify which of the following represents a compound. i) ii) Explain your reasoning. 6. Classify each of the following as pure substance or mixture. i) ii) Explain your reasoning. 7. Describe the change of states of water when you boil 50.0 ml of water in a tightly closed container. After cooling the water to the room temperature, the resulting volume of water was measured. Would you expect to see the change of the volume of water? Explain your answer.
8. The following represents the liquid state of water (H 2 O). a) Which of the following diagrams best represents water (H 2 O) molecules after liquid water was heated to vaporize? i) ii) iii) Is vaporization physical or chemical change? Explain your reasoning. b) Water (H 2 O) can be decomposed into hydrogen gas (H 2 ) and oxygen gas (O 2 ) by the process called electrolysis. Draw the diagram ii) of hydrogen gas and oxygen gas. i) ii) Electrolysis Is an electrolysis physical or chemical change? Explain your reasoning.
9. Which of the following indicates chemical change? i) ii) Explain why. 10. State the Law of Conservation of Mass in your own words. If you dissolve 3.00 grams of sugar in 50.0 g of water, what would be the total mass of the mixture of sugar and water? When you dissolve 3.00 grams of Alka-Selzer in 50.0 g of water, the total mass of the mixture turned out to be less than 53.0 grams. Explain why. Does the process of dissolving Alka-Selzer in water disobey the Law of Conservation of Mass? Explain.
11. Sample of solid iodine was placed in a sealed vacuum tube. The weight of the tube with iodine solid was 12.5 grams. When the tube was heated, it was filled with iodine gas. iodine solid (I 2 ) Heating iodine gas (I 2 ) a) What is the name of the change from solid to gas? b) Is this change physical or chemical? Explain why. c) Which of the following statements is correct? i) The weight of the tube after heating is less than 12.5 grams because a gas weighs less than a solid. ii) The weight of the tube before or after heating is the same because mass is conserved during the change. d) Represent the change of solid iodine to gaseous iodine by depicting several iodine molecules as shown below. = iodine (I 2 ) solid iodine gaseous iodine heating
12. Mixture of substances A and B was separated by filtration process shown below. glass rod Filter paper Funnel Filter paper Funnel beaker beaker filtration after filtration a) Discuss whether filtration is a physical or chemical process. b) Which of the following represents water? i) ii) iii) unable to determine 13. Substance A and substance B were mixed in a beaker. After stirring the mixture vigorously, it was divided into two equal portions. To separate the substance A and B for each portion, filtration method was used and the following results were obtained. Mass of substance A Mass of substance B Portion I 12.5 g 23.3 g Portion II 16.7 g 19.1 g a) Discuss whether mixing A and B is a physical or a chemical process. b) Is the mixture homogeneous or heterogeneous? Explain your reasoning.
Unit 2: Measurements Learning objectives; to read and record measurements with correct number of significant figures to use correct metric units with the quantity being measured Unit 2: Worksheet For each of the following, record the value of the measurement with correct units. A. Measurement of length Ruler (in cm) Measurement
B. Measurement of volume Graduated cylinder (in ml) scale reading uncertainty scale reading uncertainty scale reading uncertainty 9 10 11 Beaker (in ml) Buret (in ml) scale reading uncertainty scale reading uncertainty
Unit 3: Double Replacement Reaction Learning objectives; to understand the general pattern of double replacement reactions. to predict whether the reactions occur to write complete balanced chemical (or formula) equations. Unit 3: Worksheet 1. Write balanced chemical equations for the following reactions. A. Precipitation Reaction Na Cl - Na Cl - Cl - Na Ag NO 3 - Ag Ag NO 3 - NO 3 - Na Na NO 3 - NO 3 - Na NO 3 - AgCl (s) AgCl(s) AgCl (s) Chemical equation: B. Gas Formation Reaction Na Na CO 3 2- Na Na CO 3 2- CO 3 Na Na 2- Cl- H Cl - Cl - Cl - Cl - H H H H Cl - H CO 2(g) CO 2(g) CO 2(g) Na Cl - Na Na Cl - Na Cl - Na Cl - Cl - Cl - Na Chemical equation:
C. Acid-Base Neutralization Na OH - Na H Cl - OH - Cl - H Cl - Na Na H Cl - Na Cl - OH - Na Cl - OH - OH - H Cl - Na Cl - Na Chemical equation: 2. Draw the diagram for each of the following double replacement reactions after writing complete balanced equations and classify each of the reactions as precipitation, gas formation, or acid-base neutralization reaction. A. Chemical equation: KOH (aq) H 2 SO 4(aq) Classification of the reaction: B. Chemical equation: Na 2 SO 3(aq) HCl (aq) Classification of the reaction:
C. Chemical equation: BaCl 2(aq) KNO 3(aq) Classification of the reaction: