Chapter 3:
Matter - Properties and Change
Section 3.11. Identify the characteristics of a substance.
2. Distinguish between physical and chemical properties.
3. Differentiate among the physical states of matter.
Section 3.2 1. Define physical change and list several common physical changes.
2. Define chemical change and list several indications that a chemical change has taken place.
3. Apply the law of conservation of mass to chemical restrictions.
Section 3.3 1. Contrast mixtures and substances.
2. Classify mixtures as homogeneous or heterogeneous.
3. List and describe several techniques used to separate mixtures.
Section 3.4 1. Distinguish between elements and compounts.
2. Describe the organization of elements on the periodic table.
3. Explain how all compounds obey the laws of definite and multiple proportions.
Section 3.1 Properties of Matter
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Section 3.2 Changes in Matter
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Section 3.3 Mixtures of Matter
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Section 3.4 Elements and Compounds
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Section 3.1 Properties of Matter
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Section 3.2 Changes in Matter
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Section 3.3 Mixtures of Matter
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Section 3.4 Elements and Compounds
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Section 3.1 Properties of Matter
Standard 2 d - Chemical Bonds
View Standard 2 State Standard: In a liquid the inter-molecular forces are weaker that in a solid, so that the molecules can move in a random pattern relative to one another
Students Will be able to:Compare and contrast the intermolecular forces that determine the states of matter Book Reference Pages: 58, 59
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Section 3.2 Changes in Matter
Standard 3 E - Conservation of Matter and Stoichiometry
View Standard 3 State Standard: How to calculate the masses of reactants and products in a chemical reaction from the mass of one of the reactants or products, and the relevant atomic masses.
Students Will be able to:Perform an experiment to determine the quantitative relationships between reactants and products in a balanced chemical equation. I&E (12A): Select and use appropriate tools and technology (such as computer-linked probes, spreadsheets and graphing calculators) to perform tests, collect data, analyze relationships, and display data. I&E (12B): Identify and communicate sources of unavoidable experimental error. I&E (12C): Identify possible reasons for inconsistent results, such as sourced of error or uncontrolled conditions. Book Reference Pages: 63-65
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Section 3.3 Mixtures of Matter
Standard 6 f - Solutions
View Standard 6 State Standard: How molecules in a solution are separated or purified by the methods of chromatography and distillation.
Students Will be able to:Book Reference Pages: 69
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Section 3.4 Elements and Compounds
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Dictionary Definitions
● Law of Multiple Proportions Visit Site
● Hydrologic- Water Cycle - demonstrating physical changes in nature Visit Site
● Water dimer animation - hydrogen bonding Visit Site
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General
● Element, Compound, mix (molecular level w MDL models you can rotate)- Applets USC Visit Site
● Chromatography - background and types Visit Site
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Physical/Chemical
● On-line quiz w answers (10 questions) from Math & Sci Act Ctr Visit Site
● Short interactive lesson, followed by 7 questions w ans & explanations. Click box in top left of screen to get started. Visit Site
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States of Matter
● Animation of States of Matter (Visionlearning) Visit Site
● Liquid N2 poured into erlenmeyer flask, then long rubber tube put down into the nitrogen. It comes out other end of tube and condenses water from air around it as it exits Visit Site
● Animation showing 3 states of matter. Pretty nice because you see temp, macro and nano views of water as it changes. Visit Site
● 3 states of matter using NaCl from USC Visit Site
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Wigger Vids
● Methane ( CH4 ) and oxygen produce water and carbon dioxide ( CO2 ) . This demonstration shows water condense on outside of a pan be heated on a gas stove Visit Site
● A dilute solutin of phenol red is distilled using an 250 mL flask, hot plate to heat the solution, and collecting distilled water in 250 mL beaker. The condensing unit has a water jacket to cool down the steam so the less of the condensed water is lost to the atmosphere. Visit Site
● Copper is subjected to concentrated nitric acid and is completely dissolved into the acid solution, making a blue colored solution of copper nitrate. Visit Site
● First Law LAB - Group 1 mixing in zip lock bag Visit Site
● Fisst Law LAB - Group 2 mixing in zip lock bag Visit Site
● First Law LAB - Group 3 mixing in zip lock bag Visit Site
● ChemThink.com Ch 3 - Particulate Nature of Matter - Part 1 - questions 1-7 - Vid to help you understand Visit Site
● ChemThink.com Ch 3 - Particulate Nature of Matter - Part 2 - questions - last 4 questions - Vid to help you understand Visit Site
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