Proust: elements combine to form compounds in a fixed proportion by weightĢ.2.1.3. each announced contradictory laws around 1800Ģ.2.1.2. 1000 grams of lead combines with 77 grams of oxygen to form 1077 grams of yellow lead oxideĢ.1.4. Mass is neither created nor destroyed in chemical reactionsĢ.1.3. Total weight of products equals total weight of reactantsĢ.1.2. Other chemists worked to discover other quantitative lawsġ.4. showed that mass was not lost or gained 1.3. discovered that weights of chemical are importantġ.2.4. discovered that general rules applyġ.2.2. Lavoisier set the stage for determining laws of chemistry 1.2.1. combining properties of elements required the assumption of discrete particles of matter 1.2. combinations of elements create the rich variety of substances which compose the universe and lifeġ.1.2. world would be dull and lifeless if composed onlyof uncombined elements 1.1.1. Use the law of of conservation of mass to balance simple chemical equations 1. Demonstrate understanding of the symbolic representation of chemical elementsand compoundsġ.9. Demonstrate knowledge of the rules for naming simple chemical compoundsġ.8. Show how the laws of chemistry can be used to determine the relative weightsof atomsġ.7. Use Avagadro's law to reconcile atomic theory and the law of combining volumesġ.6. Describe the controversy surrounding the law of combining volumesġ.5. State the law of combining volumes and cite some examplesġ.4. Correlate the hypotheses of Dalton's atomic theory with the laws of chemistryġ.3. State five laws of chemistry and explain them using examples.ġ.2. How much ammonia will this reaction produce? Objectives 1.1. How much hydrogen will be required to completely react with 280 grams of nitrogen gas. Why can we change the coefficients but not the subscripts in a chemical formula.ġ.2.12. How does the law of conservation of mass help in balancing chemical equations?ġ.2.11. Use the periodic table to find the chemical symbols for the following elements: gold, silver, lead, potassium, sodium, siliconġ.2.10. How do the laws of chemistry allow us to determine the relative atomic weights of the elements?ġ.2.9. How does the modern concept of atoms differ from that of the ancient Greeks? 1.2.7. What is Avagadro's hypothesis and how did it reconcile the law of combining volumes with Dalton's atomic theory?ġ.2.6. Discuss the law of combining volumes and the controversy surrounding its acceptance.ġ.2.5. What is the difference between an atom and an element? Between an atom and a molecule?ġ.2.4. Discuss the relationship between the laws of chemistry and Dalton's atomic theory.ġ.2.3. Why did the Greek philosophers reject the original atomic theory of Democritus?ġ.2.2. Compare and contrast the Law of Constant Proportions and the Law of Multiple Proportions. Briefly describe the controversy surrounding Berthollet and Proust.ġ.1.3. Name and describe the meaning of the three fundamental laws of chemistry? 1.1.2. We will learn about the law of combiningvolumes and the ensuing controversy which was finally resolved after Dalton's deathby Avagadro's hypothesis with an elegance we have come to expect.Īt the end of the program we will turn our attention to chemical symbols and equations. Text References Speilberg & Anderson, none Booth & Bloom, 234-245 Coming Upīefore we're done with this program we will have learned about the laws of chemistryand how they led an opinionated schoolmaster named John Dalton to formulate a newtheory of atoms based on the quantitative laws.
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