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Q.P.S. Update

Q.P.S. Update. Update QPS- Chemical Bond and Reaction Test Tomorrow. Today’s Goal: Summarize how the law of conservation of matter applies to chemical bonds and equations. This is what will be covered on the Test. Ch 4 Bonds and Reactions Test. Why do atoms Combine?

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Q.P.S. Update

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  1. Q.P.S. Update Update QPS- Chemical Bond and Reaction Test Tomorrow Today’s Goal: Summarize how the law of conservation of matter applies to chemical bonds and equations.

  2. This is what will be covered on the Test Ch 4 Bonds and Reactions Test Why do atoms Combine? Compare Covalent and Ionic Bonds. Illustrate what the valence electrons do in both bond types. Explain the Law of the Conservation of Matter. Balance a chemical equation. Explain the difference between a chemical and physical change.

  3. Write the correct balanced formula equation for the following reaction. • Solid sodium combines with chlorine gas to produce solid sodium chloride. 2Na(s) + Cl2(g)  2NaCl(s) • 2. Illustrate the following bonds with Lewis Structures and a bond structure. • Covalent: H + O

  4. 3. Why do elements combine? To form compounds and find stability with a complete shell of valence electrons. • 4. Balance the following chemical reaction. • Sr(OH)2 + FeCl3 SrCl2 + Fe(OH)3 3Sr(OH)2 + 2FeCl33SrCl2 + 2Fe(OH)3

  5. 5. Create a Venn Diagram comparing Covalent and Ionic Bonds • 6. Why is it important to balance chemical equations • Why should the # of atoms that react yield the same # of products? Supports the law of conservation of matter

  6. 7. Describe (using examples) the difference between a chemical and physical change. Physical Chemical • 8. Illustrate the following bonds with Lewis Structures • Ionic: Na + Cl

  7. Bonds and Reactions Test Why do atoms Combine? Compare Covalent and Ionic Bonds. Illustrate what the valence electrons do in both bond types. Explain the Law of the Conservation of Matter. Balance a chemical equation. Explain the difference between a chemical and physical change.

  8. Chemical Bonds and Reaction ReviewQuestions

  9. Chapter Review Question 1 Ancient thinkers who invented a basic form of chemistry, but mixed it with magical beliefs and superstitions were known as _______. A. alchemists B. botanists C. scientists D. zoologists IN: 8.1.1

  10. Chapter Review Question 1 Ancient thinkers who invented a basic form of chemistry, but mixed it with magical beliefs and superstitions were known as _______. A. alchemists B. botanists C. scientists D. zoologists IN: 8.1.1

  11. Chapter Review Answer The answer is A. Modern chemists owe the origins of their science to the alchemists. IN: 8.1.1

  12. Chapter Review Question 2 NH3 is an example of a _______. A. bond B. compound C. molecule D. polar molecule IN: 8.3.8

  13. Chapter Review Question 2 NH3 is an example of a _______. A. bond B. compound C. molecule D. polar molecule IN: 8.3.8

  14. Chapter Review Answer The answer is B. In this case, the compound being described is ammonia. IN: 8.3.8

  15. Chapter Review Question What is the term for molecules that have an even number of charges? Answer Nonpolar molecules have an even number of charges. The only totally nonpolar molecules are molecules formed by the bonding of atoms of the same element. IN: 8.3.8

  16. Chapter Review Question When two pairs of electrons are both involved in a covalent bond, what is formed? IN: 8.3.8

  17. Chapter Review When two pairs of electrons are both involved in a covalent bond, what is formed? Answer A double bond is formed. When three pairs are involved, it is known as a triple bond. IN: 8.3.8

  18. Chapter Review Question What type of bond is formed when electrons are shared unevenly? A. covalent bond B. ionic bond C. metallic bond D. polar bond IN: 8.3.8

  19. Chapter Review Question What type of bond is formed when electrons are shared unevenly? A. covalent bond B. ionic bond C. metallic bond D. polar bond IN: 8.3.8

  20. Chapter Review Answer The answer is D. The bonds between the oxygen atom and hydrogen atoms in the water molecule are an example of a polar bond. IN: 8.3.8

  21. Standardized Test Practice Question A series of chemical symbols and numbers that shows which elements are present in a compound, as well as how many atoms of each element are present, is known as a _______. A. chemical bond B. chemical compound C. chemical formula D. chemical set IN: 8.3.8

  22. Standardized Test Practice Question A series of chemical symbols and numbers that shows which elements are present in a compound, as well as how many atoms of each element are present, is known as a _______. A. chemical bond B. chemical compound C. chemical formula D. chemical set IN: 8.3.8

  23. Standardized Test Practice Answer The answer is C. Chemical formulas are mathematical models that help us understand actual properties of element and compounds. IN: 8.3.8

  24. Standardized Test Practice Question What does the formula NH3 tell you? • There are three nitrogen and three hydrogen • atoms in this compound. • B. There are three nitrogen atoms and one • hydrogen atoms in this compound. • C. There are three hydrogen atoms and one • nitrogen atoms in this compound. • D. There is one nitrogen atom and one hydrogen • atom in this compound. IN: 8.3.11

  25. Standardized Test Practice Question What does the formula NH3 tell you? • There are three nitrogen and three hydrogen • atoms in this compound. • B. There are three nitrogen atoms and one • hydrogen atoms in this compound. • C. There are three hydrogen atoms and one • nitrogen atoms in this compound. • D. There is one nitrogen atom and one hydrogen • atom in this compound. IN: 8.3.11

  26. Standardized Test Practice Answer The answer is C. The formula tells you that the ratio is one nitrogen atom to three hydrogen atoms. IN: 8.3.11

  27. Standardized Test Practice Question How many electrons are there in this atom’s outermost energy level? A. 1 B. 5 C. 7 D. 14 IN: 8.3.11

  28. Standardized Test Practice Question How many electrons are there in this atom’s outermost energy level? A. 1 B. 5 C. 7 D. 14 IN: 8.3.11

  29. Standardized Test Practice Answer The answer is C. The dots give the number of electrons in the outer energy level, not necessarily the total number of electrons. IN: 8.3.11

  30. Chapter Review Question Many kinds of food need to be refrigerated in order to keep them from spoiling. Knowing what you now know about chemistry, can you explain why this is so? IN: 8.3.11

  31. Chapter Review Answer A decrease in temperature decreases reaction rates. Since spoilage is a chemical reaction, refrigeration of perishable food will slow down its tendency to spoil. IN: 8.3.11

  32. Chapter Review Question According to the law of the conservation of mass, the mass of the _______ must be the same as the mass of the _______. IN: 8.3.12

  33. Chapter Review Answer The mass of the products must be the same as the mass of the reactants. IN: 8.3.12

  34. Standardized Test Practice Question Even if it isn’t written into a chemical equation, _______ is always part of any chemical reaction. A. energy B. sound C. tonality D. vibration IN: 8.3.15

  35. Standardized Test Practice Question Even if it isn’t written into a chemical equation, _______ is always part of any chemical reaction. A. energy B. sound C. tonality D. vibration IN: 8.3.15

  36. Standardized Test Practice Answer The answer is A. Energy may be needed to start the reaction or it may be given off as a result of the reaction, but it is always involved. IN: 8.3.15

  37. Review and Reinforce • Use the time remaining to: • Complete Ch. 4 Study Guide • Review using websites on Ch. 4 Homepage.

  38. Chemical Reactions Test Learning Goal • Demonstrate your knowledge of chemical bonds and reactions. After the test, complete section 5.1 beginning on page 184

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