Review ppt2

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Review ppt2

  1. 1. Chemistry Final Review Game Ms. Bradley
  2. 2. Periodic Table <ul><li>What group does calcium belong to? </li></ul><ul><li>What group does lithium belong to? </li></ul>
  3. 3. Periodic Table <ul><li>Group 7 are called the ____________ </li></ul><ul><li>Group 8 are called the ____________ </li></ul>
  4. 4. Rates of Reaction <ul><li>What is a ‘rate’? </li></ul>
  5. 5. Rates of Reaction <ul><li>Which reacts the SLOWEST? </li></ul><ul><ul><li>a. A large tablet of alka seltzer </li></ul></ul><ul><ul><li>b. Half of a tablet of alka seltzer </li></ul></ul><ul><ul><li>c. Powdered alka seltzer </li></ul></ul><ul><ul><li>d. They all react at the same rate </li></ul></ul>
  6. 6. Rates of Reaction <ul><li>If the temperature of a reaction is higher, is the reaction rate faster or slower? </li></ul><ul><li>Why? </li></ul>
  7. 7. Physical and Chemical Changes <ul><li>Which of the following is NOT a physical change? </li></ul><ul><ul><li>A. cutting paper </li></ul></ul><ul><ul><li>B. molding clay </li></ul></ul><ul><ul><li>C. burning wood </li></ul></ul><ul><ul><li>D. grinding metal </li></ul></ul>
  8. 8. Physical and Chemical Changes <ul><li>What observations can you look for that shows a chemical reaction has occurred? </li></ul>
  9. 9. Acids/Bases <ul><li>Acids taste _________ </li></ul><ul><li>Bases taste _________ </li></ul>
  10. 10. Acids/Bases <ul><li>Hydroxides (OH-) are all _________ </li></ul><ul><li>Hydronium (H+) are all __________ </li></ul>
  11. 11. Acids/Bases <ul><li>Monoprotic, diprotic, triprotic acids </li></ul><ul><li>Mono means ______ </li></ul><ul><li>Di means ______ </li></ul><ul><li>Tri means ______ </li></ul><ul><li>Protic means ______ </li></ul>
  12. 12. Acids/Bases name if time <ul><li>Which of the following is a DIprotic acid? </li></ul><ul><ul><li>H 3 PO 4 </li></ul></ul><ul><ul><li>H 2 SO 4 </li></ul></ul><ul><ul><li>HBr </li></ul></ul><ul><ul><li>CH 3 COOH </li></ul></ul>
  13. 13. Pressure <ul><li>1 atm= _____ torr </li></ul><ul><li>1 atm= _____ mmHg </li></ul><ul><li>100 torr= _______ mmHg </li></ul>
  14. 14. Pressure <ul><li>Convert 795 mmHg to atm </li></ul><ul><li>Convert 1.50atm to torr </li></ul>
  15. 15. Partial Pressures <ul><li>OOPS! We didn’t have time to do this…. Real quick! </li></ul><ul><li>Dalton’s law of partial pressures…. </li></ul>
  16. 16. Ideal Gas Law <ul><li>The ideal gas law equation is…. </li></ul><ul><li>If I have pressure, volume, and temperature.. What can I use the ideal gas law to find? </li></ul>
  17. 17. Reaction symbols <ul><li>(s)= _________________ </li></ul><ul><li>(l)= _________________ </li></ul><ul><li>(g)= _________________ </li></ul><ul><li>(aq)= _________________ </li></ul><ul><li>What does (aq) mean? </li></ul>
  18. 18. Types of reactions <ul><li>What are the 5 types of reactions? </li></ul><ul><li>In a decomposition you have _____ reactant and _____ products. </li></ul><ul><li>In a ________________ reaction, two compounds form two new compounds. </li></ul>
  19. 19. Elements/Compounds/Mixtures <ul><li>Where do I find elements? </li></ul><ul><li>What is a compound? </li></ul><ul><li>What is the difference between homogeneous and heterogeneous mixtures? </li></ul>
  20. 20. Electron Configuration <ul><li>What is the electron configuration for N (nitrogen)? </li></ul><ul><li>What is the electron configuration for Mg (magnesium)? </li></ul>
  21. 21. Lewis Structures <ul><li>C= ______ bonds </li></ul><ul><li>N= ______ bonds </li></ul><ul><li>O= ______ bonds </li></ul><ul><li>H= ______ bonds </li></ul>
  22. 22. Lewis Structures <ul><li>Bonding in molecules that cannot be correctly represented by a single (one) Lewis structure is…. </li></ul><ul><li>a. polyatomic </li></ul><ul><li>b. resonance </li></ul><ul><li>c. single bonding </li></ul><ul><li>d. double bonding </li></ul>
  23. 23. Lewis Structures <ul><li>How many total electrons are in the lewis structure for CO 2 ? </li></ul><ul><li>How many total electrons are in the lewis structure for CH 4 ? </li></ul><ul><li>How many total electrons are in the lewis structure for Li 2 S? </li></ul>
  24. 24. Oxidation numbers <ul><li>The sum of all oxidation numbers in a compound equals _______. </li></ul><ul><li>What is the oxidation number of hydrogen in most compounds? </li></ul><ul><li>What is the oxidation number of oxygen in most compounds? </li></ul>
  25. 25. Percent Composition <ul><li>Part/Whole x 100= percent composition </li></ul><ul><li>What is the percent composition of oxygen in carbon monoxide? </li></ul><ul><li>What is the percent composition of hydrogen in ammonia (NH 3 )? </li></ul>
  26. 26. Empirical and Molecular Formulas <ul><li>_______________ formulas are the simplest form of a formula with the lowest subscripts. </li></ul><ul><li>Is C 3 H 12 an empirical or molecular formula? </li></ul>
  27. 27. Nomenclature (naming) <ul><li>When do you use the prefixes mono, di, tri, etc… in ionic or covalent bonded molecules? </li></ul><ul><li>What is the name for MgCl 2 ? </li></ul><ul><li>What is the name for SF 6 ? </li></ul>
  28. 28. Bonding (ionic, covalent, metallic) <ul><li>______ bonds are between a metal and a nonmetal with positive and negative charges. </li></ul><ul><li>______ bonds are between 2 nonmetals. </li></ul><ul><li>_______ bonds have a sea of electrons. </li></ul>
  29. 29. <ul><li>Mole ratio </li></ul><ul><li>Stoich </li></ul><ul><li>Exo/endo </li></ul><ul><li>Precipitate </li></ul><ul><li>Atom </li></ul><ul><li>Radioactive cookies </li></ul><ul><li>Balance </li></ul><ul><li>Molar mass </li></ul><ul><li>Essay portion </li></ul>

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