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Ch 100: Exam #3 Review Information· Exam will be given at 2 p.m., March 17, 2003 (Monday) in JH Room 115· Exam will be roughly 1 hour in length· bring a scientific calculator & a single-sided (3” x 5”) sheet of notesInformation Provided:· Periodic Table· Electronegativity valuesNotes:Exam will cover chapters 5, 6, 7 & 9 Go over reading material and homework as well as lecture notesGo over class worksheetsSpecific Study Points:Ch 5: electron orbitals & shellsCh 6: Lewis structures, types of chemical bonds and electronegativityCh 7: the mole & Avogadro’s number, calculate grams from moles, calculate moles from # of atoms/molecules, calculate grams from # of atoms/molecule, calculate molar concentration from grams of solute dissolved in volume of solution, calculate # of atoms/molecules of solute in a volume of solutionCh 9: balancing chemical reactions, activation vs. bond energy, exothermic vs.endothermic chemical reactionsQuestions to consider:1. Electron orbitals: · What is the outer electron configuration for an element? E.g. O or K· What is the total electron configuration for an element? E.g. Ne or N2. Electron Shells· How many electrons are in the outer shell of an element? E.g. O or K· How many electrons can a particular shell hold?3. Chemical bonding· Write out the Lewis structure for the following elements: N, Mg, Ar· What is the electronegativity for the following elements: F, Ca, O, H, Na, N, Cl ?· Determine the type of chemical bond between the following elements:· C and H· N and H· Ca and Cl· O and H· Na and F· What are the major differences between single, double and triple covalent bonds?4. The Mole & Avogadro’s Number· You have 1.23x1023 atoms of Na. How many moles do you have?· You have 1.3 moles of Cu. How many atoms do you have?· You have 10 g of C. How many moles of C do you have?· You have 2.5 moles of S. How many grams do you have? 5. Molar mass?· What is the molar mass for: Ba, O2, MgCl2, C2H66. Concentration (Mass concentration, % v/v, Molarity)· You dissolve 10 g of MgCl2 in water to make 0.5 L of solution. What is the mass concentration (grams/L) of the solution?· You dissolve 10 g of MgCl2 in water to make 0.5 L of solution. What is the molar concentration (molarity) of the solution?· You have a 0.10 M solution of HCl. How many moles of H+ ions are in 0.05 L?· You have a 0.10 M solution of HCl. How many H+ ions are in 0.05 L?· You want to prepare 0.10 L of HCl solution (0.10 M ). How much HCl in grams do you need to mix with water to get this concentration?7. Chemical reactions· What role does a catalyst play in a chemical reaction?· How are activation energy and bond energy different?· What factors affect the rate of a chemical reaction?8. Balancing Chemical Reactions· See your worksheet for practice balancing chemical equations· Know difference between reactants and products· Be able to balance an unbalanced chemical reaction· Be able to write out an unbalanced chemical reaction from a story problem· From a balanced chemical reaction can you determine the molar ratio of each reactant and product in the reaction?9. Exothermic vs. endothermic chemical reactions· Is energy absorbed or released when a chemical bond is formed?· Is energy absorbed or released when a chemical bond is broken?· What determines whether a chemical reaction is endothermic or endothermic?· A certain chemical reaction requires 10 J of energy to break all of its chemical bonds and 15 J of energy are released when all of the new bonds have been formed. Is this an endothermic or an exothermic chemical


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PCC CH 100 - Study Notes

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