1. Preparing for ACS Exam Preparing for ACS Exam General Chemistry -1 (1411) Dr. Vinu Johnson, Ph.D. Chemistry Faculty

2. What I will talk about this morning: Exam details Exam giving strategies Exam preparation Review of main concepts Credit: Quotesgram.com

3. Exam Details: 70 Questions with four answer choices 110 minutes = 1.57 minutes per question ! Serial number Sign Check-in form at the beginning of the exam. Sign Check-out form at the end of the exam. DO NOT MARK OR WRITE ON THE EXAM BOOKLET. THERE WILL BE A PENALTY IF YOU DO SO !!!

4. Exam giving strategies: You will face 3 categories of questions: 1.Certain 2.50/50 3.Clueless Make these 3 categories on a scratch paper Read the question carefully – Time Management. Based on your confidence write that Q# in one of the three categories. If it is a “certain” answer, mark it on the scantron form. If not, skip the question.

5. Exam giving strategies: Scantron form: Use a good condition form. Check the Question number. Mark the box completely Erase completely if selecting another answer choice. √

6. Exam Preparation: Every Chapter has a Summary section at the end – look at it. Start from first chapter – look at your notes. Refer to the handout of what you should know from each chapter. Work out at least one example of that topic. Practice giving tests. http://antoine.frostburg.edu/chem/senese/101/101-sample-exam-1a.shtml http://www.sciencegeek.net/Chemistry/taters/directory.shtml http://chelsinicole.hubpages.com/hub/Preparing-for-the-American-Chemical- Society-General-Chemistry-Exam http://chelsinicole.hubpages.com/hub/Preparing-for-the-American-Chemical- Society-General-Chemistry-Exam http://mhchem.org/223/classroom/wlExACS.htm

7. Exam Preparation: On the day of Exam: Relax - STRESS is a Memory Buster ! Psych yourself up – be CONFIDENT. Close your eyes and revise the concepts. Leave early (consider any traffic delays) Be sure to bring a scantron form, calculator & pencil. Be sure to have snacked / cup of coffee to keep your energy level up. Do breathing exercise if you feel anxious. National Education Association (nea.org)

8. Review of Concepts

9. Analytical & problem solving skills Which of the above pictures best represents a solid ionic compound? A) picture (a) B) picture (b) C) picture (c) D) picture (d) Which of the above pictures best represents a gaseous covalent compound?

10. Analytical & problem solving skills Which of the following underlined items is not an extensive property? A) the volume of a glucose solution B) the diameter of a soap bubble C) the mass of a diamond D) the color of a cobalt compound

11. CHAPTER 0 MATTER AND ENERGY States of matter / Forms of Energy / Classes of matter Properties of matter : Physical vs Chemical Density SI unit, conversions Scientific notations versus standard notations Interconversion of temperature units Significant numbers – rules Dimensional analysis Dimensional analysis 2 -3 Questions

12. CHAPTER 1 ATOMS, IONS & MOLECULES Structure of atom Isotopes Atomic number, Mass number, Atomic Mass. Moles & Molar Masses 2 -3 Questions

13. CHAPTER 2 ATOMIC STRUCTURE Waves and related definitions Wave equation, Energy of photon Quantum numbers Rules governing orbital filling Effective nuclear charge Z eff Electronic configurations Atomic radii, electronegativity. 7 Questions

14. CHAPTER 3 IONIC BONDS AND SOME MAIN-GROUP CHEMISTRY Atom, ions, polyatomic ions. Intramolecular bonds : Ionic versus Covalent. Elements that tend to lose electrons versus that gains them Radii of neutral versus charged monoatomic ions. Ionization energy, predict ionization energy difference. Give the formulas and names of a) common cations and anions, b) polyatomic ions, c) ionic compounds. 3 – 4 Questions

15. CHAPTER 4 COVALENT BONDS Define bond dissociation energy, D. From a list of compounds, predict which are ionic and which are molecular. Relate electronegativity to electron affinity and ionization energy. Write electron-dot symbols for atoms, and tell how many electrons must be shared to enable the atom to achieve a completed valence shell. Give the symbol of the noble gas with the same number of valence electrons. Draw electron-dot structures for polyatomic molecules and ions, recognizing when multiple bonding is needed. Resonance structure, formal charge. 3 – 4 Questions

16. CHAPTER 5 MOLECULAR SHAPES VSEPR model to predict the geometries of molecules and polyatomic ions. Hybridization Hybridization: sp 3 hybrid orbitals vs sp 2 hybrid orbitals vs sp hybrid orbitals. 5 – 6 Questions

17. CHAPTER 6 MASS RELATIONSHIPS IN CHEMICAL REACTIONS For simple chemical reactions, write and balance chemical equations. formula of a compound Calculate molar mass. Interconvert grams, moles, and numbers of formula units. Determine the number of moles and grams of one reactant needed to react with a given number of moles and grams of another reactant and the number of moles and grams of product(s) that result from the reaction. Calculate percent yield. Identify the limiting and excess reagents in a reaction mixture. how to prepare a solution of known molarity by dissolving a solid in a solvent. how to prepare a solution of known molarity by diluting a more concentrated solution. Interconvert solution molarity, solution volume, solute moles, and solute grams Determine the percent composition and empirical formula of a compound 6 – 8 Questions

18. CHAPTER 7 REACTIONS IN AQUEOUS SOLUTION Classify reactions as precipitation, acid-base neutralization, or redox. Classify substances as strong electrolytes, weak electrolytes, or nonelectrolytes Write molecular, ionic, and net ionic equations for precipitation, acid-base, and redox reactions Use solubility guidelines to determine whether a compound is likely to be soluble in water. solubility guidelines to predict the product of a precipitation reaction. Identify the common strong acids and strong bases. Assign oxidation numbers to each atom in a chemical species. Use the activity series to predict whether a redox reaction will occur. 7 – 9 Questions

19. CHAPTER 8 THERMOCHEMISTRY: CHEMICAL ENERGY Define energy. Potential and kinetic energy. concepts of heat and temperature Define and calculate PV work. Know whether work is being done by the system or on the system. Differentiate between energy and enthalpy, and perform calculations interconverting the two.  H vs  E. Given a balanced chemical equation and enthalpy change for a chemical reaction, calculate the enthalpy change per mole or per gram of each reactant and product Perform calculations involving specific heat (or molar heat capacity), heat flow, and temperature change, Specific Heat. Enthalpy calculations based on Hess Law, Heats of formation, Bond Dissociation 6 – 7 Questions

20. CHAPTER 9 GASES: THEIR PROPERTIES AND BEHAVIOR Perform calculations converting between different units of pressure Determine the pressure of a gas using an open-end manometer. Understand visual representations of the gas laws. the ideal gas law to calculate pressure, volume, moles of gas, or temperature, given the other three variables. Perform stoichiometric calculations relating the mass of a reactant to the mass, moles, and volume or pressure of a gaseous product. Daltons law of Partial Pressure, Rate of diffusion. 7 Questions