CHEM 1410 Final Exam Review PDF

CHEM 1410 – FINAL EXAM REVIEW Please use the Final Exam Provided Information on Canvas, which will be given to use on the final exam. You will also be given the VSEPR Table and the Periodic Table. This review is NOT all encompassing – it is simply meant to be a reminder for content to go back and s...

CHEM 1410 – FINAL EXAM REVIEW Please use the Final Exam Provided Information on Canvas, which will be given to use on the final exam. You will also be given the VSEPR Table and the Periodic Table. This review is NOT all encompassing – it is simply meant to be a reminder for content to go back and study in greater detail. It is HIGHLY recommended that you review the four regular-semester exams in preparation for the cumulative final exam. I also recommend reviewing recitation packets, exam review packets, and quizzes. 1. Consider MgF2 and answer the following questions: Part A: Is it ionic or covalent? How do you know? Part B: What is the systematic name for this compound? Part C: What charges are present on these ions? Part D: Is it soluble in water? Part E: Write the electronic configuration for Mg and for F. 2. How many grams of H2O are formed by complete conversion of 32.00 g O2 with excess H2 according to the following equation: 2 H2 + O2 → 2 H2O 3. Which molecule contains a triple bond? Draw each Lewis structure to confirm. (A) F2 (B) Cl2 (C) O2 (D) I2 (E) N2 4. Write total and net ionic equation for the following reaction. Identify the spectator ions. 3CaCl2 (aq) + 2 K3PO4 (aq) → Ca3(PO4)2 (s) + 6 KCl (aq) 1 5. When you run a reaction in a lab, you use a calorimeter to determine that 216 kJ of heat is absorbed. Pick the correct statement below. a. the reaction is exothermic; ΔH = +216 kJ b. the reaction is endothermic; ΔH = -216 kJ c. the reaction is exothermic; ΔH = -216 kJ d. the reaction is endothermic; ΔH = +216 kJ e. the reaction will not run because of the heat required 6. What would ∆H° (in kJ) be for the production of 75.00 g of Al2O3(s)? 4Al (s) + 3O2 (g) → 2Al2O3 (s) ∆H° = - 3351 kJ 7. If 7.30 g of HCl and 4.00 g of NH3 are mixed, how many grams of NH4Cl can be formed? [MM: HCl = 36.5 g/mol; NH3 = 17.0 g/mol; NH4Cl = 53.5 g/mol] HCl(g) + NH3(g) → NH4Cl(s) How much remains of the excess reactant? 8. What are the stoichiometric coefficients needed to balance the following reaction: ____ CH4 + ____ O2 → ____ CO2 + ____ H2O 9. What is the oxidation number for phosphorus in H3PO4? 2 10. Choose the correct 4 quantum numbers for the unpaired electron of aluminum. Write why the others might be incorrect (i.e., doesn’t follow the rules of assigning quantum numbers, correspond to a different electron, etc.) a. n = 3, l = 0, ml = +2, ms = + ½ b. n = 1, l = 5, ml = -1, ms = + ½ c. n = 2, l = 0, ml = 0, ms = 1 d. n = 3, l = 1, ml = +1, ms = + ½ e. n = 2, l = 1, ml = +1, ms = 1 11. Based on the reaction below, which statement is false? N2 (g) + 3 H2 (g)  2 NH3 (g) ∆H = - 46.11 kJ a. The reaction as written is endothermic. b. For the reverse reaction, ∆H° =+46.11 kJ c. 1 mole nitrogen reacts with 3 moles hydrogen to form 2 moles ammonia. d. The reaction as written is exothermic. e. This is the thermochemical equation for the formation of ammonia. 12. Which of the following is an example of a chemical change? a. Condensing water vapor in the air to dew b. Boiling water c. Melting wax d. Broiling a steak on a grill e. Mixing salt and sugar 13. Which of the following statements is correct about covalently bound atoms? Fix the statements that are incorrect. a. 2 electrons cannot be shared unequally between two atoms. b. 4 electrons can be shared equally between the two atoms. c. It is an electrostatic attraction between two oppositely charged ions. d. The electrons avoid a space called the overlap region of two orbitals. e. A covalent bond occurs when one electron is completely transferred from one atom to another. 14. Convert the following: 5.7x105 µg = ____ mg ? 3 15. Which ionic formula is incorrect? Fix it. a. NaCO3 b. KNO2 c. Sr(CN)2 d. (NH4)2SO4 e. NH4Cl 16. How many σ and π bonds are in the following: a. Single bond b. Double bond c. Triple bond 17. If you have 2.7 grams of KBr [MM = 119 g/mol], how many mL of water are needed to make a 3.6 M solution? 18. Consider the following reaction: Fe (s) + Cu2+ (aq) → Fe2+ (aq) + Cu (s). Which species in this reaction is being oxidized and which species is being reduced? a. Cu = oxidized; Fe = reduced b. Cu2+ = oxidized; Fe2+ = reduced c. Fe = oxidized; Cu2+ = reduced d. Cu2+ = oxidized; Cu = reduced e. None, this is not a redox reaction. 19. Consider P2S5 and answer the following questions. Part A: Is it ionic or covalent? How do you know? Part B: What is the systematic name for this compound? Part C: Write the electron configuration for P and S. Part D: Draw the orbital energy diagram for the valence electrons for P and S (in the shell n = 3). 4 20. What is the electron domain geometry and molecular geometry for NH3? Draw both the 3D shape and the Lewis structure. What is the hybridization of the orbitals around the central atom? How many lone pairs of electrons will you find on the central atom? 21. Predict the products for the following, remembering to balance the equation and write the appropriate phases: BaCl2 (aq) + K2SO4 (aq) → ? 22. The value of ∆H° for the following reaction is -72 kJ. How many kJ of heat will be evolved when 3.0 g of HBr is formed in this reaction? H2(g) + Br2(g) → 2HBr(g) 23. A neutral molecule has the general form AX2E. What is the orbital hybridization (sp, sp2, or sp3) of A? 24. A photon of light A has a longer wavelength than light B. Light A has: a. a higher frequency. b. a greater velocity. c. lower energy. d. a shorter wavelength. e. more joules contained in it. 25. What volume does 2.5 grams of carbon dioxide occupy at 293 K and 0.984 atm? 5 26. How many grams of NaCl are contained in 500 mL of 0.40 M NaCl? 27. What is the frequency of electromagnetic radiation with a wavelength of 530 mm? 28. Which of the following molecules cannot participate in hydrogen bonding? Why not? a. CH3OH b. HF c. NH3 d. CH3OCH3 e. H2O 29. A 1200 mL sample of helium gas is at a pressure of 350 mmHg and a temperature of 300 K. What volume (in mL) will this gas sample occupy if the pressure is increased to 700 mmHg and the temperature is increased to 400 K? 30. Which statement about Lewis structures is correct? a. When a cation is made, one must add electrons to the count of valence electrons. b. All elements must obey the octet rule. c. The element beryllium will have 2 valence electrons. d. One must remove electrons from the count of valence electrons when an anion is made. e. Lewis structures are a 3D representation of a molecule. 31. Write the formation reaction of CH3CH2OH (l). 32. How many hydrogen atoms are there in a 0.500 g sample of methane, CH4? 6 33. Identify the atom based on the electron configuration: 1s2 2s2 2p6 3s2 3p5. Draw the Lewis dot symbol for the element. How many protons, neutrons, and electrons are present a neutral atom of this element? Write this in the complete atomic symbol format. 34. Which of the following molecules is nonpolar? Draw the VSEPR structures and show your dipole arrows to prove it. a. CHF3 b. NF3 c. BF3 d. H2O e. HCN 35. Write the full electron configuration and noble gas configuration for calcium? 36. Consider PCl5. Part A: Write the full electron configuration for P and Cl. Part B: Write the noble gas configuration for P and Cl. Part C: How many electrons does P need for a full octet? How about Cl? Part D: Do P and Cl transfer electrons or share electrons when in a bond? Part E: Is this an ionic or covalent bond? Part F: Name the compound. 7  Part G: Draw the Lewis structure for the compound. Part H: Calculate the formal charge for P and one Cl atom. Part I: Draw the VSEPR structure for the compound. i. What is the name of the electron domain geometry? ii. What is the name of the molecular geometry? iii. What are the ideal bond angles in the molecule? iv. Is the molecule polar or nonpolar? 37. Consider acetylene: C2H2. Part A: Is this an ionic or covalent molecule? Part B: Draw the Lewis structure. Part C: What is the orbital hybridization for each carbon? How do you know? Part D: Label the sigma and pi bonds in the molecule. Part E: If it takes one photon of wavelength 750 nm to excite an electron in acetylene, what is the energy of this photon? What is the frequency of the photon? 8 38. Solutions of cadmium sulfate and potassium sulfide are mixed together. (Cadmium has a charge of +2) Part A: Write the reaction, including phases, for this reaction. What products, if any, will be formed from mixing these solutions? Part B: Write the total ionic equation. Part C: Identify the spectator ions, if any are present. Part D: Write the net ionic equation for the reaction. Part E: How many moles of CdSO4 are in 750.0 mL of 0.850 M CdSO4? 9