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Quarterly Study-guide-MP2- CP Chem M Bonding-Naming and properties for Ionic and Covalent Bonding, Lewis structures and shapes Chapter 7-8-9 Multiple Choice: Identify the choice that best completes the statement or answers the question. 1. Which of these is the correct Lewis Dot Diagram for Calcium? a. b. c. d. a b c d e. f. g. h. e f g h 2. Which of these is the correct Lewis Dot Diagram for Chlorine? a. b. c. d. a b c d e. f. g. h. 3.Which is the charge that results when magnesium becomes an ion? a. +2 c. +3 b. -3 d. -2 4. Which is the correct formula for the compound formed between beryllium and nitrogen? a. BeN c. Be3N2 b. Be3N d. Be2N3 5. What is the correct formula for the compound formed between magnesium and the phosphate ion? a. MgPO4 c. Mg3(PO4)2 e f g h b. Mg3PO2 d. MgP2O8 6. Which is the correct name for the compound CoCO3? a. Carbon Oxygen c. Cobalt Carbonate Carbonate b. Cobalt (II) Carbonate d. Cobalt Carbonoxide 7. What is the formula unit of sodium nitride? a. NaN c. Na N b. Na N d. NaN 8. What is the name of the ionic compound formed from potassium and chlorine? a. potassium chlorine c. potassium chloride 9. 10. 11. 12. 13. 14. 15. 16. 17. b. potassium chlorium d. potassium chlorate An ionic bond is a bond between ____. a. a cation and an anion c. the ions of two different metals b. valence electrons and d. the ions of two cations different nonmetals Which of the following is true about the melting temperature of potassium chloride? a. The melting temperature is relatively high. b. The melting temperature is variable and unpredictable. c. The melting temperature is relatively low. d. Potassium chloride does not melt. Which of the following pairs of elements is most likely to form a covalent compound? a. magnesium and c. oxygen and chlorine fluorine d. sodium and b. lithium and bromine aluminuim Which is a physical property of ionic compounds in their solid state? a. good conductor of electricity b. weak attractive forces between ions c. low boiling point d. high melting point Under what conditions can potassium bromide conduct electricity? a. only when melted b. only when dissolved c. only when it is in crystal form d. only when melted or dissolved in water Covalent compounds display which of these properties? a. They are hard, brittle solids b. They have high melting and boiling points c. They display luster. d. Their intermolecular forces are relatively weak. Which is the correct name for the compound N2O4? a. tetranitrogen dioxide c. dinitrogen quadoxide b. dinitrogen tetroxide d. nitrogen oxide Which is the formula for the compound sulfur hexachloride? a. S6Cl c. SCl5 b. SCl6 d. S2Cl3 How do atoms achieve noble-gas electron configurations in single covalent bonds? a. One atom completely loses two electrons to the other atom in the bond. b. Two atoms share two pairs of electrons. c. Two atoms share two electrons. d. Two atoms share one electron. 18. How many covalent bonds are formed between two iodine atoms? a. 1 c. 3 b. 2 d. 4 19. Which of the following elements can form diatomic molecules held together by triple covalent bonds? a. carbon b. oxygen c. fluorine d. nitrogen 20. What molecular shape does the compound CBr4 have? a. trigonal planar c. linear b. tetrahedral d. bent 21. Choose the correct molecular geometries for the following molecules or ions below a. linear c. trigonal planar b. bent d. tetrahedral 22. Why do atoms share electrons in covalent bonds? a. to become ions and attract each other b. to attain a noble-gas electron configuration c. to become more polar d. to increase their atomic numbers 23. Which molecule has a single covalent bond? a. CO b. Cl c. CO d. N 24. What causes water molecules to have a bent shape, according to VSEPR theory? a. repulsive forces between unshared pairs of electrons b. interaction between the fixed orbitals of the unshared pairs of oxygen c. ionic attraction and repulsion d. the unusual location of the free electrons 25. What is the shape of a molecule with a triple bond? a. tetrahedral b. pyramidal c. bent d. linear 26. Which of the following compounds contains the Mn ion? a. MnS b. MnBr c. Mn O d. MnO 27. Which of the following formulas represents an ionic compound? a. CS b. BaI c. N O d. PCl 28. Which of the following shows correctly an ion pair and the ionic compound the two ions form? a. Sn , N ; Sn N b. Cu , O ; Cu O c. Cr , I ; CrI d. Fe , O ; Fe O 29. In which of the following is the name and formula given correctly? a. sodium oxide, NaO b. barium nitride, BaN c. cobaltous chloride, CoCl d. stannic fluoride, SnF 30. Which of the following compounds contains the lead(II) ion? a. PbO b. PbCl4 c. Pb2O d. Pb2S 31. Which of the following correctly shows a prefix used in naming binary molecular compounds with its corresponding number? a. deca-, 7 b. nona-, 9 c. hexa-, 8 d. octa-, 4 Numeric Response 32. How many electrons are shared in a single covalent bond? 33. How many unshared pairs of electrons does the nitrogen atom in ammonia (NH3) possess? CHEMISTRY TEST STUDY GUIDE Ch. 11 – Chemical Reactions Read over your notes, and rework your homework assignments, labs, quizzes, and tests. You will do AWESOME on this test if you can do the following things. Introduction to Chemical Reactions • Know the difference between a skeleton equation and a balanced equation. • Explain how the law of conservation of mass relates to atoms in a chemical reaction. • Know where chemical reactions take place-Everywhere! Balancing Equations • Balance a written chemical equation. • Translate and balance word equations (including states). Types of Reactions • Identify the type of reaction. IDENTIFY THE TYPE OF THE REACTION, THEN BALANCE THE REACTION 1) ___Sb + ___I2 → ___SbI3 2) ___Li + ___H2O → ___LiOH + ___H2 3) ___AlCl3 → ___Al + ___Cl2 4) ___C6H12 + ___O2 → ___CO2 + ___H2O 5) ___AlCl3 + ___Na2CO3 → ___Al2(CO3)3 + ___NaCl 6) ___HNO3 + ___Ba(OH)2 → ___Ba(NO3)2 + ___H2O 7) ___Al + ___Pb(NO3)2 → ___Al(NO3)3 + ___Pb WORD TO FORMULA, THEN IDENTIFY THE TYPE OF REACTION, THEN BALANCE. 8) Aqueous solutions of ammonium chloride and lead(II) nitrate produce lead(II) chloride precipitate and aqueous ammonium nitrate. 9) Iron metal reacts with aqueous silver (I) nitrate to produce aqueous iron(III) nitrate and silver metal. 10) Solid potassium nitrate yields solid potassium nitrite and oxygen gas. 11) Calcium metal reacts with chlorine gas to produce solid calcium chloride. 12) Fluorine gas added to aqueous potassium chloride produces aqueous potassium fluoride and chlorine gas. 13) Phosphorous reacts with oxygen gas to produce solid diphosphorous pentoxide. Chemical Reactions Review – Ch. 8 ANSWER KEY 1. synthesis 2Sb + 3I2 → 2SbI3 2. single replacement 2Li + 2H2O → 2LiOH + H2 3. decomposition 2AlCl3 → 2Al + 3Cl2 4. combustion C6H12 + 9O2 → 6CO2 + 6H2O 5. double replacement 2AlCl3 + 3Na2CO3 → Al2(CO3)3 + 6NaCl 6. double replacement 2HNO3 + Ba(OH)2 → Ba(NO3)2 + 2H2O 7. single replacement 2Al + 3Pb(NO3)2 → 2Al(NO3)3 + 3Pb 8. double replacement 2NH4Cl(aq) + Pb(NO3)2(aq) → PbCl2(s) + 2NH4NO3(aq) 9. single replacement Fe(s) + 3AgNO3(aq) → Fe(NO3)3(aq) + 3Ag(s) 10. decomposition 2KNO3(s) → 2KNO2(s) + O2(g) 11. synthesis Ca(s) + Cl2(g) → CaCl2(s) 12. single replacement F2(g) + 2KCl(aq) → 2KF(aq) + Cl2(g) 13. synthesis 4P(s) + 5O2(g) → 2P2O5(s) Moles and Moles Calculations Chapter 10: Section 10.1: All Section 10.2: Does not include mole-volume of gas. Vocabulary: Mole 1 mole = 1 molar mass (g) 1 mole = 6.02 x 1023 representative particles Molar Mass (also known as formula mass Avagadro’s Number Representative Particles (molecules, atoms etc) Skills and Mathematical Operations: a. Convert moles to mass and mass to moles b. Convert moles to number of representative particles and number of particles to moles. c. Convert mass to number of particles and number of particles to mass. Mole Road Map: Mass mole particle Hint: Review prior worksheets and quizzes. Pay attention to the units of the numbers in the problems. Remember, you are only solving ratios. Problems: 1. How many moles are in 220 g of CO2? 2. One mole of (NH4)2HPO4 contains _?_ moles of hydrogen atoms. 3. The atomic mass of sodium is 23. The number of moles in 46g of sodium is ________. 4. The molar mass of ammonia is _________. 5. What is the number of molecules in 4.25 g of ammonia? 6. How many grams of sulfur dioxide are there in 1.20 x 1024 molecules of the compound? 7. How many moles are in 45 molecules of NH3? Answers: 1. 4 moles moles 2. 9 moles 3. 2 moles 4. 17 5. 1.5 x 1023 moleules 6. 128 g 7. 7.5 x 10-23 Stoichiometry Chapter 12 Section 12.1 Section 12.2 Does not include volume-volume calculations. Do understand molecules of product. Skills: a. Reading balanced chemical reactions. b. Using the coefficients in the reaction to determine mole relationships between different substances in the reaction. c. Calculate moles from mass and mass from moles. d. Use coefficients from reaction to relate moles. Sample Problems: 1. Calculate the number of moles of hydrogen chloride produced from 10 moles of hydrogen. H2(g) + Cl2(g) → 2HCl(g) 2. Calculate the number of moles of chlorine needed to form 14 moles of iron(III) chloride. 2Fe(s) + 3Cl2(g) → 2FeCl3(s) 3. Calculate the number of grams of nitrogen dioxide that are produced from 4 moles of nitric oxide. 2NO(g) + O2(g) → 2NO2(g) 4. Calculate the mass of oxygen produced from the decomposition of 75.0 g of potassium chlorate. 2KClO3(s) → 2KCl(s) + 3O2(g) 5. Calculate the mass of silver needed to react with chlorine to produce 84 g of silver chloride. 2Ag(s) + Cl2(g) 2AgCl(s) Answers: 1. 20 moles 2. 21 moles 3. 184 g 4. 29.5 g 5. 63.4 g