Chemistry A Final Exam Review Packet Fall 2016 The topics and questions on this review are intended to help you study for the final exam. The exam will include both multiple choice and short answer questions worth approximately 15% of your overall grade. Materials: #2 pencil, a calculator, your red reference sheet, and your periodic table. Cell phones are not allowed at any point during the final exam period. Unit 2: Parts of the Atom, Isotopes, Average Atomic Mass, and Nuclear Chemistry 2.1. Identify important features of the Billiard Ball, Plum Pudding, Rutherford, Bohr Planetary, and Quantum Mechanical models of the atom. 2.2. Describe similarities and differences between the Billiard Ball, Plum Pudding, Rutherford, Bohr Planetary, and Quantum Mechanical models of the atom. 2.3. Describe the parts of the atom including charge, relative mass, and location within the atom. 2.4. Given an element, use the Periodic Table to determine numbers of protons, neutrons, and electrons for a neutral atom. 2.5. Write shorthand notation to represent neutral atoms and ions. 2.6. Given shorthand notation for a neutral atom or ion, determine the numbers of protons, neutrons, and electrons present. 2.7. Identify similarities and differences between isotopes of an element. 2.10. Calculate the average atomic mass of an element given the mass and abundance of each stable isotope of the element. 2.11. Given shorthand notation, locate and plot a nucleus on a graph of n 0 versus p +. 2.12. On a graph of n 0 versus p + use the position of a plotted nucleus relative to the band of stability to predict the stability of a nucleus. 2.13. On a graph of n 0 versus p + use the position of a plotted nucleus relative to the band of stability to predict the type of decay the nucleus will undergo. 2.14. Given an isotope write a balanced nuclear equation for alpha, beta plus, beta minus, or gamma decay. 2.17. Determine whether an isotope undergoes fission, fusion, or alpha, beta plus, beta minus, or gamma decay when given a nuclear equation. 2.19. Balance a nuclear equation by writing the shorthand notation for a missing nucleus or subatomic particle. Unit 3: Bohr & Quantum Models, Electromagnetic Spectrum, Electron Configurations, and Periodic Trends 3.1. Compare different types of electromagnetic radiation in terms of wavelength, frequency, energy, and speed. 3.2. Complete calculations relating speed, wavelength, frequency, and energy of electromagnetic radiation. 3.6. Use the Periodic Table to write electron configurations (longhand) for neutral atoms of an element. 3.8. Use the electron configuration of an atom to determine the # of valence electrons. 3.9. Use the electron configuration of an atom to predict the most common oxidation state. 3.10. Use the Periodic Table to write electron configurations (longhand) for ions. 3.11. Use the Periodic Table to write shorthand electron configurations for neutral atoms and ions. 3.12. Use the periodic table to predict relative differences in atomic radius, ionization energy, and electronegativity for specific elements. 3.13. Use atomic structure (principle energy levels & nuclear charge) to explain why periodic trends in atomic radius, ionization energy, and electronegativity occur. Resources Chapter 5: Atomic Structure (pg. 106-126) Chapter 13: Electrons in Atoms (pg. 361 363) Learning Objectives and Vocabulary Atomic History: A Timeline Notes: Parts of the Atom Chapter 28: Nuclear Chemistry (pg. 848 856) Learning Objectives and Vocabulary Unit 2: Nuclear Chemistry Resources Chapter 13: Electrons and Light (pg. 363 379) Chapter 14: Periodic Trends (pg. 398 406) Learning Objectives and Vocabulary Notes: Bohr & Quantum Models, EM Spectrum, e Configurations, and Periodic Trends Reading: Light & the EM Spectrum
Unit 4: Ionic & Covalent Compounds 4.1. Determine the number of valence electrons for a neutral atom of an element using the Periodic Table. 4.2. Use the number of valence electrons and type of element (metal or nonmetal) to predict the common oxidation state. 4.3. Identify ions as cations or anions. 4.4. Write a neutral formula unit for the ionic compound formed from two ions. 4.5. Name an ionic compound given the formula. 4.6. Given a compound name or formula, determine the oxidation state of each ion within an ionic compound. 4.7. Write a neutral formula unit for an ionic compound given the compound name. 4.8. Predict whether two elements will form an ionic or covalent compound based on their location on the periodic table. 4.9. Describe the difference between ionic and covalent bonds in terms of how valence electrons are distributed. 4.10. Identify common physical properties of ionic and covalent compounds (physical state, relative melting point, solubility in water, conductivity of aqueous solutions). 4.11. Name a covalent compound given the formula. 4.12. Write the formula of a covalent compound given the compound name. 4.13. Identify and name diatomic elements. 4.14. Given a compound formula or name, classify the compound as ionic or covalent. Unit 4: Writing & Balancing Equations, and Reaction Types 4.15. Model chemical equations using a sketch. 4.16. Write a sentence to describe a chemical equation using correct names for substances and describing physical state. 4.17. Given a sentence describing a chemical reaction, write a chemical equation including correct formulas and an indication of physical state (s, l, g, aq). 4.18. Use coefficients to write a balanced chemical equation that demonstrates law of conservation of mass. 4.19. Identify patterns for the five reaction types: synthesis, decomposition, combustion, double-replacement, and single-replacement. 4.20. Identify reaction type given a complete chemical equation (reactants and products). 4.21. Identify reaction type given the reactants only. 4.22. Use reaction type to predict the products of synthesis, decomposition, combustion, double-replacement, and single-replacement reactions. 4.23. Use the periodic table to predict the phase (solid, liquid, gas) of an element. 4.24. Use the solubility guidelines to predict the phase (s, aq) of an ionic compound in water. Resources Chapters 6: Chemical Names and Formulas (pg. 133 163) Chapter 15: Ionic Bonding and Ionic Compounds (pg. 413 426) Learning Objectives and Vocabulary Notes: Types of Chemical Bonds - Ionic and Covalent Bonds Resources Chapter 8: Chemical Reactions (pg. 203 228) Notes: Chemical Reactions Investigating Patterns in Chemical Reactions Notes: Types of Chemical Reactions 4.25. Use the activity series to predict whether two reactants (element and compound) will undergo a single-replacement reaction. 4.26. Use observations of a chemical reaction to make conclusions about the products formed.
Atomic Structure and the Periodic Table: Ch 5 (pg. 106 126) and Ch 13 (361 363) 1. Sketch the 5 atomic models, labeling any important features. Describe the related experiments/evidence, list key features of the model, and note any modifications to previous models. Sketch Billiard Ball Model Experiments or Evidence Key Features Modifications to Previous Models Plum Pudding Model Rutherford Model Bohr Model Quantum Model 2. Explain how two isotopes of the same element are similar, and how they are different. 3. Complete the following table. Assume atoms are neutral unless the # of p + & e or symbol indicates otherwise. Shorthand Name Atomic # Mass Number # of protons # of neutrons # of electrons 34 32 16S 2 131 53I 29 14Si 4 197 79 4. What information is needed to calculate the average atomic mass of an element? 24 18 20 22 18
5. Calculate the average atomic mass of bromine. The two isotopes of bromine have atomic masses and relative abundances of 78.92 amu (50.69 %) and 80.92 amu (49.31 %). 6. Calculate the average atomic mass of lead using the following data for four lead isotopes. Show your work, and report the answer using the correct units. Isotope mass (amu) relative abundance (%) Pb-204 204 1.37 Pb-206 206 26.26 Pb-207 207 20.82 Pb-208 208 51.55 Nuclear Chemistry: Ch 28 (pg. 848-856) 7. Plot each of the isotopes listed below, and determine whether the nucleus is stable. If unstable, predict the type of decay. Isotope # p + #n 0 Stable or Unstable? Decay Type (α, β, β+, none) 154 60Nd 21 10Ne 78 39Y 251 97Bk 130 50Sn 206 82Pb 97 42Mo 102 49In 8. Write the balanced nuclear reaction for the α decay of Am-241. Number of Neutrons 150 140 130 120 110 100 90 80 70 60 50 40 30 Plot of Nuclear Stability 20 9. Write the balanced nuclear reaction for the β decay of Co-75. 10 0 10. Write the balanced nuclear reaction for the β+ decay of F-18. 0 10 20 30 40 50 60 70 80 90 100 110 Atomic Number (# of Protons) 11. Balance each of the following nuclear reactions by filling in the missing information. Identify the type of process (fusion, fission, alpha, beta-minus, beta-plus, or gamma) and write it in the box. 1 0n + 236 93 Np + 90 38 Sr + 10 1 0 n 12 6C + 16 8S 223 87Fr + 4 2 He 52 26Fe + +1 0 e + 0 0 γ 234 90Th + 234 91 Pa 208 82Pb + 62 28 Ni 1 0n + 235 92 U + 131 50 Sn + 2 1 0 n 230 90Th 230 90Th +
Light and Atomic Spectra: Notes (EM Spectrum) & Ch 13 (pg. 372 379) Refer to Figure 1 in the Light & Electromagnetic Radiation reading packet to answer the following questions. 12. Order the following in terms of increasing Energy. A. Infrared radiation from a heat lamp B. X-rays used in a dental office C. Signal from a shortwave radio D. Ultraviolet radiation from the sun 13. Now arrange the types of EM radiation in terms of increasing frequency: 14. Arrange the types of EM radiation in order of increasing wavelength: Use the equations on your red reference sheet to answer the following problems about light. 15. Calculate the frequency of light that has a wavelength of 6.56 10 7 m. 16. A mercury lamp emits radiation with a wavelength of 4.36 10 7 m. a. Calculate the frequency of this radiation. b. Calculate the energy of this radiation. 17. Calculate the energy of a photon of red light with a frequency 1.02 10 6 Hz. 18. Calculate the frequency of light with an energy of 2.35 10 15 J. Quantum Mechanical Model: Ch 13 (pg. 363 370) 19. These electron configurations have errors. Circle the errors and write the correct configurations. a.!"!"!" 1s 2s 2p b.!"!"!"!"!"!"!_!_ 1s 2s 2p 3s 3p c.!"!"!"!"!"!!!"!"!_ 1s 2s 2p 3s 3p d.!"!"!"!"!"!"!"!"!"!"!"!"!"!" 1s 2s 2p 3s 3p 3d 20. Write the longhand electron configuration and indicate the oxidation state and # of valence e for these atoms: # valence e - oxidation state a. Magnesium b. Sulfur c. Selenium
21. Write the longhand electron configurations and indicate number of valence electrons for the following ions: # valence e - a. Na 1+ b. Cl 1 c. Se 2 22. Write the shorthand electron configurations, and indicate oxidation state and # of valence e for the following: # valence e - oxidation state a. Arsenic b. Strontium c. Seaborgium 23. Write the shorthand electron configurations, and indicate the # of valence e for the following: # valence e - a. Po 4+ b. Sr 2+ c. Os 4+ Periodic Trends: Ch 14 (pg. 398 406) 24. Define the following terms, and list the factors that will cause them to increase or decrease. 25. Indicate which element in each pair has the greater atomic radius. a. Na or Li b. Sr or Mg c. C or Ge d. Se or O 26. Indicate which element in each pair has a higher 1st ionization energy. a. Li or B b. Mg or Ar c. Cs or Al d. Si or Pb 27. Indicate which element in each pair has a higher electronegativity. a. Cl or F b. C or N c. Mg or Sr d. As or Ca
Ionic and Covalent Compounds: Ch 6, 15.1 & 15.2 (pg. 133 163 and 413 426) 28. What is the charge on the ion typically formed by each element? a. O c. Na b. I b. Li 1+ d. Al d. P 3 e. Ni f. Mg 29. How many electrons does the neutral atom gain or lose to form the indicated ion? a. Cr 3+ c. Cl 1 e. Ca 2+ f. O 2 30. List the properties (phase, relative melting point, solubility, conductivity, etc.) of ionic & covalent compounds: Ionic Compounds Covalent Compounds 31. Complete this table by writing correct formulas and names for the compounds formed by combining the ions. O 2 OH PO 4 3 Ca 2+ Al 3+ Pb 4+ 32. Name the following compounds (HINT: Check to see if they are ionic or covalent first): K 2 CO 3 Cu(OH) 2 N 2 O 5 PI 3 NaCN FeCl 3 NBr 3 P 4 O 6 33. Write formulas for the following compounds: magnesium sulfate sodium hydroxide dinitrogen tetrafluoride sulfur dioxide dichlorine monoxide potassium dichromate tin(ii) fluoride nitrogen tribromide
Balancing Equations and Reaction Types: Ch 8 (Pg. 203 228) 34. Draw a model representing atoms and compounds for the following reactions. a.) 2P (s) + 5F 2 (g)! 2PF 5 (g) b.) 2C 2 H 2 (g) + 5O 2 (g)! 4CO 2 (g) + 2H 2 O (g) Write a sentence to describe each chemical equation given above. Correctly name each reactant and product and include the physical state. a.) b.) 35. Write 1-2 sentences explaining how the balanced chemical equations a and b in question 34 above demonstrate the law of conservation of mass. 36. Write a sentence to describe the following chemical equation. Correctly name each reactant and product and include physical states. Ca (s) + 2 H 2 O (l)! H 2 (g) + Ca(OH) 2 (s) 37. Write an equation to represent the reaction described by the following sentences. Compound formulas should be written correctly (neutral ionic compounds) and indicate the physical state (s, l, g, aq). Solid iron and oxygen gas react to produce solid iron(iii) oxide. Solid copper reacts with aqueous hydrogen nitrate to produce aqueous copper(ii) nitrate, liquid dihydrogen monoxide, and nitrogen dioxide gas. 38. Use the solubility guidelines, identify each of the following as soluble (aq) or insoluble (s) in water. Ca 3 (PO 4 ) 2 BaCO 3 KCl CdS (NH 4 ) 3 PO 4 Cr(SO 4 ) 3 AgCl Co(NO 3 ) 3 Al(C 2 H 3 O 2 ) 3 H 2 SO 3 CaSO 4 AlPO 4
39. For each of the following double-replacement reactions, predict the products, indicate the physical state of each product (s, l, g, or aq) according to the solubility chart, and balance the chemical equation. K 2 SO 4 (aq) + AlCl 3 (aq)! ( ) + ( ) BaCl 2 (aq) + Cu 2 SO 4 (aq)! ( ) + ( ) NaOH (aq) + H 3 PO 4 (aq)! ( ) + ( ) 40. Use the Activity Series to predict whether each of the following reactions occurs. If there is no reaction, indicate this by writing no reaction. For reactions that do occur, predict the products, balance the chemical equation, and indicate the physical state (s, l, g, aq) for each product. Au (s) + KNO 3 (aq)! Mg (s) + H 2 SO 4 (aq)! Cu (s) + H 2 O (l)! Al (s) + CuSO 4 (aq)! Br 2 (l) + MgF 2 (aq)! Na (s) + H 2 O (l)! Co (s) + Ba(ClO 3 ) 2 (aq)! Cl 2 (g) + ZrI 4 (aq)! 41. Balance the following chemical equations and identify each reaction type: Reaction Type: Fe(OH) 3 (s)! Fe 2 O 3 (s) + H 2 O (l) Li (s) + O 2 (g)! Li 2 O (s) Li (s) + Fe 2 O 3 (s)! Fe (s) + Li 2 O (aq) Al (s) + CuSO 4 (aq)! Al 2 (SO 4 ) 3 (aq) + Cu (s) NaCl (aq) + H 2 SO 4 (aq)! Na 2 SO 4 (g) + HCl (aq) C 3 H 8 O (l) + O 2 (g)! CO 2 (g) + H 2 O (g)
42. The reactants for different chemical reactions are given below. Complete the following steps: Step 1: Label the types of reactions. Step 2: Predict the product(s) and write the correct neutral formulas. Step 3: Indicate physical state of each product. Step 4: Balance the chemical equations using coefficients. Type of Reaction: Mg (s) + Al(NO 3 ) 3 (aq)! Na 2 CO 3 (aq) + NH 4 OH (aq)! HCl (aq) + Ca(OH) 2 (s)! SF 6 (g)! Ca (s) + Cl 2 (g)! C 4 H 10 O (l) + O 2 (g)! K (s) + H 2 O (l)! C 4 H 10 (g) + O 2 (g)! Pb (s) + FeCl 3 (aq)! Ga (s) + O 2 (g)! Al(OH) 3 (s) + HC 2 H 3 O 2 (aq)! Co (s) + H 2 SO 4 (aq)! cobalt(ii) ion