Chemistry 40S Exam Review Fall 2023 PDF

Chemistry 40S EXAM REVIEW This package gives you a sampling of long-answer questions from each of the units we covered this year. It DOES NOT cover all the theory, so be sure to use your NOTES as well. Remember, your unit outcomes (what you should know) are on t...

Chemistry 40S EXAM REVIEW This package gives you a sampling of long-answer questions from each of the units we covered this year. It DOES NOT cover all the theory, so be sure to use your NOTES as well. Remember, your unit outcomes (what you should know) are on the front of each unit booklet. Also use tests and quizzes to help you prepare. Topics Covered: Oxidation and Reduction and Electrochemistry: oxidation numbers, oxidizing agents and reducing agents balancing half and full redox reactions in acidic or basic solutions electrolytic cells, electroplating and Faraday's calculations electrochemical cells and corrosion Chemical Kinetics: reaction rates and factors affecting rates the collision theory reaction mechanisms P.E. diagrams: catalyzed and uncatalyzed rate laws, reaction orders Chemical Equilibrium and Ksp: mass action expressions, kc and kp % yield of product ICE charts Le Chateliers principle graph interpretation and drawing ([ ] vs time) calculating ksp or molar solubilities effect of a common ion on solubility determining whether or not a precipitate will form Acids and Bases: electrolytes vs nonelectrolytes Arrhenius vs Bronsted Lowry Definitions Conjugate Acid-Base Pairs Self Ionization of Water (Kw) / Ionization Constants, Ka and Kb pH scale and calculations of pH, pOH, [H+], [OH-] Indicators Neutralization problems Titrations Atomic Structure: quantum mechanical model of the atom electron configurations and orbital diagrams wavelength, frequency and energy calculations spectra (continuous vs. bright line) periodic trends (atomic and ionic radii, ionization energy and electronegativity)  Electrochemistry 1. For the following reactions: - Give the oxidation numbers of all the elements involved - identify the elements being oxidized and reduced - identify the oxidizing agent and the reducing agent a. Mn02 + 4 HCl → MnCl2 + Cl2 + 2 H2O b. 2 CrO2- + CIO- + OH- → 2 CrO42- + 3 Cl- + H20 2. Balance the following half reactions: a. MnO4- → Mn2O3 (acidic solution) b. As04-3 → AsO2- (basic) 3. Refer to your half-reaction table to determine if a spontaneous reaction will occur when the following are mixed together. If a reaction does occur, write the products of the reaction. a. Ni2+ + Al b. Ag + Cu2+ c. Sn + I- d. Li + Zn2+ 4. Will the following reaction proceed spontaneously? Cr2O72- + Fe2+ + 14 H+ → 2 Cr3+ + 6 Fe3+ + 7 H20 5. Balance the following redox reactions using either the half-cell method or the oxidation number method. a. Sb2O5 + I- → Sb3+ + I2 (acidic) b. Cr(OH)3 + Cl0- + OH- → CrO42-+ CI- (basic) c. H2C2O4 + Cr207-2 → CO2 + Cr3+ (acidic) 6. For the example: Cr(s) + Pb2+ → Cr3+ + Pb(s) a. Draw an electrochemical cell that utilizes the above reaction. b. Write each half-reaction. c. Label the anode and cathode. d. Write a balanced equation. e. Indicate the direction of electron flow. f. Calculate the voltage. 7. Calculate the E° value of the following reactions and predict if the reaction is spontaneous in the forward or reverse direction: a. Mn02 + 4H+ + 2 CI- → Mn2+ + Cl2 + 2 H2O b. 2 Fe3+ + 2 I- → 2 Fe2+ + l2(s) 8. Aqueous NaI is electrolyzed. a. Write the equation for both the reduction and the oxidation. b. Write the overall equation and calculate the minimum voltage necessary for the reaction to proceed. c. Describe any change in pH as the reaction proceeds. 9. An aqueous solution contains K+, Ni2+, Zn2+, Cu2+, Al3+. Which ions can be extracted by electrolysis of the solution? 10. How would you construct an electrolytic cell to plate a cheap metal in chromium? Label the anode, cathode, and electrolyte. Give the two half reactions. 11. If a current of 5.00 A is run for 25 minutes, what mass of nickel could be deposited from a solution of Ni(NO3)2? 12. For what length of time must a 3.50 A current run in order to deposit 20.0 g of Cu (s) from a solution of Cu(NO3)2?  Electrochemistry Answers 1a. Mn02 + 4 HCl → MnCl2 + Cl2 + 2 H2O Mn+4 is reduced/ O.A. +4 -2 +1 -1 +2 -1 0 +1 -2 Cl- is oxidized / R.A. b. 2 CrO2- + CIO- + OH- → 2 CrO42- + 3 Cl- + H20 Cr+3 is oxidized/R.A. +3 -2 +1 -2 -2+1 +6 -2 -1 +1 -2 Cl+ is reduced/O.A. 2 a. 10 H+ + 2MnO4- + 8e- → Mn2O3 + 5H2O b. 2H2O +As04-3 + 2e- → AsO2- + 4OH- 3. a. Ni2+ + Al spont. (Ni and Al3+) b. Ag + Cu2+ nonspont. c. Sn + I- no rxn. d. Li + Zn2+ spont. (Li+ and Zn) 4. spontaneous reaction. 5. a. 10H++Sb2O5+ 4I-→ 2Sb3++2I2+5 H2O b. 3 OH-+2Cr(OH)3+3Cl0- +OH- →2CrO42-+3CI-+5H2O c. 8H+ + 3H2C2O4 + Cr207-2 → 6CO2 + 2Cr3+ + 7H20 6. For the example: Cr(s) + Pb2+ → Cr3+ + Pb(s) anode e- cathode Cr Pb Oxidation; Cr → Cr3+ + 3e- (Eo= -0.74 V) Reduction: Pb2+ + 2e- → Pb (Eo= -0.13V) Pb2+ Redox: 2Cr + 3Pb2+ → 2Cr3+ + 3Pb Eo = +0.61V NO3- Cr3+ NO3- 7. a. Eo = -0.14V – nonspontaneous b. Eo = +0.23V - spontaneous 8. a. Reduction: 2H2O + 2e- → 2OH- + H2 Oxidation: 2I- → I2 + 2e- b. Redox: 2H2O + 2I- → 2OH- + H2 + I2 E0 = - 1.37 V c. OH- is produced as the reaction proceeds. pH will increase as the mixture becomes more basic. 9. Cu2+ ions will be reduced to Cu. 10. anode cathode cheap metal Cr Reduction: Cr3+ + 3e- → Cr Oxidation: Cr → Cr3+ + 3e- Cr3+ NO3- 11. Mass = 2.29 g 12. t=289.5 min  Kinetics 1. State 5 factors that determine the rate of a chemical reaction. 2. State the collision theory of chemical reaction. 3. According to the collision theory reaction rate depends on what two factors? 4. What two factors determine the effectiveness of a collision? 5.What is a reaction mechanism? 6. What is the rate determining step in a reaction mechanism? 7. Derive a possible reaction mechanism for the overall reaction:2A2B + C2D2 → 2 CB + 2A2D 8. For the following reaction mechanism, determine the overall reaction and identify any catalysts and intermediates. 2A + B → AB + A AB +C → ABC ABC + C → AC2 +B AC + AC → A2C +C 9. What two things about the nature of the reactants determines the reaction rate? 10. a. Draw a potential energy graph for an exothermic reaction. b. One the graph indicate the position of the reactants, products, and the activated complex. c. Indicate on the graph the following energies: PE of the reactants, PE of the products, PE of the activated complex, activation energy for the forward reaction, activation energy for the reverse reaction, and the heat of reaction. d. Indicate the energy graph for this reaction with a catalyst. e. Is the reverse reaction exothermic or endothermic? 11. Define reaction rate in words and with an equation. What does the rate law for a chemical reaction tell you about the reaction? 12. For the reaction 2A + 3B → C + 2D the initial [A] was 0.25 M and 80 seconds later the [A] was 0.050 M. What was the average rate of reaction for each of the four substances? 13. [I2] changes from 0.400 M at time = 0 to 0.300 M at time = 4.00 minutes. Calculate the average reaction rate in moles I2 consumed per litre per minute. I2 + Cl2 → 2ICl 14. From the data, below: a. determine the average rate of reaction for the second interval from 20 to 40 seconds and for the third interval from 40 to 60 seconds. b. graph [A] versus time. c. find from your graph the instantaneous reaction rate at t = 40.0 s. Time (s ) 0.0 20.0 40.0 60.0 80.0 [A] (M) 0.34 0.17 0.092 0.052 0.028 15. From the table below: Trial [A] [B] [C] Rate of Reaction (M/s) 1 6.0 12.6 2.0 0.045 2 12.0 12.6 2.0 0.090 3 12.0 4.2 2.0 0.010 4 12.0 4.2 4.0 0.010 a) Determine the order of the reaction with respect to each of the three reactants. b) State the overall rate law for this reaction. c) What is the rate constant. d) Find the rate of the reaction when [A] = 8.0 M, [B] = 10.0 M, [C] = 3.0 M 16. At a given temperature, the average rate is 1.88 x 10-4 moles of N2 consumed per liter per second. N2 + 3H2 → 2NH3 Express the rate in moles H2 consumed per second and moles NH3 produced per second. 17. 2NO + Cl2 →2NOCl Use the following data to determine the rate law for this reaction. Calculate the value of the rate constant. Initial [NO] (M) Initial [Cl2] (M) Initial Rate (M) 0.50 0.50 1.90 x 10-2 1.00 0.50 7.60 x 10-2 1.00 1.00 1.520 x 10-1 18. For the following reaction express the rate in terms of the change in concentration of the reactant and relate this to the rate of formation of each product: 2A+3B → C 19. In the reaction 3 A → 5 B, [B] rises from 0.5602 M to 0.6400 M in 3.25 minutes. What is the average rate of consumption of A during this time interval? 20. What is the rate law expression for: A + 2 B → 3 C, if we know the reaction occurs in one step? 21. Determine the rate law and rate constant from the following data:  Kinetics Answers 1. 5 factors: nature of the substances, concentration of reacting species, pressure, temperature, surface area. 2. The collision theory describes chemical reactions as a series of bimolecular collisions between reacting particles. 3. Reaction rate is dependent on the number of collisions per time and the effectiveness of the collisions. 4. The particles must have enough energy(activation or threshold energy) and the proper geometry in order to be effective and form product. 5. A reaction mechanism is a series of simple steps involving bimolecular collisions (tri- molecular are rare), between reacting particles, intermediates and catalysts. 6. The rate determining step is the slowest step in the reaction mechanism. 7. A possible reaction mechanism is: A2B + C2D2 → A2D2 + C2B A2B + A2D2 → 2A2D + B C2B + B → 2CB 8. A + C + 2 AC → AC2 + A2C Catalyst: B Intermediates: AB, ABC 9. Surface area and physical state (phase) 10.. d) Curve with the catalyst e) endothermic Activated complex P.E. a a = activation energy (forward) Reactants b = PE reactants f c = Heat of reaction d = PE of activated complex b c d e e = activation energy (reverse) f = PE of products products Time 11. Reaction rate is a measure of how quickly reactants are used up / time or how quickly products are made / time. R = k [ ]x Rate law describes how changes in a reactant concentration affects the rate of the reaction. 12. RA = - ( 0.050 – 0.25) / 80 s = 0.0025 M/s Rc = ½ RA = ½ (0.0025) = 0.00125 M/s RB = 3/2 RA = 3/2 ( 0.0025) = 0.00375 M/s RD = RA = 0.0025 M/s 13. RI2 = 0.025 M/min 14a. 0.0039 M/s b. 0.002 M/s c. slope of tangent on graph 15. a. R = k[A]1 , R = k[B]2 , R = k[C]0 b. R = k[A]1[B]2[C]0 c. k = 4.7 x 10-5 M-2s-1 d. R = 0.0376 M/s 16. RH2 = 5.64 x 10-4 M/s RNH3 = 3.76 x 10-4 M/s 17. R = k [NO]2[Cl2]1, k = 0.152 M-2s-1 18. Rate of A = 2/3 - ∆ [ B] / ∆ t , Rate of A = 2 ∆ [ C] / ∆ t 19. Rate of A = 2.46 x 10-4 M/s 20. R = k[A]1[B]2 21. R = k[A]2[B]2 , k = 0.694 M-3s-1  Equilibrium and Ksp 1. Calculate the Kc for the following equilibrium: 2SO3(g) ↔ 2SO2(g) O2(g) when [SO3] = 0.0160 M, [SO2] = 0.00560 M, [O2] = 0.00210 M 2. Predict the effect on the equilibrium if the following changes occur to the given reaction: N2(g) + 3H2(g) ↔ 2NH3(g) + 92 kJ a) increase [N2] b) increase [NH3] c) increase temperature d) increase volume e) add a catalyst 3. How would the following affect the equilibrium? H2(g) + CO2(g) ↔ H2O(g) + CO(g) a) adding H2O(g) d) decreasing the pressure b) removing CO(g) e) adding something that absorbs CO2 c) adding H2 f) increasing the volume of the container 4. For the following equations write the equilibrium expressions (in terms of both concentration and pressure) and predict the relative amount of reactants and products at equilibrium. a) 4 NH3(g) + 5 O2(g) ↔ 4 NO(g) + 6 H2O(g) kc = 5.0 x 10-19 b) PbSO3(s) + H3O+(aq) ↔ Pb2+(aq) + HSO3-(aq)+ H2O(l) kc = 2.3 x 10-9 c) 2CO(g) + O2(g) ↔ 2CO2(g) kp = 2.0 x 10-5 d) 2 N2H4(g) + 2 NO2(g) ↔ 3N2(g) + 4H2O(g) kp = 3.0 x 10-2 5. If 6.0 mol of CO(g) and 6.0 mol of H2O(g) are placed into a 2.0L container and the reaction is allowed to reach equilibrium, what is the equilibrium concentration of each species? CO(g) + H2O(g) ↔ H2(g) + CO2(g) kc = 0.80 6. H2(g) + I2(g) ↔ 2HI(g) kc = 46 If 2.0 mol of each H2 and I2 and 3.0 mol of HI are placed into a 1.0 L flask and allowed to reach equilibrium. Find the concentration of each species at equilibrium. 7. Kc for the reaction: A + 2B ↔ C is 3.63. The data in the table shows the concentrations of two different reaction mixtures. Are the two systems at equilibrium? If not, which way does the reaction need to proceed to reach equilibrium? Reaction Mixture [A] M [B] M [C] M 1 0.500 0.621 0.700 2 0.250 0.525 0.250 8. At 2273 K, Kc = 6.2 x 10-4, N2(g) + O2(g) ↔ 2NO(g) If [N2] = 0.05200 M and [O2] = 0.00120M, what is the [NO] at equilibrium? 9. How will the equilibrium of: Heat + CH4(g) + 2 H2S(g) ↔ CS2(g) + 4 H2(g) be affected by the following: a) addition of CH4(g) d) decrease in the volume of the container b) addition of H2(g) e) decrease in the temperature c) removal or CS2(g) 10. Sketch concentration vs. time graphs for the reaction in #9 if the system is initially at equilibrium and then: ([CH4] < [H2S] < [CS2] < [H2]) i) some H2S is added. iii) CS2 is removed ii) the temperature is decreased 11. What is the ksp value for a salt. X2Z3, if it is found that 0.0058 g will dissolve in 2500 mL of water? (molar mass of this substance is 250 g/mol) 12. If the ksp for magnesium fluoride is 6.4 x 10-9, what is it's molar solubility in a) pure water b) 0.035M MgI 13. Will a precipitate of calcium fluoride form if 12.0 mL of 0.0030 M calcium chloride is mixed with 10.5 mL of 0.0025 M sodium fluoride? (ksp of CaF2 = 3.90 x 10-11) 14. Give the Kc and Kp expressions for the following reactions a. 2 N2O5(g) ↔ 2 N2O4(g) + O2(g) b. Bi2S3(s) + 6 H+(aq) ↔ 2 Bi3+(aq) + 3 H2S(g) 15. Consider the following reaction H2(g) + CO2(g) ↔ H2O(g) + CO(g) Two moles of each reactant are allowed to react in a 0.50 L container until equilibrium is established. If the equilibrium concentration of CO2(g) is 0.78 M: a. What is the equilibrium concentration of each of the other substances? b. What is kc? c. What is the percentage yield? 16. Consider the following reaction taking place in a closed container and at equilibrium: 2A + 2B ↔ C + 2D At equilibrium, the [C] is 3.5 M, the [D] is 1.9 M, and the [A] is 2.6 M. The equilibrium constant is 0.78 at this particular temperature. What is the [B]? 17. Kc = 5.0 x 10-5 for the reaction 2NO(g) + O2(g) ↔ 2 NO2(g) If we have [NO] = 4.0 x 103M, [O2] = 3.40 x 104 M, [NO2] = 2.1 x 10-3M a) Is the system at equilibrium? b) If not, which way will the reaction have to shift to get their? 18. For the reaction: A + B ↔ C + D (balanced), the Kc is 64 at a certain temperature. Suppose 6.0 moles of each reactant is placed into a 4.0 L reaction chamber and allowed to go to equilibrium. Find the number of moles of each substance present at equilibrium. 19 Calcium sulfate, CaSO4, has a Ksp of 1.65 x 10-6. What is its solubility in a 0.15 M solution of MgSO4? 20. Iron (II) iodide. FeI2, has a molar solubility of 7.3 x 10-9 M, a. What is the concentration of the Fe2+ and the I- ions in a saturated solution? b. What is the Ksp of iron (II) iodide? 21. Lead Chloride. PbCl2, has a Ksp of 1.7 x 10-5. A student mixed 75 mL of 0.035 M Pb(NO3)2 and 170 mL of 0.0030 M NaCI. Did a precipitate of lead chloride form? 22. Consider the reaction A + heat ↔ B taking place in a closed vessel and at equilibrium. Suppose at equilibrium there is more of A than B. a. Draw a concentration versus time graph showing the system at equilibrium initially, then responding to a decrease of A and reaching equilibrium again. b. Draw a concentration versus time graph showing the system at equilibrium responding to an increase in temperature and returning to equilibrium again. 23. Each of the following reactions has come to equilibrium. What will be the effect on the equilibrium amount of each substance in the system when the change described below is made? a. 2 H2(g) + 2NO(g) ↔ N2(g) + 2 H20(g) Pressure is increased. b. SO2(g) + ½ O2(g) ↔ S03(g) + 23 kcal Temperature is increased. c. P4(g) + 6H2(g) ↔ 4 PH3(g) H2(g) is added.  Equilibrium and Ksp Answers 1. 2.57 x 10-4 2. a) shift right b) shift left c) shift left d) shift left (P ↓) e) speeds up rxn 3. a) shifts left b) shifts right c) shift right d) no effect e) shifts left f) no effect 4. a) Kc = [NO]4[H2O]6 Kp = PNO4 ∙ PH2O6 b) Kc = [Pb][HSO3] Kp = nil [NH3]4[O2]5 PNH34 ∙ PO25 [H3O+] - little products formed, Kc < 1 c) Kc = [CO2]2 Kp = PCO22 d) Kc = [N2]3[H2O]4 Kp = PN23 ∙ PH2O4 [CO]2[O2] PCO2 ∙ PO2 [N2H4]2[NO2]2 PN2H42 ∙ PNO22 5. x = 1.42M 6. x = 1.20M 7. a) Kc = 3.63 @ equilibrium b) Kc = 3.63 @ equilibrium 8. [NO] = 1.97 x 10-4M 9. a) shift right b) shift left c) shift right d) shift left e) shift left 11. 7.43 x 10-24 12. a) 1.17 x 10-3M b) 2.14 x 10-4M 13. Q = 2.18 x 10-9 Q > ksp ppt will form 14. a) Kc = [N2O4]2[O2] Kp = PN2O42 ∙ PO2 b) Kc = [Bi3+]2[H2S]3 Kp = PH2S3 [N2O5]2 PN2O52 [H+] 15. [H2] = 0.78 M [H2O] = [CO] = 3.22 M b) 17.04 c) 80% 16. [B] = 1.55M 17. Q = 8.10 x 10-18 Q < Kc therefore, not at equilibrium b) shifts right 18. A = 1.5 – 1.33 = 0.178M n = CV n = 0.178(4) = 0.712 moles B = 1.5 – 1.33 = 0.178M n = CV n = 0.178(4) = 0.712 moles C = 1.33 (4) = 5.32 moles D = 1.33 (4) = 5.32 moles 19. 1.1 x 10-5M 20. [Fe+] = 7.3 x 10-9M, [I] = 1.46 x 10-8 M b) ksp = 1.56 x 10-24 21. Q = 4.64 x 10-8 Q < ksp therefore, a precipitate will not form 23. a) [products] increase, [reactants] decrease b) [reactants] increase, [products] decrease c) pressure increases, [products] increase, [reactants] decrease  Acids and Bases 1. Benzoic acid, C6H5COOH, ionizes 2.6%. For a 0.35 M solution, what would be the [H3O+]? 2. A 0.050 L water solution contains 0.0045 g of HNO3. Calculate the [H3O+] and [OH-]. 3. The pH of a 0.28 M solution of a weak acid, HA, is 4.5. Calculate the ka for this acid. 4. If 39.0 mL of a 0.52 M H2SO4 solution is titrated with a 0.40 M NaOH solution, what volume of base was used? 5. Define an electrolyte. How are the terms strong, weak, concentrated and dilute properly used with respect to electrolytes? 6. State Arrhenius' theory as to why substances (ionic and molecular) conduct electricity in solution. 7. Give the Arrhenius definition of an acid and state 5 properties of acids. 8. Give the Arrhenius definition of a base and state the 4 properties of a base. 9. What is the equilibrium expression for an acid. Ka? What does its value tell you? 10. Give the Bronsted-Lowry definition of an acid and a base. 11. Give an example of a Bronsted-Lowry conjugate acid-base pair. How do they differ? 12. A solution has a [H+] of 0.00040 M. Find the [OH], pH and pOH. 13. A solution has a [OH] of 6.Ox 10-4 M. What is the [H+], pH, and the pOH. 14. What colour is litmus, phenolphthalien, and methyl orange in acid and base? 15. An acid, HA, is mixed to a concentration of 0.0050 M. The resulting pH is 3.3. What is the Ka for this acid? 16. Hydrofluoric acid, HF, has a Ka of 6.8x10-4. Find the pH of a 0.20 M solution of this acid. 17. Acetic acid, CH3COOH, has a Ka of 1.8x10-5. Find the % ionization of a 0.10 M solution. 18. It took 28.6 ml of 0.0020 M HCl to neutralize 50.0 ml of NaOH. What was the [NaOH]? 19. What volume of 0.060 M HCl is needed to titrate 50 ml of 0.020 M Ba(OH)2? 20. Find the final pH when 20.0 ml of 0.0060 M HCl is mixed with 30.0 ml of 0.0050 M NaOH.  Acid and Bases Answers 1. 9.1 x 10-3M = [H3O+] (monoprotic) 2. 2. [H+] = 1.43 x 10-3M [OH-]=6.99 x 10-12M 3. Ka = 3.56 x 10-9 4. 101.4 mL #5 – 10 use notes. 11. Conjugate A-B pairs: 2 substances that are related by the loss of gain of a single [H +] ion HSO3 + H2O ↔ H3O+ + SO3- Acid base c.a. c.b. Conjugate base – what remains of the original acid once it has lost its proton Conjugate acid – the substance formed when the original base accepts the proton 12. [OH-] = 2.5 x 10-11M pH = -log(0.0004) = 3.4 pOH = -log(2.5 x 10-11) = 10.6 13. [H+] = 1.67 x 10-11M pH = -log(1.67 x 10-11M) = 10.78 pOH = 14 – 10.78 = 3.22 14. Acid Base Litmus red litmus – red red litmus – blue Blue litmus – red blue litmus – blue Phenolphalein colourless red Methyl orange red yellow 15. Ka = 5.56 x 10-5 16. pH = 1.93 17. 1.34% 18. Cb = 1.144 x 10-3M 19. Va = 33mL 20. pH = 10.8  Atomic Structure 1. Calculate the frequency of red light with a wavelength of 6.50 x 10 -7m. 2. The longer the wavelength, the _____________ the frequency, is an _____________ relationship. 3. Which color has the longest wavelength?_____________ 4. Which color has the shortest wavelength?_____________ 5. On the EM Spectrum, which type of wave has the longest wavelength? ________________ 6. On the EM Spectrum, which type of wave has the shortest wavelength? _________________ 7. What is the energy of x- radiation with a 1 x 10-6 m wavelength? 8. What is the energy (Joules) of Violet light with a frequency = 7.50 x 10 14 Hz. 9. The higher the frequency, the _______________ (higher / lower) the energy. This is an example of a/an _________________ (inverse/direct) relationship. 10. The higher the wavelength, the _______________ (higher / lower) the energy. This is an example of a/an _________________ (inverse/direct) relationship. 11. Which color has the most energy?_____________ 12. Which color has the least energy?_____________ 13. On the EM Spectrum, which type of wave has the most energy? _________________ 14. On the EM Spectrum, which type of wave has the least energy? _________________ Electron Configuration & Orbital Filling Diagram Using the Long Method, give the Electron Configuration: 15. Magnesium (Mg):_______________________________________________________ 16. Potassium (K):__________________________________________________________ 17. Lithium (Li):____________________________________________________________ 18. Nickel (Ni): ____________________________________________________________ Identify the following Elements: 19. 1s2 2s2 2p2: __________________ 20. 1s2 2s2 2p6: __________________ 21. [Ar] 4s2 3d10 4p6: __________________ 22. [Kr] 5s2 4d1: __________________ Identify the following elements: 23. ________ 1s2 2s2 2p4 24. ________ 1s2 2s2 2p6 3s2 3p5 25. ________ 1s2 2s2 2p6 3s2 3p6 4s2 3d9 26. ________ [Ne] 3s2 3p3 27. ________ [Kr] 5s2 4d6 Determine the Electron Configuration using the short Method: 28. sulfur ________________________________________________________________ 29. strontium _____________________________________________________________ 30. bromine ______________________________________________________________ 31. zirconium _____________________________________________________________ 32. molybdenum __________________________________________________________ Electron Configuration Review 33. The s orbital is _______________ shaped, appears in ________ ( a number) shape/s, and can hold ____ e-. 34. The p orbital is _______________ shaped, appears in ________ ( a number) shape/s, and can hold ____ e-. 35. The d orbital, appears in ________ ( a number) shape/s, and can hold ____ e-. 36. The f orbital appears in ________ ( a number) shape/s, and can hold ____ e-. 37. The Aufbau Principle states that __________________________________________ 38. Hunds Rule states that __________________________________________________ 39. Pauli exclusion principal states that ________________________________________ 40. In the electron cloud model, ______ percentage of electrons are predicted to be located in the cloud/orbital. 41. Calculate the wavelength given the frequency of radiation is 6.10 x 1014 Hz 42. Calculate the frequency of light with wavelength = 2.50 x 10-7m 43. What is the energy of cell phone radiation with a 1m wavelength? 44. What is the energy (Joules) of Violet light with a frequency = 7.50 x 1014 Hz. 45. photons are: __________________________________________________________ 46. The dual nature of light deals with light as __________and light as ___________: 47. When absorbed energy, electrons go from the ground state to the excited state. As they return to the ground state, they release their energy in the form of:__________________ Created With Tiny Scanner Created With Tiny Scanner Created With Tiny Scanner Created With Tiny Scanner Created With Tiny Scanner