Part 1. Preparation and Color of Solutions. Experiment 1 (2 session lab) Electrons and Solution Color. Pre-lab Report, page 29

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1 Experiment 1 (2 session lab) Electrons and Solution Color Pre-lab Report, page 29 Session 1 One hour discussion (E2) Two hour lab (E1) Aim to complete Parts 1, 2, and 3 of E1. Part 1. Preparation and Color of Solutions Goals Successfully prepare a solution of known Molarity. Determine if it possible to predict the color of a salt solution from the structure of the salt s cation. Part 1. Preparation and Color of Solutions 1 Teams prepare solutions with different metal ions H+ Hydrogen Record the color of solutions. IIIA IVA VA 3 4 Li+ Be Lithium Beryllium 1 1 Na+ Sodium 1 9 K+ Potassium 3 7 Rb Rubidium 5 5 Cs Cesium 1 2 Mg2+ Magnesium IIIB IVB VB VIB VIIB VIIIB! VIIIB IB IIB Ca2+ Sc Calcium ScandiumTitanium Ti V Vanadium Cr3+ Chromium 2 5 Mn Manganese 2 6 Fe3+ Iron 2 7 Co2+ Cobalt Ni2 + Cu2+ Nickel Copper Zn2+ Zinc 3 8 Sr Y 4 0 Zr 4 1 Nb 4 2 Mo 4 3 Tc 4 4 Ru 4 5 Rh 4 6 Pd 4 7 Ag+ 4 8 Strontium Yitrium Zirconiudenum Niobium TechnetiumRuthenium RhodiumPalladium Silver Molyb Ba2+ La* Hf Ta W Re Os Ir Pt Au Barium LanthanumHafnium Tantalum Tungsten Rhenium Osmium Iridium Platinum Gold Cd2+ Cadmium Hg2+ Mercury 1 3 Al3+ Aluminum Ga Galium Ge Germanium 4 9 In 5 0 Sn Iridium Tin Tl P b 2+ Thallium Lead Sb Antimony 8 3 Bi Bismuth Solution Color Solutions with ions of the same metal element with different ion charges may have different colors. 1 H+ Hydrogen IIIA IVA VA 3 4 Li+ Be Lithium Beryllium DEMO: V 2+ vs. V 3+ etc Na+ Mg2+ Sodium Magnesium IIIB IVB VB VIB VIIB VIIIB! VIIIB IB IIB 1 9 K+ Potassium 3 7 Rb Rubidium Ca2+ Sc Ti V Cr3+ Mn Calcium ScandiumTitanium Vanadium Chromium Manganese 3 8 Sr Y 4 0 Zr Strontium Yitrium Zirconium Nb Niobium Mo Molybdenum 4 3 Tc Technetium 2 6 Fe3+ Iron 2 7 Co2+ Cobalt Ni2 + Cu2+ Nickel Copper Zn2+ Zinc 4 4 Ru 4 5 Rh 4 6 Pd 4 7 Ag+ 4 8 Ruthenium RhodiumPalladium Silver Cd2+ Cadmium 1 3 Al3+ Aluminum Ga Ge Galium Germanium Periodic Table with common metal ion charges In Sn2+ Sb Iridium Tin Antimony 1

2 Part 1 Data analysis and discussion. Is the presence or absence of salt solution color predictable from? Placement of the metal ion s element in the periodic table? The metal ion s radius? The metal ion s electron configuration? Questions 1-4, p.39 Course theme There are structure and property and periodic table relationships Useful web sites are: Discussion Preparation Manipulate the class data. You will NOT get points for just reproducing the class data. Discussion Preparation Refer to the two grading rubricks, pages Note that one discussion grading rubrick refers to an exam question. Refer to the discussion information, page

3 Part 3. Solution Color and Light Interaction. What is the relationship between the visible color of a solution and its absorption and transmission of visible light wavelengths? Use a spectrophotometer to examine the relationship between solution color and absorption and transmission of visible light. Discussion question 5 Light source Diffraction grating Sample solution Detector Spectrophotometer Spectrophotometer 1. Record visible wavelength colors (Part 2) 2. Record sample absorbance across the visible spectrum to produce an absorption spectrum. 3

4 Absorption Spectrum A plot of absorbance versus wavelength Absorbance λmax Light Absorbance vs. Transmission ABSORBANCE = -LOG TRANSMITTANCE 0% 10% T 100% 2 1 A 0 Abs = 1 10% light transmitted Abs = 2 1% light transmitted Solution preparation Chem.125/126 Mascot Calibration line Volumetric flasks 4

5 Moles and the Periodic Table? National Mole Day: October 23. Why?? H He Li Be C Ne Na Mg Si Ar K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ge Kr Rb Sr 41 Nb Mo Tc 44 Ru 45 Rh 50 Sn 54 Xe Cs Fr (223) Ba Ra Y La Ac (227) 40 Zr Hf Rf (261) Ta Ha (262) 58 Ce Th W (263) 59 Pr Pa (231) (99) 75 Re Nd U Os Pm (145) 93 Np (237) Ir Sm Pu (242) 46 Pd Pt Eu Am (243) 47 Ag Au Gd Cm (245) 48 Cd Hg Tb Bk (249) 5 B Al Ga In Tl Dy Cf (251) Pb Ho Es (254) 7 N P As Sb Bi Er Fm (255) 8 O S Se Te Po (209) 69 Tm Md (256) 9 F Cl Br I At (210) 70 Yb No (254) Rn (222) 71 Lu Lr (257) Mole = mol = 6.02 x item = atomic wt (g) = formula wt (g) H He Li Na K Rb Cs Fr (223) 4 Be Mg Ca Sr Ba Ra Mole of H 2 O = grams? 21 Sc Y La Ac (227) 22 Ti Zr Hf Rf (261) 23 V Nb Ta Ha (262) 24 Cr Mo W (263) 25 Mn Tc (99) 75 Re Fe Ru Os Co Rh Ir Ni Pd Pt Cu Ag Au Zn Cd Hg B Al Ga In Tl C Si Ge Sn Pb N P As Sb Bi O S Se Te Po (209) 9 F Cl Br I At (210) 10 Ne Ar Kr Xe Rn (222) 58 Ce Th Pr Pa (231) 60 Nd Pm (145) 62 Sm Eu U Np (237) 94 Pu (242) 95 Am (243) 64 Gd Cm (245) 65 Tb Bk (249) 66 Dy Cf (251) Ho Er Es (254) 100 Fm (255) Tm Yb Lu Md (256) 102 No (254) 103 Lr (257) 5

6 Molar Reflections* Yesterday I took a drink of water And something strange happened in my head I made an actual connection With something that my chemistry teacher said I could visualize lots and lots of molecules Movin in the water to and fro and then I thought If I just drank 18 grams of water I just drank a mole of H 2 O! Molar reflections, my mind is running free Making connections between the world and chemistry A mole is more than a number, more than just a word It s an amount that s equal to 6.02 times ten to the twenty third! Moles and solution concentration #M = Molarity of Solution # = moles per 1000mL of solution or mmoles per ml of solution *Mike Offutt 2002 Solution preparation What is the formula weight of copper sulfate? CuSO 4 5 H 2 O = Hydrated copper sulfate CuSO H 2 O CuSO 4 = anhydrous copper sufate Example CuSO 4 5 H 2 O = Cu + S + 4 ( O ) + 5 (2 x H + O) = (16) + 5 (2 + 16) = DEMO Solution preparation 1. You prepare 100 ml of 0.10 M copper sulfate using CuSO 4 5H 2 O. How many grams of CuSO 4 5H 2 O (FW = ) do you weigh out? g x 0.10 mol x 100 ml = 2.50 g 1 mol 1000 ml DEMO 6

7 Solution preparation Solution Preparation Calibration line 2. Your teammate adds 1 liter (1000 ml) of water to g of NaCl to prepare 1.0 M NaCl. The resulting solution was too dilute ( < 1.0 M ). Why? = g NaCl Volumetric flasks 0.1 M Copper sulfate Transfer 2.50 g of CuSO 4 5H 2 O to a 100 ml Vol flask and add water to the 100 ml calibration line Solution dilution Solution Dilution Initial mols or mmoles = Final mmol or mmoles Add H 2 O Burets clamped to ring stand One buret with water; one buret with sample to be diluted Deliver the volume (ml) of sample to be diluted into a flask. Deliver the needed volume (ml) of water into the flask. 7

8 Dilution of Solutions Solution Dilution Initial mol or mmol = Final mol or mmol M 1 V 1 = M 2 V 2 initial mmoles = final mmoles If V= milliliters: M x V = If V= liters: M x V = mmol x ml = mmol ml mol x L = mol L Add H 2 O 0.10 M x 10 ml.05 M x 20 ml add 10 ml H 2 O 1 mmol = 1 mmol Q. What volume of 0.20 M Ni(NO 3 ) 2 and water do you use to prepare 10 ml of 0.16 M Ni(NO 3 ) 2? M 1 V 1 = M 2 V 2 Q. What volume of 0.20 M Ni(NO 3 ) 2 and water do you use to prepare 10 ml of 0.16 M Ni(NO 3 ) 2? M 1 V 1 = M 2 V M x? ml = 0.16 M x 10 ml ml 0.20 M Ni(NO 3 ) 2 + ml H 2 O? 8 ml 0.20 M Ni(NO 3 ) ml H 2 O 8

9 Any Questions? Contact 9

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