ADDITIONAL EXERCISES

These exercises are not divided by category, although they are roughly in the order of the topics in the chapter. They are not paired. 

87 Suppose a scientist repeats the Millikan oil-drop experiment but reports the charges on the drops using an unusual (and imaginary) unit called the warmomb (wa). The scientist obtains the following data for four of the drops  

The diameter of a rubidium atom is 4.95 A. We will consider two different ways of placing the atoms on a surface. In arrangement A, all the atoms are lined up with one another to form a square grid. Arrangement B is called a close-packed arrangement because the atoms sit in the depressions formed by the previous row of atoms  

94 The element oxygen has three naturally occurring isotopes, with 8, 9, and 10 neutrons in the nucleus, respectively. 

95 The element lead (Pb) consists of four naturally occurring isotopes with atomic masses 203.97302, 205.97444, 206.97587, and 207.97663 amu. The relative abundances of these four isotopes are 1.4, 24.1, 22.1, and 52.4% respectively. From these data, calculate the atomic weight of lead. 

57 (a) Classify each of the following as a pure substance, a solution, or a heterogeneous mixture a gold coin, a cup of coffee, a wood plank, (b) What ambiguities are there in answering part (a) from the descriptions given  

58 (a) What is the difference between a hypothesis and a theory (b) Explain the difference between a theory and a scientific law. Which addresses how matter behaves, and which addresses why it behaves that way  

59 A sample of ascorbic acid (vitamin C) is synthesized in the laboratory. It contains 1.50 g of carbon and 2.00 g of oxygen. Another sample of ascorbic acid isolated from citrus fruits contains 6.35 g of carbon. How many grams of oxygen does it contain Which law are you assuming in answering this question  

60 TWo students determine the percentage of lead in a sample as a laboratory exercise. The true percentage is 22.52%. The students results for three determinations are as follows  

61 Is the use of significant figures in each of the following statements appropriate Why or why not (a) Apple sold 

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As an additional exercise, the current-voltage curve of the supporting electrolyte (1M potassium chloride) may be evaluated this gives the residual current directly and no extrapolation is required for the determination of / and Id. 

In this section, we sketch the nature of the three VB state framework as a template to describe bimolecular nucleophilic substitutions ( S. -2)[7, 12, 13], Although it remains to be seen if three VB states are sufficient to describe the title reaction system in solution, this is still a useful additional exercise to expose the reasoning underlying the practical application of our theory. The wave function to describe the Sa/2 reaction... 

Additional Exercises Potassium dichromate, K2Cr207 potassium chlorate, KClOj. 

Additional Exercises Sodium nitrate, NaN03 lead nitrate, Pb(N03)2. 

Additional Exercises Manganese chloride, MnCtrlHiO magnesium sulfate, MgS04-7H20. 

Additional Exercises Calcium chloride, CaCl2-6H20 sodium thiosulfate, Na2S203-6H20. 

Additional Exercises Chromous acetate, Cr(C2H302)2 chromous sulfate, CrS04-7H20 chromous chloride, CrCl2-4H20 Anderson and Riffe, J. Ind. Eng. Chem., 8, 24 (1916) Reeoura, Ann. Chim. Phys., (6) 10, 6 (1887). 

Additional Exercises Cuprous sulfite, Cu2S03, Groger, Z. anorg. Chem., 28, 154 (1901). 

Additional Exercises Bismuth nitrate, Bi(N03) ,-5H20 aluminum nitrate, Al(N0j)j-18Hi0 trisodium phosphate, Na3PO.rl2H20. 

Additional Exercises Lead chromate, PbC rO, calcium phosphate, Ca3(PC>4)2 ferrous oxalate, Fe(C2C>4) sodium chloride, NaCl, precipitated from a saturated solution by HC1 gas, Richards and Wells, Revision of the atomic weights of sodium and chlorine, J. Am. Chem. Soc., 27, 459 (1905). 

Additional Exercises Calcium hydroxide from sodium hydroxide and calcium chloride silver nitrite from silver nitrate and sodium nitrite manganese sulfite, MnSChSHsO, from manganese chloride and sodium sulfite (adding a little S02 to the solution) mercuric iodide from potassium iodide and mercuric chloride. 

Additional Exercises Preparation of a low-boiling metal such as rubidium or cesium, Graves, J. Chern. Educ., 9, 1274 (1932) Grosse, Ber., 59B, 2646 (1926). 

References Mellor, IX, 90 Read, J. Ind. Eng. Chetn., 20,97(1928). Additional Exercises Purification of iodine preparation of ammonium carbonate from calcium carbonate and ammonium chloride mercuric chloride from mercuric sulfate and sodium chloride. 

Additional Exercises Ultramarine, Thorpe, Dictionary Wienard s blue, Jordan, Z. angew. Chem., 6, 684 (1893) reduction of BaSCb to BaS burning pure marble to CaO. 

Additional Exercises Copper oxide from copper (for combustion) bismuth iodide. 

Additional Exercises Phosphorus bromide, PBr5 antimony chloride, SbCl3. 

Additional Exercise Barium peroxide from hydrogen peroxide. 

Additional Exercises BaS from BaSO, Ca3P2 from Ca3(PO.i)2. 

Additional Exercises NaHC03 NaHS03 KHSCh Ca(H2P04)2. 

Additional Exercises Zinc basic acetate, Zn40(CsHa02)6, Auger and Robin, Compt. rend., 178, 1546 (1924). 

Additional Exercise Ammonium perborate, Melikoff and Pissarjewsky, loc. cit. 

Additional Exercises Phosphonium bromide, PH4Br phosphorus pentachloride, PC16 iodine trichloride, IC13. 

Additional Exercise Potassium fluozirconate from crude zirconium oxide. 

Additional Exercise Bromostannic acid, H2SnBr6-8H20, Seubert, loc. cit. 

Additional Exercise Sodium tetrathionate, Na2S406-2Hs0. 

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