SPECTROSCOPY: QUALITATIVE ANALYSIS WITH LIGHT Waves, Light, and Atomic Spectra ! % " # & & ' (" % & # $ $ ) * + # & # " (" + # ! "# " # + ", & # " " - & " ! , " # !" #$% $% &' " () " $ '" %#" ( * ( ! & ! ! ! " # " ! & ! " ! #" & # " . # ) & " & & / "!& # " " & , "# 01 # # & ! ! & " " # " ! # , " & "" .& " & " & #" & 3 " # " " 1 "! 0 2 !# # , # , " " " " # ) ! # ! .( .(/ * 0 1 ( )( 1 " !& " # " " !& & " " (" 4 ! # " # 1 " " & )( " # " & ) & & , " & " & " & & ( (0 *2 .(0$+(3,( 1 ) " / " " & " & ! 5 ! " 1 & & " "& " # " # " ! & (" ! 2 42 .(5 ( , & & ! & " " "! ) & & + , ( -1 + & & (" , & ! #" & " 1 " & !& " # " # 6 (" ! ! & ! +(3,( & & 7 8 " 7 &8 " 6 & ! & & " (5 & & " & + ! & & # 6 " & ! ! # " " & 1 & # (" " & " & (" & 9 " # ! : ! & (" & " # "# ) # # ! " " & & # " " ! & 2 .(5 ( !& %() 0 ; " # " 9 " # & (" (" & : & ' & (" & & 6 # " & (" " & , & 9 7 ,8 : $ ) & & # & 0 " ! & " & " (" & Can you state a generalization relating the frequency of a wave to its wavelength? )(' ( (0 *2 .(06 0 , .( 4%(0 , .( & ! " " & & + # "# " 7 + & & : ! # 9 ! (* (( ( 8 9 & & & : " & ! " ! & + " " '" < , " & 4 # & 9 & #" & / " & : ! ! ! + , ( -) # & & & %() 0 , / " 1 ) & ! # & , " 7 # !8 & # ! ) 6 ; " # " ) ) ) 4 & & & " & & & & 0 1 & & " 0 . & + , , & !# 01 ) & & !# " ! !# " 7 8 (" ! && & & & & " Is there any relationship between the frequency of the wave and the wavelength of the standing wave? 7 0 + ) *2 .( = " # # & & " , & & & ' " >: 1 9 ,# " " 7 !8 # & # " & !# / " 1 # #" / " & # & & ! " & ! & , # & & "! & / & # # 1 & & # ! " " " ! & ! 8 & # & & # + ! & & " ! & ) 7 " ' " ?: " ! & " "# " & # & , (" & " " & 7 # # # " 7 & ) 8 " ! & 9 & : & & & " & & & 1 " & & " & " # " # 1 A?!BBB " ! # & " # " " # " ! & # '" @ " & & , & + ,( - & & " 1 8' " , 4 # " 9 & & " + , (7-1 7 8 " & ! " ! " " " # " & "# # " , " & " "" '" C ; " # + , (8& & & " & & #0 ( ( 0 5 , " " " # , 1 " , ( & #"# ; " " # " # " ; " " # , 6 5 " " " '" ? & # " # 5 , / " & & " & # # 42 .(5 ( 5 , " " & & " " ! & @! " & 4& " & & 01 & 5 + , (965 " " " " 1 , ; "& & 1# " " : # ) (" " 9 A# ) " &! 01 " # List the colors you see in the spectroscope, in order of increasing frequency and decreasing wavelength: __________ __________ __________ __________ __________ __________ Increasing frequency Decreasing wavelength 5 ( -1 & 6 # # # & (+ ; " ! & (" & # ( ) & 0) $ ,( * ( & " # (" :1 & # # ,& ) ) " # 09 ; " :+ & , & # $D %=4=1.=5 %;= & D; " # " & # # # + # 0 " " # " 01 # ! " & "# " " " 9 " " 05 , & 2 1 = = 21== 5 = 21=1.2'5 2 1 & & =# " " " 8 " & ) "# 0 " ! 0+ ! " " 1, " & " # , " " ", " ! ; " # " & " & '" E 4 & & & " 9 :" A F ABAB ! 0 (" " " " + , (:- 6 "# ! & 9: = & " " " ) 5 (4 -; ( < , 4 54.0-! 0( ,0 " " " # 0 .4(4 (( 4 * 0(1 ( )( = ( " & ) ! ! " ! =# " # 1 # , # , 9 : (" A F ABG " 5 , " " " ) 0 " " " 05 , # & "# # 0 " ! !& & & " # "" " # 1# ) & ! & % & " " " " & , 5 # & " # " , " " ! # 05 , & " & " " =# #" # 5 , <! " # Solids produce a __________ spectrum. Gases produce a __________ spectrum. 5 ( -1 " " " # 6 # # 6 # , # " # " 9 " 0 ! ' ( 0, ()( + # " " # * ( , # '" H & , " ) " & ! # "" + " & " " ! '" H " & " , # & 1 & , # " & (" 4 " " 1 & + , (>6 & 1 + " " " " ' ! " # " # & " # 7 8 " (" " . " # & " HH ) "# " # " " ! 2 & 1 " (" " " # 1# Violet Violet Blue Green Yellow Yellow ! & # # " > + # # " # + "& # , 5 (7-1 & # 404.6 nm 407.7 435.8 546.0 576.7 579.0 " " ", & " ! " ! # & .& # / " ! & , & " # " " & ", & & & # " " 7 =I8#" " 1 ", & 5#) , "& ! 1 " # ", & 9 )! J! ; K: " " ", & & / + & " " # & 7 # "# && & 7 # # ; "& 8 # & # 1& # " " # # ! : " 1# , 89 , # # " : # " !/ " " # & " & # # " @1 , # ! " , " " 1 1 " # ?BEE % "# , " " # "# ,1 " , & # # & ! & ?B? C J! ; & 1 K: " / " + , (?61 8# " ! 9 " " # :& & " "& # 1 ?BEE " 1 ", & 5#) , "& ! " # # " , & ; "& + # + " " # # " 7 =I8#" 1 7 " " # , "# && & 7 # 89 1& , # " & > / " # & " " 1# @ 1 , , " & : & " # # " !/ " " # ", & 9 )! ! " " & , % "# , " " # "# ,1 " 8 & # ) " # ?B? C 1 7 8# " ! "& # 9 " " # :& & + " ?BEE " " & # , 7 ", & 8 # ) 8 7 ) 8# " ! " # & "& " & & N 6= / " # & # ! & " & 7" # & # , ", & ", & # ", & # & # " # 1 4& & , 7 ", & + ,( " ! " # (" ; " "", & & & , # " " ", & ) # " & & " # , " ! " "# " # # ,; " 1# ? ; " & 7 # ! ' " # ! & ! " " " ", & & , & ? @ " 4 # & " # # 8 & & , LM @ , & # , "& " & &! " " " ! " & , , ! # # Thallium Cadmium Hydrogen Zinc Helium 378 535 361 468 480 509 644 397 410 434 486 656 384 468 472 481 638 361 371 382 389 396 403 412 414 439 448 469 471 492 502 588 668 5 ( 2 " )( , : 4 & , " % * & 2 & , ! " # & , & " & & 7 # # 8 " # " " & " ! " # # # , & ! # & (" & (" # & # " 389 456 460 525 527 540 542 583 601 621 635 656 663 672 " Mercury 392 399 413 427 460 497 610 624 671 " 366 405 408 436 546 577 579 # 5 ( " 3 & " ! # " 9 ' " AA: 2 # 2 ! # " , & " ! ! & (" " " " ' " A< + / " 470 472 483 488 534 540 576 585 588 603 607 616 622 627 640 651 653 660 668 672 Lithium " # # & Cesium : @ 0'5 ( " % " & " " " " 3 " " # Neon 467 498 515 567 568 589 590 615 616 9 ) (.(5 6 4(59 = " Sodium + ,( # - / " # & " & " ! # ! (" ! " " # ! - # & ! # ' & " ! < 9 < ! K<! A BBABGCEH / " <& " # " # : " # : / " & " # 1 # @! (" " " " # > # <9 > 9" # # " " 9 : 1# & >NO < : 1" @ ? NO < " # & + ,( - - (" !# ! & # . & & @NO < A % 1 " " & (" - " BBABGCEH A . " # < ) # # # # + " # # $ ! 0 ! " ! " " ! " & " CNO < " " / " # 0 # " " & > O< & 0 ) " 9 : # " ! ? O< # 0 ) " 0) " # , " " # 0 Hydrogen Spectral Lines predicted by Bohr’s planetary electron model for electron jumps ending on orbit two. Electron transition Wavelength of emitted light Color of emitted light. 3 4 5 6 656.4 nm 486.3 nm _______nm _______nm Red Blue-Green Violet Violet (difficult to see) 2 2 2 2 Table 5 Electron transitions, wavelengths, and colors of hydrogen spectral lines predicted by Bohr’s planetary electron model. The wavelengths predicted for the 5->2 and 6 -> 2 electron transitions are not included in this table. They are left for you to compute. LABORATORY REPORT Your report should include your data and conclusions derived for each of the experimental topics. Be sure to include your spectra chart, your mercury calibration graph, and the measurements you made on the unknown colored slides.