7. Calculate the expected M+1 and M+2 relative intensities assuming M+ has a relativeintensity of 100% (base peak). Use the isotope masses contained in the table below.a. CioH20d. C10H19CIb. CaH12O2e. CioH19Brc. C8H16N2 ElementNatural abundanceCarbon12C13C98.89%1.11%Hydrogen2H99.99%0.01%Nitrogen14N15N99.64%0.36%Oxygen16017018099.76%0.04%0.20%33s34S36S325Sulfur4.22%0.02%95.0%0.76%19FFluorine100%37CI35CI24.23%Chlorine75.77%8lBr79B.49.31%Bromine50.69%

The y-axis of a mass spectrum is relative abundance (relative intensity). Calculates how much of an…

7. Calculate the expected +1 and M+2 relative intensities assuming M+ has a relative intensity of 100% (base peak). Use the isotope masses contained in the table below. a. CioH20 d. C10H19CI b. C8H12O2 e. CioH19Br c. CaH16N2

7. Calculate the expected +1 and M+2 relative intensities assuming M+ has a relative intensity of 100% (base peak). Use the isotope masses contained in the table below. a. CioH20 d. C10H19CI b. C8H12O2 e. CioH19Br c. CaH16N2

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Profiles Tab Window Help My Par: M You GS The Acti C Get C Fill C The C Fll C The C The C Wh b Ans keAssignment/takeCovalentActivity.do?locator=assignment-take [Review Topics] [References] Use the References to access important values if needed for this question. 1A 8A H 2A 3A 4A SA 6A 7A He LI Be BCNO F Ne Na Mg 38 4B 58 68 7B - 88 ¬ 1B 28 AI Si P S CI Ar K Ca Sc Ti V Cr Mn FeCo Ni Cu Zn Ga Ge As Se Br Kr Rb SrY ZrND Mo Tc Ru Rh Pd Ag cd In Sn Sb Te Xe Cs Ba La HT Ta w Re Os Ir Pt Ru Hg TI Pb BI Po At Rn Fr Ra Ac Rf Ha Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu Th Pa UNp Pu Am Cm Bk Cr Es Fm Md No Lr Analyze the following reaction by looking at the electron configurations given below each box. Put a number and a symbol in each box to show the number and kind of the corresponding atom or ion. (Use the lowest possible coefficients. Omit states of matter.) atom atom metal ion nonmetal ion (1s²2s²2p°3s²) (1s²2s²2p*) (1s²2s2p°) (1s²2s 2p°) Submit Answer Retry Entire Group 9 more group…
1 q eq req req O :Ö-As-Ö: c. Selenite ion, SeO;². :0: :0-Se- :Ö: Se-Ö :Ö: :Ö-Se-Ö: [ HOPPA Submit Answer -0: :0-Se-0: Se 2- Show Hint 2- 2- 2- Retry Entire Group 8 more group attempts remaining Cengage Learning | Cengage Technical Support
5. Describe the principle on which each of the following GC detectors are based: (a) flame ionization, (b) electron capture,
Model 5: Isotope Natural Abundances Atom Most common isotope C O S N CI Br 12C (100) 160 (100) 32S (100) 14N (100) 35 CI (100) Jump in Mass Next most common isotope (no. extra neutrons) (no. found for every 100 atoms of most common isotope) +1 13C (1.11) 180 (0.20) 34S (4.40) 15N (0.38) 37 Cl (32.5) "¹Br (98.0) 79Br (100) For example: There are 1.11 *C atoms on the planet for every 100 ¹2C atoms. Equivalent ways of saying this are: There are likely to be 111 1³C atoms in a sample of 10,111 carbon atoms or 1.10% of the carbon on the planet is 1³C (since 111/10,111 x 100% = 1.10%). Critical Thinking Questions 15. What does the superscript to the left of each atom label tell you (e.g., the 12 in ¹2C)?
IA BA H2A 3A 4A 5A 6A 7A He U Be B CNOF Ne 18 2e Al No Mg 38 48 58 62 7828 K Ca Sc Ti V Si P S Cl Ar Ge As Se Br Kr Cr Mn Fe Co Ni Cu Zn Ga I need correct answer with clear handwriting I'll upvote your answer Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn Fr Ra Rc RT Ha Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Th Pa U Np Cm Bk Cf Es Fm Md 4 and period 2 (1) The element with a valence electron configuration of 2s22p6 is in group SA and period 4 (2) The element with a valence electron configuration of 4s24p2 is in group 6A
Pronies lab Window Help Workshop X PB 11.3 Pers X DZL Homepag X ent/takeCovalentActivity.do?locator=assignment-take ap X docx 1A H2A Li Be A Na Mg 38 48 58 68 7888 K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Fr Ra Rc Rf Ha *** Submit Answer Akon - Be X 3A 4A 5A 6A 7A He BCNO F Ne 18 2B Al Si P S Cl Ar Ga Ge As Se Br Kr w- Workshop.docx NOV 28 tv (1) What is the element with an electron configuration of 1s22s22p63s²3p64s23d¹? In Sn Sb Te I Xe Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr (2) What is the element with an electron configuration of 1s²22s22p63s23p64s¹? Q 8A Retry Entire Group 9 more group attempts remaining Pb Bi Po At Rn .l C From the X A P OWLv2 | X Previous W O
Use the molecular orbital energy diagram below to answer the questions about bond order for the negative ion 0₂. Number of Number of Bonding electrons Antibonding electrons This corresponds to: A. Single bond Double bond C. Triple bond D. Half of a bond O2 Bond Order E. Between a single and double bond F. Between a double and a triple bond G. No bond, O₂ does not form
Sr rontium 37.62 56 Ba Barium 137.3 9 7 Fr ancium 223) Yttrium 88. F 88 Ra Radiu 22f a. 1 b. 3 c. 5.0 mL d. 2.3 mL e. 5.6 mL c. 5 9. How many milliliters of 10.0 M H₂SO4 are needed to prepare 500.0 mL of 0.10 M H₂SO4? 50 mL a. b. 78 mL d. 7 seed
I need the chart filled out with an explanation please :))