Chemistry: The Central Science, Books a la Carte Edition & Solutions to Red Exercises for Chemistry & Mastering Chemistry with Pearson eText -- Access Card Package
1st Edition
ISBN: 9780134024516
Author: Theodore E. Brown, H. Eugene LeMay, Bruce E. Bursten, Catherine Murphy, Patrick Woodward, Matthew E. Stoltzfus
Publisher: PEARSON
expand_more
expand_more
format_list_bulleted
Videos
Textbook Question
Chapter 15, Problem 48E
[6.100] The Chemistry and Life box in Section 6.7 described the techniques called NMR and MRI.
Instruments for obtaining MRI data are typically labeled with a frequency, such as 600 MHz. In what region of the
- What is the value of ΔE in Figure 6.27 that would correspond to the absorption of a photon of radiation with frequency 450 MHz?
- When the 450-MHz photon is absorbed, does it change the spin of the electron or the proton on a hydrogen atom?
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Students have asked these similar questions
7.99. What are the condensed electron configurations of
the following ground-state atoms and ions? How
many unpaired electrons are there in each? (a) K; (b)
K¹; (c) S²-; (d) N; (e) Ba; (f) Ti¹+; (g) Al
3. (a) Sketch the s orbital and the 3 types of p orbitals.
(b) Which of the quantum numbers govern,i. the shape of an orbital?il. the energy of an orbital?ili. the spin properties of the electron?iv. the spatial orientation of the orbital?
(c) Write the electron configuration for the following elements in the ground state.i. P and p3-(atomic number =15).il. Ca and Caz+ (atomic number =20).(d) If n= 3, find thei. angular Momentum Quantum Number, /il. subshell designation.ili. magnetic Quantum number, m,iv. number of orbitals in subshells.
6.113 When an electron makes a transition between energylevels of a hydrogen atom, there are no restrictions onthe initial and final values of the principal quantumnumber n. However, there is a quantum mechanicalrule that restricts the initial and final values of theorbital angular momentum l. This is the selectionrule, which states that Δl = ±1; that is, in atransition, the value of l can only increase or decreaseby 1. According to this rule, which of the followingtransitions are allowed:
Chapter 15 Solutions
Chemistry: The Central Science, Books a la Carte Edition & Solutions to Red Exercises for Chemistry & Mastering Chemistry with Pearson eText -- Access Card Package
Ch. 15.2 - Molybdenum metal must absorb radiation with a...Ch. 15.2 - Titanium metal requires a photon with a minimum...Ch. 15.2 - Prob. 15.2.1PECh. 15.2 - Classify each of the following statements as...Ch. 15.3 - Prob. 15.3.1PECh. 15.3 -
6 38 Indicate whether energy is emitted or...Ch. 15.3 - Using Equation 6.5. calculate the energy of an...Ch. 15.3 - Prob. 15.4.2PECh. 15.4 - The visible emission lines observed by Balmer all...Ch. 15.4 - Prob. 15.5.2PE
Ch. 15.4 - Prob. 15.6.1PECh. 15.4 - The hydrogen atom can absorb light of wavelength...Ch. 15.5 - Prob. 15.7.1PECh. 15.5 - Prob. 15.7.2PECh. 15.5 - Use the de Brogue relationship to determine the...Ch. 15.5 - Prob. 15.8.2PECh. 15.6 - Neutron diffraction is an important technique for...Ch. 15.6 - The electron microscope has been widely used to...Ch. 15.6 - Prob. 15.10.1PECh. 15.6 - An AM radio station broadcasts at 1010 kHz, and...Ch. 15.6 - One type of sunburn occurs on exposure to UV light...Ch. 15.6 - Prob. 15.11.2PECh. 15.7 - Prob. 15.12.1PECh. 15.7 - A stellar object is emitting radiation at 3.55 mm....Ch. 15 - Prob. 1DECh. 15 - Prob. 1ECh. 15 - Identify the group of elements that corresponds to...Ch. 15 - Prob. 3ECh. 15 - Using the periodic table as a guide, write the...Ch. 15 -
Arrange Be, C, K, and Ca in order of increasing...Ch. 15 - Prob. 6ECh. 15 - Prob. 7ECh. 15 - Prob. 8ECh. 15 - Consider the isoelectronic ions F- and Na+. (a)...Ch. 15 - Prob. 10ECh. 15 - Prob. 11ECh. 15 - Prob. 12ECh. 15 - Give the values for n, I,and mlfor each orbital in...Ch. 15 - Prob. 14ECh. 15 - Prob. 15ECh. 15 - Which of the following represent impossible...Ch. 15 - For the table that follows, write which orbital...Ch. 15 - Sketch the shape and orientation of the following...Ch. 15 - Prob. 19ECh. 15 - Prob. 20ECh. 15 - Two possible electron configurations for an Li...Ch. 15 -
6.70 An experiment called the Stern—Gerlach...Ch. 15 - Prob. 23ECh. 15 - Prob. 24ECh. 15 - What are "valence electrons"? What are "core...Ch. 15 - For each element, indicate the number of valence...Ch. 15 - Write the condensed electron configurations for...Ch. 15 - Write the condensed electron configurations for...Ch. 15 - Identify the specific element that corresponds to...Ch. 15 - Prob. 30ECh. 15 - Prob. 31ECh. 15 - Prob. 32ECh. 15 - Prob. 33ECh. 15 - Prob. 34ECh. 15 - Prob. 35ECh. 15 - Prob. 36ECh. 15 - Prob. 37ECh. 15 - In an experiment to study the photoelectric...Ch. 15 - Prob. 39ECh. 15 - Prob. 40ECh. 15 - Prob. 41ECh. 15 - Prob. 42ECh. 15 - Prob. 43ECh. 15 - Prob. 44ECh. 15 - Prob. 45ECh. 15 - Prob. 46ECh. 15 - Prob. 47ECh. 15 - [6.100] The Chemistry and Life box in Section 6.7...Ch. 15 - Prob. 49ECh. 15 - [6.104] In the experiment shown schematically...Ch. 15 - Microwave ovens use microwave radiation to heat...Ch. 15 - Prob. 52ECh. 15 - The discovery of hafnium, element number 72,...Ch. 15 - Account for formation of the following series of...Ch. 15 - Prob. 55ECh. 15 - The two most common isotopes of uranium are 235U...Ch. 15 - Hypothetical elements X and Y form a molecule XY2,...Ch. 15 - Prob. 58ECh. 15 - Prob. 59ECh. 15 - Prob. 60ECh. 15 - Prob. 61ECh. 15 - Prob. 62ECh. 15 - Prob. 63ECh. 15 - Prob. 64ECh. 15 - Consider the following statements about first...Ch. 15 - Prob. 66ECh. 15 - Prob. 67ECh. 15 -
Write the electron configurations for (a) Ga3+...Ch. 15 - Prob. 69AECh. 15 - Prob. 70AECh. 15 - Prob. 71AECh. 15 - Prob. 72AECh. 15 - Prob. 73AECh. 15 - Prob. 74AECh. 15 - Consider the hypothetical reaction A(g) 2B(g). A...Ch. 15 - 15.76 As shown in Table 15.2, the equilibrium...Ch. 15 - Prob. 77AECh. 15 - Prob. 78AECh. 15 - Prob. 79AECh. 15 - Prob. 80AECh. 15 - Prob. 81AECh. 15 - Prob. 82AECh. 15 - Prob. 83AECh. 15 - Prob. 84AECh. 15 - Prob. 85AECh. 15 - Prob. 86AECh. 15 - Prob. 87AECh. 15 - Prob. 88AECh. 15 - Prob. 89AECh. 15 - Prob. 90AECh. 15 - Prob. 91AECh. 15 - Prob. 92AECh. 15 - Prob. 93IECh. 15 - Prob. 94IECh. 15 - Prob. 95IECh. 15 - Prob. 96IECh. 15 - Write the equilibrium-constant expression for the...Ch. 15 - In Section 11.5, we defined the vapor pressure of...Ch. 15 - Prob. 99IECh. 15 - Prob. 100IE
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- 6.103 Atomic absorption spectroscopy is based on the atomic spectra of the elements being studied. It can be used to determine the impurities in a metal sample. If an element is present, light at the appropriate wavelength is absorbed. You are working with a metal stamping company and the rolled steel you use to form panels for automobile doors is failing at an alarming rate. There is some chance that the problem is unacceptably high levels of manganese in the steel. Given that the atomic spectrum of manganese has three lines near 403 nm, how could you use a spectrometer to determine the amount of manganese in the steel?arrow_forwardFor each of the statements below, indicate whether it is true or false and explain your reasoning. (1 sentence ) 1/ It takes more energy to ionize an electron from the 2s orbital than an electron from the 2p orbital in the Li2+ ion. 2/ The electron affinity of the Ne atom is larger than the electron affinity of the F atom. 3/ K* has a larger radius than Ar. 4/ For a diatomic molecule, in which the internuclear axis is the z-axis, the 3dz? orbital cannot mix with the 2px orbital. 5/ The internuclear distance of O2 increases as it takes an additional electron to become O2".arrow_forwardThe Chemistry and Life box in Section 6.7 described the techniquescalled NMR and MRI. (a) Instruments for obtainingMRI data are typically labeled with a frequency, such as 600MHz. In what region of the electromagnetic spectrum doesa photon with this frequency belong? (b) What is the valueof ΔE in Figure 6.27 that would correspond to the absorptionof a photon of radiation with frequency 450 MHz? (c) Whenthe 450-MHz photon is absorbed, does it change the spin ofthe electron or the proton on a hydrogen atom?arrow_forward
- Q4: Find the wave length of the electromagnetic radiation, which emitted from an atom, when two electrons jump from ( 5th to 2nd ) orbit and the other from ( 3rd to 1º) orbit? Note that the ground energy equal to (-13.6eV). (Ans. 435 nm, 102 nm).arrow_forwardAssume that the filling of orbitals must be sequential, -1 →0→1(corresponding to px → Py→ p2) What element (use the symbol only) have the four quantum number set for the last electron added? 1. (3,1,0,-1/2) 2. (4,3,-2,+1/2) : 3. (2,1,0,-1/2) What is the four quantum number set for the last electron added to the following elements: 4. Sn = ( 5. Cf = ( How many electrons have the following quantum number sets? 6. (3,?,?,-1/2) = 7. (?,0,0,?) = %3D 8. (2,1,?,?) = 9. (?,?,1,-1/2) = 10. (7,?,-1,-1/2) =arrow_forward(4.10a, continued). Each electron in an atom may be characterized by a set of four quantum numbers (n, l, mỵ, mg). For each of the following, tell how many different sets of quantum numbers are possible, such that each set contains all the values listed. If it is not possible to write a set of 4 quantum numbers, write N/A (not allowed). a) n = 2, l = 2 b) n = 2, l = 0 c) n = 4, l = 2, mį = +3 d) n = 4, l =3, m¡ = -2 e) n = 3, l = 1, mį = 0 f) n = 3, l = 1 Write each set of four quantum numbers in parentheses, and follow the sequence without a comma: (n I mị mg). For example, a set for 1s subshell can be written as (1 0 0 +½) or (1 0 0 -½) where n =1, l = 0, m¡ = 0, mɛ = +½ or -/½. Only 2 sets are possible. Answer: no. of sets possible per given No. of orbitals (n I m¡ mg) subshell d) n = 4, l =3, mį = -2 e) n = 3, l = 1, mį = 0 For this part, please f) n = 3, l = 1 answer on the next pagearrow_forward
- 7.5 B What must the distance be between charges of +2.25 and −1.86 for the attractive force between them to be the same as that between charges of +4.06 and −2.11 separated by a distance of 2.16 pm?arrow_forwardPhotoelectron spectroscopy applies the principle of the pho-toelectric effect to study orbital energies of atoms and mol-ecules. High-energy radiation (usually UV or x-ray) is absorbedby a sample and an electron is ejected. The orbital energy can becalculated from the known energy of the radiation and the mea-sured energy of the electron lost. The following energy differ-ences were determined for several electron transitions:ΔE 2→1=4.098X10⁻¹⁷J, ΔE 3→1=4.854X10⁻¹⁷J, ΔE 5→1=5.242X10⁻¹⁷J, ΔE 4→2=1.024X10⁻¹⁷J Calculate the energy change and the wavelength of a photon emitted in the following transitions:(a) Level 3→2 (b) Level4→1 (c) Level5→4arrow_forward3- Consider the atom having the electron configuration 1s 2s2 2p 3s 3p. Assume that the z components of both the orbital and spin angular momenta of the electron in the 3p subshell are positive. What are the quantum numbers that describe the state of this electron? On=3,1= 1, m = 1, s = 1/2 n = 3,1 = 2, m = 1, s = 1/2 On= 3,1= 2, m 2, s =-1/2 On=3,13D 1, m = 2, s = 1/2 On=3,1 1, m = -1, s = 1/2 %3Darrow_forward
- 6.124 When a compound containing cesium ion is heatedin a Bunsen burner flame, photons with an energy of4.30 × 10−19 J are emitted. What color is the cesiumflame?arrow_forwardA typical plasma in an ICP increases the temperature of an atom by about 9000 K (i.e. from 273 K to 9273 K). If the energy difference for an atom between its ground and excited state is ΔE = 3.00 * 10-19 J, calculate the ratio of electrons in the excited state compared to the ground state. Assume the degeneracy of the ground state is 1, while the excited state is 3. constant: kboltzman = 1.381 * 10-23 J/Karrow_forward2. Electrons in molecules can be found in orbitals that extend over more than one atom. Consider one electron that is confined in a molecular orbital that extends over 8 adjacent carbon atoms. The electron can move freely between the 8 atoms. a) Using the one-dimensional particle-in-the-box model, calculate the energy required to promote an electron from the n = 2 to the n = 5 level. The length of the box is determined by the C-C bond distance, which is 139 pm.Note: The following information may or may not be useful. ?? = ?2ℎ28???2 Planck's constant = 6.626 x 10-34 J·s; Mass of Electron = 9.109 x 10-28 g; Rydberg constant = 1.097 x 107 m-1; Speed of Light = 2.998 x 108 m·s-1 b) What frequency of light would cause this excitation?c) Now imagine a straight chain of 2000 carbon atoms. Assume that the orbital extends over the entire chain and repeat the calculation for the required energy to promote an electron from the n = 2 to n = 5 level. d) Would you expect…arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Chemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning
Chemistry for Engineering Students
Chemistry
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Cengage Learning
Gerade and Ungerade Molecular Orbitals. (SYMMETRY OF MOLECULAR ORBITALS); Author: Edmerls;https://www.youtube.com/watch?v=dPY-lT5LN60;License: Standard YouTube License, CC-BY
Symmetry and chemical bonding part – 5 Molecular orbital formation (CHE); Author: Vidya-mitra;https://www.youtube.com/watch?v=g-42GmpBu0I;License: Standard Youtube License