Chemistry

Chemistry: The Central Science | 12th Edition | ISBN: 9780321696724 | Authors: Theodore E. Brown; H. Eugene LeMay; Bruce E. Bursten; Catherine Murphy; Patrick Woodward
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Chemistry: The Central Science 12th Edition solutions

Author: Theodore E. Brown; H. Eugene LeMay; Bruce E. Bursten; Catherine Murphy; Patrick Woodward
Publisher: Prentice Hall
ISBN: 9780321696724

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Chapter 3 Problems

Chapter: 3 Problem: 39E

Chemistry: The Central Science 12
The visible emission lines observed by Balmer all involved nf = 2. (a) Explain why only the lines with nf = 2 were observed in the visible region of the electromagnetic spectrum. (b) Calculate the wavelengths of the first three lines in the Balmer seriesthose for which ni = 3,4 and 5and identify th

Chapter: 3 Problem: 40E

Chemistry: The Central Science 12
Problem 40E Bohrs Model; Matter Waves (Sections) The Lyman series of emission lines of the hydrogen atom are those for which nf = 1. (a) Determine the region of the electromagnetic spectrum in which the lines of the Lyman series are observed. (b) Calculate the wavelengths of the first three lines

Chapter: 3 Problem: 41E

Chemistry: The Central Science 12
One of the emission lines of the hydrogen atom has a wavelength of 93.8 nm. (a) In what region of the electromagnetic spectrum is this emission found? (b) Determine the initial and final values of n associated with this emission.

Chapter: 3 Problem: 48E

Chemistry: The Central Science 12
Calculate the uncertainty in the position of (a) an electron moving at a speed of (3.000.01) X 105 m/s, (b) a neutron moving at this same speed. (The masses of an electron and a neutron are given in the table of fundamental constants in the inside cover of the text.) (c) What are the implications of

Chapter: 3 Problem: 77AE

Chemistry: The Central Science 12
Certain elements emit light of a specific wavelength when they are burned. Historically, chemists used such emission wavelengths to determine whether specific elements were present in a sample. Characteristic wavelengths for some of the elements are given in the following table:

Chapter: 3 Problem: 1E

Chemistry: The Central Science 12
Consider the water wave shown here. (a) How could you measure the speed of this wave? (b) How would you determine the wavelength of the wave? (c) Given the speed and wavelength of the wave, how could you determine the frequency of the wave? (d) Suggest an independent experiment to determine the frequ

Chapter: 3 Problem: 1PE

Chemistry: The Central Science 12
Problem 1PE Concepts of Wavelength and Frequency Two electromagnetic waves are represented in the margin. (a) Which wave has the higher frequency? (b) If one wave represents visible light and the other represents infrared radiation, which wave is which? If one of the waves in the margin represent

Chapter: 3 Problem: 2E

Chemistry: The Central Science 12
A popular kitchen appliance produces electromagnetic radiation with a frequency of 2450 MHz. With reference to Figure 6.4, answer the following: (a) Estimate the wavelength of this radiation. (b) Would the radiation produced by the appliance be visible to the human eye? (c) If the radiation is not vi

Chapter: 3 Problem: 2PE

Chemistry: The Central Science 12
(a) A laser used in eye surgery to fuse detached retinas produces radiation with a wavelength of 640.0 nm. Calculate the frequency of this radiation.(b) An FM radio station broadcasts electromagnetic radiation at a frequency of 103.4 MHz (megahertz; . Calculate the wavelength of this radiation. The s

Chapter: 3 Problem: 3E

Chemistry: The Central Science 12
The following diagrams represent two electromagnetic waves. Which wave corresponds to the higher-energy radiation? Explain. [Section 6.2]

Chapter: 3 Problem: 3PE

Chemistry: The Central Science 12
Problem 3PE Energy of a Photon Calculate the energy of one photon of yellow light that has a wavelength of 589 nm. (a) A laser emits light that has a frequency of 4.69 1014 s-1. What is the energy of one photon of this radiation? (b) If the laser emits a pulse containing 5.0 1017 photons of this

Chapter: 3 Problem: 4E

Chemistry: The Central Science 12
Problem 4E Visualizing Concepts As shown in the accompanying photograph, an electric stove burner on its highest setting exhibits an orange glow. (a) When the burner setting is changed to low, the burner continues to produce heat but the orange glow disappears. How can this observation be explaine

Chapter: 3 Problem: 4PE

Chemistry: The Central Science 12
Indicate whether each of the following electronic transitions emits energy or requires the absorption of energy: (a) n = 3 to n = 1; (b) n = 2 to n = 4.

Chapter: 3 Problem: 5E

Chemistry: The Central Science 12
The familiar phenomenon of a rainbow results from the diffraction of sunlight through raindrops. (a) Does the wavelength of light increase or decrease as we proceed outward from the innermost band of the rainbow? (b) Does the frequency of light increase or decrease as we proceed outward? (c) Suppose

Chapter: 3 Problem: 5PE

Chemistry: The Central Science 12
Problem 5PE Calculate the velocity of a neutron whose de Broglie wavelength is 500 pm. The mass of a neutron is given in the table inside the back cover of the text

Chapter: 3 Problem: 6E

Chemistry: The Central Science 12
A certain quantum mechanical system has the energy levels shown in the diagram below. The energy levels are indexed by a single quantum number that is an integer. (a) As drawn, which quantum numbers are involved in the transition that requires the most energy? (b) Which quantum numbers are involved

Chapter: 3 Problem: 6PE

Chemistry: The Central Science 12
Subshells of the Hydrogen Atom (a) Without referring to Table 6.2, predict the number of subshells in the fourth shell, that is, for . (b) Give the label for each of these subshells. (c) How many orbitals are in each of these subshells?

Chapter: 3 Problem: 7E

Chemistry: The Central Science 12
Consider a fictitious one-dimensional system with one electron. The wave function for the electron, drawn at the top of the next page, is \(\psi(x)=\sin x\) from to \(x=2 \pi\). (a) Sketch the probability density, \(\Psi^{2}(x)\), from \(x=0\) to \(x=2 \pi\). (b) At what value or values of \(x\) wil

Chapter: 3 Problem: 7PE

Chemistry: The Central Science 12
Problem 7PE (a) Write the electron configuration for phosphorus, element 15. (b) How many unpaired electrons does a phosphorus atom possess?

Chapter: 3 Problem: 8E

Chemistry: The Central Science 12
The contour representation of one of the orbitals for the n = 3 shell of a hydrogen atom is shown below. (a) What is the quantum number l for this orbital? (b) How do we label this orbital? (c) How would you modify this sketch to show the analogous orbital for the n = 4 shell? [Section 6.6]

Chapter: 3 Problem: 8PE

Chemistry: The Central Science 12
Problem 8PE Electron Configurations for a Group What is the characteristic valence electron configuration of the group 7A elements, the halogens? Which family of elements is characterized by an ns2np2 electron configuration in the outermost occupied shell?

Chapter: 3 Problem: 9E

Chemistry: The Central Science 12
The drawing below shows part of the orbital diagram for an element. (a) As drawn, the drawing is incorrect. Why? (b) How would you correct the drawing without changing the number of electrons? (c) To which group in the periodic table does the element belong? [Section 6.8]

Chapter: 3 Problem: 9PE

Chemistry: The Central Science 12
Use the periodic table to write the condensed electron configuration for (a) Co (element 27), (b) Te (element 52).

Chapter: 3 Problem: 10E

Chemistry: The Central Science 12
State where in the periodic table these elements appear: (a) elements with the valence-shell electron configuration \(ns^{2}np^{5}\) (b) elements that have three unpaired p electrons (c) an element whose valence electrons are \(4s^{2}4p^{1}\) (d) the d-block elements

Chapter: 3 Problem: 11E

Chemistry: The Central Science 12
Problem 11E The Wave Nature of Light (Section) What are the basic SI units for (a) the wavelength of light, (b) the frequency of light, (c) the speed of light?

Chapter: 3 Problem: 12E

Chemistry: The Central Science 12
Problem 12E The Wave Nature of Light (Section) (a) What is the relationship between the wavelength and the frequency of radiant energy? (b) Ozone in the upper atmosphere absorbs energy in the 210230-nm range of the spectrum. In what region of the electromagnetic spectrum does this radiation occur?

Chapter: 3 Problem: 13E

Chemistry: The Central Science 12
Problem 13E The Wave Nature of Light (Section) Label each of the following statements as true or false. For those that are false, correct the statement. (a) Visible light is a form of electromagnetic radiation. (b) Ultraviolet light has longer wavelengths than visible light. (c) X rays travel fa

Chapter: 3 Problem: 14E

Chemistry: The Central Science 12
Problem 14E The Wave Nature of Light (Section) Determine which of the following statements are false and correct them. (a) The frequency of radiation increases as the wavelength increases. (b) Electromagnetic radiation travels through a vacuum at a constant speed, regardless of wavelength. (c) In

Chapter: 3 Problem: 15E

Chemistry: The Central Science 12
Problem 15E The Wave Nature of Light (Section) Arrange the following kinds of electromagnetic radiation in order of increasing wavelength: infrared, green light, red light, radio waves, X rays, ultraviolet light.

Chapter: 3 Problem: 16E

Chemistry: The Central Science 12
Problem 16E The Wave Nature of Light (Section) List the following types of electromagnetic radiation in order of increasing wavelength: (a) the gamma rays produced by a radioactive nuclide used in medical imaging; (b) radiation from an FM radio station at 93.1 MHz on the dial; (c) a radio signal

Chapter: 3 Problem: 17E

Chemistry: The Central Science 12
Problem 17E The Wave Nature of Light (Section) (a) What is the frequency of radiation that has a wavelength of 10 ?m, about the size of a bacterium? (b) What is the wavelength of radiation that has a frequency of 5.50 1014 s-1? (c) Would the radiations in part (a) or part (b) be visible to the

Chapter: 3 Problem: 18E

Chemistry: The Central Science 12
(a) What is the frequency of radiation whose wavelength is 5.1x10-5 ? (b) What is the wavelength of radiation that has a frequency of 2.5x108s-1 (c) Would the radiations in part (a) or part (b) be detected by an X-ray detector? (d) What distance does electromagnetic radiation travel in 10.5 fs?

Chapter: 3 Problem: 19E

Chemistry: The Central Science 12
An argon ion laser emits light at 532 nm. What is the frequency of this radiation? Using Figure 6.4, predict the color associated with this wavelength.

Chapter: 3 Problem: 20E

Chemistry: The Central Science 12
It is possible to convert radiant energy into electrical energy using photovoltaic cells. Assuming equal efficiency of conversion, would infrared or ultraviolet radiation yield more electrical energy on a per-photon basis?

Chapter: 3 Problem: 21E

Chemistry: The Central Science 12
Problem 21E If human height were quantized in one-foot increments, what would happen to the height of a child as she grows up?

Chapter: 3 Problem: 22E

Chemistry: The Central Science 12
Problem 22E Quantized Energy and Photons (Section) Einsteins 1905 paper on the photoelectric effect was the first important application of Plancks quantum hypothesis. Describe Plancks original hypothesis, and explain how Einstein made use of it in his theory of the photoelectric effect.

Chapter: 3 Problem: 23E

Chemistry: The Central Science 12
(a) Calculate the energy of a photon of electromagnetic radiation whose frequency is \(6.75 \times 10^{12}\) \(s^{-1}\). (b) Calculate the energy of a photon of radiation whose wavelength is 322 nm. (c) What wavelength of radiation has photons of energy \(2.87 \times 10^{-18}\) J?

Chapter: 3 Problem: 24E

Chemistry: The Central Science 12
Problem 24E (a) A red laser pointer emits light with a wavelength of 650 nm. What is the frequency of this light? (b) What is the energy of one of these photons? (c) The laser pointer emits light because electrons in the material are excited (by a battery) from their ground state to an upper exci

Chapter: 3 Problem: 25E

Chemistry: The Central Science 12
(a) Calculate and compare the energy of a photon of wavelength with that of wavelength . (b) Use Figure to identify the region of the electromagnetic spectrum to which each belongs.

Chapter: 3 Problem: 26E

Chemistry: The Central Science 12
Problem 26E Quantized Energy and Photons (Section) An AM radio station broadcasts at 1010 kHz, and its FM partner broadcasts at 98.3 MHz. Calculate and compare the energy of the photons emitted by these two radio stations.

Chapter: 3 Problem: 27E

Chemistry: The Central Science 12
Problem 27E Quantized Energy and Photons (Section) One type of sunburn occurs on exposure to UV light of wavelength in the vicinity of 325 nm. (a) What is the energy of a photon of this wavelength? (b) What is the energy of a mole of these photons? (c) How many photons are in a 1.00 mJ burst of t

Chapter: 3 Problem: 28E

Chemistry: The Central Science 12
The energy from radiation can be used to cause the rupture of chemical bonds. A minimum energy of 941 kJ/mol is required to break the nitrogennitrogen bond in N2. What is the longest wavelength of radiation that possesses the necessary energy to break the bond? What type of electromagnetic radiation

Chapter: 3 Problem: 29E

Chemistry: The Central Science 12
Quantized Energy and Photons (Section) A diode laser emits at a wavelength of 987 nm. (a) In what portion of the electromagnetic spectrum is this radiation found? (b) All of its output energy is absorbed in a detector that measures a total energy of 0.52 J over a period of 32 s. How many

Chapter: 3 Problem: 30E

Chemistry: The Central Science 12
Problem 30E Quantized Energy and Photons (Section) A stellar object is emitting radiation at 3.55 mm. (a) What type of electromagnetic spectrum is this radiation? (b) If a detector is capturing 3.2 108 photons per second at this wavelength, what is the total energy of the photons detected in 1.0

Chapter: 3 Problem: 31E

Chemistry: The Central Science 12
Problem 31E Quantized Energy and Photons (Section) Molybdenum metal must absorb radiation with a minimum frequency of 1.09 1015 s-1 before it can eject an electron from its surface via the photoelectric effect. (a) What is the minimum energy needed to eject an electron? (b) What wavelength of ra

Chapter: 3 Problem: 32E

Chemistry: The Central Science 12
Sodium metal requires a photon with a minimum energy of to emit electrons. (a) What is the minimum frequency of light necessary to emit electrons from sodium via the photoelectric effect? (b) What is the wavelength of this light? (c) If sodium is irradiated with light of , what is the maximum possib

Chapter: 3 Problem: 33E

Chemistry: The Central Science 12
Problem 33E Bohrs Model; Matter Waves (Sections) Explain how the existence of line spectra is consistent with Bohrs theory of quantized energies for the electron in the hydrogen atom.

Chapter: 3 Problem: 34E

Chemistry: The Central Science 12
Problem 34E (a) In terms of the Bohr theory of the hydrogen atom, what process is occurring when excited hydrogen atoms emit radiant energy of certain wavelengths and only those wavelengths? (b) Does a hydrogen atom expand or contract as it moves from its ground state to an excited state?

Chapter: 3 Problem: 35E

Chemistry: The Central Science 12
Problem 35E Bohrs Model; Matter Waves (Sections) Is energy emitted or absorbed when the following electronic transitions occur in hydrogen? (a) from n = 4 to n = 2, (b) from an orbit of radius 2.12 to one of radius 8.46 , (c) an electron adds to the H+ ion and ends up in the n = 3 shell?

Chapter: 3 Problem: 36E

Chemistry: The Central Science 12
Problem 36E Bohrs Model; Matter Waves (Sections) Indicate whether energy is emitted or absorbed when the following electronic transitions occur in hydrogen: (a) from n = 2 to n = 6, (b) from an orbit of radius 4.76 to one of radius 0.529 , (c) from the n = 6 to the n = 9 state.

Chapter: 3 Problem: 37E

Chemistry: The Central Science 12
(a) Using Equation 6.5, calculate the energy of an electron in the hydrogen atom when n = 6 and when n = 2. Calculate the wavelength of the radiation released when an electron moves from n = 6 n = 2. (b) Is this line in the visible region of the electromagnetic spectrum? If so, what color is it?

Chapter: 3 Problem: 38E

Chemistry: The Central Science 12
(a) Calculate the energies of an electron in the hydrogen atom for n = 1 and for \(n=\infty\). How much energy does it require to move the electron out of the atom completely (from n = 1 to \(n=\infty\) ), according to Bohr? Put your answer in kJ/mol. (b) The energy for the process \(\mathrm{H}+\)

Chapter: 3 Problem: 42E

Chemistry: The Central Science 12
Problem 42E The hydrogen atom can absorb light of wavelength 2626 nm. (a) In what region of the electromagnetic spectrum is this absorption found? (b) Determine the initial and final values of n associated with this absorption.

Chapter: 3 Problem: 43E

Chemistry: The Central Science 12
Use the de Broglie relationship to determine the wavelengths of the following objects: (a) an 85-kg person skiing at 50 km/hr, (b) a 10.0-g bullet fired at 250 m/s, (c) a lithium atom moving at \(2.5 \times 10^5\) m/s, (d) an ozone (\(O_3\)) molecule in the upper atmosphere moving at 550 m/s.

Chapter: 3 Problem: 44E

Chemistry: The Central Science 12
Problem 44E Bohrs Model; Matter Waves (Sections) Among the elementary subatomic particles of physics is the muon, which decays within a few nanoseconds after formation. The muon has a rest mass 206.8 times that of an electron. Calculate the de Broglie wavelength associated with a muon traveling at

Chapter: 3 Problem: 45E

Chemistry: The Central Science 12
Neutron diffraction is an important technique for determining the structures of molecules. Calculate the velocity of a neutron needed to achieve a wavelength of 0.955 . (Refer to the inside cover for the mass of the neutron).

Chapter: 3 Problem: 46E

Chemistry: The Central Science 12
The electron microscope has been widely used to obtain highly magnified images of biological and other types of materials. When an electron is accelerated through a particular potential field, it attains a speed of 8.95 X 106 m/s. What is the characteristic wavelength of this electron? Is the wavelen

Chapter: 3 Problem: 47E

Chemistry: The Central Science 12
Problem 47E Bohrs Model; Matter Waves (Sections) Using Heisenbergs uncertainty principle, calculate the uncertainty in the position of (a) a 1.50-mg mosquito moving at a speed of 1.40 m/s if the speed is known to within 0.01 m/s; (b) a proton moving at a speed of (5.00 0.01) 104 m/s. (The mass

Chapter: 3 Problem: 49E

Chemistry: The Central Science 12
Problem 49E Quantum Mechanics and Atomic Orbitals (Sections) (a) Why does the Bohr model of the hydrogen atom violate the uncertainty principle? (b) In what way is the description of the electron using a wave function consistent with de Broglies hypothesis? (c) What is meant by the term probabili

Chapter: 3 Problem: 50E

Chemistry: The Central Science 12
Problem 50E Quantum Mechanics and Atomic Orbitals (Sections) (a) According to the Bohr model, an electron in the ground state of a hydrogen atom orbits the nucleus at a specific radius of 0.53 . In the quantum mechanical description of the hydrogen atom, the most probable distance of the electron f

Chapter: 3 Problem: 51E

Chemistry: The Central Science 12
Problem 51E Quantum Mechanics and Atomic Orbitals (Sections) (a) For n = 4, what are the possible values of l? (b) For l = 2, what are the possible values of ml? (c) If ml is 2, what are the possible values for l?

Chapter: 3 Problem: 52E

Chemistry: The Central Science 12
Problem 52E Quantum Mechanics and Atomic Orbitals (Sections) How many possible values for l and ml are there when (a) n = 3, (b) n = 5?

Chapter: 3 Problem: 53E

Chemistry: The Central Science 12
Problem 53E Quantum Mechanics and Atomic Orbitals (Sections) Give the numerical values of n and l corresponding to each of the following orbital designations: (a) 3p, (b) 2s,(c) 4f,(d) 5d.

Chapter: 3 Problem: 54E

Chemistry: The Central Science 12
Problem 54E Quantum Mechanics and Atomic Orbitals (Sections) Give the values for n, l, and ml for (a) each orbital in the 2p subshell, (b) each orbital in the 5d subshell.

Chapter: 3 Problem: 55E

Chemistry: The Central Science 12
Problem 55E Quantum Mechanics and Atomic Orbitals (Sections) Which of the following represent impossible combinations of n and l? (a) 1p, (b) 4s, (c) 5f, (d) 2d

Chapter: 3 Problem: 56E

Chemistry: The Central Science 12
Problem 56E Quantum Mechanics and Atomic Orbitals (Sections) For the table that follows, write which orbital goes with the quantum numbers. Dont worry about x, y, z subscripts. If the quantum numbers are not allowed, write not allowed. N l ml Orbital 2 1 -1 2p (example) 1 0 0 3 -3 2

Chapter: 3 Problem: 57E

Chemistry: The Central Science 12
Quantum Mechanics and Atomic Orbitals (Sections) Sketch the shape and orientation of the following types of orbitals: (a) s, (b) pz, (c) dxy.

Chapter: 3 Problem: 58E

Chemistry: The Central Science 12
Problem 58E Quantum Mechanics and Atomic Orbitals (Sections) Sketch the shape and orientation of the following types of orbitals: (a) px, (b) dz2, (c) dx2 - y2.

Chapter: 3 Problem: 59E

Chemistry: The Central Science 12
(a) What are the similarities of and differences between the 1s and 2s orbitals of the hydrogen atom? (b) In what sense does a 2p orbital have directional character? Compare the directional characteristics of the \(p_x\) and \(d_{x^2 - y^2}\) orbitals. (That is, in what direction or region of spac

Chapter: 3 Problem: 60E

Chemistry: The Central Science 12
(a) With reference to Figure 6.18, what is the relationship between the number of nodes in an s orbital and the value of the principal quantum number? (b) Identify the number of nodes; that is, identify places where the electron density is zero, in the orbital; in the 3s orbital. (c) What information

Chapter: 3 Problem: 61E

Chemistry: The Central Science 12
For a given value of the principal quantum number, n, how do the energies of the s, p, d, and f subshells vary for (a) hydrogen, (b) a many-electron atom?

Chapter: 3 Problem: 62E

Chemistry: The Central Science 12
Problem 62E Many-Electron Atoms and Electron Configurations (Sections) (a) The average distance from the nucleus of a 3s electron in a chlorine atom is smaller than that for a 3p electron. In light of this fact, which orbital is higher in energy? (b) Would you expect it to require more or less ener

Chapter: 3 Problem: 63E

Chemistry: The Central Science 12
Many-Electron Atoms and Electron Configurations (Sections) (a) What experimental evidence is there for the electron having a spin? (b) Draw an energy-level diagram that shows the relative energetic positions of a 1s orbital and a 2s orbital. Put two electrons in the 1s orbital. (c) Draw an arrow

Chapter: 3 Problem: 64E

Chemistry: The Central Science 12
Problem 64E Many-Electron Atoms and Electron Configurations (Sections) (a) State the Pauli exclusion principle in your own words. (b) The Pauli exclusion principle is, in an important sense, the key to understanding the periodic table. (c) Explain.

Chapter: 3 Problem: 65E

Chemistry: The Central Science 12
Problem 65E Many-Electron Atoms and Electron Configurations (Sections) What is the maximum number of electrons that can occupy each of the following subshells? (a) 3p, (b) 5d, (c) 2s, (d) 4f.

Chapter: 3 Problem: 66E

Chemistry: The Central Science 12
What is the maximum number of electrons in an atom that can have the following quantum numbers: (a) , , (b) (c) (d) ?

Chapter: 3 Problem: 67E

Chemistry: The Central Science 12
Problem 67E Many-Electron Atoms and Electron Configurations (Sections) (a) What are valence electrons? (b) What are core electrons? (c) What does each box in an orbital diagram represent? (d) What quantity is represented by the half arrows in an orbital diagram?

Chapter: 3 Problem: 68E

Chemistry: The Central Science 12
Problem 68E For each element, indicate the number of valence electrons, core electrons, and unpaired electrons in the ground state: (a) carbon, (b) phosphorus, (c) neon.

Chapter: 3 Problem: 69E

Chemistry: The Central Science 12
Problem 69E Many-Electron Atoms and Electron Configurations (Sections) Write the condensed electron configurations for the following atoms, using the appropriate noble-gas core abbreviations: (a) Cs, (b) Ni, (c) Se, (d) Cd, (e) U, (f) Pb.

Chapter: 3 Problem: 70E

Chemistry: The Central Science 12
Problem 70E Many-Electron Atoms and Electron Configurations (Sections) Write the condensed electron configurations for the following atoms and indicate how many unpaired electrons each has: (a) Mg, (b) Ge, (c) Br, (d) V, (e) Y, (f) Lu.

Chapter: 3 Problem: 71E

Chemistry: The Central Science 12
Problem 71E Many-Electron Atoms and Electron Configurations (Sections) Identify the specific element that corresponds to each of the following electron configurations and indicate the number of unpaired electrons for each: (a) 1s22s2, (b) 1s22s22p4, (c) [Ar]4s13d5, (d) [Kr]5s24d105p4.

Chapter: 3 Problem: 72E

Chemistry: The Central Science 12
Problem 72E Many-Electron Atoms and Electron Configurations (Sections) Identify the group of elements that corresponds to each of the following generalized electron configurations and indicate the number of unpaired electrons for each: (a) [noble gas] ns2np5 ________________ (b) [noble gas] ns2(n

Chapter: 3 Problem: 73E

Chemistry: The Central Science 12
Problem 73E Many-Electron Atoms and Electron Configurations (Sections) What is wrong with the following electron configurations for atoms in their ground states? (a) 1s22s23s1, (b) [Ne]2s22p3, (c) [Ne]3s23d5.

Chapter: 3 Problem: 74E

Chemistry: The Central Science 12
The following electron configurations represent excited states. Identify the element, and write its ground-state condensed electron configuration. (a) , (b) (c)

Chapter: 3 Problem: 75AE

Chemistry: The Central Science 12
Consider the two waves shown here, which we will consider to represent two electromagnetic radiations: (a) What is the wavelength of wave A? Of wave B? (b) What is the frequency of wave A? Of wave B? (c) Identify the regions of the electromagnetic spectrum to which waves A and B belong

Chapter: 3 Problem: 76AE

Chemistry: The Central Science 12
Problem 76AE If you put 120 volts of electricity through a pickle, the pickle will smoke and start glowing orange-yellow. The light is emitted because sodium ions in the pickle become excited; their return to the ground state results in light emission. (a) The wavelength of this emitted light is 58

Chapter: 3 Problem: 78AE

Chemistry: The Central Science 12
Problem 78AE In June 2004, the CassiniHuygens spacecraft began orbiting Saturn and transmitting images to Earth. The closest distance between Saturn and Earth is 746 million miles. What is the minimum amount of time it takes for the transmitted signals to travel from the spacecraft to Earth?

Chapter: 3 Problem: 79AE

Chemistry: The Central Science 12
Problem 79AE The rays of the Sun that cause tanning and burning are in the ultraviolet portion of the electromagnetic spectrum. These rays are categorized by wavelength. So-called UV-A radiation has wavelengths in the range of 320380 nm, whereas UV-B radiation has wavelengths in the range of 290320

Chapter: 3 Problem: 80AE

Chemistry: The Central Science 12
Problem 80AE The watt is the derived SI unit of power, the measure of energy per unit time: 1 W = 1 J/s. A semiconductor laser in a CD player has an output wavelength of 780 nm and a power level of 0.10 mW. How many photons strike the CD surface during the playing of a CD 69 minutes in length?

Chapter: 3 Problem: 81AE

Chemistry: The Central Science 12
Carotenoids are yellow, orange, and red pigments synthesized by plants. The observed color of an object is not the color of light it absorbs but rather the complementary color, as described by a color wheel such as the one shown here. On this wheel, complementary colors are across from each other. (a

Chapter: 3 Problem: 82AE

Chemistry: The Central Science 12
A photocell is a device used to measure the intensity of light. In a certain experiment, when light of wavelength 630 nm is directed onto the photocell, electrons are emitted at the rate of 2.6 X 10-12 C/s (coulombs per second). Assume that each photon that impinges on the photocell emits one electro

Chapter: 3 Problem: 83AE

Chemistry: The Central Science 12
In an experiment to study the photoelectric effect, a scientist measures the kinetic energy of ejected electrons as a function of the frequency of radiation hitting a metal surface. She obtains the following plot. The point labeled " " corresponds to light with a wavelength of . (a) What is the valu

Chapter: 3 Problem: 84AE

Chemistry: The Central Science 12
The human retina has three types of receptor cones, each sensitive to a different range of wavelengths of visible light, as shown in this figure (the colors are merely to differentiate the three curves from one another; they do not indicate the actual colors represented by each curve): (a) Es

Chapter: 3 Problem: 85AE

Chemistry: The Central Science 12
The series of emission lines of the hydrogen atom for which nf = 3 is called the Paschen series. (a) Determine the region of the electromagnetic spectrum in which the lines of the Paschen series are observed. (b) Calculate the wavelengths of the first three lines in the Paschen seriesthose for which

Chapter: 3 Problem: 86AE

Chemistry: The Central Science 12
When the spectrum of light from the Sun is examined in high resolution in an experiment similar to that illustrated in Figure 6.9, dark lines are evident. These are called Fraunhofer lines, after the scientist who studied them extensively in the early nineteenth century. Altogether, about 25,000 line

Chapter: 3 Problem: 87AE

Chemistry: The Central Science 12
Bohrs model can be used for hydrogen-like ionsions that have only one electron, such as HE+ and Li2+ . (a) Why is the Bohr model applicable to HE+ ions but not to neutral He atoms? (b) The ground-state energies of H, HE+, Li2+ and are tabulated as follows: By examining these numbers, propose

Chapter: 3 Problem: 88AE

Chemistry: The Central Science 12
An electron is accelerated through an electric potential to a kinetic energy of . What is its characteristic wavelength? [Hint: Recall that the kinetic energy of a moving object is , where is the mass of the object and is the speed of the object.]

Chapter: 3 Problem: 89AE

Chemistry: The Central Science 12
In the television series Star Trek, the transporter beam is a device used to beam down people from the Starship Enterprise to another location, such as the surface of a planet. The writers of the show put a Heisenberg compensator into the transporter beam mechanism. Explain why such a compensator (wh

Chapter: 3 Problem: 90AE

Chemistry: The Central Science 12
Problem 90AE Which of the quantum numbers governs (a) the shape of an orbital, (b) the energy of an orbital, (c) the spin properties of the electron, (d) the spatial orientation of the orbital?

Chapter: 3 Problem: 91AE

Chemistry: The Central Science 12
Consider the discussion of radial probability functions in A Closer Look in Section 6.6.(a) What is the difference between the probability density as a function of r and the radial probability function as a function of r ? (b) What is the significance of the term in the radial probability functions

Chapter: 3 Problem: 92AE

Chemistry: The Central Science 12
For orbitals that are symmetric but not spherical, the contour representations (as in Figures 6.22 and 6.23) suggest where nodal planes exist (that is, where the electron density is zero). For example, the px orbital has a node wherever x = 0. This equation is satisfied by all points on the yz plane,

Chapter: 3 Problem: 93AE

Chemistry: The Central Science 12
The Chemistry and Life box in Section 6.7 described the techniques called NMR and MRI. (a) Instruments for obtaining MRI data are typically labeled with a frequency, such as 600 MHz. Why do you suppose this label is relevant to the experiment? (b) What is the value of in Figure 6.27 that would corre

Chapter: 3 Problem: 94AE

Chemistry: The Central Science 12
Suppose that the spin quantum number, \(m_s\), could have three allowed values instead of two. How would this affect the number of elements in the first four rows of the periodic table?

Chapter: 3 Problem: 95AE

Chemistry: The Central Science 12
Problem 95AE Using the periodic table as a guide, write the condensed electron configuration and determine the number of unpaired electrons for the ground state of (a) Si, (b) Zn, (c) Zr, (d) Sn, (e) Ba, (f) Tl.

Chapter: 3 Problem: 96AE

Chemistry: The Central Science 12
Problem 96AE Scientists have speculated that element 126 might have a moderate stability, allowing it to be synthesized and characterized. Predict what the condensed electron configuration of this element might be.

Chapter: 3 Problem: 97IE

Chemistry: The Central Science 12
Problem 97IE Microwave ovens use microwave radiation to heat food. The energy of the microwaves is absorbed by water molecules in food and then transferred to other components of the food. (a) Suppose that the microwave radiation has a wavelength of 11.2 cm. How many photons are required to heat 20

Chapter: 3 Problem: 98IE

Chemistry: The Central Science 12
Problem 98IE The stratospheric ozone (O3) layer helps to protect us from harmful ultraviolet radiation. It does so by absorbing ultraviolet light and falling apart into an O2 molecule and an oxygen atom, a process known as photodissociation. O3(g)?O2(g) + O(g) Use the data in Appendix C to calculat

Chapter: 3 Problem: 99IE

Chemistry: The Central Science 12
Problem 99IE The discovery of hafnium, element number 72, provided a controversial episode in chemistry. G. Urbain, a French chemist, claimed in 1911 to have isolated an element number 72 from a sample of rare earth (elements 5871) compounds. However, Niels Bohr believed that hafnium was more likel

Chapter: 3 Problem: 100IE

Chemistry: The Central Science 12
(a) Account for formation of the following series of oxides in terms of the electron configurations of the elements and the discussion of ionic compounds in Section 2.7: . (b) Name these oxides. (c) Consider the metal oxides whose enthalpies of formation (in kJ mol-1) are listed here.

Chapter: 3 Problem: 101IE

Chemistry: The Central Science 12
Problem 101IE The first 25 years of the twentieth century were momentous for the rapid pace of change in scientists understanding of the nature of matter. (a) How did Rutherfords experiments on the scattering of a particles by a gold foil set the stage for Bohrs theory of the hydrogen atom? (b) In

Chapter: 3 Problem: 102IE

Chemistry: The Central Science 12
The two most common isotopes of uranium are 235U and 238U . (a) Compare the number of protons, the number of electrons, and the number of neutrons in atoms of these two isotopes. (b) Using the periodic table in the front inside cover, write the electron configuration for a U atom.(c) Compare your ans

Chapter: 3 Problem: 103IE

Chemistry: The Central Science 12
Imagine sunlight falling on three square areas. One is an inert black material. The second is a photovoltaic cell surface, which converts radiant energy into electricity. The third is an area on a green tree leaf. Draw diagrams that show the energy conversions in each case, using Figure 5.9 as a mode

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