Problem 1PE: Practice Exercise 7.1
Helium derives its name from the Latin name for the sun. Helium was discovered... Problem 2PE: Practice Exercise 7.2
Radio station KRED in Eureka, (California, broadcasts electromagnetic... Problem 3PE: Calculate the wavelength in micrometers, m, of radiation expected when n1=4 and n2=6. Report your... Problem 4PE: Practice Exercise 7.4
Calculate the wavelength in nanometers of the spectral line in the visible... Problem 5PE: What is the energy of the radiation emitted when an electron in a hydrogen drops from an energy... Problem 6PE: Practice Exercise 7.6
If the energy of light emitted from a hydrogen atom as an electron moves from... Problem 7PE: Calculate the energy of an electron in its lowest energy state trapped on a one-dimensional wire... Problem 8PE: Practice Exercise 7.8
If an electron moves from a one-dimensional wire with a length of 1 nm at n =... Problem 9PE: Practice Exercise 7.9
What are the values of n and for the following subshells? (a) 4d, (b) 5f and... Problem 10PE: What subshells would be found in the shells with n=2 and n=5? How is the number of subshells related... Problem 11PE: Without looking at the tables in the text, how many electrons are there in a d subshell? (Hint: How... Problem 12PE Problem 13PE: Practice Exercise 7.13
Draw orbital diagrams for (a) Na, (b) S, and (c) Ar. (Hint: Recall how we... Problem 14PE: Practice Exercise 7.14
Use Figure 7.18 to predict the electron configurations of (a) Si, (b) Ti, and... Problem 15PE: Can an dement with an even atomic number be paramagnetic? (Hint: Try writing the orbital diagrams of... Problem 16PE: Practice Exercise 7.16
Use orbital diagrams to determine how many unpaired electrons are in each of... Problem 17PE: Practice Exercise 7.17
Use the periodic table to predict the electron configurations of (a) Mg, (b)... Problem 18PE: Use the periodic table to predict the electron configurations of (a) O, S, Se and (b) P, N, Sb. What... Problem 19PE: Practice Exercise 7.19
Write shorthand configurations and abbreviated orbital diagrams for (a) Zr... Problem 20PE: Write shorthand configurations and abbreviated orbital diagrams for (a) P and (b) Sn. Where... Problem 21PE: Practice Exercise 7.21
Give an example of a valence shell with more than eight electrons. If that is... Problem 22PE Problem 23PE Problem 24PE: Practice Exercise 7.24
Use the periodic table to determine the smallest atom or ion in each group,... Problem 25PE: Use the periodic table to select the atom with the most positive value for its first ionization... Problem 26PE Problem 1RQ: In general terms, why do we call light electromagnetic radiation? Problem 2RQ: In general, what does the term frequency imply? What is meant by the term frequency of light? What... Problem 3RQ: What is meant by the term wavelength of light? What symbol is used for it? Problem 4RQ: 7.4 Sketch a picture of a wave and label its wavelength and its amplitude. Indicate how frequency... Problem 5RQ: Which property of light waves is a measure of the brightness of the light? Which specifies the color... Problem 6RQ: Arrange the following regions of the electromagnetic spectrum in order of increasing wavelength... Problem 7RQ: 7.7 What wavelength range is covered by the visible spectrum?
Problem 8RQ: Arrange the following colors of visible light in order of increasing wavelength: orange, green,... Problem 9RQ: What is the equation that relates the wavelength and frequency of a light wave? (Define all symbols... Problem 10RQ: How is the frequency of a particular type of radiation related to the energy associated with it?... Problem 11RQ: 7.11 What is a photon?
Problem 12RQ: Show that the energy of a photon is given by the equation E=hc Problem 13RQ: Examine each of the following pairs and state which of the two has the higher energy: (a) microwaves... Problem 14RQ: What is a quantum of energy? Problem 15RQ Problem 16RQ Problem 17RQ: Describe Niels Bohrs model of the structure of the hydrogen atom. Problem 18RQ Problem 19RQ: Why does the equation for the energy of an electron in a Bohr atom have a negative sign? Problem 20RQ: In what way was Bohrs theory a success? How failure? Problem 21RQ: 7.21 How does the behavior of very small particles differ from that of the larger, more massive... Problem 22RQ: Describe the phenomenon called diffraction. How can this be used to demonstrate that de Broglies... Problem 23RQ: What experiment could you perform to determine whether a beam was behaving as a wave or as a stream... Problem 24RQ: 7.24 What is wave/particle duality?
Problem 25RQ Problem 26RQ: What is the collapsing atom paradox? Problem 27RQ: How does quantum mechanics resolve the collapsing atom paradox? Problem 28RQ: What are the names used to refer to the theories that apply the matterwave concept to electrons in... Problem 29RQ: What is the term used to describe a particular waveform of a standing wave for an electron? Problem 30RQ: What are the three properties of orbitals in which we are most interested? Why? Problem 31RQ: What are the allowed values of the principal quantum number? Of the secondary quantum numbers? Of... Problem 32RQ: What information does each type of quantum number give for an atomic orbital? Problem 33RQ: How does the value of n in the Rydberg equation relate to the principle quantum number, n? Problem 34RQ: Why is (a) the d subshell in the Period 4 designated as 3d and (b) the f subshell in Period 7... Problem 35RQ: Why does every shell contain an s subshell? Problem 36RQ: How many orbitals are found in (a) an s subshell, (b) a p subshell, (c) a d subshell, and (d) an f... Problem 37RQ: 7.37 If the value of for an electron in an atom is 2, could another electron in the same subshell... Problem 38RQ: 7.38 What physical property of electrons leads us to propose that they spin like a toy top?
Problem 39RQ: Explain the two magnetic properties that are affected by the number of unpaired electrons. Problem 40RQ: What is the Pauli exclusion principle? What effect does it have on the populating of orbitals by... Problem 41RQ: What are the possible values of the spin quantum number? Problem 42RQ: Suppose an electron in an atom has the following set of quantum numbers: n=2,l=1,ml=1,ms=+12. What... Problem 43RQ Problem 44RQ Problem 45RQ: Within any given shell, how do the energies of the s, p, d, and f subshells compare? How do the... Problem 46RQ Problem 47RQ: Give the electron configurations of the elements in Period 2 of the periodic table. Problem 48RQ: 7.48 Using your own words, describe how to use the periodic table to write the electron... Problem 49RQ: Give the correct electron configurations of (a) Cr and (b) Cu. Explain why they do not have the... Problem 50RQ: What is the correct electron configuration of silver? Why is this electron configuration different... Problem 51RQ: How are the electron configurations of the elements in a given group similar? Illustrate your answer... Problem 52RQ: Define the terms valence shell and valence electrons. Define core electrons. Problem 53RQ: Why do we use probabilities when we discuss the position of an electron in the space surrounding the... Problem 54RQ: Sketch the approximate shape of (a) a 1s orbital and (b) a 2p orbital. Problem 55RQ: How does the size of a given type of orbital vary with n? Problem 56RQ: How are the p orbitals of a given p subshell oriented relative to each other? Problem 57RQ: What is a nodalplane? How are the number of nodal planes relate to the value of l? Problem 58RQ: What is a radial node? How are the number of radial nodes related to the value of n and l? Problem 59RQ: 7.59 How many nodal planes does a p orbital have? How many does a d orbital have?
Problem 60RQ: On appropriate coordinate axes, sketch the shape of the following d orbitals: (a) dxy , (b) dx2y2,... Problem 61RQ: What is the meaning of effective nuclear charge? How does the effective nuclear charge felt by the... Problem 62RQ: *7.62 Explain why a 3s electron in Al experiences a greater effective nuclear charge than a 3p... Problem 63RQ: Explain why the atomic size varies across the periodic table and down the periodic table. Problem 64RQ: Explain why cations are smaller than their uncharged atoms and anions are larger than their... Problem 65RQ Problem 66RQ: Going from left to right in the periodic table, why are the size changes among the transition... Problem 67RQ Problem 68RQ Problem 69RQ: Explain why ionization energy increases from left to right in a period and decreases from top to... Problem 70RQ Problem 71RQ Problem 72RQ Problem 73RQ: Why does phosphorus have a larger first ionization energy than sulfur? Problem 74RQ Problem 75RQ: 7.75 For sulfur, write an equation for the change associated with (a) its first electron affinity... Problem 76RQ: 7.76 Why does Cl have a more exothermic electron affinity than F? Why does Br have a less exothermic... Problem 77RQ Problem 78RQ: How is electron affinity related, to effective nuclear charge? On this basis, explain the relative... Problem 79RQ: 7.79 What is the frequency in hertz of blue light having a wavelength of 436 nm?
Problem 80RQ: Ultraviolet light with a wavelength of more than 295 nm has little germicidal value. What is the... Problem 81RQ: Ozone protects the earths inhabitants from the harmful effects of ultraviolet light arriving from... Problem 82RQ: The meter is defined as the length of the path light travels in a vacuum during the time interval of... Problem 83RQ: In New York City, radio station WCBS broadcasts its FM signal at a frequency of 101.1 megahertz... Problem 84RQ: Sodium vapor lamps are often used in residential street lighting. Sodium gives off two yellow lines... Problem 85RQ: 7.85 Calculate the energy in joules of a photon of red light having a frequency of . What is the... Problem 86RQ: Calculate the energy in joules of a photon of green light having a wavelength of 563 nm. Problem 87RQ: In the spectrum of hydrogen, there is a line with a wavelength of 410.3 nm. (a) What color is this... Problem 88RQ: 7.88 In the spectrum of sodium, there is a line with a wavelength of 589 nm. (a) What color is this... Problem 89RQ: Use the Rydberg equation to calculate the wavelength in nanometers of the spectral line of hydrogen... Problem 90RQ: 7.90 Use the Rydberg equation to calculate the wavelength in nanometers of the spectral line of... Problem 91RQ: Calculate the wavelength and energy in joules of the spectral line produced in the hydrogen spectrum... Problem 92RQ: Calculate the energy in joules and the wavelength in nanometers of the spectral line produced in the... Problem 93RQ: What is the letter code for a subshell with (a)l=1and(b)l=3? Problem 94RQ: 7.94 What is the letter code for a subshell with ?
Problem 95RQ: What is the value of l for (a) an f orbital and (b) a d orbital? Problem 96RQ: 7.96 What is the value of for (a) a p orbital and (b) a g orbital?
Problem 97RQ: What are the values of n and l for the subshells: (a) 3s, (b) 5d? Problem 98RQ: Give the values of n and l for the subshells: (a) 4p,(b) 6f Problem 99RQ: For the shell with n = 6, what are the possible values of l? Problem 100RQ: 7.100 What values of are possible for a shell with n = 4?
Problem 101RQ: In a particular shell, the largest value of l is 7. What is the value of n for this shell? Problem 102RQ: What is the value of n for a shell if the largest value of l is 5? Problem 103RQ: What are the possible values of ml for a subshell with (a)l=1and(b)l=3? Problem 104RQ: If the value of l for an electron in an atom is 5, what are the possible values of ml that this... Problem 105RQ: If the value of ml for an electron in an atom is -4, what is the smallest value of l that the... Problem 106RQ: How many orbitals are there in an h subshell (l=5)? What are the possible values of ml? Problem 107RQ: 7.107 Give the complete set of quantum numbers for all of the electrons that could populate the 2p... Problem 108RQ: 7.108 Give the complete set of quantum numbers for all of the electrons that could populate the 3d... Problem 109RQ: *7.109 In an antimony atom, how many electrons have ?
Problem 110RQ Problem 111RQ: Give the electron configurations of (a)S,(b)K,(c)Ti,and(d)Sn. Problem 112RQ: 7.112 Write the electron configurations of (a) As, (b) Cl, (c) Ni, and (d) Si.
Problem 113RQ: 7.113 Which of the following atoms in their ground states are expected to be paramagnetic: (a) Mn,... Problem 114RQ: Which of the following atoms in their ground states are expected to be diamagnetic: (a) Ba, (b) Se,... Problem 115RQ Problem 116RQ Problem 117RQ: Write the abbreviated electron configurations for (a)Ni,(b)Cs,(c)Ge,(d)Br, and(e)Bi. Problem 118RQ: Write the abbreviated electron configurations for (a)Al,(b)Se,(c)Ba,(d)Sb,and(e)Gd. Problem 119RQ: Draw complete orbital diagrams for (a) Mg and (b) Ti. Problem 120RQ: Draw complete orbital diagrams for (a) As and (b) Ni. Problem 121RQ: 7.121 Draw orbital diagrams for the abbreviated configurations of
Problem 122RQ: Draw orbital diagrams for the abbreviated configurations of (a)Al,(b)Se,(c)Ba,and(d)Sb. Problem 123RQ: What is the value of n for the valence shells of (a)Sn,(b)K,(c)Br,and(d)Bi? Problem 124RQ: What is the value of n for the valence shells of (a) Al, (b) Sc, (c) Ba, and (d) Sb? Problem 125RQ: Give the configuration of the valence shell for (a) Na, (b) Al, (c) Ge, and (d) P. Problem 126RQ: Give the configuration of the valence shell for (a) Mg, (b) Br, (c) Ga, and (d) Pb. Problem 127RQ: Draw the orbital diagram for the valence shell of (a) Na, (b) Al, (c) Ge, and (d) P. Problem 128RQ: Draw the orbital diagram for the valence shell of (a) Mg, (b) Br, (c) Ga, and (d) Pb. Problem 129RQ Problem 130RQ Problem 131RQ: 7.131 Choose the larger atom in each pair: (a) Mg or S; (b) As or Bi.
Problem 132RQ: Choose the larger atom in each pair: (a) Al or Ar; (b) Tl or In. Problem 133RQ Problem 134RQ: Place the following in order of increasing size: N3-,Mg2+,Na+,Ne,F-,O2-. Problem 135RQ: Choose the larger particle in each pair: (a)NaorNa+;(b)Co3+orCo2+;(c)ClorCl-. Problem 136RQ: Choose the larger particle in each pair: (a)SorS2(b)Al3+orAl;(c)Au+orAu3+. Problem 137RQ: Choose the atom with the larger ionization energy in each pair: (a) B or N; (b) Se or S; (c) Cl or... Problem 138RQ: Choose the atom with the larger ionization energy in each pair: (a) Li or Rb; (b) Al or F; (c) F or... Problem 139RQ: Choose the atom with the more exothermic electron affinity in each pair: (a) I or Br; (b) Ga or As. Problem 140RQ: Choose the atom with the more exothermic electron affinity in each pair: (a) S or As; (b) Si or N. Problem 141RQ: 7.141 Use the periodic table to select the element in the following list for which there is the... Problem 142RQ: Use the periodic table to select the element in the following list for which there is the largest... Problem 143RQ: The human ear is sensitive to sound ranging from 20.0to2.00104Hz. The speed of sound is 330 m/s in... Problem 144RQ: *7.144 Microwaves are used to heat food in microwave ovens. The microwave radiation is absorbed by... Problem 145RQ: In the spectrum of hydrogen, there is a line with a wavelength of 410.3 nm. Use the Rydberg equation... Problem 146RQ: *7.146 Calculate the wavelength in nanometers of the shortest wavelength of light emitted by a... Problem 147RQ: Which of the following electronic transitions could lead to the emission of light from an atom?... Problem 148RQ: Calculate the wavelength of an electron moving at (a) the speed of light, (b) one-tenth the speed of... Problem 149RQ: 7.149 What, if anything, is wrong with the following electron configurations for atoms in their... Problem 150RQ: 7.150 Suppose students gave the following orbital diagrams for the 2s and 2p subshell in the ground... Problem 151RQ: 7.151 How many electrons are in p orbitals in an atom of gallium?
Problem 152RQ: What are the quantum numbers of the electrons that are lost by an atom of cobalt when it forms the... Problem 153RQ: 7.153 The removal of an electron from the hydrogen atom corresponds to raising the electron to the... Problem 154RQ: Use orbital diagrams to illustrate what happens when an oxygen atom gains two electrons. On the... Problem 155RQ: *7.155 From the data available in this chapter, determine the ionization energy of (a) , (b) , and... Problem 156RQ: 7.156 For an oxygen atom, which requires more energy, the addition of two electrons or the removal... Problem 157RQ: Write out the orbital diagram of N in the ground state. Without adding any more orbitals, write out... Problem 158RQ: The ions He+andLi2+ have line spectra that can be calculated using a modified Bohr equation. The... Problem 159RQ: A neon sign is a gas discharge tube in which electrons traveling from the cathode to the anode... Problem 160RQ: How many grams of water could have its temperature raised by 5.0C by a mole of photons that have a... Problem 161RQ: 7.161 It has been found that when the chemical bond between chlorine atoms in is formed, 328 kJ is... Problem 162RQ: *7.162 Using the ionization energy for sodium, would a photon with a wavelength of 23.7 nm be able... Problem 163RQ: *7.163 Using photons with a wavelength of 23.7 nm, determine the kinetic energies of all of the... Problem 164RQ: 7.164 Our understanding of the quantum mechanical atom has been developing since the early 1900s.... Problem 165RQ: When a copper atom loses an electron to become a Cu+ ion, what are the possible quantum numbers of... Problem 166RQ: 7.166 Paired electrons cancel each others magnetic fields. Why can’t unpaired electrons have... Problem 167RQ format_list_bulleted