CHEMISTRY:MOLECULAR NATURE (LL)W/ACCESS
7th Edition
ISBN: 9781119497325
Author: JESPERSEN
Publisher: WILEY
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Chapter 7, Problem 165RQ
When a copper atom loses an electron to become a
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Chapter 7 Solutions
CHEMISTRY:MOLECULAR NATURE (LL)W/ACCESS
Ch. 7 - Practice Exercise 7.1
Helium derives its name from...Ch. 7 - Practice Exercise 7.2
Radio station KRED in...Ch. 7 - Calculate the wavelength in micrometers, m, of...Ch. 7 - Practice Exercise 7.4
Calculate the wavelength in...Ch. 7 - What is the energy of the radiation emitted when...Ch. 7 - Practice Exercise 7.6
If the energy of light...Ch. 7 - Calculate the energy of an electron in its lowest...Ch. 7 - Practice Exercise 7.8
If an electron moves from a...Ch. 7 - Practice Exercise 7.9
What are the values of n and...Ch. 7 - What subshells would be found in the shells with...
Ch. 7 - Without looking at the tables in the text, how...Ch. 7 - Prob. 12PECh. 7 - Practice Exercise 7.13
Draw orbital diagrams for...Ch. 7 - Practice Exercise 7.14
Use Figure 7.18 to predict...Ch. 7 - Can an dement with an even atomic number be...Ch. 7 - Practice Exercise 7.16
Use orbital diagrams to...Ch. 7 - Practice Exercise 7.17
Use the periodic table to...Ch. 7 - Use the periodic table to predict the electron...Ch. 7 - Practice Exercise 7.19
Write shorthand...Ch. 7 - Write shorthand configurations and abbreviated...Ch. 7 - Practice Exercise 7.21
Give an example of a...Ch. 7 - Prob. 22PECh. 7 - Prob. 23PECh. 7 - Practice Exercise 7.24
Use the periodic table to...Ch. 7 - Use the periodic table to select the atom with the...Ch. 7 - Prob. 26PECh. 7 - In general terms, why do we call light...Ch. 7 - In general, what does the term frequency imply?...Ch. 7 - What is meant by the term wavelength of light?...Ch. 7 - 7.4 Sketch a picture of a wave and label its...Ch. 7 - Which property of light waves is a measure of the...Ch. 7 - Arrange the following regions of the...Ch. 7 - 7.7 What wavelength range is covered by the...Ch. 7 - Arrange the following colors of visible light in...Ch. 7 - What is the equation that relates the wavelength...Ch. 7 - How is the frequency of a particular type of...Ch. 7 - 7.11 What is a photon?
Ch. 7 - Show that the energy of a photon is given by the...Ch. 7 - Examine each of the following pairs and state...Ch. 7 - What is a quantum of energy?Ch. 7 - Prob. 15RQCh. 7 - Prob. 16RQCh. 7 - Describe Niels Bohrs model of the structure of the...Ch. 7 - Prob. 18RQCh. 7 - Why does the equation for the energy of an...Ch. 7 - In what way was Bohrs theory a success? How...Ch. 7 - 7.21 How does the behavior of very small particles...Ch. 7 - Describe the phenomenon called diffraction. How...Ch. 7 - What experiment could you perform to determine...Ch. 7 - 7.24 What is wave/particle duality?
Ch. 7 - Prob. 25RQCh. 7 - What is the collapsing atom paradox?Ch. 7 - How does quantum mechanics resolve the collapsing...Ch. 7 - What are the names used to refer to the theories...Ch. 7 - What is the term used to describe a particular...Ch. 7 - What are the three properties of orbitals in which...Ch. 7 - What are the allowed values of the principal...Ch. 7 - What information does each type of quantum number...Ch. 7 - How does the value of n in the Rydberg equation...Ch. 7 - Why is (a) the d subshell in the Period 4...Ch. 7 - Why does every shell contain an s subshell?Ch. 7 - How many orbitals are found in (a) an s subshell,...Ch. 7 - 7.37 If the value of for an electron in an atom...Ch. 7 - 7.38 What physical property of electrons leads us...Ch. 7 - Explain the two magnetic properties that are...Ch. 7 - What is the Pauli exclusion principle? What effect...Ch. 7 - What are the possible values of the spin quantum...Ch. 7 - Suppose an electron in an atom has the following...Ch. 7 - Prob. 43RQCh. 7 - Prob. 44RQCh. 7 - Within any given shell, how do the energies of the...Ch. 7 - Prob. 46RQCh. 7 - Give the electron configurations of the elements...Ch. 7 - 7.48 Using your own words, describe how to use the...Ch. 7 - Give the correct electron configurations of (a) Cr...Ch. 7 - What is the correct electron configuration of...Ch. 7 - How are the electron configurations of the...Ch. 7 - Define the terms valence shell and valence...Ch. 7 - Why do we use probabilities when we discuss the...Ch. 7 - Sketch the approximate shape of (a) a 1s orbital...Ch. 7 - How does the size of a given type of orbital vary...Ch. 7 - How are the p orbitals of a given p subshell...Ch. 7 - What is a nodalplane? How are the number of nodal...Ch. 7 - What is a radial node? How are the number of...Ch. 7 - 7.59 How many nodal planes does a p orbital have?...Ch. 7 - On appropriate coordinate axes, sketch the shape...Ch. 7 - What is the meaning of effective nuclear charge?...Ch. 7 - *7.62 Explain why a 3s electron in Al experiences...Ch. 7 - Explain why the atomic size varies across the...Ch. 7 - Explain why cations are smaller than their...Ch. 7 - Prob. 65RQCh. 7 - Going from left to right in the periodic table,...Ch. 7 - Prob. 67RQCh. 7 - Prob. 68RQCh. 7 - Explain why ionization energy increases from left...Ch. 7 - Prob. 70RQCh. 7 - Prob. 71RQCh. 7 - Prob. 72RQCh. 7 - Why does phosphorus have a larger first ionization...Ch. 7 - Prob. 74RQCh. 7 - 7.75 For sulfur, write an equation for the change...Ch. 7 - 7.76 Why does Cl have a more exothermic electron...Ch. 7 - Prob. 77RQCh. 7 - How is electron affinity related, to effective...Ch. 7 - 7.79 What is the frequency in hertz of blue light...Ch. 7 - Ultraviolet light with a wavelength of more than...Ch. 7 - Ozone protects the earths inhabitants from the...Ch. 7 - The meter is defined as the length of the path...Ch. 7 - In New York City, radio station WCBS broadcasts...Ch. 7 - Sodium vapor lamps are often used in residential...Ch. 7 - 7.85 Calculate the energy in joules of a photon of...Ch. 7 - Calculate the energy in joules of a photon of...Ch. 7 - In the spectrum of hydrogen, there is a line with...Ch. 7 - 7.88 In the spectrum of sodium, there is a line...Ch. 7 - Use the Rydberg equation to calculate the...Ch. 7 - 7.90 Use the Rydberg equation to calculate the...Ch. 7 - Calculate the wavelength and energy in joules of...Ch. 7 - Calculate the energy in joules and the wavelength...Ch. 7 - What is the letter code for a subshell with...Ch. 7 - 7.94 What is the letter code for a subshell with...Ch. 7 - What is the value of l for (a) an f orbital and...Ch. 7 - 7.96 What is the value of for (a) a p orbital and...Ch. 7 - What are the values of n and l for the subshells:...Ch. 7 - Give the values of n and l for the subshells: (a)...Ch. 7 - For the shell with n = 6, what are the possible...Ch. 7 - 7.100 What values of are possible for a shell with...Ch. 7 - In a particular shell, the largest value of l is...Ch. 7 - What is the value of n for a shell if the largest...Ch. 7 - What are the possible values of ml for a subshell...Ch. 7 - If the value of l for an electron in an atom is 5,...Ch. 7 - If the value of ml for an electron in an atom is...Ch. 7 - How many orbitals are there in an h subshell...Ch. 7 - 7.107 Give the complete set of quantum numbers for...Ch. 7 - 7.108 Give the complete set of quantum numbers for...Ch. 7 - *7.109 In an antimony atom, how many electrons...Ch. 7 - Prob. 110RQCh. 7 - Give the electron configurations of...Ch. 7 - 7.112 Write the electron configurations of (a) As,...Ch. 7 - 7.113 Which of the following atoms in their ground...Ch. 7 - Which of the following atoms in their ground...Ch. 7 - Prob. 115RQCh. 7 - Prob. 116RQCh. 7 - Write the abbreviated electron configurations for...Ch. 7 - Write the abbreviated electron configurations for...Ch. 7 - Draw complete orbital diagrams for (a) Mg and (b)...Ch. 7 - Draw complete orbital diagrams for (a) As and (b)...Ch. 7 - 7.121 Draw orbital diagrams for the abbreviated...Ch. 7 - Draw orbital diagrams for the abbreviated...Ch. 7 - What is the value of n for the valence shells of...Ch. 7 - What is the value of n for the valence shells of...Ch. 7 - Give the configuration of the valence shell for...Ch. 7 - Give the configuration of the valence shell for...Ch. 7 - Draw the orbital diagram for the valence shell of...Ch. 7 - Draw the orbital diagram for the valence shell of...Ch. 7 - Prob. 129RQCh. 7 - Prob. 130RQCh. 7 - 7.131 Choose the larger atom in each pair: (a) Mg...Ch. 7 - Choose the larger atom in each pair: (a) Al or Ar;...Ch. 7 - Prob. 133RQCh. 7 - Place the following in order of increasing size:...Ch. 7 - Choose the larger particle in each pair:...Ch. 7 - Choose the larger particle in each pair:...Ch. 7 - Choose the atom with the larger ionization energy...Ch. 7 - Choose the atom with the larger ionization energy...Ch. 7 - Choose the atom with the more exothermic electron...Ch. 7 - Choose the atom with the more exothermic electron...Ch. 7 - 7.141 Use the periodic table to select the element...Ch. 7 - Use the periodic table to select the element in...Ch. 7 - The human ear is sensitive to sound ranging from...Ch. 7 - *7.144 Microwaves are used to heat food in...Ch. 7 - In the spectrum of hydrogen, there is a line with...Ch. 7 - *7.146 Calculate the wavelength in nanometers of...Ch. 7 - Which of the following electronic transitions...Ch. 7 - Calculate the wavelength of an electron moving at...Ch. 7 - 7.149 What, if anything, is wrong with the...Ch. 7 - 7.150 Suppose students gave the following orbital...Ch. 7 - 7.151 How many electrons are in p orbitals in an...Ch. 7 - What are the quantum numbers of the electrons that...Ch. 7 - 7.153 The removal of an electron from the hydrogen...Ch. 7 - Use orbital diagrams to illustrate what happens...Ch. 7 - *7.155 From the data available in this chapter,...Ch. 7 - 7.156 For an oxygen atom, which requires more...Ch. 7 - Write out the orbital diagram of N in the ground...Ch. 7 - The ions He+andLi2+ have line spectra that can be...Ch. 7 - A neon sign is a gas discharge tube in which...Ch. 7 - How many grams of water could have its temperature...Ch. 7 - 7.161 It has been found that when the chemical...Ch. 7 - *7.162 Using the ionization energy for sodium,...Ch. 7 - *7.163 Using photons with a wavelength of 23.7 nm,...Ch. 7 - 7.164 Our understanding of the quantum mechanical...Ch. 7 - When a copper atom loses an electron to become a...Ch. 7 - 7.166 Paired electrons cancel each others magnetic...Ch. 7 - Prob. 167RQ
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- Assign a correct set of four quantum numbers for (a) Each electron in a nitrogen atom. (b) The valence electron in a sodium atom. (c) A 3d electron in a nickel atom.arrow_forwardThe following shapes each represent an orbital of an atom in a hypothetical universe. The small circle is the location of the nucleus in each orbital. a If you placed an electron in each orbital, which one would be higher in energy? b When an electron makes a transition from the orbital represented on the right to the orbital on the left, would you expect energy to be absorbed or released? c Draw a sketch of an orbital of the same type that would be higher in energy than either of the two pictured orbitals.arrow_forwardHow many unpaired electrons are there in an atom of (a) phosphorus? (b) potassium? (c) plutonium (Pu)?arrow_forward
- Write one possible set of quantum numbers for the valence electrons of calcium.arrow_forwardHow many unpaired electrons are there in the following atoms? (a) aluminum (b) argon (c) arsenicarrow_forwardHow many electrons in an atom can have the following quantum designation? (a) 1s (b) 4d, m l =0(c) n=5,l=2arrow_forward
- Using the Bohr model, determine the energy in joules of the photon produced when an electron in a He+ ion moves from the orbit with n = 5 to the orbit with n = 2.arrow_forwardThe four most abundant elements by mass in the human body are oxygen, carbon, hydrogen, and nitrogen. These four elements make up about 96% of the human body. The next four most abundant elements are calcium, phosphorus, magnesium, and potassium. Excluding hydrogen, which of these elements would have the smallest size? largest size? smallest first ionization energy? largest first ionization energy?arrow_forwardElement 106 has been named seaborgium, Sg, in honor of Glenn Seaborg, discoverer of the first transuraniurn element. a. Write the expected electron configuration for element 106. b. What other element would be most like element 106 in its properties?arrow_forward
- On which quantum numbers does the energy of an electron depend in each of the following? a. a one-electron atom or ion b. an atom or ion with more than one electronarrow_forwardFor each of the following elements, specify the extent to which the subshell containing the distinguishing electron is filled (s2, p3, p5, d4, etc.). a. 13Al b. 23V c. 20Ca d. 36Krarrow_forwardAre the following statements true for the hydrogen atom only, true for all atoms, or not true for any atoms? a. The principal quantum number completely determines the energy of a given electron. b. The angular momentum quantum number, l, determines the shapes of the atomic orbitals. c. The magnetic quantum number, ml, determines the direction that the atomic orbitals point in space.arrow_forward
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