Chemistry: The Molecular Nature of Matter
7th Edition
ISBN: 9781118516461
Author: Neil D. Jespersen, Alison Hyslop
Publisher: WILEY
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Chapter 7, Problem 68RQ
Interpretation Introduction
Interpretation:
The equations for the first and third ionization energy of oxygen are to be represented.
Concept Introduction:
Electrons are present around the nucleus and are placed at a certain distance from it. Nucleus contains protons which have attractive power over the electrons.
Electrons can be removed or added to an atom during any
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What are ionization energy for atoms :
(a) F
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(c) Ba
(a) Identify the number of electrons in the ground-state outer shell of atomic oxygen (atomic number 8).(b) How many electrons are in the ground-state outer shell of fluorine?
Question:Consider two elements, Element A and Element B, from the periodic table. Element A is located in Group 1 and Period 3, while Element B is located in Group 16 and Period 2.
(a) Which element would have a larger atomic radius, Element A or Element B? Justify your answer.
(b) Predict the ionization energy of Element A and Element B. Which element would have a higher ionization energy? Explain your reasoning.
(c) Based on their positions in the periodic table, which element would be more likely to form a stable cation? Provide a brief explanation for your choice.
Chapter 7 Solutions
Chemistry: The Molecular Nature of Matter
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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