Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Textbook Question
Chapter 7, Problem 82E
In defining the sizes of orbitals, why must we use an arbitrary value, such as 90% of the probability of finding an electron in that region?
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Chapter 7 Solutions
Chemistry
Ch. 7 - Four types of electromagnetic radiation (EMR) are...Ch. 7 - Characterize the Bohr model of the atom. In the...Ch. 7 - What experimental evidence supports the quantum...Ch. 7 - List the most important ideas of the quantum...Ch. 7 - What are quantum numbers? What information do we...Ch. 7 - How do 2p orbitals differ from each other? How do...Ch. 7 - Four blocks of elements in a periodic table refer...Ch. 7 - What is the difference between core electrons and...Ch. 7 - Prob. 9RQCh. 7 - The radius trend and the ionization energy trend...
Ch. 7 - Prob. 1ALQCh. 7 - Defend and criticize Bohrs model. Why was it...Ch. 7 - The first four ionization energies for the...Ch. 7 - Compare the first ionization energy of helium to...Ch. 7 - Which has the larger second ionization energy,...Ch. 7 - Explain why a graph of ionization energy versus...Ch. 7 - Without referring to your text, predict the trend...Ch. 7 - Account for the fact that the line that separates...Ch. 7 - Make sense of the fact that metals tend to lose...Ch. 7 - Explain electron from a quantum mechanical...Ch. 7 - Which is larger, the H 1s orbital or the Li 1s...Ch. 7 - There are an infinite number of allowed electronic...Ch. 7 - Prob. 13ALQCh. 7 - Choose the best response for the following. The...Ch. 7 - Consider the following statement "The ionization...Ch. 7 - Prob. 16ALQCh. 7 - How does probability fit into the description of...Ch. 7 - What is meant by an orbital?Ch. 7 - Explain the difference between the probability...Ch. 7 - Is the following statement true or false? The...Ch. 7 - Which is higher in energy, the 2s or 2p orbital,...Ch. 7 - Prove mathematically that it is more energetically...Ch. 7 - What type of relationship (direct or inverse) e...Ch. 7 - What do we mean by the frequency of...Ch. 7 - Explain the photoelectric effectCh. 7 - Describe briefly why the study of electromagnetic...Ch. 7 - How does the wavelength of a fast-pitched baseball...Ch. 7 - The following is an energy-level diagram for...Ch. 7 - The Bohr model works for only one electron...Ch. 7 - We can represent both probability and radial...Ch. 7 - Consider the representations of the p and d atomic...Ch. 7 - The periodic table consists of four blocks of...Ch. 7 - Many times the claim is made that subshells...Ch. 7 - Prob. 36QCh. 7 - Elements with very large ionization energies also...Ch. 7 - The changes in electron affinity as one goes down...Ch. 7 - Why is it much harder to explain the line spectra...Ch. 7 - Scientists use emission spectra to confirm the...Ch. 7 - Does the minimization of electron-electron...Ch. 7 - In the hydtogen atom, what is the physical...Ch. 7 - On which quantum numbers does the energy of an...Ch. 7 - Although Mendeleev predicted the existence of...Ch. 7 - Photosynthesis uses 660-nm light to convert CO2...Ch. 7 - An FM radio station broadcasts at 99.5 MHz....Ch. 7 - Microwave radiation has a wavelength on the order...Ch. 7 - A photon of ultraviolet (UV) light possesses...Ch. 7 - Octyl methoxycinoamate and oxybenzone are common...Ch. 7 - Human color vision is " produced" by the nervous...Ch. 7 - Consider the following waves representing...Ch. 7 - One type of electromagnetic radiation has a...Ch. 7 - Carbon absorbs energy at a wavelength of 150. nm....Ch. 7 - X rays have wavelengths on the order of 1 1010 m....Ch. 7 - The work function of an element is the energy...Ch. 7 - It takes 208.4 kJ of energy to remove 1 mole of...Ch. 7 - It takes 7.21 1019 J of energy to remove an...Ch. 7 - Ionization energy is the energy required to remove...Ch. 7 - Calculate the de Broglie wavelength for each of...Ch. 7 - Neutron diffraction is used in determining the...Ch. 7 - A particle has a velocity that is 90.% of the...Ch. 7 - Calculate the wavelength of light emiued when each...Ch. 7 - Calculate the wavelength of light emitted when...Ch. 7 - Using vertical lines, indicate the transitions...Ch. 7 - Using vertical lines, indicate the transitions...Ch. 7 - Consider only the transitions involving the first...Ch. 7 - Assume that a hydrogen atoms electron has been...Ch. 7 - Does a photon of visible light ( 400 to 700 nm)...Ch. 7 - An electron is excited from the n = 1 ground state...Ch. 7 - Calculate the maximum wavelength of light capable...Ch. 7 - Consider an electron for a hydrogen atom in an...Ch. 7 - An excited hydrogen atom with an electron in the n...Ch. 7 - An excited hydrogen atom emits light with a...Ch. 7 - Using the Heisenberg uncertainty principle,...Ch. 7 - The Heisenberg uncertainty principle can be...Ch. 7 - What are the possible values for the quantum...Ch. 7 - Identify each of the following orbitals and...Ch. 7 - Which of the following sets of quantum numbers are...Ch. 7 - Which of the following sets of quantum numbers are...Ch. 7 - What is the physical significance of the value of...Ch. 7 - In defining the sizes of orbitals, why must we use...Ch. 7 - Total radial probability distributions for the...Ch. 7 - Tbe relative orbital levels for the hydrogen atom...Ch. 7 - How many orbitals in an atom can have the...Ch. 7 - How many electrons in an atom can have the...Ch. 7 - Give the maximum number of electrons in an atom...Ch. 7 - Give the maximum number of electrons in an atom...Ch. 7 - Draw atomic orbital diagrams representing the...Ch. 7 - For elements l36, there are two exceptions to the...Ch. 7 - The elements Si, Ga, As, Ge, Al, Cd, S, and Se are...Ch. 7 - Write the expected electron configurations for...Ch. 7 - How many electrons would be predicted in the...Ch. 7 - For each of the following elements, which set of...Ch. 7 - Write the expected ground-state electron...Ch. 7 - Using only the periodic table inside the front...Ch. 7 - Given the valence electron orbital level diagram...Ch. 7 - Identify the following elements. a. An excited...Ch. 7 - In the ground state of mercury, Hg, a. how many...Ch. 7 - In the ground state of element 115, Uup, a. how...Ch. 7 - Give a possible set of values of the four quantum...Ch. 7 - Give a possible set of values of the four quantum...Ch. 7 - Valence electrons are those electrons in the...Ch. 7 - How many valence electrons do each of the...Ch. 7 - A certain oxygen atom has the electron...Ch. 7 - Which of the following electron configurations...Ch. 7 - Which of elements 1-36 have two unpaired electrons...Ch. 7 - The first-row transition metals from chromium...Ch. 7 - One bit of evidence that the quantum mechanical...Ch. 7 - Identify how many unpaired electrons are present...Ch. 7 - Prob. 111ECh. 7 - Arrange the following groups of atoms in order of...Ch. 7 - Prob. 113ECh. 7 - Arrange the atoms in Exercise 108 in order of...Ch. 7 - In each of the following sets, which atom or ion...Ch. 7 - In each of the following sets, which atom or ion...Ch. 7 - Element 106 has been named seaborgium, Sg, in...Ch. 7 - The first ionization energies of As and Se are...Ch. 7 - Rank the elements Be, B, C, N, and O in order of...Ch. 7 - Consider the following ionization energies for...Ch. 7 - The following graph plots the first, second, and...Ch. 7 - For each of the following pairs of elements (C and...Ch. 7 - For each of the following pairs of elements (Mg...Ch. 7 - The electron affinities of the elements from...Ch. 7 - In the second row of the periodic table, Be, N,...Ch. 7 - Prob. 127ECh. 7 - Order the atoms in each of the following sets from...Ch. 7 - The electron affinity for sulfur is more negative...Ch. 7 - Which has the more negative electron affinity, the...Ch. 7 - Write equations corresponding to the following: a....Ch. 7 - Using data from the text, determine the following...Ch. 7 - Prob. 133ECh. 7 - Prob. 135ECh. 7 - Cesium was discovered in natural mineral waters in...Ch. 7 - 'The bright yellow light emitted by a sodium vapor...Ch. 7 - Does the information on alkali metals in Table 2-8...Ch. 7 - Predict the atomic number of the next alkali metal...Ch. 7 - "Lithium" is often prescribed as a...Ch. 7 - Prob. 142ECh. 7 - Complete and balance the equations for the...Ch. 7 - Complete and balance the equations for the...Ch. 7 - An unknown element is a nonmetal and has a valence...Ch. 7 - A carbon-oxygen double bond in a certain organic...Ch. 7 - Photogray lenses incorporate small amounts of...Ch. 7 - Mars is roughly 60 million km from the earth. How...Ch. 7 - Consider the following approximate visible light...Ch. 7 - One of the visible lines in the hydrogen emission...Ch. 7 - Using Fig. 2-30, list the elements (ignore the...Ch. 7 - Are the following statements true for the hydrogen...Ch. 7 - Although no currently known elements contain...Ch. 7 - Which of the following orbital designations are...Ch. 7 - The four most abundant elements by mass in the...Ch. 7 - Consider the eight most abundant elements in the...Ch. 7 - An ion having a 4+ charge and a mass of 49.9 u has...Ch. 7 - The successive ionization energies for an unknown...Ch. 7 - In the ground state of cadmium, Cd, a. how many...Ch. 7 - Consider the following idealized PES spectrum for...Ch. 7 - It takes 476 kJ to remove 1 mole of electrons from...Ch. 7 - Calculate, to four significant figures, the...Ch. 7 - Assume that a hydrogen atoms electron bas been...Ch. 7 - Determine the maximum number of electrons that can...Ch. 7 - Consider the ground state of arsenic, As. How many...Ch. 7 - Which of the following statements is(are) true? a....Ch. 7 - Identify the following three elements. a. The...Ch. 7 - For each of the following pairs of elements,...Ch. 7 - Which of the following statements is(are) true? a....Ch. 7 - Three elements have the electron configurations...Ch. 7 - The figure below represents part of the emission...Ch. 7 - One of the emission spectral lines for Be3+ has a...Ch. 7 - The figure below represents part of the emission...Ch. 7 - When lhe excited electron in a hydrogen atom falls...Ch. 7 - Prob. 177CPCh. 7 - For hydrogen atoms, the wave function for the...Ch. 7 - The wave function for the 2pz, orbital in the...Ch. 7 - Answer the following questions, assuming that ms,...Ch. 7 - Assume that we are in another universe with...Ch. 7 - Without looking at data in the text, sketch a...Ch. 7 - The following numbers are the ratios of second...Ch. 7 - We expect the atomic radius to increase going down...Ch. 7 - The ionization energy for a 1s electron in a...Ch. 7 - An atom of a particular element is traveling at...Ch. 7 - As the weapons officer aboard the Srarship...Ch. 7 - Answer the following questions based on the given...
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- 6.32 What are the mathematical origins of quantum numbers?arrow_forwardSketch a picture of the 90% boundary surface of an s orbital and the px orbital. Be sure the latter drawing shows why the p orbital is labeled px and not py, for example.arrow_forward• list the number of orbitals of each type (1s, 3p, etc) in an atom.arrow_forward
- • rank various orbitals in terms of size and energy.arrow_forwardUse the mathematical expression for the 2pz wave function of a one-electron atom (see Table 5.2) to show that the probability of finding an electron in that orbital anywhere in the x-y plane is 0. What are the nodal planes for a dxz orbital and for a dx2y2 orbital?arrow_forwardIn 1885, Johann Balmer, a mathematician, derived the following relation for the wavelength of lines in the visible spectrum of hydrogen =364.5 n2( n2 4) where in nanometers and n is an integer that can be 3, 4, 5, . . . Show that this relation follows from the Bohr equation and the equation using the Rydberg constant. Note that in the Balmer series, the electron is returning to the n=2 level.arrow_forward
- Defend and criticize Bohrs model. Why was it reasonable that such a model was proposed, and what evidence was there that it "works"? Why do we no longer "believe" in it?arrow_forwardInvestigating Energy Levels Consider the hypothetical atom X that has one electron like the H atom but has different energy levels. The energies of an electron in an X atom are described by the equation E=RHn3 where RH is the same as for hydrogen (2.179 1018 J). Answer the following questions, without calculating energy values. a How would the ground-state energy levels of X and H compare? b Would the energy of an electron in the n = 2 level of H be higher or lower than that of an electron in the n = 2 level of X? Explain your answer. c How do the spacings of the energy levels of X and H compare? d Which would involve the emission of a higher frequency of light, the transition of an electron in an H atom from the n = 5 to the n = 3 level or a similar transition in an X atom? e Which atom, X or H, would require more energy to completely remove its electron? f A photon corresponding to a particular frequency of blue light produces a transition from the n = 2 to the n = 5 level of a hydrogen atom. Could this photon produce the same transition (n = 12 to n = 5) in an atom of X? Explain.arrow_forwardSuppose that the spin quantum number could have the values 12,0 and 12 . Assuming that the rules governing the values of the other quantum numbers and the order of filling sublevels were unchanged, (a) what would be the electron capacity of an s sublevel? a p sublevel? a d sublevel? (b) how many electrons could fit in the n=3 level? (c) what would be the electron configuration of the element with atomic number 8? 17?arrow_forward
- Heated lithium atoms emit photons of light with an energy of 2.9611019 J. Calculate the frequency and wavelength of one of these photons. What is the total energy in 1 mole of these photons? What is the color of the emitted light?arrow_forwardExplain the difference between (a) the Bohr model of the atom and the quantum mechanical model. (b) wavelength and frequency. (c) the geometries of the three different p orbitals.arrow_forwardAlthough we may draw the 4s orbital with the shape of a ball, there is some probability of finding the electron outside the ball we draw. Is this statement true or false? Comment on this statement.arrow_forward
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