Chemistry 10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
1 Chemical Foundations 2 Atoms, Molecules, And Ions 3 Stoichiometry 4 Types Of Chemical Reactions And Solution Stoichiometry 5 Gases 6 Thermochemistry 7 Atomic Structure And Periodicity 8 Bonding: General Concepts 9 Covalent Bonding: Orbitals 10 Liquids And Solids 11 Properties Of Solutions 12 Chemical Kinetics 13 Chemical Equilibrium 14 Acids And Bases 15 Acid-base Equilibria 16 Solubility And Complex Ion Equilibria 17 Spontaneity, Entropy, And Free Energy 18 Electrochemistry 19 The Nucleus: A Chemist's View 20 The Representative Elements 21 Transition Metals And Coordination Chemistry 22 Organic And Biological Molecules Chapter7: Atomic Structure And Periodicity
Chapter Questions Section: Chapter Questions
Problem 1RQ: Four types of electromagnetic radiation (EMR) are ultraviolet, microwaves, gamma rays, and visible.... Problem 2RQ: Characterize the Bohr model of the atom. In the Bohr model, what do we mean when we say something is... Problem 3RQ: What experimental evidence supports the quantum theory of light? Explain the wave-particle duality... Problem 4RQ: List the most important ideas of the quantum mechanical model of the atom. Include in your... Problem 5RQ: What are quantum numbers? What information do we get from the quantum numbers n, l, and ml? We... Problem 6RQ: How do 2p orbitals differ from each other? How do 2p and 3p orbitals differ from each other? What is... Problem 7RQ: Four blocks of elements in a periodic table refer to various atomic orbitals being filled. What are... Problem 8RQ: What is the difference between core electrons and valence electrons? Why do we emphasize the valence... Problem 9RQ Problem 10RQ: The radius trend and the ionization energy trend are exact opposites. Does this make sense? Problem 1ALQ Problem 2ALQ: Defend and criticize Bohrs model. Why was it reasonable that such a model was proposed, and what... Problem 3ALQ: The first four ionization energies for the elements X and Y are shown below. The units are not... Problem 4ALQ: Compare the first ionization energy of helium to its second ionization energy, remembering that both... Problem 5ALQ: Which has the larger second ionization energy, lithium or beryllium? Why? Problem 6ALQ: Explain why a graph of ionization energy versus atomic number (across a row) is not linear. Where... Problem 7ALQ: Without referring to your text, predict the trend of second ionization energies for the elements... Problem 8ALQ: Account for the fact that the line that separates the metals from the nonmetals on the periodic... Problem 9ALQ: Make sense of the fact that metals tend to lose electrons and nonmetals tend to gain electrons. Problem 10ALQ: Explain electron from a quantum mechanical perspective, including a discussion of atomic radii,... Problem 11ALQ: Which is larger, the H 1s orbital or the Li 1s orbital? Why? Which has the larger radius, the H atom... Problem 12ALQ: There are an infinite number of allowed electronic transitions in the hydrogen atom. Why dont we see... Problem 13ALQ Problem 14ALQ: Choose the best response for the following. The ionization energy for the chlorine atom is equal in... Problem 15ALQ: Consider the following statement "The ionization energy for the potassium atom is negative, because... Problem 16ALQ Problem 17ALQ: How does probability fit into the description of the atom? Problem 18ALQ: What is meant by an orbital? Problem 19ALQ: Explain the difference between the probability density distribution for an orbital and its radial... Problem 20ALQ: Is the following statement true or false? The hydrogen atom has a 3s orbital. Explain. Problem 21ALQ: Which is higher in energy, the 2s or 2p orbital, in hydrogen? Is this also true for helium? Explain. Problem 22ALQ: Prove mathematically that it is more energetically favorable for a fluorine atom to take an electron... Problem 23Q: What type of relationship (direct or inverse) e xists between wavelength, frequency, and photon... Problem 24Q: What do we mean by the frequency of electromagnetic radiation? Is the frequency the same as the... Problem 25Q: Explain the photoelectric effect Problem 26Q: Describe briefly why the study of electromagnetic radiation bas been important to our understanding... Problem 27Q: How does the wavelength of a fast-pitched baseball compare to the wavelength of an electron... Problem 28Q: The following is an energy-level diagram for electronic transitions in the Bohr hydrogen atom. a.... Problem 29Q: The Bohr model works for only one electron species. Why do we discuss it in this text (what's good... Problem 30Q: We can represent both probability and radial probability versus distance from the nucleus for a... Problem 31Q: Consider the representations of the p and d atomic orbitals in Figs. 2-15 and 2- 17. What do the +... Problem 32Q: The periodic table consists of four blocks of elements that correspond to s, p, d, and f orbitals... Problem 35Q: Many times the claim is made that subshells half-filled with electrons are particularly stable. Can... Problem 36Q Problem 37Q: Elements with very large ionization energies also tend to have highly negative (favorable) electron... Problem 38Q: The changes in electron affinity as one goes down a group in the periodic table are not nearly as... Problem 39Q: Why is it much harder to explain the line spectra of polyelectronic atoms and ions than it is to... Problem 40Q: Scientists use emission spectra to confirm the presence of an element in materials of unknown... Problem 41Q: Does the minimization of electron-electron repulsions correlate with Hund's rule? Problem 42Q: In the hydtogen atom, what is the physical significance of the for which n = and E = 0? Problem 43Q: On which quantum numbers does the energy of an electron depend in each of the following? a. a... Problem 44Q: Although Mendeleev predicted the existence of several undiscovered elements, he did not predict the... Problem 45E: Photosynthesis uses 660-nm light to convert CO2 and H2O into glucose and O2. Calculate the frequency... Problem 46E: An FM radio station broadcasts at 99.5 MHz. Calculate the wavelength of the corresponding radio... Problem 47E: Microwave radiation has a wavelength on the order of 1.0 cm. Calculate the frequency and the energy... Problem 48E: A photon of ultraviolet (UV) light possesses enough energy to mutate a strand of human DNA. What is... Problem 49E: Octyl methoxycinoamate and oxybenzone are common ingredients in sunscreen applications. These... Problem 50E: Human color vision is " produced" by the nervous system based on how three different cone receptors... Problem 51E: Consider the following waves representing electromagnetic radiation: Which wave has the longer... Problem 52E: One type of electromagnetic radiation has a frequency of 107.1 MHz, another type has a wavelength of... Problem 53E: Carbon absorbs energy at a wavelength of 150. nm. The total amount of energy emitted by a carbon... Problem 54E: X rays have wavelengths on the order of 1 1010 m. Calculate the energy of 1.0 1010 m X rays in... Problem 55E: The work function of an element is the energy required to remove an electron from the surface of the... Problem 56E: It takes 208.4 kJ of energy to remove 1 mole of electrons from an atom on the surface of rubidium... Problem 57E: It takes 7.21 1019 J of energy to remove an electron from an iron atom. What is the maximum... Problem 58E: Ionization energy is the energy required to remove an electron from an atom in the gas phase. The... Problem 59E: Calculate the de Broglie wavelength for each of the following. a. an electron with a velocity 10.%... Problem 60E: Neutron diffraction is used in determining the structures of molecules. a. Calculate the de Broglie... Problem 61E: A particle has a velocity that is 90.% of the speed of light. If the wavelength of the particle is... Problem 63E: Calculate the wavelength of light emiued when each of the following transitions occur in the... Problem 64E: Calculate the wavelength of light emitted when each of the following transitions occur in the... Problem 65E: Using vertical lines, indicate the transitions from Exercise 57 on an energy-level diagram for the... Problem 66E: Using vertical lines, indicate the transitions from Exercise 58 on an energy-level diagram for the... Problem 67E: Consider only the transitions involving the first four energy levels for a hydrogen atom: a. How... Problem 68E: Assume that a hydrogen atoms electron has been excited to the n = 5 level. How many different... Problem 69E: Does a photon of visible light ( 400 to 700 nm) have sufficient energy to excite an electron in a... Problem 70E: An electron is excited from the n = 1 ground state to the n = 3 state in a hydrogen atom. Which of... Problem 71E: Calculate the maximum wavelength of light capable of removing an electron for a hydrogen atom from... Problem 72E: Consider an electron for a hydrogen atom in an excited state. The maximum wavelength of... Problem 73E: An excited hydrogen atom with an electron in the n = 5 state emits light having a frequency of 6.90 ... Problem 74E: An excited hydrogen atom emits light with a wavelength of 397.2 nm to reach the energy level for... Problem 75E: Using the Heisenberg uncertainty principle, calculate x for each of the following. a. an electron... Problem 76E: The Heisenberg uncertainty principle can be expressed in the form Eth4 where E represents energy and... Problem 77E: What are the possible values for the quantum numbers n, l, and ml? Problem 78E: Identify each of the following orbitals and determine the n and l quantum numbers. Explain your... Problem 79E: Which of the following sets of quantum numbers are not allowed in the hydrogen atom? For the sets of... Problem 80E: Which of the following sets of quantum numbers are not allowed? For each incorrect set, state why it... Problem 81E: What is the physical significance of the value of 2 at a particular point in an atomic orbital? Problem 82E: In defining the sizes of orbitals, why must we use an arbitrary value, such as 90% of the... Problem 83E: Total radial probability distributions for the helium, neon, and argon atoms are shown in the... Problem 84E: Tbe relative orbital levels for the hydrogen atom can be represented as Draw the relative orbital... Problem 85E: How many orbitals in an atom can have the designation 5p, 3dz2, 4d, n = 5, n = 4? Problem 86E: How many electrons in an atom can have the designation lp, 6dx2y2, 4f, 7py, 2s, n = 3? Problem 87E: Give the maximum number of electrons in an atom that can have these quantum numbers: a. n = 4 b. n =... Problem 88E: Give the maximum number of electrons in an atom that can have these quantum numbers: a. n = 0, l =... Problem 89E: Draw atomic orbital diagrams representing the ground-state electron configumtion for each of the... Problem 90E: For elements l36, there are two exceptions to the filling order as predicted from the periodic... Problem 91E: The elements Si, Ga, As, Ge, Al, Cd, S, and Se are all used in the manufacture of various... Problem 92E: Write the expected electron configurations for each of the following atoms: Cl, Sb, Sr, W, Pb, Cf. Problem 93E: How many electrons would be predicted in the ground state for the following elements? a. zirconium... Problem 94E: For each of the following elements, which set of orbitals is last to till in the ground state? a.... Problem 95E: Write the expected ground-state electron configuration for the following. a. the element with one... Problem 96E: Using only the periodic table inside the front cover of the text, write the expected ground-state... Problem 97E: Given the valence electron orbital level diagram and the description, identify the element or ion.... Problem 98E: Identify the following elements. a. An excited state of this element has the electron configuration... Problem 99E: In the ground state of mercury, Hg, a. how many electrons occupy atomic orbitals with n = 3? b. how... Problem 100E: In the ground state of element 115, Uup, a. how many electrons have n = 5 as one of their quantum... Problem 101E: Give a possible set of values of the four quantum numbers for all the electrons in a boron atom and... Problem 102E: Give a possible set of values of the four quantum numbers for the 4s and 3d electrons in titanium. Problem 103E: Valence electrons are those electrons in the outermost principal quantum level (highest n level) of... Problem 104E: How many valence electrons do each of the following elements have, and what are the specific valence... Problem 105E: A certain oxygen atom has the electron configuration 1s22s22px22py2. How many unpaired electrons are... Problem 106E: Which of the following electron configurations correspond to an excited state? Identify the atoms... Problem 107E: Which of elements 1-36 have two unpaired electrons in the ground state? Problem 108E: The first-row transition metals from chromium through zinc all have some biologic function in the... Problem 109E: One bit of evidence that the quantum mechanical model is correct lies in the magnetic properties of... Problem 110E: Identify how many unpaired electrons are present in each of the followiog in the ground state: O,... Problem 111E Problem 112E: Arrange the following groups of atoms in order of increasing size. a. Rb, Na, Be b. Sr, Se, Ne c.... Problem 113E Problem 114E: Arrange the atoms in Exercise 108 in order of increasing first ionization energy. Problem 115E: In each of the following sets, which atom or ion bas the smallest radius? a. H, He b. Cl, In, Se c.... Problem 116E: In each of the following sets, which atom or ion has the smallest ionization energy? a. Ca, Sr, Ba... Problem 117E: Element 106 has been named seaborgium, Sg, in honor of Glenn Seaborg, discoverer of the first... Problem 119E: The first ionization energies of As and Se are 0.947 and 0.941 MJ/mol, respectively. Rationalize... Problem 120E: Rank the elements Be, B, C, N, and O in order of increasing first ionization energy. Explain your... Problem 121E: Consider the following ionization energies for aluminum:... Problem 122E: The following graph plots the first, second, and third ionization energies for Mg, Al, and Si.... Problem 123E: For each of the following pairs of elements (C and N) (Ar and Br) pick the atom with a. more... Problem 124E: For each of the following pairs of elements (Mg and K) (F and Cl) pick the atom with a. more... Problem 125E: The electron affinities of the elements from aluminum to chlorine are 44, 120, 74, 200.4, and ... Problem 126E: In the second row of the periodic table, Be, N, and Ne all have positive (unfavorable) electron... Problem 127E Problem 128E: Order the atoms in each of the following sets from the least negative electron affinity to the most.... Problem 129E: The electron affinity for sulfur is more negative than that for oxygen. How do you account for this? Problem 130E: Which has the more negative electron affinity, the oxygen, atom or the O ion? Explain your answer. Problem 131E: Write equations corresponding to the following: a. the fourth ionization energy of Se b. the... Problem 132E: Using data from the text, determine the following values (justify your answer): a. the electron... Problem 133E Problem 135E Problem 137E: Cesium was discovered in natural mineral waters in 1860 by R. W. Bunsen and G. R. Kirchhoff, using... Problem 138E: 'The bright yellow light emitted by a sodium vapor lamp consists of two emission Lines at 589.0 and... Problem 139E: Does the information on alkali metals in Table 2-8 of the text confirm the general periodic trends... Problem 140E: Predict the atomic number of the next alkali metal after francium and give its ground-state electron... Problem 141E: "Lithium" is often prescribed as a mood-stabilizing drug. Do you think the lithium prescribed is in... Problem 142E Problem 143E: Complete and balance the equations for the following reactions. a. Li(s) + N2(g) b. Rb(s) + S(s) Problem 144E: Complete and balance the equations for the following reactions. a. Cs(s) + H2O(l) b. Na(s) + Cl2(g) Problem 145AE: An unknown element is a nonmetal and has a valence electron configuration of ns2np4 a. How many... Problem 146AE: A carbon-oxygen double bond in a certain organic molecule absorbs radiation that has a frequency of... Problem 147AE: Photogray lenses incorporate small amounts of silver chloride in the glass of the lens. When light... Problem 149AE: Mars is roughly 60 million km from the earth. How long does it take for a radio signal originating... Problem 150AE: Consider the following approximate visible light spectrum: Barium emits light in the visible region... Problem 151AE: One of the visible lines in the hydrogen emission spectrum corresponds to the n = 6 to n = 2... Problem 152AE: Using Fig. 2-30, list the elements (ignore the lanthanides and actinides) that have ground-state... Problem 153AE: Are the following statements true for the hydrogen atom only, true for all atoms, or not true for... Problem 154AE: Although no currently known elements contain electrons in g orbitals in the ground state, it is... Problem 155AE: Which of the following orbital designations are incorrect: 1s, 1p, 7d, 9s, 3f, 4f, 2d? Problem 156AE: The four most abundant elements by mass in the human body are oxygen, carbon, hydrogen, and... Problem 157AE: Consider the eight most abundant elements in the human body, as outlined in Exercise 156. Excluding... Problem 158AE: An ion having a 4+ charge and a mass of 49.9 u has 2 electrons with principal quantum number n = 1.8... Problem 159AE: The successive ionization energies for an unknown element are I1 = 896 kJ/mol I2 = 1752 kJ/mol I3 =... Problem 160AE: In the ground state of cadmium, Cd, a. how many electrons have l = 2 as one of their quantum... Problem 162AE: Consider the following idealized PES spectrum for potassium: Explain the location and relative... Problem 163CWP: It takes 476 kJ to remove 1 mole of electrons from the atoms at the surface of a solid metal. How... Problem 164CWP: Calculate, to four significant figures, the longest and shortest wavelengths of light emitted by... Problem 165CWP: Assume that a hydrogen atoms electron bas been excited to the n = 6 level. How many different... Problem 166CWP: Determine the maximum number of electrons that can have each of the following designations: 2f,... Problem 167CWP: Consider the ground state of arsenic, As. How many electrons have l = 1 as one of their quantum... Problem 168CWP: Which of the following statements is(are) true? a. The 2s orbital in the hydrogen atom is larger... Problem 169CWP: Identify the following three elements. a. The ground-state electron configuration is [Kr]5s24d105p4.... Problem 170CWP: For each of the following pairs of elements, choose the one that correctly completes the following... Problem 171CWP: Which of the following statements is(are) true? a. F has a larger first ionization energy than does... Problem 172CWP: Three elements have the electron configurations 1s22s22P63s2, 1s22s22p63s23p4, and... Problem 173CP: The figure below represents part of the emission spectrum for a one-electron ion in the gas phase.... Problem 174CP: One of the emission spectral lines for Be3+ has a wavelength of 253.4 nm for an electronic... Problem 175CP: The figure below represents part of the emission spectrum for a one-electron ion in lhe gas phase.... Problem 176CP: When lhe excited electron in a hydrogen atom falls from n = 5 to n = 2, a photon of blue light is... Problem 177CP Problem 178CP: For hydrogen atoms, the wave function for the state n = 3, l = 0, ml = 0 is... Problem 179CP: The wave function for the 2pz, orbital in the hydrogen atom is 2pl=142(za0)3/2e/2cos where a0 is the... Problem 180CP: Answer the following questions, assuming that ms, could have three values rather than two and that... Problem 181CP: Assume that we are in another universe with different physical laws. Electrons in this universe are... Problem 182CP: Without looking at data in the text, sketch a qualitative graph of the third ionization energy... Problem 183CP: The following numbers are the ratios of second ionization energy to first ionization energy: Na: 9.2... Problem 184CP: We expect the atomic radius to increase going down a group in the periodic table. Can you suggest... Problem 185CP: The ionization energy for a 1s electron in a silver atom is 2.462 106 kJ/mol. a. Determine an... Problem 187CP: An atom of a particular element is traveling at 1.00% of the speed of light. The de Broglie... Problem 188IP: As the weapons officer aboard the Srarship Chemistry, it is your duty to configure a photon torpedo... Problem 190IP: Answer the following questions based on the given electron configurations and identify the elements.... Problem 152AE: Using Fig. 2-30, list the elements (ignore the lanthanides and actinides) that have ground-state...
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Concept explainers
What is Hund’s rule?Choice one from below.
1)The lowest energy is obtained if the number of electrons with different spins is maximized.
2)The lowest energy is obtained if the number of electrons with the same spin is maximized.
3)The highest energy is obtained if electrons are only placed in s orbitals.
4)The number of electrons in p orbitals must be half the atomic number Z .
Study of body parts and their functions. In this combined field of study, anatomy refers to studying the body structure of organisms, whereas physiology refers to their function.
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