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 1ALQ
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Concept explainers
What is the definition of spectrophotometry? electromagnetic waves (the whole spectra)
b. Spectrophotometry is the quantitative measurement of the reflection or transmission properties of a material as a function of wavelength
Interaction between an electric field and a magnetic field.
Expert Solution
Introduction
Spectrophotometry is an analytical technique used to measure the light absorption properties of a sample. It is commonly used in the fields of chemistry, biochemistry, and medicine to determine the concentration of a solution or to identify unknown compounds. The technique uses a light source, such as a lamp or laser, to measure the amount of light that is absorbed by the sample. The sample is placed in a spectrophotometer and the reading is measured on a scale known as absorbance.
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