1 Chemical Foundations 2 Atomic Structure And Periodicity 3 Bonding: General Concepts 4 Molecular Structure And Orbitals 5 Stoichiometry 6 Types Of Chemical Reactions And Solution Stoichiometry 7 Chemical Energy 8 Gases 9 Liquids And Solids 10 Properties Of Solutions 11 Chemical Kinetics 12 Chemical Equilibrium 13 Acids And Bases 14 Acid- Base Equilibria 15 Solubility And Complex Lon Equilibria 16 Spontaneity, Entropy, And Free Energy 17 Electrochemistry 18 The Nucleus: A Chemist's View 19 The Representative Elements 20 Transition Metals And Coordination Chemistry 21 Organic And Biological Molecules Chapter2: 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 Problem 8ALQ: Account for the fact that the line that separates the metals from the nonmetals on the periodic... Problem 9ALQ: Explain electron from a quantum mechanical perspective, including a discussion of atomic radii,... Problem 10ALQ: Choose the best response for the following. The ionization energy for the chlorine atom is equal in... Problem 11ALQ: Consider the following statement "The ionization energy for the potassium atom is negative, because... Problem 12ALQ Problem 13ALQ: How does probability fit into the description of the atom? Problem 14ALQ Problem 15ALQ Problem 16ALQ: Is the following statement true or false? The hydrogen atom has a 3s orbital. Explain. Problem 17ALQ: Which is higher in energy, the 2s or 2p orbital, in hydrogen? Is this also true for helium? Explain. Problem 18ALQ: Prove mathematically that it is more energetically favorable for a fluorine atom to take an electron... Problem 19Q: What type of relationship (direct or inverse) e xists between wavelength, frequency, and photon... Problem 20Q: What do we mean by the frequency of electromagnetic radiation? Is the frequency the same as the... Problem 21Q: Explain the photoelectric effect Problem 22Q: Describe briefly why the study of electromagnetic radiation bas been important to our understanding... Problem 23Q: How does the wavelength of a fast-pitched baseball compare to the wavelength of an electron... Problem 24Q: The following is an energy-level diagram for electronic transitions in the Bohr hydrogen atom. a.... Problem 25Q: The Bohr model works for only one electron species. Why do we discuss it in this text (what's good... Problem 26Q: We can represent both probability and radial probability versus distance from the nucleus for a... Problem 27Q Problem 28Q: The periodic table consists of four blocks of elements that correspond to s, p, d, and f orbitals... Problem 29Q Problem 30Q Problem 31Q: Elements with very large ionization energies also tend to have highly negative (favorable) electron... Problem 32Q Problem 33Q Problem 34Q: Scientists use emission spectra to confirm the presence of an element in materials of unknown... Problem 35Q: Does the minimization of electron-electron repulsions correlate with Hund's rule? Problem 36Q Problem 37Q Problem 38Q: Many more anhydrous lithium salts are hygroscopic (readily absorb water) than are those of the other... Problem 39E: The laser in an audio CD player uses light with a wavelength of 7.80 102 nm. Calculate the... Problem 40E: An FM radio station broadcasts at 99.5 MHz. Calculate the wavelength of the corresponding radio... Problem 41E: Microwave radiation has a wavelength on the order of 1.0 cm. Calculate the frequency and the energy... Problem 42E: A photon of ultraviolet (UV) light possesses enough energy to mutate a strand of human DNA. What is... Problem 43E: Octyl methoxycinoamate and oxybenzone are common ingredients in sunscreen applications. These... Problem 44E: Human color vision is " produced" by the nervous system based on how three different cone receptors... Problem 45E: Consider the following waves representing electromagnetic radiation: Which wave has the longer... Problem 46E: One type of electromagnetic radiation has a frequency of 107.1 MHz, another type has a wavelength of... Problem 47E: Carbon absorbs energy at a wavelength of 150. nm. The total amount of energy emitted by a carbon... Problem 48E: X rays have wavelengths on the order of 1 1010 m. Calculate the energy of 1.0 1010 m X rays in... Problem 49E: The work function of an element is the energy required to remove an electron from the surface of the... Problem 50E: It takes 208.4 kJ of energy to remove 1 mole of electrons from an atom on the surface of rubidium... Problem 51E: It takes 7.21 1019 J of energy to remove an electron from an iron atom. What is the maximum... Problem 52E: Ionization energy is the energy required to remove an electron from an atom in the gas phase. The... Problem 53E: Calculate the de Broglie wavelength for each of the following. a. an electron with a velocity 10.%... Problem 54E: Neutron diffraction is used in determining the structures of molecules. a. Calculate the de Broglie... Problem 55E: A particle has a velocity that is 90.% of the speed of light. If the wavelength of the particle is... Problem 56E: Calculate the velocities of electrons with de Broglie wavelengths of 1.0 102 nm and 1.0 nm. Problem 57E: Calculate the wavelength of light emiued when each of the following transitions occur in the... Problem 58E: Calculate the wavelength of light emitted when each of the following transitions occur in the... Problem 59E: Using vertical lines, indicate the transitions from Exercise 57 on an energy-level diagram for the... Problem 60E: Using vertical lines, indicate the transitions from Exercise 58 on an energy-level diagram for the... Problem 61E: Calculate the longest and shortest wavelengths of light emilled by electrons in the hydrogen atom... Problem 62E: Assume that a hydrogen atoms electron has been excited to the n = 5 level. How many different... Problem 63E: Does a photon of visible light ( 400 to 700 nm) have sufficient energy to excite an electron in a... Problem 64E: An electron is excited from the n = 1 ground state to the n = 3 state in a hydrogen atom. Which of... Problem 65E: Calculate the maximum wavelength of light capable of removing an electron for a hydrogen atom from... Problem 66E: Consider an electron for a hydrogen atom in an excited state. The maximum wavelength of... Problem 67E: An excited hydrogen atom with an electron in the n = 5 state emits light having a frequency of 6.90 ... Problem 68E: An excited hydrogen atom emits light with a wavelength of 397.2 nm to reach the energy level for... Problem 69E: Using the Heisenberg uncertainty principle, calculate x for each of the following. a. an electron... Problem 70E: The Heisenberg uncertainty principle can be expressed in the form Eth4 where E represents energy and... Problem 71E: What are the possible values for the quantum numbers n, l, and ml? Problem 72E: Identify each of the following orbitals and determine the n and l quantum numbers. Explain your... Problem 73E: Which of the following sets of quantum numbers are not allowed in the hydrogen atom? For the sets of... Problem 74E: Which of the following sets of quantum numbers are not allowed? For each incorrect set, state why it... Problem 75E: What is the physical significance of the value of 2 at a particular point in an atomic orbital? Problem 76E: In defining the sizes of orbitals, why must we use an arbitrary value, such as 90% of the... Problem 77E: Total radial probability distributions for the helium, neon, and argon atoms are shown in the... Problem 78E: Tbe relative orbital levels for the hydrogen atom can be represented as Draw the relative orbital... Problem 79E: How many orbitals in an atom can have the designation 5p, 3dz2, 4d, n = 5, n = 4? Problem 80E: How many electrons in an atom can have the designation lp, 6dx2y2, 4f, 7py, 2s, n = 3? Problem 81E: Give the maximum number of electrons in an atom that can have these quantum numbers: a. n = 4 b. n =... Problem 82E: Give the maximum number of electrons in an atom that can have these quantum numbers: a. n = 0, l =... Problem 83E: Draw atomic orbital diagrams representing the ground-state electron configumtion for each of the... Problem 84E: For elements l36, there are two exceptions to the filling order as predicted from the periodic... Problem 85E: The elements Si, Ga, As, Ge, Al, Cd, S, and Se are all used in the manufacture of various... Problem 86E: The elements Cu, O, La, Y, Ba, Tl, and Bi are all found in high-temperature ceramic superconductors.... Problem 87E: Write the expected electron configurations for each of the following atoms: Sc, Fe, P, Cs, Eu, Pt,... Problem 88E: Write the expected electron configurations for each of the following atoms: Cl, Sb, Sr, W, Pb, Cf. Problem 89E: The four most abundant elements by mass in the human body are oxygen, carbon, hydrogen, and... Problem 90E: The first-row transition metals from chromium through zinc all have some biologic function in the... Problem 91E: Write the expected ground-state electron configuration for the following. a. the element with one... Problem 92E: Using only the periodic table inside the front cover of the text, write the expected ground-state... Problem 93E: Given the valence electron orbital level diagram and the description, identify the element or ion.... Problem 94E: Identify the following elements. a. An excited state of this element has the electron configuration... Problem 95E: In the ground state of mercury, Hg, a. how many electrons occupy atomic orbitals with n = 3? b. how... Problem 96E: In the ground state of element 115, Uup, a. how many electrons have n = 5 as one of their quantum... Problem 97E: Give a possible set of values of the four quantum numbers for all the electrons in a boron atom and... Problem 98E: Give a possible set of values of the four quantum numbers for the 4s and 3d electrons in titanium. Problem 99E: Valence electrons are those electrons in the outermost principal quantum level (highest n level) of... Problem 100E: How many valence electrons do each of the following elements have, and what are the specific valence... Problem 101E: A certain oxygen atom has the electron configuration 1s22s22px22py2. How many unpaired electrons are... Problem 102E: Which of the following electron configurations correspond to an excited state? Identify the atoms... Problem 103E: Which of elements 1-36 have two unpaired electrons in the ground state? Problem 104E: Which of elements 1-36 have one unpaired electron in the ground state? Problem 105E: One bit of evidence that the quantum mechanical model is correct lies in the magnetic properties of... Problem 106E: Identify how many unpaired electrons are present in each of the followiog in the ground state: O,... Problem 107E Problem 108E: Arrange the following groups of atoms in order of increasing size. a. Rb, Na, Be b. Sr, Se, Ne c.... Problem 109E: Arrange the atoms in Exercise 107 in order of increasing first ionization energy. Problem 110E: Arrange the atoms in Exercise 108 in order of increasing first ionization energy. Problem 111E: In each of the following sets, which atom or ion bas the smallest radius? a. H, He b. Cl, In, Se c.... Problem 112E: In each of the following sets, which atom or ion has the smallest ionization energy? a. Ca, Sr, Ba... Problem 113E Problem 115E: The first ionization energies of As and Se are 0.947 and 0.941 MJ/mol, respectively. Rationalize... Problem 116E: Rank the elements Be, B, C, N, and O in order of increasing first ionization energy. Explain your... Problem 117E Problem 118E: The following graph plots the first, second, and third ionization energies for Mg, Al, and Si.... Problem 119E Problem 120E: For each of the following pairs of elements (Mg and K) (F and Cl) pick the atom with a. more... Problem 121E: The electron affinities of the elements from aluminum to chlorine are 44, 120, 74, 200.4, and ... Problem 122E: In the second row of the periodic table, Be, N, and Ne all have positive (unfavorable) electron... Problem 123E Problem 124E: Order the atoms in each of the following sets from the least negative electron affinity to the most.... Problem 125E: The electron affinity for sulfur is more negative than that for oxygen. How do you account for this? Problem 126E: Which has the more negative electron affinity, the oxygen, atom or the O ion? Explain your answer. Problem 127E: Write equations corresponding to the following: a. the fourth ionization energy of Se b. the... Problem 128E: Using data from the text, determine the following values (justify your answer): a. the electron... Problem 129E: Cesium was discovered in natural mineral waters in 1860 by R. W. Bunsen and G. R. Kirchhoff, using... Problem 130E: 'The bright yellow light emitted by a sodium vapor lamp consists of two emission Lines at 589.0 and... Problem 131E: Does the information on alkali metals in Table 2-8 of the text confirm the general periodic trends... Problem 132E Problem 133E Problem 134E: Complete and balance the equations for the following reactions. a. Cs(s) + H2O(l) b. Na(s) + Cl2(g) Problem 135AE Problem 136AE: A carbon-oxygen double bond in a certain organic molecule absorbs radiation that has a frequency of... Problem 137AE: Mars is roughly 60 million km from the earth. How long does it take for a radio signal originating... Problem 138AE: Consider the following approximate visible light spectrum: Barium emits light in the visible region... Problem 139AE: One of the visible lines in the hydrogen emission spectrum corresponds to the n = 6 to n = 2... Problem 140AE Problem 141AE: Are the following statements true for the hydrogen atom only, true for all atoms, or not true for... Problem 142AE Problem 143AE: The four most abundant elements by mass in the human body are oxygen, carbon, hydrogen, and... Problem 144AE: Which of the following orbital designations are incorrect: 1s, 1p, 7d, 9s, 3f, 4f, 2d? Problem 145AE: The successive ionization energies for an unknown element are I1 = 896 kJ/mol I2 = 1752 kJ/mol I3 =... Problem 146AE: An unknown element is a nonmetal and has a valence electron configuration of ns2np4 a. How many... Problem 147AE: While Mendeleev predicted the existence of several undiscovered elements. he did not predict the... Problem 148AE: Photosynthesis uses 660-nm light to convert CO2 and H2O into glucose and O2. Calculate the frequency... Problem 149AE: Photogray lenses incorporate small amounts of silver chloride in the glass of the lens. When light... Problem 150CWP: It takes 476 kJ to remove 1 mole of electrons from the atoms at the surface of a solid metal. How... Problem 151CWP Problem 152CWP Problem 153CWP: Determine the maximum number of electrons that can have each of the following designations: 2f,... Problem 154CWP: Consider the ground state of arsenic, As. How many electrons have l = 1 as one of their quantum... Problem 155CWP: Which of the following statements is(are) true? a. The 2s orbital in the hydrogen atom is larger... Problem 156CWP: Identify the following three elements. a. The ground-state electron configuration is [Kr]5s24d105p4.... Problem 157CWP Problem 158CWP Problem 159CWP: Three elements have the electron configurations 1s22s22P63s2, 1s22s22p63s23p4, and... Problem 160CP: One of the emission spectral lines for Be3+ has a wavelength of 253.4 nm for an electronic... Problem 161CP: The figure below represents part of the emission spectrum for a one-electron ion in lhe gas phase.... Problem 162CP: When lhe excited electron in a hydrogen atom falls from n = 5 to n = 2, a photon of blue light is... Problem 163CP Problem 164CP: For hydrogen atoms, the wave function for the state n = 3, l = 0, ml = 0 is... Problem 165CP: The wave function for the 2pz, orbital in the hydrogen atom is 2pl=142(za0)3/2e/2cos where a0 is the... Problem 166CP: Answer the following questions, assuming that ms, could have three values rather than two and that... Problem 167CP: Assume that we are in another universe with different physical laws. Electrons in this universe are... Problem 168CP: Without looking at data in the text, sketch a qualitative graph of the third ionization energy... Problem 169CP: The following numbers are the ratios of second ionization energy to first ionization energy: Na: 9.2... Problem 170CP: We expect the atomic radius to increase going down a group in the periodic table. Can you suggest... Problem 171CP: The ionization energy for a 1s electron in a silver atom is 2.462 106 kJ/mol. a. Determine an... Problem 172IP: Answer the following questions based on the given electron configurations and identify the elements.... Problem 173IP: As the weapons officer aboard the Srarship Chemistry, it is your duty to configure a photon torpedo... Problem 66E: Consider an electron for a hydrogen atom in an excited state. The maximum wavelength of...
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Consider an electron in a hydrogen atom at energy level n = x. The wavelength of electromagnetic radiation required to remove the electron completely from the hydrogen atom was 820.5 nm.
a) Determine the initial energy level (n = x).
b) Calculate the energy of electronic transition in kJ/mol
c) Wasthehydrogenatomingroundstateorexcitedstatebeforetheelectronremoved?
Interaction between an electric field and a magnetic field.
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