1 Chemistry: An Introduction 2 Measurements And Calculations 3 Matter 4 Chemical Foundations: Elements, Atoms, And Ions 5 Nomenclature 6 Chemical Reactions: An Introduction 7 Reactions In Aqueous Solutions 8 Chemical Composition 9 Chemical Quantities 10 Energy 11 Modern Atomic Theory 12 Chemical Bonding 13 Gases 14 Liquids And Solids 15 Solutions 16 Acids And Bases 17 Equilibrium 18 Oxidation–reduction Reactions And Electrochemistry 19 Radioactivity And Nuclear Energy 20 Organic Chemistry 21 Biochemistry Chapter11: Modern Atomic Theory
11.1 Rutherford’s Atom 11.2 Electromagnetic Radiation 11.3 Emission Of Energy By Atoms 11.4 The Energy Levels Of Hydrogen 11.5 The Bohr Model Of The Atom 11.6 The Wave Mechanical Model Of The Atom 11.7 The Hydrogen Orbitals 11.8 The Wave Mechanical Model: Further Development 11.9 Electron Arrangements In The First 18 Atoms On The Periodic Table 11.10 Electron Configurations And The Periodic Table 11.11 Atomic Properties And The Periodic Table Chapter Questions Section: Chapter Questions
Problem 1ALQ: ow does probability ?t into the description of the atom? Problem 2ALQ Problem 3ALQ Problem 4ALQ: onsider the following statements: “The ionization energy for the potassium atom is negative because... Problem 5ALQ: n going across a row of the periodic table, protons and electrons are added and ionization energy... Problem 6ALQ Problem 7ALQ: rue or false? The hydrogen atom has a 3 orbital. Explain. Problem 8ALQ Problem 9ALQ: ake sense of the fact that metals tend to lose electrons and nonmetals tend to gain electrons. Use... Problem 10ALQ: Show how using the periodic table helps you find the expected electron configuration of any element. Problem 11ALQ: r Questions 11—13, you will need to consider ionizations beyond the first ionization energy. For... Problem 12ALQ Problem 13ALQ Problem 14ALQ Problem 15ALQ Problem 16ALQ: What evidence do we have that energy levels in an atom are quantized? State and explain the... Problem 17ALQ: Explain the hydrogen emission spectrum. Why is it significant that the calm emitted is not while?... Problem 18ALQ: There am an infinite number of allowed transitions in the hydrogen atom. Why don‘t we see more lines... Problem 19ALQ: You have learned that each orbital is allowed two electrons, and this pattern is evident on the... Problem 20ALQ: Atom A has valence electrons that are lower in energy than the valence electrons of Atom B. Which... Problem 21ALQ Problem 1QAP Problem 2QAP: hat questions were left unanswered by Rutherford’s experiments? Problem 3QAP Problem 4QAP Problem 5QAP Problem 6QAP Problem 7QAP: he “Chemistry in Focus" segment Light as a Sex Attractant discusses fluorescence. In fluorescence,... Problem 8QAP Problem 9QAP: hen lithium salts are heated in a flame, they emit red light. When copper salts are heated in a... Problem 10QAP: The energy of a photon of visible light emitted by an excited atom is the energy change that takes... Problem 11QAP Problem 12QAP: An excited atom can release some or all of its excess energy by emitting a(n) and thus move to a... Problem 13QAP: How is the energy carried per photon of light related to the wavelength of the light? Does... Problem 14QAP: When an atom energy from outside, the atom goes from a lower energy state to a higher energy state. Problem 15QAP: Describe briefly why the study of electromagnetic radiation has been important to our understanding... Problem 16QAP: What does it mean to say that the hydrogen atom has discrete energy levels? How is this fact... Problem 17QAP: Because a given element’s atoms emit only certain photons of light. only certain are occurring in... Problem 18QAP: How does the energy possessed by an emitted photon compare to the difference in energy levels that... Problem 19QAP Problem 20QAP: When a tube containing hydrogen atoms is energized by passing several thousand volts of electricity... Problem 21QAP: What are the essential points of Bohr‘s theory of the structure of the hydrogen atom? Problem 22QAP: According to Bohr, what happens to the electron when a hydrogen atom absorbs a photon of light of... Problem 23QAP: How does the Bohr theory account for the observed phenomenon of the emission of discrete wavelengths... Problem 24QAP: Why was Bohr's theory for the hydrogen atom initially accepted, and why was it ultimately discarded? Problem 25QAP: What major assumption (that was analogous to what had already been demonstrated for electromagnetic... Problem 26QAP: Discuss briefly the difference between an orbit (as described by Bohr for hydrogen) and an orbital... Problem 27QAP: Discuss briefly the difference between an orbit (as described by Bohr for hydrogen) and an orbital... Problem 28QAP: Section 11.6 uses a "firefly" analogy to illustrate how the wave mechanical modal for the atom... Problem 29QAP: Your text describes the probability map for an s orbital using an analogy to the earth’s atmosphere.... Problem 30QAP: Consider the following representation of a set of p orbitals for an atom: mg... Problem 31QAP: What are the differences between the :math>2s orbital and the 1s orbital of hydrogen? How are they... Problem 32QAP: What overall shape do the 2p and 3p orbitals have? How do the 2p orbitals differ from the 3p... Problem 33QAP Problem 34QAP: When the electron in hydrogen is in the n=3 principal energy level, the atom is in a/an state. Problem 35QAP: Although a hydrogen atom has only one electron, the hydrogen atom possesses a complete set of... Problem 36QAP: Complete the following table. trong>Value of n Possible Sublevels 1 2 3 4 Problem 37QAP: When describing the electrons in an orbital, we use arrows pointing upward and downward ( and ) to... Problem 38QAP: Why can only two electrons occupy a particular orbital? What is this idea called? Problem 39QAP: How does the energy of a principal energy level depend on the value of n? Does a higher value of n... Problem 40QAP: The number of sublevels in a principal energy level (increases/Decreases as n increases. Problem 41QAP: According to the Pauli exclusion principle, a given orbital can contain only electrons. Problem 42QAP Problem 43QAP: Which of the following orbital designations is(are) possible? msp;a.1sc.2db.2pd.4f Problem 44QAP: Which of the following orbital designations is (are} not possible? msp;a.3fc.4db.5sd.1p Problem 45QAP: Which orbital is the first be filled in any atom? Why? Problem 46QAP: When a hydrogen atom is in its ground state, in which orbital is its electron found? Why? Problem 47QAP Problem 48QAP: How are the electron arrangements in a given group (vertical column) of the periodic table related?... Problem 49QAP: Write the full electron configuration ( 1s22s2 etc.) for each of the following elements. >a.... Problem 50QAP: To which element does each of the following electron configurations correspond?... Problem 51QAP: Write the full electron configuration (1s32s2,etc.) for each of the following elements. phosphorus,... Problem 52QAP: To which element does each of the following electron configurations correspond?... Problem 53QAP: Write the complete orbital diagram for each of the following elements, using boxes to represent... Problem 54QAP Problem 55QAP Problem 56QAP: For each of the following, give an atom and its complete electron configuration that would be... Problem 57QAP: Why do we believe that the valence electrons of calcium and potassium reside in the 4s orbital... Problem 58QAP: Would you expect the Valence electrons of rubidium and strontium to reside in the 5s or the 4d... Problem 59QAP: Using the symbol of the previous noble gas in indicate the core electrons, write the electron... Problem 60QAP Problem 61QAP Problem 62QAP: How many valence electrons does each of the following atoms have? rubidium, Z=37 c. aluminum, Z=13... Problem 63QAP: How many 3d electrons are found in each of the following element? >a. nickel, Z=28 c. manganese,... Problem 64QAP: Based on the elements’ locations on the periodic table, how many 4d electrons would be predicted for... Problem 65QAP: For each of the following elements, indicate which set of orbitals is filled last. radium, Z=88 c.... Problem 66QAP: Write the valence-electron configuration of each of the following elements, basing your answer on... Problem 67QAP Problem 68QAP: The “Chemistry in Focus" segment The Chemistry of Bohrium discusses element 107. bohrium (Bh). What... Problem 69QAP: What are some of the physical properties that distinguish the metallic element from the nonmetals?... Problem 70QAP Problem 71QAP: Give some similarities than exist among the elements of Group 1. Problem 72QAP: Give some similarities that exist among the elements of Group 7. Problem 73QAP: Which of the following elements most easily gives up electrons during reactions Li, K, or Cs?... Problem 74QAP: Which elements in a given period (horizontal row) of the periodic table lose electrons most easily?... Problem 75QAP: Where are the most nonmetallic elements located on the periodic table? Why do these elements pull... Problem 76QAP: Why do the metallic elements of a given period (horizontal row) typically have much lower ionization... Problem 77QAP Problem 78QAP: The “Chemistry in Focus" segment Fireworks discusses some of the chemicals that give rise to the... Problem 79QAP Problem 80QAP: In each of the following sets of elements, which element would he expected to have the highest... Problem 81QAP: Arrange the following sets of elements in order of increasing atomic size.... Problem 82QAP: In each of the following sets of elements, indicate which element has the smallest atomic size.... Problem 83AP: Consider the bright line spectrum of hydrogen shown in Fig. 11.10 . Which line in the spectrum... Problem 84AP Problem 85AP: The portion of the electromagnetic spectrum between wavelengths of approximately 400 and 700... Problem 86AP: A beam of light can be thought of as consisting of a stream of light particles called . Problem 87AP Problem 88AP: The Energy levels of hydrogen (and other atoms) are , which means that only certain values of energy... Problem 89AP: According to Bohr, the electron in the hydrogen atom moved around the nucleus in circular paths... Problem 90AP: Which of the following statements is false concerning orbitals? An orbital is a region of space... Problem 91AP: Electrons found in the outemost principal energy level of an atom are referred to as electrons. Problem 92AP: An unknown element is a nonmetal and has a valence-electron configuration of ns2np4 . How many... Problem 93AP Problem 94AP: The current model of the atom in which essentially all of an Atom’s mass is contained in a very... Problem 95AP Problem 96AP Problem 97AP: Without referring to your textbook or a periodic table, write the full electron configuration, the... Problem 98AP Problem 99AP Problem 100AP Problem 101AP: ight waves move through space at a speed of ters per second. Problem 102AP Problem 103AP: ow does the attractive force that the nucleus exerts on an electron change with the principal energy... Problem 104AP Problem 105AP: ased on the ground-state electron configuration of iodine, how many electrons occupy the, p and d... Problem 106AP: lement X, which has a valence shell configuration of ns2np4 , was isolated in a laboratory. Which of... Problem 107AP: hy do we believe that the three electrons in the 2p sublevel of nitrogen occupy different orbitals? Problem 108AP Problem 109AP Problem 110AP Problem 111AP Problem 112AP: ank the following elements in order of increasing atomic size: Ge,S,F,Rb,Mn. Problem 113AP Problem 114AP Problem 115AP Problem 116AP Problem 117AP: n each of the following sets of elements, indicate which element shows the most active chemical... Problem 118AP Problem 119CP: Determine the maximum number of electrons that can have each of the following designations... Problem 120CP: hich of the following statements is(are) true? The 2s orbital in the hydrogen atom is larger than... Problem 121CP: ive the electron configurations for the following atoms. Do not use the noble gas notation. Write... Problem 122CP Problem 123CP Problem 124CP Problem 125CP Problem 126CP Problem 82QAP: In each of the following sets of elements, indicate which element has the smallest atomic size....
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Consider the atoms P. I, and Ba. Select the atom for each of the following statements.
has the greatest electron affinity .
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