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 96E: In the ground state of element 115, Uup, a. how many electrons have n = 5 as one of their quantum...
Related questions
Which statement is false?
Group of answer choices
1 The spin quantum number can have values of +½ or −½.
2 The 4s orbitals have lower energy than the 3d orbitals (for transition metals ).
3 No two electrons can have the same four quantum numbers.
4 The electron density at a point is proportional to the square of the wave function φ2 at that point.
5 For a given value of the principal quantum number n , the angular momentum quantum number ℓ can have integer values ranging from 0 to n .
Definition Definition Product of the moment of inertia and angular velocity of the rotating body: (L) = Iω Angular momentum is a vector quantity, and it has both magnitude and direction. The magnitude of angular momentum is represented by the length of the vector, and the direction is the same as the direction of angular velocity.
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