Chemistry & Chemical Reactivity 9th Edition
ISBN: 9781133949640
Author: John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher: John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
1 Basic Concepts Of Chemistry 2 Atoms Molecules And Ions 3 Chemical Reactions 4 Stoichiometry: Quantitative Information About Chemical Reactions 5 Principles Of Chemical Reactivity: Energy And Chemical Reactions 6 The Structure Of Atoms 7 The Structure Of Atoms And Periodic Trends 8 Bonding And Molecular Structure 9 Bonding And Molecular Structure: Orbital Hybridization And Molecular Orbitals 10 Gases And Their Properties 11 Intermolecular Forces And Liquids 12 The Solid State 13 Solutions And Their Behavior 14 Chemical Kinetics: The Rates Of Chemical Reactions 15 Principles Of Chemical Reactivity: Equilibria 16 Principles Of Chemical Reactivity: The Chemistry Of Acids And Bases 17 Principles Of Chemical Reactivity: Other Aspects Of Aqueous Equilibria 18 Principles Of Chemical Reactivity: Entropy And Free Energy 19 Principles Of Chemical Reactivity: Electron Transfer Reactions 20 Environmental Chemistry-earth's Environment, Energy, And Sustainability 21 The Chemistry Of The Main Group Elements 22 The Chemistry Of The Transistion Elements 23 Carbon: Not Just Another Element 24 Biochemistry 25 Nuclear Chemistry L Let's Review Chapter6: The Structure Of Atoms
6.1 Electromagnetic Radiation 6.2 Quantization: Planck, Einstein, Energy, And Photons 6.3 Atomic Line Spectra And Niels Bohr 6.4 Particle-wave Duality: Prelude To Quantum Mechanics 6.5 The Modern View Of Electronic Structure: Wave Or Quantum Mechanics 6.6 The Shapes Of Atomic Orbitals 6.7 One More Electron Property: Electron Spin Chapter Questions Section: Chapter Questions
Problem 1PS: Answer the following questions based on Figure 6.2: (a) Which type of radiation involves less... Problem 2PS: Consider the colors of the visible spectrum. (a) Which colors of light involve less energy than... Problem 3PS: Traffic signals are often now made of LEDs (light-emitting diodes). Amber and green ones are... Problem 4PS: Suppose you are standing 225 m from a radio transmitter. What is your distance from the transmitter... Problem 5PS: Green light has a wavelength of 5.0 102 nm. What is the energy, in joules, of one photon of green... Problem 6PS: Violet light has wavelength of about 410 nm. What is its frequency? Calculate the energy of one... Problem 7PS: The most prominent line in the emission spectrum of aluminum is at 396.15nm. What is the frequency... Problem 8PS: The most prominent line in the emission spectrum of magnesium is 285.2 nm. Other lines are found at... Problem 9PS: Place the following types of radiation in order of increasing energy per photon: (a) yellow light... Problem 10PS: Place the following types of radiation in order of increasing energy per photon: (a) radiation... Problem 11PS: An energy of 3.3 1019 J/atom is required to cause a cesium atom on a metal surface to lose an... Problem 12PS: You are an engineer designing a switch that works by the photoelectric effect. The metal you wish to... Problem 13PS: The most prominent line in the spectrum of mercury is at 253.652 nm. Other lines are located at... Problem 14PS: The most prominent line in the spectrum of neon is found at 865.438 nm. Other lines are located at... Problem 15PS: A line in the Balmer series of emission lines of excited H atoms has a wavelength of 410.2 nm... Problem 16PS: What are the wavelength and frequency of the radiation involved in the least energetic emission line... Problem 17PS: Consider only transitions involving the n = 1 through n = 5 energy levels for the H atom (see... Problem 18PS: Consider only transitions involving the n = 1 through n = 4 energy levels for the hydrogen atom (see... Problem 19PS: The energy emitted when an electron moves from a higher energy state to a lower energy state in any... Problem 20PS: If energy is absorbed by a hydrogen atom in its ground state, the atom is excited to a higher energy... Problem 21PS: Calculate the wavelength and frequency of light emitted when an electron changes from n = 3 to n = 1... Problem 22PS: Calculate the wavelength and frequency of light emitted when an electron changes from n = 4 to n = 3... Problem 23PS: An electron moves with a velocity of 2.5 X 108 cm/s. What is its wavelength? Problem 24PS: A beam of electrons (m = 9.11 X 1031 kg/electron) has an average speed of 1.3 X 108 m/s. What is the... Problem 25PS: Calculate the wavelength, in nanometers, associated with a 46-g golf ball moving at 30. m/s (about... Problem 26PS: A rifle bullet (mass = 1.50 g) has a velocity of 7.00 x 102 mph (miles per hour). What is the... Problem 27PS: (a) When n = 4, what are the possible values of ? (b) When is 2, what are the possible values of m... Problem 28PS: (a) When n = 4, = 2, and m = 1, to what orbital type does this refer? (Give the orbital label, such... Problem 29PS: A possible excited state of the H atom has the electron in a 4p orbital. List all possible sets of... Problem 30PS: A possible excited state for the H atom has an electron in a 5d orbital. List all possible sets of... Problem 31PS: How many subshells occur in the electron shell with the principal quantum number n = 4? Problem 32PS Problem 33PS: Explain briefly why each of the following is not a possible set of quantum numbers for an electron... Problem 34PS: Which of the following represent valid sets of quantum numbers? For a set is invalid, explain... Problem 35PS: What is the maximum number of orbitals that can be identified by each of the following sets of... Problem 36PS: What is the maximum number of orbitals that can be identified by each of the following sets of... Problem 37PS: Explain briefly why each of the following is not a possible set of quantum numbers for an electron... Problem 38PS: Explain briefly why each of the following is not a possible set of quantum numbers for an electron... Problem 39PS: State which of the following orbitals cannot exist according to the quantum theory: 2s, 2d, 3p, 3f,... Problem 40PS: State which of the following orbitals cannot exist according to the quantum theory: 3p, 4s, 2f, and... Problem 41PS: Write a complete set of quantum numbers (n, , m) that quantum theory allows for each of the... Problem 42PS: Write a complete set of quantum numbers (n, , and m) for each of the following orbitals: (a) 5f, (b)... Problem 43PS: A particular orbital has n = 4 and = 2. What must this orbital be: (a) 3p, (b) 4p, (c) 3d, or (d)... Problem 44PS: A given orbital has a magnetic quantum number of m = 1. This could not be a(n) (a) f orbital (b) d... Problem 45PS Problem 46PS Problem 47GQ: Which of the following are applicable when explaining the photoelectric effect? Correct any... Problem 48GQ Problem 49GQ: Give the number of nodal surfaces through the nucleus (planar nodes) for each orbital type: s, p, d,... Problem 50GQ: What is the maximum number of s orbitals found in a given electron shell? The maximum number of p... Problem 51GQ: Match the values of l shown in the table with orbital type (s, p, d, or f). Problem 52GQ: Sketch a picture of the 90% boundary surface of an s orbital and the px orbital. Be sure the latter... Problem 53GQ: Complete the following table. Problem 54GQ: Excited H atoms have many emission lines. One series of lines, called the Pfund series, occurs in... Problem 55GQ: An advertising sign gives off red light and green light. (a) Which light has higher-energy photons?... Problem 56GQ: Radiation in the ultraviolet region of the electro-magnetic spectrum is quite energetic. It is this... Problem 57GQ: A cell phone sends signals at about 850 MHz (where 1 MHz = 1 106 Hz or cycles per second). (a) What... Problem 58GQ: Assume your eyes receive a signal consisting of blue light, = 470 nm. The energy of the signal is... Problem 59GQ: If sufficient energy is absorbed by an atom, an electron can be lost by the atom and a positive ion... Problem 60GQ: Suppose hydrogen atoms absorb energy so that electrons are excited to the n = 7 energy level.... Problem 61GQ: Rank the following orbitals in the H atom in order of increasing energy: 3s, 2s, 2p, 4s, 3p, 1s, and... Problem 62GQ: How many orbitals correspond to each of the following designations? (a) 3p (b) 4p (c) 4Px (d) 6d (e)... Problem 63GQ: Cobalt-60 is a radioactive isotope used in medicine for the treatment of certain cancers. It... Problem 64GQ: Exposure to high doses of microwaves can cause tissue damage. Estimate how many photons, with = 12... Problem 65GQ: When the Sojourner spacecraft landed on Mars in 1997, the planet was approximately 7.8 107 km from... Problem 66GQ: The most prominent line in the emission spectrum of chromium is found at 425.4 nm. Other lines in... Problem 67GQ: Answer the following questions as a summary quiz on the chapter. (a) The quantum number n describes... Problem 68GQ: Answer the following questions as a summary quiz on this chapter. (a) The quantum number n describes... Problem 69GQ: For an electron in a hydrogen atom, calculate the energy of the photon emitted when an electron... Problem 70IL: A solution of KMnO4 absorbs light at 540 nm (page 206). What is the frequency of the light absorbed?... Problem 71IL Problem 72IL: The spectrum shown here is for aspirin. The vertical axis is the amount of light absorbed, and the... Problem 73IL: The infrared spectrum for methanol. CH3OH, is illustrated below. It shows the amount of light in the... Problem 74SCQ: Bohr pictured the electrons of the atom as being located in definite orbits about the nucleus, just... Problem 75SCQ: Light is given off by a sodium- or mercury-containing streetlight when the atoms are excited. The... Problem 76SCQ Problem 77SCQ: What does wave-particle duality mean? What are its implications in our modem view of atomic... Problem 79SCQ Problem 80SCQ: Suppose you live in a different universe where a different set of quantum numbers is required to... Problem 81SCQ: A photon with a wavelength of 93.8 nm strikes a hydrogen atom, and light is emitted by the atom. How... Problem 82SCQ: Explain why you could or could not measure the wavelength of a golf ball in flight. Problem 83SCQ Problem 41PS: Write a complete set of quantum numbers (n, , m) that quantum theory allows for each of the...
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The angular momentum quantum number (l) determines the overall size of an orbital.
True or False
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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