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 expand_more
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 expand_more
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 format_list_bulleted
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