Chemistry & Chemical Reactivity
9th Edition
ISBN: 9781133949640
Author: John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher: Cengage Learning
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Chapter 6.2, Problem 1CYU
Calculate the energy per mole of photons for the laser used in Blu-ray players (λ = 405 nm)
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Chapter 6 Solutions
Chemistry & Chemical Reactivity
Ch. 6.1 - (a) Which color in the visible spectrum has the...Ch. 6.1 - 1. Which of the following types of electromagnetic...Ch. 6.1 - What is the wavelength of an FM radio signal that...Ch. 6.2 - Calculate the energy per mole of photons for the...Ch. 6.2 - Prob. 1RCCh. 6.2 - Prob. 2RCCh. 6.3 - Prob. 1CYUCh. 6.3 - The Lyman series of spectral lines for the H atom,...Ch. 6.3 - 1. Based on Bohr's theory, which of the following...Ch. 6.3 - Based on Bohr's theory, which of the following...
Ch. 6.4 - Calculate the wavelength associated with a neutron...Ch. 6.4 - 1. The wavelength associated with an electron...Ch. 6.5 - 1. What label is given to an orbital with quantum...Ch. 6.5 - 2. How many orbitals are in the n = 4...Ch. 6.5 - Prob. 3RCCh. 6.6 - 1. Which of the following is not a correct...Ch. 6.6 - Which of the following sets of quantum numbers...Ch. 6.6 - How many nodal planes exist for a 5d orbital? (a)...Ch. 6.7 - Which of the following is a valid set of quantum...Ch. 6 - Answer the following questions based on Figure...Ch. 6 - Consider the colors of the visible spectrum. (a)...Ch. 6 - Traffic signals are often now made of LEDs...Ch. 6 - Suppose you are standing 225 m from a radio...Ch. 6 - Green light has a wavelength of 5.0 102 nm. What...Ch. 6 - Violet light has wavelength of about 410 nm. What...Ch. 6 - The most prominent line in the emission spectrum...Ch. 6 - The most prominent line in the emission spectrum...Ch. 6 - Place the following types of radiation in order of...Ch. 6 - Place the following types of radiation in order of...Ch. 6 - An energy of 3.3 1019 J/atom is required to cause...Ch. 6 - You are an engineer designing a switch that works...Ch. 6 - The most prominent line in the spectrum of mercury...Ch. 6 - The most prominent line in the spectrum of neon is...Ch. 6 - A line in the Balmer series of emission lines of...Ch. 6 - What are the wavelength and frequency of the...Ch. 6 - Consider only transitions involving the n = 1...Ch. 6 - Consider only transitions involving the n = 1...Ch. 6 - The energy emitted when an electron moves from a...Ch. 6 - If energy is absorbed by a hydrogen atom in its...Ch. 6 - Calculate the wavelength and frequency of light...Ch. 6 - Calculate the wavelength and frequency of light...Ch. 6 - An electron moves with a velocity of 2.5 X 108...Ch. 6 - A beam of electrons (m = 9.11 X 1031 kg/electron)...Ch. 6 - Calculate the wavelength, in nanometers,...Ch. 6 - A rifle bullet (mass = 1.50 g) has a velocity of...Ch. 6 - (a) When n = 4, what are the possible values of ?...Ch. 6 - (a) When n = 4, = 2, and m = 1, to what orbital...Ch. 6 - A possible excited state of the H atom has the...Ch. 6 - A possible excited state for the H atom has an...Ch. 6 - How many subshells occur in the electron shell...Ch. 6 - Prob. 32PSCh. 6 - Explain briefly why each of the following is not a...Ch. 6 - Which of the following represent valid sets of...Ch. 6 - What is the maximum number of orbitals that can be...Ch. 6 - What is the maximum number of orbitals that can be...Ch. 6 - Explain briefly why each of the following is not a...Ch. 6 - Explain briefly why each of the following is not a...Ch. 6 - State which of the following orbitals cannot exist...Ch. 6 - State which of the following orbitals cannot exist...Ch. 6 - Write a complete set of quantum numbers (n, , m)...Ch. 6 - Write a complete set of quantum numbers (n, , and...Ch. 6 - A particular orbital has n = 4 and = 2. What must...Ch. 6 - A given orbital has a magnetic quantum number of m...Ch. 6 - Prob. 45PSCh. 6 - Prob. 46PSCh. 6 - Which of the following are applicable when...Ch. 6 - Prob. 48GQCh. 6 - Give the number of nodal surfaces through the...Ch. 6 - What is the maximum number of s orbitals found in...Ch. 6 - Match the values of l shown in the table with...Ch. 6 - Sketch a picture of the 90% boundary surface of an...Ch. 6 - Complete the following table.Ch. 6 - Excited H atoms have many emission lines. One...Ch. 6 - An advertising sign gives off red light and green...Ch. 6 - Radiation in the ultraviolet region of the...Ch. 6 - A cell phone sends signals at about 850 MHz (where...Ch. 6 - Assume your eyes receive a signal consisting of...Ch. 6 - If sufficient energy is absorbed by an atom, an...Ch. 6 - Suppose hydrogen atoms absorb energy so that...Ch. 6 - Rank the following orbitals in the H atom in order...Ch. 6 - How many orbitals correspond to each of the...Ch. 6 - Cobalt-60 is a radioactive isotope used in...Ch. 6 - Exposure to high doses of microwaves can cause...Ch. 6 - When the Sojourner spacecraft landed on Mars in...Ch. 6 - The most prominent line in the emission spectrum...Ch. 6 - Answer the following questions as a summary quiz...Ch. 6 - Answer the following questions as a summary quiz...Ch. 6 - For an electron in a hydrogen atom, calculate the...Ch. 6 - A solution of KMnO4 absorbs light at 540 nm (page...Ch. 6 - Prob. 71ILCh. 6 - The spectrum shown here is for aspirin. The...Ch. 6 - The infrared spectrum for methanol. CH3OH, is...Ch. 6 - Bohr pictured the electrons of the atom as being...Ch. 6 - Light is given off by a sodium- or...Ch. 6 - Prob. 76SCQCh. 6 - What does wave-particle duality mean? What are its...Ch. 6 - Prob. 79SCQCh. 6 - Suppose you live in a different universe where a...Ch. 6 - A photon with a wavelength of 93.8 nm strikes a...Ch. 6 - Explain why you could or could not measure the...Ch. 6 - Prob. 83SCQ
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- This laser emits green light with a wavelength of 533 nm. (a) What is the energy, in joules, of one photon of light at this wavelength? (b) If a particular laser produces 1.00 watt (W) of power (1 W = 1 J/s), how many photons are produced each second by the laser?arrow_forward6.17 The laser in most supermarket barcode scanners operates at a wavelength of 632.8 nm. What is the energy of a single photon emitted by such a laser? What is the energy of one mole of these photons?arrow_forwardCalculate the energy per mole of photons (in kJ/mol) for red light with a wavelength of 700 nm. Calculate the energy per mole of photons (in kJ/mol) for UV-B light with a wavelength of 300 nm. How many times more energetic is this UV-B than this red light?arrow_forward
- A photon of light produced by a surgical laser has an energy of 3.0271019 J. Calculate the frequency and wavelength of the photon. What is the total energy in 1 mole of photons? What is the color of the emitted light?arrow_forwardYou are an engineer designing a switch that works by the photoelectric effect. The metal you wish to use in your device requires 6.7 1019 J/atom to remove an electron. Will the switch work if the light falling on the metal has a wavelength of 540 nm or greater? Why or why not?arrow_forwardThe photoelectric work function of potassium is 2.29 eV. A photon of energy greater than this ejects the electron with the excess as kinetic energy. Suppose light of wavelength 455 nm ejects an electron from the surface of potassium. What is the speed of the ejected electron?arrow_forward
- The lasers used in supermarket scanners emit red light at a wavelength of 633 nm. Compact disc players use lasers that emit light (that is not visible) at 840 nm. Which photonsthose emitted by supermarket scanners or compact disc (CD) playerscontain more energy per photon? Supermarket scanners CD players They both contain the same amount of energy per photon.arrow_forwardAs the weapons officer aboard the Srarship Chemistry, it is your duty to configure a photon torpedo to remove an electron from the outer hull of an enemy vessel. You know that the work function (the binding energy of the electron) of the hull of the enemy ship is 7.52 1019 J. a. What wavelength does your photon torpedo need to be to eject an electron? b. You find an extra photon torpedo with a wavelength of 259 nm and fire it at the enemy vessel. Does this photon torpedo do any damage to the ship (does it eject an electron)? c. If the hull of the enemy vessel is made of the element with an electron configura tion of [Ar]4s13d10, what metal is this?arrow_forwardCalculate the wavelength of the Balmer line of the hydrogen spectrum in which the initial n quantum number is 5 and the final n quantum number is 2.arrow_forward
- A bright violet line occurs at 435.8 nm in the emission spectrum of mercury vapor. What amount of energy, in joules, must be released by an electron in a mercury atom to produce a photon of this light?arrow_forward6.96 When a helium atom absorbs light at 58.44 nm, an electron is promoted from the 1s orbital to a 2p orbital. Given that the ionization energy of (ground state) helium is 2372 kJ/ mol, find the longest wavelength of light that could eject an electron from the excited state helium atom.arrow_forwardThe eyes of certain reptiles pass a single visual signal to the brain when the visual receptors are struck by photons of a wavelength of 850 nm. If a total energy of 3.151014 J is required to trip the signal, what is the minimum number of photons that must strike the receptor?arrow_forward
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