General Chemistry: Atoms First
2nd Edition
ISBN: 9780321809261
Author: John E. McMurry, Robert C. Fay
Publisher: Prentice Hall
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Chapter 2, Problem 2.116CHP
Interpretation Introduction
Interpretation:
The number of photons required to raise the temperature of a
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General Chemistry: Atoms First
Ch. 2.1 - What is the frequency of a gamma ray with = 3.56 ...Ch. 2.1 - What is the wavelength in meters of an FM radio...Ch. 2.1 - Two electromagnetic waves are represented below....Ch. 2.2 - The Balmer equation can be extended beyond the...Ch. 2.2 - What is the longest-wavelength line in nanometers...Ch. 2.2 - What is the shortest-wavelength line in nanometers...Ch. 2.3 - What is the energy in kilojoules per mole of...Ch. 2.3 - The biological effects of a given dose of radiant...Ch. 2.3 - The work function of zinc metal is 350 kJ/mol....Ch. 2.3 - What is the work function of nickel metal if light...
Ch. 2.4 - What is the de Broglie wavelength in meters of a...Ch. 2.6 - Extend Table 2.2 to show allowed combinations of...Ch. 2.6 - Give orbital notations for electrons in orbitals...Ch. 2.6 - Give the allowed combinations of three quantum...Ch. 2.7 - Prob. 2.15PCh. 2.7 - Give a possible combination of n and l quantum...Ch. 2.9 - Calculate in kilojoules per mole the energy...Ch. 2.12 - Look at the electron configurations in Figure...Ch. 2.13 - Give expected ground-state electron configurations...Ch. 2.13 - Take a guess. What do you think is a likely...Ch. 2.13 - Identify the atom with the following ground-state...Ch. 2.14 - Which atom in each of the following pairs would...Ch. 2.14 - Prob. 2.23PCh. 2 - Where on the blank outline of the periodic table...Ch. 2 - Where on the periodic table do elements that meet...Ch. 2 - One of the elements shown on the following...Ch. 2 - Two electromagnetic waves are represented below....Ch. 2 - Prob. 2.28CPCh. 2 - The following orbital-filling diagram represents...Ch. 2 - Prob. 2.30CPCh. 2 - Identify each of the following orbitals, and give...Ch. 2 - Which has the higher frequency, red light or...Ch. 2 - Prob. 2.33SPCh. 2 - The Hubble Space Telescope detects radiant energy...Ch. 2 - Prob. 2.35SPCh. 2 - What is the wavelength in meters of ultraviolet...Ch. 2 - Prob. 2.37SPCh. 2 - Calculate the energies of the following waves in...Ch. 2 - The MRI (magnetic resonance imaging) body scanners...Ch. 2 - A certain cellular telephone transmits at a...Ch. 2 - Prob. 2.41SPCh. 2 - What is the wavelength in meters of photons with...Ch. 2 - What is the energy of each of the following...Ch. 2 - The data encoded on CDs, DVDs, and Blu-ray discs...Ch. 2 - The semimetal germanium is used as a component in...Ch. 2 - Prob. 2.46SPCh. 2 - According to the values cited in Problem 2.46, the...Ch. 2 - The work function of silver metal is 436 kJ/mol....Ch. 2 - What is the work function of gold metal in kJ/mol...Ch. 2 - Protons and electrons can be given very high...Ch. 2 - If a proton (mass = 1.673 1024 g) is accelerated...Ch. 2 - What is the de Broglie wavelength in meters of a...Ch. 2 - What is the de Broglie wavelength in meters of a...Ch. 2 - At what speed in meters per second must a 145 g...Ch. 2 - What velocity would an electron (mass = 9.11 1031...Ch. 2 - Use the Heisenberg uncertainty principle to...Ch. 2 - The mass of a helium-4 atom is 4.0026 u, and its...Ch. 2 - What are the four quantum numbers, and what does...Ch. 2 - What is the Heisenberg uncertainty principle, and...Ch. 2 - Why do we have to use an arbitrary value such as...Ch. 2 - How many nodal surfaces does a 4s orbital have?...Ch. 2 - Prob. 2.62SPCh. 2 - How does electron shielding in multielectron atoms...Ch. 2 - Give the allowable combinations of quantum numbers...Ch. 2 - Give the orbital designations of electrons with...Ch. 2 - Tell which of the following combinations of...Ch. 2 - Which of the following combinations of quantum...Ch. 2 - What is the maximum number of electrons in an atom...Ch. 2 - What is the maximum number of electrons in an atom...Ch. 2 - The wavelength of light at which the Balmer series...Ch. 2 - One series of lines of the hydrogen spectrum is...Ch. 2 - Prob. 2.72SPCh. 2 - Excited rubidium atoms emit red light with = 795...Ch. 2 - Why does the number of elements in successive...Ch. 2 - Prob. 2.75SPCh. 2 - Prob. 2.76SPCh. 2 - Prob. 2.77SPCh. 2 - According to the aufbau principle, which orbital...Ch. 2 - Prob. 2.79SPCh. 2 - Prob. 2.80SPCh. 2 - Give the expected ground-state electron...Ch. 2 - Prob. 2.82SPCh. 2 - Draw orbital-filling diagrams for atoms with the...Ch. 2 - Prob. 2.84SPCh. 2 - Prob. 2.85SPCh. 2 - Prob. 2.86SPCh. 2 - Prob. 2.87SPCh. 2 - Prob. 2.88SPCh. 2 - Prob. 2.89SPCh. 2 - Prob. 2.90SPCh. 2 - Prob. 2.91SPCh. 2 - Prob. 2.92SPCh. 2 - Which atom in each of the following pairs has a...Ch. 2 - Prob. 2.94SPCh. 2 - Prob. 2.95SPCh. 2 - What is the expected ground-state electron...Ch. 2 - Prob. 2.97SPCh. 2 - Orbital energies in single-electron atoms or ions,...Ch. 2 - Prob. 2.99CHPCh. 2 - Prob. 2.100CHPCh. 2 - Prob. 2.101CHPCh. 2 - Prob. 2.102CHPCh. 2 - What is the wavelength in meters of photons with...Ch. 2 - Prob. 2.104CHPCh. 2 - The second in the SI system is defined as the...Ch. 2 - Prob. 2.106CHPCh. 2 - Prob. 2.107CHPCh. 2 - Cesium metal is often used in photoelectric...Ch. 2 - Prob. 2.109CHPCh. 2 - Prob. 2.110CHPCh. 2 - Prob. 2.111CHPCh. 2 - Youre probably familiar with using Scotch Tape for...Ch. 2 - Hard wintergreen-flavored candies are...Ch. 2 - Prob. 2.114CHPCh. 2 - Prob. 2.115CHPCh. 2 - Prob. 2.116CHPCh. 2 - Prob. 2.117CHPCh. 2 - Prob. 2.118CHPCh. 2 - X rays with a wavelength of 1.54 1010 m are...Ch. 2 - Prob. 2.120CHPCh. 2 - Assume that the rules for quantum numbers are...Ch. 2 - Given the subshells 1s, 2s, 2p, 3s, 3p, and 3d,...Ch. 2 - Prob. 2.123CHPCh. 2 - A minimum energy of 7.21 1019 J is required to...Ch. 2 - A photon produced by an X-ray machine has an...Ch. 2 - An energetically excited hydrogen atom has its...Ch. 2 - Prob. 2.127MP
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- Warm objects emit electromagnetic radiation in the infrared region. Heat lamps employ this principle to generate infrared radiation. Water absorbs infrared radiation with wavelengths near 2.80 m. Suppose this radiation is absorbed by the water and converted to heat. A 1.00-L sample of water absorbs infrared radiation, and its temperature increases from 20.0C to 30.0C. How many photons of this radiation are used to heat the water?arrow_forwardA particular microwave oven delivers 750 watts. (A watt is a unit of power, which is the joules of energy delivered, or used, per second.) If the oven uses microwave radiation of wavelength 12.6 cm, how many photons of this radiation are required to heat 1.00 g of water 1.00C, assuming that all of the photons are absorbed?arrow_forwardThis 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_forward
- An FM radio station found at 103.1 on the FM dial broadcasts at a frequency of 1.031188s1 (103.1 MHz). What is the wavelength of these radio waves in meters?arrow_forwardA hydrogen atom in the ground stale absorbs a photon whose wavelength is 95.0 nm. The resulting excited atom then emits a photon of 1282 nm. What are the regions of the electromagnetic spectrum for the radiations involved in these transitions? What is the principal quantum number of the final state resulting from the emission from the excited atom?arrow_forward(a) Which color in the visible spectrum has the highest frequency? Which has the lowest frequency? (b) Is the wavelength of the radiation used in a microwave oven (2.45 GHz) longer or shorter than that from your favorite FM radio station (for example, 91.7 MHz)? (c) Are the wavelengths of x-rays longer or shorter than those of ultraviolet light? (d) Calculate the frequency of green light with a wavelength of 510. nm.arrow_forward
- Investigating Energy Levels Consider the hypothetical atom X that has one electron like the H atom but has different energy levels. The energies of an electron in an X atom are described by the equation E=RHn3 where RH is the same as for hydrogen (2.179 1018 J). Answer the following questions, without calculating energy values. a How would the ground-state energy levels of X and H compare? b Would the energy of an electron in the n = 2 level of H be higher or lower than that of an electron in the n = 2 level of X? Explain your answer. c How do the spacings of the energy levels of X and H compare? d Which would involve the emission of a higher frequency of light, the transition of an electron in an H atom from the n = 5 to the n = 3 level or a similar transition in an X atom? e Which atom, X or H, would require more energy to completely remove its electron? f A photon corresponding to a particular frequency of blue light produces a transition from the n = 2 to the n = 5 level of a hydrogen atom. Could this photon produce the same transition (n = 12 to n = 5) in an atom of X? Explain.arrow_forwardA baseball weighs 142 g. A professional pitcher throws a fast ball at a speed of 100 mph and a curve ball at 80 mph. What wavelengths are associated with the motions of the baseball? If the uncertainty in the position of the ball is 12 wavelength, which ball (fast ball or curve) has a more precisely known position? Can the uncertainty in the position of a curve ball be used to explain why batters frequently miss it?arrow_forwardWhat wavelength of electromagnetic radiation corresponds to a frequency of 7.76 109 s1 ? Note that Plancks constant is 6.63 1034 J s, and the speed of light is 3.00 108 m/s.arrow_forward
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