Chemistry for Engineering Students
3rd Edition
ISBN: 9781285199023
Author: Lawrence S. Brown, Tom Holme
Publisher: Cengage Learning
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Chapter 6, Problem 6.24PAE
6.21 The electron binding energy fur copper metal is
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Chapter 6 Solutions
Chemistry for Engineering Students
Ch. 6 - describe trace analysis and explain its role in...Ch. 6 - describe waves in terms of frequency, wavelength,...Ch. 6 - Prob. 3COCh. 6 - relate the frequency, wavelength, and amplitude of...Ch. 6 - describe the photoelectric effect by stating what...Ch. 6 - Prob. 6COCh. 6 - • use Planck’s equation to calculate the energy of...Ch. 6 - Prob. 8COCh. 6 - Prob. 9COCh. 6 - • describe similarities and differences between...
Ch. 6 - Prob. 11COCh. 6 - Prob. 12COCh. 6 - • identify an orbital (as 1s, 3p, etc.) from its...Ch. 6 - • list the number of orbitals of each type (1s,...Ch. 6 - • sketch the shapes of s and p orbitals and...Ch. 6 - • rank various orbitals in terms of size and...Ch. 6 - Prob. 17COCh. 6 - Prob. 18COCh. 6 - Prob. 19COCh. 6 - Prob. 20COCh. 6 - Prob. 6.1PAECh. 6 - 6.2 Unlike XRF, AAS cannot be used for...Ch. 6 - Prob. 6.3PAECh. 6 - Prob. 6.4PAECh. 6 - Prob. 6.5PAECh. 6 - Prob. 6.6PAECh. 6 - Explain why light is referred to as...Ch. 6 - Prob. 6.8PAECh. 6 - 6.7 Arrange the following regions of the...Ch. 6 - 6.8 Calculate the wavelength in meters, of...Ch. 6 - 6.9 If a string of decorative lights includes...Ch. 6 - 6.10 Define the term refraction.Ch. 6 - 6.11 Define the term photon.Ch. 6 - Prob. 6.14PAECh. 6 - 6.12 Find the energy of a photon with each of the...Ch. 6 - 6.13 Place these types of radiation in order of...Ch. 6 - 6.14 For photon with the following energies,...Ch. 6 - Prob. 6.18PAECh. 6 - 6.16 Various optical disk drives rely on laser...Ch. 6 - 6.17 The laser in most supermarket barcode...Ch. 6 - 6.18 Assume that a microwave oven operates at a...Ch. 6 - 6.19 Fill in the blanks below to complete a...Ch. 6 - 6.20 When light with a wavelength of 58.5 nm...Ch. 6 - 6.21 The electron binding energy fur copper metal...Ch. 6 - What is the difference between continuous and...Ch. 6 - Prob. 6.26PAECh. 6 - 6.23 Describe how the Bohr model of the atom...Ch. 6 - 6.24 According to the Bohr model of the atom, what...Ch. 6 - 6.25 Define the term ground state.Ch. 6 - 6.26 The figure below depicts the first four...Ch. 6 - 6.27 Refer w the data and energy-Ievel diagram...Ch. 6 - 6.28 A neon atom cmi light at many wavelengths,...Ch. 6 - 6.29 A mercury atom emits light at many...Ch. 6 - 6.30 How did the observation of electron...Ch. 6 - 6.31 Why do we use a wave function to describe...Ch. 6 - 6.32 What are the mathematical origins of quantum...Ch. 6 - Prob. 6.37PAECh. 6 - 6.34 Which of the following represent valid sets...Ch. 6 - 6.35 A particular orbital has n = 4 and l = 2....Ch. 6 - 6.36 Why are there no 2d orbitals?Ch. 6 - 6.34 What is the maximum number of electrons in an...Ch. 6 - 6.38 How many orbitals correspond to each of the...Ch. 6 - Prob. 6.43PAECh. 6 - Prob. 6.44PAECh. 6 - 6.40 Referring to Figure 6.15, draw a 4p orbitals,...Ch. 6 - Prob. 6.46PAECh. 6 - 6.43 Define the term spin paired.Ch. 6 - 6.44 On what does the Pauli exclusion principle...Ch. 6 - Prob. 6.49PAECh. 6 - Prob. 6.50PAECh. 6 - Prob. 6.51PAECh. 6 - 6.47 Depict two ways to place electrons in the 2p...Ch. 6 - 6.48 Write the ground state electron configuration...Ch. 6 - 6.49 Which of these electron configurations are...Ch. 6 - 6.50 From the list of atoms and ions given,...Ch. 6 - Prob. 6.56PAECh. 6 - Prob. 6.57PAECh. 6 - Prob. 6.58PAECh. 6 - Describe how valence electron configurations...Ch. 6 - Why is there no element to the immediate right of...Ch. 6 - Prob. 6.61PAECh. 6 - Prob. 6.62PAECh. 6 - 6.55 Explain why the s block of the periodic table...Ch. 6 - Prob. 6.64PAECh. 6 - Prob. 6.65PAECh. 6 - 6.60 Use the electron configurations of the alkali...Ch. 6 - 6.61 Using only a periodic table as a guide,...Ch. 6 - 6.62 Define the term ionization energy....Ch. 6 - 6.63 At which ionization for chlorine would you...Ch. 6 - 6.64 Arrange the following atoms in order of...Ch. 6 - Prob. 6.71PAECh. 6 - 6.66 Which element would you expect to have the...Ch. 6 - Prob. 6.73PAECh. 6 - 6.68 Indicate which species in each pair has the...Ch. 6 - 6.69 Compare the elements Na, B, Al, and C with...Ch. 6 - 6.70 Rank the following in order of decreasing...Ch. 6 - 6.71 Several excited states of the neon atom are...Ch. 6 - Prob. 6.78PAECh. 6 - Prob. 6.79PAECh. 6 - 6.92 The photoelectric effect can he used to...Ch. 6 - 6.93 A mercury atom is initially in its lowest...Ch. 6 - Prob. 6.82PAECh. 6 - 6.95 A metallic sample is known to be barium,...Ch. 6 - 6.96 When a helium atom absorbs light at 58.44 nm,...Ch. 6 - 6.97 Arrange the members of each of the following...Ch. 6 - 6.98 Arrange the following sets of anions in order...Ch. 6 - 6.99 The photoelectric effect can he used in...Ch. 6 - 6.100 Some spacecraft use ion propulsion engines....Ch. 6 - 6.101 Laser welding is a technique in which a...Ch. 6 - Prob. 6.90PAECh. 6 - 6.103 Atomic absorption spectroscopy is based on...Ch. 6 - 6.104 The red color in fireworks is the result of...Ch. 6 - 6.105 When we say that the existence of atomic...Ch. 6 - 6.106 When Bohr devised his model for the atom,...Ch. 6 - Prob. 6.95PAE
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- Light with a wavelength of 405 nm fell on a strontium surface, and electrons were ejected. If the speed of an ejected electron is 3.36 105 m/s, what energy was expended in removing the electron from the metal? Express the answer in joules (per electron) and in kilojoules per mole (of electrons).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_forwardLight with a wavelength of 425 nm fell on a potassium surface, and electrons were ejected at a speed of 4.88 105 m/s. What energy was expended in removing an electron from the metal? Express the answer in joules (per electron) and in kilojoules per mole (of electrons).arrow_forward
- Heated lithium atoms emit photons of light with an energy of 2.9611019 J. Calculate the frequency and wavelength of one of these photons. What is the total energy in 1 mole of these photons? What is the color of the emitted 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_forwardIt requires 799 kJ of energy to break one mole of carbon-oxygen double bonds in carbon dioxide. What wavelength of light does this correspond to per bond? Is there any transition in the hydrogen atom that has at least this quantity of energy to one photon?arrow_forward
- Neutrons are used to obtain images of the hydrogen atoms in molecules. What energy must be imparted to each neutron in a neutron beam to obtain a wavelength of 10.0 pm? Obtain the energy in electron volts (eV) (1 eV = 1.602 1019 J).arrow_forward6.29 A mercury atom emits light at many wavelengths, two of which are at 435.8 and 546.1 nm. Both of these transitions are to the same final state. (a) What is the energy difference between the two states for each transition? (b) lf a transition between the two higher energy states could be observed, what would be the frequency of the light?arrow_forwardA 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_forward
- As 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_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_forwardThe green line in the atomic spectrum of thallium has a wavelength of 535 nm. Calculate the energy of a photon of this light.arrow_forward
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