1 Introduction To Chemistry 2 Atoms And Molecules 3 Molecules, Moles, And Chemical Equations 4 Stoichiometry 5 Gases 6 The Periodic Table And Atomic Structure 7 Chemical Bonding And Molecular Structure 8 Molecules And Materials 9 Energy And Chemistry 10 Entropy And The Second Law Of Thermodynamics 11 Chemical Kinetics 12 Chemical Equilibrium 13 Electrochemistry 14 Nuclear Chemistry Chapter6: The Periodic Table And Atomic Structure
Chapter Questions Section: Chapter Questions
Problem 1CO: describe trace analysis and explain its role in materials testing. Problem 2CO: describe waves in terms of frequency, wavelength, and amplitude. Problem 3CO Problem 4CO: relate the frequency, wavelength, and amplitude of light to characteristics such as color and... Problem 5CO: describe the photoelectric effect by stating what sort of experiment is involved and what results... Problem 6CO Problem 7CO: • use Planck’s equation to calculate the energy of a photon from its wavelength or frequency. Problem 8CO Problem 9CO Problem 10CO: • describe similarities and differences between the Bohr model and the quantum mechanical model of... Problem 11CO Problem 12CO Problem 13CO: • identify an orbital (as 1s, 3p, etc.) from its quantum numbers, or vice versa. Problem 14CO: • list the number of orbitals of each type (1s, 3p, etc) in an atom. Problem 15CO: • sketch the shapes of s and p orbitals and recognize orbitals by their shapes. Problem 16CO: • rank various orbitals in terms of size and energy. Problem 17CO Problem 18CO Problem 19CO Problem 20CO Problem 6.1PAE Problem 6.2PAE: 6.2 Unlike XRF, AAS cannot be used for nondestructive testing. Explain why not. Problem 6.3PAE Problem 6.4PAE Problem 6.5PAE Problem 6.6PAE Problem 6.7PAE: 6.7 Arrange the following regions of the electromagnetic spectrum in order of increasing frequency:... Problem 6.8PAE: 6.8 Calculate the wavelength in meters, of radiation of the following frequencies. (a) 5.001015s1... Problem 6.9PAE: 6.9 If a string of decorative lights includes bulbs with wave-lengths of 480, 580, and 700 mm, what... Problem 6.10PAE: 6.10 Define the term refraction. Problem 6.11PAE: 6.11 Define the term photon. Problem 6.12PAE: 6.12 Find the energy of a photon with each of the following frequencies (see Table 1.2 if needed).... Problem 6.13PAE: 6.13 Place these types of radiation in order of increasing energy per photon. (a) green light from a... Problem 6.14PAE: 6.14 For photon with the following energies, calculate the wavelength and identify the region of the... Problem 6.15PAE Problem 6.16PAE: 6.16 Various optical disk drives rely on laser operating at different wavelengths, with shorter... Problem 6.17PAE: 6.17 The laser in most supermarket barcode scanners operates at a wavelength of 632.8 nm. What is... Problem 6.18PAE: 6.18 Assume that a microwave oven operates at a frequency of 1.001011s1 . (a) What is the wavelength... Problem 6.19PAE: 6.19 Fill in the blanks below to complete a description of the photoelectric effect experiment. (You... Problem 6.20PAE: 6.20 When light with a wavelength of 58.5 nm strikes the surface of tin metal, electrons are ejected... Problem 6.21PAE: 6.21 The electron binding energy fur copper metal is 7.181019J . Find the longest wavelength of... Problem 6.22PAE Problem 6.23PAE: 6.23 Describe how the Bohr model of the atom accounts for the spectrum of the hydrogen atom. Problem 6.24PAE: 6.24 According to the Bohr model of the atom, what happens when an atom absorbs energy? Problem 6.25PAE: 6.25 Define the term ground state. Problem 6.26PAE: 6.26 The figure below depicts the first four energy levels in a hydrogen atom. The three transitions... Problem 6.27PAE: 6.27 Refer w the data and energy-Ievel diagram shown in Problem 6.26, and find the wavelength of... Problem 6.28PAE: 6.28 A neon atom cmi light at many wavelengths, two of which are at 616.4 and 638.3 nm. Both of... Problem 6.29PAE: 6.29 A mercury atom emits light at many wavelengths, two of which are at 435.8 and 546.1 nm. Both of... Problem 6.30PAE: 6.30 How did the observation of electron diffraction affect the development of the quantum... Problem 6.31PAE: 6.31 Why do we use a wave function to describe electrons? Problem 6.32PAE: 6.32 What are the mathematical origins of quantum numbers? Problem 6.33PAE Problem 6.34PAE: 6.34 Which of the following represent valid sets of quantum numbers? For a set that is invalid,... Problem 6.35PAE: 6.35 A particular orbital has n = 4 and l = 2. What type of orbital must this be? (a) 3p, (b) 4p,... Problem 6.36PAE: 6.36 Why are there no 2d orbitals? Problem 6.37PAE: 6.34 What is the maximum number of electrons in an atom that can have the following quantum numbers?... Problem 6.38PAE: 6.38 How many orbitals correspond to each of the following designations? (a) 3p, (b) 4p, (c) 4px,... Problem 6.39PAE Problem 6.40PAE: 6.40 Referring to Figure 6.15, draw a 4p orbitals, showing all of its nodes. Problem 6.41PAE: 6.41 Consider a 3d orbital. (a) What are the allowed values for the n and l quantum numbers for a 3d... Problem 6.42PAE Problem 6.43PAE: 6.43 Define the term spin paired. Problem 6.44PAE: 6.44 On what does the Pauli exclusion principle place a limit? Problem 6.45PAE Problem 6.46PAE Problem 6.47PAE: 6.47 Depict two ways to place electrons in the 2p orbitals for a nitrogen atom. Which depiction is... Problem 6.48PAE: 6.48 Write the ground state electron configuration for (a) B, (b) Ba, (c) Be, (d) Bi, (e) Br. Problem 6.49PAE: 6.49 Which of these electron configurations are for atoms in the ground state? In excited states?... Problem 6.50PAE: 6.50 From the list of atoms and ions given, identify any pairs that have the same electron... Problem 6.51PAE Problem 6.52PAE Problem 6.53PAE Problem 6.54PAE Problem 6.55PAE: 6.55 Explain why the s block of the periodic table contains two columns, the p block contains six... Problem 6.56PAE Problem 6.57PAE Problem 6.58PAE Problem 6.59PAE Problem 6.60PAE: 6.60 Use the electron configurations of the alkali metals and your knowledge of orbitals and quantum... Problem 6.61PAE: 6.61 Using only a periodic table as a guide, arrange each of the following series of atoms in order... Problem 6.62PAE: 6.62 Define the term ionization energy. Distinguish between the first ionization energy and the... Problem 6.63PAE: 6.63 At which ionization for chlorine would you expect the first large jump in ionization energy?... Problem 6.64PAE: 6.64 Arrange the following atoms in order of increasing ionization energy: Li, K, C, and N. Problem 6.65PAE Problem 6.66PAE: 6.66 Which element would you expect to have the largest second ionization energy, Na, C, or F? Why? Problem 6.67PAE Problem 6.68PAE: 6.68 Indicate which species in each pair has the more favorable (more negative) electron affinity.... Problem 6.69PAE: 6.69 Compare the elements Na, B, Al, and C with regard to the following properties. (a) Which has... Problem 6.70PAE: 6.70 Rank the following in order of decreasing ionization energy: Cl , F, Ne+ , S, S . Problem 6.71PAE: 6.71 Several excited states of the neon atom are important in the operation of a helium-neon laser.... Problem 6.72PAE: 6.72 LED bulbs offer a fairly new lighting alternative, and are becoming increasingly popular in... Problem 6.73PAE: 6.73 How much energy could be saved each year by replacing incandescent bulbs with LED bulbs? Assume... Problem 6.74PAE Problem 6.75PAE Problem 6.76PAE Problem 6.77PAE Problem 6.78PAE Problem 6.79PAE: 6.79 How does the charge of electrons provide some rationale for Hund’s rule? Problem 6.80PAE: 6.80 Describe how valence electron configurations account for some of the similarities in chemical... Problem 6.81PAE: 6.81 Why is there no element to the immediate right of magnesium in the periodic table? Problem 6.82PAE: 6.82 A particular element has the following values for its first four ionization energies: 900,... Problem 6.83PAE: 6.83 The graph below shows the first three ionization energies for sodium, magnesium, and aluminum.... Problem 6.84PAE: 6.84 Which graph correctly depicts the first ionization energy of three elements in groups 14... Problem 6.85PAE: 6.85 The visible lines in the hydrogen atom emission spectrum arise from transitions with a final... Problem 6.86PAE: 6.86 An excited He+ ion returns to the ground state by emitting a series of three photons, with... Problem 6.87PAE Problem 6.88PAE Problem 6.89PAE Problem 6.90PAE Problem 6.91PAE: 6.91 What is the only noble gas that does not have an ns2np6 electron configuration? How can it be a... Problem 6.92PAE: 6.92 The photoelectric effect can he used to measure the value of Planck's constant. Suppose that a... Problem 6.93PAE: 6.93 A mercury atom is initially in its lowest possible (or ground state) energy level. The atom... Problem 6.94PAE Problem 6.95PAE: 6.95 A metallic sample is known to be barium, cesium, lithium, or silver. The electron binding... Problem 6.96PAE: 6.96 When a helium atom absorbs light at 58.44 nm, an electron is promoted from the 1s orbital to a... Problem 6.97PAE: 6.97 Arrange the members of each of the following sets of cations in order of increasing ionic... Problem 6.98PAE: 6.98 Arrange the following sets of anions in order of increasing ionic radii. (a) Cl,S2,P3, (b)... Problem 6.99PAE: 6.99 The photoelectric effect can he used in engineering designs for practical applications. For... Problem 6.100PAE: 6.100 Some spacecraft use ion propulsion engines. These engines create thrust by ionizing atoms and... Problem 6.101PAE: 6.101 Laser welding is a technique in which a tightly focused laser beam is used to deposit enough... Problem 6.102PAE Problem 6.103PAE: 6.103 Atomic absorption spectroscopy is based on the atomic spectra of the elements being studied.... Problem 6.104PAE: 6.104 The red color in fireworks is the result of having strontium-containing salts in the fireworks... Problem 6.105PAE: 6.105 When we say that the existence of atomic spectra tells us that atoms have specific energy... Problem 6.106PAE: 6.106 When Bohr devised his model for the atom, was he using deductive or inductive reasoning?... Problem 6.107PAE Problem 6.68PAE: 6.68 Indicate which species in each pair has the more favorable (more negative) electron affinity....
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Which has the more negative electron affinity , O or C? Explain your answer.
Definition Definition Change in energy of a neutral gaseous atom when an electron is added to the atom to form a negative ion.
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