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ChemistryChemistry for Engineering Students6.87 Why do valence electrons experience a smaller effective nuclear charge rather than the full charge of the nucleus?
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6.87 Why do valence electrons experience a smaller effective nuclear charge rather than the full charge of the nucleus?

BuyFind

Chemistry for Engineering Students

4th Edition
Lawrence S. Brown + 1 other
Publisher: Cengage Learning
ISBN: 9781337398909
BuyFind

Chemistry for Engineering Students

4th Edition
Lawrence S. Brown + 1 other
Publisher: Cengage Learning
ISBN: 9781337398909

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Chapter 6, Problem 6.87PAE
Textbook Problem

6.87 Why do valence electrons experience a smaller effective nuclear charge rather than the full charge of the nucleus?

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Chapter 6 Solutions

Chemistry for Engineering Students
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Ch. 6 - describe trace analysis and explain its role in...Ch. 6 - describe waves in terms of frequency, wavelength,...Ch. 6 - interconvert between the frequency and wavelength...Ch. 6 - relate the frequency, wavelength, and amplitude of...Ch. 6 - describe the photoelectric effect by stating what...Ch. 6 - • explain how the results of the photoelectric...Ch. 6 - • use Planck’s equation to calculate the energy of...Ch. 6 - • use ideas about conservation of energy to...Ch. 6 - • use an energy-level diagram to predict the...Ch. 6 - • describe similarities and differences between...
Ch. 6 - • recognize how quantum numbers arise as a...Ch. 6 - • define the term orbital.Ch. 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 - • use the Pauli exclusion principle and Hund’s...Ch. 6 - • explain the connection between valence electron...Ch. 6 - • define the following properties of atoms: atomic...Ch. 6 - • state how the above properties vary with...Ch. 6 - 6.1 Trace analysis may be carried out via...Ch. 6 - 6.2 Unlike XRF, AAS cannot be used for...Ch. 6 - 6.3 In analysis by atomic absorption spectroscopy,...Ch. 6 - 6.4 An X-ray fluorescence instrument must include...Ch. 6 - 6.5 The fluorescence emitted in XRF is also in the...Ch. 6 - 6.6 As part of its analytical capabilities, the...Ch. 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 - 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 - 6.15 For photon with the following energies,...Ch. 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 - 6.22 What was novel about Bohr’s of the atom?Ch. 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 - 6.33 What are the allowed values for the principal...Ch. 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 - 6.39 Define the term nodal plane (or node).Ch. 6 - 6.40 Referring to Figure 6.15, draw a 4p orbitals,...Ch. 6 - 6.41 Consider a 3d orbital. (a) What are the...Ch. 6 - 6.42 Does the fact that the fourth quantum number...Ch. 6 - 6.43 Define the term spin paired.Ch. 6 - 6.44 On what does the Pauli exclusion principle...Ch. 6 - 6.45 Define the term shielding.Ch. 6 - 6.46 What is effective nuclear charge and how does...Ch. 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 - 6.51 halogen lamps rely on the predictable...Ch. 6 - 6.52 Distinguish between the terms core electrons...Ch. 6 - 6.53 If another 50 elements were discovered, how...Ch. 6 - 6.54 Which blocks of the periodic table comprise...Ch. 6 - 6.55 Explain why the s block of the periodic table...Ch. 6 - 6.56 Look at the table of electron configurations...Ch. 6 - 6.57 The magnetic properties of atoms provide...Ch. 6 - 6.58 The more unpaired electrons an element...Ch. 6 - 6.59 How does the effective nuclear charge help...Ch. 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 - 6.65 How do we explain the fact that the...Ch. 6 - 6.66 Which element would you expect to have the...Ch. 6 - 6.67 Answer each of die following questions. (a)...Ch. 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 - 6.72 LED bulbs offer a fairly new lighting...Ch. 6 - 6.73 How much energy could be saved each year by...Ch. 6 - 6.74 Which of the waves depicted here has the...Ch. 6 - 6.75 What is the relationship between the number...Ch. 6 - 6.76 What is the difference between continuous and...Ch. 6 - 6.77 The p and d orbitals are sometimes referred...Ch. 6 - 6.78 Why does the size of an orbital have an...Ch. 6 - 6.79 How does the charge of electrons provide some...Ch. 6 - 6.80 Describe how valence electron configurations...Ch. 6 - 6.81 Why is there no element to the immediate...Ch. 6 - 6.82 A particular element has the following values...Ch. 6 - 6.83 The graph below shows the first three...Ch. 6 - 6.84 Which graph correctly depicts the first...Ch. 6 - 6.85 The visible lines in the hydrogen atom...Ch. 6 - 6.86 An excited He+ ion returns to the ground...Ch. 6 - 6.87 Why do valence electrons experience a smaller...Ch. 6 - 6.88 Why does the existence of line spectra imply...Ch. 6 - 6.89 The Rb+ ion happens, by coincidence, to be...Ch. 6 - 6.90 How does the screening by core electrons...Ch. 6 - 6.91 What is the only noble gas that does not have...Ch. 6 - 6.92 The photoelectric effect can he used to...Ch. 6 - 6.93 A mercury atom is initially in its lowest...Ch. 6 - 6.94 When a photoelectric effect experiment was...Ch. 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 - 6.102 Ionization gauges for pressure measurement...Ch. 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 - 6.107 The photochemical reaction that initiates...

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