Principles of Modern Chemistry
8th Edition
ISBN: 9781305079113
Author: David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher: Cengage Learning
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Textbook Question
Chapter 5, Problem 4P
Label the orbitals described by each of the following sets of quantum numbers:
(a)
(b)
(c)
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Chapter 5 Solutions
Principles of Modern Chemistry
Ch. 5 - Which of the following combinations of quantum...Ch. 5 - Which of the following combinations of quantum...Ch. 5 - Label the orbitals described by each of the...Ch. 5 - Label the orbitals described by each of the...Ch. 5 - Estimate the probability of finding an electron...Ch. 5 - Using Table 5.2, write down the mathematical...Ch. 5 - How many radial nodes and how many angular nodes...Ch. 5 - How many radial nodes and how many angular nodes...Ch. 5 - Use the mathematical expression for the 2pz wave...Ch. 5 - (a) Use the radial wave function for the 3p...
Ch. 5 - Calculate the average distance of the electron...Ch. 5 - The helium ion He+ is a one-electron system whose...Ch. 5 - Spectroscopic studies show that Li can have...Ch. 5 - Spectroscopic studies of Li also show that...Ch. 5 - Spectroscopic studies show that Na can have...Ch. 5 - Using data from Problems 13 and 15, calculate the...Ch. 5 - Give the ground-state electron configurations of...Ch. 5 - Give the ground-state electron configurations of...Ch. 5 - Prob. 19PCh. 5 - Write ground-state electron configurations for the...Ch. 5 - Identify the atom or ion corresponding to each of...Ch. 5 - Identify the atom or ion corresponding to each of...Ch. 5 - Predict the atomic number of the (as yet...Ch. 5 - (a) Predict the atomic number of the (as yet...Ch. 5 - Suppose that the spin quantum number did not...Ch. 5 - Suppose that the spin quantum number had three...Ch. 5 - Photoelectron spectra of mercury (Hg) atoms...Ch. 5 - Quantum mechanics predicts that the energy of the...Ch. 5 - Prob. 29PCh. 5 - Photoelectron spectroscopy studies of silicon...Ch. 5 - Photoelectron spectroscopy studies have determined...Ch. 5 - Prob. 32PCh. 5 - For each of the following pairs of atoms or ions,...Ch. 5 - For each of the following pairs of atoms or ions,...Ch. 5 - Predict the larger ion in each of the following...Ch. 5 - Prob. 36PCh. 5 - The first ionization energy of helium is...Ch. 5 - The energy needed to remove one electron from a...Ch. 5 - Without consulting any tables, arrange the...Ch. 5 - Both the electron affinity and the ionization...Ch. 5 - The cesium atom has the lowest ionization energy,...Ch. 5 - Until recently, it was thought that Ca was...Ch. 5 - In the hydrogen atom, the transition from the 2p...Ch. 5 - The energy needed to ionize an atom of element X...Ch. 5 - Suppose an atom in an excited state can return to...Ch. 5 - For the Li atom, the energy difference between the...Ch. 5 - How does the 3dxy orbital of an electron in O7+...Ch. 5 - The wave function of an electron in the lowest...Ch. 5 - An atom of sodium has the electron configuration...Ch. 5 - (a) The nitrogen atom has one electron in each of...Ch. 5 - Chromium(IV) oxide is used in making magnetic...Ch. 5 - Prob. 52APCh. 5 - Arrange the following seven atoms or ions in order...Ch. 5 - Which is higher, the third ionization energy of...Ch. 5 - The outermost electron in an alkali-metal atom is...Ch. 5 - In two-photon ionization spectroscopy, the...Ch. 5 - For the H atom, the transition from the 2p state...Ch. 5 - (a) Give the complete electron configuration...Ch. 5 - What experimental evidence does the periodic table...
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- Which of the following sets of quantum numbers correctly represents a 4p orbital? (a) n = 4, = 0, m = 1 (b) n = 4, = 1, m = 0 (c) n = 4, = 2, m = 1 (d) n = 4, = 1, m =2arrow_forwardWhat is the maximum number of electrons that can occupy a f subshell (l = 3)?arrow_forwardA 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_forward
- Give the possible values of a. the principal quantum number, b. the angular momentum quantum number, c. the magnetic quantum number, and d. the spin quantum number.arrow_forwardPlanck originated the idea that energies can be quantized. What does the term quantized mean? What was Planck trying to explain when he was led to the concept of quantization of energy? Give the formula he arrived at and explain each of the terms in the formula.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_forward
- According to a relationship developed by Niels Bohr, for an atom or ion that has a single electron, the total energy, En, of an electron in a stable orbit of quantum number n is En = [Z2/n2] (2.179 1018 J) where Z is the atomic number. Calculate the ionization energy for the electron in a ground-state He+ ion.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_forwardWhat experimental evidence supports the quantum theory of light? Explain the wave-particle duality of all matter .. For what size particles must one consider both the wave and the particle properties?arrow_forward
- 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_forwardHow does the wavelength of a fast-pitched baseball compare to the wavelength of an electron traveling at 110 the speed of light? What is the significance of this comparison? See Example 2-3.arrow_forwardImagine a world in which the rule for the l quantum number is that values start with 1 and go up to n. The rules for the n and mi quantum numbers are unchanged from those of our world. Write the quantum numbers for the first two shells (i.e., n = 1 and n = 2).arrow_forward
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