Inorganic Chemistry
5th Edition
ISBN: 9781292134147
Author: Housecroft, Catherine E.
Publisher: Pearson,
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Textbook Question
Chapter 1, Problem 18P
How many atomic orbitals make up the set with n=4 and l=3? What label is given to this set of orbitals? Write down a set of quantum numbers that defines each orbital in the set.
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Chapter 1 Solutions
Inorganic Chemistry
Ch. 1 - Chromium has four isotopes C2450r, C2452r, C2453r...Ch. 1 - Prob. 2PCh. 1 - Using the list of naturally occurring isotopes in...Ch. 1 - Hydrogen possesses three isotopes, but tritium ,...Ch. 1 - (a) By using the data in appendix 5, account for...Ch. 1 - Calculate the corresponding wavelength of...Ch. 1 - State which of the following n'n transitions in...Ch. 1 - Calculate the energy (in kJ per mole of photons)...Ch. 1 - 1.9 Four of the lines in Balmer series are at...Ch. 1 - 1.10 Using the Bohr model, determine the values of...
Ch. 1 - 1.11 How is the (a) energy and (b) size of an ns...Ch. 1 - 1.12 Write down a set of quantum numbers that...Ch. 1 - Do the three 4p atomic orbitals possess the same...Ch. 1 - How many radial nodes does each of the following...Ch. 1 - 1.15 Comment on the differences between plots of...Ch. 1 - 1.16 Write down the sets of quantum numbers that...Ch. 1 - Write down the three sets of quantum numbers that...Ch. 1 - How many atomic orbitals make up the set with n=4...Ch. 1 - Prob. 19PCh. 1 - (a) Will a plot of R(r) for the 1s atomic orbital...Ch. 1 - Prob. 21PCh. 1 - Prob. 22PCh. 1 - Write down the six sets of quantum numbers that...Ch. 1 - For a neutral atom, X, the following atomic...Ch. 1 - Using the concepts of shielding and penetration,...Ch. 1 - For each of the following atoms, write down a...Ch. 1 - 1.27 Draw energy level diagrams (see Fig. 1.15) to...Ch. 1 - 1.28 Write down the ground state electronic...Ch. 1 - Write down (with reasoning) the ground state...Ch. 1 - Draw energy level diagrams to show the ground...Ch. 1 - The ground state electronic configuration of a...Ch. 1 - (a) Write down an equation that defines the...Ch. 1 - 1.33 The first four ionization energies of an atom...Ch. 1 - 1.34 In Fig. 1.16, identify the trend in the first...Ch. 1 - 1.35 Figure 1.17 shows the values of for the...Ch. 1 - Using the data in Table 1.5, determine a value for...Ch. 1 - Prob. 37PCh. 1 - What is the evidence that the aufbau principle is...Ch. 1 - The first list in the table on the left contains...Ch. 1 - Prob. 40PCh. 1 - Using data from appendix 8, construct a graph to...Ch. 1 - The sign convention for electron affinity can...Ch. 1 - Prob. 43PCh. 1 - 1.45 Figure 1.18 shows the emission spectrum of...
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- • identify an orbital (as 1s, 3p, etc.) from its quantum numbers, or vice versa.arrow_forwardWhat type of electron orbital (i.e., s, p, d, or f) is designated by an electron with quantum numbers (a) n=1,l=0,m l =0(b) n=3,l=2,m l =1? (c) n=4,l=3,m l =3arrow_forwardWhich 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_forward
- One bit of evidence that the quantum mechanical model is correct lies in the magnetic properties of matter. Atoms with unpaired electrons are attracted by magnetic fields and thus are said to exhibit pararamagnetism. The degree to which this effect is observed is directly related to the number of unpaired electrons present in the atom. Consider the ground-state electron configurations for Li, N, Ni, Te, Ba, and Hg. Which of these atoms would be expected to be paramagnetic, and how many unpaired electrons are present in each paramagnetic atom?arrow_forwardExplain the difference between (a) the Bohr model of the atom and the quantum mechanical model. (b) wavelength and frequency. (c) the geometries of the three different p orbitals.arrow_forwardSuppose that the spin quantum number did not exist, and therefore only one electron could occupy each orbital of a many-electron atom. Give the atomic numbers of the first three noble-gas atoms in this case.arrow_forward
- Sketch an orbital contour that is expected for an electron that has n = 3 and = 2.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_forwardAlthough no currently known elements contain electrons in g orbitals in the ground state, it is possible that these elements will be found or that electrons in excited states of known elements could being orbitals. For g orbitals, the value of l is 4. What is the lowest value of n for which g orbitals could exist? What are tile possible values of ml? How many electrons could a set of g orbitals hold?arrow_forward
- Suppose that the spin quantum number could have the values 12,0 and 12 . Assuming that the rules governing the values of the other quantum numbers and the order of filling sublevels were unchanged, (a) what would be the electron capacity of an s sublevel? a p sublevel? a d sublevel? (b) how many electrons could fit in the n=3 level? (c) what would be the electron configuration of the element with atomic number 8? 17?arrow_forwardAssign a correct set of four quantum numbers for (a) Each electron in a nitrogen atom. (b) The valence electron in a sodium atom. (c) A 3d electron in a nickel atom.arrow_forwardConstruct an energy level diagram showing all orbitals for the hydrogen atom up to n=5, labeling each orbital with its appropriate quantum numbers. How many different orbitals are in each shell?arrow_forward
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