Physical Chemistry
2nd Edition
ISBN: 9781133958437
Author: Ball, David W. (david Warren), BAER, Tomas
Publisher: Wadsworth Cengage Learning,
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Chapter 12, Problem 12.29E
Using a periodic table (or Table 12.1), find the elements whose electron configurations do not follow the aufbau principle strictly. Comment on any relationship between these elements or their place within the periodic table.
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Only trace amounts of the synthetic element darmstadtium, atomic number 110, have been obtained. The element is so highly unstable that no observations of its properties have been possible. Based on its position in the periodic table, propose three different reasonable valence electron configurations for this element.
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DO NOT base your answer on tabulated values since exceptions may occur.
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polonium
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Four main-group elements a, b, c and d are highlighted in the outline of the Periodic Table below:
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a, b,
Important: don't try to figure out exactly which elements are marked, and then use your knowledge of the properties of each specific element. You don't need
to. You will also be marked wrong for any answer, correct or not, that can't be determined from only the rough location of each marked element in the Periodic
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3
Chapter 12 Solutions
Physical Chemistry
Ch. 12 - In the Stern-Gerlach experiment, silver atoms were...Ch. 12 - Prob. 12.2ECh. 12 - Prob. 12.3ECh. 12 - Suppose s=12 for an electron. Into how many parts...Ch. 12 - Using and labels, write two possible...Ch. 12 - List all possible combinations of all four quantum...Ch. 12 - What are the degeneracies of the H atom...Ch. 12 - Prob. 12.8ECh. 12 - a Differentiate between the quantum numbers s and...Ch. 12 - Is the spin orbital 1s for the H atom still...
Ch. 12 - Draw a diagram analogous to Figure 11.15, but now...Ch. 12 - Are mathematical expressions for the following...Ch. 12 - Prob. 12.13ECh. 12 - Prob. 12.14ECh. 12 - a Assume that the electronic energy of Li was a...Ch. 12 - Spin orbitals are products of spatial and spin...Ch. 12 - If 1 and 2 are the individual wavefunctions for...Ch. 12 - Show that the correct behavior of a wavefunction...Ch. 12 - Prob. 12.19ECh. 12 - Why isnt the electron configuration of beryllium,...Ch. 12 - Prob. 12.21ECh. 12 - Write a Slater determinant for the lithide ion,...Ch. 12 - Why does the concept of antisymmetric...Ch. 12 - a Construct Slater determinant wavefunctions for...Ch. 12 - Prob. 12.25ECh. 12 - Prob. 12.26ECh. 12 - Prob. 12.27ECh. 12 - Suppose an electron had three possible values of...Ch. 12 - Using a periodic table or Table 12.1, find the...Ch. 12 - Write an acceptable electron configuration for...Ch. 12 - Prob. 12.31ECh. 12 - Prob. 12.32ECh. 12 - Prob. 12.33ECh. 12 - An anharmonic oscillator has the potential...Ch. 12 - Prob. 12.35ECh. 12 - In a particle-in-a-box having length a, the...Ch. 12 - Prob. 12.37ECh. 12 - Prob. 12.38ECh. 12 - Prob. 12.39ECh. 12 - The Stark effect is the change in energy of a...Ch. 12 - Prob. 12.41ECh. 12 - Prob. 12.42ECh. 12 - Prob. 12.43ECh. 12 - Show that a variation theory treatment of H using...Ch. 12 - Prob. 12.45ECh. 12 - Explain why assuming an effective nuclear charge,...Ch. 12 - Prob. 12.47ECh. 12 - Consider a real system. Assume that a real...Ch. 12 - Prob. 12.49ECh. 12 - Prob. 12.50ECh. 12 - Prob. 12.51ECh. 12 - Prob. 12.52ECh. 12 - State the Born-Oppenheimer approximation in words...Ch. 12 - Prob. 12.54ECh. 12 - Spectroscopy deals with differences in energy...Ch. 12 - Prob. 12.56ECh. 12 - What is the bond order for the lowest excited...Ch. 12 - The helium atom was defined as two electrons and a...Ch. 12 - Explain how we know that the first in equation...Ch. 12 - Prob. 12.60ECh. 12 - Prob. 12.61ECh. 12 - Use molecular orbital arguments to decide whether...Ch. 12 - Prob. 12.63ECh. 12 - Prob. 12.65ECh. 12 - Prob. 12.67ECh. 12 - Prob. 12.68E
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- Consider the eight most abundant elements in the human body, as outlined in Exercise 156. Excluding hydrogen, which of these elements would have the smallest size? largest size? smallest first ionization energy? largest first ionization energy?arrow_forwardWhen we first learn to write electron configurations for atoms, we use the Pauli Exclusion Principle (PEP) and Hund's Rules to ensure that what we write is consistent with what we observe in nature, the Periodic Table. Consider carbon and oxygen and write the correct ground state electron configurations for both; having done so, reflect on how you intuitively used the PEP and Hund's Rules. Now think about the formal statement of the PEP written as Postulate 6 of Quantum Mechanics. All electronic wave functions must be antisymmetric under the interchange of any two electrons. Now we come to it; determine the most stable atomic term symbol for both elements and explain Hund's Rules (see below) are manifested in the singular that you used to write the correct ground state electron configurations. Hund's Rules 1. The state with the largest value of S is the most stable, and stability decreases with decreasing S. 2. For states with the same value of S, the state with the largest value of L…arrow_forwardBoth the electron affinity and the ionization energy of chlorine are higher than the corresponding quantities for sulfur. Explain why in terms of the electronic structure of the atoms.arrow_forward
- There are three rules electrons normally follow when occupying orbitals in an atom. (i) Name each of these rules and then (ii) explain how each rule has an effect on the electron filling order. To illustrate these rules, (iii) draw a diagram of the electron filling pattern for oxygen. Note: Do not just write out the electron configuration; you must draw some form of diagram that explains the order electronsarrow_forwardWrite out in full the ground state configuration (all of the electrons) in the element bromine (atomic number = 35). There are three different abbreviated ways to write out the electron configuration using the symbolic form for the elements in group 18 (8A). Write out the one using the heaviest group 18 (8A) element.arrow_forwardIn Section 8.6, we estimated the effective nuclear charge on beryllium’s valence electrons to be slightly greater than 2+. What would a similar process predict for the effective nuclear charge on boron’s valence electrons? Would you expect the effective nuclear charge to be different for boron’s 2s electrons compared to its 2p electron? In what way? (Hint: Consider the shape of the 2p orbital compared to that of the 2s orbital.)arrow_forward
- Four main-group elements a, b, c and d are highlighted in the outline of the Periodic Table below: a b d с List these elements below by increasing ionization energy. For example, if a has the lowest ionization energy and b the next highest, then your list should start a, b, ... Important: don't try to figure out exactly which elements are marked, and then use your knowledge of the properties of each specific element. You don't need to. You will also be marked wrong for any answer, correct or not, that can't be determined from only the rough location of each marked element in the Periodic Table. 0000 xarrow_forwardWrite general outer electron configurations (nsxnpy) for groups 6A and 7A in the periodic table. The electron affinity of each group 7A element is more negative than that of each corresponding group 6A element. Use the electron configurations to explain why this is so.arrow_forwardThe electron configuration can also be represented by writing the symbol for the occupied subshell and adding a superscript to indicate the number of electrons in that subshell. For example, consider a carbon atom having an atomic number of 6. The total number of electrons in a neutral carbon atom is 6. The electron configuration of the carbon atom represented by the orbital diagram is This electron configuration can be written as C-1111 18 28 2p 1² 28² 2p² where 1s, 2s, and 2p are the occupied subshells, and the superscript "2" is the number of electrons in each of these subshells Use the rules for determining electron configurations to write the electron configuration for Ca Express your answer in complete form in order of orbital filling. For example, 1s 2s should be entered as 15 225 2. ▸ View Available Hint(s)arrow_forward
- II Electron Configuration and Orbital Diagrams Directions: Write the complete electron configuration of the following elements and draw their orbital diagrams. State whether the element is paramagnetic or diamagnetic. The first one is done for you. Number of electrons Magnetic Property Electron Element Orbital Diagram Configuration IL 1 Lithium Paramagnetic 1s22s1 1s 25 2p 3s Oxygen Fluorine Bromine Silicon Potassium Кгуpton Sulfur Manganese Sodium Zincarrow_forwardIdentify three atoms from their electron configurations. Correlate the elements to the appropriate ionization energies and atomic radii. You have determined that the electron configuration of 1s²2s²2p⁶3s² corresponds to the element Mg. You have determined the identity of three elements based electron configurations. These three elements have the following three first ionization energies: 590, 738, and 999 kJ/mol The element with the electron configuration of 1s²2s²2p⁶3s² corresponds to which ionization energy?arrow_forwardConsider Si, S, and P.1) Based purely on ideas of electron screening and effective nuclear charge, which of these elements do you expect to have the highest first ionization energy?2) Based on experimental data, P has the highest first ionization energy. Explain this observation in terms of electron configuration arguments.arrow_forward
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