Chemical Principles
8th Edition
ISBN: 9781305581982
Author: Steven S. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Chapter 13, Problem 15E
An alternative definition of electronegativity isElectronegativity=constant (I.E. −E.A.) where I.E. is the ionization energy and E.A. is the electronaffinity using the sign conventions of this book. Use datain Chapter 12 to calculate the (I.E. −E.A.) term for F, Cl,Br, and I. Do these values show the same trend as theelectronegativity values given in this chapter? The firstionization energies of the halogens are 1678, 1255, 1138,and 1007 kJ/mol, respectively. (Hint: Choose a constantso that the electronegativity of fluorine equals 4.0. Usingthis constant, calculate relative electro-negativities for theother halogens and compare to values given in the text.)
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Write electron configurations for the most stable ion formed by each of the elements Al, Sr, 0, and I (when in stable ionic compounds).
(Express your answer as a series of orbitals. For example, the electron configuration of Li would be entered in complete form as Is 2s' or in condensed form as [He]2s.)
Electron configuration for the most stable ion of Al =
%3D
Electron configuration for the most stable ion of Sr =
Electron configuration for the most stable ion of O =
Electron configuration for the most stable ion of I =
%3D
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See image below. Can you please show me how to solve this? I got -910kJ/mol as the lattice energy..
Chapter 13 Solutions
Chemical Principles
Ch. 13 - Explain the electronegativity trends across a row...Ch. 13 - Prob. 2DQCh. 13 - Prob. 3DQCh. 13 - Prob. 4DQCh. 13 - Prob. 5DQCh. 13 - Prob. 6DQCh. 13 - Prob. 7DQCh. 13 - Prob. 8DQCh. 13 - Prob. 9DQCh. 13 - Arrange the following molecules from most to least...
Ch. 13 - Prob. 11DQCh. 13 - Prob. 12DQCh. 13 - Prob. 13ECh. 13 - Prob. 14ECh. 13 - An alternative definition of electronegativity...Ch. 13 - Prob. 16ECh. 13 - Without using Fig. 13.3, predict the order of...Ch. 13 - Without using Fig. 13.3, predict which bond in...Ch. 13 - Prob. 19ECh. 13 - Prob. 20ECh. 13 - Indicate the bond polarity (show the partial...Ch. 13 - Prob. 22ECh. 13 - Prob. 23ECh. 13 - Prob. 24ECh. 13 - Prob. 25ECh. 13 - Prob. 26ECh. 13 - Prob. 27ECh. 13 - Prob. 28ECh. 13 - Prob. 29ECh. 13 - Prob. 30ECh. 13 - Prob. 31ECh. 13 - Give an example of an ionic compound where both...Ch. 13 - What noble gas has the same electron configuration...Ch. 13 - Which of the following ions have noble gas...Ch. 13 - Give three ions that are isoelectronic with...Ch. 13 - Prob. 36ECh. 13 - Predict the empirical formulas of the ionic...Ch. 13 - Which compound in each of the following pairs of...Ch. 13 - Use the following data to estimate Hf for...Ch. 13 - Use the following data to estimate Hf for...Ch. 13 - Consider the following:...Ch. 13 - In general, the higher the charge on the ions in...Ch. 13 - Consider the following energy changes: a....Ch. 13 - Prob. 44ECh. 13 - Prob. 45ECh. 13 - The lattice energies of FeCl3,FeCl2,andFe2O3 are...Ch. 13 - Prob. 47ECh. 13 - Prob. 48ECh. 13 - Prob. 49ECh. 13 - Prob. 50ECh. 13 - Prob. 51ECh. 13 - Prob. 52ECh. 13 - Prob. 53ECh. 13 - Prob. 54ECh. 13 - Prob. 55ECh. 13 - Prob. 56ECh. 13 - Prob. 57ECh. 13 - Prob. 58ECh. 13 - Prob. 59ECh. 13 - Prob. 60ECh. 13 - Prob. 61ECh. 13 - Prob. 62ECh. 13 - Prob. 63ECh. 13 - Prob. 64ECh. 13 - Prob. 65ECh. 13 - Prob. 66ECh. 13 - Prob. 67ECh. 13 - Prob. 68ECh. 13 - Prob. 69ECh. 13 - Prob. 70ECh. 13 - Prob. 71ECh. 13 - Prob. 72ECh. 13 - Prob. 73ECh. 13 - Prob. 74ECh. 13 - Prob. 75ECh. 13 - Prob. 76ECh. 13 - Prob. 77ECh. 13 - Prob. 78ECh. 13 - Prob. 79ECh. 13 - Prob. 80ECh. 13 - Prob. 81ECh. 13 - Prob. 82ECh. 13 - Prob. 83ECh. 13 - Prob. 84ECh. 13 - Prob. 85ECh. 13 - Prob. 86ECh. 13 - Prob. 87ECh. 13 - Prob. 88ECh. 13 - Prob. 89ECh. 13 - Prob. 90ECh. 13 - Prob. 91ECh. 13 - Prob. 92ECh. 13 - Prob. 93ECh. 13 - Prob. 94ECh. 13 - Prob. 95ECh. 13 - Predict the molecular structure and the bond...Ch. 13 - Prob. 97ECh. 13 - Two variations of the octahedral geometry are...Ch. 13 - Prob. 99ECh. 13 - Predict the molecular structure and the bond...Ch. 13 - Which of the molecules in Exercise 96 have net...Ch. 13 - Prob. 102ECh. 13 - Give two requirements that should be satisfied for...Ch. 13 - What do each of the following sets of...Ch. 13 - Prob. 105ECh. 13 - Consider the following Lewis structure, where E is...Ch. 13 - Consider the following Lewis structure, where E is...Ch. 13 - Prob. 108ECh. 13 - Prob. 109ECh. 13 - Which of the following molecules have net dipole...Ch. 13 - Prob. 111AECh. 13 - Prob. 112AECh. 13 - Prob. 113AECh. 13 - Prob. 114AECh. 13 - Prob. 115AECh. 13 - There are two possible structures of XeF2Cl2 ,...Ch. 13 - Prob. 117AECh. 13 - Prob. 118AECh. 13 - Prob. 119AECh. 13 - Prob. 120AECh. 13 - Prob. 121AECh. 13 - Prob. 122AECh. 13 - Prob. 123AECh. 13 - Prob. 124AECh. 13 - Prob. 125AECh. 13 - Prob. 126AECh. 13 - Prob. 127AECh. 13 - Prob. 128AECh. 13 - Prob. 129AECh. 13 - Prob. 130AECh. 13 - Prob. 131AECh. 13 - Prob. 132AECh. 13 - Prob. 133CPCh. 13 - Prob. 134CPCh. 13 - Given the following information: Heat of...Ch. 13 - Prob. 136CPCh. 13 - A promising new material with great potential as...Ch. 13 - Think of forming an ionic compound as three steps...Ch. 13 - Prob. 139CPCh. 13 - Prob. 140CPCh. 13 - Calculate the standard heat of formation of the...Ch. 13 - Prob. 142CPCh. 13 - Prob. 143MP
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- Assuming that the distances between the two ions are the same in all cases, which of the following ion pairs has the smallest electrostatic potential energy? Select one: a. Fe3+- Cl- b. K*- I c. Ca2+- s²- O d. Al3+- p3- e. Lit- 02-arrow_forwarding and lea X G The element in period 5 that has X ent/takeCovalentActivity.do?locator-assignment-take 3 eq 2. The central nitrogen atom V A. Obeys the octet rule B. Has an incomplete octet. C. Has an expanded octet. Submit Answer [Review Topics] [References] Use the References to access important values if needed for this question. Lewis Structures Lewis Structures are used to describe the covalent bonding in molecules and ions. Draw a Lewis structure for NH4 and answer the following questions based on your drawing. 1. For the central nitrogen atom: The number of lone pairs The number of single bonds = The number of double bonds= 3 Retry Entire Group 4+ C Solved The following Lewis diagr X 00 144 6 9 more group attempts remaining + 0 44 ort sc A ENG deleta Previous back space 16 ☆ Next 11:55 AM 11/28/2022 end 1arrow_forward6. Using the periodic table, arrange the following in increasing order: a. Electronegativity: Fr, Rn, Cs, At b. Atomic radius: Xe, F. Rb Sn ,Sr c. First ionization energy: Al, Ar, Cs Na d. lonic radii: Se?, Rb', Srt, Parrow_forward
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- Write electron configurations for the most stable ion formed by each of the elements , Ba, Se, and Cl (when in stable ionic compounds). (Express your answer as a series of orbitals. For example, the electron configuration of Li would be entered in complete form as 1s2 2s1 or in condensed form as [He]2s1.) a.) Electron configuration for the most stable ion of Ba b.) Electron configuration for the most stable ion of Se c.) Electron configuration for the most stable ion of Clarrow_forwardWhich of the following atoms would be expected to form negative ions in binary ionic compounds and which would be expected to form positive ions?arrow_forward7. Which families or groups are likely to form the following ions? a. +1 b.-1 c. +2 d. -2 e. +3arrow_forward
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