The drawing shows three point charges arranged in three different ways. The charges are +q, -q, and -q; each has the same magnitude, with one positive and the other two negative. In each of the arrangements the distance d is the same. Rank the arrangements in descending order (largest first) according to the magnitude of the net electrostatic force that acts on the positive charge. +9 O C, B, A A, B, C OB, A, C OC, A, B A d -9 -9 d +q B d 9 d +q 90° d C -9

The drawing shows three point charges arranged in three different ways. The charges are +q, -q, and -q; each has the same magnitude, with one positive and the other two negative. In each of the arrangements the distance d is the same. Rank the arrangements in descending order (largest first) according to the magnitude of the net electrostatic force that acts on the positive charge. +9 O C, B, A A, B, C OB, A, C OC, A, B A d -9 -9 d +q B d 9 d +q 90° d C -9

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter8: Bonding: General Concepts

Section: Chapter Questions

Problem 3ALQ

See similar textbooks

Similar questions

Think of forming an ionic compound as three steps (this is a simplification, as with all models): (I) removing an electron from the metal; (2) adding an electron to the nonmetal; and (3) allowing the metal cation and nonmetal anion to come together. a. What is the sign of the energy change for each of these three processes? b. In general, what is the sign of the sum of the first two processes? Use examples to support your answer. c. What must be the sign of the sum of the three process d. Given your answer to part c, why do ionic bonds occur? e. Given your above explanations, why is NaCl stable but not Na2Cl? NaCl2? What about MgO compared to MgO2? Mg2O?
Arrange the following series of compounds in order of increasing lattice energies. (a) NaBr, NaCl, KBr (b) MgO, CaO, CaCl2 (c) LiF, BeF2, BeO
Define the term lattice energy. Why, energetically, do ionic compounds form? Fig. 3-8 illustrates the energy changes involved in the formation of MgO(s) and NaF(s). Why is the lattice energy of MgO(s) so different from that of NaF(s)? The magnesium oxide is composed of Mg2+ and O2 ions. Energetically, why does Mg2+O2 form and not Mg+O? Why doesnt Mg3+O3 form?
Compare the properties of an ionic material such as sodium chloride with a room-temperature ionic liquid. Explain this difference.
hat is the enthalpy change for a process? Is enthalpy a state function? In what experimental apparatus are enthalpy changes measured?
n your own words, what is meant by the term electronegativity? What are the trends across and down the periodic table for electronegativity? Explain them, and describe how they are consistent with trends of ionization energy and atomic radii.
The lattice energy of KF is 794 kJ/mol, and the interionic distance is 269 pm. The Na—F distance in NaF, which has the same structure as KF, is 231 pm. Which of the following values is the closest approximation of the lattice energy of NaF: 682 kJ/mol, 794 kJ/mol, 924 kJ/mol, 1588 kJ/mol, or 3175 kJ/mol? Explain your answer.
Which of the following atoms would be expected to form negative ions in binary ionic compounds and which would be expected to form positive ions: P, I, Mg, Cl, In, Cs, O, Pb, Co?
For each of the answers in Problem 59, state whether the species is polar or nonpolar.