Concept explainers
Using data from Table 8.5, calculate the magnitude of the partial charges in HI.
0.15
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Chemistry
- 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?arrow_forwardCalculate H for the following process: K(g)+Br(g)KBr(s) The lattice energy of KBr is 689 kJ/mol, and the ionization energy of K is 419 kJ/mol. The electron affinity of Br is given in Table 8.4. See Problem 8.119.arrow_forwardCompare the properties of an ionic material such as sodium chloride with a room-temperature ionic liquid. Explain this difference.arrow_forward
- 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?arrow_forwardExplain the decomposition of nitroglycerin in terms of relative bond enthalpies.arrow_forwardWhy do nonmetals tend to form anions rather than cations?arrow_forward
- Describe the formation of a sodium chloride crystal from atoms.arrow_forwardUsing the standard enthalpy of formation data in Appendix G. determine which bond is stronger: the PCl bond in PCl3(g) or in PCl5(g)?arrow_forwardElement First Ionization Energy (kJImol) Second Ionization Energy (kiImol) I K 419 3050 Ca 590 1140 75. Use principles of atomic structure to answer each of the following: (a) The radius of the Ca atom is 197 pm; the radius of the Ca2+ ion is 99 pm. Account for the difference. (b) The lattice energy of CaO(s) is 3460 kJ/mol; the lattice energy of K2O is 2240 kJ/mol. Account for the difference. (c) Given these ionization values, explain the difference between Ca and K with regard to their first and second ionization energies. Element First Ionization Energy (kJ/mol) Second Ionization Energy (kJ/mol) K 419 3050 Ca 590 1140 (d) The first ionization energy of Mg is 738 kJ/mol and that of Al is 578 kJ/mol. Account for this difference.arrow_forward
- Write the Lewis structure for each of the following. You may wish to review the chapter on chemical bonding and molecular geometry. (a) PH3. (b) PH4+. (c) P2H4. (d) PO43-. (e) PF5arrow_forwardFor each of the following, write an equation that corresponds to the energy given. a. lattice energy of NaCl b. lattice energy of NH4Br c. lattice energy of MgS d. O9O double bond energy beginning with O2(g) as a reactantarrow_forward9. Use the following data to calculate the lattice energy of Cao. The enthalpy of formation of Cao is –636 kj/mol. The enthalpy of sublimation of Ca is +192 kj/mol, the first ionization energy of Ca is +590 kj/mol, and the second ionization energy of Ca is +1145 kj/mol. The enthalpy of dissociation of 02 is +494 kj/mol of 02 molecules, the first electron affinity of O is -141 kj/mol of 0 atoms, and the second electron affinity of 0 is +845 kj/mol of 0¯ ions.arrow_forward
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