Question 5 (Problem 2.16) Calculate the coulombic foree of attraction between Ca and O in CaO, which has the NaCl- type structure. Given a 0 238 nm
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- Compare the magnitude of the lattice energy for each of the following two ion pairs. (a) Ni²+ and O²- separated by a distance of 220 pm (b) Mn²+ and O²- separated by a distance of 431 pmCompare the magnitude of the lattice energy for each of the following two ion pairs. (a) Ni²+ and O²- separated by a distance of 394 pm (b) K+ and Br¯ separated by a distance of 358 pmOnl X S Write electro X 6 uzdLQYhAS X G Predict the t X X Periodic Tab X how.com/ilrn/takeAssignment/takeCovalentActivity.do?locator=Dassignment-take Consider the following: Na(s) + Br2 (g) → NaBr(s) AH = -367 kJ/mol %3D Lattice energy of NaBr(s) Ionization energy of Na(g) Bond energy of Br2 (g) Electron affinity of Br(g) -742 kJ/mol 495KJ/mol 193 kJ/mol -325 kJ/mol Use these data to determine the heat of sublimation of Na(s). AHsub kJ
- (a) Is lattice energy usually endothermic or exothermic?(b) Write the chemical equation that represents the processof lattice energy for the case of NaCl. (c) Would you expectsalts like NaCl, which have singly charged ions, to havelarger or smaller lattice energies compared to salts like CaOwhich are composed of doubly-charged ions?3. Determine the net electrostatic energy in kJ/mol for solid state (a) cuprous iodide, (b) zinc fluoride, and (c) strontium oxide.Ammonium chloride, NH4Cl, is a very soluble salt in water.(a) Draw the Lewis structures of the ammonium and chlorideions. (b) Is there an N—Cl bond in solid ammonium chloride?(c) If you dissolve 14 g of ammonium chloride in 500.0 mLof water, what is the molar concentration of the solution?(d) How many grams of silver nitrate do you need to add tothe solution in part (c) to precipitate all of the chloride as silverchloride?
- Use principles of atomic structure to answer each of the following: (1] (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 K20 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 lonization Energy (kJ/mol) Second lonization 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.NaCl and KF have the same crystal structure. The only differencebetween the two is the distance that separates cationsand anions. (a) The lattice energies of NaCl and KF are givenin Table 8.1. Based on the lattice energies, would you expectthe Na¬Cl or the K¬F distance to be longer? (b) Use theionic radii given in Figure 7.8 to estimate the Na¬Cl andK¬F distances.Calculate the lattice enthalpy for RbC1. You will need the following information: Species AfH°, kJ/mol Rb(g) RbCl(s) Cl(g) 80.9 - 435.4 121.3 Enthalpy of ionization for Rb(g) is 403.0 kJ/mol; electron attachment enthalpy for Cl(g) is −349.0 kJ/mol. Lattice enthalpy = kJ/mol
- Calculate the lattice energy of RbCl using the following data: AH (k) Rb(3) Rb(g) Chig) CI(g) + e Rb(s) + ¾Cl(g} Rb(g) Rb"(g) + e¯ 86 409 2CI(g) CF(g) RÜCI(s) 242 -355 435Which of the following is the correct representation of partial charges at the indicated atoms? a. I = δ+; II = δ–; III = δ– b. I = δ–; II = δ–; III = δ– c. I = δ+; II = δ+; III = δ+ d. I = δ–; II = δ+; III = δ– e. I = δ+; II = δ–; III = δ+b)) Calculate the electronegativity of Si (rcov = 1.175 Ao). using the equation. X = 0.359 (Zeff ÷ r2cov) + 0.7441