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- How many grams of gaseous MgCl2 are needed to give the same electrostatic attractive energy as 0.5 mol of gaseous LiCI? The ionic radii are LI* = 76 pm, Mg*2 = 72 pm, and Cl" 181 pm. mol MgCl2 (round to third decimal place) %3DYou are spending the summer working for a chemical company. Your boss has asked you to determine where a chlorine ion of effective charge -e would situate itself near a carbon dioxide ion. The carbon dioxide ion is composed of 2 oxygen ions each with an effective charge -2e and a carbon ion with an effective charge +3e. These ions are arranged in a line with the carbon ion sandwiched midway between the two oxygen ions. The distance between each oxygen ion and the carbon ion is 3.0 x 10-11 m. Assuming that the chlorine ion is on a line that is perpendicular to the axis of the carbon dioxide ion and that the line goes through the carbon ion, what is the equilibrium distance for the chlorine ion relative to the carbon ion on this line? For simplicity, you assume that the carbon dioxide ion does not deform in the presence of the chlorine ion. Looking in your trusty physics textbook, you find the charge of the electron is 1.60 x 10-19 C.H2 (g) + Na (s) → F2 (g) + He (g) →
- Using the following data, calculate the lattice energy of calcium chloride: Ca2+(g) + 2Cl– (g) → CaCl2(s) ΔHlattice = ? Sublimation enthalpy of calcium ΔH = 177.8 kJ/mol First ionization energy of calcium ΔH = 590.2 kJ/mol Second ionization energy of calcium ΔH = 1144.2 kJ/mol First electron affinity of chlorine ΔH = –349 kJ/mol Heat of formation of CaCl2(s) ΔH = –795.4 kJ/mol Bond energy of Cl2 (see Table 2) Use Hess’s law to calculate the lattice energy of calcium chloride. set-up must show all the chemical equations and you must show how their H values add up to give your answer.Use the data given below to construct a Born-Haber cycle to determine the lattice energy of CaO. △ H°(kJ) Ca(s) → Ca(g) 193 Ca(g) → Ca+1(g) + e⁻ 590 Ca+1(g) → Ca+2(g) + e⁻ 1010 2 O(g) → O2(g) -498 O(g) + e⁻ → O-1(g) -141 O-1(g) + e⁻ → O-2(g) 878 Ca(s) + (1/2) O2(g) → CaO(s) -635The lattice energy of NaBr is –752 kJ/mol. This energy corresponds to which reaction below? Na(s) + 1/2 Br2(g) → NaBr(s) Na(g) + Br(g) → NaBr(s) Na(g) + Br(g) → NaBr(s) Na+(g) + Br–(g) → NaBr(s) Na+(aq) + Br–(aq) → NaBr(s)
- Rank the elements or compounds in the table below in decreasing order of their boiling points. That is, choose 1 next to the substance with the highest boiling point, choose 2 next to the substance with the next highest boiling point, and so on. substance A B с D chemical symbol, chemical formula or Lewis structure O=N : Cl : : Cl: - C=C CaCl, C12 Cl: : Cl : : Cl : boiling point (Choose one) ↑ ✓ (Choose one) 1 (highest) 2 3 4 (lowest) (Choose one) (Choose one) ŵ 00. 18 ArThe ionic radii of element E and a different metallic element, M, are shown in the following table: Both elements form oxides, E2O and MO. If lattice energy is defined as the energy required to separate an ionic solid into individual separate gaseous ions, would the lattice energy of MO be less than, equal to, or greater than the lattice energy of the oxide E2O? Justify your answer in terms of Coulomb's law1. Caleulate the lattice energy of LiF, given the following: Li(s) + %F:(g) → LiF(s) AH =-617 kJ AH = -520 kJ Li"(g) + e(g) → Li(g) Li(s) →Li(g) F(g) → F(g) + e (g) F:(g) →2F(g) AH = 161 kJ AH = 328 kJ AH = 154 kJ
- In the crystal structure of CsCl (cesium chloride), Cs + ions form the base of a cube while a Cl− ion occupies its center (see Figure 1). Each edge of the cube measures 0.4 nm. Each electron lacks Cs + ions (therefore, the charge of each is + e), while the Cl− ion has one in excess (therefore its charge is -e). (a) What is the magnitude of the resulting electrostatic force exerted by the eight Cs + on the Cl− ion? (b) If one of the Cs + ions is missing, the crystal is said to be imperfect. What is the magnitude of the resulting electrostatic force that the seven Cs + ions then exert on the Cl− ion?Construct a Born-Haber cycle for the formation of the hypothetical compound NaCl2, where the sodium ion has a 2+ charge (the 2nd ionization energy for sodium is given in Table 7.2 in the textbook). Part A How large would the lattice energy need to be for the formation of NaCl2 to be exothermic? Part B If we were to estimate the lattice energy of NaCl2 to be roughly equal to that of MgCl2 (2326 kJ/mol from Table 8.2 in the textbook), what value would you obtain for the standard enthalpy of formation, ΔH∘f, of NaCl2?Use the data given below to construct a Born-Haber cycle to determine the lattice energy of CaO. A H°(kJ) Ca(s) → Ca(g) 193 Ca(g) → Cat (g) + e 590 Cat (g) → Ca2+(g) + e 1010 20(g) → O2(g) -498 O(g) + e O(g) -141 O(g) + e → O2(g) 878 Ca(s) + O2(g) → CaO(s) -> -635 O-2667 kJ O-3414 kJ O +1397 kJ +3028 kJ O-2144 kJ
