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- Construct a Born–Haber cycle for the formation of the hypotheticalcompound NaCl2, where the sodium ion has a 2+charge (the second ionization energy for sodium is given inTable 7.2). (a) How large would the lattice energy need to befor the formation of NaCl2 to be exothermic? (b) If we wereto estimate the lattice energy of NaCl2 to be roughly equalto that of MgCl2 (2326 kJ/mol from Table 8.1), what valuewould you obtain for the standard enthalpy of formation,ΔHf°, of NaCl2?The strength of a covalent bond depends upon the size of the atoms and the bond order. In general short bonds are strong bonds. For each pair of covalently bonded atoms, choose the one expected to have the higher bond energy. (A) N=N (B) N-N (C) CEC (D) C=C Use the References to access important values if needed for this question. (A,B) (C,D)Do you expect the constant ,1 in (9.30) describing the susceptibility of the covalent bond to be positive or negative? Why?
- (ii) Construct and label a Born-Haber cycle for strontium difluoride, SrF2. Calculate the lattice energy of SrF2 using the following data: First electron affinity of fluoride =–328.0 kJ mol"1 First ionization energy of strontium = 549.0 kJ mol" Second ionization energy of strontium = 1064.0 kJ mol"! Enthalpy of atomization of fluoride = 75.3 kJ mol" Enthalpy of atomization of strontium = 164.0 kJ mol"! Enthalpy of formation of strontium difluoride = -1224.4 kJ mol"!X Incorrect. The net potential energy between two adjacent ions, E, may be represented by EN = = A + B ph Where A, B, and n are constants whose values depend on the particular ionic system. Calculate the bonding energy Eo in terms of the parameters A, B, and n using the following procedure: (1) Differentiate EN with respect to r, and then set the resulting expression equal to zero, since the curve of EN versus r is a minimum at Eo. (2) Solve for r in terms of A, B, and n, which yields ro, the equilibrium interionic spacing. (3) Determine the expression for Eo by substitution of ro into the above equation for EN. Which of the following equations represents the expression for Eo? Eo O Eo O Eo Eo O Eo = = = = = I I B 2/(2-n) A (4) nB (4) 1/(1-n) B 1/(1-n) A (A)" nB n/(2-n) A B 1/(1-n) (B)¹ nA + + + + + A n/(2-n) (4)" A (4)" nB B A n/(1-n) (4)" <| n/(1-n) A nB 5) ² B 1/(2-n) B B\n/(1-n) (B)" nAThe strength of a covalent bond depends upon the size of the atoms and the bond order. In general short bonds are strong bonds. For each pair of covalently bonded atoms, choose the one expected to have the higher bond energy. (A) C-C (B) CEC (C) C=O (D) C-O Use the References to access important values if needed for this question. (A,B) (C,D)
- Use the References to access important values if needed for this question. The strength of a covalent bond depends upon the size of the atoms and the bond order. In general short bonds are strong bonds. For each pair of covalently bonded atoms, choose the one expected to have the higher bond energy. (A) C=N (В) С-N (А,B) (С) С-0 (D) C-O (C,D)(a) Imagine that a Born-Haber cycle is being constructed by a colleague, to determine the lattice energy of a hypothetical magnesium halide salt, where X is the halide ion. The colleague makes the following list: First and second ionisations of Mg; 737 and 1451 Sublimation energy of Mg; 147 Electron affinity of X; 200 Atomisation enthalpy of X₂; 400 Enthalpy of formation of MgX₂; -450 2+ 2e+ Mg(+2X (8) b 2+ 2e + Mg( + X2 (8) a + Mg(g) + X₂ (8) 1451 Mg(g) + X₂ (8) Mg(s) + X2 (8) f 147 2+ Mg(g) +2X(g) MgX2 (s) d Sadly the colleague becomes discouraged and leaves the document incomplete, simply drawing boxes around unknown quantities. Complete the calculation by writing down the boxed quantities a-f on your answer paper. You may assume that the units are kJ mol-¹.AH (kJ/mole) -306.4 species PC13 (g) PCls (g) P (g) Cl (g) 1. -398.9 +314.5 +121.4 Calculate the P-Cl bond energy in PCI3 and in PCI..
- Which of the following compounds requires the most energy to convert one mole of the solid into separateions?(a) MgO(b) SrO(c) KF(d) CsF(e) MgF2The iodine monobromide molecule, IBr, has a bond lengthof 2.49 Å and a dipole moment of 1.21 D. (a) Which atom ofthe molecule is expected to have a negative charge? (b) Calculatethe effective charges on the I and Br atoms in IBr inunits of the electronic charge, e.For which of the following substances is the least energy required to convert one mole of the solid into separate ions? (a) MgO (b) SrO (c) KF (d) CsF (e) MgF2