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- The bond dissociation energy, in kJ, to break 1 hydrogen-carbon bond(s) in 1 mol of HCECH molecules is Single Bond H CNO с H 432 411 386 459 C=C Multiple CC Bonds CN **All values in kJ/mol** 346 305 167 358 201 Question 45 of 47 C=N 615 O=O C=N O 142 602 C=O 799 835 C=O 1072 494 887 N=N 942Find the valence or factor of the following compounds which will be used as "n" to compute for their equivalent weights. i. (NH4)2SO4 ii. H3PO4 iii. ZnSO4 iv. FeCl3 v. Al(OH)37.13 Figure 7-2 depicts the interactions of an ion with its first nearest neighbors, second nearest neighbors, and third nearest neighbors in a lattice, (a) Would the interactions with the fourth nearest neighbors be attractive or repulsive? (b) Based on Coulomb's law, how would the relative sizes of the terms compare if the potential energy were expressed as V=V1st+V2nd+V3rd+V4th ?
- Estimate ΔrH° for forming 2 mol ammonia from molecular nitrogen and molecular hydrogen. Is this reaction exothermic or endothermic?Question: Assuming the distance d is the same for all of these, rank them in order of increasing electrostatic potential energy. Hint: -1 Answer only: ||| < | < || I +1 -3 II -1 -2 III +1 at's cThe bond dissociation energy, in kJ, to break 3 bond(s) in 1 mole of CH4 molecules is Single H Bond 432 411 386 459 O NO I H с Multiple Bonds C=C C=C CN **All values in kJ/mol** 346 305 167 358 201 C=N 615 0=0 C=N 887 N=N O 142 602 C=O 799 835 C=O 1072. 494 942
- Using Lewis symbols and Lewis structures, diagram the formationof SiCl4 from Si and Cl atoms, showing valence-shellelectrons. (a) How many valence electrons does Si have initially?(b) How many valence electrons does each Cl haveinitially? (c) How many valence electrons surround the Siin the SiCl4 molecule? (d) How many valence electrons surroundeach Cl in the SiCl4 molecule? (e) How many bondingpairs of electrons are in the SiCl4 molecule?What are the formal charges on the sulfur (S), carbon (C), and nitrogen (N) atoms, respectively, in the "best" or most realistic Lewis structure shown below? The possible Lewis structures for the thiocyanate ion, SCN, are S=c=N] $-c=Ñ]' [:s=C-N;T Structure A Structure B Structure C Express your answers as integers separated by commas. • View Available Hint(s) formal charge on sulfur (S), carbon (C) and nitrogen (N) atoms = SubmitWhat is the electrostatic potential energy (in joules) betweentwo protons that are separated by 62 pm?
- The bond dissociation energy, in kJ, to break 1 bond in 1 mole of CO2 molecules is Single H Bond 432 411 386 459 HUN O C C=C C=C Multiple Bonds CN 346 305 167 358 602 201 O 142 C=O 799 CEO 1072 835 C=N 615 0=0 494 C=N 887 NEN 942 **All values in kJ/mol**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?18. When one electron is added to an oxygen molecule, a superoxide ion (O₂) is formed. The addition of two elec- trons gives a peroxide ion (O2). Removal of an electron from O₂ leads to O₂. 2 (a) Construct the correlation diagram for O₂. (b) Give the valence electron configuration for each of the following species: Oz, O₂, O₂, O3-. 2 (c) Give the bond order of each species. (d) Predict which species are paramagnetic. (e) Predict the order of increasing bond dissociation energy among the species.