Some chemical and structural features of molecules are unaccounted for by valence bond theory. Recognizing how molecular orbital theory describes these systems will lead to a better understanding of these molecules' physical properties and reactivity. 1st attempt Draw an additional resonace struture for the cation shown: ཡི "。 12D + See Periodic Table See Hint
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- Estimate ΔrH° for forming 2 mol ammonia from molecular nitrogen and molecular hydrogen. Is this reaction exothermic or endothermic?The table below contains some mean bond energy data: Bond H—H C-C N≡N Mean bond energy /kJ mol–1 436 348 944 (i) Balance the equation below for the formation of one mole of ammonia, NH3, from its elements. N2 + H2 → NH3 DH = -38 kJmol-1 (ii) Use the data in the table above to calculate the bond energy of N – H bond in NH3 in the reaction given in (i) above. Comment on why the value obtained is referred to as ‘mean bond enthalpy’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 U D chemical symbol, chemical formula or Lewis structure H H 1 | H-C C 1 I I H H H Ar H I Ag : 0: C-O-H :0: ||| H-C-C-C-H 44 boiling point ✓ (Choose one) 1 (highest) 2 W N 3 4 (lowest) (Choose one) ↑ (Choose one) (Choose one) ↑
- 22.) Estimate the enthalpy of reaction of the given reaction using the following data: C3H6 (g) + Hz (g) → C3H8 (g) Bond С-Н H-H С-С C=C Bond Energy (kJ/mol) 614 413 432 347 a.) -220 kJ/mol b.) -286 kJ/mol c.) -127 kJ/mol d.) 286 kJ/mol 23.) Calculate the standard enthalpy of combustion of aniline from the following standard enthalpies of formations. C6H5NH2 (1) + 31/4 02 (g) –→ 6 CO2 (g) + ½ N2 (g) + 7/2 H2O (1) H20 (1) CO2 (g) -393.51 C6H5NH2 (1) -285.83 A:H° (kJ/mol) +31.1 c.) -3123 kJ/mol d.) -4107 kJ/mol a.) -3393 kJ/mol b.) -3330 kJ/molIf heat of atomization of PCl5 is x kJ mol-1 then average bond dissociation enthalpy P-Cl bond isCalculate the enthalpy of formation, AHF° in kJ, of hydrogen peroxide, H2O2(g), from the relevant bond energy data. Bond Bond energy Bond Bond energy O-H 463 kJ mol-1 H-H 436 kJ mol-1 O=O 498 kJ mol-1 O-O 138 kJ mol-1 -285 +285 +130 -380 -130
- 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 C D chemical symbol, chemical formula or Lewis structure H :0: I | H H-C-C-0-C-H F₂ H :O: ||| : 0: H H 1 .. H H 1 HIC-C-N-C-H H H :NEN 0: boiling point (Choose one) ✓ (Choose one) ✓ (Choose one) (Choose one) XQ6 The table below contains some mean bond energy data: Bond H-HC-CNEN Mean bond energy /kJ mol-¹436 348 944 (i) Balance the equation below for the formation of one mole of ammonia, NH3, from its elements. -38 kJmol-¹ N₂ + H₂ (ii) Use the data in the table above to calculate the bond energy of N-H bond in NH3 in the reaction given in (i) above. Comment on why the value obtained is referred to as 'mean bond enthalpy' (Show working as this question will be assessed using grade descriptors 1, 3 & 7) Bond H-HC-HC-C Mean bond energy /kJ mol-¹436 418 348 (iii) Use the equation below and data from the table to calculate a value for the C=C bond energy in ethene. H H T T HH T T C=C + H-H→ H-C-C-H I T H H I H T H NH3 Ethene DH = AH = -136 kJ mol-¹ EthaneWhat 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 = Submit
- 1:25 ul 4G ( Gym buddies HL_DP2.pdf Page 1 of 14 Section A 1. Which equation represents the bond enthalpy for the H-Br bond in hydrogen bromide? A. HBr(g)-H(g)+Br(g) B. HBr(g)-H(g)+Br(1) C. HBr(g)-H(g)+12B12(1) D. HBr(g)-H(g)+12B12(g) 2. Which process is endothermic? A. CH4(g)+202(g)-CO2(g)+2H2O(g) B. HCI(aq)+NaOH(aq)¬NaCI(aq)+H2O(I) C. CaCO3(s)-CaO(s)+CO2(g) D. H2O(g)-H20(1) 3. Hydrazine reacts with oxygen. N2Ha(l) + O2(g) → Na(g) + 2H2O(0) AH = -623 kJ What is the standard enthalpy of formation of NaH«(i) in kJ? The standard enthalpy of formation of H2O(1) is -286 kJ. A. -623 - 286 B. -623 + 572 C.-572 + 623 D. -286 + 623 4. Which statement is correct for this reaction? FezO3 (s) + 3CO (g) - 2Fe (s) + 3CO2 (g) AH = -26.6 kJ A. 13.3 kJ are released for every mole of Fe produced. B. 26.6 kJ are absorbed for every mole of Fe produced. C. 53.2 kJ are released for every mole of Fe produced. D. 26.6 kJ are released for every mole of Fe produced. 5. Which statements are correct? 1. The…Cesium Chloride: Equilibrium Distance 1 point possible (graded) Physical constants that you may need: Elementary Charge e = 1.60218 × 10-19 C Vacuum Permittivity ε0 = 8.85419 × 10-12 C2 Jm Cesium is the most reactive metal in the periodic table. It reacts vigorously with molecular compounds such as water or chlorine gas to produce ionic compounds. The dissociation energy of gaseous cesium chloride into neutral atoms is AEd = 439 kJ/mol. CsCl (g) → Cs (g) + Cl (g) AE = AEd Potential Energy Interatomic distance r k] AEd = 439 mol Estimate the equilibrium distance re in gaseous cesium chloride. Report the value in picometers. lonization energy of cesium: 375.5 k.J mol Electron affinity of chlorine: 348.7 kJ mol pm Submit You have used 0 of 10 attempts SaveRank 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 C D H chemical symbol, chemical formula or Lewis structure H :0: 44 - C- C-H H - H 1 C I Ar H H | | - C - | 1 H H H Ag H CIO : 0: H boiling point ✓ (Choose one) 1 (highest) 2 3 4 (lowest) (Choose one) ✓ (Choose one) ✓