SCH4U Lee 2.3

A student claims “C = O bonds have a larger bond energy than the other types of bonds involved in this reaction, which means they require more energy input to make.” Do you agree or disagree with the students claim? Explain your response.

I need part C, please explain how to do the problem, it would help a lot!!

General Chemistry 4th Edition McQuarrie • Rock • Gallogly University Science Books presented by Macmillan Learning Use the molar bond enthalpy data in the table to estimate the Average molar bond enthalpies. (Hbond) value of AHn for the equation rxn Bond kJ . mol-1 Bond kJ . mol-1 CCI, (g) + 2 F, (g) CF,(g) + 2 Cl, (g) O-H 464 C=N 890 0-0 142 N-H 390 The bonding in the molecules is shown. С-О 351 N-N 159 to O=0 502 N=N 418 F-F CI-CI CI + + C=0 730 N=N 945 F-F C-CI С-С 347 F-F 155 C=C 615 Cl-CI 243 C=C 811 Br-Br 192 С-Н 414 Н-Н 435 С-F 439 Н-F 565 С-СІ 331 Н-СІ 431 С-Br 276 Н-Br 368 С-N 293 H-S 364 C=N 615 S-S 225 kJ

Ethane, a minority component of natural gas, burns to form carbon dioxide and water according to this reaction:2H3C−CH3(g)+7O2(g)→4CO2(g)+6H2O(g)2H3C−CH3(g)+7O2(g)→4CO2(g)+6H2O(g) Note that the average bond energy for the breaking of a bond in CO2CO2 is 799 kJ/molkJ/mol.   Use average bond energies to calculate ΔHrxnΔHrxn for this reaction.

Write the chemical equation for the formation of CHCH from the single, isolated HH and CC atoms. equation: C(g)+H(g)⟶CH(g)C(g)+H(g)⟶CH(g) Bond dissociation energies Bond Energy (kJ/molkJ/mol) H−HH−H 436 H−FH−F 569 H−CH−C 410 H−BrH−Br 366 H−IH−I 298 Using the table of bond energies, determine Δ?ΔH for the reaction. Think about the sign of the energy value in this reaction. Δ?=ΔH=

Use the bond energies provided to estimate AH°rxn for the reaction below. PCI3(g) + Cl2(g) → PCI5(1) AH°rxn = ? Bond Bond Energy_(kJ/mol). CI-CI 243 P-CI 331

Choose the best Lewis structure from those presented below. (It will help to work out the missing formal charges for the atoms in these different structures) [Image description: Lewis structure A has a N atom singly bound to two O atoms. There is one electron pair on N. One O atom has three electron pairs and the other O atom has two electron pairs and another single bond to a H atom. Lewis structure B has a O atom, 01, singly bound to a N atom and doubly bound to another O atom, O2. There is one electron pair on O1 and two electron pairs on O2. On the N atom there are two electron pairs and another single bond to a H atom. Lewis structure C has a O atom, 01, singly bound to another O atom, O2, and doubly bound to a N atom. There are is one electron pair on 01 and two electron pairs plus another singly bond to a H atom on 02. There are two electron pair on N. Lewis structure D has a N atom singly bound to a O atom, O1, and doubly bound to another O atom, O2. There are two electron…

In going from reactants to products, does the total bond energy increase, decrease, or stay about the same? Briefly explain your reasoning.

13) The average C−C bond dissociation energy (D) is 350 kJ/mol and the average C=C bond dissociation energy is 728 kJ/mol. Based on these values, which is stronger: a σ or a π bond?

Estimate the heat of the following gas-phase reaction. CH4 + 2Br2 --> CH2Br2 + 2HBr. ΔH=?  Bond Type                                            Bond Enegry(kJ/mol) C-H                                                                      413 Br-Br                                                                    193 C-Br                                                                      276 H-Br                                                                      363

Use bond energy data (based on the energy bond) to approximate the ∆H for the following  chemical reaction.  C6H12O6(s) → 2 CH3CH2OH(l) + 2 CO2(g) ∆H = ?

Consider the reaction 2H₂ + O₂ --> 2H₂O. One way to imagine this reaction (this is NOT how it really happens) is by breaking all the bonds in H₂ and O2, and then forming new bonds in the H₂O. In the three boxes below, draw out: 2H₂ + O2 (Showing all the bonds) What it would look like if all the bonds in 2H₂ + O2 broke 2H₂O (showing all the bonds)

Determine the bond energy for HCI ( in kJ/mol HCI) using he balanced cremiculequecticnand bund energles listed? also c double bond to N is 615, read numbets carefully please!!!! Determine the bund energy for UCI (in kJ/mol cl) using me balanced chemical equation and bund energies listed? 51 (My (9) +312(g)-73(g) + 3(g) =-330. KJ спод bond energy Hryn H-H bond band 432 C-1 413 C=C 839 NH 391 C=O 1010 S-1 343 6-H 02 498 N-N 160 467 N=N C-C 341 CL- 243 418 339 N-Br 243 C-O 358 Br-Br C=C C-Br 274 193 614 (-1 216 (=olin (02) 799 C=N 618

[References] The compound oxygen difluoride is quite reactive, giving oxygen and HF when treated with water: OF2(g) + H20(g)→ 0g) + 2HF(g) =-318 kJ ot Using bond energies, calculate the bond dissociation energy of the O-F bond in OF7. Average Bond Energies (kJ/mol) Single Bonds Multiple Bonds pt N-H 391 149 C=C 614 432 565 H-H 839 495 745 1072 607 418 941 pt H--F N-N 160 208 C=C N-F 272 |-Br 175 H-CI H-Br 427 363 295 N-CI N-Br C=0* C=D0 200 pt H-1 243 S-H 347 N-O 201 S-F 327 N=N N N 253 S-CI S-Br 467 413 347 305 358 C-H 146 218 C--C C--N C-O C--F C-CI C-Br O-O 891 C=N C-N S-S 266 190 203 O-F 615 0-CI 340 393 360 452 485 O-I 一 234 Si-Si 339 276 Si-H Si-C Si-O e F-F 154 253 240 259 F-CI F-Br Cl-CI C-S 237 239 218 193 Cl--Br Br--Br *C== O(in CO,) - 799 O-F bond dissociation energy: kJ mol Submit Answer Try Another Version 1 item attempt remaining nything %3D

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.

Lewis structure of H2S. Any polar bonds in molecule? Polar or non polar?

Resonance a): C1 Resonance b): C1 C2 03 C4 C5 06 C2 03 C4 C5 06 Resonance c): C1 C2 03 C4 C5 06 Resonance d): C1 C2 03 C4 C5 06 When examining the Lewis structures of organic molecules, to determine the location a reaction will occur, a chemist must identify the sites of maximum and minimum electron density, which is often emphasized by showing the formal charge on the atoms. The ability to quickly recognize the presence or absence of formal charges on atoms is an important skill. You should be able to recognize bonding around the common elements in organic chemistry, and determine the formal charge on the atom based on the number of bonds. The key elements to recognize include carbon, nitrogen, phosphorous, oxygen, sulfur and the halides. For every one of these elements there is a pattern of bonds and lone pairs which will allow rapid determination of formal charge without going through the exercise shown below in determining the formal charge on the nitrogen atom in diethyl amine:…

Calculate the enthalpy change for the reaction shown below between ammonia and phosgene to produce urea and HCI. Use the bond-dissociation energies listed in the table. Bond H-CI H-N C-CI C-N CI + 2 NH3 AHBDE (kJ/mol) 432 339 397 748 AHrxn = +444 kJ/mol AHrxn= -888 kJ/mol AHrxn= -444 kJ/mol AHrxn= +888 kJ/mol .C. HẠN-“NH, * 2 H-CI

I only need part C

14.

ELECTRONIC STRUCTURE AND CHEMICAL BONDING Predicting deviations from ideal bond angles Consider the bromate (BrO3) anion. What is the central atom? Enter its emical symbol. How many lone pairs are around the central atom? What is the ideal angle between the bromine-oxygen bonds? Compared to the ideal angle, you would expect the actual angle between the bromine-oxygen bonds to be ... 0 口。 (choose one)

H 4 H. H:Y:H H The Lewis representation above depicts a reaction between hydrogen (blue) and a main-group element from group (red). | bond(s) In this representation, each Y atom needs with atoms of H. |electron(s) to complete its octet, and gains these electrons by forming unshared electron pair(s) and |bonding electron pair(s) in the product molecule. There are The bonds in the product are|