CHEM213exam1S24_key

A mixture of Hz and Clz is stable, but a bright flash of light passing through it can cause the mixture to explode. The light causes Cl2 molecules to split into Cl atoms, which are highly reactive. What wavelength of light, in nm, is necessary to cause the Cl2 molecules to split? The bond energy of Clz is 242.6 kJ/mole. Part 1 Your answer is correct. Calculate the energy, in J, needed to break 1 Cl-CI bond if it takes 242.6 kJ to break a mole of Cl-CI bonds. Enter your response in scientific notation as 1.00e-10, for example. 40.3e-20 eTextbook and Media Hint Attempts: 2 of 15 used Part 2 Your answer is incorrect. What frequency of light is necessary to cause the Clz molecules to split? Enter your response in scientific notation as 1.00e-10, for example.

2. The Lewis structure for the acetate ion [C₂H3O2]¹ is given below: le a. Read section 1.9. What is the geometry (shape) around each of the carbon atoms in the acetate ion - tetrahedral, trigonal planar or linear? b. Each of the oxygen atoms in the acetate ion have an octet. Draw all lone pairs of electrons in the acetate ion given above. c. Read section 1.7. Use electron pushing to generate a resonance structure of the acetate Lewis structure given above.

b. There is one additional resonance structure. NH₂ c. There is a total of five resonance structures (including the original structure). : OH

Consider the molecules — BrF5. A. Draw the best Lewis structure for this molecule. Label any atoms with nonzero formal charge. B. Label each bond angle. As part of your answer be sure to include if it is more or less than the ideal bond angle.  C. What is the electron geometry around the bromine atom? D. Are the bonds in the molecule polar? E. Is the overall molecule polar? — CH2 F2 . A. Draw the best Lewis structure for this molecule. B. Label each bond angle. Answers for A-D here: C. Redraw the shape of the molecule. Draw all dipoles. D. Is the overall molecule polar? — Consider the molecule CH2 CF2 . A. Draw the best Lewis structure for this molecule. B. Label each bond angle. C. Redraw the shape of the molecule (according to the exacting specifications of your instructor). Draw all dipoles. D. Is the overall molecule polar?

APTER 8 CHAPTER ASSESSMENT Covalent Bonding Reviewing Vocabulary Match the definition in Column A with the term in Column B. Column A Column B 1. The tendency of an atom in a compound to attract electrons I 2. A kind of bond in which there is unequal sharing of electrons a. structural formula b. molecule 3. Any bond in which there is electron sharing c. VSEPR model 4. The particle formed when two or more atoms bond covalently d. coordinate covalent bond 5. Reactions that occur when more energy is released forming new e. hybridization bonds than is required to break bonds in the initial reactants f. oxyacid 6. A kind of bond in which electrons are shared in an area centered between the two atoms g. electronegativity 7. A kind of bond formed by overlap of parallel orbitals h. sigma bond 8. Any acidic compound that contains oxygen i. polar covalent j. pi bond 9. A model that shows how the atoms are arranged in a molecule k. covalent bond m. 10. Reactions that occur when more energy is…

2. Use the table below to estimate AH for the reaction NO + O3 → NO2 + O2. Does this reaction consume or produce heat? Single Bond Energies (kJ/mol of bonds) н сN oS F C Br I Н 436 C 413 346 N 391 305 163 O 463 358 201 146 S 347 272 226 - F 565 485 283 190 284 155 Cl 432 339 192 218 255 253 242 Br 366 285 201 217 249 216 193 - I 299 213 201 278 208 175 151 - - Multiple Bond Energies (kJ/mol of bonds) C=C 602 C=N 615 C=O 799 C=C 835 CEN 887 C=O 1072 N=N 418 N=O 607 N=N 945 O=O 498

Draw the Lewis structure for CO. A. Calculate the formal charge on each atom in CO. B. Draw the dipole for CO. C. Calculate the oxidation numbers for the carbon and oxygen atoms in CO. D. Formal charges, dipoles, and oxidation numbers are different ways of understanding the charges on covalently-bonded atoms. They tend to agree or be similar. At least in some ways, they disagree for CO. Formal charge guidelines assume that all bonding electrons are shared evenly between the two bonded atoms. Oxidation number guidelines assume that the more electronegative atom in the bond gets all of the electrons. Dipole theory assumes that the bonded electrons are associated more with the more electronegative atom. Now that you understand the basis for the oxidation number guidelines, determine the oxidation number for each carbon in propane assuming that the more electronegative atom gets all of the bonded electrons. You will need to draw the Lewis structure of propane for your answer.

How much energy (in kJ) is required to separate (break) one mole of H-H bonds? Bond Length (pm) Energy (kJ/mol) H-H 74 436 H-C 106.8 413 H-N 101.5 391 H-O 97.5 467 O A) +436 kJ B) -436 kJ O C) +74 kJ D) -74 kJ E) 106.8 kJ

Given the table of bond energies, which of the following is an accurate comparison of the energetics of breaking bonds? H-H 436 H-F 569 H-CI 432 H-Br 366 H-I 298 C-H 410 C-c 350 CIN 300 C10 350 C-F 450 CICI 330 C-Br 270 CII 240 Table of Average Bond Energies (kJ/mole) N-H 390 NIN 240 N-F 270 N CI 200 N-Br 240 N1O 200 O-H 460 O O 142 O -F 180 O -CI 200 220 ✓ F-F 157 F-Cl 251 F-Br 234 Cl-Cl Cl-Br 243 219 Br-Br 194 1-1 153 179 1-Br I-CI 208 280 1-F C=C C=0 CIN C=S 010 498 N=N 418 N=0 607 C C C=O C=N NEN 611 745 615 477 835 1077 891 941 It is harder to break a C-C single bond than a C=C double bond because breaking the single bond releases more energy. It is harder to break a C-C double bond than a C-C single bond because breaking the double bond requires more energy. It is harder to break a C-C single bond than a C=C double bond because breaking the single bond requires more energy. It is harder to break a C=C double bond than a C-C single bond because breaking the double bond releases…

Р ed Lewis structure H-CC-H [H_H_O_H]* Η N_0_a: Is the proposed Lewis structure reasonable? Yes. No, it has the wrong number of valence electrons. The correct number is: No, it has the right number of valence electrons but doesn't satisfy the octet rule. The symbols of the problem atoms are:* Yes. No, it has the wrong number of valence electrons. The correct number is: No, it has the right number of valence electrons but doesn't satisfy the octet rule. The symbols of the problem atoms are:* Yes. No, it has the wrong number of valence electrons. The correct number is: No, it has the right number of valence electrons but doesn't satisfy the octet rule. The symbols of the problem atoms are:*

Fill in the table. Central atom is listed first. A. Write the number of valence electrons below the formulaB. Draw the Lewis structureC & D. Write the Electron Group Geometry and Molecular Shape NamesE. Write the bond angleF. Write the molecular polarity. "P" for polar and "NP" for nonpolar. SpeciesValenceElectrons(1 pt.) LewisStructure(2 pt.) Electron PairGeometryName(1 pt.) Molecular ShapeName (1 pts.) BondAngle (1 pt.) Molecular Polarity(1 pt.) PO43-           NOBr           Upload

Given the table of bond energies, which of the following is an accurate comparison of the energetics of breaking bonds? H-H 436 H-F 569 H-CI 432 H-Br 366 H-I 298 C-H 410 C-C 350 CIN 300 C10 350 C-F 450 C-Cl 330 C-Br 270 CII 240 Table of Average Bond Energies (kJ/mole) N-H 390 NIN 240 N-F 270 N_CI 200 N-Br 240 N1O 200 0 H 010 0-F O -CI O -1 460 142 180 200 220 Y F-F 157 F-Cl 251 F-Br 234 CI-CI 243 Cl-Br 219 Br-Br 1-1 1-Br I-CI I-F 194 153 179 208 280 C=C C=0 C=N C=S 010 N=N N=O C C C=O CEN NEN 611 745 615 477 498 418 607 835 1077 891 941 It is harder to break a C-C single bond than a C=C double bond because breaking the single bond releases more energy. It is harder to break a C-C double bond than a C-C single bond because breaking the double bond requires more energy. It is harder to break a C-C single bond than a C=C double bond because breaking the single bond requires more energy. It is harder to break a C=C double bond than a C-C single bond because breaking the double bond…

1. How can you tell if a compound is covalent? 2. What distinguishes a covalent bond from an ionic bond? 3. How do you know how many valence electrons an atom has? 4. What is electronegativity? Is electronegativity a property of atoms or bonds? 5. What is polarity? Is polarity a property of atoms or bonds? 6. Describe in detail the N-F bond in terms of the relevant electronegativities and polarities. 7. What does VSEPR stand for and how does it allow one to predict the shapes of covalent molecules?

2. Draw the lewis structures for both resonance structures of the OCBr+ ion and select the statement that is true a. The molecule sometimes looks like one resonances structure, and at other times it looks like the other resonance structure b. In one resonance structure, the carbon is in the center, and in the other one, the oxygen is in the center c. The bond between carbon and oxygen would best be described as 2.5 bonds (halfway between a double and a triple bond) d. In one resonance structure the positive charge is on the bromine, and in the other, it is on the carbon.

4. CHCl3 a. Lewis structure Electronic geometry_ C. d. Molecular shape_ e. Bond angle? b. Draw the different bonds and label their polarity. inorpelt b Soigns broff 02 8

Draw the Lewis structure for the molecule, AX3, where A has 5 valence electrons and X (which is more electronegative than A) has 7 valence electrons. Which choice correctly describes the Lewis structure? a) the structure has three A—X single bonds and one lone pair of electrons on A b) the structure has two A—X single bonds, one A=X double bond, and no lone pairs of electrons on A c) the structure has two A—X single bonds, one A=X double bond, and one lone pair of electrons on A d) the structure has three A—X single bonds and two lone pairs of electrons on A e) the structure has three A—X single bonds and no lone pairs of electrons on A