Answered: A. Complete the table Bond formation… | bartleby

Chemistry In Focus

Chemistry In Focus

7th Edition

ISBN:9781337399692

Author:Tro, Nivaldo J.

Publisher:Tro, Nivaldo J.

Chapter5: Chemical Bonding

Section: Chapter Questions

Problem 44E

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A. Complete the table
Bond formation according What happened to the
e's?
Type of compound
formed
Given
to atoms
| 1, polar bond
2. nonpolar bond
3. ionic bond
B. Draw the chemical bond of the following: [Lewis Dot]
1. Phosphorous (P-Group VA) +
Chlorine (CI-Group VIIA)
2. Aluminum (Al 13) +
Sulfur (S 16)
3. Nitrogen (N-Group VA) + Flourine (F-Group VIIA)
4. Potassium (K19)
+ Oxygen (08)
5. Astatine (At-Group VIIA)
Astatine (At-Group VIIA)

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7.97 Consider the structure shown below for as well as any other important resonance structures. (a) What is the expected O—N—O bond angle in this structure? (b) The molecule contains N—O bonds of two different lengths. How many sborter N—O bonds would be present?
Which of the following statements is/are true? Correct the false statements. a. It is impossible to satisfy the octet rule for all atoms in XeF2. b. Because SF4 exists, OF4 should also exist, because oxygen is in the same family as sulfur. c. The bond in No+ should be stronger than the bond in No. d. As predicted from the two Lewis structures for ozone, one oxygen-oxygen bond is stronger than the other oxygen-oxygen bond.
What is meant by a chemical bond? Why do atoms form bonds with each other? Why do some elements exist as molecules in nature instead of as free atoms?
G. N. Lewis developed a model for chemical bonding that you have learned in this chapter. His theory was extremely successful and is used today at all levels of chemistry, from the introductory class to the research laboratory. Why was Lewis theory so successful?
There are two main types of covalent bond breakage. In ho-molytic breakage , each atom in the bond gets one of the shared electrons. In some cases, the electronega-tivity of adjacent atoms affects the bond energy. In heterolytic breakage, one atom gets both electrons and the other gets none;thus, a cation and an anion form. (a) Why is the C−C bond in H₃C−CF₃(423 kJ/mol) strongerthan that in H₃C−CH₃(376 kJ/mol)?(b) Use bond energy and any other data to calculate the heat ofreaction for the heterolytic cleavage of O₂.
Use Lewis symbols and Lewis structures to diagram the formationof PF3 from P and F atoms, showing valence-shellelectrons. (a) How many valence electrons does P have initially?(b) How many valence electrons does each F haveinitially? (c) How many valence electrons surround the P inthe PF3 molecule? (d) How many valence electrons surroundeach F in the PF3 molecule? (e) How many bonding pairs ofelectrons are in the PF3 molecule?
5)A) In which case is the bond polarity incorrect?a) δ+H–Fδ–b) δ+K–Oδ–c) δ+Mg–H δ–d) δ-Cl–Iδ+e) δ-Si–Sδ+ B) In the Lewis structure for SeF6, the central sulfur atom shares __________ electrons.a) 4b) 8c) 10d) 12e) None of the aboveC) Consider the following moleculesI. BF3II. CHBr3 (C is the central atom)III. Cl2IV. XeBr2V. PBr5VI. SCl4 Select the molecule(s) that fit the given statement. Which molecules violate the octet rule?A) I, II, IVB) I, II, III, IV, VIC) III, V, VID) I, IV, VIE) I, IV, V, VI
Using bond energies from the table below, estimate ΔH for the reaction below. The two oxygens in the reactant are each bound to carbon. One of the hydrogens is bound to carbon.HCOOH(g) ↔ H2(g) + CO2(g) Bond Energies, kJ/mol Single Bonds H C N O S F Cl Br I H 432 C 411 346 N 386 305 167 O 459 358 201 142 S 363 272 --- --- 286 F 565 485 283 190 284 155 Cl 428 327 313 218 255 249 240 Br 362 285 243 201 217 249 216 190 I 295 213 --- 201 --- 278 208 175 149 Multiple Bonds C=C 602 C=N 615 C=O 799 CºC 835 CºN 887 CºO 1072 N=N 418 N=O 607 S=O (in SO2) 532 NºN 942 O2 494 S=O (in SO3) 469
(a) Describe the molecule xenon trioxide, XeO3, usingfour possible Lewis structures, one each with zero, one,two, or three Xe¬O double bonds. (b) Do any of theseresonance structures satisfy the octet rule for every atomin the molecule? (c) Do any of the four Lewis structureshave multiple resonance structures? If so, how many resonancestructures do you find? (d) Which of the Lewisstructures in part (a) yields the most favorable formalcharges for the molecule?
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Draw the Lewis Structure of XeF4 Molecular Geometry? Ideal Bond Angles? Are there Polar Bonds Present (Indicate on Lewis do structure Is there an Overall Dipole? Octet rule violator and how?
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