1. Three iodine (1) atoms can form both a cation, 13+¹ and an anion, 13¹. Predict the molecular shape of both ions. Hint: "All work" should include valence electron counts and a Lewis Dot structure.

1. Three iodine (1) atoms can form both a cation, 13+¹ and an anion, 13¹. Predict the molecular shape of both ions. Hint: "All work" should include valence electron counts and a Lewis Dot structure.

Pushing Electrons

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Chapter2: Resonance Structures

Section: Chapter Questions

Problem 18EQ: The cyclohexane carboxylate anion has a Lewis structure Pushing a pair of unshared electrons away...

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The cyclohexane carboxylate anion has a Lewis structure Pushing a pair of unshared electrons away from the negatively charged oxygen atom and, at the same time, pushing a pair of pi electrons toward the other oxygen will generate a second resonance structure. Thus,
12ab
Acetylene 1C2H22 and nitrogen 1N22 both contain a triplebond, but they differ greatly in their chemical properties.(a) Write the Lewis structures for the two substances. (b) Byreferring to Appendix C, look up the enthalpies of formationof acetylene and nitrogen. Which compound is more stable?(c) Write balanced chemical equations for the completeoxidation of N2 to form N2O51g2 and of acetylene to formCO21g2 and H2O1g2. (d) Calculate the enthalpy of oxidationper mole for N2 and for C2H2 (the enthalpy of formationof N2O51g2 is 11.30 kJ>mol). (e) Both N2 and C2H2 possesstriple bonds with quite high bond enthalpies (Table 8.3).Calculate the enthalpy of hydrogenation per mole for bothcompounds: acetylene plus H2 to make methane, CH4;nitrogen plus H2 to make ammonia, NH3.
Dichlorine heptaoxide, Cl₂O₇, can be viewed as two ClO₄ groups sharing an O atom. Draw a Lewis structure for Cl₂O₇ with the lowest formal charges, and predict any deviation fromthe ideal for the Cl-O-Cl bond angle.
“Inert” xenon actually forms several compounds, especially with the highly electronegative elements oxygen and fluorine. The simple fluorides XeF2, XeF4, and XeF6 are all formed by direct reaction of the elements. As you might expect from the size of the xenon atom, the Xe¬F bond is not a strong one. Calculate the Xe¬F bond energy in XeF6, given that the enthalpy of formation is -402 kJ/mol.
Consider peroxynitrite (chemical formula: ONOO−), a structural isomer of the nitrate anion. It is generated in the cell when nitric oxide (NO) reacts with the superoxide radical anion (O2-.). Peroxynitrite is a potent oxidant and nitrating agent and can lead to DNA and protein damage (this is the complete question) Draw the correct Lewis structure for peroxynitrite and indicate approximate bond angles. Tell how many molecular degrees of freedom of motion are present in peroxynitrite and what motions they correspond to.
Propylene, C3H6, is a gas that is used to form the importantpolymer called polypropylene. Its Lewis structure is given. (a) What is the total number of valence electrons in the propylenemolecule? (b) How many valence electrons are usedto make σ bonds in the molecule? (c) How many valenceelectrons are used to make π bonds in the molecule? (d) Howmany valence electrons remain in nonbonding pairs in themolecule? (e) What is the hybridization at each carbon atomin the molecule?
The carbonate anion, CO32- , is a resonance hybrid. Draw all of the important resonance structures for this molecule. If an atom has a nonzero formal charge, be sure the formal charge is shown clearly in the structure. Use the resonance structures to calculate the average formal charge on each O atom (which are all equivalent in the "true" structure). [Note: all of the important contributing resonance structures have octets around each atom that desires an octet.]
Some chemists believe that satisfaction of the octet ruleshould be the top criterion for choosing the dominant Lewisstructure of a molecule or ion. Other chemists believe thatachieving the best formal charges should be the top criterion.Consider the dihydrogen phosphate ion, H2PO4-, inwhich the H atoms are bonded to O atoms. (a) What is thepredicted dominant Lewis structure if satisfying the octetrule is the top criterion? (b) What is the predicted dominantLewis structure if achieving the best formal charges is the topcriterion?
Which substance in each of the following pairs would you expect to have the higher boiling point? (a) Ne or Xe, (b) CO2 or CS2, (c) CH4 or Cl2, (d) F2 or LiF, (e) NH3 or PH3 (a) Ne; (b) CS2; (c) CH4; (d) F2 ; (e) NH3 (a) Xe; (b) CS2; (c) Cl2; (d) LiF ; (e) PH3 O (a) Xe; (b) CS2; (c) Cl2; (d) LiF ; (e) NH3 (a) Xe; (b) CS2; (c) Cl2; (d) F2 ; (e) NH3 (a) Xe; (b) C02; (c) CH4 ; (d) LiF ; (e) PH3
Write a Lewis structure for the NO3 - ion. Include resonance structures?
Draw the Lewis structures for each of the following ionsor molecules. Identify those in which the octet rule is notobeyed; state which atom in each compound does not followthe octet rule; and state, for those atoms, how manyelectrons surround these atoms: (a) PH3, (b) AlH3, (c) N3-,(d) CH2Cl2, (e) SnF62-.

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