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Practice Exercise 1 The sulfate ion, SO,2 , can be drawn in many ways. If you minimize formal charge on the sulfur, how many S=0

Practice Exercise 1 The sulfate ion, SO,2 , can be drawn in many ways. If you minimize formal charge on the sulfur, how many S=0

Principles of Modern Chemistry
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter3: Atomic Shells And Classical Models Of Chemical Bonding
Section: Chapter Questions
Problem 94AP: The molecular ion S3N3 has the cyclic structure All SN bonds are equivalent. (a) Give six...
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Practice excercise 1

Science, Fourteenth Edition, by Theodore L. Brown, H. Eugene LeMay, Bruce E. Bursten, Catherine J. Murphy, Patrick M. Woodward, and Matthew W. Stoltzfus. Published by Pearson. Copyright © 2018 by Pearson Education, Inc. SECTION 8.6 Resonance Structures 319 electronegative than C or S. Therefore, we expect any neg- ative formal charge to reside on the N atom (guideline 2). For these two reasons, the middle Lewis structure is the dominant one for NCS. double bonds should you draw in the Lewis structure? (a) 0 (b) 1 (c) 2 (d) 3 (e) 4 Practice Exercise 2 The cyanate ion, NCO¯, has three possible Lewis structures. (a) Draw these three structures and assign formal charges in each. (b) Which Lewis structure is dominant? Practice Exercise 1 The sulfate ion, SO42 , can be drawn in many ways. If you minimize formal charge on the sulfur, how many S=0 A CLOSER LOOK Oxidation Numbers, Formal Charges, and Actual Partial Charges In Chapter 4 we introduced the rules for assigning oxidation num- bers to atoms. The concept of electronegativity is the basis of these roughly 3.0/(3.0 + 2.1) numbers. An atom's oxidation number is the charge the atom would ing pair, whereas the H atom would have 2.1/(3.0 + 2.1) = 0.41 of have if its bonds were completely ionic. That is, in determining oxi- dation number, all shared electrons are counted with the more elec- more electronegative Cl atom might therefore be expected to have = 0.59 of the electrical charge in the bond- %3D %3D the charge. Because the bond consists of two electrons, the Cl atom's share is 0 59 × 2e =1 18e. or 0 18e more than the neutral Clatom. MacBook Air DII DD 吕0 888 F11 F9 F10 F7 F8 F6 F4 F5 F3 F1 F2 & 2$ 4 5 7 2 00 #3
Transcribed Image Text:Science, Fourteenth Edition, by Theodore L. Brown, H. Eugene LeMay, Bruce E. Bursten, Catherine J. Murphy, Patrick M. Woodward, and Matthew W. Stoltzfus. Published by Pearson. Copyright © 2018 by Pearson Education, Inc. SECTION 8.6 Resonance Structures 319 electronegative than C or S. Therefore, we expect any neg- ative formal charge to reside on the N atom (guideline 2). For these two reasons, the middle Lewis structure is the dominant one for NCS. double bonds should you draw in the Lewis structure? (a) 0 (b) 1 (c) 2 (d) 3 (e) 4 Practice Exercise 2 The cyanate ion, NCO¯, has three possible Lewis structures. (a) Draw these three structures and assign formal charges in each. (b) Which Lewis structure is dominant? Practice Exercise 1 The sulfate ion, SO42 , can be drawn in many ways. If you minimize formal charge on the sulfur, how many S=0 A CLOSER LOOK Oxidation Numbers, Formal Charges, and Actual Partial Charges In Chapter 4 we introduced the rules for assigning oxidation num- bers to atoms. The concept of electronegativity is the basis of these roughly 3.0/(3.0 + 2.1) numbers. An atom's oxidation number is the charge the atom would ing pair, whereas the H atom would have 2.1/(3.0 + 2.1) = 0.41 of have if its bonds were completely ionic. That is, in determining oxi- dation number, all shared electrons are counted with the more elec- more electronegative Cl atom might therefore be expected to have = 0.59 of the electrical charge in the bond- %3D %3D the charge. Because the bond consists of two electrons, the Cl atom's share is 0 59 × 2e =1 18e. or 0 18e more than the neutral Clatom. MacBook Air DII DD 吕0 888 F11 F9 F10 F7 F8 F6 F4 F5 F3 F1 F2 & 2$ 4 5 7 2 00 #3
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