Pushing Electrons
4th Edition
ISBN: 9781133951889
Author: Weeks, Daniel P.
Publisher: Cengage Learning
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Chapter 2, Problem 6EQ
Pairs of unshared electrons can be pushed. One Lewis structure for the methoxy-methyl cation is
It is not possible to push electrons toward the other carbon, because it is not a receptor. If you tried to push electrons to this carbon, you would generate a pentavalent carbon, which is not possible.
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An incomplete Lewis structure is shown below. The structure only shows the atoms and how they are connected. The molecule has a net charge of +1.
H
H
N
H
Complete the Lewis structure giving all atoms full octets. If there is more than one way to do this, draw resonance structures showing all possibilities. If not, just
draw one Lewis structure. Be sure to write in any non-zero formal charges.
Click and drag to start drawing a structure.
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Draw Lewis structure(s) for the carbonate lon (CO₂). If there are equivalent resonance structures, draw all of them.
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Draw one structure per sketcher box, and separate added sketcher boxes with the symbol.
Do not include overall lon charges or formal charges in your drawing.
Do not draw double bonds to oxygen unless they are needed in order for the central atom to obey the octet rule.
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b Draw Lewis structure(s) for the acetaldehyde molecule (CH₂CHO). If there are equivalent resonance structures, draw all of the
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Draw one structure per sketcher box, and separate added sketcher boxes with the symbol.
Do not include overall ion charges or formal charges in your drawing.
Do not draw double bonds to oxygen unless they are needed in order for the central atom to obey the octet rule.
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What possible error(s) exist in the Lewis structure (assume we are trying to represent the best
possible Lewis structure for the NO₂S ion knowing N is the central atom in this polyatomic ion)?
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The best structure would have double bond and two lone pairs on each oxygen atom and a single bond with
three lone pairs on the sulfur.
There are no errors. This is the best possible structure.
The Lewis structure above does not minimize formal charges, thus is the not the best possible structure.
The nitrogen atom has an expanded octet, and this structure is impossible.
The Lewis structure contains the wrong number of electrons, thus this structure is impossible.
Chapter 2 Solutions
Pushing Electrons
Ch. 2 - One Lewis structure for the 2-butenyl cation is...Ch. 2 - Prob. 2EQCh. 2 - One structure for the conjugate acid of acetone...Ch. 2 - Similarly, a resonance structure for the conjugate...Ch. 2 - Prob. 5EQCh. 2 - Pairs of unshared electrons can be pushed. One...Ch. 2 - One structure for the acetoxonium ion is Clearly,...Ch. 2 - Prob. 8EQCh. 2 - There are no important resonance structures for...Ch. 2 - Prob. 10EQ
Ch. 2 - Prob. 11EQCh. 2 - Prob. 12EQCh. 2 - Prob. 13EQCh. 2 - Prob. 14EQCh. 2 - Prob. 15EQCh. 2 - Prob. 16EQCh. 2 - Prob. 17EQCh. 2 - The cyclohexane carboxylate anion has a Lewis...Ch. 2 - One Lewis structure for the enolate anion of...Ch. 2 - Prob. 20EQCh. 2 - Prob. 21EQCh. 2 - Prob. 22EQCh. 2 - Prob. 23EQCh. 2 - Prob. 24EQCh. 2 - Prob. 25EQCh. 2 - Prob. 26EQCh. 2 - Prob. 27EQCh. 2 - Prob. 28EQ
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Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- Consider the pyrosulfate ion, S2O72-. It has no sulfur–sulfur nor oxygen–oxygen bonds. (a) Write a Lewis structure for the pyrosulfate ion using only single bonds. (b) What is the formal charge on the sulfur atoms for the Lewis structure you drew in part (a)? (c) Write another Lewis structure using six bonds and two O—S bonds. (d) What is the formal charge on each atom for the structure you drew in part (c)?arrow_forwardThis Lewis structure for SF5+ is drawn incorrectly. What error was made when determining the number of valence electrons?arrow_forwardWrite all resonance structures of chlorobenzene, C6H5Cl, a molecule with the same cyclic structure as benzene. In all structures, keep the CCl bond as a single bond. Which resonance structures are the most important?arrow_forward
- For each of the following, use formal charges to choose the Lewis formula that gives the best description of the electron distribution: a ClO2F b SO2 c ClO3arrow_forwardSuccessive substitution of F atoms for H atoms in the molecule NH3 produces the molecules NH2F, NHF2, and NF3. a. Draw Lewis structures for each of the four molecules. b. Using VSEPR theory, predict the geometry of each of the four molecules. c. Specify the polarity (polar or nonpolar) for each of the four molecules.arrow_forwardDraw a Lewis structure for each of the following molecules or ions. (a) CS2 (b) BF4 (c) HNO2 (where the bonding is in the order HONO) (d) OSCl2 (where S is the central atom)arrow_forward
- A common trait of simple organic compounds is to have Lewis structures where all atoms have a formal charge of zero. Consider the following incomplete Lewis structure for an organic compound called methyl cyanoacrylate, the main ingredient in Super Glue. Draw a complete Lewis structure for methyl cyanoacrylate in which all atoms have a formal charge of zero.arrow_forwardThree resonance forms can be drawn for the molecule N2O. Which resonance form is likely to more closely resemble the structure of this molecule? (a) (b) (c)arrow_forwardSulfuric acid is the industrial chemical produced in greatest quantity worldwide. About 90 billion pounds are produced each year in the United States alone. Write the Lewis structure for sulfuric acid, H2SO4, which has two oxygen atoms and two OH groups bonded to the sulfur.arrow_forward
- 1. For which of the following species, SO32−, NO+, or NO2+, is the bonding described by two or more resonance structures? SO32− and NO+ NO+ and NO2+ NO2+ SO32−arrow_forwardDraw the Lewis structures for all seven diatomic elements (H2, N2, O2,F2, Cl2,Br2, I2) . Even though Br and I are not in the first 3 periods it is useful to consider them here.arrow_forwardDraw one BEST Lewis structure for the generic molecule XY4Z. Don't worry about resonance structures. Include all formal charges. Element X is the least electronegative. EN values: X = 3.0, Y = 3.5, Z = 4.0. For neutral atoms, element X has 8 valence electrons and element Y has 7, and Z has 6. The highest occupied principal energy level of the central atom is greater than 2. Is the measured/approximate bond angle(s) equal to, less than, or greater than the angle predicted by VSEPR theory? Briefly explain why (in ~1 sentence). Draw the best wedge-dash structure and add dipole moments (if applicable). If there is a net dipole moment, draw it. If not, write “nonpolar."arrow_forward
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