Homework Help is Here – Start Your Trial Now!
Science
Chemistry
formal charges: all of the atoms are 0 formal charges: sulfur and two oxygen atoms are 0, the other two oxygens are each -1 formal charges: sulfur is 0 and the oxygen atoms are each -0.75 because 4*(-0.75)=-3 bond angle: all are 90 degrees because there are 4 groups around sulfur bond angle: all are 109.5 degrees because there are 4 groups around sulfur bond angle: both 90 and 120 degrees because there are 5 bonds to sulfur geometry: tetrahedral geometry: square planar geometry: see saw O SO bond order: the single bonds are 1 and the double bonds are 2 SO bond order: all four bonds are 1.5 O SO bond order: half of the time cach bond is one and the other half of the time cach bond is

formal charges: all of the atoms are 0 formal charges: sulfur and two oxygen atoms are 0, the other two oxygens are each -1 formal charges: sulfur is 0 and the oxygen atoms are each -0.75 because 4*(-0.75)=-3 bond angle: all are 90 degrees because there are 4 groups around sulfur bond angle: all are 109.5 degrees because there are 4 groups around sulfur bond angle: both 90 and 120 degrees because there are 5 bonds to sulfur geometry: tetrahedral geometry: square planar geometry: see saw O SO bond order: the single bonds are 1 and the double bonds are 2 SO bond order: all four bonds are 1.5 O SO bond order: half of the time cach bond is one and the other half of the time cach bond is

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
See similar textbooks
icon
Related questions
Question
The best Lewis structure for sulfate is shown here. There are several other equivalent resonance forms of this Lewis structure. Choose from the following all the correct details of sulfate.
**Educational Content: Understanding the Lewis Structure for Sulfate** The best Lewis structure for sulfate is illustrated. Several equivalent resonance forms exist for this structure. From the options below, identify all the correct details of the sulfate ion. **Diagram Explanation:** - The diagram shows a central sulfur (S) atom bonded to four oxygen (O) atoms. - The structure is enclosed in brackets with a -2 charge indicating it is a sulfate ion. - Each oxygen is connected to the sulfur by a single bond, and each oxygen atom has three lone pairs of electrons, meeting the octet rule. **Options for Correct Details:** - [ ] **Formal charges: all of the atoms are 0** - [ ] **Formal charges: sulfur and two oxygen atoms are 0, the other two oxygens are each -1** - [ ] **Formal charges: sulfur is 0 and the oxygen atoms are each -0.75 because 4*(-0.75)=-3** - [ ] **Bond angle: all are 90 degrees because there are 4 groups around sulfur** - [ ] **Bond angle: all are ~109.5 degrees because there are 4 groups around sulfur** - [ ] **Bond angle: both 90 and 120 degrees because there are 5 bonds to sulfur** Explore the characteristics of sulfate further and verify your understanding of molecular geometry and formal charges.
Transcribed Image Text:**Educational Content: Understanding the Lewis Structure for Sulfate** The best Lewis structure for sulfate is illustrated. Several equivalent resonance forms exist for this structure. From the options below, identify all the correct details of the sulfate ion. **Diagram Explanation:** - The diagram shows a central sulfur (S) atom bonded to four oxygen (O) atoms. - The structure is enclosed in brackets with a -2 charge indicating it is a sulfate ion. - Each oxygen is connected to the sulfur by a single bond, and each oxygen atom has three lone pairs of electrons, meeting the octet rule. **Options for Correct Details:** - [ ] **Formal charges: all of the atoms are 0** - [ ] **Formal charges: sulfur and two oxygen atoms are 0, the other two oxygens are each -1** - [ ] **Formal charges: sulfur is 0 and the oxygen atoms are each -0.75 because 4*(-0.75)=-3** - [ ] **Bond angle: all are 90 degrees because there are 4 groups around sulfur** - [ ] **Bond angle: all are ~109.5 degrees because there are 4 groups around sulfur** - [ ] **Bond angle: both 90 and 120 degrees because there are 5 bonds to sulfur** Explore the characteristics of sulfate further and verify your understanding of molecular geometry and formal charges.
### Formal Charges: 1. **All of the atoms are 0** - Description: This indicates that the formal charge for each atom in the molecule is zero, suggesting a neutral molecule. 2. **Sulfur and two oxygen atoms are 0, the other two oxygens are each -1** - Description: This distribution shows that sulfur and two oxygen atoms do not carry a charge, while the other two oxygen atoms have a formal charge of -1. 3. **Sulfur is 0 and the oxygen atoms are each -0.75 because 4*(-0.75) = -3** - Description: Sulfur has no charge, while each oxygen atom has a partial negative charge, summing up to a total formal charge contribution of -3. ### Bond Angles: 1. **All are 90 degrees because there are 4 groups around sulfur** - Description: This implies a geometry where bond angles are all 90°, typically seen in square planar arrangements. 2. **All are ~109.5 degrees because there are 4 groups around sulfur** - Description: This suggests a tetrahedral geometry where bond angles are approximately 109.5°. 3. **Both 90 and 120 degrees because there are 5 bonds to sulfur** - Description: Indicates a molecular geometry with bond angles of both 90° and 120°, characteristic of seesaw or trigonal bipyramidal geometries. ### Geometry: 1. **Tetrahedral** - Description: A molecular geometry with four groups around the central atom, creating bond angles of about 109.5°. 2. **Square Planar** - Description: A molecular shape where four atoms are positioned at the corners of a square on the same plane. 3. **See Saw** - Description: A molecular geometry that arises from a trigonal bipyramidal arrangement with one fewer substituent, leading to both 90° and 120° bond angles. ### SO Bond Order: 1. **The single bonds are 1 and the double bonds are 2** - Description: This indicates that single sulfur-oxygen bonds have a bond order of 1, while double bonds have a bond order of 2. 2. **All four bonds are 1.5** - Description: Each sulfur-oxygen bond has an average bond order of 1.5, suggesting
Transcribed Image Text:### Formal Charges: 1. **All of the atoms are 0** - Description: This indicates that the formal charge for each atom in the molecule is zero, suggesting a neutral molecule. 2. **Sulfur and two oxygen atoms are 0, the other two oxygens are each -1** - Description: This distribution shows that sulfur and two oxygen atoms do not carry a charge, while the other two oxygen atoms have a formal charge of -1. 3. **Sulfur is 0 and the oxygen atoms are each -0.75 because 4*(-0.75) = -3** - Description: Sulfur has no charge, while each oxygen atom has a partial negative charge, summing up to a total formal charge contribution of -3. ### Bond Angles: 1. **All are 90 degrees because there are 4 groups around sulfur** - Description: This implies a geometry where bond angles are all 90°, typically seen in square planar arrangements. 2. **All are ~109.5 degrees because there are 4 groups around sulfur** - Description: This suggests a tetrahedral geometry where bond angles are approximately 109.5°. 3. **Both 90 and 120 degrees because there are 5 bonds to sulfur** - Description: Indicates a molecular geometry with bond angles of both 90° and 120°, characteristic of seesaw or trigonal bipyramidal geometries. ### Geometry: 1. **Tetrahedral** - Description: A molecular geometry with four groups around the central atom, creating bond angles of about 109.5°. 2. **Square Planar** - Description: A molecular shape where four atoms are positioned at the corners of a square on the same plane. 3. **See Saw** - Description: A molecular geometry that arises from a trigonal bipyramidal arrangement with one fewer substituent, leading to both 90° and 120° bond angles. ### SO Bond Order: 1. **The single bonds are 1 and the double bonds are 2** - Description: This indicates that single sulfur-oxygen bonds have a bond order of 1, while double bonds have a bond order of 2. 2. **All four bonds are 1.5** - Description: Each sulfur-oxygen bond has an average bond order of 1.5, suggesting
Expert Solution
Step 1

In case of SO4^2- many resonating structures can be drawn. But, we can also drawn only two degenerates resonance structures. 

F.C. = No. of valence shell electrons - No. of covalent bonds - 2*no. of l.p. 

For S atom = 6-6-2*0 = 0 

For single bonded O = 6-1-2*3 = -1 

For double bonded O = 6-2-2*2 = 0 

Hence, the correct statement is : b. Formal charge : S and two O atoms are 0 while the other two O atoms are -1 each. 

steps

Step by step

Solved in 2 steps with 1 images

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Similar questions
  • SEE MORE QUESTIONS
Recommended textbooks for you
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY
SEE MORE TEXTBOOKS