Here is a picture of a possible structure for Co. What is the formal charge of the central CI? A :0: 7- :0 +3 +2 +1 00 -1 -2 -3 CI- cl—8: :0:

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...
icon
Related questions
icon
Concept explainers
Question
### Possible Structure of \( ClO_4^- \)

Below is an image depicting a possible Lewis structure for the perchlorate ion (\( ClO_4^- \)):

#### Structure A
- In this structure, a central chlorine (Cl) atom is bonded to four oxygen (O) atoms.
- Each oxygen atom forms a double bond with the central chlorine atom.
- The chlorine atom has no lone pairs, while each oxygen atom has four lone pairs.
- The entire structure carries a negative charge, represented by a minus sign outside a bracket enclosing the structure.

#### Question
What is the formal charge of the central Cl in this structure?

#### Answer Choices
- \(+3\)
- \(+2\)
- \(+1\)
- \(0\)
- \(-1\)
- \(-2\)
- \(-3\)

### Explanation on Formal Charge
To determine the formal charge of the central Cl atom in this structure, use the formal charge formula:
\[ \text{Formal Charge} = ( \text{Valence Electrons} ) - ( \text{Non-bonding Electrons} + \frac{1}{2} \text{Bonding Electrons} ) \]

For chlorine (Cl):
- Valence Electrons: 7 (since chlorine is in group 17 of the periodic table)
- Non-bonding Electrons: 0 (chlorine has no lone pairs in this structure)
- Bonding Electrons: 8 (chlorine forms double bonds with 4 oxygens, so 4 x 2 = 8)

Formal Charge Calculation for Cl:
\[ \text{Formal Charge} = 7 - (0 + \frac{1}{2} \times 8) \]
\[ = 7 - 4 \]
\[ = +3 \]

#### Conclusion
The formal charge of the central Cl in structure \( A \) is \( +3 \).
Transcribed Image Text:### Possible Structure of \( ClO_4^- \) Below is an image depicting a possible Lewis structure for the perchlorate ion (\( ClO_4^- \)): #### Structure A - In this structure, a central chlorine (Cl) atom is bonded to four oxygen (O) atoms. - Each oxygen atom forms a double bond with the central chlorine atom. - The chlorine atom has no lone pairs, while each oxygen atom has four lone pairs. - The entire structure carries a negative charge, represented by a minus sign outside a bracket enclosing the structure. #### Question What is the formal charge of the central Cl in this structure? #### Answer Choices - \(+3\) - \(+2\) - \(+1\) - \(0\) - \(-1\) - \(-2\) - \(-3\) ### Explanation on Formal Charge To determine the formal charge of the central Cl atom in this structure, use the formal charge formula: \[ \text{Formal Charge} = ( \text{Valence Electrons} ) - ( \text{Non-bonding Electrons} + \frac{1}{2} \text{Bonding Electrons} ) \] For chlorine (Cl): - Valence Electrons: 7 (since chlorine is in group 17 of the periodic table) - Non-bonding Electrons: 0 (chlorine has no lone pairs in this structure) - Bonding Electrons: 8 (chlorine forms double bonds with 4 oxygens, so 4 x 2 = 8) Formal Charge Calculation for Cl: \[ \text{Formal Charge} = 7 - (0 + \frac{1}{2} \times 8) \] \[ = 7 - 4 \] \[ = +3 \] #### Conclusion The formal charge of the central Cl in structure \( A \) is \( +3 \).
Expert Solution
steps

Step by step

Solved in 4 steps

Blurred answer
Knowledge Booster
Theories of Bonding
Learn more about
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
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