Bond Type (lonic, pure Total Shared Lone Molecular Bond Hybrid Molecule Name Polarity Lewis Structure Bonding Pairs Pairs Shape Angle Orbital covalent, polar covalent) Pairs Dihydrogen Polar Example H,0 1.24 4 2 2 Bent 104.5 Monoxide covalent BF3 NH," PCI, 3 Bef2 CO2 CF4 SCI, 7 NH3 CBr4 SnClz 10 LO 00
Bond Type (lonic, pure Total Shared Lone Molecular Bond Hybrid Molecule Name Polarity Lewis Structure Bonding Pairs Pairs Shape Angle Orbital covalent, polar covalent) Pairs Dihydrogen Polar Example H,0 1.24 4 2 2 Bent 104.5 Monoxide covalent BF3 NH," PCI, 3 Bef2 CO2 CF4 SCI, 7 NH3 CBr4 SnClz 10 LO 00
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...
Related questions
Question
PLEASEEEE HELP ME ASAP!!!
Use you knowledge of Lewis structures, polarity, Table 1, and Table 2 to complete the table below for each molecule listed.
![The image is a table designed to classify and describe various molecules. Each row represents a different molecule, organized under several columns with specific headings. Here is a detailed explanation of the columns and what they represent:
1. **Molecule**: This column lists the chemical formula of the molecule.
2. **Name**: This column provides the common name of the molecule.
3. **Polarity**: This column indicates the polarity of the molecule, measured numerically.
4. **Bond Type**: This specifies whether the bonds within the molecule are ionic, pure covalent, or polar covalent.
5. **Lewis Structure**: This depicts the Lewis structure (electron dot diagram) of the molecule. An example shows the structure for water (H₂O).
6. **Total Bonding Pairs**: This column shows the total number of bonding electron pairs in the molecule.
7. **Shared Pairs**: This details the number of electron pairs shared between atoms in bonds.
8. **Lone Pairs**: This notes the number of lone electron pairs on the central atom.
9. **Molecular Shape**: The geometry of the molecule is described here (e.g., bent, linear).
10. **Bond Angle**: The angle in degrees between bonds in the molecule.
11. **Hybrid Orbital**: Indicates the type of hybrid orbitals involved (e.g., sp³).
### Example Row
- **Molecule**: H₂O
- **Name**: Dihydrogen Monoxide
- **Polarity**: 1.24
- **Bond Type**: Polar covalent
- **Lewis Structure**: Depicts the structure with two lone pairs on the oxygen and bonds to hydrogen.
- **Total Bonding Pairs**: 4
- **Shared Pairs**: 2
- **Lone Pairs**: 2
- **Molecular Shape**: Bent
- **Bond Angle**: 104.5
- **Hybrid Orbital**: sp³
The rows 1 to 10 are reserved for other molecules, following the same format. Only the example for water is filled out in the image. Each entry is expected to provide similar detailed information about the respective molecule.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Feba21ff9-1e37-4047-8aa8-165325f7b8a1%2F44b956e4-9f4d-4d71-941c-53f0d7880b41%2F4i1vq8_processed.png&w=3840&q=75)
Transcribed Image Text:The image is a table designed to classify and describe various molecules. Each row represents a different molecule, organized under several columns with specific headings. Here is a detailed explanation of the columns and what they represent:
1. **Molecule**: This column lists the chemical formula of the molecule.
2. **Name**: This column provides the common name of the molecule.
3. **Polarity**: This column indicates the polarity of the molecule, measured numerically.
4. **Bond Type**: This specifies whether the bonds within the molecule are ionic, pure covalent, or polar covalent.
5. **Lewis Structure**: This depicts the Lewis structure (electron dot diagram) of the molecule. An example shows the structure for water (H₂O).
6. **Total Bonding Pairs**: This column shows the total number of bonding electron pairs in the molecule.
7. **Shared Pairs**: This details the number of electron pairs shared between atoms in bonds.
8. **Lone Pairs**: This notes the number of lone electron pairs on the central atom.
9. **Molecular Shape**: The geometry of the molecule is described here (e.g., bent, linear).
10. **Bond Angle**: The angle in degrees between bonds in the molecule.
11. **Hybrid Orbital**: Indicates the type of hybrid orbitals involved (e.g., sp³).
### Example Row
- **Molecule**: H₂O
- **Name**: Dihydrogen Monoxide
- **Polarity**: 1.24
- **Bond Type**: Polar covalent
- **Lewis Structure**: Depicts the structure with two lone pairs on the oxygen and bonds to hydrogen.
- **Total Bonding Pairs**: 4
- **Shared Pairs**: 2
- **Lone Pairs**: 2
- **Molecular Shape**: Bent
- **Bond Angle**: 104.5
- **Hybrid Orbital**: sp³
The rows 1 to 10 are reserved for other molecules, following the same format. Only the example for water is filled out in the image. Each entry is expected to provide similar detailed information about the respective molecule.
Expert Solution
![](/static/compass_v2/shared-icons/check-mark.png)
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution!
Trending now
This is a popular solution!
Step by step
Solved in 2 steps with 2 images
![Blurred answer](/static/compass_v2/solution-images/blurred-answer.jpg)
Recommended textbooks for you
![Chemistry](https://www.bartleby.com/isbn_cover_images/9781305957404/9781305957404_smallCoverImage.gif)
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
![Chemistry](https://www.bartleby.com/isbn_cover_images/9781259911156/9781259911156_smallCoverImage.gif)
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
![Principles of Instrumental Analysis](https://www.bartleby.com/isbn_cover_images/9781305577213/9781305577213_smallCoverImage.gif)
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
![Chemistry](https://www.bartleby.com/isbn_cover_images/9781305957404/9781305957404_smallCoverImage.gif)
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
![Chemistry](https://www.bartleby.com/isbn_cover_images/9781259911156/9781259911156_smallCoverImage.gif)
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
![Principles of Instrumental Analysis](https://www.bartleby.com/isbn_cover_images/9781305577213/9781305577213_smallCoverImage.gif)
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
![Organic Chemistry](https://www.bartleby.com/isbn_cover_images/9780078021558/9780078021558_smallCoverImage.gif)
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
![Chemistry: Principles and Reactions](https://www.bartleby.com/isbn_cover_images/9781305079373/9781305079373_smallCoverImage.gif)
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
![Elementary Principles of Chemical Processes, Bind…](https://www.bartleby.com/isbn_cover_images/9781118431221/9781118431221_smallCoverImage.gif)
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY