![General, Organic, and Biological Chemistry - 4th edition](https://www.bartleby.com/isbn_cover_images/9781259883989/9781259883989_largeCoverImage.gif)
Concept explainers
(a)
Interpretation:
Bonds formed between H and Br should be classified as polarcovalent or ionic based on the electronegativity of atoms.
Concept Introduction:
The electronegativity of atoms defines the bond characteristics, as the electron distribution of the bond can be predicted by electronegativity. Electronegativity is tendency to pull bond electrons towards an atom. Electronegativity difference between bonded atoms defines the nature of bond as stated in the following table.
Electronegativity difference | Type of bond | Electron distribution in bond. |
0.5 > | Nonpolar | Electrons are equally distributed. |
0.5 -1.9 | Polar covalent | Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom). |
1.9 ≤ | Ionic | Electron has been donated to the more electronegative atom from less electronegative atom. |
![Check Mark](/static/check-mark.png)
Answer to Problem 63P
The bond between H and Br atom is polar covalent.
Explanation of Solution
The electronegativity of H and Br atom is 2.1 and 2.8 respectively. The electronegativity difference will be 0.7.
Since,
Electronegativity difference | Type of bond | Electron distribution in bond. |
0.5 > | Nonpolar | Electrons are equally distributed. |
0.5 -1.9 | Polar covalent | Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom). |
1.9 ≤ | Ionic | Electron has been donated to the more electronegative atom from less electronegative atom. |
Thus, the bond will be polar covalent in nature.
(b)
Interpretation:
Bonds formed between Na and S should be classified as polar covalent or ionic based on the electronegativity of atoms.
Concept Introduction:
The electronegativity of atoms defines the bond characteristics, as the electron distribution of the bond can be predicted by electronegativity. Electronegativity is tendency to pull bond electrons towards an atom. Electronegativity difference between bonded atoms defines the nature of bond as stated in the following table.
Electronegativity difference | Type of bond | Electron distribution in bond. |
0.5 > | Nonpolar | Electrons are equally distributed. |
0.5 -1.9 | Polar covalent | Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom). |
1.9 ≤ | Ionic | Electron has been donated to the more electronegative atom from less electronegative atom. |
![Check Mark](/static/check-mark.png)
Answer to Problem 63P
The bond between Na and S atom is polar covalent.
Explanation of Solution
The electronegativity of Na and S atom is 0.9 and 2.5 respectively. The electronegativity difference will be 1.6.
Since,
Electronegativity difference | Type of bond | Electron distribution in bond. |
0.5 > | Nonpolar | Electrons are equally distributed. |
0.5 -1.9 | Polar covalent | Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom). |
1.9 ≤ | Ionic | Electron has been donated to the more electronegative atom from less electronegative atom. |
Thus, the bond will be polar covalent in nature.
(c)
Interpretation:
Bonds formed between N and C should be classified as polar covalent or ionic based on the electronegativity of atoms.
Concept Introduction:
The electronegativity of atoms defines the bond characteristics, as the electron distribution of the bond can be predicted by electronegativity. Electronegativity is tendency to pull bond electrons towards an atom. Electronegativity difference between bonded atoms defines the nature of bond as stated in the following table.
Electronegativity difference | Type of bond | Electron distribution in bond. |
0.5 > | Nonpolar | Electrons are equally distributed. |
0.5 -1.9 | Polar covalent | Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom). |
1.9 ≤ | Ionic | Electron has been donated to the more electronegative atom from less electronegative atom. |
![Check Mark](/static/check-mark.png)
Answer to Problem 63P
The bond between N and C atom is polar covalent.
Explanation of Solution
The electronegativity of N and C atom is 3.0 and 2.7 respectively. The electronegativity difference will be 0.5.
Since,
Electronegativity difference | Type of bond | Electron distribution in bond. |
0.5 > | Nonpolar | Electrons are equally distributed. |
0.5 -1.9 | Polar covalent | Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom). |
1.9 ≤ | Ionic | Electron has been donated to the more electronegative atom from less electronegative atom. |
Thus, the bond will be polar covalent in nature.
(d)
Interpretation:
Bonds formed between Li and O should be classified as polar covalent or ionic based on the electronegativity of atoms.
Concept Introduction:
The electronegativity of atoms defines the bond characteristics, as the electron distribution of the bond can be predicted by electronegativity. Electronegativity is tendency to pull bond electrons towards an atom. Electronegativity difference between bonded atoms defines the nature of bond as stated in the following table.
Electronegativity difference | Type of bond | Electron distribution in bond. |
0.5 > | Nonpolar | Electrons are equally distributed. |
0.5 -1.9 | Polar covalent | Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom). |
1.9 ≤ | Ionic | Electron has been donated to the more electronegative atom from less electronegative atom. |
![Check Mark](/static/check-mark.png)
Answer to Problem 63P
The bond between Li and O is ionic.
Explanation of Solution
The electronegativity of Li and O atom is 1.0 and 3.5 respectively. The electronegativity difference will be 2.5.
Since,
Electronegativity difference | Type of bond | Electron distribution in bond. |
0.5 > | Nonpolar | Electrons are equally distributed. |
0.5 -1.9 | Polar covalent | Electrons are unequally distributed between bonded atoms. (more electrons towards more electronegative atom). |
1.9 ≤ | Ionic | Electron has been donated to the more electronegative atom from less electronegative atom. |
Thus, the bond will be ionic in nature.
Want to see more full solutions like this?
Chapter 4 Solutions
General, Organic, and Biological Chemistry - 4th edition
- Draw the major product of this reaction. Ignore inorganic byproducts. Problem 17 of 35 1. CH3CH2Li O H 2. Neutralizing work-up @ Atoms, Bonds and Rings Draw or tap a new boarrow_forwardWill this convert the C=O to an alcohol? Or does its participation in the carboxy group prevent that from happening?arrow_forwardI have some reactions here for which I need to predict the products. Can you help me solve them and rewrite the equations, as well as identify the type of reaction? Please explain it to me.I have some reactions here for which I need to predict the products. Can you help me solve them and rewrite the equations, as well as identify the type of reaction? Please explain it to marrow_forward
- Help me i dont know how to do itarrow_forwardCan you explain how to draw a molecular orbital diagram for the given molecule? It is quite difficult to understand. Additionally, could you provide a clearer illustration? Furthermore, please explain how to draw molecular orbital diagrams for any other given molecule or compound as well.arrow_forwardCurved arrows are used to illustrate the flow of electrons. Using the provided starting and product structures, draw the curved electron-pushing arrows for the following reaction or mechanistic step(s). Be sure to account for all bond-breaking and bond-making steps. Prob 10: Select to Add Arrows THEarrow_forward
- Curved arrows are used to illustrate the flow of electrons using the provided starting and product structures draw the curved electron pushing arrows for the following reaction or mechanistic steps Ether(solvent)arrow_forwardThis deals with synthetic organic chemistry. Please fill in the blanks appropriately.arrow_forwardUse the References to access important values if needed for this question. What is the IUPAC name of each of the the following? 0 CH3CHCNH₂ CH3 CH3CHCNHCH2CH3 CH3arrow_forward
- Living By Chemistry: First Edition TextbookChemistryISBN:9781559539418Author:Angelica StacyPublisher:MAC HIGHEROrganic ChemistryChemistryISBN:9781305580350Author:William H. Brown, Brent L. Iverson, Eric Anslyn, Christopher S. FootePublisher:Cengage Learning
- Chemistry: Matter and ChangeChemistryISBN:9780078746376Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl WistromPublisher:Glencoe/McGraw-Hill School Pub CoWorld of Chemistry, 3rd editionChemistryISBN:9781133109655Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCostePublisher:Brooks / Cole / Cengage LearningChemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning
![Text book image](https://www.bartleby.com/isbn_cover_images/9781559539418/9781559539418_smallCoverImage.gif)
![Text book image](https://www.bartleby.com/isbn_cover_images/9781305580350/9781305580350_smallCoverImage.gif)
![Text book image](https://www.bartleby.com/isbn_cover_images/9781133109655/9781133109655_smallCoverImage.jpg)
![Text book image](https://www.bartleby.com/isbn_cover_images/9781337398909/9781337398909_smallCoverImage.gif)