Table of contents

1. A Review of General Chemistry5h 5m
2. Molecular Representations1h 14m
3. Acids and Bases2h 46m
4. Alkanes and Cycloalkanes4h 17m
5. Chirality3h 39m
6. Thermodynamics and Kinetics1h 22m
7. Substitution Reactions1h 48m
8. Elimination Reactions2h 30m
9. Alkenes and Alkynes2h 9m
10. Addition Reactions3h 19m
11. Radical Reactions1h 58m
12. Alcohols, Ethers, Epoxides and Thiols2h 42m
13. Alcohols and Carbonyl Compounds2h 17m
14. Synthetic Techniques1h 26m
15. Analytical Techniques:IR, NMR, Mass Spect7h 3m
16. Conjugated Systems6h 13m
17. Ultraviolet Spectroscopy51m
18. Aromaticity2h 34m
19. Reactions of Aromatics: EAS and Beyond5h 1m
20. Phenols55m
21. Aldehydes and Ketones: Nucleophilic Addition4h 56m
22. Carboxylic Acid Derivatives: NAS2h 51m
23. The Chemistry of Thioesters, Phophate Ester and Phosphate Anhydrides1h 10m
24. Enolate Chemistry: Reactions at the Alpha-Carbon1h 53m
25. Condensation Chemistry2h 9m
26. Amines1h 43m
27. Heterocycles2h 0m
28. Carbohydrates5h 53m
29. Amino Acids4h 20m
30. Peptides and Proteins2h 42m
31. Catalysis in Organic Reactions1h 30m
32. Lipids 2h 50m
33. The Organic Chemistry of Metabolic Pathways2h 52m
34. Nucleic Acids1h 32m
35. Transition Metals6h 14m
36. Synthetic Polymers1h 49m

1. A Review of General Chemistry

Electronegativity

Organic Chemistry

1. A Review of General Chemistry

Electronegativity

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4:25 minutes

Problem 51a

Textbook Question

Which bond is stronger? Briefly explain why.
a.

Verified step by step guidance

Step 1: Understand the concept of bond strength. Bond strength is determined by the bond dissociation energy, which is the energy required to break a bond in a molecule. Stronger bonds have higher bond dissociation energies.

Step 2: Identify the types of bonds being compared. For example, single bonds (sigma bonds), double bonds (one sigma and one pi bond), or triple bonds (one sigma and two pi bonds). Triple bonds are generally stronger than double bonds, which are stronger than single bonds.

Step 3: Consider the atomic size and electronegativity of the atoms involved in the bond. Smaller atoms form shorter and stronger bonds, while higher electronegativity differences can lead to stronger polar bonds.

Step 4: Evaluate resonance and hybridization effects. Bonds in resonance structures may be delocalized, which can affect their strength. Similarly, bonds involving sp-hybridized orbitals are shorter and stronger than those involving sp2 or sp3 orbitals.

Step 5: Compare the bond dissociation energies or use the above factors to determine which bond is stronger. Provide a brief explanation based on the factors influencing bond strength, such as bond order, atomic size, and hybridization.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Bond Strength

Bond strength refers to the amount of energy required to break a bond between two atoms. It is influenced by factors such as the type of bond (single, double, or triple), the electronegativity of the atoms involved, and the bond length. Generally, shorter bonds and those involving greater overlap of atomic orbitals are stronger.

Types of Chemical Bonds

Chemical bonds can be categorized into ionic, covalent, and metallic bonds. Covalent bonds, formed by the sharing of electrons, can be further classified into single, double, and triple bonds, with triple bonds being the strongest due to increased electron sharing. Understanding these types helps in comparing bond strengths effectively.

Electronegativity

Electronegativity is a measure of an atom's ability to attract and hold onto electrons in a bond. Atoms with high electronegativity tend to form stronger bonds with other atoms, as they can pull shared electrons closer, resulting in a more stable bond. This concept is crucial for understanding why certain bonds are stronger than others.

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Related Practice

Textbook Question

(i) Using the periodic trend, choose the more electronegative atom in each pair. For one pair, you'll need to look at the actual Pauling values. (ii) For which one? (iii) Why?

(d) B vs. Si