Table of contents

1. Matter and Measurements4h 31m
2. Atoms and the Periodic Table5h 23m
3. Ionic Compounds2h 18m
4. Molecular Compounds2h 18m
5. Classification & Balancing of Chemical Reactions3h 17m
6. Chemical Reactions & Quantities2h 27m
7. Energy, Rate and Equilibrium3h 46m
8. Gases, Liquids and Solids3h 25m
9. Solutions4h 10m
10. Acids and Bases3h 29m
11. Nuclear Chemistry56m
BONUS: Lab Techniques and Procedures1h 38m
BONUS: Mathematical Operations and Functions47m
12. Introduction to Organic Chemistry1h 34m
13. Alkenes, Alkynes, and Aromatic Compounds2h 12m
14. Compounds with Oxygen or Sulfur1h 6m
15. Aldehydes and Ketones1h 1m
16. Carboxylic Acids and Their Derivatives1h 11m
17. Amines39m
18. Amino Acids and Proteins1h 51m
19. Enzymes1h 37m
20. Carbohydrates1h 41m
21. The Generation of Biochemical Energy2h 8m
22. Carbohydrate Metabolism2h 22m
23. Lipids2h 26m
24. Lipid Metabolism1h 45m
25. Protein and Amino Acid Metabolism1h 37m
26. Nucleic Acids and Protein Synthesis2h 54m

4. Molecular Compounds

Multiple Bonds

GOB Chemistry

4. Molecular Compounds

Multiple Bonds

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Multiple Choice

Identify the least stable covalent bond.

N–C

F–Na

N=C

N≡C

all same strength

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Verified step by step guidance

Understand that covalent bonds involve the sharing of electron pairs between atoms. The stability of a covalent bond is influenced by factors such as bond order, electronegativity differences, and atomic size.

Examine the bond types given: N–C, F–Na, N=C, N≡C. Note that F–Na is not a covalent bond; it is an ionic bond due to the large electronegativity difference between fluorine and sodium.

Consider bond order: Single bonds (e.g., N–C) are generally less stable than double bonds (e.g., N=C) and triple bonds (e.g., N≡C) because higher bond orders mean more shared electrons, leading to stronger bonds.

Evaluate electronegativity differences: A large difference in electronegativity between bonded atoms can lead to polar covalent bonds, which may be less stable than nonpolar covalent bonds.

Conclude that among the covalent bonds listed, N–C is likely the least stable due to its single bond nature, compared to the double bond N=C and the triple bond N≡C, which are stronger due to higher bond orders.