Tetravalency of carbon hybridization and shapes of simple molecules - One Line Questions

1. The C-C single bond length in ethane (C₂H₆) is approximately: — 154 pm
2. The C=C double bond length in ethene (C₂H₄) is approximately: — 134 pm
3. The C≡C triple bond length in ethyne (C₂H₂) is approximately: — 120 pm
4. What is the approximate percentage of s-character in sp³ hybridization? — 25%
5. What is the approximate percentage of s-character in sp² hybridization? — 33.3%
6. What is the approximate percentage of s-character in sp hybridization? — 50%
7. The bond angle in methane (CH₄), where carbon is sp³ hybridized, is approximately: — 109.5°
8. The bond angle in ethene (C₂H₄), where carbon is sp² hybridized, is approximately: — 120°
9. The bond angle in ethyne (C₂H₂), where carbon is sp hybridized, is approximately: — 180°
10. The shape of the carbon dioxide (CO₂) molecule is: — Linear
11. Which of the following carbon atoms undergoes sp³ hybridization? — Carbon in CH₄
12. Which of the following carbon atoms undergoes sp² hybridization? — Carbon in C₂H₄
13. Which of the following carbon atoms undergoes sp hybridization? — Carbon in C₂H₂
14. Which of the following molecules has a central carbon atom that is sp³ hybridized and exhibits a tetrahedral geometry? — Methane (CH₄)
15. Which of the following molecules has a central carbon atom that is sp² hybridized and exhibits a trigonal planar geometry? — Ethene (C₂H₄)
16. Which of the following is a consequence of carbon's tetravalency? — Formation of chains and rings
17. Which type of overlap leads to the formation of pi bonds? — Sideways overlap of p orbitals
18. What is the role of hybridization in explaining the shapes of molecules? — It describes the mixing of atomic orbitals to form new hybrid orbitals with specific spatial orientations
19. A molecule with sp³ hybridized carbon atoms will have a geometry that is: — Tetrahedral
20. The shape of a molecule with sp² hybridized carbon atoms is typically: — Trigonal planar
21. A molecule with sp hybridized carbon atoms will have a geometry that is: — Linear
22. The shape of a molecule where a carbon atom is bonded to three other atoms and has no lone pairs is: — Trigonal planar
23. The shape of a molecule where a carbon atom is bonded to two other atoms and has no lone pairs is: — Linear
24. The shape of a carbocation (e.g., CH₃⁺) is: — Trigonal planar
25. The shape of a carbanion (e.g., CH₃⁻) is: — Pyramidal
26. The shape of a carbon free radical (e.g., CH₃•) is typically: — Trigonal planar
27. Which type of overlap leads to the formation of sigma bonds? — Both B and C
28. Which type of hybridization is adopted by carbon when it forms four single bonds? — sp³
29. The hybridization of carbon in methane (CH₄) is: — sp³
30. In ethene (C₂H₄), each carbon atom is hybridized as: — sp²
31. In ethyne (C₂H₂), each carbon atom is hybridized as: — sp
32. The presence of a double bond in a molecule indicates that the carbon atoms involved are hybridized as: — sp²
33. The presence of a triple bond in a molecule indicates that the carbon atoms involved are hybridized as: — sp
34. In benzene (C₆H₆), each carbon atom is hybridized as: — sp²
35. In CO₂, the carbon atom is hybridized as: — sp
36. The hybridization of the carbon atom in a carbonyl group (C=O) is: — sp²
37. When a carbon atom forms a single bond, a double bond, and a single bond, its hybridization is: — sp²
38. When a carbon atom forms two double bonds, its hybridization is: — sp
39. The hybridization of carbon in a carbocation (e.g., CH₃⁺) is typically: — sp²
40. The hybridization of carbon in a carbanion (e.g., CH₃⁻) is typically: — sp³
41. In graphite, carbon atoms are hybridized as: — sp²
42. In diamond, carbon atoms are hybridized as: — sp³
43. The hybridization of carbon in a free radical (e.g., CH₃•) is generally considered to be: — sp²
44. Which type of bond is formed by the overlap of one s orbital and one p orbital? — sp hybridization
45. Which type of bond is formed by the overlap of one s orbital and two p orbitals? — sp² hybridization
46. Which type of bond is formed by the overlap of one s orbital and three p orbitals? — sp³ hybridization
47. The concept of hybridization helps explain: — The observed bond angles and molecular shapes
48. What is the characteristic valency of a carbon atom in organic compounds? — Four
49. In a carbon atom forming a double bond, how many pi bonds are present? — One
50. In a carbon atom forming a triple bond, how many pi bonds are present? — Two
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