Polar covalent bonds involve the unequal sharing of electrons between two atoms. The polarity of a bond is determined by the difference in electronegativity between the atoms. For each molecule below, indicate the hybridization state and molecular geometry of each carbon. Rank the indicated bonds from weakest to strongest
The Correct Answer and Explanation is:
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Based on the image, the questions seem to involve the following:
1. Hybridization state and molecular geometry for each carbon:
For each molecule in the image:
- Methane (CH₄): The carbon in methane is sp³ hybridized, and the molecular geometry is tetrahedral.
- Ethene (C₂H₄): The carbon in ethene is sp² hybridized, with a trigonal planar geometry.
- Ethyne (C₂H₂): The carbon in ethyne is sp hybridized, and the geometry is linear.
2. Ranking bonds from weakest to strongest:
- C-C (single bond in ethane): Weakest.
- C=C (double bond in ethene): Stronger than C-C, but weaker than C≡C.
- C≡C (triple bond in ethyne): Strongest bond.
Explanation:
- Hybridization refers to the mixing of atomic orbitals to form hybrid orbitals that participate in bonding. The type of hybridization depends on the number of bonding regions around the atom.
- In sp³ hybridization (tetrahedral geometry), there are four bonding regions, as seen in methane.
- In sp² hybridization (trigonal planar geometry), there are three bonding regions, typical of ethene.
- In sp hybridization (linear geometry), there are two bonding regions, seen in ethyne.
- Bond strength depends on the number of shared electron pairs:
- Single bonds (C-C) are the weakest.
- Double bonds (C=C) are stronger due to the additional shared electrons.
- Triple bonds (C≡C) are the strongest as they involve the sharing of three pairs of electrons.
