객관식
In a benzene molecule , where are the pi electrons delocalized?
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1. A Review of General Chemistry
Resonance Structures
객관식
Which of the following pairs of structures represent resonance forms that contribute to the same resonance hybrid?
A
A pair of structures for where one has both double bonds and the other has one triple bond and one single bond
B
A pair of structures for benzene where one has alternating single and double bonds and the other has all single bonds
C
A pair of structures for where the chlorine atom is attached to different carbon atoms
D
A pair of structures for (ozone) where the double bond and single bond are switched between the two terminal oxygens
검증된 단계별 안내1
Step 1: Understand the concept of resonance forms. Resonance structures are different Lewis structures for the same molecule that differ only in the placement of electrons, not the arrangement of atoms. They contribute to a resonance hybrid, which is the actual structure of the molecule.
Step 2: Analyze the first pair (CO2) where one structure has two double bonds and the other has one triple bond and one single bond. Since the connectivity of atoms is the same and only the electron distribution changes, these can be resonance forms if the bonding pattern is valid.
Step 3: Examine the second pair (benzene) where one structure has alternating single and double bonds and the other has all single bonds. The structure with all single bonds does not represent a valid resonance form because it changes the bonding framework, not just electron placement.
Step 4: Consider the third pair (CH3CH2Cl) where chlorine is attached to different carbon atoms. These are not resonance forms but rather different isomers because the connectivity of atoms changes.
Step 5: Look at the fourth pair (ozone, O3) where the double bond and single bond switch between the two terminal oxygens. This is a classic example of resonance forms because the atoms remain connected the same way, and only the electron placement changes, contributing to the resonance hybrid.
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