객관식
Which of the following best represents the correct Lewis structure for (C2H4O)?
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1. A Review of General Chemistry
Lewis Structure
객관식
Which of the following best describes the Lewis structure of the molecule?
A
It does not exist as a stable neutral molecule; is not a valid Lewis structure for a neutral species.
B
It consists of four chlorine atoms forming a tetrahedral structure with each atom sharing electrons equally.
C
It consists of four chlorine atoms bonded together in a linear chain, each with three lone pairs.
D
It consists of four chlorine atoms arranged in a square planar geometry, each sharing one single bond with a central atom.
검증된 단계별 안내1
Step 1: Identify the molecular formula and the atoms involved. Here, \( \mathrm{Cl}_4 \) implies four chlorine atoms bonded together without any other element present.
Step 2: Recall the typical bonding behavior of chlorine atoms. Chlorine is a halogen with seven valence electrons and typically forms only one single bond to complete its octet.
Step 3: Consider the possibility of bonding between chlorine atoms. Since chlorine atoms prefer to form one bond each, a molecule consisting solely of four chlorine atoms bonded together (\( \mathrm{Cl}_4 \)) would require multiple bonds per atom or unusual bonding patterns, which are not stable or common.
Step 4: Analyze the given options in terms of molecular geometry and bonding. For example, a tetrahedral structure requires a central atom bonded to four others, but here all atoms are chlorine, so no central atom exists to form such a structure.
Step 5: Conclude that \( \mathrm{Cl}_4 \) as a neutral molecule is not stable or valid because chlorine atoms do not form multiple bonds with each other to create such a species; thus, the Lewis structure for \( \mathrm{Cl}_4 \) does not exist as a stable neutral molecule.
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