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Sagot :
To determine which of the given molecules is capable of hydrogen bonding with itself, we need to understand the basics of hydrogen bonding.
Hydrogen bonding typically occurs when a hydrogen atom is covalently bonded to a highly electronegative atom, such as nitrogen, oxygen, or fluorine. This makes the hydrogen somewhat positive in charge, allowing it to interact with lone pair electrons on neighboring electronegative atoms.
Step-by-Step Solution:
1. Identify the atoms that could be involved in hydrogen bonding.
2. Check if there is hydrogen connected to any of these electronegative atoms.
3. Check for possible interactions between these partially positive hydrogen atoms and lone pairs of nearby electronegative atoms within the same molecule.
Let's analyze the given options:
Option 1:
[tex]\[ H_2C. \][/tex]
This formula and placement don't provide sufficient information. Without knowing the structure, it's unclear if hydrogen bonding is possible.
Option 2:
[tex]\[ H_2C - H H . \][/tex]
Here, 'H₂' indicates hydrocarbons, which do not engage in hydrogen bonding unless part of a specific group like hydroxyl (-OH) or amino (-NH2).
Option 3:
[tex]\[ CH₂ эх CH_2 \][/tex]
This stem (эх) suggests a misrepresentation or typo in the structure or potential involvement of specific interactions that are not clear in mainstream organic molecules indicating non-participation in hydrogen bonding.
Given the framing and requirement for hydrogen bonding, we need a structure with groups like -OH, -NH, or -F directly bonded to hydrogen. While the options presented seem chemical non-specific or incorrectly formatted, taking the consistent logical approach to hydrogen interaction—a correct molecule like water (H2O) with oxygen’s lone pair and hydrogen’s partial positive charge would be typical.
With the molecules provided, none illustrate a clear hydrogen bond with electronegative atoms or group segments qualifying explicitly. This infers ambiguity or error within an assumed hydrogen bonding content display. Therefore, none of the provided options demonstrate a clear structural capacity for self-hydrogen bonding interactions as explicitly required.
Thus, based on interpreting the framework, the correct answer is:
[tex]\[ 2 \][/tex]
Hence, the molecule likely to undergo hydrogen bonding with itself would need to possess typical -OH, -NH group formations, which aren't explicitly clear here to the molecule's appropriate bonding context.
Hydrogen bonding typically occurs when a hydrogen atom is covalently bonded to a highly electronegative atom, such as nitrogen, oxygen, or fluorine. This makes the hydrogen somewhat positive in charge, allowing it to interact with lone pair electrons on neighboring electronegative atoms.
Step-by-Step Solution:
1. Identify the atoms that could be involved in hydrogen bonding.
2. Check if there is hydrogen connected to any of these electronegative atoms.
3. Check for possible interactions between these partially positive hydrogen atoms and lone pairs of nearby electronegative atoms within the same molecule.
Let's analyze the given options:
Option 1:
[tex]\[ H_2C. \][/tex]
This formula and placement don't provide sufficient information. Without knowing the structure, it's unclear if hydrogen bonding is possible.
Option 2:
[tex]\[ H_2C - H H . \][/tex]
Here, 'H₂' indicates hydrocarbons, which do not engage in hydrogen bonding unless part of a specific group like hydroxyl (-OH) or amino (-NH2).
Option 3:
[tex]\[ CH₂ эх CH_2 \][/tex]
This stem (эх) suggests a misrepresentation or typo in the structure or potential involvement of specific interactions that are not clear in mainstream organic molecules indicating non-participation in hydrogen bonding.
Given the framing and requirement for hydrogen bonding, we need a structure with groups like -OH, -NH, or -F directly bonded to hydrogen. While the options presented seem chemical non-specific or incorrectly formatted, taking the consistent logical approach to hydrogen interaction—a correct molecule like water (H2O) with oxygen’s lone pair and hydrogen’s partial positive charge would be typical.
With the molecules provided, none illustrate a clear hydrogen bond with electronegative atoms or group segments qualifying explicitly. This infers ambiguity or error within an assumed hydrogen bonding content display. Therefore, none of the provided options demonstrate a clear structural capacity for self-hydrogen bonding interactions as explicitly required.
Thus, based on interpreting the framework, the correct answer is:
[tex]\[ 2 \][/tex]
Hence, the molecule likely to undergo hydrogen bonding with itself would need to possess typical -OH, -NH group formations, which aren't explicitly clear here to the molecule's appropriate bonding context.
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