- #1
ihaveabutt
- 17
- 0
This is not a homework question.
Is the following molecule capable of making hydrogen bonds
- Thread starter ihaveabutt
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SUMMARY
The discussed molecule is capable of accepting hydrogen bonds due to the presence of electronegative oxygen atoms, despite lacking hydrogen atoms to act as donors. The double-bonded oxygens (C=O) do not prevent hydrogen bonding; rather, they can still interact with polar molecules like water. However, the overall polarity of the molecule is low, which may result in weaker hydrogen bonding interactions.
PREREQUISITES- Understanding of hydrogen bonding mechanisms
- Knowledge of molecular polarity and electronegativity
- Familiarity with molecular structures, specifically C=O bonds
- Basic principles of intermolecular forces
- Research the role of electronegativity in hydrogen bonding
- Study molecular polarity and its effects on intermolecular interactions
- Explore examples of hydrogen bond acceptors and donors in organic molecules
- Investigate the strength of hydrogen bonds in various chemical environments
Chemistry students, molecular biologists, and researchers interested in intermolecular forces and hydrogen bonding in organic compounds.
This is not a homework question.
- #2
- 3,753
- 4,198
It could accept hydrogen bonds from other molecules, but given that it doesn't have any hydrogens, it would not be able to act as a hydrogen bond donor.
- #3
ihaveabutt
- 17
- 0
Ygggdrasil said:
With the oxygens all double bonded to the carbons where would the hydrogen bond to?
- #4
- 3,753
- 4,198
Well, what is needed for an atom in a molecule to act as a hydrogen bond acceptor? (hint: read https://en.wikipedia.org/wiki/Hydrogen_bond)
- #5
aroc91
- 181
- 5
ihaveabutt said:
There's nothing preventing a double bonded oxygen from accepting a hydrogen bond.
- #6
aclark609
- 35
- 1
ihaveabutt said:
Hydrogen bonds aren't the same as the bonds between the double bonded C=O. Oxygen and Nitroghen have a very high electronegativity (They love electrons). So in a molecule they are bonded to, they hold most of the negative charge creating poles within the molecule, because if they have the electrons, the other atoms don't leaving them with a positive charge. If another molecule is introduced (say water) that is polar and contains hydrogen, their poles can interact creating an attractive force that's not really a bond but like I said just an attractive force. This interaction is considered hydrogen bonding. So you see it doesn't matter that double bond's exist between the C=O as long as there is dipole attractive forces.
However, in this particular molecule, I don't think the hydrogen bonding would be that strong because it is not all that polar to begin with. But hydrogen bonds could exist because the molecule is slightly polar.