Is the following molecule capable of making hydrogen bonds

AI Thread Summary
The discussion centers on the ability of a molecule with double-bonded oxygens to engage in hydrogen bonding. It is clarified that while the molecule cannot act as a hydrogen bond donor due to the absence of hydrogen atoms, it can still accept hydrogen bonds from other molecules. The presence of double-bonded oxygens does not prevent them from accepting hydrogen bonds, as hydrogen bonds are distinct from the covalent bonds formed by C=O. The high electronegativity of oxygen and nitrogen creates polar interactions, allowing for hydrogen bonding with other polar molecules, such as water. However, the strength of these hydrogen bonds in the discussed molecule may be limited due to its relatively low polarity.
ihaveabutt
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This is not a homework question.
 
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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.
 
Ygggdrasil said:
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.

With the oxygens all double bonded to the carbons where would the hydrogen bond to?
 
ihaveabutt said:
With the oxygens all double bonded to the carbons where would the hydrogen bond to?

There's nothing preventing a double bonded oxygen from accepting a hydrogen bond.

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ihaveabutt said:
With the oxygens all double bonded to the carbons where would the hydrogen bond to?

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.
 
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