The disproportionate potential in H-bonds

[sunspot]

Hydrogen bonds are more than a dipole potential between a hydrogen atom and the unbonded electrons of an highly electronegative atom. What makes hydrogen bonds unique is that the hydrogen goes into a hydrogen bond carrying the primary burden of the potential. The shared electrons will have a lower potential to form the hydrogen bond.

 

This anomaly can be understood by looking at the hydrogen bonding in water. A water molecule will have four hybrid sp3 orbitals. The hydrogen of water are bonded to two of these four orbitals. The other two hybrid orbitals are occupied by unshared electrons that participate in hydrogen bonding.

 

The hybrid orbitals allow the covlantly bonded hydrogen to share electrons with the oxygen, but at a higher orbital distance due to the P-character of the hybrid orbitals. In other words, hydrogen is optimized for 1S orbitals, but is induced by the bond with oxygen to share electrons with a lot of P-character. This sort of ionizes the electrons shared by hydrogen away from its preferred 1S orbital. It still has electron density to balance most of its positive charge, but it is being held further away from its 1S orbtal than is optimum.

 

The oxygen, on the other hand, gains the electron density to become slightly negative, but these electron are placed in hybrid orbitals more in line with the octet and the p-orbital needs of oxygen, As such, although the charge dipole will balance, the hydrogen has a higher overall potential.

 

Data that supports this is connected to hydrogen bond energy dropping drastically with deviation from linear hydrogen bonding angles. In other words, if we maintain the distance between the hydrogen and shared electrons within a hydrogen bond, but only shift the bond angle, this should not affect a purely electrostatic attraction. In the case of hydrogen bonds, the angle deviation has more to do with losing the ability to line up orbitals. The linear arrangment allows the hydrogen to compensation for its p-character ionization. If we shift the angle, the hydrogen bond energy becomes more dependant on electrostatic attraction, which is not as effiecient for the hydrogen.

 

Another supporting observation is the contraction of water when it melts. The only other material in nature that does this is the metal Antimony. When water is ice the hydrogen bonds are linear and the potential of the hydrogen is minimized due to the p-orbital sharing with the unbonded electrons of oxygen. When we heat ice and cause it to melt, the oxygen will twist away. This alters the hydrogen bond angles causing the lower potential electrostatic force to have get much closer to lower the potential.

 

In liquid water the hydrogen would like to line up the oxygen for linear hydrogen bonds but often as to settle for the closer electrostatic bonding attraction. This causes hydrogen to maintain some of its original residual orbital based potential. The extra potential left in the hydrogen of liquid water, ionize metallic electrons, catalyzing oxidation. In other words, metals will corrode much faster in low oxygen solubile water, than in high oxygen soluble dry air, due to the residual potential of the hydrogen of water acting as a catalyst. As we heat water the potential increases due to the electrostatic attraction expanding. Ice is not a good catalyst due to the potential of the hydrogen being low.

 

What is significant about the disproportionate potential within hydrogen bonding hydrogen, it that it is what defines the living state. In other words, hydrogen bonding is another layer of chemistry that sits on top of the covalent chemistry of bio-molecules and integrates the loose dynamics of life. It the basis for the properties of DNA, RNA, protein and water, and through hydration within water, the basis for the activity of all the small dissolved chemical and ions. What this means in practical terms is "the living state in one variable". I am not going to teach this for free. When you teach for free you get sh*t on. If you are paid people listen because it worth something. Sort of silly but thats how the game seems to work.

[Bluenoise]

Hydrogen bonds are more than a dipole potential between a hydrogen atom and the unbonded electrons of an highly electronegative atom. What makes hydrogen bonds unique is that the hydrogen goes into a hydrogen bond carrying the primary burden of the potential. The shared electrons will have a lower potential to form the hydrogen bond.

 

First of all a hydrogen bond isn't a dipole potential between hydrogen atoms and unbonded electrons. A hydrogen bond arrises from a dipole potential between hydrogen atoms and unbonded electrons. Secondly hydrogen doesn't carry the burden of the potential it releases the potential energy by forming a bond and satisfying the dipole potential.

 

you seem to have it mixxed up. Unbound hydrogen doner and acceptor have potential energy.

Bound hydrogen doner and acceptor have released the potential.

 

 

This anomaly can be understood by looking at the hydrogen bonding in water. A water molecule will have four hybrid sp3 orbitals. The hydrogen of water are bonded to two of these four orbitals. The other two hybrid orbitals are occupied by unshared electrons that participate in hydrogen bonding.

 

anomaly? what anomaly hydrogen bonding is very simple and very well understood.

 

The hybrid orbitals allow the covlantly bonded hydrogen to share electrons with the oxygen, but at a higher orbital distance due to the P-character of the hybrid orbitals. In other words, hydrogen is optimized for 1S orbitals, but is induced by the bond with oxygen to share electrons with a lot of P-character. This sort of ionizes the electrons shared by hydrogen away from its preferred 1S orbital. It still has electron density to balance most of its positive charge, but it is being held further away from its 1S orbtal than is optimum.

 

The oxygen, on the other hand, gains the electron density to become slightly negative, but these electron are placed in hybrid orbitals more in line with the octet and the p-orbital needs of oxygen, As such, although the charge dipole will balance, the hydrogen has a higher overall potential.

 

Data that supports this is connected to hydrogen bond energy dropping drastically with deviation from linear hydrogen bonding angles. In other words, if we maintain the distance between the hydrogen and shared electrons within a hydrogen bond, but only shift the bond angle, this should not affect a purely electrostatic attraction. In the case of hydrogen bonds, the angle deviation has more to do with losing the ability to line up orbitals. The linear arrangment allows the hydrogen to compensation for its p-character ionization. If we shift the angle, the hydrogen bond energy becomes more dependant on electrostatic attraction, which is not as effiecient for the hydrogen.

 

Another supporting observation is the contraction of water when it melts. The only other material in nature that does this is the metal Antimony. When water is ice the hydrogen bonds are linear and the potential of the hydrogen is minimized due to the p-orbital sharing with the unbonded electrons of oxygen. When we heat ice and cause it to melt, the oxygen will twist away. This alters the hydrogen bond angles causing the lower potential electrostatic force to have get much closer to lower the potential.

 

In liquid water the hydrogen would like to line up the oxygen for linear hydrogen bonds but often as to settle for the closer electrostatic bonding attraction. This causes hydrogen to maintain some of its original residual orbital based potential. The extra potential left in the hydrogen of liquid water, ionize metallic electrons, catalyzing oxidation. In other words, metals will corrode much faster in low oxygen solubile water, than in high oxygen soluble dry air, due to the residual potential of the hydrogen of water acting as a catalyst. As we heat water the potential increases due to the electrostatic attraction expanding. Ice is not a good catalyst due to the potential of the hydrogen being low.

 

What is significant about the disproportionate potential within hydrogen bonding hydrogen, it that it is what defines the living state. In other words, hydrogen bonding is another layer of chemistry that sits on top of the covalent chemistry of bio-molecules and integrates the loose dynamics of life. It the basis for the properties of DNA, RNA, protein and water, and through hydration within water, the basis for the activity of all the small dissolved chemical and ions. What this means in practical terms is "the living state in one variable".

 

ha ha ha ha ha ha

 

You think that unequal energy from hydrogen bonding in varying angles can explain the living state!!!! ha ha ah ah ah ah ah ha ha ha ha ha ha ha ha ha ha

 

oh wait I need to breath

 

ha ha ha ha ha ha ha ha ha ha ha ha ha

 

Listen here a puddle of water forms transient hydrogen bonds at varying angles but it is not alive. So thinking that you can reduce life to one simple interaction is just ... ha ha ha ha ha ha ha ha ha ha ha

 

I am not going to teach this for free. When you teach for free you get sh*t on. If you are paid people listen because it worth something. Sort of silly but thats how the game seems to work.

 

Why do you think that someone would want to pay to listen to your convoluted confusing explainations on an incredibly simple subject that you obviously don't understand yourself.

 

 

Honestly sunspot why do you seem to thing that everything revolves around hydrogen bonding? Like did the god of hydrogen bonding come to you in a dream and tell you to try to start a cult around hydrogen bonding?