Mixing
Can =NH2+ in Arginine's side chain form hydrogen bonding at physiological pH?
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I know that at physiological pH, Arginine will have its $ce{=NH}$ protonated to $ce{=NH2+}$. I was wondering if this $ce{=NH2+}$ can still form a hydrogen bond by being a donor? And does the positive charge on Nitrogen affect the hydrogen bonding's strength? My confusion stems from the definition of hydrogen bonding, which says that hydrogen's electron cloud needs to be withdrawn by a more electronegative atom like $ce{F, O, N}$ to be partially positive enough to participate. Therefore, I believe that the positively charged N will withdraw electrons from hydrogens more strongly, leading to more partially positively charged hydrogen and eventually stronger H-bonding with another molecule. Could someone please verify this for me?
Moreover, I have seen $ce{=O}$ and $ce{=N}$ forming hydrogen bonding by being an acceptor. However, I tried search but did not find any example of $ce{=NH3+}$ or $ce{=NH2R+}$ or NHR2+ forming hydrogen bonding as a donor. So can a Nitrogen with a double bond still participate in hydrogen bonding as a donor?
hydrogen-bond proteins amino-acids
edited Jan 13 at 20:42
A.K.
9,03452366
asked Jan 13 at 17:34
EllBe EllBe
313
$endgroup$
add a comment |
$begingroup$
I know that at physiological pH, Arginine will have its $ce{=NH}$ protonated to $ce{=NH2+}$. I was wondering if this $ce{=NH2+}$ can still form a hydrogen bond by being a donor? And does the positive charge on Nitrogen affect the hydrogen bonding's strength? My confusion stems from the definition of hydrogen bonding, which says that hydrogen's electron cloud needs to be withdrawn by a more electronegative atom like $ce{F, O, N}$ to be partially positive enough to participate. Therefore, I believe that the positively charged N will withdraw electrons from hydrogens more strongly, leading to more partially positively charged hydrogen and eventually stronger H-bonding with another molecule. Could someone please verify this for me?
Moreover, I have seen $ce{=O}$ and $ce{=N}$ forming hydrogen bonding by being an acceptor. However, I tried search but did not find any example of $ce{=NH3+}$ or $ce{=NH2R+}$ or NHR2+ forming hydrogen bonding as a donor. So can a Nitrogen with a double bond still participate in hydrogen bonding as a donor?
hydrogen-bond proteins amino-acids
edited Jan 13 at 20:42
A.K.
9,03452366
asked Jan 13 at 17:34
EllBe EllBe
313
$endgroup$
$begingroup$
Welcome to Chemistry.SE! Please note that formulas can be better expressed with $ce{ }$ for chemical formulas/equations, $ $ for math term/equations, and $pu{ }$ for units. More information is available in this meta post Also, take a minute to look over the help center and tour page to better understand our guidelines and question policies if you haven't already.
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– A.K.
Jan 13 at 20:42
add a comment |
$begingroup$
I know that at physiological pH, Arginine will have its $ce{=NH}$ protonated to $ce{=NH2+}$. I was wondering if this $ce{=NH2+}$ can still form a hydrogen bond by being a donor? And does the positive charge on Nitrogen affect the hydrogen bonding's strength? My confusion stems from the definition of hydrogen bonding, which says that hydrogen's electron cloud needs to be withdrawn by a more electronegative atom like $ce{F, O, N}$ to be partially positive enough to participate. Therefore, I believe that the positively charged N will withdraw electrons from hydrogens more strongly, leading to more partially positively charged hydrogen and eventually stronger H-bonding with another molecule. Could someone please verify this for me?
Moreover, I have seen $ce{=O}$ and $ce{=N}$ forming hydrogen bonding by being an acceptor. However, I tried search but did not find any example of $ce{=NH3+}$ or $ce{=NH2R+}$ or NHR2+ forming hydrogen bonding as a donor. So can a Nitrogen with a double bond still participate in hydrogen bonding as a donor?
hydrogen-bond proteins amino-acids
edited Jan 13 at 20:42
A.K.
9,03452366
asked Jan 13 at 17:34
EllBe EllBe
313
$endgroup$
I know that at physiological pH, Arginine will have its $ce{=NH}$ protonated to $ce{=NH2+}$. I was wondering if this $ce{=NH2+}$ can still form a hydrogen bond by being a donor? And does the positive charge on Nitrogen affect the hydrogen bonding's strength? My confusion stems from the definition of hydrogen bonding, which says that hydrogen's electron cloud needs to be withdrawn by a more electronegative atom like $ce{F, O, N}$ to be partially positive enough to participate. Therefore, I believe that the positively charged N will withdraw electrons from hydrogens more strongly, leading to more partially positively charged hydrogen and eventually stronger H-bonding with another molecule. Could someone please verify this for me?
Moreover, I have seen $ce{=O}$ and $ce{=N}$ forming hydrogen bonding by being an acceptor. However, I tried search but did not find any example of $ce{=NH3+}$ or $ce{=NH2R+}$ or NHR2+ forming hydrogen bonding as a donor. So can a Nitrogen with a double bond still participate in hydrogen bonding as a donor?
hydrogen-bond proteins amino-acids
hydrogen-bond proteins amino-acids
edited Jan 13 at 20:42
A.K.
9,03452366
asked Jan 13 at 17:34
EllBe EllBe
313
edited Jan 13 at 20:42
A.K.
9,03452366
asked Jan 13 at 17:34
EllBe EllBe
313
edited Jan 13 at 20:42
A.K.
9,03452366
edited Jan 13 at 20:42
A.K.
9,03452366
edited Jan 13 at 20:42
A.K.
9,03452366
9,03452366
asked Jan 13 at 17:34
EllBe EllBe
313
asked Jan 13 at 17:34
EllBe EllBe
313
asked Jan 13 at 17:34
EllBe EllBe
313
313
$begingroup$
Welcome to Chemistry.SE! Please note that formulas can be better expressed with $ce{ }$ for chemical formulas/equations, $ $ for math term/equations, and $pu{ }$ for units. More information is available in this meta post Also, take a minute to look over the help center and tour page to better understand our guidelines and question policies if you haven't already.
$endgroup$
– A.K.
Jan 13 at 20:42
add a comment |
$begingroup$
Welcome to Chemistry.SE! Please note that formulas can be better expressed with $ce{ }$ for chemical formulas/equations, $ $ for math term/equations, and $pu{ }$ for units. More information is available in this meta post Also, take a minute to look over the help center and tour page to better understand our guidelines and question policies if you haven't already.
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– A.K.
Jan 13 at 20:42
$begingroup$
Welcome to Chemistry.SE! Please note that formulas can be better expressed with $ce{ }$ for chemical formulas/equations, $ $ for math term/equations, and $pu{ }$ for units. More information is available in this meta post Also, take a minute to look over the help center and tour page to better understand our guidelines and question policies if you haven't already.
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– A.K.
Jan 13 at 20:42
$begingroup$
Welcome to Chemistry.SE! Please note that formulas can be better expressed with $ce{ }$ for chemical formulas/equations, $ $ for math term/equations, and $pu{ }$ for units. More information is available in this meta post Also, take a minute to look over the help center and tour page to better understand our guidelines and question policies if you haven't already.
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– A.K.
Jan 13 at 20:42
add a comment |
1 Answer
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Yes, the arginine side chain is an excellent hydrogen bond donor. Charged N-H groups are even better hydrogen bond donors than the corresponding neutral N-H groups. Here is an article that gives examples of arginine side chains in hydrogen bonds. It showcases bidendate hydrogen bonds (i.e. two hydrogen bonds from the arginine side chain) with carboxylates and with nitrogenous bases of nucleic acids.
Specifically for proteins, if the hydrogen bond donor is positively charged (e.g. Arg+) and the hydrogen bond acceptor is negatively charged (e.g. Glu-), you have a combination of ionic and hydrogen bond interaction, which is particularly strong. It is often referred to as a salt bridge, such as in this example. If you take a close look at the arginine side chain, you will see that it is protonated (i.e. positively charged) and interacts with two negatively charged carboxylate groups.
answered Jan 13 at 18:16
Karsten TheisKarsten Theis
1,680323
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1 Answer
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$begingroup$
Yes, the arginine side chain is an excellent hydrogen bond donor. Charged N-H groups are even better hydrogen bond donors than the corresponding neutral N-H groups. Here is an article that gives examples of arginine side chains in hydrogen bonds. It showcases bidendate hydrogen bonds (i.e. two hydrogen bonds from the arginine side chain) with carboxylates and with nitrogenous bases of nucleic acids.
Specifically for proteins, if the hydrogen bond donor is positively charged (e.g. Arg+) and the hydrogen bond acceptor is negatively charged (e.g. Glu-), you have a combination of ionic and hydrogen bond interaction, which is particularly strong. It is often referred to as a salt bridge, such as in this example. If you take a close look at the arginine side chain, you will see that it is protonated (i.e. positively charged) and interacts with two negatively charged carboxylate groups.
answered Jan 13 at 18:16
Karsten TheisKarsten Theis
1,680323
$endgroup$
add a comment |
$begingroup$
Yes, the arginine side chain is an excellent hydrogen bond donor. Charged N-H groups are even better hydrogen bond donors than the corresponding neutral N-H groups. Here is an article that gives examples of arginine side chains in hydrogen bonds. It showcases bidendate hydrogen bonds (i.e. two hydrogen bonds from the arginine side chain) with carboxylates and with nitrogenous bases of nucleic acids.
Specifically for proteins, if the hydrogen bond donor is positively charged (e.g. Arg+) and the hydrogen bond acceptor is negatively charged (e.g. Glu-), you have a combination of ionic and hydrogen bond interaction, which is particularly strong. It is often referred to as a salt bridge, such as in this example. If you take a close look at the arginine side chain, you will see that it is protonated (i.e. positively charged) and interacts with two negatively charged carboxylate groups.
answered Jan 13 at 18:16
Karsten TheisKarsten Theis
1,680323
$endgroup$
add a comment |
$begingroup$
Yes, the arginine side chain is an excellent hydrogen bond donor. Charged N-H groups are even better hydrogen bond donors than the corresponding neutral N-H groups. Here is an article that gives examples of arginine side chains in hydrogen bonds. It showcases bidendate hydrogen bonds (i.e. two hydrogen bonds from the arginine side chain) with carboxylates and with nitrogenous bases of nucleic acids.
Specifically for proteins, if the hydrogen bond donor is positively charged (e.g. Arg+) and the hydrogen bond acceptor is negatively charged (e.g. Glu-), you have a combination of ionic and hydrogen bond interaction, which is particularly strong. It is often referred to as a salt bridge, such as in this example. If you take a close look at the arginine side chain, you will see that it is protonated (i.e. positively charged) and interacts with two negatively charged carboxylate groups.
answered Jan 13 at 18:16
Karsten TheisKarsten Theis
1,680323
$endgroup$
Yes, the arginine side chain is an excellent hydrogen bond donor. Charged N-H groups are even better hydrogen bond donors than the corresponding neutral N-H groups. Here is an article that gives examples of arginine side chains in hydrogen bonds. It showcases bidendate hydrogen bonds (i.e. two hydrogen bonds from the arginine side chain) with carboxylates and with nitrogenous bases of nucleic acids.
Specifically for proteins, if the hydrogen bond donor is positively charged (e.g. Arg+) and the hydrogen bond acceptor is negatively charged (e.g. Glu-), you have a combination of ionic and hydrogen bond interaction, which is particularly strong. It is often referred to as a salt bridge, such as in this example. If you take a close look at the arginine side chain, you will see that it is protonated (i.e. positively charged) and interacts with two negatively charged carboxylate groups.
answered Jan 13 at 18:16
Karsten TheisKarsten Theis
1,680323
edited Jan 13 at 22:53
answered Jan 13 at 18:16
Karsten TheisKarsten Theis
1,680323
answered Jan 13 at 18:16
Karsten TheisKarsten Theis
1,680323
answered Jan 13 at 18:16
Karsten TheisKarsten Theis
1,680323
1,680323
add a comment |
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$begingroup$
Welcome to Chemistry.SE! Please note that formulas can be better expressed with $ce{ }$ for chemical formulas/equations, $ $ for math term/equations, and $pu{ }$ for units. More information is available in this meta post Also, take a minute to look over the help center and tour page to better understand our guidelines and question policies if you haven't already.
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– A.K.
Jan 13 at 20:42