Difference in Basic Amino Structures
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I'm having a hard time understanding why my slides in my biology course have two different representations of the "basic structure" of the amino acid:
1:
2:
The top one seem like what I would expect. The bottom one, it looks like the amine group gained a Hydrogen ion and the Carboxyl group lost one. Also, the center carbon gained an H. I honestly don't know if this description is even correct or not.
I'm extremely new to this level of biology, so very simple explanations are much appreciated. I just don't totally understand why there are two versions of the basic structure.
Also, I apologize if the tag is wrong, again, this isn't my major, so I'm very new to this material.
biochemistry
asked 12 hours ago
joe_04_04joe_04_04
1234
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add a comment |
$begingroup$
I'm having a hard time understanding why my slides in my biology course have two different representations of the "basic structure" of the amino acid:
1:
2:
The top one seem like what I would expect. The bottom one, it looks like the amine group gained a Hydrogen ion and the Carboxyl group lost one. Also, the center carbon gained an H. I honestly don't know if this description is even correct or not.
I'm extremely new to this level of biology, so very simple explanations are much appreciated. I just don't totally understand why there are two versions of the basic structure.
Also, I apologize if the tag is wrong, again, this isn't my major, so I'm very new to this material.
biochemistry
asked 12 hours ago
joe_04_04joe_04_04
1234
New contributor
joe_04_04 is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
Check out our Code of Conduct.
$endgroup$
$begingroup$
Ugly pictures in both cases :)
$endgroup$
– Alchimista
10 hours ago
add a comment |
$begingroup$
I'm having a hard time understanding why my slides in my biology course have two different representations of the "basic structure" of the amino acid:
1:
2:
The top one seem like what I would expect. The bottom one, it looks like the amine group gained a Hydrogen ion and the Carboxyl group lost one. Also, the center carbon gained an H. I honestly don't know if this description is even correct or not.
I'm extremely new to this level of biology, so very simple explanations are much appreciated. I just don't totally understand why there are two versions of the basic structure.
Also, I apologize if the tag is wrong, again, this isn't my major, so I'm very new to this material.
biochemistry
asked 12 hours ago
joe_04_04joe_04_04
1234
New contributor
joe_04_04 is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
Check out our Code of Conduct.
$endgroup$
I'm having a hard time understanding why my slides in my biology course have two different representations of the "basic structure" of the amino acid:
1:
2:
The top one seem like what I would expect. The bottom one, it looks like the amine group gained a Hydrogen ion and the Carboxyl group lost one. Also, the center carbon gained an H. I honestly don't know if this description is even correct or not.
I'm extremely new to this level of biology, so very simple explanations are much appreciated. I just don't totally understand why there are two versions of the basic structure.
Also, I apologize if the tag is wrong, again, this isn't my major, so I'm very new to this material.
biochemistry
biochemistry
asked 12 hours ago
joe_04_04joe_04_04
1234
New contributor
joe_04_04 is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
Check out our Code of Conduct.
asked 12 hours ago
joe_04_04joe_04_04
1234
New contributor
joe_04_04 is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
Check out our Code of Conduct.
asked 12 hours ago
joe_04_04joe_04_04
1234
New contributor
joe_04_04 is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
Check out our Code of Conduct.
asked 12 hours ago
joe_04_04joe_04_04
1234
asked 12 hours ago
joe_04_04joe_04_04
1234
1234
New contributor
joe_04_04 is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
Check out our Code of Conduct.
New contributor
joe_04_04 is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
Check out our Code of Conduct.
joe_04_04 is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
Check out our Code of Conduct.
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Ugly pictures in both cases :)
$endgroup$
– Alchimista
10 hours ago
add a comment |
$begingroup$
Ugly pictures in both cases :)
$endgroup$
– Alchimista
10 hours ago
$begingroup$
Ugly pictures in both cases :)
$endgroup$
– Alchimista
10 hours ago
$begingroup$
Ugly pictures in both cases :)
$endgroup$
– Alchimista
10 hours ago
add a comment |
1 Answer
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Your description is more or less correct, but so are both images. The bottom images shows the predominant form the amino acid would take at neutral pH (or any pH between ~2 and ~9.5). This is because the caroboxylic acid (-COOH) and amino (-NH2) groups are a weak acid and base and can lose or gain a proton (hydrogen cation), respectively. pH below the pKa of the functional group (~2 for carboxylic acid and ~9.5 for amino) favours protonation whereas pH above the pKa favours deprotonation. Also note that the "centre carbon" (the α-carbon) did not gain a proton in the second image, it's just drawn differently.
You could try this website for an overview of acid/base chemistry and perhaps these Wikipedia sections on zwitterions and isoelectric points with respect to amino acids, though there are many alternative sources of material available if you search for them. This question and answer may also be useful for you, at least eventually.
answered 11 hours ago
canadianercanadianer
14.7k43374
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To expand slightly on this answer, this is valid for these sorts of chemical structures more generally in organic chemistry, too. When you see groups like these that act as weak acids/bases, you should think of them existing chemically in both forms, with the ratio dependent on the pH. People will switch back and forth between them freely because that's how the molecules actually exist, as well.
$endgroup$
– Bryan Krause
11 hours ago
add a comment |
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1 Answer
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$begingroup$
Your description is more or less correct, but so are both images. The bottom images shows the predominant form the amino acid would take at neutral pH (or any pH between ~2 and ~9.5). This is because the caroboxylic acid (-COOH) and amino (-NH2) groups are a weak acid and base and can lose or gain a proton (hydrogen cation), respectively. pH below the pKa of the functional group (~2 for carboxylic acid and ~9.5 for amino) favours protonation whereas pH above the pKa favours deprotonation. Also note that the "centre carbon" (the α-carbon) did not gain a proton in the second image, it's just drawn differently.
You could try this website for an overview of acid/base chemistry and perhaps these Wikipedia sections on zwitterions and isoelectric points with respect to amino acids, though there are many alternative sources of material available if you search for them. This question and answer may also be useful for you, at least eventually.
answered 11 hours ago
canadianercanadianer
14.7k43374
$endgroup$
$begingroup$
To expand slightly on this answer, this is valid for these sorts of chemical structures more generally in organic chemistry, too. When you see groups like these that act as weak acids/bases, you should think of them existing chemically in both forms, with the ratio dependent on the pH. People will switch back and forth between them freely because that's how the molecules actually exist, as well.
$endgroup$
– Bryan Krause
11 hours ago
add a comment |
$begingroup$
Your description is more or less correct, but so are both images. The bottom images shows the predominant form the amino acid would take at neutral pH (or any pH between ~2 and ~9.5). This is because the caroboxylic acid (-COOH) and amino (-NH2) groups are a weak acid and base and can lose or gain a proton (hydrogen cation), respectively. pH below the pKa of the functional group (~2 for carboxylic acid and ~9.5 for amino) favours protonation whereas pH above the pKa favours deprotonation. Also note that the "centre carbon" (the α-carbon) did not gain a proton in the second image, it's just drawn differently.
You could try this website for an overview of acid/base chemistry and perhaps these Wikipedia sections on zwitterions and isoelectric points with respect to amino acids, though there are many alternative sources of material available if you search for them. This question and answer may also be useful for you, at least eventually.
answered 11 hours ago
canadianercanadianer
14.7k43374
$endgroup$
$begingroup$
To expand slightly on this answer, this is valid for these sorts of chemical structures more generally in organic chemistry, too. When you see groups like these that act as weak acids/bases, you should think of them existing chemically in both forms, with the ratio dependent on the pH. People will switch back and forth between them freely because that's how the molecules actually exist, as well.
$endgroup$
– Bryan Krause
11 hours ago
add a comment |
$begingroup$
Your description is more or less correct, but so are both images. The bottom images shows the predominant form the amino acid would take at neutral pH (or any pH between ~2 and ~9.5). This is because the caroboxylic acid (-COOH) and amino (-NH2) groups are a weak acid and base and can lose or gain a proton (hydrogen cation), respectively. pH below the pKa of the functional group (~2 for carboxylic acid and ~9.5 for amino) favours protonation whereas pH above the pKa favours deprotonation. Also note that the "centre carbon" (the α-carbon) did not gain a proton in the second image, it's just drawn differently.
You could try this website for an overview of acid/base chemistry and perhaps these Wikipedia sections on zwitterions and isoelectric points with respect to amino acids, though there are many alternative sources of material available if you search for them. This question and answer may also be useful for you, at least eventually.
answered 11 hours ago
canadianercanadianer
14.7k43374
$endgroup$
Your description is more or less correct, but so are both images. The bottom images shows the predominant form the amino acid would take at neutral pH (or any pH between ~2 and ~9.5). This is because the caroboxylic acid (-COOH) and amino (-NH2) groups are a weak acid and base and can lose or gain a proton (hydrogen cation), respectively. pH below the pKa of the functional group (~2 for carboxylic acid and ~9.5 for amino) favours protonation whereas pH above the pKa favours deprotonation. Also note that the "centre carbon" (the α-carbon) did not gain a proton in the second image, it's just drawn differently.
You could try this website for an overview of acid/base chemistry and perhaps these Wikipedia sections on zwitterions and isoelectric points with respect to amino acids, though there are many alternative sources of material available if you search for them. This question and answer may also be useful for you, at least eventually.
answered 11 hours ago
canadianercanadianer
14.7k43374
answered 11 hours ago
canadianercanadianer
14.7k43374
answered 11 hours ago
canadianercanadianer
14.7k43374
answered 11 hours ago
canadianercanadianer
14.7k43374
14.7k43374
$begingroup$
To expand slightly on this answer, this is valid for these sorts of chemical structures more generally in organic chemistry, too. When you see groups like these that act as weak acids/bases, you should think of them existing chemically in both forms, with the ratio dependent on the pH. People will switch back and forth between them freely because that's how the molecules actually exist, as well.
$endgroup$
– Bryan Krause
11 hours ago
add a comment |
$begingroup$
To expand slightly on this answer, this is valid for these sorts of chemical structures more generally in organic chemistry, too. When you see groups like these that act as weak acids/bases, you should think of them existing chemically in both forms, with the ratio dependent on the pH. People will switch back and forth between them freely because that's how the molecules actually exist, as well.
$endgroup$
– Bryan Krause
11 hours ago
$begingroup$
To expand slightly on this answer, this is valid for these sorts of chemical structures more generally in organic chemistry, too. When you see groups like these that act as weak acids/bases, you should think of them existing chemically in both forms, with the ratio dependent on the pH. People will switch back and forth between them freely because that's how the molecules actually exist, as well.
$endgroup$
– Bryan Krause
11 hours ago
$begingroup$
To expand slightly on this answer, this is valid for these sorts of chemical structures more generally in organic chemistry, too. When you see groups like these that act as weak acids/bases, you should think of them existing chemically in both forms, with the ratio dependent on the pH. People will switch back and forth between them freely because that's how the molecules actually exist, as well.
$endgroup$
– Bryan Krause
11 hours ago
add a comment |
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$begingroup$
Ugly pictures in both cases :)
$endgroup$
– Alchimista
10 hours ago