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Flame test color for non-ionic compounds
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$begingroup$
What color would a non-ionic compound, such as $ce{NH4OH}$ or $ce{HCl}$, produce in a flame test? Is no color produced, or is it different for each compound?
analytical-chemistry identification
edited 1 hour ago
andselisk
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asked 3 hours ago
xXGETREKTXxxXGETREKTXx
61
New contributor
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$endgroup$
add a comment |
$begingroup$
What color would a non-ionic compound, such as $ce{NH4OH}$ or $ce{HCl}$, produce in a flame test? Is no color produced, or is it different for each compound?
analytical-chemistry identification
edited 1 hour ago
andselisk
20.8k770136
asked 3 hours ago
xXGETREKTXxxXGETREKTXx
61
New contributor
xXGETREKTXx is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
Check out our Code of Conduct.
$endgroup$
1
$begingroup$
I'm confused. I would consider both $ce{NH4OH}$ and $ce{HCl}$ to be ionic compounds.
$endgroup$
– MaxW
1 hour ago
add a comment |
$begingroup$
What color would a non-ionic compound, such as $ce{NH4OH}$ or $ce{HCl}$, produce in a flame test? Is no color produced, or is it different for each compound?
analytical-chemistry identification
edited 1 hour ago
andselisk
20.8k770136
asked 3 hours ago
xXGETREKTXxxXGETREKTXx
61
New contributor
xXGETREKTXx is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
Check out our Code of Conduct.
$endgroup$
What color would a non-ionic compound, such as $ce{NH4OH}$ or $ce{HCl}$, produce in a flame test? Is no color produced, or is it different for each compound?
analytical-chemistry identification
analytical-chemistry identification
edited 1 hour ago
andselisk
20.8k770136
asked 3 hours ago
xXGETREKTXxxXGETREKTXx
61
New contributor
xXGETREKTXx is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
Check out our Code of Conduct.
edited 1 hour ago
andselisk
20.8k770136
asked 3 hours ago
xXGETREKTXxxXGETREKTXx
61
New contributor
xXGETREKTXx is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
Check out our Code of Conduct.
edited 1 hour ago
andselisk
20.8k770136
edited 1 hour ago
andselisk
20.8k770136
edited 1 hour ago
andselisk
20.8k770136
20.8k770136
asked 3 hours ago
xXGETREKTXxxXGETREKTXx
61
New contributor
xXGETREKTXx is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
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asked 3 hours ago
xXGETREKTXxxXGETREKTXx
61
asked 3 hours ago
xXGETREKTXxxXGETREKTXx
61
61
New contributor
xXGETREKTXx is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
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New contributor
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1
$begingroup$
I'm confused. I would consider both $ce{NH4OH}$ and $ce{HCl}$ to be ionic compounds.
$endgroup$
– MaxW
1 hour ago
add a comment |
1
$begingroup$
I'm confused. I would consider both $ce{NH4OH}$ and $ce{HCl}$ to be ionic compounds.
$endgroup$
– MaxW
1 hour ago
1
1
$begingroup$
I'm confused. I would consider both $ce{NH4OH}$ and $ce{HCl}$ to be ionic compounds.
$endgroup$
– MaxW
1 hour ago
$begingroup$
I'm confused. I would consider both $ce{NH4OH}$ and $ce{HCl}$ to be ionic compounds.
$endgroup$
– MaxW
1 hour ago
add a comment |
1 Answer
1
active
oldest
votes
$begingroup$
Flame emission (or better atomic emission) does not care whether your starting compound was ionic or not. Everything decomposes into flame either into atoms or very simple molecules. The blue color you see from the flame is also from very small molecules which exist in the flame.
https://en.wikipedia.org/wiki/File:Spectrum_of_blue_flame.png
Ordinary flame like the Bunsen burner is way too cold for non-metals. However if we were to heat HCl or ammonium hydroxide in a confined "container", eventually you would start to see atomic emission from hydrogen, oxygen, nitrogen and chlorine. Most of the non-metal emission (p-block) lies in the UV or deep UV. You won't be able to see anything with bare eyes.
answered 1 hour ago
M. FarooqM. Farooq
2,825316
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$begingroup$
Flame emission (or better atomic emission) does not care whether your starting compound was ionic or not. Everything decomposes into flame either into atoms or very simple molecules. The blue color you see from the flame is also from very small molecules which exist in the flame.
https://en.wikipedia.org/wiki/File:Spectrum_of_blue_flame.png
Ordinary flame like the Bunsen burner is way too cold for non-metals. However if we were to heat HCl or ammonium hydroxide in a confined "container", eventually you would start to see atomic emission from hydrogen, oxygen, nitrogen and chlorine. Most of the non-metal emission (p-block) lies in the UV or deep UV. You won't be able to see anything with bare eyes.
answered 1 hour ago
M. FarooqM. Farooq
2,825316
$endgroup$
add a comment |
$begingroup$
Flame emission (or better atomic emission) does not care whether your starting compound was ionic or not. Everything decomposes into flame either into atoms or very simple molecules. The blue color you see from the flame is also from very small molecules which exist in the flame.
https://en.wikipedia.org/wiki/File:Spectrum_of_blue_flame.png
Ordinary flame like the Bunsen burner is way too cold for non-metals. However if we were to heat HCl or ammonium hydroxide in a confined "container", eventually you would start to see atomic emission from hydrogen, oxygen, nitrogen and chlorine. Most of the non-metal emission (p-block) lies in the UV or deep UV. You won't be able to see anything with bare eyes.
answered 1 hour ago
M. FarooqM. Farooq
2,825316
$endgroup$
add a comment |
$begingroup$
Flame emission (or better atomic emission) does not care whether your starting compound was ionic or not. Everything decomposes into flame either into atoms or very simple molecules. The blue color you see from the flame is also from very small molecules which exist in the flame.
https://en.wikipedia.org/wiki/File:Spectrum_of_blue_flame.png
Ordinary flame like the Bunsen burner is way too cold for non-metals. However if we were to heat HCl or ammonium hydroxide in a confined "container", eventually you would start to see atomic emission from hydrogen, oxygen, nitrogen and chlorine. Most of the non-metal emission (p-block) lies in the UV or deep UV. You won't be able to see anything with bare eyes.
answered 1 hour ago
M. FarooqM. Farooq
2,825316
$endgroup$
Flame emission (or better atomic emission) does not care whether your starting compound was ionic or not. Everything decomposes into flame either into atoms or very simple molecules. The blue color you see from the flame is also from very small molecules which exist in the flame.
https://en.wikipedia.org/wiki/File:Spectrum_of_blue_flame.png
Ordinary flame like the Bunsen burner is way too cold for non-metals. However if we were to heat HCl or ammonium hydroxide in a confined "container", eventually you would start to see atomic emission from hydrogen, oxygen, nitrogen and chlorine. Most of the non-metal emission (p-block) lies in the UV or deep UV. You won't be able to see anything with bare eyes.
answered 1 hour ago
M. FarooqM. Farooq
2,825316
answered 1 hour ago
M. FarooqM. Farooq
2,825316
answered 1 hour ago
M. FarooqM. Farooq
2,825316
answered 1 hour ago
M. FarooqM. Farooq
2,825316
2,825316
add a comment |
add a comment |
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1
$begingroup$
I'm confused. I would consider both $ce{NH4OH}$ and $ce{HCl}$ to be ionic compounds.
$endgroup$
– MaxW
1 hour ago