Name: flame test metal color clues
Uploaded: 2020-03-26T07:22:25.000Z
Duration: 2 min 47 s
Channel: JoVE

K12 Standards

Texas Essential Knowledge and Skills

High School

Chemistry and Physics

IPC.7

IPC.7.E

Metal Flame Emission

Die Flammenprüfung ist eine Analysetechnik, bei der eine Probe auf eine Flamme aufgebracht wird und das charakteristische Emissionsspektrum zur Identifizierung verschiedener Elemente verwendet wird. Wenn diese Technik zur Identifizierung von Metallspezies verwendet wird, wird sie als Metallflammenemissionsprüfung bezeichnet. Wenn einigen Metallen durch eine heiße Flamme ausreichend Energie zugeführt wird, emittieren sie Licht mit einer charakteristischen Wellenlänge oder Farbe. Sie können dieses Phänomen deutlich erkennen, wenn Sie sich ein Feuerwerk ansehen.
Unterschiedliche Metalle geben unterschiedliche Farben ab. So können wir die Farbe des emittierten Lichts verwenden, um das vorhandene Metall zu bestimmen. Aber bevor wir weiter in die Technik eintauchen, gehen wir einen Schritt zurück. Atome haben mehrere Energieniveaus für ihre Elektronen, die für jedes Element unterschiedlich sind.
Wenn sich ein Elektron auf seinem niedrigstmöglichen Energieniveau befindet, spricht man davon, dass es sich in seinem Grundzustand befindet. Wenn ein Atom Energie absorbiert, wird es angeregt, und die Elektronen im Atom bewegen sich aus dem Grundzustand auf ein höheres Energieniveau. Wenn sich die Elektronen wieder in einen niedrigeren Zustand, den Grundzustand, entspannen, wird die gewonnene überschüssige Energie in Form von emittiertem Licht freigesetzt.
Die Wellenlänge des emittierten Lichts hängt von dem Energieniveau ab, auf das das Elektron angeregt wurde, und dem Niveau, auf das es sich wieder entspannt. Diese emittierte Wellenlänge oder Lichtfarbe ist spezifisch für das vorhandene Atom und wird verwendet, um eine Metallprobe im Metallflammenemissionstest zu identifizieren.
Beim Metallflammenemissionstest tragen wir eine Metallprobe auf eine heiße Flamme auf und beobachten die Farbe des emittierten Lichts. Zum Beispiel gibt Barium in der Flamme eine gelblich-grüne Farbe ab, während Kupfer blaugrün und Kalium rosa-violett abgibt.
Nun besteht eine Probe tatsächlich aus dem Metall, Metallionen, Metalloxiden, Metallhydroxiden und Metallsalzen. Und da Atome und Moleküle unterschiedlich Energie aufnehmen und abgeben, enthält das emittierte Licht tatsächlich eine Reihe von Wellenlängen und Intensitäten, die ein Emissionsspektrum bilden.
Ein Spektralphotometer wird verwendet, um den Wellenlängenbereich des emittierten Lichts zu messen. 
In diesem Labor verwenden Sie den Flammenemissionstest von Metallen, um verschiedene Metalle zu identifizieren und dann das emittierte und absorbierte Licht mit einem Spektralphotometer zu analysieren.

emission von metallflammen

<h4>Emission von Metallflammen</h4>
Die Flammenprüfung ist eine Analysetechnik, bei der eine Probe in eine Flamme gelegt wird und die charakteristische Flammenfarbe zur Identifizierung der Substanz verwendet wird. Jedes Element hat eine charakteristische Lichtemission, wenn es in eine Flamme gelegt wird, was bedeutet, dass jedes Element eine einzigartige Farbe erzeugt. Dieses Phänomen wird bei Feuerwerken genutzt, bei denen die Farbe des Feuerwerkskörpers einer bestimmten Eigenschaft eines Metalls entspricht. Die Emission von farbigem Licht aus einer brennenden Probe ist das direkte Ergebnis der Energieabsorption des metallischen Bauteils aufgrund der Anregung durch die Flamme und der Emission von Licht.
<h4>Elektronen-Aufregung</h4>
Wenn eine atomare oder molekulare Spezies Energie absorbiert, wird die Energie auf vier verschiedene Arten genutzt. Zunächst wird die Energie in der Translation genutzt, wodurch sich die Moleküle schneller bewegen. Zweitens wird die Energie in Schwingung umgewandelt, wodurch sich der Abstand zwischen den Spezies schnell ändert. Drittens bewirkt die Energie eine Rotation, die die Rotation der Atome um die Bindungen im Molekül induziert. Schließlich führt die absorbierte Energie zu einer Elektronenanregung, die dazu führt, dass sich die Elektronen aus dem stabilsten Zustand oder Grundzustand auf ein höheres Energieniveau bewegen.
Nach dem Bohrschen Modell des Wasserstoffs existieren Elektronen in einem Atom in diskreten Zuständen, die einzelnen Schalen oder Orbitalen um den Kern entsprechen. Der niedrigste Energiezustand wird als Grundzustand bezeichnet und durch die Notation von n = 1 dargestellt. Angeregte Energiezustände haben höhere Energien und werden durch die Notation von n = 2, 3, 4 usw. dargestellt.
Damit Elektronen in einen höheren Energiezustand gelangen können, müssen sie eine Energiemenge absorbieren, die der Differenz zwischen ihrem Grundzustand und dem höheren Energiezustand entspricht. Wenn ein Elektron beispielsweise eine Energiemenge absorbiert, die der Differenz zwischen dem Grundzustand und dem Energieniveau von n=3 entspricht, bewegt sich das Elektron auf das Energieniveau von n=3. Ein Elektron kann sich spontan wieder in den Grundzustand oder ein anderes niedrigeres Energieniveau entspannen. In diesem Fall wird ein Photon emittiert, das die absorbierte Energie freisetzt.
Die freigesetzte Energie wird in Form von Licht abgegeben. Das emittierte Licht hat eine charakteristische Energie und damit Wellenlänge, die mit den Energieniveaus des Atoms korreliert. Sichtbares Licht, also das Licht, das der Mensch mit seinen Augen sehen kann, reicht von etwa 400 nm bis 700 nm im elektromagnetischen Spektrum.
Atomare Absorptionen und Emissionen sind diskrete Wellenlängen, die als Linien bezeichnet werden. Diese Linien sind einzigartige Merkmale eines Elements, wie z. B. ein Barcode, und können zur Identifizierung des Elements verwendet werden.
<h4>Emissionstest für Metallflammen</h4>
Bei der Prüfung der Flammenemission von Metallen wird eine Metallprobe in eine Flamme gelegt. Die Flamme liefert die Energie, um Elektronen auf ein höheres Energieniveau anzuregen. Wenn sich die Elektronen wieder in den Grundzustand entspannen, wird Licht mit einer spezifischen Energie emittiert, die relativ zu den Energieniveaus der Atome in der Probe ist. Da verschiedene Atome unterschiedliche Energieniveaus haben, ist die von einer Probe absorbierte und abgegebene Energie und damit die Wellenlänge spezifisch für die Probe.
Metalle haben charakteristische atomare Emissionswellenlängen im sichtbaren Bereich, die durch visuelle Inspektion leicht bestimmt werden können. Zum Beispiel hat Lithium eine rote Farbe, Natrium eine gelbe Farbe, Kalium eine rosa-violette Farbe und Barium eine gelbgrüne Farbe.
Während atomare Emissionen diskrete Wellenlängen oder Linien sind, enthalten die meisten Metallproben nicht nur das Metall, sondern auch verschiedene Metallionen, Oxide und Salze. Da jedes Atom eine charakteristische Wellenlänge des Lichts absorbiert und emittiert, enthält das absorbierte und emittierte Licht aus dem Flammentest einen Bereich von Wellenlängen. So können Atomabsorptions- und Emissionsspektren für die Probe mit einem Spektralphotometer gemessen werden.
Die Wellenlängen und Formen der Spektren sind für jede Substanz einzigartig. Zum Beispiel hängt die relative Intensität von Merkmalen im Spektrum von der Konzentration der Spezies ab. Die absoluten Intensitäten sind abhängig von der Entfernung von der Probe zum Spektralphotometer.
<h4>Referenzen</h4>
<ol>
	<li style="font-size:17px">Kotz, J.C., Treichel Jr., P.M., Townsend, J.R. (2012). Chemie und chemische Reaktivität. Belmont, Kalifornien: Brooks/Cole, Cengage Lernen.</li>
	<li style="font-size:17px">Silderberg, M.S. (2009). Chemie: Die molekulare Natur von Materie und Veränderung. Boston, MA: McGraw Hill.</li>
	<li style="font-size:17px">Harris, D.C. (2015). Quantitative chemische Analyse. New York, NY: W.H. Freeman und Company.</li>
</ol>

Emission von Metallflammen

Emission von Metallflammen
Die Flammenprüfung ist eine Analysetechnik, bei der eine Probe in eine Flamme gelegt wird und die charakteristische Flammenfarbe zur Identifizierung von Flammen verwendet wird.

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flame test metal color clues

Flame testing uses a metal sample and a flame to identify a substance by its color. Each element gives off a characteristic light emission in the flame, so the color can help distinguish one element from another. This same idea appears in fireworks, where different metal components create different colors.

The color comes from energy absorbed by the metallic component. When a species absorbs energy, that energy can go into translation, vibration, rotation, or electron excitement. Electron excitement is the key step in flame emission because it moves electrons from the ground state, the lowest energy state, to a higher energy level.

In the Bohr model of hydrogen, these energy states are separate, or discrete. The ground state is written as n = 1, and higher states are written as n = 2, 3, 4, and so on. An electron moves up only if it absorbs the exact energy difference between its current level and the higher one.

The electron can then relax back to the ground state or another lower level. When that happens, a photon is released as light. The emitted light has a specific energy and wavelength, and visible light ranges from about 400 nm to 700 nm. These atomic absorption and emission wavelengths are discrete lines, and they act like a barcode for identifying an element.

In a metal flame emission test, the flame supplies the energy that excites the electrons. As the electrons fall back down, the sample gives off light with a wavelength tied to its atomic energy levels. Because different atoms have different energy levels, the emitted wavelength is specific to the sample.

Many metals show visible colors that are easy to spot by eye. Lithium gives a red color, sodium gives yellow, potassium gives pink-purple, and barium gives yellow-green. Real samples often contain metal ions, oxides, and salts as well as the metal itself, so the light from the flame test can include a range of wavelengths.

That range can also be measured with a spectrophotometer as atomic absorption and emission spectra. The shapes and wavelengths of the spectra are unique for each substance. The relative intensity of spectral features depends on concentration, while the absolute intensity depends on the distance from the sample to the spectrophotometer.

Flame Test Metal Color Clues

lab techniques

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boiling points

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extraction

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simple distillation

Separating Liquids by Boiling Point

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steam distillation

Steam Distillation and Low-Boiling Separation

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TLC Separation by Polarity

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column chromatography

Separating Mixtures by Polarity

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synthesis of luminol

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esterification

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identification-of-unknown-aldehydes-and-ketones

Carbonyl Tests for Aldehydes and Ketones

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lewis-structures-of-molecular-compounds-and-polyatomic-ions

Lewis Structures of Molecular Compounds and Polyatomic Ions

To draw Lewis structures for complicated molecules and molecular ions, it is helpful to follow a step-by-step procedure as outlined:


	Determine the ...

Bond Energies and Bond Lengths

Stable molecules exist because covalent bonds hold the atoms together. The strength of a covalent bond is measured by the energy required to break it, ...

Bonding in Metals

Metallic bonds are formed between two metal atoms. A simplified model to describe metallic bonding has been developed by Paul Dr&#xFC;de called the ...

Model basic atomic structure and relate an element's atomic structure to its bonding, reactivity, and placement on the Periodic Table.

IPC.7.A

physical-and-chemical-properties-of-matter

Physical and Chemical Properties of Matter

The characteristics that enable us to distinguish one substance from another are called properties.

Physical Properties of Matter

A physical property is ...

atomic-radii-and-effective-nuclear-charge

Atomic Radii and Effective Nuclear Charge

The elements in groups of the periodic table exhibit similar chemical behavior. This similarity occurs because the members of a group have the same number ...

Ionic Radii

Ionic radius is the measure used to describe the size of an ion. A cation always has fewer electrons and the same number of protons as the parent atom; it ...

Ionization Energy

The amount of energy required to remove the most loosely bound electron from a gaseous atom in its ground state is called its first ionization energy ...

Electron Affinity

The electron affinity (EA) is the energy change for adding an electron to a gaseous atom to form an anion (negative ion).



This process can be either ...

Alkali Metals

Group 1 elements are soft and shiny metallic solids. They are malleable, ductile, and good conductors of heat and electricity. The melting points of the ...

Halogens

Group 17 elements, known as halogens, are nonmetals. At room temperature, fluorine and chlorine are gases, bromine is a liquid, and iodine a solid. ...

Use patterns within the Periodic Table to predict the relative physical and chemical properties of elements.

IPC.7.B

Science concepts. The student knows that relationships exist between the structure and properties of matter. The student is expected to:

Flame Test Metal Color Clues

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