Flame Test & Spectroscopy – Chemistry Exam

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Flame Test & Spectroscopy – Chemistry Exam

The key terms of these chemistry tests include Flame Test, Spectroscopy, Element, Wavelength, Electromagnetic Radiations.


Part 1 Flame Test

Create and complete a data table for Part One of the lab. It should include the name of
the element (or unknown) examined and the color of the observed flame.

Flame Test & Spectroscopy - Chemistry

Identify each unknown from Part One of the lab and briefly explain why you identified
each unknown as you did.

Answer

Unknown 1: From the data gathered I infer that the first Unknown Substance is Lithium as they both have the same flame color.
Unknown 2: From the data gathered I infer that the second Unknown Substance is Potassium as they both have the same flame color.


Part 2 Spectroscopy

Create and complete a data table for Part Two of the lab. It should include the name of
the element, the colors, and the wavelength values of the observed lines.

Flame Test & Spectroscopy - Chemistry

Describe the line spectrum of the star. Give the color and wavelength value of the five
brightest lines in the spectrum.

Answer

The star spectrum had a color in almost every possible place. The five brightest
colors were

  1. Purple – 415 nm
  2. Blue – 435 nm
  3. Teal – 500 nm
  4. Yellow – 550 nm
  5. Red – 705 nm

Conclusion

Explain, in your own words, why different elements produce different colors of light when heated.

When heated, electrons emit light, the reason that the elements produce different
colors is because of the amount of electrons they have.


Why do you think elements must be heated before they emit colored light?

When electromagnetic radiations occur on an atom, the electrons in the atom
absorb energy from the radiations and jump from lower energy orbits to higher orbits of
energy. But the greater amount of energy makes the atom unstable. Due to this the
excited electrons tend to come back to the lower energy levels by losing energy. The
energy lost is also electromagnetic radiation, which is emitted in the form of photons.
Due to this, photons emit all wavelengths/frequencies.


What element do you think is the most abundant in the star that you observed in Part Two? Explain your answer.

Neon in my opinion, is the most abundant in the stars observed in Part two, for the reason that it contains every mutual color in the spectrum.


Part 1 Flame Test

Create and complete a data table for Part One of the lab. It should include the name of
the element (or unknown) examined and the color of the observed flame.

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Identify each unknown from Part One of the lab and briefly explain why you identified
each unknown as you did.

Answer

Unknown 1: From the data gathered I infer that the first Unknown Substance is Lithium as they both have the same flame color.
Unknown 2: From the data gathered I infer that the second Unknown Substance is Potassium as they both have the same flame color.


Part 2 Spectroscopy

Create and complete a data table for Part Two of the lab. It should include the name of
the element, the colors, and the wavelength values of the observed lines.

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Describe the line spectrum of the star. Give the color and wavelength value of the five
brightest lines in the spectrum.

Answer

The star spectrum had a color in almost every possible place. The five brightest
colors were

  1. Purple – 415 nm
  2. Blue – 435 nm
  3. Teal – 500 nm
  4. Yellow – 550 nm
  5. Red – 705 nm

Conclusion

Explain, in your own words, why different elements produce different colors of light when heated.

When heated, electrons emit light, the reason that the elements produce different
colors is because of the amount of electrons they have.


What element do you think is the most abundant in the star that you observed in Part Two? Explain your answer.

Neon in my opinion, is the most abundant in the stars observed in Part two, for the reason that it contains every mutual color in the spectrum.


Why do you think elements must be heated before they emit colored light?

When electromagnetic radiations occur on an atom, the electrons in the atom
absorb energy from the radiations and jump from lower energy orbits to higher orbits of
energy. But the greater amount of energy makes the atom unstable. Due to this the
excited electrons tend to come back to the lower energy levels by losing energy. The
energy lost is also electromagnetic radiation, which is emitted in the form of photons.
Due to this, photons emit all wavelengths/frequencies.


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