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The short answer is these bands represent the (frequency) wavelengths which correspond to orbital configurations for the atom (matter).
Absorption is used to identify chemical bonds of elements & compounds by radiating a substance across a range of frequencies & measuring the magnitude of the signal at these frequencies in chemical analysis of a sample.
Emission is based upon the same principle except that the substance is heated to the point that it emits radiation (light).
What else can I help you with?
What colors of visible light are found in the emission spectrum of hydrogen?
Red, blue, green, and violet are found in the emission spectrum of hydrogen.
Who created the hydrogen line emission spectrum?
The hydrogen line emission spectrum was discovered by physicists Johann Balmer, Johannes Rydberg, and Niels Bohr. They observed that hydrogen gas emitted specific wavelengths of light, which formed a distinct spectrum now known as the Balmer series.
Which scientists discovered a mathematical equation that allowed one to calculate the wavelengths of each of the bright lines in the hydrogen emission spectrum?
The mathematical equation that allows one to calculate the wavelengths of each line in the hydrogen emission spectrum was discovered by Danish physicist Niels Bohr in 1913 as part of his model of the hydrogen atom. This equation is known as the Balmer equation and helped to explain the spectral lines observed in hydrogen emission spectra.
How does the theory of Bohr explain the spectrum of hydrogen?
The Bohr theory explains the spectrum of hydrogen by proposing that electrons orbit the nucleus in fixed, quantized energy levels. When an electron transitions between these levels, it absorbs or emits energy in the form of photons, leading to specific wavelengths of light. This results in the distinct spectral lines observed in hydrogen's emission and absorption spectra, corresponding to the differences in energy between the quantized orbits. By calculating these energy differences, Bohr was able to accurately predict the wavelengths of the spectral lines observed experimentally.
What is the difference between sunlight produced spectrum and hydrogen gas produced spectrum?
Sunlight produced spectrum is continuous and contains a broad range of wavelengths, while hydrogen gas produced spectrum consists of discrete lines at specific wavelengths due to the unique energy levels of hydrogen atoms. Sunlight spectrum is continuous due to the various processes that produce light, whereas hydrogen gas spectrum is a result of the energy levels of hydrogen atoms emitting photons of specific wavelengths.
How do the emission wavelengths for helium and hydrogen differ?
The emission wavelengths for helium and hydrogen differ because they have different electron configurations. Helium emits light at specific wavelengths corresponding to its unique electron transitions, while hydrogen emits light at different wavelengths due to its own electron transitions.
Why does helium have more emission lines than hydrogen?
Helium has more emission lines than hydrogen because it has more electrons and energy levels, leading to more possible transitions between these levels and the emission of different wavelengths of light.
What colors of visible light are found in the emission spectrum of hydrogen?
Red, blue, green, and violet are found in the emission spectrum of hydrogen.
Why does hydrogen emit different wavelengths of light than mercury?
Hydrogen emits different wavelengths of light than mercury because each element has a unique arrangement of electrons in its atoms. When electrons in hydrogen atoms move between energy levels, they emit specific wavelengths of light. In contrast, mercury atoms have different electron configurations, leading to the emission of different wavelengths of light.
What is the color of hydrogen plasma?
Hydrogen plasma appears as a pinkish or purplish color due to the emission of specific wavelengths of light as the electrons in the plasma become excited and then de-excite.
Why do the emission spectra for hydrogen and helium differ?
The emission spectra for hydrogen and helium differ because each element has a unique arrangement of electrons in their atoms. This arrangement causes them to emit different wavelengths of light when excited, resulting in distinct spectral lines.
How do the emission spectra for hydrogen and helium differ from each other?
The emission spectra for hydrogen and helium differ in the specific wavelengths of light they emit. Hydrogen emits light in distinct lines corresponding to transitions of its electrons between energy levels, while helium emits a continuous spectrum of light.
Who created the hydrogen line emission spectrum?
The hydrogen line emission spectrum was discovered by physicists Johann Balmer, Johannes Rydberg, and Niels Bohr. They observed that hydrogen gas emitted specific wavelengths of light, which formed a distinct spectrum now known as the Balmer series.
Which scientists discovered a mathematical equation that allowed one to calculate the wavelengths of each of the bright lines in the hydrogen emission spectrum?
The mathematical equation that allows one to calculate the wavelengths of each line in the hydrogen emission spectrum was discovered by Danish physicist Niels Bohr in 1913 as part of his model of the hydrogen atom. This equation is known as the Balmer equation and helped to explain the spectral lines observed in hydrogen emission spectra.
Explain why ionized calcium can form absorption lines but ionized hydrogen can not.?
every atom can absorb light at different specific wavelengths (a useful fingerprint), these wavelengths correspond to the amount of energy it takes to move the atom's electrons from their ground state to an excited state, this is the cause of absorption lines. the atom will soon emit the light again (at the same wavelength, as the electron moves from excited to ground states), but in a random direction, this is the source of emission lines. an ion is an atom that has lost one or all of its electrons. in the case of a calcium ion, there are still some electrons present, atomic hydrogen has only one electron, so once it becomes ionised there are no electrons to create absorption lines.
How does the theory of Bohr explain the spectrum of hydrogen?
The Bohr theory explains the spectrum of hydrogen by proposing that electrons orbit the nucleus in fixed, quantized energy levels. When an electron transitions between these levels, it absorbs or emits energy in the form of photons, leading to specific wavelengths of light. This results in the distinct spectral lines observed in hydrogen's emission and absorption spectra, corresponding to the differences in energy between the quantized orbits. By calculating these energy differences, Bohr was able to accurately predict the wavelengths of the spectral lines observed experimentally.
Why is the emission spectrum of hydrogen made of discrete wavelengths rather than a continum of wavelengths?
The emission spectrum of all elements is made of discrete wavelengths. Electrons only exist in particular orbitals. They do not spin willy-nilly around the nucleus. If they receive energy, they jump from one orbital to a higher orbital. When they fall back to a lower orbital, they give off a discrete amount amount of energy. That discrete amount of energy comes as the form of light of a particular wavelength. Look at it as an electron having to be on one or another step instead of a ramp. Instead of continually rolling, it goes one step at a time.
