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What transition energy corresponds to an absorption line at 460nm?
The transition energy corresponding to an absorption line at 460nm is about 2.7 electronvolts (eV). This energy is calculated using Planck's equation, E = hc/λ, where h is Planck's constant, c is the speed of light, and λ is the wavelength in meters.
What transition energy corresponds to an absorption line at 460 nm?
4.32 x 10^-19 j
What is the second longest wavelength in the absorption spectrum of hydrogen?
The second longest wavelength in the absorption spectrum of hydrogen corresponds to the transition from the n=2 to n=4 energy levels. This transition produces a spectral line known as the H-alpha line, which falls in the red part of the visible spectrum at a wavelength of 656.3 nm.
What is the wavelength of the hydrogen atom in the 2nd line of the Balmer series?
The wavelength of the hydrogen atom in the 2nd line of the Balmer series is approximately 486 nm. This corresponds to the transition of an electron from the third energy level to the second energy level in the hydrogen atom.
Is the spacing between the lines in the spectrum of an element constant or does it vary?
The spacing between the lines in the spectrum of an element are constant. This is called the emission spectrum of an element. Each element has a unique emission spectra that will be the same each time.
What transition energy corresponds to an absorption line at NM?
3.96 10-19 j
What transition energy corresponds to an absorption line at 460nm?
The transition energy corresponding to an absorption line at 460nm is about 2.7 electronvolts (eV). This energy is calculated using Planck's equation, E = hc/λ, where h is Planck's constant, c is the speed of light, and λ is the wavelength in meters.
What transition energy corresponds to an absorption line at 460 nm?
4.32 x 10^-19 j
What is an absorption line?
An absorption line is a line which corresponds to the absorption of electromagnetic radiation at a specific wavelength.
What is the second longest wavelength in the absorption spectrum of hydrogen?
The second longest wavelength in the absorption spectrum of hydrogen corresponds to the transition from the n=2 to n=4 energy levels. This transition produces a spectral line known as the H-alpha line, which falls in the red part of the visible spectrum at a wavelength of 656.3 nm.
What transition energy corresponds to an absorption line at 502nm?
The transition energy corresponding to an absorption line at 502nm can be calculated using the formula E = hc/λ, where E is the energy, h is Planck's constant, c is the speed of light, and λ is the wavelength. Plugging in the values, we get E = (6.63 x 10^-34 J s * 3 x 10^8 m/s) / (502 x 10^-9 m) ≈ 3.96 x 10^-19 J.
What do Each of the colored lines in hydrogen's emission spectrum corresponds with?
Each colored line in hydrogen's emission spectrum corresponds to a specific transition of an electron between energy levels in the hydrogen atom. The wavelengths of these lines are unique to each transition, creating a distinct pattern that can be used to identify elements and their energy levels.
What frequency corresponds to an Absorption line at 527?
5.69 × 1014 Hz
What frequency corresponds to an absorption line at 460?
6.52 1014 Hz
What causes the lines in an atomice spectrum?
The lines in an atomic spectrum are caused by the emission or absorption of photons as electrons move between different energy levels within the atom. Each line corresponds to a specific energy transition, and the distinct set of lines is unique to each element, making them a fingerprint for identifying elements.
The lowest wave no. absorption line in the rot. spectrum of NO molecule is at 3.440 cm-1. Calculate the corresponding frequency of absorption Which are the two energy level of transition?
The corresponding frequency of absorption is 3.440 cm-1 * 2.99792 x 10^10 cm/s = 1.032 x 10^11 Hz. The two energy levels involved in this transition correspond to the rotational energy levels of the NO molecule.
Why would the absorption spectrum of each element have lines in the same places as in its emission spectrum?
The absorption spectrum of an element have lines in the same places as in its emission spectrum because each line in the emission spectrum corresponds to a specific transition of electrons between energy levels. When light is absorbed by the element, electrons move from lower energy levels to higher ones, creating the same lines in the absorption spectrum as the emission spectrum. The frequencies of light absorbed and emitted are the same for a specific element, resulting in matching lines.
