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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.
What is a spectrum that comes from noncompressed gas called?
The spectrum that comes from a noncompressed gas is called an emission spectrum. It consists of discrete lines of light at specific wavelengths that are emitted when electrons in the gas atoms move to lower energy levels.
Spectral lines produced from the radiant energy emitted from excited atoms are thought to be due to the movements of electrons?
That’s correct. Spectral lines are produced when electrons in atoms move between energy levels. When an electron drops to a lower energy level, it emits a photon of a specific energy corresponding to a specific wavelength of light, creating spectral lines in the emitted light spectrum.
What is atomic spectra explain its types?
Atomic spectra refer to the distinct lines of light emitted or absorbed by atoms when electrons transition between energy levels. There are two main types of atomic spectra: emission spectra, which are produced when electrons fall to lower energy levels and release energy as photons, resulting in bright lines on a dark background; and absorption spectra, which occur when electrons absorb energy and move to higher energy levels, showing dark lines on a continuous spectrum. Each element has a unique atomic spectrum, acting like a fingerprint for identification.
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.
How is the bright light spectra of elements produced?
An emission or absorption line in a spectrum that arises when an electron moves between two energy levels in an atom. A jump to a higher level requires an input of energy, and produces a dark absorption line. A drop to a lower level releases energy, producing a bright emission line.
Determine the region of the electromagnetic spectrum in which the lines of the Paschen series are observed?
The Paschen series lines are observed in the infrared region of the electromagnetic spectrum, specifically in the range between approximately 820 nm to 1220 nm. These spectral lines correspond to transitions within the hydrogen atom where electrons move from higher energy levels to the third energy level (n=3).
What is produced as electrons move from one carrier to the next?
the ATP generated
Origin of line spectrum?
A line spectrum is produced when electrons in an atom transition between discrete energy levels. When an electron absorbs energy, it can move to a higher energy level; when it falls back to a lower level, it emits energy in the form of light at specific wavelengths. This emission creates a series of distinct lines, each corresponding to a specific transition, resulting in a unique spectral fingerprint for each element. The line spectrum is characteristic of the element and can be used to identify it in various applications, such as spectroscopy.
How The spectral lines produced by elements all look the same.?
The spectral lines produced by elements are unique and distinct because they correspond to specific energy transitions within the atom, which are characteristic of each element. These lines are produced when electrons move between energy levels in the atom, emitting or absorbing light of specific wavelengths. This results in a pattern of lines that serve as a "fingerprint" for each element, allowing scientists to identify the elements present in a sample.
Mention two defects in Rutherford atomic model?
according to classical theory, electrons being the charged particles should release or emit energy continuously and they should ultimately fall into the nucleus. if the electrons emit energy continuously, they should form a continuous spectrum but in fact, line spectrum was observed.
When is the characteristic bright-line spectrum of an atom produced?
In the laboratory in a flame test. Electrons are excited to higher energy levels and when they fall back light is emitted. The frequency (colour), v is related to the energy by Plancks equation, E=hv
