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Different elements release different photons of light when the electrons absorb energy and get excited. The excited electron jumps up to different energy levels and then returns to the ground state by releasing the extra energy that it just absorbed in the form of light. Different elements have different atoms with different amounts of electrons in different places. Because of this, the power of the photons they emit are different, causing different spectral lines. (the power of the photons makes a difference because the different colors of lines are caused by different intensities of the wavelength and frequency, but that's kind of another story.)
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What particle is responsible for spectra?
Spectra are produced by interaction of electromagnetic radiation with matter, typically atoms or molecules. The particle responsible for spectra is the photon, which carries energy and interacts with electrons in the atoms or molecules to produce the spectral lines observed in both emission and absorption spectra.
Why do stellar spectra have absorption lines?
Need a different, better answer.
Why is it that different light sources have different types of spectra?
Different atoms have a different number of electrons. This is why they show different spectra.
How can the existence of spectra help to prove that energy levels in atoms exist?
The existence of spectra — such as emission or absorption lines — indicates that atoms emit or absorb specific energies in quantized amounts. These spectral lines correspond to transitions between distinct energy levels in atoms. Therefore, the observation of spectra provides empirical evidence that energy levels in atoms do indeed exist.
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.
How do Spectra from neutral atoms compared with spectra from ionized atoms of the same element?
Spectra from neutral atoms show a series of discrete lines corresponding to transitions between different energy levels within the atom. These lines are unique to each element and can be used to identify the element. When an atom is ionized, electrons are removed, leading to changes in the energy levels and resulting in a different set of spectral lines. The spectra from ionized atoms will have different line patterns and energy levels compared to those of neutral atoms of the same element.
What particle is responsible for spectra?
Spectra are produced by interaction of electromagnetic radiation with matter, typically atoms or molecules. The particle responsible for spectra is the photon, which carries energy and interacts with electrons in the atoms or molecules to produce the spectral lines observed in both emission and absorption spectra.
Why do stellar spectra have absorption lines?
Need a different, better answer.
Why is it that different light sources have different types of spectra?
Different atoms have a different number of electrons. This is why they show different spectra.
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.
Why are the hydrogen Balmer lines strong in the spectra of medium temperature stars and weak in the spectra of hot and cool stars?
Balmer lines are produced by colliding hydrogen atoms with electrons excited to 2nd energy level. Cool stars don't have enough collision to excite the electrons, hot stars have too much collision and excite the electrons beyond 2nd energy level.
What are the differences between line spectra and continuous spectra in terms of their characteristics and properties?
Line spectra are composed of distinct, discrete lines of light at specific wavelengths, while continuous spectra consist of a continuous range of wavelengths without distinct lines. Line spectra are produced by excited atoms emitting light at specific energy levels, while continuous spectra are emitted by hot, dense objects like stars. Line spectra are unique to each element and can be used to identify elements, while continuous spectra are characteristic of hot, dense objects emitting thermal radiation.
How can the existence of spectra help to prove that energy levels in atoms exist?
The existence of spectra — such as emission or absorption lines — indicates that atoms emit or absorb specific energies in quantized amounts. These spectral lines correspond to transitions between distinct energy levels in atoms. Therefore, the observation of spectra provides empirical evidence that energy levels in atoms do indeed exist.
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.
How are elements identified fro bright line spectra?
Elements are identified from bright line spectra by comparing the observed spectral lines with known emission spectra of elements. Each element emits a unique set of spectral lines due to the characteristic energy levels of its electrons. By matching the observed lines with known patterns, scientists can determine the elements present in a sample.
Why do we say atomic spectra are like fingerprints of the elements?
Atomic spectra are like fingerprints of elements because each element has a unique set of discreet emission or absorption lines in its spectrum. These lines correspond to specific energy levels of electrons within the atoms of that element. By analyzing the pattern and position of these lines in a spectrum, scientists can identify the elements present in a sample.
Why do different elements have different line spectra and not a continuous spectrum of light?
Different elements have different line spectra because each has a unique arrangement of energy levels for its electrons. When electrons transition between these energy levels, they emit or absorb specific wavelengths of light, creating distinct lines in the spectrum. This results in discrete lines rather than a continuous spectrum.
