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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 does the energy of spectral lines represent?
an emission spectrum is produced after atoms are supplied with electrical energy afterwhich they emit energies as they return to ground state after excitement. the emission spectrum is produced with coloured lines on a dark background. these lines all have different wavelengths thus different frequencies and different quantums of energy. each level has a different energy and since these lines show properties of different energies they show also that atoms have discrete energy levels.
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?
Hydrogen Balmer lines are strong in medium temperature stars because this range of temperatures allows for the excitation of hydrogen atoms to higher energy levels that produce these lines. In hot stars, the atoms are ionized, making it harder to form the lines, while in cool stars, the atoms are not as excited, leading to weaker Balmer lines in their spectra.
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.
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 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.
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 atomic spectra show individual lines instead of continuous spectra?
Atomic spectra show individual lines instead of continuous spectra because each line corresponds to a specific energy level transition of electrons within the atom. When electrons move between energy levels, they emit or absorb energy in the form of light at specific wavelengths, creating distinct spectral lines. This results in the observed pattern of individual lines in atomic spectra.
