0
The absorption spectrum of a hydrogen atom contains dark bands at specific wavelengths The emission spectrum of a hydrogen atom contains bright bands at the same wavelengths Explain what causes ther?
Wiki User
∙ 13y ago
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).
Wiki User
∙ 13y ago
Add your answer:
Earn +20 pts
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.
Which scientists discovered a mathematical equation that allowed one to calculate the wavelengths of each of the bright lines in the hydrogen emission spectrum?
Niels Bohr had the first theoretical explanation. It was based on his very early quantum mechanics - that has now been completely scrapped.
What are true about Bohr's model of the hydrogen atom?
Electrons can exist only in certain allowed discrete energy states/ Photon absorption and emission are the result of transitions between energy states/ Electrons with more energy have orbits further from the nucleus
Who created the hydrogen line emission spectrum?
Niels Bohr in 1913.
What is the simplest atom that contains one proton one electron and no neutrons?
Hydrogen
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.
What is the primary visible color of an emission nebula?
Emission nebulae can emit photons of many wavelengths, but the predominant color is red. They can also emit blue and pink colors (which are also part of the Balmer series of the hydrogen atom).
What is the Balmer Series?
The Balmer series is a section of the hydrogen atomic emission line spectrum. They show the wavelengths of light emitted when electrons transition back to the n = 2 quantum level.
Why don't they see hydrogen Balmer lines in the spectra of stars with temperatures of 3200 K?
These stars are so cool that nearly all of the hydrogen atoms are in the ground state. The visible-light Balmer absorption lines of hydrogen are produced by electrons moving from the 1st excited state to a higher orbit. However in M class stars most of the hydrogen is in the ground state, and absorption from the the ground state occurs at ultraviolet wavelengths.
Why is hydrogen an 'emission free' fuel?
It is emission free because it only produces water
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.
How can absorption and emission spectra be used by the Hubble space telescope to study the structured of stars or other objects found in deep space?
The light generated by stars is mostly generated by hydrogen fusion. The light emitted from hydrogen has a distinctive emission spectrum. The emission spectrum undergoes shifting when the source and the receiver (Hubble) are moving in relation to each other. The spectrum will shift to the higher frequencies and shorter wavelengths ("blue shift") when the source and receiver are moving towards each other. Due to the "fact" that the universe is expanding, the source and receiver are moving away from each other. This causes the emission spectrum to shift to lower frequencies and longer wavelengths ("red shift"). The amount of red shift is an indication of the rate at which the cource and the receiver are moving away from each other. The expanding of the universe implies that the farther a source is from the receiver, the farther away the source and receiver are from each other. The red shifts of current objects have estimated that the farthest objects that we see are ~10-15 (not sure of exact number) billion light years distant from earth. As for absorption, the light emitted from a star that passes through gases of interspace and of planets will be absorbed at different wavelengths depending on the elements contained within the gas. This allows the determination of planetary atmospheres and intergalactic clouds.
Which element did Bohr study the line emission spectrum of?
Niels Bohr studied the emission lines of Hydrogen.
Which scientists discovered a mathematical equation that allowed one to calculate the wavelengths of each of the bright lines in the hydrogen emission spectrum?
Niels Bohr had the first theoretical explanation. It was based on his very early quantum mechanics - that has now been completely scrapped.
What are true about Bohr's model of the hydrogen atom?
Electrons can exist only in certain allowed discrete energy states/ Photon absorption and emission are the result of transitions between energy states/ Electrons with more energy have orbits further from the nucleus
What is a hydrogen filter for a telescope?
A filter to let through certain wavelenghts of light. The wavelengths that Hydrogen is most active in. Other light does not get through so objects that "shine" in those wavelengths do not show in the image.
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.
