The line spectrum of hydrogen is produced when electrons:
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Spectral photons are emitted or absorbed during energy-level transitions.
The Balmer series is obtained when an electron falls to the energy level:
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All Balmer transitions end at the second energy level.
The visible spectral series of hydrogen is called the:
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The Balmer series lies mainly in the visible region.
The Lyman series of hydrogen lies mainly in the:
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Lyman transitions terminate at n = 1.
The Rydberg equation is used to calculate the:
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The Rydberg formula gives wavelengths of hydrogen spectral lines.
The Paschen series of hydrogen lies mainly in the:
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Paschen transitions terminate at n = 3.
The Brackett series of hydrogen is found mainly in the:
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Brackett transitions terminate at n = 4.
The frequency of emitted radiation is related to photon energy by:
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Planck's equation relates photon energy and frequency.
The energy of a photon emitted by an atom is equal to:
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Photon energy is ΔE = hf.
The spectral lines of an element are useful for identifying the element because they are:
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Each element has characteristic allowed energy transitions and spectral lines.
The ground state of an atom corresponds to:
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The ground state is the atom's minimum-energy state.
When an electron moves from a higher energy level to a lower energy level, the atom:
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The energy difference is released as a photon.
The Lyman series is obtained when an electron falls to:
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Lyman transitions terminate at the first energy level.
A bright-line spectrum is also called an:
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Bright lines are characteristic of emission spectra.
A dark-line spectrum produced when continuous light passes through a cooler gas is called:
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Cooler atoms absorb specific wavelengths from continuous radiation.
The Paschen series is obtained when an electron falls to:
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Paschen transitions terminate at the third energy level.
The wavelength and frequency of electromagnetic radiation are related by:
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The speed of light equals wavelength multiplied by frequency.
When an atom absorbs energy, an electron may move from:
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Absorption of energy can excite an electron to a higher level.
The series limit occurs when the upper quantum number:
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The series converges as the upper energy level approaches infinity.
According to Bohr's model, an electron in a stationary orbit:
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Bohr postulated that electrons in stationary states do not radiate energy.
