5909098
Description
Mind Map by Lester Stoffels, updated more than 1 year ago
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Absorption and Emission Spectra
- Energy
Levels
- An electron in a hydrogen atom can
occupy any one of the fixed energy
levels
- These different energy levels are
the same for all hydrogen atoms.
- In the ground state, the electrons CLOSEST
to the nucleus have the lowest energy.
- The difference in the energy levels
DECREASES as the electron moves away from
the nucleus
- An electron in a hydrogen atom can
occupy any one of the fixed energy
levels
- Absorption Spectra
- An absorption specctra seen on earth is the VISIBLE SPECTRUM OF LIGHT,
with black lines corresponding to the absorptions of energy by the electrons
- These spectra are seen from earth when
atoms in the chromosphere around stars
absorb light
- Electrons absorb a
'photon'
- Excited electrons move up to a higher energy level- they are
PREMOTED. This is what produces the lines on the Absorption
spectrum
- The EM radiation absorbed by each hydrogen
atom has a definite frequency, related to the
difference in energy levels by AE=hv
- The EM radiation absorbed by each hydrogen
atom has a definite frequency, related to the
difference in energy levels by AE=hv
- Excited electrons move up to a higher energy level- they are
PREMOTED. This is what produces the lines on the Absorption
spectrum
- An absorption specctra seen on earth is the VISIBLE SPECTRUM OF LIGHT,
with black lines corresponding to the absorptions of energy by the electrons
- Emission
Spectra
- Black background with
coloured lines on it
- These correspond to the emissions
of energy by the electrons
- These correspond to the emissions
of energy by the electrons
- An emission spectrum is seen when a
chemical burns with a coloured flame
- Electrons first absorb a 'photon'
- Excited electrons move up to a higher
energy level- they are premoted
- Electrons then drop back to lower
energy levels. This is what produces
the lines on emission spectra
- The E.R emitted by each H atom has a definite frequency
related to the difference in energy levels by AE=hv
- Since AE is different for each transition, the
frequency is different for each transition, and
so is the colour of the lines.
- Since AE is different for each transition, the
frequency is different for each transition, and
so is the colour of the lines.
- The E.R emitted by each H atom has a definite frequency
related to the difference in energy levels by AE=hv
- Electrons then drop back to lower
energy levels. This is what produces
the lines on emission spectra
- Excited electrons move up to a higher
energy level- they are premoted
- Black background with
coloured lines on it
- Similarities
- Both line
spectra
- Lines in the same position
for each element
- Lines become closer at
higher frequencies
- Set of lines representing
transitions to a particular
level
- Both line
spectra
- Differences
- Bright lines on black background OR
black lines on coloured background
- Bright lines on black background OR
black lines on coloured background
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