5.7 Spectral Lines of Hydrogen
Which of the following statements is(are) incorrect?
All of the above (The Paschen series appears in the UV region; the Lyman series appears in the visible region; the Pfund series appears in the visible region)
Bohr's model predicts the hydrogen atom could emit electromagnetic radiation which can be observed in the _____ region.
All of the above (visible, infrared, ultraviolet)
What electron transition series corresponds to the emission of visible light?
Balmer series
Based on the wavelengths of the spectral lines...
Bohr was able to calculate the energies that the hydrogen electron would have in each of its allowed energy levels
Delta E is...
Change in energy
Which of the following electronic jumps in a hydrogen atom will require the most energy?
From n=1 to n=2
Electron transitions within the hydrogen atom are grouped based on the ending energy level of the transition. Choose the name of the electron transition series of the hydrogen atom to the ending energy level. _____ Lyman series
n=1
The ground state of the spectra is...
n=1
Electron transitions within the hydrogen atom are grouped based on the ending energy level of the transition. Choose the name of the electron transition series of the hydrogen atom to the ending energy level. _____ Balmer series
n=2
The first excited state of the spectra is...
n=2
Electron transitions within the hydrogen atom are grouped based on the ending energy level of the transition. Choose the name of the electron transition series of the hydrogen atom to the ending energy level. ______ Paschen series
n=3
The emission spectrum of atomic hydrogen is divided into ____ spectral series.
6
Lyman series
E(n) to E(n=1); ultraviolet range
Balmer series
E(n) to E(n=2); visible range
Paschen series
E(n) to E(n=3); near infrared range
Brackett series
E(n) to E(n=4); rather in the infrared range
Pfund seres
E(n) to E(n=5)
Humphrey series
E(n) to E(n=6)
Emission lines for hydrogen correspond to...
Energy changes related to electron transitions
The difference in energy between the n=1 and the n=2 energy levels of a hydrogen atom is 1.64 × 10^−18 J. What happens when an electron transitions from n=2 to n=1?
Exactly 1.64 × 10^−18 J of energy is released
The excited state is the stable state of an atom.
FALSE
When a hydrogen atom absorbs one or more quanta of energy, the electron is elevated to a lower energy level.
FALSE
Which of the following is a shortcoming of Bohr's theory?
It was only successful for atoms which have a single electron
To find out the series of which a number belongs to, you...
Math: do 1/the number and multiply that by 10^-2 and 1/10^-9 On the Spectrum: if it lays in the visible region, it is Balmer, if not, use the produced exponent to find the series
To move from the ground state to the excited state, an electron:
Must absorb one or more quanta of energy
Does the Bohr model work for atoms other than hydrogen?
No
n the hydrogen atom's spectrum, series lines are found at 12,186.3 cm^−1. The hydrogen atom belongs to the _____ series.
Paschen
A transition from a higher energy level to the energy level n=3 produces the Paschen series.
TRUE
The hydrogen spectrum shows presence of quantized energy levels.
TRUE
The frequency of the radiation emitted by an atom is directly related to the difference in energy between the levels.
TRUE (when two variables are on the same side in an equation, they are directly related; when on opposite sides, they are indirectly)
The Bohr model works only for
The hydrogen atom
The equation E=hv is...
The light of a particular frequency being emitted
What happens to the spacing between energy levels in the hydrogen atom as one proceeds further and further from the nucleus?
The spacing between energy levels decreases
Electron transitions within the hydrogen atom are grouped based on the ending energy level of the transition. Choose the name of the electron transition series of the hydrogen atom to the ending energy level. _________Brackett series
n=4
