A
Which atom did Bohr based his model on?
Hydrogen atom
True or False: The shorter the wavelength, the higher the energy
True
The fifth line in Balmer series is formed when electron undergo transition from …… to ……
n=7 to n=2
A photon of light with wavelength 434 nm falls in the visible light region and forms a line in the emission spectrum of hydrogen atom.
State the name of this emission spectrum series.
Balmer series
When electrons falls back to lower energy level, it releases energy in the form of ……
Light OR photons
Indicate the transition of electron that gives the longest wavelength in Lyman series.
n=2 to n=1
Line Q and line R has a wavelength of 2625 nm and 1944 nm respectively.
Which line has higher energy?
Line R
The …… line of any series is the most intense line.
First
Hydrogen atom is said to be ionised when electron is removed from ….. to …..
n=1 to n=Infinity
The energy level that an electron falls down to that releases a photon of visible light.
n=2
The state of an atom with all of its electrons at their lowest possible energy levels.
Ground state
Formula that relates energy and wavelength
Energy = hc/wavelength
Lyman series is located in which electromagnetic spectrum?
Ultraviolet
If the ionisation energy of 1 Hydrogen electron is 2.18 x 10-18 J, how can you find the ionisation energy of 1 mol of Hydrogen atom?
2.18 x 10-18 J x NA (6.02 x 1023 mol-1)
Brackett series is formed when electrons at the excited state make a transition from higher energy level to …..
n=4
A photon has a frequency of 1.02 x 1016 Hz. Calculate its wavelength.
2.94 x 10-8 m
A photon has a wavelength of 3.10 x 10-5 m. Calculate its frequency.
9.67 x 1012 Hz
A photon has a wavelength of 6.9 x 10-6 m. Calculate its frequency.
4.3 x 1013 Hz
A photon has a wavelength of 2625 nm. Calculate its frequency.
1.143 x 1014 Hz
A photon has a wavelength of 2625 nm. Calculate its energy.
7.572 x 10-20 J
Calculate the wavelength of the second line in Lyman series.
1.026 x 10-7 m
The wavelength of a photon emitted in Brackett series of hydrogen emission spectrum is 2625nm.
Determine the initial and final energy level corresponding to this emission.
nf = 4
ni = 6
Determine the transition of electron which emitted photon with wavelength 1280 nm in Pachen series.
From n=5 to n=3
Calculate the energy change for the formation of the line with the lowest energy in Paschen series.
-1.06 x 10-19 J
If an electron of hydrogen atom is excited to n=7 and falls to a lower energy level to form Paschen series,
Calculate the energy emitted (in kJ mol-1) due to this transition.
119.0 kJ mol-1