Quiz - Early Quantum Theory | Early Quantum Theory
Which one of the following types of radiation has the highest wavelength?
X rays < UV light < visible light < IR light
Which one of the following types of radiation has the highest frequency?
UV light < IR light < microwaves < radio waves
c = λv ⇒ frequency is inversely proportional to the wavelength
UV light > IR light > microwaves > radio waves
What is the energy of one photon with a wavelength of 2.25 x 10-2 m?
4.97 x 10-44 J
8.83 x 10-24 J
1.13 x 1023 J
2.01 x 1043 J
h = Planck’s constant = 6.626 x 10-34 J.s
c = speed of light = 3.00 x 108 m.s-1
What is the frequency of radiation which has an energy of 1.52 x 106 J per mole of photons?
1.38 x 1063 Hz
2.29 x 1039 Hz
3.81 x 1015 Hz
2.63 x 10-16 Hz
E = nhv
n = number of photons = 1 mol = 6.022 x 1023 photons
Which statement below is incorrect regarding early quantum theory?
Bohr’s model of the atom accounts for the absorption and emission spectrum of hydrogen atom
Bohr’s model of the atom accounts for the Rydberg equation
Energy states in the hydrogen atom are quantized
None of the above
What is the energy of one electron in the second orbital of a hydrogen atom?
-5.45 x 10-19 J
5.45 x 10-19 J
-1.83 x 1018 J
1.83 x 1018 J
En = energy of the orbital n
n = number of the orbital = 2
According to the Bohr model for the hydrogen atom, how is the energy required to excite an electron from n=3 to n=4 compared to the energy required to excite an electron from n=2 to n=3?
Either equal or greater