# Quiz 1 - Early Quantum Theory | Early Quantum Theory

## General Chemistry 1 - Quiz 1 - Early Quantum Theory

Which one of the following types of radiation has the highest wavelength?

Wavelength:

X rays < UV light < visible light < IR light

Which one of the following types of radiation has the highest frequency?

Wavelength:

UV light < IR light < microwaves < radio waves

c = λv ⇒ frequency is inversely proportional to the wavelength

⇒ Frequency:

UV light > IR light > microwaves > radio waves

What is the energy of one photon with a wavelength of 2.25 x 10^{-2} m?

E = $\frac{\mathrm{hc}}{\mathrm{\lambda}}$

h = Planck’s constant = 6.626 x 10^{-34} J.s

c = speed of light = 3.00 x 10^{8} m.s^{-1}

What is the frequency of radiation which has an energy of 1.52 x 10^{6} J per mole of photons?

E = nhv

n = number of photons = 1 mol = 6.022 x 10^{23} photons

Which statement below is incorrect regarding early quantum theory?

What is the energy of one electron in the second orbital of a hydrogen atom?

E_{n} = $\frac{-2.1799\times {10}^{-18}}{{\mathrm{n}}^{2}}$

E_{n} = 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?

$\frac{1}{{3}^{2}}$ - $\frac{1}{{4}^{2}}$ $<$ $\frac{1}{{2}^{2}}$ - $\frac{1}{{3}^{2}}$