Bohr's Atomic Model

the diagram show

• the formation of continous spectrum

• the formation of line spectrum

At excited state electron is _______________and it will fall back to lower energy level and released a specific amount of ________________ in form of light (photon).

• unstable, energy

• stable, wavelength

Calculate the energy of electron at n=6

• 6.06 x 10^-20 J

• 3.63 x10^-20 J

• -6.06 x10^-20 J

• -3.63 x10^-20 J

Transition of electron from an excited state to a ground state of n = 5 formed a photon. Which of the following series belongs to this respective transition?

• Balmer

• Pfund

• Brackett

• Lyman

• Paschen

Which of the following Hydrogen atom series of spectrum is NOT in infrared region in electromagnetic region?

• Balmer

• Brackett

• Pfund

• Lyman

• Paschen

If energy is supplied, electron ___________ the energy and is promoted from a _____ energy level to a ______ higher energy level.

• absorbed; lower; higher

• emitted; lower; higher

• absorbed; higher; lower

• emitted; higher; lower

Calculate the energy required to excite an electron from n =2 to n= 4.

• 2. 05 x 10⁶ J

• -2. 05 x 10⁶ J

• 4.09 x10^-19 J

• - 4.09 x10^-19 J

Which series of hydrogen emission spectrum lines has frequencies that fall in the range of ultraviolet?

• Lyman series

• Balmer series

• paschen series

• all of the above

Electrons drop from higher energy level to energy level ____ in Paschen series

• 1

• 2

• 3

• 4

Which the equation show the relationship between energy and frequency of radiation.

• $\Delta E\ =\frac{hc}{\lambda}$

• $\Delta E=hv$

• $\lambda\ =\ \frac{c}{v}$

• $En=-\ R_{H\ }\left(\frac{1}{n^2}\right)$