What is the energy in joules, required to shift the electron of the hydrogen atom from the first Bohr orbit to the fifth Bohr orbit and what is the wavelength of the light emitted when the electron returns to the ground state? The ground state electron energy is –2.18 × 10^{–11} ergs.The ground-state electron energy is –2.18 × 10^{–11} ergs.

Asked by Abhisek | 1 year ago | 77

Energy (E) associated with the n^{th} Bohr orbit of an atom is:

\(E_{5}=\dfrac{-(2.18\times 10^{-18})Z^{2}}{(n)^{2}}\)

Where, Z denotes the atom’s atomic number

Ground state energy

\(=-2.18 \times 10^{–11}\, ergs\\ =-2.18 \times 10^{–11} \times 10^{–7}\, J \\ =-2.18 \times 10^{–18} \, J\)

The required energy for an electron shift from n = 1 to n = 5 is:

\(\Delta E=E_{5}-E_{1}\\ \\ =[(\dfrac{-(2.18\times 10^{-18}\, J)(1)^{2}}{(5 )^{2}})-(-2.18\times 10^{-18})]\\ \\ =(2.18\times 10^{-18})[1-\dfrac{1}{25}]\\ \\ =(2.18\times 10^{-18})[\dfrac{24}{25}]\\ \\ =2.0928\times 10^{-18}\, J\)

The wavelength of the emitted light

= \(\dfrac{hc}{E }E=\dfrac{(6.626\times 10^{-34})(3\times 10^{8})}{(2.0928\times 10^{-18})}\\ \\ =9.498\times 10^{-8}\, m= 950 Å\)

Answered by Abhisek | 1 year agoAnswer the following questions:-

**(a)** How many sub-shells are associated with n = 4?

**(b)** How many electrons will be present in the sub-shells having m_{s} value of \(- \dfrac{1}{2}\) for n = 4?

Indicate the number of unpaired electrons in:

**(a)** P

**(b) **Si

**(c)** Cr

**(d)** Fe

**(e)** Kr

The unpaired electrons in Al and Si are present in 3p orbital. Which electrons will experience more effective nuclear charge from the nucleus?

Among the following pairs of orbitals which orbital will experience the larger effective nuclear charge?

**(i) **2s and 3s,

**(ii)** 4d and 4f,

**(iii)** 3d and 3p

The bromine atom possesses 35 electrons. It contains 6 electrons in 2p orbital, 6 electrons in 3p orbital and 5 electrons in 4p orbital. Which of these electron experiences the lowest effective nuclear charge?