The ground state energy of hydrogen atom is -13.6eV. What are P.E. and K.E. of electron in this state?
A. `2.18xx10^(-14)J`
B. `2.18xx10^(-16)J`
C. `2.18xx10^(-18)J`
D. `2.18xx10^(-19)J`
Correct Answer - C
Here the ground state energy , (E) `=-13.6eV` since, K.E. of the electron `=-13.6eV`
`=13-6xx1.6xx10^(-19)J=21.76xx10^(-19)J=2.18xx10^(-18)J`.
Correct Answer - D
The ground state of hydrogen (n=1) is represented by K, the first excited state (n=2) is represented by L,the second excited state (n=3) is represent byb...
Correct Answer - A
Here, `E=-13.6eV=-13.6xx1.6xx10^(-19)=-2.2xx10^(-18)J`
`E=(-e^2)/(8piepsilon_0r)`
`therefore` As orbital radius,
`r=(-e^2)/(8piepsilon_0E)=(9xx10^(9)xx(1.6xx10^(-19))^2)/(2xx(2.2xx10^(-18)))=5.3xx10^(-11)m`.
Correct Answer - D
Here, `r_1=5.30xx10^(-11)m,v_1=2.2xx10^6ms^(-1)`
In the second excited state, `r_n=n^2r_1,v_n=(v_1)/(n)`
`therefore r_2=4r_1=4xx5.30xx10^(-11)m=2.12xx10^(-10)m` and `v_2=(v_1)/(2)=(2.2xx10^(6))/(2)ms^(-1)=1.1xx10^(6)ms^(-1)`
Correct Answer - B
`E_(1) = (hc)/(lambda) [(1)/(n_(1)^(2)) - (1)/(n_(2)^(2))]`
For second excited state to first excited state
`E_(1) = (hc)/(lambda) [1/4 - 1/9] rArr (hc)/(lambda) ((5)/(36))`
For first excited state...
Correct Answer - A::C::D
`122.4 = (13.6Z^(2))/(1^(2)) rArr Z = 3, 91.8 = 122.4[1-(1)/(4)]`
So an electron of KE `91.8 eV` can transfer its energy to this atom.