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Based on equation E=-2.178 xx10^(-18)...

Based on equation ` E=-2.178 xx10^(-18) J ((Z^2)/(n^2))` certain conclusions are written , which of them is not correct ?

A

for n=1 the electron has a more negative energy than it does for n=6 which means that the electron is more lossely bound in the smallest allowed orbit

B

the negative sign in equation simply means that the energy of electron bound to the nuclelus is lower than it would be if the electrons were at the infinite distance from the nucleus

C

larger the value of n the larger is the orbit radius

D

equation can be used to calculate the change in energy when the electron change orbit

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The correct Answer is:
A
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Based on equation E = -2.178 xx 10^-18 J((Z^2)/(n^2)) , certain conclusions are written. Which of them is not correct ?

Based on equation E = -2.178 xx 10^-18 J((Z^2)/(n^2)) , certain conclusions are written. Which of them is not correct ?

Energy of an electron is givem by E = - 2.178 xx 10^-18 J ((Z^2)/(n^2)) . Wavelength of light required to excited an electron in an hydrogen atom from level n = 1 to n = 2 will be (h = 6.62 xx 10^-34 Js and c = 3.0 xx 10^8 ms^-1 ).

Energy of electron is given by E=-2.178xx10^(-18)((Z^(2))/(n^(2))) J. Wavelength of light required to excited an electron in an hydrogen atom from level n=1 to n=2 will be (h=6.62xx10^(-34)J*s and c=3.0xx10^(8)m*s^(-1)) -

The energy associatied with the first orbit in the hydrogen atom is - 2.17 xx 10^(-18) "J atom" ^(-1) . What is the energy associated with the fifth orbit ?

According to Bohr's theory, the electronic energy of an electron in the n^(th) orbit is given by E_(n) = (-2.17 xx 10^(-18))xx(z^2)/(n^(2)) J Calculate the longest wavelength of light that will be needed in remove an electron from the third Bohr orbit of He^(o+)

According to Bohr's theory,the electronic energy of a atom in the nth orbit is given by E_(n) = (-2.17 xx 10^(-18))/(n^(2)) J Calculate the longest wavelength of light that will be needed in remove an electron the third Bohr orbit of He^(+)

The electron energy in hydrogen atom is given by E_(n)=-(2.18 xx 10^(-18))/(n^2) J . Calculate the energy required to remove an electron completely from the n=2 orbit. What is the longest wavelength of light in cm that can be used to cause this transition?

The energy of stable states of the hydrogen atom is given by E_(n)=-2.18xx10^(-8)//n^(2)[J] where n denotes the principal quantum number. In what spectral range is the Lyman series lying?

Energy of an electron in the ground state of the hydrogen atom is -2.18xx10^(-18)J . Calculate the ionisation enthalpy of atomic hydrogen in terms of J mol^(-1) . Hint: Apply the idea of mole concept to derive the answer.

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