Based on equation E=-2.178xx10^-18 J(Z^2...

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

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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 electron energy of hydrogen atom in the ground state works out to be - 2.18 xx 10^(-18) J per atom. Calculate what will happen to the position of the electron in this atom if an energy of 1.938 xx 10^(-18) J is supplied to the each hydrogen atom.

The energy associated with the first orbit of hydrogen atom is -2.18x10^(-18) J.What is the energy associated with the fifth orbit?

Enegy of an electron in the ground state of the H. atom is -2.18xx10^(-18)J . Calculate the ionisation enthalpy off atomic hydrogen in terms of J*mol^(-1) .

(1) The energy associated with the first orbit in the hydrogen atom is -2.18xx10^(-18)J*"atom"^(-1) . What is the energy associated with the fifth orbit? (2) Calculate the radius of Bohr's fifth orbit for hydrogen atom.

The electron energy is hydrogen atom is given by E"(n)=(-2.18xx10^(-18)) 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?

According to Bohr's theory, energy of electron in n-th orbit of H-atom, E_(n)=-(21.76xx10^(-19))/(n^(2))J . Find the longest wavelength of radiation required to remove one electron from the 3rd orbit of He^(+) ion.

The energy of electron of H atom is, E_n = -(2.18xx10^-18)/n^2 J. How amount of energy is required to remove the electron from n = 2 orbit? What is the value of longest wave length of light required to remove this electron?

Each molecule of a gas, contains 2 hydrogen atoms, 1.78 xx 10^(-22) g chlorine, 2 carbon atoms and 1.25 xx 10^(-22) g of an unknown metal. Its molecular weight will be

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