Wavelength of light required to excite an electron in an hydrogen atom from level n=1 to n=2 will be: (IIT-JEE MAIN 2013)Įnergy required to excite electron from n=1 to n=2 will be equal to the energy difference between these levels. Question-5) Energy of an electron is given by E = -2.178 x 10 -18 (Z 2/n 2) J. The energy of electron in 1st level for He + can be written as: Since negative of Ionization energy is the energy of first stationery state, for He +, the energy of 1st level is -19.6 x 10 -18 J atom -1. The energy of the first stationary state ( n = 1) of Li 2+ is: (AIEEE-2003) Question-4) Ionization energy of He + is 19.6 x 10 -18 J atom -1. Hence we can take negative of ionization energy as the energy of the ground state (n=1). Ionization energy = ΔE (∞,1) = E ∞- E 1 = - E 1 Now we can calculate the energy required to excite the electron from n = 1 to n = 2 as follows. Hence ionization energy must be equal to the energy difference between these two orbits. Ionization enthalpy is the energy required to take the electron from n = 1 orbit to n = ∞ orbit. This can be done by using ionization enthalpy data.
The energy required to excite the electron from n = 1 to n = 2 is: The energy required to excite the electron in the atom from n=1 to n=2 is: (AIEEE-2008)Į n = -K/n 2 (for hydrogen atom), where K is a constant. Question-3) The ionization enthalpy of hydrogen atom is 1.312 x 10 -6 J mol -1. Though questions like this are not perfect, choose the correct answers wisely among the options given. What to do when questions like this are asked?īe flexible in your thinking. To show that the questions given in entrance exams are always not perfect. Actually it is the energy of electron in the n th orbit and not just for 1 st orbit. This is not a good question because 'r' value is a variable and depends on the principal quantum number, n. Total Energy of electron, E total = Potential energy (PE) + Kinetic energy (KE)įor an electron revolving in a circular orbit of radius, r around a nucleus with Z positive charge,Į total = (-Ze 2/r) + (Ze 2/2r) = -Ze 2/2r
Question-2) If the electron of a hydrogen atom is present in the first orbit, the total energy of the electron is: (Eamcet - 2003-E) Ĭlick here for CSIR NET - GATE - SET Study MaterialĮnergy of electron in the nth Bohr's orbit - Followup questions & answers Question-1) With increase in principal quantum number, n, the energy difference between adjacent energy levels in Hydrogen atom: (Eamcet - 2009-M)ĭ) Decreases for lower values of n and increases for higher values of nįrom the previous problem, we can clearly see the decrease in energy difference between adjacent levels with increase in the principal quantum number, n. The ratio of energy of electrons in the orbits of hydrogen atom is:Į 1 : E 2 : E 3 : E 4. The energies of electrons in the Bohr's orbits of hydrogen atom expressed in eV are: OrbitĮxcited state(s) represent n = 2, 3, 4. Since Z = 1 for hydrogen above equation can be further simplified to: The energy of an electron in Bohr’s orbit of hydrogen atom is given by the expression: The possible energy value(s) of the excited state(s) for electrons in Bohr orbits of hydrogen is (are) : Question - The energy of an electron in the first Bohr orbit of H atom is -13.6 eV. To get an idea about Energy of electron in Bohr's orbit. Energy of electron| nth Bohr's orbit|Hydrogen atom|formulaĮNERGY OF ELECTRON IN n th BOHR'S ORBIT.
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