Hydrogen atom:
The electronic ground state of hydrogen atom contains one electron in the first orbit. If sufficient energy is provided, this electron can be promoted to higher energy levels. The electronic energy of a hydrogen-like species (any atom//ions with nuclear charge Z and one electron) can be given as
`E_(n)=-(R_(H)Z^(2))/(n^(2))` where `R_(H)= "Rydberg constant," n= "principal quantum number"`
The energy in Joule of an electron in the second orbit of H- atom is:
Hydrogen atom:
The electronic ground state of hydrogen atom contains one electron in the first orbit. If sufficient energy is provided, this electron can be promoted to higher energy levels. The electronic energy of a hydrogen-like species (any atom//ions with nuclear charge Z and one electron) can be given as
`E_(n)=-(R_(H)Z^(2))/(n^(2))` where `R_(H)= "Rydberg constant," n= "principal quantum number"`
The energy in Joule of an electron in the second orbit of H- atom is:
The electronic ground state of hydrogen atom contains one electron in the first orbit. If sufficient energy is provided, this electron can be promoted to higher energy levels. The electronic energy of a hydrogen-like species (any atom//ions with nuclear charge Z and one electron) can be given as
`E_(n)=-(R_(H)Z^(2))/(n^(2))` where `R_(H)= "Rydberg constant," n= "principal quantum number"`
The energy in Joule of an electron in the second orbit of H- atom is:
Text Solution
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The correct Answer is:
`-5.45xx10^(-19) J`
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Hydrogen atom: The electronic ground state of hydrogen atom contains one electron in the first orbit. If sufficient energy is provided, this electron can be promoted to higher energy levels. The electronic energy of a hydrogen-like species (any atom//ions with nuclear charge Z and one electron) can be given as E_(n)=-(R_(H)Z^(2))/(n^(2)) where R_(H)= "Rydberg constant," n= "principal quantum number" Total energy required to remove two electrons from He is :
Hydrogen atom: The electronic ground state of hydrogen atom contains one electron in the first orbit. If sufficient energy is provided, this electron can be promoted to higher energy levels. The electronic energy of a hydrogen-like species (any atom//ions with nuclear charge Z and one electron) can be given as E_(n)=-(R_(H)Z^(2))/(n^(2)) where R_(H)= "Rydberg constant," n= "principal quantum number" The energy required to promote the ground state electron of H-atom to the first excited state is: When an electron returns from a higher energy level to a lower energy level, energy is given out in the form of UV//Visible radiation.
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Hydrogen atom: The electronic ground state of hydrogen atom contains one electron in the first orbit. If sufficient energy is provided, this electron can be promoted to higher energy levels. The electronic energy of a hydrogen-like species (any atom//ions with nuclear charge Z and one electron) can be given as E_(n)=-(R_(H)Z^(2))/(n^(2)) where R_(H)= "Rydberg constant," n= "principal quantum number" The ratio of energy of an electron in the ground state Be^(3-) ion to that of ground state H atom is: The kinetic and potential energies of an electron in the H atoms are given as K.E. =e^(2)/(4 pi epsilon_(0)2r) and P.E.=-1/(4pi epsilon_(0)) e^(2)/r
Hydrogen atom: The electronic ground state of hydrogen atom contains one electron in the first orbit. If sufficient energy is provided, this electron can be promoted to higher energy levels. The electronic energy of a hydrogen-like species (any atom//ions with nuclear charge Z and one electron) can be given as E_(n)=-(R_(H)Z^(2))/(n^(2)) where R_(H)= "Rydberg constant," n= "principal quantum number" The ratio of energy of an electron in the ground state Be^(3-) ion to that of ground state H atom is: The kinetic and potential energies of an electron in the H atoms are given as K.E. =e^(2)/(4 pi epsilon_(0)2r) and P.E.=-1/(4pi epsilon_(0)) e^(2)/r
A
`16`
B
`4`
C
`1`
D
`8`
Hydrogen atom: The electronic ground state of hydrogen atom contains one electron in the first orbit. If sufficient energy is provided, this electron can be promoted to higher energy levels. The electronic energy of a hydrogen-like species (any atom//ions with nuclear charge Z and one electron) can be given as E_(n)=-(R_(H)Z^(2))/(n^(2)) where R_(H)= "Rydberg constant," n= "principal quantum number" A gaseous excited hydrogen-like species with nuclear charge Z can emit radiations of six different photon energies. (a) The principal quantum number of the excited state is : (b) It was observed that when this excited species emits photons of energy =2.64 eV when it comes to next lower energy state. Calculate the nuclear charge of the species. The least energy required to remove an electron from a species is know as the ionization energy (I.E.) of the species. The experimental I.E. of He atom is 24.58 eV .
Hydrogen atom: The electronic ground state of hydrogen atom contains one electron in the first orbit. If sufficient energy is provided, this electron can be promoted to higher energy levels. The electronic energy of a hydrogen-like species (any atom//ions with nuclear charge Z and one electron) can be given as E_(n)=-(R_(H)Z^(2))/(n^(2)) where R_(H)= "Rydberg constant," n= "principal quantum number" A gaseous excited hydrogen-like species with nuclear charge Z can emit radiations of six different photon energies. (a) The principal quantum number of the excited state is : (b) It was observed that when this excited species emits photons of energy =2.64 eV when it comes to next lower energy state. Calculate the nuclear charge of the species. The least energy required to remove an electron from a species is know as the ionization energy (I.E.) of the species. The experimental I.E. of He atom is 24.58 eV .
A
`6`
B
`5`
C
`4`
D
`3`
The energy of an electron in second Bohr orbit of hydrogen atom is :
The energy of an electron in second Bohr orbit of hydrogen atom is :
A
`- 5. 44 xx 10^(-19) eV`
B
`- 5.44 xx 10 ^(-19) cal `
C
`-5.44 xx 1 ^(-19) KJ`
D
` - 5.44 xx 10 ^(-19) J`
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Hydrogen atom: The electronic ground state of hydrogen atom contains one electron in the first orbit. If sufficient energy is provided, this electron can be promoted to higher energy levels. The electronic energy of a hydrogen-like species (any atom//ions with nuclear charge Z and one electron) can be given as E_(n)=-(R_(H)Z^(2))/(n^(2)) where R_(H)= "Rydberg constant," n= "principal quantum number" Calculate the wavelength of light (nm) for the electronic transition of H-atom from the first excited state to ground state. In the model of hydrogen like atom put forward by Niels Bohr (1913) the electron orbits around the central nucleus. the bohr radius of n^(th) orbit of a hydrogen-like species is given by r= k n^(2)/Z " " where, k is constant
Hydrogen atom: The electronic ground state of hydrogen atom contains one electron in the first orbit. If sufficient energy is provided, this electron can be promoted to higher energy levels. The electronic energy of a hydrogen-like species (any atom//ions with nuclear charge Z and one electron) can be given as E_(n)=-(R_(H)Z^(2))/(n^(2)) where R_(H)= "Rydberg constant," n= "principal quantum number" Calculate the following : (a) the kinetic energy (in eV) of an electron in the ground state of hydrogen atom. (b) the potential energy (in eV) of an electron in the ground state of hydrogen atom.
Hydrogen atom: The electronic ground state of hydrogen atom contains one electron in the first orbit. If sufficient energy is provided, this electron can be promoted to higher energy levels. The electronic energy of a hydrogen-like species (any atom//ions with nuclear charge Z and one electron) can be given as E_(n)=-(R_(H)Z^(2))/(n^(2)) where R_(H)= "Rydberg constant," n= "principal quantum number" What is the principal quantum number, n' of the orbit of Be^(3) that has the same Bohr radius as that of ground state hydrogen atom ?
The energy of an electron in the nth Bohr orbit of hydrogen atom is
The energy of an electron in n^"th" orbit of hydrogen atom is