One of the fundamental laws of physics is that matter is most stable with the lowest possible energy. Thus, the electron in a hydrogen atom usually moves in the n=1 orbit, the orbit in which it has the lowest energy. When the electon is in this lowest energy orbit, the atom is said to be in its ground electronic state. If the atom receives energy from an outside source, it is possible for the electron to move ot an orbit with a higher n value, in which case the atoms is in an excited state with a higher energy.
The law of conservation of energy says that we cannot create or destroy energy. Thus, if a certain amount of external energy is required to excite an electron from one energy level to another, then that same amount of energy will be liberated when the electron returns to its initial state.
Lyman series is observed when the electron returns to the lowest orbit while Balmer series is formed when the electron returns returns to second orbit. Similarly, Paschen, Brackett and Pfund series are formed when electrons returns to the third, fourth and fifth orbits from higher energy orbits respectively.
When electrons return form `n_(2) " to " n_(1)` state, the number of lines in the spectrum will equal to
`((n_(2)-n_(1))(n_(2)-n_(1)+1))/(2)`
If the electon comes back from energy level having energy `E_(2)` to energy level having energy `E_(1)`, then the difference may be expressed in terms of energy of photon as :
`E_(2)-E_(1)=DeltaE, deltaE implies (hc)/(lambda)`
Since, h and c are constant, `deltaE` corresponds to definite energy. Thus, each transition from one energy level to another will produce a radiatiob of definite wavelength. This is actually Wave number of a spectral line is given by the formula
`barv=R((1)/(n_(1)^(2))-(1)/(n_(2)^(2)))`.
where R is a Rydberg's constant `(R=1.1xx10^(7) m^(-1))`
What transition in the hydrogen spectrum would have the same wavelength as Balmer transitio, `n=4 " to "n=2` in the `He^(+)` spectrum?
One of the fundamental laws of physics is that matter is most stable with the lowest possible energy. Thus, the electron in a hydrogen atom usually moves in the n=1 orbit, the orbit in which it has the lowest energy. When the electon is in this lowest energy orbit, the atom is said to be in its ground electronic state. If the atom receives energy from an outside source, it is possible for the electron to move ot an orbit with a higher n value, in which case the atoms is in an excited state with a higher energy.
The law of conservation of energy says that we cannot create or destroy energy. Thus, if a certain amount of external energy is required to excite an electron from one energy level to another, then that same amount of energy will be liberated when the electron returns to its initial state.
Lyman series is observed when the electron returns to the lowest orbit while Balmer series is formed when the electron returns returns to second orbit. Similarly, Paschen, Brackett and Pfund series are formed when electrons returns to the third, fourth and fifth orbits from higher energy orbits respectively.
When electrons return form `n_(2) " to " n_(1)` state, the number of lines in the spectrum will equal to
`((n_(2)-n_(1))(n_(2)-n_(1)+1))/(2)`
If the electon comes back from energy level having energy `E_(2)` to energy level having energy `E_(1)`, then the difference may be expressed in terms of energy of photon as :
`E_(2)-E_(1)=DeltaE, deltaE implies (hc)/(lambda)`
Since, h and c are constant, `deltaE` corresponds to definite energy. Thus, each transition from one energy level to another will produce a radiatiob of definite wavelength. This is actually Wave number of a spectral line is given by the formula
`barv=R((1)/(n_(1)^(2))-(1)/(n_(2)^(2)))`.
where R is a Rydberg's constant `(R=1.1xx10^(7) m^(-1))`
What transition in the hydrogen spectrum would have the same wavelength as Balmer transitio, `n=4 " to "n=2` in the `He^(+)` spectrum?
The law of conservation of energy says that we cannot create or destroy energy. Thus, if a certain amount of external energy is required to excite an electron from one energy level to another, then that same amount of energy will be liberated when the electron returns to its initial state.
Lyman series is observed when the electron returns to the lowest orbit while Balmer series is formed when the electron returns returns to second orbit. Similarly, Paschen, Brackett and Pfund series are formed when electrons returns to the third, fourth and fifth orbits from higher energy orbits respectively.
When electrons return form `n_(2) " to " n_(1)` state, the number of lines in the spectrum will equal to
`((n_(2)-n_(1))(n_(2)-n_(1)+1))/(2)`
If the electon comes back from energy level having energy `E_(2)` to energy level having energy `E_(1)`, then the difference may be expressed in terms of energy of photon as :
`E_(2)-E_(1)=DeltaE, deltaE implies (hc)/(lambda)`
Since, h and c are constant, `deltaE` corresponds to definite energy. Thus, each transition from one energy level to another will produce a radiatiob of definite wavelength. This is actually Wave number of a spectral line is given by the formula
`barv=R((1)/(n_(1)^(2))-(1)/(n_(2)^(2)))`.
where R is a Rydberg's constant `(R=1.1xx10^(7) m^(-1))`
What transition in the hydrogen spectrum would have the same wavelength as Balmer transitio, `n=4 " to "n=2` in the `He^(+)` spectrum?
A
n=3 to n=1
B
n=3 to n=2
C
n=4 to n=1
D
n=2 to n=1
Text Solution
Verified by Experts
Topper's Solved these Questions
Similar Questions
Explore conceptually related problems
The lowest energy state of electron is known as:
The only electron in the hydrogen atom resides under ordinary conditions on the first orbit. When energy is supplied, the electron moves to higher energy orbit depending on the amount of energy absorbed. When this electron returns to any of the lower orbits, it emits energy. Lyman series is formed when the electron returns to the lowest orbit while Balmer series is formed when the electron returns to second orbit. Similarly, Paschen, Brackett and Pfund series are formed when electron returns to the third, fourth orbits from higher energy orbits respectively (as shown in figure) Maximum number of lines produced when an electron jumps from nth level to ground level is equal to (n(n-1))/(2) . For example, in the case of n = 4, number of lines produced is 6. (4 rarr 3, 4 rarr 2, 4 rarr 1, 3 rarr 2, 3 rarr 1, 2 rarr 1) . When an electron returns from n_(2) to n_(1) state, the number of lines in the spectrum will be equal to ((n_(2) - n_(1))(n_(2)-n_(1) +1))/(2) If the electron comes back from energy level having energy E_(2) to energy level having energy E_(2) then the difference may be expressed in terms of energy of photon as E_(2) - E_(1) = Delta E, lambda = (h c)/(Delta E) . Since h and c are constant, Delta E corresponds to definite energy, thus each transition from one energy level to another will prouce a higher of definite wavelength. THis is actually observed as a line in the spectrum of hydrogen atom. Wave number of the line is given by the formula bar(v) = RZ^(2)((1)/(n_(1)^(2)) - (1)/(n_(2)^(2))) Where R is a Rydberg constant (R = 1.1 xx 10^(7)) (i) First line of a series : it is called .line of logest wavelength. or .line of shortest energy.. (ii) Series limit of last of a series : It is the line of shortest wavelength or line of highest energy. The difference in the wavelength of the 2^(nd) line of Lyman series and last line of Bracket series in a hydrogen sample is
The energy of the electron in the hydrogen atom depends on
The shell which has lowest energy in an atom is
The energy of an electron present in Bohr's second orbit of hydrogen atom is
The energy required to excite the electron from ground state of hydrogen atom to first excited state is
The energy of the electron in the hydrogen atom is given by the expression