Atoms Flashcards
what did Thomson model explain
1) uniformly distributed positive charge
2) electron->watermelon seed
3)plum pudding model
limitation of the Thomson model
1) origin of spectral series
2)alpha particle scattering
Rutherford model
1)small and massive central core of +ve charge
2)the size of nucleus is very small
Rutherford model limitation
1)cannot explain the stability of atom
2)they would emit a continuous spectrum instead of the actually observed line spectrum
BOHR’S ATOMIC MODEL
1)Electrons revolve around the nucleus in fixed circular paths called
Orbits or Shells.
2)Electron in its own shell does not lose or gain energy. It loses or
gains energy when it jumps from one shell to another
3)The Angular Momentum of electron is quantized in the shell.
L = (nh)/(2pi)
Bohr radius of hydrogen
r = 0.53 (n^2)/z A
bohr radius formula
(Eon^2h^2)/pimz*e^2
velocity of electron
v = 2.186 x 10^6 * z/n
potential energy of electron
P.E=-e^2/(4piEo*r)
energy of hydrogen in the Nth orbit
E=-13.6/n^2 eV
energy of atom
-2pi^2mk^2e^4/h^2*n^2
frequency of emitted photon
h*mu=En2-En1
Rydberg formula for the spectrum of hydrogen series
wave number=r[1/(n1^2)-1/(n2^2)]
r->rydberg constant->1.097310^7 m^-1
lyman series
electron jumps from higher energy level to n=1 energy level
ultraviolet region
wave number=R[1/(1^2)-1/(n2^2)]
balmer series
electron from n=3,4,4,etc to n=2
visible region
wave number=R[1/(2^2)-1/n2^2]
paschen series
electron from n=4,5,,etc to n=3
infrared region
wave number =R[1/3^2-1/n2^2]
brackett series
electron from n=5,6,etc to n=4
infrared region
wave number=R[1/4^2-1/n2^2]
pfund series
electron from n=6,7,etc to n=5
infrared region
wave number=R[1/5^2-1/n2^2]
limitation of bohr theory
-> This theory is only applicable for hydron-like series
-> Why only circular orbits not elliptical orbits
->electron has a wave nature so orbits of electrons are not defined
->does not explain the further splitting of spectral lines in a magnetic
and electric field
excitaion energy
energy required to jump from lower to higher state
ionisation energy
energy required to remove an electron from an atom
relationship between kinetic energy and potential energy
P.E=-2 K.E