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(c) Distance of closest approach, r0 = 2Ze2/(4πε0)E
Here E = ½ mv2 = KE of the α particle.
Bohr’s atomic model:-
(a) The central part of the atom called nucleus, contains whole of positive charge and almost whole of the mass of atom. Electrons revolve round the nucleus in fixed circular orbits.
(b) Electrons are capable of revolving only in certain fixed orbits, called stationary orbits or permitted orbits. In such orbits they do not radiate any energy.
(c) While revolving permitted orbit an electron possesses angular momentum L (= mvr) which is an integral multiple of h/2π.
L=mvr =n (h/2π)
Here n is an integer and h is the Planck’s constant.
(d) Electrons are capable of changing the orbits. On absorbing energy they move to a higher orbit while emission of energy takes place when electrons move to a lower orbit. If f is the frequency of radiant energy,
hf= W2-W1
Here W2 is the energy of electron in lower orbit and W1 is the energy of electron in higher orbit.
(e) All the laws of mechanics can be applied to electron revolving in a stable orbit while they are not applicable to an electron in transition.
Bohr’s Theory of Atom:-
(a) Orbital velocity of electron:- vn= 2πkZe2/nh
For a particular orbit (n= constant), orbital velocity of electron varies directly as the atomic number of the substance.
vn∝Z
(b) For a particular element (Z= constant), orbital velocity of the electron varies inversely as the order of the orbit.
vn∝1/n
(c) v = nh/2πmr
Relation between vn and v1:-vn = v1/n
Radius of electron:-
r= n2h2/4π2kmZe2
So, r∝n2
For, C.G.S system (k = 1), r = n2h2/4π2mZe2
S.I (k = 1/4πε0), r =(ε0/π) (n2h2/mZe2)
Kinetic energy of the electron:- It is the energy possessed by the electron by virtue of its motion in the orbit.
K.E = ½ mv2 = ½ k (Ze2/r)
Potential energy:- It is the energypossessed by the electronby virtue of its position near the nucleus.
P.E = -k (Ze2/r )
Total energy:-
W= K.E + P.E
W=- ½ k (Ze2/r) = -k2 2π2Z2me4/n2h2
For, C.G.S (k = 1), W = - [2π2Z2me4/n2h2]
For, S.I. ( k = 1/4πε0), W = - (1/8ε02) [Z2me4/n2h2]
Since, W∝1/n2, a higher orbit electron possesses a lesser negative energy (greater energy) than that of a lower orbit electron.
Frequency, wavelength and wave number of radiation:-
Frequency, f = k2[2π2Z2me4/h3] [1/n12 – 1/n22]
Wave number of radiation,
Here R is the Rydberg’s constant and its value is,
R= k2 [2π2Z2me4/ch3]
Bohr’s theory of hydrogen atom (Z=1):-
(a) Radius of orbit:-
r= n2h4/4π2me2 (C.G.S)
r= (ε0/π) (n2h2/me2) (S.I)
(b) Energy of electron:-
W= 2π2me4/n2h2 (C.G.S)
W =(1/8ε0)[me4/n2h2]
(c) Frequency, wavelength and wave number of radiation:-
C.G.S:- k =1 and Z=1
Frequency= f=2π2me4/h3 [1/n12 – 1/n22]
Wave number = 1/λ = 2π2me4/ch3 [1/n12 – 1/n22]
S.I:- k =1/4πε0 and Z=1
Frequency= f = (1/8ε0) (me4/h3)[1/n12 – 1/n22]
Wave number = 1/λ = (1/8ε02) (me4/ch3)[1/n12 – 1/n22]
Rydberg’s constant:- R=k2 =2π2z2 me4/ch3
For hydrogen atom, Z = 1, R = RH = k2 (2π2 me4/ch3).
For C.G.S system (k=1), RH = 2π2 me4/ch3
For S.I system (k=1/4πε0), RH = (1/8ε02) (me4/ch3)
Wave number, 1/λ = RH [1/n12 – 1/n22]
Hydrogen Spectrum:-
(a) For Lyman series:- 1/λ = R [1– 1/n2], n = 2,3,4…..∞
(b) For Balmer series:- 1/λ = R [1/22 – 1/n2], n =3,4,5…..∞
(c) For Paschen series:-1/λ = R [1/32 – 1/n2], n =4,5,6…..∞
(d) For Brackett series:-1/λ = R [1/42 – 1/n2], n =5,6,7…..∞
(e) P-fund series:-1/λ = R [1/52 – 1/n2], n =6,7,8…..∞
Series limits (λmin):-
(a) Lyman:- λmin = 912 Å
(b) Balmer:-λmin = 3645 Å
(c) Paschen:- λmin = 8201 Å
Energy levels of hydrogen atom:-
W = -k22π2me4/n2h2
For, n=1, W1 = -13.6 eV
For the first excited state, n=2, W2 =W1/4 = (-13.6/4) eV = -3.4 eV
For the second excited state, n=3, W3 =W1/9 = (-13.6/9) eV = -1.51 eV
Similarly, for other excited states, W4 = -0.85 eV and W5 = -0.54 eV
Number of emission lines from excited state:-n = n(n-1)/2
Ionization energy:-
- E1 = +(13.6Z2)eV
(a) For H-atom, I.E = 13.6 eV
(b) For He+ ion, I.E = 54.4 eV
(c) For Li++ ion, I.E = 122.4 eV
Ionization potential:-
(a) For H-atom, I.P = 13.6 eV
(b) For He+ ion, I.P = 54.42 eV
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