What are the postulates of Bohr's model of hydrogen atom?Discuss the importance of this model to explain
various series of line spectra in hydrogen atom
Answers
Answer:
Postulates of Bohr’s Model of an Atom
1.In an atom, electrons (negatively charged) revolve around the positively charged nucleus in a definite circular path called as orbits or shells.
2.Each orbit or shell has a fixed energy and these circular orbits are known as orbital shells.
The energy levels are represented by an integer (n=1, 2, 3…) known as the quantumnumber This range of quantum number starts from nucleus side with n=1 having the lowest energy level. The orbits n=1, 2, 3, 4… are assigned as K, L, M, N…. shells and when an electron attains the lowest energy level it is said to be in the ground state.
3.The electrons in an atom move from a lower energy level to a higher energy level by gaining the required energy and an electron moves from a higher energy level to lower energy level by losing energy.
Explanation:
Hope this may help you.....
Answer:
Postulates of Bohr’s Hydrogen atom:
1. An atom has a number of stable orbits in which an electron can reside without the emission of radiant energy. Each orbit corresponds, to a certain energy level.
2. An electron may jump spontaneously from one orbit (energy level E1) to the other orbit (energy level E2, where E2 > E1); then the change in energy in the electron jump is given by Planck’s equation:
∆E = E2-E1= hv
Where h = Planck’s constant , v = frequency of light emitted.
3. The motion of an electron in a circular orbit is restricted in such a manner that its angular momentum is an integral multiple of h/2π, Thus
mvr = nh/2π, where m = mass of the electron
v = velocity of the electron , r = radius of the orbit an
n = an integer called principal quantum number of the electron.
4. A special surface around nucleus which contained orbits of equal energy and radius was called shell. The 'energy levels' or 'shells' or 'orbits' are represented in two ways: either by the numbers 1, 2, 3, 4, 5 and 6 or by letters K, L, M, N, O and P. The energy levels are counted from centre outwards.
5. Each energy level is associated with a fixed amount of energy. The shell nearest to the nucleus has minimum energy and the shell farthest from the nucleus has maximum energy. • There is no change in the energy of electrons as long as they keep revolving with the same energy level. But, when an electron jumps from a lower energy level to a higher one, some energy is absorbed while some energy is emitted.
The importance of this model to exxplain the various series of line spectra in hydrogen atom:
Bohr tells us that the electrons in the Hydrogen atom can only occupy discrete orbits around the nucleus where they do not radiate energy.
When the electron moves from one allowed orbit to another it emits or absorbs photons of energy matching exactly the separation between the energies of the given orbits (emission/absorption spectrum).
We see these photons as lines of coloured light (let’s say, the Balmer Series) in emission or dark lines in absorption.
Explanation:
The first is incorrect because Electrons do not orbit. They entangle into arrays at either end of the Dumbbell Nucleus . These are separated by Entangled Valence Electrons, which are held in an Inertial Entanglement with their Protons. When the Proton jumps Quantum State, the entanglement is broken unless the Electron jumps to a Muon, as the jump causes reversal of Chirality of the Outer Shell.
The second postulate essentially still works, but if Bohr believed in spontaneity then he really did not have the first clue about Quantum Mechanics which although 4D is entirely deterministic, and this has been demonstrated mathematically way beyond any reasonable doubt.