_{}Total energy of (E) of an electron revolving in nth orbit is equal to sum of

**kinetic energy**and

**Potential energy**.

We know the
electron revolve around nucleus due balancing of two forces columbic and
centrifugal forces

This is the
famous Bohr’s equation applicable to Hydrogen like atoms or ions as He

^{+1}, Li^{+2}, Be^{+3}
etc.

The factor
(4 pi epsilon zero) is known as permittivity factor and its numerical value is
1.11268*10

^{-10}C^{2}N^{-1}M^{-2 }( In CGS Unit K= 1)
Pi= 22/7=
3.424, me=9.109 *10

^{-31}kg, e = 1.602 *10^{-10}C and h= 6.626*10^{-34}j-s**Calculation of E**

_{n}in SI Unit:**Bohr’s energy in electron volt:**

We know that,
1eV = 1.602 *10

^{-19}J hence**Energy in term of Rydberg’s Constant:**

**Relation between Total energy (TE), Kinetic energy (KE) and Potential energy (PE):**

**Important conclusions:**

**(1)**The minus sign for the energy of an electron in an orbit represents attraction between the +vely charged nucleus and negatively charged electron.

**(2)**Energy of an electron at infinite distance from the nucleus is zero.

**(3)**As an electron approaches the nucleus, the electrical attraction increases, energy of electron decreases and it becomes negative.

**(4)**Energy of an electron increases as the value of

**‘n’**increases i.e.

**(5)**Value of

**‘n’**remaining unchanged, the amount of energy associated with an electron remains unaltered.

**(6)**Energy of electron in

**first**,

**second**,

**third**and

**fourth**orbit are

**–13.6, –3.4, –1.5, and –0.85 eV**/atom respectively.

**(7)**Although the energy of electron increases with increase in the value of

**‘n’ (orbit),**yet the difference of energy between successive orbits decreases. Thus

**E**etc….

_{2}– E_{1}> E_{3}– E_{2}> E_{4}– E_{3}> E_{5}– E_{4}>,
In the Bohr, atom electrons can be found only in allowed orbits, and these allowed orbits are at different energies. The orbits are analogous to a set of stairs in which the gravitational potential energy is different for each step and in which a ball can be found on any step but never in between. Atom chapter in chemistry is very important because it is very useful in higher studies and if you keep your basic concepts clear from the beginning then it is easy for you to solve any numerical of the atom.

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