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5.ATOMIC STRUCTURE eLearn.Punjab

E4 = - 1313.31 = -82.08 kJmol-1
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E5 = - 1313.31 = -52.53 kJmol-1
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E∞ = - 1313.31 = 0 kJmol-1 (electron is free from the nucleus)
∞2

The values of energy differences between adjacent orbits can be calculated as follows

E2-E1 = (-328.32)-(-1313.31) = 984.99 kJmol-1
E3-E2 = (-145.92)-(-328.32) = 182.40 kJmol-1
E4-E3 = (-82.08)-(-145.92) = 63.84 kJmol-1
The differences in the values of

energy go on decreasing from lower

to higher orbits.

E2 -E1 >E3 -E2 >E4 -E3 >..........................

The energy difference between

first and infinite levels of energy is

calculated as:

E„ - E1 = 0 - (-1313.31) = 1313.31
kJmol-1

1313.31 kJmol-1 is the ionization

energy of hydrogen. This value

is the same as determined Fig (5.12) Energy values associated with an
experimentally. These values show electron in vanous orbits in hydrogen atom
that the energy differences between

adjacent orbits of Bohr’s model of hydrogen atom go on decreasing sharply.

Keep in mind, that distances between adjacent orbits increase. The Fig (5.12) makes the idea

clear.

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