The energy level depends on the value of n+l where n is the principal quantum number and 'l' is the azimuthal quantum number. For same value of n+l, higher the value of n, higher is the energy level. The value of l is 0,1,2 and 3 for s, p, d and f respectively.
a)
Orbital | 3d | 4s |
n | 3 | 4 |
l | 2 | 0 |
n+l | 5 | 4 |
Thus, 3d is higher in energy because it has higher value of n+l
b)
Orbital | 4p | 5s |
n | 4 | 5 |
l | 1 | 0 |
n+l | 5 | 5 |
Here, the n+l values are equal. Hence, higher n has higher energy. Thus, 5s has higher energy level.
c)
Orbital | 3d | 3p |
n | 3 | 3 |
l | 2 | 1 |
n+l | 5 | 4 |
Thus, 3d is higher in energy because it has higher value of n+l
d)
Orbital | 5s | 4f |
n | 5 | 4 |
l | 0 | 3 |
n+l | 5 | 7 |
Thus, 4f is higher in energy because it has higher value of n+l
5. Indicate the higher of the two energy states in each of the following pairs: a....
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Determine the number of distinct quantum states for each of the following configurations. In each case, list the spectroscopic symbols of the allowed states. (a) two equivalent d electrons [e.g. (3d)?] (b) two non-equivalent d electrons [e.g. (3d)-(4d'] (c) the configuration (4p)(48) (d) the configuration (2p)? (3p)1 Use Hund's rules to predict the ordering in energy of the (3d)2 states-i.e. those found in Part (a) of Problem 1.
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The 5p subshell lies immediately above which of the following subshells in energy? (Which subshell is just below the 5p in energy) A.5s B.4f C.5d D.4d E.4p
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