Putting the quantum numbers together

Each time you move higher in a major energy level, you add another orbital type. So when you move from energy level 1 to energy level 2 (n = 2), there can be both s and p orbitals. 

If you write out the quantum numbers for energy level 3, you see s, p, and d orbitals. 

Chemists find quantum numbers useful when they re looking at chemical reactions and bonding (and those are things many chemists like to study). But they find two other representations for electrons — energy level dieigreuns and electron configurations — more useful and easier to work with. 

Chemists use both of these things to represent which energy level, subshell, and orbital are occupied by electrons in any particular atom. Chemists use this information to predict what type of bonding will occur with a peirticular element cuid to show exactly which electrons are being used. These representations are also useful in showing why certain elements behave in similar ways. 

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In order to obtain the total (atomic) angular momentum (mechanical moment), we must put the quantum numbers together... 

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