How many radial nodes are in a given atomic orbital as a function of #n# and #l#?
The total number of nodes in general is given by
#"Number of Nodes" = n - 1#,
#n#is the principal quantum number, and #n = 1, 2, 3, 4, . . . #, given as the numerical coefficient for the orbital.
The angular momentum quantum number
#"Number of Angular Nodes" = l#
Since there are only two types (radial, angular), it follows that:
#color(blue)(barul(|stackrel(" ")(" ""Number of Radial Nodes" = n - l - 1" ")|))#
CHALLENGE: Given the above radial density distribution, how many radial nodes are in each orbital? Can you show what it is, mathematically? If there were radial nodes in a radial density distribution, can you describe what you would see occur in the graph?