what are the differences b/w radial nodes and angular nodes ?
Node is the point of zero displacement, no electrons are found.
Radial node is a spherical surface where the probability of an electron being found is 0 and the probability density equals 0 as well. They radiate like circles away from the nucleus.
Angular nodes is a plane dividing wave functions by phase (dividing negative and positive)
Radial: Each atomic orbital will have n-l-1 radial nodes. So a 3p orbital has 3-1-1 = 1 radial node.
Angular: An atomic orbital will have l angular nodes. So, an s-orbital has 0 angular node and p-orbital has 1 angular node, and so on.
where n is principal quantum number (n can be any positive integer (1,2,3,4...)); l is angular momentum quantum number (l can equal: 0,1,2,3,4...(n-1). Notation used for l are 0 = s;1 = p;2 = d;3 = f).
Node is the point of zero displacement, no electrons are found.
Radial node is a spherical surface where the probability of an electron being found is 0 and the probability density equals 0 as well. They radiate like circles away from the nucleus.
Angular nodes is a plane dividing wave functions by phase (dividing negative and positive)
Radial: Each atomic orbital will have n-l-1 radial nodes. So a 3p orbital has 3-1-1 = 1 radial node.
Angular: An atomic orbital will have l angular nodes. So, an s-orbital has 0 angular node and p-orbital has 1 angular node, and so on.
where n is principal quantum number (n can be any positive integer (1,2,3,4...)); l is angular momentum quantum number (l can equal: 0,1,2,3,4...(n-1). Notation used for l are 0 = s;1 = p;2 = d;3 = f).
