Lecture 3 Flashcards
s orbital shape
- sphere
- does not depend on phi or theta
possible values for principal quantum number in s orbitals
n = 1, 2, 3, 4, …
possible values for orbital quantum number in s orbitals
l = 0
possible values for magnetic quantum number in s orbitals
ml = 0
nodes
consequence of wave like properties of electrons for a simple wave
difference of s orbitals
all spherical but have different nodes in the inside
orbitals
stable, 3-dimensional standing waves with no destructive interference
possible values for principal quantum number in p orbitals
n = 2, 3, 4, …
possible values for quantum number in p orbitals
l = 1
possible values for magnetic quantum number for p orbitals
ml = -1, 0, 1
nodal plane
zero electron density that bisects an orbital and contain the nucleus
px, py, pz orbitals
- perpendicular to each other
- phase is opposite on opposite side of planar node
3p orbital
- analogous to 2s orbital internal structure (contains 1 radial node and planar node from all p orbitals)
possible values for principal quantum number for d orbitals
n = 3, 4, 5, …
possible values for quantum number for d orbitals
l = 2
possible values for magnetic quantum number for d orbitals
ml = -2, -1, 0, 1, 2
dxz, dyz, dxy orbitals
have lobes between the axes and nodes in the axes
dx^2-y^2 orbital
has lobes on x and y axes
dz^2 orbital
large lobes of electron density on z plane and smaller torr in x-y plane as well as 2 conical nodes fanning out
dz^2 shape
two d orbitals (that have the same shape of other d orbitals) are added together
principal quantum number (n)
gives the size and energy of the atomic orbital
orbital quantum number (l)
gives the shape of the orbital
magnetic quantum number (ml)
gives the orientation of the orbital
