Atomic Orbitals video Flashcards
Atomic orbitals
Possible waves that fit the atomic constraints
Principle quantum number decides: (n)
The size of the orbitals
Possible quantum numbers:
any positive integer no zero
angular momentum number defines (l) (3)
Shape of orbital
-tells u if you have s,p,d orbital
*Shape of wave depends on l
angular momentum number defines (l) (2)
Shape of orbital
*Shape of wave depends on l
Possible values of l
0,…(n-1)
Magnetic quantum number (ml) defines (2)
orientation of the orbital
Where it is pointing
possible ml numbers
-l to +l (and in between.)
l=0 orbital describe (2)
s orbital
sphere
l=1 orbital describe(3)
1 angular node
Formation of an orbital with two distinct part
p orbital
describe a l=2 orbital (4)
2 angular nodes
sphere cut into 4
every time you cross a node, you switch phases
d orbital
as n get bigger…
(2)
size increase
radial nodes increase
describe what each value means: 2s
2= value of “n”
s=the shape
what orbital has no radial nodes
1s
radial node (2)
spherical surface region where the probability of finding an electron is zero.
determined by principal quantum number
angular node (5)
flat planes (or cones) where the probability of finding an electron is zero. The number of angular node present in an atom is determined by the angular momentum quantum number. Angular nodes occur as the angular momentum quantum number increases.
cuts across
upper half and bottom half of the wave are different from each other.
All of the orbitals with the same value of n are all in the
same shell
in n=2 shell there are ___ places to put electrons
4
In the n=2 shell there are ___ sub shells
2
Whenever we go from one shell to another
there is a big jump in size
in terms of n,spd,m what are
shell
subshell
oribital
defined by
shell-quantum number
subshell- spade,
orbital- m
electrons located in the outermost level
have higher energy because it takes more effort and energy to pull electrons away from the centre