Lecture 2 (Electronic Structure, Atomic Orbitals, etc.) Flashcards
The region of space defined by Ψ is called an …
atomic orbital
What are 3 quantum numbers atomic orbitals are characterized by?
Principle (energy), Orbital (shape), Magnetic (directionality)
What is a node?
A point where the electron probability is zero.
What are the types of nodes?
Angular and Radial
How many angular nodes are in s orbital?
0 angular nodes
How many angular nodes are in p orbitals?
1 angular node
How many nodes in d orbitals?
2 angular nodes
How many nodes are in f orbitals?
3 angular nodes
What is the type for the remaining nodes?
radial
What does triply degenerate mean?
3 orbitals all have the same energy
What degenerate are s orbitals?
singly degenerate
What degenerate are p orbitals?
triply degenerate
What degenerate are d orbitals?
five-fold degenerate
What degenerate are f orbitals?
seven-fold degenerate
What is the VSEPR geometry of PH3
Trigonal pyramidal
Why do trigonal pyramidal structures of heavy pnictogen hydrides have narrow bond angles?
The orthogonal p orbitals and the lone pair hosted in an orbital with mainly s character.
What is the “inert par effect”?
When heavier elements are less likely to have hybridization (mixing) of orbitals
What is the radial component of a wavefunction associated with?
size of the orbitals
What is the trend of the radial component?
it decays exponentially as the distance from the nucleus increases
What is one thing that changes in radial nodes?
the signs (+/-)
What is 4πr^2R(r)^2?
The radial probability of finding the electron in a given region of space.
What is the radial probability when the electron is at the nucleus?
zero for all orbitals
What happens when you increase n?
orbitals become larger and diffuse more, as the electrons they hosted are distributed over a larger region of space
What is a consequence because of this?
the orbitals overlap for heavier elements is less efficient and the bonds formed are weaker.
