QMA Flashcards
What did Schrodinger’s model describe?
A region in space with a high probability of finding an electron is called an orbital or cloud.
What are the 4 quantum numbers?
n, l, m, s
What does n stand for?
The energy level/cloud. It is the Principle Quantum number. Indicates how far from the nucleus the electron is and its energy.
How do you know how many electrons each energy level can hold?
2n^2
What does L stand for?
sublevel / Azimuthal Quantum Number (divides the table into s,d,p,f)
What shapes does each energy level have?
S: sphere
P: dumbell
D + F: undetermined, weird shapes
What does ml stand for?
orbital (3rd / magnetic quantum number)
Each orbital can hold how many electrons?
2
What does the surface of the orbital represent?
Where any particular electron can be found 90% of the time
how many orbitals does the S sublevel have?
1
How many orbitals does the p sublevel have
3
How many orbitals does the D sublevel have
5
How many orbitals does the F sublevel have
7
What does Ms stand for
spin. The electrons within an orbital must have opposite spins to minimize their repulsion, which we represent with opposite arrows
Coulomb’s Law
like charges repel and vice versa. The force is proportional to the magnitude of the charges and inversely proportional to the square of the distance between them.
Aufbau Principle
Electrons are placed in orbitals of lowest energy first
Pauli Exclusion Principle
An orbital can only hold 2 electrons, no 2 electrons can have the same quantum #s, they must have opposite spins
Hund’s Rule
When filling a sublevel, one electron enters each energy level until each orbital is full
How does Atomic Radius act in groups?
Increases down a group
How does Atomic Radius act in periods?
Increases right to left
