LESSON 1: ELECTRONIC STRUCTURE OF ATOMS Flashcards
The collection of values that represent an atom’s electron’s energy and location.
Quantum Numbers
It states that no two electrons can have the same set of four quantum numbers.
The Pauli Exclusion Principle
This is denoted by the letter n, describes the energy of an electron and the most probable distance of the electron from the nucleus.
Principal Quantum Number
It is also known as azimuthal quantum number, denoted by l, describes the shape of the orbital.
Orbital Angular Momentum Quantum Number
It is denoted by ml, describes the energy levels in a subshell.
Magnetic Quantum Number
It is denoted by ms, refers to the spin on the electron.
Electron Spin Quantum Number
The magnetic state of an atom with 1 or more unpaired electrons.
Paramagnetism
It states that electrons must occupy every orbital singly before any orbital is doubly occupied; may leave the atom with many unpaired electrons.
Hund’s Rule
It is characterized by paired electrons.
Diamagnestism
These are visual representations that show how electrons are distributed throughout an atom’s orbitals
Orbital Diagrams
Electrons prefer to occupy orbitals singly with parallel spin.
Hund’s Rule
How many boxes is the S orbital represented by? How many electrons are in it?
1 box, 2 electrons
How many boxes is the P orbital represented by? How many electrons are in it?
3 boxes. 6 electrons
How many boxes is the D orbital represented by? How many electrons are in it?
5 boxes, 10 electrons
How many boxes is the F orbital represented by? How many electrons are in it?
7 boxes, 14 electrons
