Module 1-3 Flashcards
The orbitals are arranged in order of increasing energy based on the principal energy levels and the sublevels where they are in. 1s 2s 2p…
Aufbau Principle
This means no atomic orbital can contain more than TWO electrons and these electrons must be of opposite spin if they are to form a pair within an orbital. The boxes… ORBITAL DIAGRAM
Pauli’s Exclusion Principle
- The most stable arrangement of electrons is one with the maximum number of unpaired electrons.
- This minimized the electron-electron repulsions and stabilizes the atom.
Up arrows first, then Down arrows
Hund’s Rule
what is s, p, d, f stands for?
Sharp
Principal
Diffuse
Fundemental
What are the noble gases?
Helium, Neon, Argon, Krypton, Xenon, Radon
Atomic mass of
Helium
Neon
Argon
Helium = 2
Neon = 10
Argon = 18
Atomic mass of
Krypton
Xenon
Radon*
Krypton = 36
Xenon = 54
Radon = 86
- These are the electrons that are found on the outermost energy level of an atom.
- These electrons are important because they give us a deep insight about the chemical property of an element.
VALENCE ELECTRONS
The use of noble gases
CORE METHOD
Paramagnetism and Diamagnetism
MAGNETIC PROPERTY
(attracted to magnetic field) refers to the magnetic state of an atom with one or more unpaired electrons.
Paramagnetism
(repelled by magnetic field) paired electrons. This causes the magnetic fields of the electrons to cancel out; there is no net magnetic moment, and the atom cannot be attracted into a magnetic field.
Diamagnetism
1s² 2s² 2p⁶ 3s² 3p⁴, ? = 6
Valence electron = 6
1s² 2s² 2p⁶ 3s² 3p⁴
Valence Shell = 3
- Numbers that are used to describe the probable
location of an electron in an atom. - These numbers work like addresses for electrons
in an atom.
Quantum numbers
describes the energy level of the electron. The energy of the electron is determined by its average distance from the nucleus. “1s² 2s² 2p⁶”
Principal Quantum Number (n)
It describes the “shape” of the orbital. It designates the sublevel which the electron is said to occupy.s = 0, p = 1, d = 2 and f =
3.
Azimuthal or Angular Momentum Quantum Number (l)
describes the shape of the orbitals in a SUBSHELL. Orbitals have shapes that are best described as spherical, polar or cloverleaf. THE BOXES
Magnetic Quantum Number (ml)
refers to the “spin” of an electron in a given orbital. It can only have two values: +1/2 and -1/2.
DOWN = -1/2 , UP = +1/2
Spin Quantum Number (ms)
