Quantum Numbers

• The azimuthal quantum number (l) determines the shape of the electron's orbital.
• The magnetic quantum number (m) specifies the orientation of an electron within its subshell, with possible values between -l and l.
• The angular momentum quantum number (l) determines the shape or orbital type, with values ranging from 0 to n-1.
• The principal quantum number (n) determines the energy level.
• The magnetic quantum number (m) specifies the orientation of the orbital in space.
• The spin quantum number (s) describes the intrinsic angular momentum of an electron.
• Each shell has a maximum capacity determined by n^2.
• Electrons can occupy only certain energy levels or orbitals based on their principal quantum number (n).
• The magnetic quantum number (ml) specifies the orientation of an orbital within its subshell, with values ranging from -l to +l.
• Electrons can have different orientations around their orbitals due to spin angular momentum.
• Spin is quantized into two states (+1/2 or -1/2).
• Each orbital can hold up to two electrons with opposite spins.
• Each orbital has a specific set of quantum numbers that determine its properties.
• Orbitals are represented by letters s, p, d, f, g...
• Electrons can only occupy orbitals that have the same value of n but different values of l.
• Sublevels are filled according to Hund's rule, which states that unpaired electrons fill first before pairing up.
• Electrons can have either +1/2 or -1/2 spin.
• S-sublevel contains one orbital at the lowest possible energy level.
• The Pauli exclusion principle states that no more than one electron can be present in any given state.
• Principal quantum number (n): Determines the size of the orbital and how far away it is from the nucleus.
• Azimuthal quantum number (l): Specifies the shape of the orbital and determines whether it's s, p, d, f, etc.
• Hund's rule applies when filling subshells with multiple electrons.
• Helium is an exception because it has two electrons and follows slightly different rules due to their interaction.
• Hydrogen-like atoms have one electron and follow the same rules as hydrogen.
• P-sublevel consists of three orbitals arranged around the nucleus with increasing energy levels.
• D-sublevel comprises five orbitals arranged around the nucleus with increasing energy levels.
• F-sublevel includes seven orbitals arranged around the nucleus with increasing energy levels.