2Q_GENCHEM1

Shell

Shell

Energy levels in an atom, denoted by the Principal Quantum Number (n).

Subshell

Sublevels that indicate the shape of orbitals, represented as s, p, d, or f.

Orbital

Specific regions within subshells where electrons can be found.

Electron Configuration

Describes the arrangement and distribution of electrons in an atom's energy levels and sublevels.

Aufbau Principle

Electrons must fill orbitals starting from the lowest energy level up.

Pauli Exclusion Principle

Each orbital can hold a maximum of 2 electrons with opposite spins.

Hund's Rule of Multiplicity

Electrons must fill orbitals singly before pairing to minimize electron repulsion.

Paramagnetism

Property of atoms with unpaired electrons that are slightly attracted to a magnetic field.

Diamagnetism

Property of atoms with all paired electrons that are slightly repelled by a magnetic field.

Octet Rule

Atoms tend to have 8 electrons in their outer shell for stability.

Valence Electrons

Electrons in the outermost shell that determine an atom's chemical reactivity.

Quantum Numbers

Set of numbers that describe the location and energy of an electron.

Lewis Electron Dot Structure (LEDS)

A representation of valence electrons of an atom as dots around the element symbol.

Electronegativity

The tendency of an atom to attract electrons to itself.

Ionic Bond

A bond formed by the transfer of electrons between atoms.

Covalent Bond

A bond formed by the sharing of electrons between atoms.

Chemical Reactivity

Elements with incomplete outer shells (valence electrons) are more reactive.

The two periodic table trends

Groups (columns) and periods (rows)

Principal Quantum Number (n)

Energy level of the electron.

Azimuthal Quantum Number (l)

The shape of the orbital

Magnetic Quantum Number ( ml )

Orientation of the orbital in space which indicates the number of orbitals within a sublevel

Spin Quantum Number (ms)

Describes the spin of the electron around its axis.

Chemical bonding

The force that holds atoms together in compounds

The exception of chemical bonding

Helium only needs 2 valence electrons to be stable, as it follows the DUET RULE. (Same with Hydrogen)

Ionic

metal + nonmetal

Covalent

nonmetal + nonmetal