Octet Rule
This rule states that atoms tend to gain, lose, or share electrons to have 8 electrons in their valence shell.
Octet Rule
This diagram shows valence electrons as dots around element symbols.
Lewis Dot Structure
This theory predicts the shape of molecules based on electron pair repulsion.
VSEPR theory
A molecule with two atoms bonded to the central atom and no lone pairs, forming a 180° bond angle.
Linear
Atoms achieve stability under the octet rule by gaining, losing, or sharing these particles.
Electrons
In a Lewis structure, this atom is usually placed in the center because it can form the most bonds.
Central atom
The molecular shape of CO₂.
Linear
A molecule with three atoms around the central atom arranged evenly in a flat triangle with 120° bond angles.
Trigonal Planar
This is the outermost electron shell where bonding usually occurs.
Valence shell
These electrons are not shared and remain on a single atom.
Lone pairs
The molecular shape of CH₄.
Tetrahedral
A molecule where the central atom has two bonding pairs and two lone pairs, causing the molecule to form a V-shape.
Bent
This group of elements naturally satisfies the octet rule and rarely forms bonds
Noble Gases
In CO₂, this atom is located at the center of the Lewis structure.
Carbon
The molecular shape of NH₃.
Trigonal Pyramidal
A molecule with three bonded atoms and one lone pair on the central atom, creating a pyramid-like shape.
Trigonal pyramidal
Atoms achieve the octet rule during bonding by doing these three processes.
Gaining, losing, or sharing electrons
The scientist who introduced the Lewis dot structure to represent valence electrons in atoms and molecules.
Gilbert N. Lewis
The molecular shape of H₂O.
Bent
A molecule with four bonded atoms around a central atom arranged in a 3D pyramid-like structure with equal bond angles (~109.5°).
Tetrahedral