Chemical Bonding Flashcards
Valence Electrons
- Electrons in the outermost orbit
- Used to bond with other atoms
Octet Rule
Atoms tend to gain , loose , or share electrons to fill their outermost energy level with eight valence electrons.
Cation
Positive Ion
Anion
Negative Ion
Polyatomic Ion
When more than one element groups together and has a charge.
Intramolecular bonding
- Forces that hold atoms together within a molecule
- 3 types : Ionic , Metallic, Covalent
Ductility
Ability to stretch
Malleability
Ability to be bent or hammered out of shape
Sea of electrons
The body of delocalized electrons that surrounds positive metal ions in metallic bonds
Alloy
Formed when other elements are introduced into a metallic crystal.
- have chemical and physical properties that are better suited to certain applications
Substitutional alloy
Atoms of the original metal are replaced by other metal atoms of the same size.
( e.g, Brass, Bronze, Sterling Silver)
Interstitial alloy
The small holes in the metallic crystal are filled with smaller atoms.
(e.g., Steel)
Single bond
Atoms share a single pair of electrons
Double bond
Atoms share two pairs of electrons
Triple bond
Atom shared three pairs of electrons
Network Covalent Crystal
Atoms that are covalently bonded to each other
Resonance
Structures that differ only in the position of double or triple bonds (shows all different positions of a bond on an atom)
Electron domain
The number of locations on the central atom where bonding can occur
Parent geometry
The geometry shape when all possible bonding locations are occupied by bonds (linear, trigonal planar, tetrahedral, trigonal bipyramidal, octahedral)
Intermolecular bonding
The attractive and repulsive forces between covalent molecules
What does VSEPR stand for? What does it allow us to do? How?
Valence Shell Electron Pair Repulsion Theory
- allows us to predict 3-D shape of a mole from from its Lewis structure
- Based on geometry that minimizes the repulsion of electrons around the central atom
