Chemical Bonding and Properties of Compounds

Chemical Bonds

Durable electrostatic attractions between atoms.

Second Law of Thermodynamics

Natural systems tend toward minimum energy states.

Octet Rule

Atoms maximize stability by achieving 8 valence electrons.

Valence Electrons

Electrons in the outermost shell of an atom.

Types of Chemical Bonds

Includes covalent, ionic, and metallic bonds.

Covalent Bond

Bond formed by sharing electrons between atoms.

Ionic Bond

Bond between metal and nonmetal via electron transfer.

Metallic Bond

Bond between metal atoms with delocalized electrons.

Polarity

Tendency to form regions of opposite charge.

Polar Covalent Bond

Unequal sharing of electrons between different elements.

Electronegativity

Tendency of an atom to attract electrons.

Diatomic Elements

Elements that exist as pairs: H, N, O, F, Cl, Br, I.

Lewis Structures

2D diagrams showing bonds between atoms.

Double Bond

Covalent bond with 2 shared electron pairs.

Triple Bond

Covalent bond with 3 shared electron pairs.

Formula Unit

Ratio of cations to anions for neutrality.

Crystal Lattice

Orderly arrangement of ions in ionic compounds.

Polyatomic Ion

Covalently bonded group of atoms with a charge.

Electron-Sea Model

Metals have cations surrounded by mobile electrons.

Intermolecular Forces

Forces attracting molecules together in compounds.

Network Covalent Substances

Atoms covalently bonded in a continuous 3D network.

Ionic Compounds

Dense, brittle solids with strong electrostatic forces.

Alloys

Mixtures of metals with one or more elements.

Properties of Metals

Malleability, ductility, luster, and conductivity due to delocalized electrons.

Linus Pauling

Conducted research into the nature of the chemical bond