Untitled Flashcards Set

Metallic Bonding

The electrostatic attraction between positively charged metal ions and a sea of delocalized electrons.

Properties of Metals

Good conductors of electricity, good conductors of heat, malleable and ductile, high melting and boiling points, high densities.

Recycling of Metals

The process of reusing metals to reduce environmental impact and conserve resources.

Ionic Bonding

Occurs between metals (cations) and non-metals (anions), involving the transfer of electrons.

Lattice Structure of Ionic Solids

A repeating 3D lattice of alternating positive and negative ions held together by strong ionic bonds.

Properties of Ionic Compounds

High melting and boiling points, hard but brittle, conducts electricity in molten or aqueous states.

Covalent Bonding

A type of chemical bonding that involves the sharing of electron pairs between atoms.

Types of Covalent Substances

Discrete molecules (small) like H₂O; covalent lattices like diamond and graphite.

Electronegativity

The ability of an atom to attract electrons.

Polar Molecules

Molecules that have an unequal sharing of electrons, resulting in regions of partial positive and negative charge.

Hydrogen Bonding

A strong intermolecular force occurring between molecules where hydrogen is bonded to N, O, or F.

Diamond

A form of carbon where each carbon atom is tetrahedrally bonded to four other carbon atoms, resulting in a very hard structure.

Graphite

A form of carbon composed of layers of carbon atoms bonded in hexagons, allowing the layers to slide over each other.

Small Molecule Properties

Low melting and boiling points and poor electrical conductivity.

Large Molecule Properties

Higher melting and boiling points than small molecules due to stronger intermolecular forces.

Common Polyatomic Ions

Includes ammonium (NH₄⁺), carbonate (CO₃²⁻), hydroxide (OH⁻), nitrate (NO₃⁻), and sulfate (SO₄²⁻).

SNAPE Rule

Sodium (Na⁺), Nitrate (NO₃⁻), Ammonium (NH₄⁺), Potassium (K⁺), and Ethanoate (CH₃COO⁻) are always soluble.