Bonding

Bonding

Atoms form links to achieve stable electron configurations.

Stable Electron Configuration

Achieved by exchanging or sharing electrons.

Chemical Bonds

Links formed between atoms through electron interactions.

Metallic Bonding

Bonding involving delocalised electrons among metal cations.

Metal Cations

Positively charged metal ions in metallic structures.

Delocalised Electrons

Valence electrons that move freely in metallic bonding.

Electrostatic Attraction

Force holding cations and electrons together in metals.

Lewis Structures

Diagrams showing valence electrons and bonding.

Valence Electrons

Electrons in the outermost shell of an atom.

Metallic Lattice

Structure formed by closely packed metal cations.

Density in Metals

Result of tightly packed spherical metal cations.

Hardness in Metals

Due to strong bonds and compact cation arrangement.

Melting Point

Temperature at which a solid becomes liquid.

Boiling Point

Temperature at which a liquid becomes gas.

Malleability

Ability to be shaped without breaking.

Ductility

Ability to be stretched into wires.

Metal Alloys

Mixtures of metals that enhance strength.

Electrical Conductivity

Ability to conduct electricity through mobile charges.

Thermal Conductivity

Ability to conduct heat through delocalised electrons.

Ionic Bonding

Bonding between cations and anions in ionic compounds.

Cations

Positively charged ions formed by losing electrons.

Anions

Negatively charged ions formed by gaining electrons.

Ionic Lattice

Alternating arrangement of cations and anions.

Electrostatic Forces

Attractive forces between oppositely charged ions.

High Melting Point

Requires energy to overcome ionic bonds in solids.

Brittleness in Ionic Compounds

Caused by repulsion of like-charged ions under pressure.

Electrical Conductivity in Liquids

Ionic compounds conduct electricity when melted or dissolved.

Ionic Crystals

Hard structures formed by tightly packed ions.

Lewis Structures for Ions

Show original valence electrons with square brackets.

Ionic Compounds

Formed by the transfer of electrons between metals and non-metals.

Covalent Molecular Bonding

Sharing of electrons between non-metal atoms.

Covalent Network Bonding

Extensive networks of covalent bonds in solids.

Common Properties of Metals

Dense, hard, high melting/boiling points, conductive.

Common Properties of Ionic Compounds

Hard, brittle, high melting/boiling points, conductive in liquid.

Electron Dot Diagrams

Visual representation of valence electrons in bonding.

Pure Substance Lewis Structure

Identical to the element's Lewis structure.

Coefficient in Compounds

Indicates the ratio of ions in the structure.

Fluid-like Nature of Metallic Bonds

Allows cations to move without breaking the structure.

Kinetic Energy in Metals

Required to break metallic bonds during melting.