Year 11 ATAR Chemistry: Bonding

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Bonding

Atoms achieve stability by exchanging or sharing electrons.

Chemical Bonds

Links formed between atoms through electron interactions.

Metallic Bonding

Bonding involving delocalised electrons among metal cations.

Ionic Bonding

Bonding between cations and anions in a lattice.

Covalent Molecular Bonding

Atoms share electrons to form discrete molecules.

Covalent Network Bonding

Atoms connected in a continuous network of bonds.

Metallic Structure

Tightly packed metal cations with free electrons.

Delocalised Electrons

Electrons that move freely between metal cations.

Valence Electrons

Electrons in the outermost shell of an atom.

Cations

Positively charged ions formed by losing electrons.

Anions

Negatively charged ions formed by gaining electrons.

Lewis Structures

Diagrams showing valence electrons and bonding.

Electron Dot Diagrams

Visual representation of valence electrons around atoms.

High Density

Tightly packed cations in metallic structures.

Hardness in Metals

Compact arrangement of metal cations increases strength.

Melting Point

Temperature at which a substance changes from solid to liquid.

Boiling Point

Temperature at which a substance changes from liquid to gas.

Malleability

Ability of metals to be shaped without breaking.

Ductility

Ability of metals to be stretched into wires.

Electrical Conductivity

Ability to conduct electricity through mobile charged particles.

Thermal Conductivity

Ability to conduct heat through kinetic electron movement.

Ionic Compounds

Salts formed by cations and anions in a lattice.

Electrostatic Forces

Attractive forces between oppositely charged ions.

Brittleness in Ionic Compounds

Breakage due to repulsion of like-charged ions.

High Melting Point in Ionic Compounds

Requires energy to overcome strong ionic bonds.

Conductivity in Liquid State

Ionic compounds conduct electricity when melted or dissolved.

Fixed Positions in Solids

Ionic compounds cannot conduct electricity in solid state.

Ionic Crystals

Hard structures due to tightly packed ionic lattices.

Electrostatic Repulsion

Force that causes similar charged ions to repel.

Lewis Structures for Ions

Show original valence shell electrons with charges.

Coefficients in Compounds

Indicate ratios of ions in ionic structures.

Noble Gas Configuration

Stable electron arrangement similar to noble gases.

Metal Alloys

Mixtures of metals to enhance strength.

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 Sharing

Key feature of covalent bonding between atoms.

Atomic Structure

Arrangement of protons, neutrons, and electrons in an atom.

Lattice Pattern

Regular arrangement of ions in ionic compounds.