Bonding and Structure - Vocabulary Flashcards

A set of vocabulary-style flashcards covering key terms from the Bonding and Structure notes, including ionic, covalent, metallic bonding, structures, and properties.

Bonding

The force of attraction that holds atoms together in molecules or crystals to form compounds.

Ionic/electrovalent bonding

Bond formed by transfer of electrons from a metal to a non-metal, creating oppositely charged ions that attract.

Cation

A positively charged ion formed when an atom loses electrons.

Anion

A negatively charged ion formed when an atom gains electrons.

Valency

The combining capacity of an atom; the number of electrons lost or gained to achieve a stable configuration.

Sodium chloride (NaCl)

An ionic compound formed from Na+ and Cl− ions; example of ionic bonding.

Covalent bonding

Bond formed by sharing of electrons between non-metal atoms, leading to covalent compounds.

Dative/Coordinate bonding

A covalent bond in which both electrons in the shared pair come from one atom.

Lone pair

A pair of electrons not involved in bonding (non-bonded pair) on an atom.

Single covalent bond

A bond formed when one pair of electrons is shared between two atoms.

Double covalent bond

A bond formed when two pairs of electrons are shared between two atoms.

Delocalized electrons

Electrons that are not confined to a single bond or atom and can move freely within a structure.

Metallic bonding

Bonding in metals due to attraction between metal ions and a ‘sea’ of delocalized electrons.

Coordination number

The number of ions surrounding a given ion in an ionic lattice.

Giant ionic structure

A large three-dimensional lattice of ions held together by strong electrostatic forces.

Simple molecular structure

Structure where molecules are held together by weak intermolecular forces and exist as discrete molecules.

Giant molecular structure

A giant covalent network where atoms are linked by covalent bonds in a 3D lattice.

Diamond

A giant covalent network of carbon with each carbon tetrahedrally bonded to four others; very hard and an insulator.

Graphite

Carbon in layered hexagonal sheets held by van der Waals forces; conducts electricity due to delocalized electrons.

Van der Waals forces

Weak intermolecular forces that hold simple molecular substances together.

Malleable

Able to be hammered or rolled into shapes without breaking, typical of metals.

Ductile

Able to be drawn into wires, typical of metals.

Electronegativity

Tendency of an atom to attract bonding electrons toward itself.

Electropositivity

Tendency of an atom to push bonding electrons away from itself.

Polar molecule

A molecule with uneven charge distribution due to differences in electronegativity.

Polar solvent

A solvent with polar molecules (e.g., water) that can dissolve ionic compounds.

Ionic compound

A compound composed of ions held together by ionic bonds; typically solids with high mp and solubility in water.

Covalent compound

A compound formed by covalent (shared-electron) bonds between non-metals; may be gases, liquids, or solids.

Bonding

The chemical combination of atoms or elements to form compounds.

Chemical Bond

The force of attraction holding atoms or elements together in a molecule/crystal.

Ionic/Electrovalent Bonding

Transfer of electrons from a metal atom to a non-metal atom; occurs between metals and non-metals.

Covalent Bonding

Sharing of electrons between two or more non-metal atoms/elements; bonding electrons are contributed by the participating atoms.

Dative/Co-ordinate Bonding

Sharing of bonding electrons donated by one atom/molecule involved.

Metallic Bonding

Attraction between metal ions and the valence electrons within the metal lattice.

Cation

Atom loses electrons to form a positively charged ion.

Anion

Atom gains electrons to form a negatively charged ion.

Electrovalent/Ionic Bond

Electrostatic force of attraction between oppositely charged ions.

Noble Gas Electronic Configuration

Achieved when metals lose electrons and non-metals gain electrons.

Single Covalent Bond

Bond formed when one pair of electrons is shared (each atom contributes one electron).

Lone Pair (Non-Bonding Pair)

Pair of valence electrons not involved in bonding.

Double Covalent Bond

Bond formed when two pairs of electrons are shared between two bonded atoms.

Triple Covalent Bond

Bond formed when three pairs of electrons are shared between two bonded atoms.

Dative/Coordinate Bond

Covalent bond where both electrons in the bond come from the same atom.

Donor Atom

Atom that provides a lone pair in dative bonding.

Acceptor Atom

Atom that accepts a lone pair in dative bonding.

Delocalized Electrons

Electrons released into a general pool within a metal lattice.

Giant Ionic Structure

Three-dimensional crystal lattice of alternating cations and anions.

Coordination Number

Number of surrounding ions around a central ion in a lattice.

Electronegativity

Tendency of an atom to attract bonding electrons toward itself.

Electropositivity

Tendency of an atom to push bonding electrons away from itself.

Simple Molecular Structure

Discrete molecules held together by relatively weak intermolecular forces.

Van der Waals Forces

Weak intermolecular forces between molecules.

Giant Atomic/Molecular Structures

Structures consisting of atoms or molecules linked by covalent bonds in a three-dimensional network.

Giant Metallic Structure

Giant lattice of positive metal ions surrounded by a sea of delocalized electrons.

Ionic Bonding Characteristics

Bonding involves electron transfer and results in an electrostatic lattice that conducts electricity only when ions are mobile.

Covalent Bonding Characteristics

Bonding involves sharing electrons; the number of shared electron pairs determines bond type.