Chemical Bonding Lecture Review

Flashcards covering the definitions, types, and properties of chemical bonding (covalent, ionic, and metallic), including Lewis diagrams and specific alloys.

Chemical bond

A mutual attraction between two atoms resulting from the simultaneous attraction between their nuclei and the outer electrons.

Metallic bonding (General Mixture)

A type of bonding formed by the combination of a metal and a metal.

Covalent bonding (General Mixture)

A type of bonding formed by the combination of a non-metal and a non-metal.

Ionic bonding (General Mixture)

A type of bonding formed by the combination of a metal and a non-metal.

Lewis dot diagram

A structural formula in which valence electrons are represented by dots or crosses; also known as an electron dot formula or a Lewis formula.

Covalent bond

The sharing of electrons between atoms of non-metals to form molecules.

Couper notation

A representation of a covalent bond where the shared electron pair is shown as a line between the atoms.

Double covalent bond

Formed when two half-filled orbitals of two atoms overlap, sharing two electrons each to obtain a noble gas structure.

Triple covalent bond

Formed when three half-filled orbitals of two atoms overlap, resulting in the sharing of three pairs of electrons ($6$ electrons total).

Relative molecular mass ($M_r$)

The sum of the relative atomic mass of the atoms in the molecule; it has no unit.

Ionic bonding

The transfer of one or more electrons from metal atoms to non-metal atoms, resulting in electrostatic forces of attraction between positive and negative ions.

Cations

Positive ions formed when metal atoms give away electrons.

Anions

Negative ions formed when non-metal atoms take up electrons.

Crystal lattice structure

The fixed arrangement of alternate positive and negative ions found in ionic compounds.

Metallic bonding

The electrostatic attraction between positive atomic residue and the sea of delocalized valence electrons surrounding them.

Delocalized electrons

Valence electrons that are free to move in a metal's crystal lattice due to low ionization energy.

Positive atomic residue

The name given to atoms that lose electrons in metallic bonding; also called positive ions.

Malleable

The property of a substance to be extended or shaped by hammering or rollers without breaking.

Ductile

The property of a substance to be stretched, pulled, or drawn into thin wire without breaking.

Metallic lustre

The shine of a metal's surface caused by free-moving electrons reflecting light.

Alloys

Harder versions of pure metals created by mixing a metal with another substance.

Steel

An alloy mixture of iron ($99,8 \text{\%}$) and carbon ($0,2 \text{\%}$) used in big buildings and bridges.

Stainless steel

A strong, rust-resistant alloy mixture of iron ($74 \text{\%}$), chromium ($18 \text{\%}$), and nickel ($8 \text{\%}$).

Bronze

A hard alloy mixture of copper ($90 \text{\%}$) and tin ($10 \text{\%}$) used in manufacturing large ships and propellers.