Chemical Bonding, Structures, and Properties

Vocabulary practice flashcards covering molecular shapes, types of covalent structures, ionic bonding, metallic bonding, electrical conductivity, and solubility across different chemical structures.

Tetrahedral

A molecular shape characterized by four bonding pairs arranged symmetrically around a central atom, exhibited by methane ($CH_4$).

Trigonal Pyramidal

A molecular geometry featuring three bonds directed downward from a central atom, forming a pyramid shape, as seen in ammonia ($NH_3$).

Angular

A non-linear molecular shape formed when a central atom has two bonding pairs at an angle to each other.

Linear (Molecular Shape)

A molecular geometry in which atoms are arranged along a straight line.

Ammonia ($NH_3$)

A molecule that adopts a trigonal pyramidal molecular shape.

Methane ($CH_4$)

A molecule that adopts a tetrahedral molecular shape.

Covalent Molecular Structure

A smaller covalent structure comprised of discrete molecules held together by weak intermolecular attractions.

Covalent Network Structure

A larger, continuous lattice structure formed by countless atoms joined by strong covalent bonds.

Molecule

A group of atoms held together by strong covalent bonds.

Monatomic (Group 0)

Substances consisting of single, unbonded atoms, typical of Group 0 noble gases.

Intermolecular Forces

Weak forces of attraction that exist between separate molecules, holding them together.

Ionic Bonding

The transfer of electrons between atoms (typically a metal and a non-metal) to produce positive and negative ions.

Ionic Lattice

A regular, repeating three-dimensional arrangement consisting of alternating positive and negative ions held by opposite electrostatic charges.

Sodium Electron Configuration in Ionic Bonding

Sodium ($2,8,1$) loses one electron to chlorine, forming a positive ion.

Chlorine Electron Configuration in Ionic Bonding

Chlorine ($2,8,7$) gains one electron from sodium, forming a negative chloride ion.

Four Covalent Networks

The four main covalent network substances: silicon, silicon dioxide, carbon (such as diamond and graphite), and boron.

Metallic Bonding

The electrostatic attraction between a lattice of positive metal ions and a surrounding sea of delocalised electrons.

Delocalised Electrons

Electrons within a metallic lattice that are not bound to any individual atom and are free to move throughout the structure.

Ductile

The mechanical property of a metal allowing it to be drawn out into long, thin wires.

Malleable

The mechanical property of metals that allows them to be hammered or pressed into different shapes without breaking.

Electrical Conductivity

The ability of a substance to conduct electricity, which requires the presence of mobile charged particles such as delocalised electrons or free ions.

Electrical Conductivity of Metals

Always conduct electricity in both solid and liquid states because electricity is a flow of electrons, and metals contain delocalised electrons.

Electrical Conductivity of Covalent Molecular Substances

Do not conduct electricity under any state because they have no free-moving charged particles.

Electrical Conductivity of Covalent Networks

Do not conduct electricity, with the sole exception of graphite.

Electrical Conductivity of Ionic Lattices

Do not conduct electricity when solid because ions are fixed, but conduct when molten or in aqueous solution because ions become mobile.

Solubility

The property describing the ability of a given substance to dissolve in a solvent.

Solubility of Covalent Networks

Never soluble in aqueous or non-aqueous solvents due to the strength of their continuous network of covalent bonds.

Solubility of Ionic Lattices

Generally dissolve in aqueous solvents such as water.

Solubility of Covalent Molecular Substances

Generally insoluble in aqueous solvents (water) but soluble in non-aqueous solvents.