Covalent Bonding and Nomenclature Flashcards

Vocabulary flashcards covering key definitions, bond properties, nomenclature rules, and physical properties of covalent and ionic compounds.

Chemical Bonding

The process by which two or more elements work together in order to achieve an actet (full valence energy level) or duet.

Ionic Bonds

Bonds formed between a metal and a nonmetal from opposite sides of the periodic table involving the transfer of electrons.

Covalent Bonds

Bonds formed between two nonmetals from the same side of the periodic table involving the sharing of electrons.

Chemical Formulas

A combination of chemical symbols that show how many of each element is present in the compound.

Molecule

A single unit of a covalent compound, defined as two or more atoms bonded together with covalent bonds.

Bonding Electrons

The valence electrons that are shared between atoms in a covalent bond.

Single Bond

A covalent bond where two atoms share 1 pair (2 total) of electrons, representing the weakest and longest covalent bond type.

Double Bond

A covalent bond where two atoms share 2 pairs (4 total) of electrons.

Triple Bond

A covalent bond where two atoms share 3 pairs (6 total) of electrons, representing the strongest and shortest covalent bond type.

Bond Length (Physical Definition)

The physical distance between the two nuclei that are covalently bonded.

Bond Length (Potential Energy Definition)

The distance between two covalently bonded atoms where the system's potential energy reaches its lowest possible point.

Diatomics

Certain reactive elements ($H_2$, $N_2$, $O_2$, $F_2$, $Cl_2$, $Br_2$, $I_2$) that bond to another identical atom when not bonded to something else.

Covalent Prefixes

Numerical prefixes used to show atom counts in covalent compounds: 1 = Mono, 2 = Di, 3 = Tri, 4 = Tetra, 5 = Penta, 6 = Hexa, 7 = Hepta, 8 = Octa, 9 = Nona.

Mono Exception Rule

The naming rule stating that the prefix 'Mono' is never used on the first element in a covalent compound.

Irregular Covalent Suffixes

Specific second element naming changes where oxygen becomes oxide, nitrogen becomes nitride, and hydrogen becomes hydride.

Covalent Compound Electrical Conductivity

Covalently bonded compounds do not conduct electricity because they have no free moving charged particles.

Covalent Compound Melting and Boiling Points

Covalent compounds have lower melting and boiling points than ionic compounds due to weaker attraction between nuclei compared to strong ionic positive/negative attraction.

Covalent Compound Appearance

Covalent compounds often do not appear crystalline, in contrast to ionic compounds where crystalline appearance is a defining characteristic.