Comprehensive Chemistry: Chemical Nomenclature, Reactions, and Stoichiometry

Vocabulary practice flashcards covering chemical nomenclature, formulas, acids, salts, reaction types, solubility rules, the law of definite proportions, and mole stoichiometry.

Chemical Formula

A combination of chemical symbols with numerical subscripts used to represent a substance, indicating both the kind and number of elements present in a compound.

Chemical Nomenclature

The systematic naming and writing of chemical formulas for elements, ions, and compounds.

Diatomic Molecule

A molecule composed of two identical atoms; the seven elements that naturally exist as diatomic molecules are $H_2$, $N_2$, $O_2$, $F_2$, $Cl_2$, $Br_2$, and $I_2$.

Binary Compound

A compound composed of two different elements only, named by keeping the first element's full name and modifying the second element's name to end in "-ide".

Valence

The combining capacity of an atom, determined by the column number of the "A" families of elements; in binary compounds, the total valence of each participating element must balance.

Binary Gas

A binary compound containing hydrogen and a non-metallic element that exists in the gaseous state at room temperature, indicated by the state symbol $(g)$.

Binary Acid

An acidic aqueous solution formed by dissolving a binary gas in water, named with the prefix "hydro-", the root of the second element with the suffix "-ic", the word "acid", and the state symbol $(aq)$.

Aqueous ($(aq)$)

A state designation written after a chemical formula indicating that a substance is dissolved in water, derived from the word meaning "made with water".

Peroxide

A class of compounds that contains one more oxygen atom than the normal oxide, named using the prefix "per-" before "oxide" and written without reducing the chemical subscripts.

Hydroxide Ion

A polyatomic ion with the formula $OH^-$, a charge of $-1$, and a valence of $1$, which combines with cations to form corrosive compounds that are the chemical opposites of acids.

Ammonium Ion

A polyatomic cation with the formula $NH_4^+$, a charge of $+1$, and a valence of $1$, which behaves chemically as a single ion and is distinct from the ammonia molecule ($NH_3$).

Oxyacid

An acid containing hydrogen, oxygen, and a non-metal or central element, which exhibits acidic character only when dissolved in water as designated by $(aq)$.

The Seven Common "-ic" Oxyacids

The reference set of oxyacids from which other oxyacids and radicals are derived: chloric acid ($HClO_3(aq)$), bromic acid ($HBrO_3(aq)$), iodic acid ($HIO_3(aq)$), nitric acid ($HNO_3(aq)$), carbonic acid ($H_2CO_3(aq)$), sulphuric acid ($H_2SO_4(aq)$), and phosphoric acid ($H_3PO_4(aq)$).

"Per-…-ic" Oxyacid

An oxyacid formed by adding one oxygen atom to the reference "-ic" acid formula, named by adding the prefix "per-" to the base acid name (e.g., $HClO_4(aq)$ is perchloric acid).

"-ous" Oxyacid

An oxyacid formed by removing one oxygen atom from the reference "-ic" acid formula, named by replacing the suffix "-ic" with "-ous" (e.g., $HClO_2(aq)$ is chlorous acid).

"Hypo-…-ous" Oxyacid

An oxyacid formed by removing two oxygen atoms from the reference "-ic" acid formula, named by adding the prefix "hypo-" and replacing the suffix "-ic" with "-ous" (e.g., $HClO(aq)$ is hypochlorous acid).

Dissociation

The chemical process in which molecules separate into positively charged cations and negatively charged anions when dissolved in water.

Oxyacid Radical

A negatively charged polyatomic anion formed when an oxyacid dissociates in water, with its negative charge and valence matching the number of hydrogen ions released.

Oxyacid Radical Nomenclature Rules

The naming system where the radical of an "-ic" acid changes its suffix to "-ate" (e.g., chlorate, $ClO_3^-$), and the radical of an "-ous" acid changes its suffix to "-ite" (e.g., chlorite, $ClO_2^-$).

Salt

A compound formed when the hydrogen ions of an acid are replaced by metal ions or ammonium ions, named by stating the cation followed by the radical.

Acid Salt

A salt formed when only some of the hydrogen ions in a polyprotic oxyacid are displaced by a metal ion, leaving one or more replaceable hydrogen atoms in the polyatomic anion.

Bicarbonate

The common name for the hydrogen carbonate radical ($HCO_3^-$), which has a valence of $1$ and forms compounds such as sodium bicarbonate ($NaHCO_3$), commonly known as baking soda.

Prefix Method (Covalent Nomenclature)

The method of naming binary covalent compounds consisting of non-metals by prefixing the elements with Greek numerals (mono-, di-, tri-, tetra-, penta-, hexa-) to show atom counts, omitting "mono-" on the first element.

Classical System Suffixes (-ous / -ic)

The traditional naming system for multivalent metal cations where the suffix "-ous" represents the lower oxidation state (e.g., stannous, ferrous, plumbous) and "-ic" represents the higher oxidation state (e.g., stannic, ferric, plumbic).

Double Displacement Reaction

A chemical reaction involving two ionic compounds where the cations exchange places according to the general formula $AB + CD \rightarrow AD + CB$, resulting in the formation of a precipitate, a gas, or water.

Precipitate

An insoluble solid product that forms from the reaction of two aqueous solutions and separates out of the mixture.

Solubility Rules

Guidelines classifying ionic compounds as soluble ($(aq)$) or insoluble ($(s)$), stating that nitrates are completely soluble, halides and sulfates are generally soluble with specific exceptions, and sulfides, carbonates, phosphates, and hydroxides are generally insoluble.

Single Replacement Reaction

A reaction in which an active element displaces another element from a compound; if the free element is less reactive than the bonded element, no reaction occurs ($\text{N.R.}$).

Law of Definite Proportions

Also called the Law of Constant Composition; states that a specific chemical compound always contains the exact same elements in the exact same fixed ratio by mass anywhere in the universe.

Percent Composition by Mass

The percentage of a compound's total mass contributed by each element, calculated using the formula: $(\text{total mass of element in formula} / \text{molar mass of compound}) \times 100\%$.

Mole (mol)

A fundamental counting unit in chemistry representing $6.02 \times 10^{23}$ particles (atoms, molecules, or formula units), functioning similarly to a chemical dozen.

Avogadro's Number

The constant value defining the number of particles in one mole of any substance, written as $6.02 \times 10^{23}$ (or $6.022 \times 10^{23}$).

Molar Mass

The mass in grams of one mole of a substance ($g\,mol^{-1}$), determined by calculating the sum of the atomic masses of all atoms present in the chemical formula.