Chemical Nomenclature, Bonding Models, and Quantitative Analysis Flashcards

Vocabulary flashcards reviewing essential chemical nomenclature rules, bonding models, stoichiometry terms, and Lewis structure principles from the lecture notes.

Binary Ionic Compound

An ionic compound consisting of a metal cation named first by its element name, followed by a nonmetal anion named with its root plus the suffix "-ide".

Lattice Energy

The amount of energy required to convert a mole of an ionic solid to its constituent ions in the gas phase (for example, $788\,\text{kJ}$ for $\text{NaCl}$).

Binary Covalent Compound

A compound formed by two nonmetals where the first element retains its full name, the second is named as an anion, and Greek prefixes denote the number of atoms present.

Molecule

A neutral combination of at least two atoms in a specific arrangement held together by chemical bonds.

Law of Definite Proportions

A law formulated by Proust in 1799 stating that all samples of a given compound, regardless of origin or preparation, contain the same proportions of their constituent elements by mass.

Law of Multiple Proportions

A law formulated by Dalton in 1804 stating that when two elements (A and B) form two different compounds, the masses of element B that combine with $1\,\text{g}$ of element A can be expressed as a ratio of small whole numbers.

Oxyacid

An acid containing hydrogen, oxygen, and another element, where an anion ending in "-ate" forms an acid ending in "-ic", and an anion ending in "-ite" forms an acid ending in "-ous".

Avogadro's Number

The exact number of atoms present in $12\,\text{g}$ of carbon-12 (${}^{12}\text{C}$), equal to $6.022 \times 10^{23}$.

Mole

The amount of substance such that a sample of a natural element with a mass equal to its atomic mass expressed in grams contains $1\,\text{mole}$ ($6.022 \times 10^{23}$) of atoms.

Molar Mass

The mass in grams of $1\,\text{mol}$ of a chemical element or compound.

Percent Composition

The percentage by mass of each constituent element present in a compound.

Combustion Analysis

A quantitative laboratory technique of burning a sample in an $\text{O}_2$-rich environment to convert all carbon to $\text{CO}_2$ and all hydrogen to $\text{H}_2\text{O}$ to determine empirical formulas.

Localized Electron Bonding Model

A bonding model positing that a molecule is composed of atoms bound together by sharing pairs of electrons using the atomic orbitals of the bound atoms.

Lone Pairs

Electron pairs localized on a specific atom that are not shared with another atom.

Bonding Pairs

Electron pairs found in the space between atoms that are shared to form covalent bonds.

Electronegativity

The ability of an atom in a molecule to attract shared electrons to itself, scaled by Linus Pauling from $0.7$ to $4.0$.

Duet Rule

The stability rule applicable to hydrogen ($\text{H}$) stating that it shares electrons to fill its 1s orbital with a total of two electrons.

Octet Rule

The principle that second-row elements starting with carbon tend to form bonds until they are surrounded by eight valence electrons.

Resonance

The condition in which more than one valid Lewis structure can be written for a particular molecule, making the true electronic structure an average of these structures.

Formal Charge

The difference between the number of valence electrons on a free atom and the number of valence electrons assigned to that atom in a molecule.