General & Quantitative Chemistry I: Foundational Concepts, Measurements, and Atomic Theory

Comprehensive vocabulary flashcards covering matter, physical states, phase diagrams, SI units, significant figures, atomic theory, periodic trends, moles, formulas, and ionic nomenclature.

Dimensional Analysis

A mathematical method used in chemical calculations that keeps track of units and offers a gut check on calculated results.

Conversion Factors

Quotients whose numerator and denominator express the identical quantity in different units, used sequentially to cancel units.

Dalton's Atomic Theory

A theoretical framework stating that matter is composed of atoms; elements are made of atoms; only atoms of the same element are identical; atoms are neither created nor destroyed in chemical reactions; and compounds form in fixed atom ratios.

Law of Multiple Proportions

A chemical law stating that when two elements combine to form more than one compound, the masses of one element combining with a fixed mass of the other are in ratios of small, whole numbers.

Molar Mass

The mass in grams of one mole of a substance, expressed in units of $\text{g/mol}$.

Avogadro's Number

A fundamental constant ($6.02 \times 10^{23}$) serving as a conversion factor between the amount of substance in moles and the number of particles, atoms, or molecules.

Empirical Formula

A chemical formula expressing the simplest whole-number ratio of the elements present in a compound.

Molecular Formula

A chemical formula that specifies the actual number and type of each atom contained within a discrete molecule.

Combustion Analysis

An experimental technique used to determine empirical formulas of hydrocarbons by combusting the sample with $\text{O}_2$ and quantitatively trapping the resulting $\text{H}_2\text{O}$ and $\text{CO}_2$ in separate absorbers.

Chemistry

The branch of science dealing with matter, the transformations matter undergoes, and the role of energy involved in these transformations.

Matter

Any physical substance that possesses mass ($m$) and occupies volume ($V$).

Phase

A sample of matter having uniform physical and chemical properties throughout, defined by its physical state and chemical composition.

Plasma

The fourth physical state of matter, consisting of a gas that has been exposed to extremely high energies.

Phase Diagram

A graphical representation that illustrates the boundaries between physical states of a substance across varying environmental pressures and temperatures.

Triple Point

The unique condition of temperature and pressure at which the solid, liquid, and gaseous phases of a substance coexist in equilibrium (for water, $0.01\,^\circ\text{C}$ and $0.006\,\text{atm}$).

Critical Point

The critical temperature and critical pressure conditions above which distinct liquid and gas phases do not exist (for water, $374\,^\circ\text{C}$ and $218\,\text{atm}$).

Groups

Vertical columns in the periodic table containing elements with similar chemical and physical properties.

Periods

Horizontal rows across the periodic table consisting of elements with similar energies and atomic masses.

Structural Formula

A chemical representation indicating how atoms are bonded to each other within a molecule, utilizing element symbols and connecting lines for bonds.

Perspective Representation

A molecular drawing technique utilizing solid wedges and dashed lines to display bonds projecting out of or receding behind the two-dimensional plane.

Ball-and-Stick Model

A three-dimensional representation of a molecule where spheres depict atomic nuclei/atoms and connecting rods illustrate chemical bonds.

Space-Filling Model

A three-dimensional scale model of a molecule displaying atoms as truncated spheres proportional to their actual relative van der Waals sizes.

Cation

A positively charged ion formed when an atom or molecule loses electrons ($\#e^- < \#p^+$).

Anion

A negatively charged ion formed when an atom or molecule gains electrons ($\#e^- > \#p^+$).

Polyatomic Ion

An electrically charged chemical species composed of two or more covalently bonded atoms.

Ionic Compound

A chemical compound composed of cations and anions held together by electrostatic attraction (ionic bonds), resulting in an electrically neutral formula.

Oxyanions

Polyatomic anions containing oxygen, named systematically using suffixes like "-ate" and "-ite" and prefixes like "per-" and "hypo-" to designate the relative number of oxygen atoms.

Absolute Zero

The lowest possible theoretical temperature ($T = 0\,\text{K}$) at which all thermal and atomic motion ceases.

Density

The intensive property of matter defined as mass per unit volume ($\rho = \frac{m}{V}$).

Joule

The derived SI unit of energy, defined as $1\,\text{J} = 1\,\text{kg}\cdot\text{m}^2/\text{s}^2$.

Exact Numbers

Numbers with no measurement uncertainty, obtained by accurate counting or precise definitions, possessing an infinite number of significant figures.

Inexact Numbers

Quantities obtained through measurement that possess an inherent degree of uncertainty determined by the measuring apparatus.

Precision

The closeness of agreement among repeated measurements of the same quantity under identical conditions, frequently quantified as a standard deviation.

Accuracy

The degree of closeness of an individual measured value to the true, standard, or accepted value.

Significant Figures

All digits in a measured value that are known with certainty plus one final estimated or uncertain digit.