Module 1: General Chemistry Flashcards

Flashcards testing vocabulary and key foundational concepts across General Chemistry Module 1.

Chemistry

The branch of science that deals with the study of matter; also known as Physical Science, Central Science, and the ABC of Pharmacy.

Antoine Lavoisier

Recognized as the Father of Modern Chemistry; authored the Law of Mass Conservation and created the first true periodic table of 33 elements.

Matter

Anything that has mass (amount of matter making up a material) and volume (amount of space occupied by matter).

Law of Definite Proportion

Also known as Proust's Law or Law of Constant Composition; states that the composition of a pure compound is always the same regardless of its source, with elements combined in constant whole-number mass proportions.

Law of Multiple Proportion

Also known as Dalton's Law; states that atoms of two or more elements may combine in different whole-number ratios to produce more than one compound.

Law of Combining Weights

States that proportions by weight of elements can be expressed in small integral units when a chemical reaction occurs.

Law of Mass Conservation

Formulated by Lavoisier; states that no change is observed in the total mass of the substances involved in a chemical reaction.

Element

A pure substance composed of only 1 kind of atom that cannot be chemically decomposed (e.g., $\text{Li}$, $\text{N}_2$).

Compound

A pure substance composed of 2 or more different elements chemically combined that may be chemically decomposed (e.g., $\text{NaCl}$, $\text{Na}_2\text{CO}_3$).

Homogenous Mixture

A mixture with uniform parts that consists of a single phase (e.g., Solutions, Alloys).

Heterogenous Mixture

A mixture with physically distinct parts consisting of multiple phases (e.g., Colloids, Suspensions).

True Solution

A uniform mixture composed of a solute and a solvent with a particle size of less than $1\,nm$.

Colloid

A mixture with particle sizes between $1\,nm$ and $0.5\,\mu m$ that exhibits the Tyndall Effect, Brownian Motion, Adsorption, and high Zeta Potential.

Suspension

A coarse mixture containing particle sizes greater than $0.5\,\mu m$, consisting of finely divided solid materials distributed in liquid.

Centrifugation

A physical separation method for mixtures based on differences in sedimentation rate.

Chromatography

A physical separation method for mixtures based on differences in solvent affinity.

Decantation

A separation method for mixtures based on differences in density or specific gravity.

Distillation

A separation method for mixtures based on differences in boiling points.

Filtration

A mechanical separation method for mixtures based on differences in particle size.

Plasma

Also known as Ionized Gas; the 4th fundamental state of matter and the most abundant state of matter in the universe.

Bose Einstein Condensate

The 5th state of matter formed by a dilute gas cooled to temperatures close to absolute zero ($0\,K$).

Phase Changes and Enthalpy System

The thermodynamic relation of state transitions (Sublimation, Melting, Vaporization, Ionization, Condensation, Freezing, Deposition, Recombination) with respect to increasing system enthalpy.

Endothermic Reaction

A process where heat is absorbed ($\Delta H = (+)$); characterized by cold surrounding temperatures, non-spontaneous nature, and bond-breaking processes.

Exothermic Reaction

A process associated with $\Delta H = (-)$; characterized by hot surrounding temperatures, spontaneous nature, and bond-forming processes.

Intrinsic Property

Also known as Intensive Property; a physical property of matter that is independent of the amount of matter present (e.g., Density, Boiling Point).

Extrinsic Property

Also known as Extensive Property; a physical property of matter that depends on the amount of matter present (e.g., Volume, Length).

J.J. Thompson

Scientist who performed the Cathode Ray Experiment, proposed the Plum-Pudding / Raisin Bread Model, and discovered negatively charged electrons.

Ernest Rutherford

Scientist who performed the Gold Foil Experiment, proposed the Nuclear Model of the atom, and discovered protons.

Isotope Notation Symbol

Standard nuclear symbol format where $X$ is the element symbol, $A$ is the Mass Number (protons + neutrons), and $Z$ is the Atomic Number (protons).

Isotope

Nuclides belonging to the same element that have the exact same atomic number / number of protons, but different mass numbers (e.g., Protium, Deuterium, Tritium).

Isobar

Nuclides that possess the same mass number despite being different chemical elements.

Isotone

Nuclides that possess the exact same number of neutrons in their nucleus.

Isoelectronic

Atoms, ions, or molecules that share the exact same number of electrons.

Node

A locus of points within an atom in which the electron probability density is equal to zero.

Heisenberg's Uncertainty Theory

States that it is physically impossible to determine simultaneously both the exact momentum and position of an electron.

Pauli's Exclusion Principle

States that no two electrons in an atom can have the exact same set of four quantum numbers.

Aufbau's Building-Up Principle

States that electrons occupy subshells of lower energy levels first before filling higher energy subshells.

Hund's Rule

Also known as the Maximum Multiplicity Rule; states that electrons fill degenerate orbitals singly first before pairing up.

Azimuthal Quantum Number (l)

Quantum number representing subshells ($s, p, d, f$) that specifies the angular momentum and shape of an electron orbital.

Bridge Elements

Diagonally related elements located in Periods 2 and 3 of the periodic table that share similar chemical behaviors (e.g., $\text{Li-Mg}$, $\text{Be-Al}$, $\text{B-Si}$).

Dmitri Mendeleev

Known as the Father of the Modern Periodic Table; arranged chemical elements based on increasing atomic mass.

Henri Moseley

Scientist who arranged chemical elements based on their atomic numbers to establish the Modern Periodic Table.

Keesom Force

An intermolecular Van der Waals attraction also called the Orientation Effect; occurs between two polar molecules (Dipole-Dipole).

Debye Force

An intermolecular Van der Waals force also called the Induction Effect; occurs between a polar and a nonpolar molecule (Dipole - Induced Dipole).

London Dispersion Force

An intermolecular force also called the Dispersion Effect; occurs between two nonpolar molecules (Induced Dipole - Induced Dipole) and causes the liquefaction of nonpolar gases.

Reaction Progress Energy Diagram

A kinetic energy coordinate showing the higher activation energy barrier and energy relationships of reactants, activated complex, and products for exothermic and endothermic reactions.

VILEORA

Mnemonic for oxidation: Valence & Oxidation State Increases, Loses Electrons, Reaction is Oxidation, agent is Reducing Agent (typical of Metals).

VDGEROA

Mnemonic for reduction: Valence & Oxidation State Decreases, Gains Electrons, Reaction is Reduction, agent is Oxidizing Agent (typical of Non-Metals).

Galvanic Electrochemical Cell

A spontaneous electrochemical setup converting chemical energy to electrical energy, featuring oxidation at the zinc anode and reduction at the copper cathode.

Le Chatelier's Principle

States that if a system at dynamic equilibrium is subjected to an external stress, the system will shift its position to counteract and relieve that stress.

Henry's Law

States that at constant temperature, the solubility of a gas in a liquid is directly proportional to the partial pressure of that gas above the liquid.

Bronsted-Lowry Theory

Acid-base theory defining acids as proton ($\text{H}^+$) donors and bases as proton acceptors.

Lewis Acid-Base Theory

Acid-base theory defining acids as electron pair acceptors and bases as electron pair donors.

Sorensen Buffer

An isotonic pharmaceutical buffer composed of $\text{NaCl}$ and Sodium Phosphate.

Isolated System

A thermodynamic system that must be adiabatic and permits no exchange of matter or energy with its surroundings.

Gibbs Free Energy Formula

Thermodynamic measure of reaction spontaneity expressed by the relation $\Delta G = \Delta H - T \Delta S$.

Graham's Law

Gas law stating that rates of diffusion and effusion of two gases are inversely proportional to the square roots of their densities ($\frac{R_1}{R_2} = \sqrt{\frac{M_2}{M_1}}$).

Becquerel (Bq)

The SI unit of radioactivity, where $1\,Bq = 2.7 \times 10^{-11}\,Ci$.