PCQA 111 — Comprehensive Summarized Reviewer (Modules 1–3)

Vocabulary flashcards covering Modules 1, 2, and 3 of PCQA 111 (Pharmaceutical Inorganic Chemistry with Qualitative Analysis), detailing key definitions, historical scientists, properties of matter, mixtures, atomic theories, subatomic constants, and quantum numbers.

Chemistry

The study of the composition, structure, properties, and change of matter, exploring how substances interact, accompanying energy changes, and governing principles.

Organic Chemistry

The study of most carbon-containing compounds and their reactions.

Inorganic Chemistry

The study of substances not classified as organic, mainly compounds that do not contain carbon.

Ancient Chemistry

Chemical practices before 1000 B.C. involving processing natural ores to produce metals for ornaments and weapons, and using embalming fluids.

Greek Philosophers

Among the first to formulate theories about matter behavior, proposing a four-substance view (fire, earth, water, air) by about 400 B.C.

Continuous Theory

Aristotle's view that matter is continuous and can be divided into smaller pieces infinitely without reaching a smallest particle.

Particle/Atomic Theory

The view associated with Democritus and Leucippus that matter is made of tiny, discrete, indivisible particles called atomos; later developed by John Dalton and accepted by modern science.

Atomos

Greek term meaning 'uncuttable,' used for the ultimate particles of matter.

Alchemy

A mystical form of chemistry concerned with aims such as converting common metals into gold; described as a pseudoscience.

Alchemist

A follower of alchemy.

Aristotle

Held that fire, water, air, and earth were building blocks of substances, and advocated the continuous theory of matter.

Archimedes

His work on pulleys, levers, and floating bodies gave rise to concepts of density and specific gravity.

Georgius Agricola / Georg Bauer

Associated with the development of systematic metallurgy, including extraction of metals from ores.

Paracelsus

Swiss alchemist/physician associated with medicinal applications of minerals.

John Dalton

Developed modern atomic theory, viewing atoms as particles composing elements and simple ratios in compounds.

Law of Multiple Proportions

When two elements form a series of compounds, the ratios of masses of the second element that combine with a fixed mass of the first can be reduced to small whole numbers.

Mendeleev and Meyer

By 1869, described different forms of the periodic table after atoms and molecules had become established concepts.

Becquerel

Discovered radioactivity in 1896, opening another area of chemical study.

Matter

Any substance that has mass and occupies space, composed of atoms and molecules containing protons, neutrons, and electrons.

Solid

State in which particles are tightly packed in a fixed, orderly arrangement, possessing definite shape and volume, with particles vibrating in place.

Liquid

State in which particles are close together but not fixed, allowing them to flow past one another; possesses definite volume but takes the shape of its container.

Gas

State whose particles are widely spaced and move independently, expanding to fill the shape and volume of its container.

Plasma

A gas-like state consisting of charged, ionized particles found in stars and artificial devices.

Ionized

Having particles that have been stripped of electrons.

General Properties of Solids

Rigidity, hardness, mechanical strength, definite size, shape, volume, vapor pressure, and sublimation.

General Properties of Liquids

Definite volume, indefinite shape, constant boiling points, viscosity, evaporation, vaporization, volatility, surface tension, and density.

General Properties of Gases

No definite shape, size, or volume; expand when heated; exert pressure; high compressibility; diffusibility.

Compressibility

Ability of a gas to be compressed due to widely separated particles.

Diffusibility

Ability of particles to spread through available space.

Viscosity

A listed property of liquids describing resistance to flow.

Volatility

A listed property of liquids related to ease of vaporization.

Surface Tension

A listed property of liquids arising at the liquid surface.

Extrinsic Property

A property that depends on the amount of matter; also called an extensive property.

Intrinsic Property

A property that is constant/characteristic of a substance and does not depend on amount; also called an intensive property.

Intensive Property

Property that does not depend on the amount of substance; examples include boiling point, freezing point, melting point, viscosity, and refractive index.

Extensive Property

Property that depends on the amount of substance; examples include height, weight, temperature, size, shape, and volume.

Mass

The amount of substance; remains the same when an object is moved to the moon.

Weight

The downward pull of an object toward Earth's center depending on gravity; on the moon it is about 1/6 of its Earth value.

Pure Substance

Matter possessing definite, fixed, unvarying composition with a unique set of properties, made of only one kind of matter.

Element

The simplest form of a substance that cannot be decomposed by chemical means; the building blocks of matter.

Metal

Element characterized by brilliant luster, ductility, malleability, and good heat/electricity conductivity.

Nonmetal

Element with characteristics generally opposite those of metals.

Metalloid

Element possessing characteristics of both metals and nonmetals.

Compound

A substance whose molecules are made of two or more kinds of atoms combined in definite proportions.

Ionic Compound

A compound classified under compounds that involves ionic bonding.

Covalent Compound

A compound classified under compounds involving covalent bonding.

Metallic Compound

A compound classified under compounds involving metallic bonding.

Organic Compound

A compound category listed under compounds.

Inorganic Compound

A compound category listed by the module, further including acids, bases, salts, and oxides.

Mixture

Matter composed of two or more substances.

Homogeneous Mixture

A mixture classified as uniform throughout.

Heterogeneous Mixture

A mixture classified as nonuniform.

Compound vs Mixture

Compounds have definite composition by weight and are chemically combined; mixtures may have components in varying proportions, retain component identities, and may be separated mechanically.

Filtration

A separation method using a filtration setup such as filter paper and funnel; useful when particle sizes differ significantly (e.g., sand and water).

Distillation

A separation method that can be used for mixed liquids with different boiling points.

Centrifugation

A separation method relying on density differences; constituents are separated by differences in their effective weights during spinning.

Sedimentation

Separation in which particles of different densities settle within a liquid.

Physical Change

A change in physical properties without changing chemical composition; no new substance is produced, although state or density may change.

Chemical Change

A change in chemical composition/constitution in which the original identity and properties are altered and at least one substance forms a new substance.

Atom

The extremely small particle described in atomic theory as composing elements.

Democritus and Leucippus

Greek philosophers who proposed the atom as an indivisible particle; Democritus coined atomos.

J.J. Thomson

Discovered the electron through cathode-ray experiments and proposed the plum-pudding model.

Ernest Rutherford

Discovered the atomic nucleus through the gold-foil experiment and identified the proton as a positively charged nuclear particle.

Erwin Schrödinger

Developed quantum mechanics and a wave equation describing electron behavior, leading to the electron-cloud model.

James Chadwick

Discovered the neutron in 1932.

Dalton's Atomic Theory

States that elements consist of atoms; atoms of a given element are identical; compounds contain atoms of more than one element in simple ratios; chemical reactions separate, combine, or rearrange atoms.

Modern Atomic Theory

States that atoms may be disintegrated in nuclear reactions; not all atoms of an element are alike; atoms can differ in mass; different elements have different properties.

Electron

A subatomic particle with negative charge, having mass $9.109 \times 10^{-31}\,\text{kg}$ and charge $-1.602 \times 10^{-19}\,\text{C}$.

Proton

A positively charged nuclear particle, having mass $1.673 \times 10^{-27}\,\text{kg}$ and charge $+1.602 \times 10^{-19}\,\text{C}$.

Neutron

A neutral nuclear particle with no charge, having mass $1.675 \times 10^{-27}\,\text{kg}$.

Atomic Number (Z)

Number of protons in the nucleus; for a neutral atom it also equals the number of electrons and identifies the element.

Mass Number (A)

Total number of protons and neutrons in the nucleus.

Nuclear Notation

Notation using A for mass number, Z for atomic number, and N for neutrons.

Neutron Calculation Formula

Calculated from mass number minus atomic number: $N = A - Z$.

Isotopes

Atoms of the same element with the same atomic number but different mass numbers; they have the same protons/electrons but different neutrons.

Quantum Numbers

Numbers used to describe an electron's trajectory/movement and the size, shape, and orientation of orbitals; described as an electron's 'address.'

Principal Quantum Number (n)

Describes orbital size, electron energy level, shell, and average electron-nucleus distance. Possible values are $1, 2, 3, \dots$; $n$ cannot be $0$.

Azimuthal/Angular Momentum Quantum Number (l)

Describes orbital shape, subshell, and orbital angular momentum. For a given $n$, $l = 0$ through $n - 1$.

Magnetic Quantum Number (ml)

Describes orbital orientation in space. Values run from $-l$ through $0$ to $+l$.

Spin Quantum Number (ms)

Gives electron spin direction; values are $+1/2$ (spin-up) or $-1/2$ (spin-down).

Energy Sublevels

Sublevels $s, p, d, f$, containing $s=1$ orbital, $p=3$ orbitals, $d=5$ orbitals, and $f=7$ orbitals.

Orbital

A region represented in the quantum model where electrons are described; each orbital can contain two electrons.

Electron Distribution/Configuration

Representation of how electrons are distributed among orbital shells and subshells, including ground-state atoms and ions.

Aufbau Principle

Rule stating that each electron occupies the lowest-energy orbital available.

Periodic Table

Organized array of chemical elements in increasing atomic number; elements in the same group/column have similar properties due to periodic law.

Periodic Law

Recurring pattern in properties when elements are arranged by increasing atomic number.

Average Atomic Mass

The mass value listed for an element, including contributions from its protons, neutrons, and electrons as described by the module.

Metals

This are lustrous, malleable, and good conductors

Non metals

Do not share metal properties

Metalloids

Share some but not all metal properties

(Upper) 31 (Lower) 15 P

EXAMPLE:

Atomic number 15 → 15 protons; mass number 31 →

16 neutrons; neutral atom → 15 electrons. Electron configuration: 1s?

2s2 2p' 3523p3.

Chemical Bond

A force of attraction between a positive ion and a negative ion or between molecules. Atoms bond to achieve more stable electron configurations, often resembling a nearby noble gas.

Octet Rule

Principle stating that atoms tend to form bonds so they achieve a stable configuration with eight electrons in the outermost shell; hydrogen is an important exception.

Octet Exceptions

Species with an odd number of electrons, fewer than an octet, or more than eight valence electrons (expanded octet).

Interatomic Bonding

Forces that hold atoms together within a molecule or compound.

Ionic Bond

Electrostatic force holding ions together in an ionic compound; formed by electron transfer from an atom of low ionization to a more electronegative element.

Cation

A positively charged ion.

Anion

A negatively charged ion.

Covalent Bond

A bond in which two electrons are shared between atoms; only valence electrons are involved.

Interatomic Bonding

Forces that hold atoms together within a molecule or compound.