GENERAL-CHEMISTRY

Volume

Volume

The amount of space occupied by an object.

Kg

Kilogram, the fundamental unit of mass.

N

Newton, the derived unit of weight.

Joules

The derived unit of energy.

Solid

A phase of matter that holds its shape and volume.

Liquid

A phase of matter that takes the shape of its container but has a fixed volume.

Gas

A phase of matter that takes the shape and volume of its container.

Phase Change

The transition of matter from one phase to another.

Fusion

Synonym for melting.

Thawing

Synonym for melting.

Recombination

Synonym for melting.

Condensation

The phase change from gas to liquid.

Rain

An example of condensation.

Sublimation

The phase change from solid to gas.

Deposition

The phase change from gas to solid.

Intermolecular Forces of Attraction (IFA)

Forces that hold molecules together in a substance.

Entropy

The measure of randomness or disorder in a system.

Mesophases

Intermediate phases between solid and liquid.

Liquid Crystals

A type of mesophase with properties of both liquids and solids.

Supercritical Fluids

A state of matter with properties of both liquids and gases.

Phase Equilibrium

The state where two phases coexist in equilibrium.

Purity

The degree to which a substance is free from impurities.

Pure Substances

Substances that are made up of only one type of atom or molecule.

Mixtures

Substances made up of two or more different types of atoms or molecules.

Compounds

Substances made up of two or more different elements chemically bonded together.

Molecules

Two or more atoms chemically bonded together.

Atoms

The smallest amount of an element.

Separatory Techniques

Methods used to separate different components of a mixture.

Filtration

Separation based on size difference.

Evaporation

Separation based on vapor pressure difference.

Distillation

Separation based on vapor pressure difference.

Sublimation

Separation based on vapor pressure difference.

Crystallization

Separation based on solubility difference.

Thermodynamic Properties

Properties of matter related to energy and temperature.

Intensive/Intrinsic Properties

Properties that are independent of mass.

Extensive/Extrinsic Properties

Properties that are dependent on mass.

Physical Properties

Properties that can be observed or measured without changing the substance's identity.

Additive Properties

Properties that can be obtained by summing the individual parts.

Constitutive Properties

Properties that depend on the type and arrangement of bonds in a substance.

Fundamental Chemistry Laws

Laws that describe the behavior of matter and chemical reactions.

Conservation of Mass

The total mass of all products of a chemical reaction is equal to the total mass of all reactants.

Law of Definite/Constant Proportions

A compound always contains the same elements in the same proportion by mass.

Law of Multiple Proportions

When two elements combine to form different compounds, the ratio of their masses is a simple whole number ratio.

Law of Reciprocal Proportion

The masses of two elements that combine with a fixed mass of a third element are in a simple whole number ratio.

Gas Laws

Laws that describe the behavior of gases.

Gay-Lussac's Law

The pressure of a gas is directly proportional to its temperature, at constant volume.

Charles' Law

The volume of a gas is directly proportional to its temperature, at constant pressure.

Avogadro's Law

Equal volumes of gases at the same temperature and pressure contain an equal number of molecules.

Ideal Gas Law

The relationship between the pressure, volume, temperature, and number of moles of a gas.

Balancing Chemical Reactions

Adjusting the coefficients in a chemical equation to ensure that the number of atoms on both sides is equal.

Thermodynamics

The study of energy and its transformations.

Law of Multiple Proportions

When chemical elements combine, they do so in a ratio of small whole numbers.

Law of Reciprocal Proportions

Elements combine in the ratio of their combining weights or chemical equivalents, or in some simple multiple or sub-multiple of that ratio.

Ideal Gas Law

BGCA = Pressure, Temperature, Volume, Moles, Gas Constant.

Dalton's Law of Partial Pressures

The total pressure in a mixture is equal to the sum of the partial pressures of each gas.

Raoult's Law

The vapor pressure of a solvent above a solution is equal to the vapor pressure of the pure solvent at the same temperature scaled by the mole fraction of the solvent present.

Concentration

The amount of a substance present in a given volume or mass of a solution.

Diffusion

The gradual mixing of molecules of one gas with the molecules of another gas by virtue of their kinetic properties.

Effusion

The passage of a gas under pressure through a small opening.

Graham's Law

The rate of diffusion of a gas is inversely proportional to the square root of its density.

Molar mass

The mass of one mole of a substance, expressed in grams per mole.

Diffusivity

The diffusion coefficient that represents the ability of a substance to diffuse through a medium.

Concentration gradient

The difference in concentration between two points in a system.

Atomic structure

The arrangement and organization of atoms, including the subatomic particles within an atom.

Democritus

An ancient Greek philosopher who proposed the concept of atoms as indivisible particles.

John Dalton

A scientist who developed the billiard ball model of atoms, suggesting that atoms are indivisible and have different masses.

J.J

A scientist who proposed the plum pudding model of atoms, suggesting that atoms contain negatively charged electrons embedded in a positively charged sphere.

Ernest Rutherford

A scientist who conducted the gold foil experiment and proposed the nuclear model of atoms, suggesting that atoms have a dense, positively charged nucleus surrounded by electrons.

Niels Bohr

A scientist who proposed the planetary model of atoms, suggesting that electrons orbit the nucleus in specific energy levels or orbits.

Erwin Schrodinger

A scientist who developed the quantum model of atoms, which describes electrons as existing in probability clouds called orbitals.

Heisenberg's Uncertainty Principle

A principle that states that it is impossible to simultaneously know the exact position and momentum of a particle.

Proton

A subatomic particle with a positive charge found in the nucleus of an atom.

Electron

A subatomic particle with a negative charge that orbits the nucleus of an atom.

Neutron

A subatomic particle with no charge found in the nucleus of an atom.

Atomic mass units

A unit of mass used to express the mass of atoms and molecules.

Isotope

Atoms of the same element that have different numbers of neutrons.

Mass number

The sum of the number of protons and neutrons in the nucleus of an atom.

Electron configuration

The arrangement of electrons in the energy levels or orbitals of an atom.

s-block

The block of elements in the periodic table that includes the alkali metals and alkaline earth metals.

p-block

The block of elements in the periodic table that includes the nonmetals, metalloids, and some metals.

d-block

The block of elements in the periodic table that includes the transition metals.

f-block

The block of elements in the periodic table that includes the lanthanides and actinides.

Hund's Rule

The rule that states that orbitals are filled up singly before pairing up in electron configurations.

Pauli's Exclusion Principle

The principle that states that no two electrons can have the same set of quantum numbers.

Diamagnetic

A property of materials that have no unpaired electrons and are weakly repelled by a magnetic field.

Paramagnetic

A property of materials that have at least one unpaired electron and are attracted to a magnetic field.

Magnetism

The property of materials that can be attracted or repelled by a magnetic field.

Periodic Table

A table that organizes elements based on their atomic number, electron configuration, and recurring chemical properties.

Jons Jakob Berzelius

A Swedish chemist who discovered several elements and introduced element symbols.

Johann Dobereiner

A German chemist who proposed the Law of Triads, which states that the middle element in a triad has an average atomic mass between the other two elements.

John Alexander Newlands

An English chemist who proposed the Law of Octaves, which states that the properties of elements repeat every eighth element.

Dmitri Mendeleev

A Russian chemist who is considered the father of the modern periodic table. He arranged elements based on their atomic mass and predicted the existence of undiscovered elements.

Bismuth

The heaviest stable atom on the periodic table.

Periodicity

The recurring pattern of properties and trends in the periodic table.

Valency (Ox

The combining capacity of an atom, determined by the number of electrons it can gain, lose, or share in a chemical reaction.

Alkaline Earth Metals

Group 2 elements on the periodic table, which are reactive metals.

Halogens

Group 17 elements on the periodic table, which are highly reactive nonmetals.

Non-metallic property

The property of not conducting electricity and heat.

Metalloids

Elements that have properties of both metals and non-metals.

Ionic size

The size of ions in different groups of the periodic table.