Chemistry Fundamentals and Thermochemistry

Comprehensive vocabulary flashcards covering the basics of chemistry, classifications of matter, atomic theory, the periodic table, and thermochemistry based on the lecture transcript.

Chemistry

The branch of science that studies matter, its properties, composition, structure, and the changes it undergoes.

Kimia

The Arabic word meaning alchemy, which is the origin of the word Chemistry.

Organic Chemistry

The study of substances that contain carbon-carbon ($C–C$) bonds, such as plastics and pharmaceuticals.

Inorganic Chemistry

The study of substances that do not contain carbon-carbon bonds, including metals, minerals, and semiconductors.

Physical Chemistry

The study of the behavior and changes of matter, the energy changes involved, and reaction rates and mechanisms.

Analytical Chemistry

The study of the components and composition of substances, such as nutrient analysis in food.

Biochemistry

The branch of chemistry that studies chemical processes in living organisms, such as metabolism and fermentation.

Macroscopic Properties

Properties of matter that can be measured directly, including length, mass, and temperature.

Microscopic Properties

Properties of matter measured indirectly, including atomic mass and molecular properties.

Volume

The amount of space occupied by an object, typically measured in $L$, $mL$, or $cm^3$.

Mass

The amount of matter contained in an object.

Weight

The force of gravity acting on an object.

Density

The mass per unit volume of a substance, calculated as $d = \frac{m}{V}$.

Matter

Anything that occupies space and has mass.

Solid

A state of matter with closely packed particles, a definite shape, and a definite volume.

Liquid

A state of matter with particles farther apart than a solid, having a definite volume but taking the shape of its container.

Gas

A state of matter with particles very far apart, having no definite shape or volume and expanding to fill its container.

Plasma

A hot ionized gas composed of positively charged ions and negatively charged electrons, affected by electric and magnetic fields.

Bose-Einstein Condensate (BEC)

A state of matter formed when atoms are cooled to temperatures very close to absolute zero, causing them to move slowly and behave as one particle.

Pure Substance

Matter with a constant composition and unique properties that cannot be separated by physical means.

Mixture

A combination of two or more substances that do not have a constant composition and can be separated by physical methods.

Homogeneous Mixture (Solution)

A mixture with a uniform composition throughout, consists of a solute and a solvent.

Heterogeneous Mixture

A mixture with a non-uniform composition, including colloids and suspensions.

Colloid

A heterogeneous mixture with particles that do not settle when left standing.

Suspension

A heterogeneous mixture with particles that settle at the bottom over time.

Compounds

Substances made of two or more elements chemically combined that can be decomposed through chemical means.

Acids

Compounds that release hydrogen ions ($H^+$) in water.

Bases

Compounds that release hydroxide ions ($OH^-$) in water.

Salts

Compounds consisting of positively charged cations and negatively charged anions.

Elements

Substances that cannot be broken down into simpler substances by chemical means, classified as metals, metalloids, or non-metals.

Physical Properties

Characteristics that can be observed or measured without changing the composition of the substance.

Chemical Properties

Characteristics only observable when a substance undergoes a change into a new substance.

Intensive Properties

Properties that do not depend on the amount of matter, such as density, color, and boiling point.

Extensive Properties

Properties that depend on the amount of matter, such as mass, volume, and length.

Physical Change

A change that alters only the appearance or form of a substance and is generally reversible.

Chemical Change

A change that produces one or more new substances through a chemical reaction and is usually not reversible.

Decantation

A separation method that allows large solid particles to settle before pouring off the liquid.

Filtration

A separation method that passes a mixture through a porous medium to separate small solid particles from liquids.

Distillation

Separation of liquids by boiling a mixture to create vapor, then cooling it back into liquid form.

Centrifugation

The use of a centrifuge to speed up the settling of solid particles from a liquid.

Solvent Extraction

The separation of substances based on their difference in solubility in a specific solvent.

Atomos

The term proposed by Democritus meaning indivisible, describing tiny particles that make up matter.

Plum Pudding Model

The atomic model proposed by J.J. Thomson where electrons are embedded in a positively charged sphere.

Quantum Mechanical Model

The model introduced by Erwin Schrödinger describing electrons as matter waves and predicting their most likely locations.

Proton

A positively charged particle found inside the nucleus of an atom.

Neutron

A neutral particle found inside the nucleus of an atom.

Electron

A negatively charged particle that surrounds the nucleus of an atom.

Atomic Number (Z)

A value equal to the number of protons in an atom; for neutral atoms, it also equals the number of electrons.

Mass Number (A)

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

Isotopes

Atoms of the same element with the same atomic number but different mass numbers due to different numbers of neutrons.

Cation

A positively charged ion formed when an atom loses electrons.

Anion

A negatively charged ion formed when an atom gains electrons.

Periodic Law

The principle that properties of elements repeat periodically when arranged by increasing atomic number.

Electronegativity

The ability of an atom to attract bonding electrons, which increases across a period and decreases down a group.

Ionization Energy

The energy required to remove an electron from an atom.

Ionic Bond

A chemical bond formed by the electrostatic attraction between positive and negative ions.

Covalent Bond

A chemical bond formed when atoms share electrons.

Mole

The amount of substance containing $6.022 \times 10^{23}$ particles.

Molar Mass

The mass of one mole of a substance expressed in $g(mol)^{-1}$.

Thermochemistry

The study of heat energy involved in chemical reactions and physical changes.

Potential Energy

Energy stored because of an object's position, composition, or condition.

Kinetic Energy

Energy possessed by an object because of its motion.

Law of Conservation of Energy

The principle stating that energy cannot be created or destroyed, only transferred or changed in form.

Heat (Q)

The transfer of thermal energy between two bodies with different temperatures, calculated as $Q = m c \rlap{--} \text{Δ} T$.

Specific Heat Capacity

The quantity of heat required to raise the temperature of one gram of a substance by one degree Celsius.

Sensible Heat

Heat that changes the temperature of a substance without changing its phase.

Latent Heat

Heat absorbed or released during a phase change at a constant temperature.

Thermal Equilibrium

A state where heat lost by one object equals the heat gained by another.

Calorimetry

The science of measuring the total heat change in a system, where total heat change equals zero.