Inorganic Chemistry Lecture and Lab - Prelims

Comprehensive vocabulary flashcards covering basic chemistry concepts, states of matter, chemical laws, reactions, atomic history, and the periodic table based on the Inorganic Chemistry lecture notes.

Chemistry

A branch of science that studies the properties of matter and the changes it undergoes.

Scientific Method

A systematic approach to research consisting of observation, question, research, and testing.

SMART

An acronym for crafting questions that are Specific, Measurable, Attainable, Relevant, and Time-bound.

Qualitative

General observations about a system.

Quantitative

Numbers obtained by various measurements of the system.

Antoine Van Lavoisier

The French chemist known as the Father of chemistry who proposed the law of conservation of mass and wrote "Elements of chemistry" in $1789$.

Inorganic chemistry

A branch of chemistry that studies elements of life but does not deal with Carbon and Hydrogen.

Organic chemistry

A branch of chemistry that deals with Carbon ($C$) and Hydrogen ($H$) and is used in the body.

Matter

Anything that occupies space and has mass.

Substances

Matter that has a definite composition.

Homogeneous mixture

A mixture that is the same throughout the solution, such as juice and water.

Heterogeneous mixture

A mixture where the composition is not uniform, such as water and oil.

Compound

A substance composed of two or more elements.

Entropy

The degree of disorderliness in a system; it is high in gases and low in solids.

Plasma

The most abundant state of matter, described as an ionized gas.

Melting

The phase change from a solid to a liquid.

Evaporation

The phase change from a liquid to a gas.

Condensation

The phase change from a gas to a liquid.

Freezing

The phase change from a liquid to a solid.

Deposition

The phase change from a gas to a solid.

Sublimation

The phase change from a solid to a gas.

Recombination

The phase change from plasma to gas.

Ionization

The phase change from gas to plasma.

Endothermic

A process that absorbs heat.

Exothermic

A process that releases heat.

Filtration

A method of separation that uses filter paper.

Decantation

A method of separation based on the difference of specific gravity and density.

Distillation

A method of separation involving a series of evaporation and condensation.

Intensive properties

Properties that are independent of the amount of substance, such as density, specific gravity, boiling point, and melting point.

Extensive properties

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

Fusion

A nuclear change involving the combination of nuclei.

Fission

A nuclear change where a nucleus splits up into two.

Law of Mass Action

States that the rate of reaction is proportional to the product of the concentration of the reactants to the power of its coefficient in a balanced equation.

Law of Conservation of Mass

States that during a chemical reaction, matter is neither created nor destroyed.

Combination Reaction

Also known as composition synthesis; a reaction where 2 substances or elements combine, e.g., $A + B \rightarrow AB$.

Precipitation Reaction

A reaction occurring when two soluble ionic compounds in aqueous solutions swap partners, forming an insoluble solid called a precipitate.

Neutralization Reaction

A reaction between a strong acid and a strong base that yields salt and water.

Combustion

A chemical reaction involving burning, such as $C_8H_{18} + O_2 \rightarrow CO_2 + H_2O$.

Carbon Monoxide Poisoning

A condition occurring when $CO$ replaces oxygen in red blood cells, often characterized by cherry red skin.

Law of Definite Proportion

States that a chemical compound always contains exactly the same proportion of elements by mass.

Atom

The building block of matter and the basic unit of life.

Molecule

A neutral group of 2 or more atoms held together by chemical bonds.

Ion

Charged particles.

Billiard Ball Model

An atomic model proposed by John Dalton describing atoms as solid, indestructible spheres.

Raisin Bread Model

Also known as the plum pudding model, proposed by J.J. Thomson, describing negatively charged electrons embedded in a positive cloud.

Nuclear Model

Proposed by Ernest Rutherford, identifying a nucleus containing protons and neutrons with electrons orbiting around it.

Planetary Model

An atomic model supported by James Chadwick.

Quantum Mechanical Model

A model by Erwin Schrodinger that treats electrons as matter waves and defines regions of probability called orbitals.

Heisenberg Uncertainty Principle

States that it is impossible to accurately determine simultaneously the exact position and motion of the electron.

Hund's Rule of Maximum Multiplicity

States that orbitals are filled up singly first before pairing.

Pauli Exclusion Principle

States that an orbital can accommodate a maximum of 2 electrons and no two electrons can have the same set of quantum numbers.

Aufbau’s Building Up Principle

States that lower energy levels are filled up first in an electron configuration.

Isotype

Nuclides with the same number of protons but different number of neutrons.

Isotones

Nuclides with the same number of neutrons but different number of protons.

Isobars

Nuclides with the same mass number but different protons, neutrons, and atomic numbers.

Law of Triads

A classification of elements proposed by Johann Wolfgang Dobereiner.

Law of Octaves

A classification of elements proposed by John Newlands.

Dmitri Mendeleev

Organized the periodic table by increasing mass number and predicted elements like Gallium and Germanium.

Henry Moseley

Organized the modern periodic table by increasing atomic number.

Stoichiometry

The branch of chemistry that calculates quantitative relationships between reactants and products in chemical reactions.