General Chemistry Review Flashcards

Comprehensive practice flashcards covering basic principles of matter, atomic structure, periodic trends, chemical bonding, acidity, and chemical kinetics based on the lecture transcript.

Chemistry

The science that deals with the study of properties, composition and changes that matter undergo.

Matter

Anything that occupies space and has mass; any material that composes of atoms, molecules, ions, or combination of these.

Intrinsic or Intensive Properties

Properties that are independent of amount, such as BP, FP, MP, Density, Optical activity and the Ratio of 2 extrinsic properties.

Extrinsic or Extensive Property

Properties that are dependent of amount, such as Mass and Volume.

Solids

Matter with a Lattice structure, orderly arrangement, definite volume, definite shape, strong IMFA, and vibrational molecular motion.

Liquid

Matter with a definite volume, definite shape, intermediate strength of IMFA, and gliding molecular motion.

Gas

Matter with indefinite volume and shape, weak IMFA strength, and constant random motion.

Plasma

An ionized gas.

Liquid Crystals

Matter with intermediate properties between solids (Lattice structure) and liquids (Flow Properties).

Law of Definite Proportions

States that elements combine in fixed ratio of whole numbers to form compounds.

Law of Multiple Proportions

States that elements combine in different ratio of whole numbers to form compounds.

Homogenous Mixture

A mixture that contains only one phase.

Brownian Movement

The zigzag movement of colloidal particles due to perfectly elastic collision.

Tyndall Effect

The scattering of light by colloidal particles.

Suspension

A mixture of insoluble substances suspended in a medium using a suspending agent.

Heterogenous Mixture

A mixture composed of 2 or more distinct phases, such as oil and water.

Direct union / Synthesis / Composition

The formation of complex substances from simpler substances, represented as $A + B \rightarrow AB$.

Decomposition / Analysis

The breakdown of a complex substance to simpler substances, represented as $AB \rightarrow A + B$.

Single Replacement

A reaction based on the activity series where a more active metal replaces a less active one: $A + BC \rightarrow AC + B$.

Double Displacement / Metathesis

A reaction in which two compounds exchange partners, represented as $AB + CD \rightarrow AD + BC$.

Organic Oxidation

The addition of oxygen, removal of hydrogen, or an increase in the number of C-O bonds.

Organic Reduction

The addition of hydrogen, removal of oxygen, or a decrease in the number of C-O bonds.

Billiard Ball Model

Dalton's model describing the atom as a hard, indestructible sphere.

Thompson Model

The Raisin Bread or Plum-Pudding Model where an atom is a sphere of positive particles with embedded negative particles.

Rutherford's Model

The Nuclear Model, established via the gold foil experiment, stating atoms consist of empty space with mass concentrated in a central nucleus.

Bohr Model

The Planetary Model where electrons move around the nucleus in circular orbits called orbitals.

Schrodinger's Model

The Quantum mechanical model where electrons reside in a 3D space called an electron cloud.

IsotoPes

Atoms with the same number of PROTONS.

IsoBars

Atoms with the same mass numBer.

IsotoNes

Atoms with the same number of NEUTRONS.

Principal Quantum Number ($n$)

Used to determine the overall energy of electrons and the size of the electron cloud; values range from $n = 1, 2, 3 \text{...} 7$.

Azimuthal / Angular Quantum Number ($\text{ℓ}$)

Determines the angular momentum and the shape of the orbital (Azi = Angular Zhape).

Hund’s Rule

States that orbitals are filled singly before pairing.

Pauli’s Exclusion Principle

States that no two electrons can have the same set of four quantum numbers.

Aufbau’s Building Up Principle

States that the buildup of electrons in an atom results from continually increasing the quantum number; used in electron configuration.

Johann Dobereiner

The scientist who proposed "Triads," where the average atomic weight of the 1st and 3rd members gave the weight of the 2nd member.

Henry Moseley

Modified the periodic law stating that properties of elements vary periodically with their atomic number.

Ionization Energy (IE)

The amount of energy needed to remove an electron from a neutral atom to convert it to a positively charged ion.

Electron Affinity (EA)

The amount of energy released when a neutral atom accepts an electron on its outermost shell to become a negatively charged ion.

Electronegativity (EN)

The tendency of an atom to attract electrons to itself when combined with another atom.

Ionic Bond

Formed by electron transfer resulting from electrostatic attraction between a metal and a nonmetal.

Covalent Bond

Formed by electron sharing resulting from atomic orbital overlap between two nonmetals.

Sigma bond ($σ$)

A head-on overlap between atomic orbitals along the internuclear axis.

Pi bond ($π$)

A lateral or sideways overlap between atomic orbitals, perpendicular to the internuclear axis.

Saturated solution

A solution containing the maximum amount of solute that will dissolve in a given solvent at a specific temperature.

Arrhenius Concept

Acids yield $H^+$ and bases yield $OH^-$.

Bronsted – Lowry Concept

Acids are proton donors and bases are proton acceptors.

Lewis Concept

Acids are electron pair acceptors and bases are electron pair donors.

Amphiprotic Compounds

Compounds that can both accept and donate protons, such as amino acids.

Collision Theory

States that the rate of reaction is proportional to the number of effective collisions requiring specific activation energy ($Ea$) and proper orientation.

Zero Order Reaction

A reaction where the rate is independent of the concentration of reactants, following the linear equation $Ct = -Kot + Co$.

Half Life ($t_{1/2}$)

The time required for the concentration of a drug to decrease by one half; for first order reactions, it is represented as $\frac{0.693}{K1}$.