General and Inorganic Medicinal Chemistry Review

A comprehensive set of practice flashcards covering general chemistry, inorganic medicinal, organic chemistry, and pharmacology based on the provided lecture transcript.

Chemistry

Science that deals with the composition, structure, and properties of substances and with the transformations or changes that they undergo; study of matter.

Antoine Lavoisier

Known as the Father of Modern Chemistry who established the law of conservation of mass.

Complete Combustion

Occurs when there is an abundant supply of oxygen, primarily producing $CO_2$ and $H_2O$.

Incomplete Combustion

Occurs when there is a limited supply of oxygen, producing carbon monoxide ($CO$), soot, and other byproducts.

Law of Conservation of Mass

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

Law of Mass Action

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

Law of Definite Proportion

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

Law of Multiple Proportion

States weights of one element combining with a fixed weight of another are in a ratio of small whole numbers.

Matter

Any substance that has mass and takes up space.

Plasma

The fourth and most abundant state of matter, composed of protons and electrons and affected by magnetic fields.

Distillation

Method of separating components of a mixture by a series of evaporation and condensation.

Decantation

Method of separating mixtures based on the difference of specific gravity or density.

Centrifugation

Method of separating finely suspended particles in a liquid by whirling the liquid at high speed.

Filtration

Method of separating an insoluble solid from a liquid using filter paper.

Chromatography

Method of separating mixtures based on differences in solvent affinities.

Intrinsic Property

Property independent of the amount of matter, such as density or boiling point.

Extrinsic Property

Property dependent on the amount of matter, such as mass or volume.

Atom

The building block of matter.

Billiard Ball Model

Proposed by John Dalton, it describes the atom as a hard, indestructible sphere.

Plum Pudding Model

Proposed by J.J. Thomson, who discovered electrons via the Cathode Ray Tube.

Nuclear Model

Proposed by Ernest Rutherford, stating atoms are mainly empty space with a positive nucleus.

James Chadwick

The discoverer of the neutron.

Planetary Model

Proposed by Niehls Bohr, describing electrons orbiting the nucleus like planets.

Quantum Model

Proposed by Erwin Schrodinger, stating electrons move in waves in a defined space called an electron cloud.

Heisenberg Uncertainty Principle

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

Aufbau Building Up Principle

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

Hund’s Rule

States that orbitals are filled up singly first before pairing.

Pauli’s Exclusion Principle

States no two electrons in an atom can have the same values for all four quantum numbers.

Isotopes

Atoms with the same number of protons but different numbers of neutrons.

Isotones

Atoms with the same number of neutrons but different numbers of protons.

Isobars

Atoms with the same mass number but different numbers of protons and neutrons.

Law of Triads

Proposed by Johann Wolfgang Dobereiner, where the middle element's mass is the average of the first and last.

Law of Octaves

Proposed by John Newlands, stating every eighth element has properties similar to the first.

Henry Moseley

Arranged the modern periodic table by increasing atomic number.

Ionization Energy

The minimum amount of energy required to remove an electron from an isolated gaseous atom or ion.

Electron Affinity

The amount of energy released when an electron attaches to a neutral atom to form an anion.

Electronegativity

The ability of an atom to attract electrons.

Alpha Hydroxy Acids

Carboxylic acids featuring a hydroxy group located one carbon atom away from the acid group, such as lactic acid.

Beta Hydroxy Acid

A carboxylic acid containing a hydroxy functional group separated by two carbon atoms, such as salicylic acid.

Buffer Capacity

The amount of a strong acid or base that must be added to a liter of solution to change the pH by 1 unit.

Collision Theory

States that a reaction occurs when reactant molecules collide.

Le Chatelier’s Principle

States that when stress is applied to a system in equilibrium, the equilibrium shifts to relieve that stress.

First-Order Kinetics

Reaction where the rate is directly proportional to the concentration of one reactant.

Zero-Order Kinetics

Reaction where the rate is independent of the concentration of the reactant(s).

Boyle’s Law

States that pressure and volume are inversely proportional at constant temperature and moles.

Charles's Law

States that volume and temperature are directly proportional at constant pressure and moles.

Dalton’s Law of Partial Pressures

States the total pressure of a gas mixture is the sum of the partial pressures of individual gases.

Enthalpy

A measure of the heat content of a system.

Entropy

The degree of disorderliness in a system.

First Law of Thermodynamics

States that energy cannot be created or destroyed, only transferred or converted.

Second Law of Thermodynamics

States the entropy of an isolated system always increases over time or remains constant in ideal cases.

Third Law of Thermodynamics

States the entropy of a perfect crystal at absolute zero is zero.

Geiger counter

A device used to measure radiations.

Becquerel (Bq)

The SI unit for radioactivity, equal to 1 disintegration per second.

Sievert (Sv)

The SI unit that measures tissue damage caused by radiation.

Electron Capture

The addition of an electron to a proton in the nucleus, transforming the proton into a neutron.

Electrolytes

Inorganic compounds which mostly constitute the solute in body fluids.

Ebstein’s anomaly

A congenital cardiac defect associated with Lithium use during pregnancy.

Wilson’s disease

Copper toxicity characterized by bronze-like skin.

Argyria

Darkened skin resulting from chronic silver exposure.

Itai-itai disease

A disease caused by cadmium toxicity.

Minamata disease

A neurotoxic condition caused by organic mercury poisoning.

Silicosis

A TB-like condition resulting from chronic inhalation of silicon dioxide ($SiO_2$).

Antiseptic

Compounds that kill or prevent microbial growth when applied to living tissues.

Disinfectant

An agent that destroys pathogenic microorganisms when applied to inanimate objects.

Simethicone

A defoaming agent useful in preventing gassy feelings caused by antacids.

Sun Protection Factor (SPF)

A measure of how well a sunscreen protects against UVB rays.

Protium

The most abundant, common, and stable isotope of Hydrogen.

Deuterium oxide

Also known as heavy water, used as a solvent in NMR Spectroscopy.

Beryllium

The most toxic metal in common use.

Hydroxyapatite

The form in which calcium is found in bones and teeth.

Polymorphism

The ability of a solid material to exist in more than one crystal structure.

Allotropism

The property of an element to exist in two or more different forms in the same physical state.

Paul Ehrlich

Known as the Father of Chemotherapy, he discovered Arsphenamine for syphilis.

Nucleophiles

Electron-rich species that attack positive charges.

Electrophiles

Electron-poor species that are attacked by negative charges.

Sigma bond

Any first bond between atoms, formed by hybridized orbitals.

Pi bond

Secondary or tertiary bonds formed by unhybridized orbitals.

Alkanes

Saturated hydrocarbons with single bonds, also known as paraffins.

Alkenes

Unsaturated hydrocarbons containing at least one double bond, also known as olefins.

Alkynes

Unsaturated hydrocarbons containing at least one triple bond, also known as acetylenes.

Huckel’s Rule

States a planar cyclic molecule is aromatic if it has $4n + 2$ pi electrons.

Enantiomers

Stereoisomers that are non-superimposable mirror images of each other.

Diastereomers

Stereoisomers that are not mirror images of each other.

Epimers

Diastereomers that differ in configuration at only one stereogenic center.

Markovnikov’s Rule

In addition of HX to alkenes, the H attaches to the carbon with more hydrogens.

Zaitsev’s Rule

In elimination reactions, the major product is the alkene with the greater number of alkyl groups attached to the double bond.

Tollens' Test

A test for aldehydes where a silver mirror is formed.

Biotransformation

The biochemical modification of a chemical compound within a living organism.

Prodrug

An inactive or less active form of a drug transformed within the body to its active form.

Glucuronidation

The most common Phase II conjugation reaction, using the coenzyme UDPGA.

Acetylation

A Phase II metabolic route for primary amino groups, using Acetyl-CoA.

First-Pass Metabolism

Extensive metabolism of orally administered drugs before reaching systemic circulation.

Red man’s syndrome

An adverse effect of Vancomycin characterized by flushing, avoidable by slow administration.

Aminoglycosides

Protein synthesis inhibitors that bind to the 30s subunit, including Streptomycin and Amikacin.

Cinchonism

Toxicity caused by cinchona alkaloids such as Quinine and Chloroquine.

Albendazole

An anthelmintic agent that works by inhibiting glucose uptake.

Ivermectin

The drug of choice for River blindness, inducing flaccid paralysis via hyperpolarization.

Praziquantel

The drug of choice for Schistosoma mansoni, inducing spastic paralysis.

Vinca Alkaloids

Plant alkaloids such as Vincristine and Vinblastine that inhibit mitotic spindle assembly.