Functional group 1

A part of a molecule that defines its reactivity and overall properties. It's responsible for how the molecule interacts with other molecules.

The study of how drugs are absorbed, distributed throughout the body, metabolized, and excreted.

The process by which a drug enters the bloodstream.

How a drug is transported throughout the body to reach its target.

The process of breaking down a drug into smaller metabolites in the body.

A carbon atom bonded to four different groups, creating a non-superimposable mirror image.

A three-dimensional representation of molecules. Wedge bonds point towards you, hashed bonds point away, and plain bonds are in the plane of the screen.

A step-by-step description of how a reaction occurs, showing the movement of electrons and formation/breaking of bonds.

A chemical species that donates electrons to form a new bond. It is typically electron-rich and has a negative charge or lone pair.

A chemical species that accepts electrons to form a new bond. It is typically electron-deficient and has a positive charge or partial positive charge.

A type of reaction where two electrons move together in a single step.

A type of reaction where one electron moves at a time, creating free radicals.

A chemical species with an unpaired electron, giving it high reactivity.

A single-headed arrow that shows the movement of one electron.

A species with an unpaired electron, often denoted with a dot.

The process of breaking a covalent bond by dividing the shared electrons equally.

A high-energy state that occurs during a reaction, where bonds are breaking and forming.

A stable molecule or ion that is formed during a reaction, existing between the reactants and products.

The energy required to reach the transition state, and therefore initiate the reaction.

A representation of the energy changes that occur throughout a reaction.

The stability of the intermediate radical formed during a reaction determines the distribution of products.

A type of chemical bond interaction where electrons from a sigma bond (single bond) are delocalized into an adjacent empty p orbital, stabilizing the molecule.

A radical with one unpaired electron on a carbon atom directly attached to a benzene ring. It's unusually stable due to resonance.

A radical with one unpaired electron on a carbon atom directly attached to a double bond. It's unusually stable due to resonance.

Describes the delocalization of electrons within a molecule, where electrons are not confined to a single bond but can be shared across multiple atoms.

Structures that show the possible arrangements of electrons in a molecule; not actual isomers, but rather representations of the extreme possibilities of electron location.

A structure representing the average of all possible resonance structures, where the electrons are delocalized and do not have a definite position.

A type of covalent bond formed by the overlap of p orbitals, allowing electrons to delocalize across multiple atoms.

Describes the stability of a molecule due to the delocalization of electrons through resonance, which helps to distribute charges and lower the overall energy of the molecule.

A special type of arrow used to show the movement of electrons in resonance structures, indicating that different contributing forms are possible but only one actual structure exists.

A resonance structure that contributes more to the overall structure of the molecule than others, usually the one with the most covalent bonds and minimal charge separation.

A resonance structure that contributes less to the overall structure of the molecule, usually the one with fewer covalent bonds and more charge separation.

A chemical compound containing only carbon and hydrogen atoms joined by single bonds. They are saturated hydrocarbons, meaning they have no double or triple bonds.

The process of breaking down a molecule into smaller parts, often through the addition of oxygen or other atoms.

The process of adding electrons to a molecule, often by removing oxygen or other atoms.

The point at which a drug interacts with its target molecule to exert its effect. It can be a specific receptor, enzyme, or other cellular component.

A type of drug that binds to a specific receptor or enzyme and prevents it from working, effectively stopping the cellular process.

A type of inhibitor where the drug forms a strong, irreversible covalent bond with its target, permanently inactivating it.

The tendency of a molecule to resist degradation or breakdown, especially when exposed to various chemical environments.

The process by which a drug is eliminated from the body, typically through urine, feces, or breath. It's the way the body gets rid of the drug.

The change in the concentration of a drug over time. It's a measure of how quickly the drug is absorbed, distributed, metabolized, and excreted.

The effect of a drug on the body, including its therapeutic effects and potential side effects.

The study of the chemical processes involved in the synthesis, metabolism, and degradation of drugs.

The movement of electrons in a chemical reaction, shown by curly arrows. A single-headed arrow indicates the movement of one electron, while a double-headed arrow indicates two electrons moving together.

The process of administering a drug into the body (e.g., swallowing a pill, injection, etc.)

Resonance structures are different ways of representing the electron distribution within a molecule, showing how electrons can be delocalized across multiple atoms. They are not real isomers, but rather extreme possibilities of where the electrons might be located.

Resonance structures are used to describe the delocalization of electrons in a molecule. This delocalization helps to stabilize the molecule by distributing the charge and energy across multiple atoms.

Sp3 hybridized atoms don't participate in resonance because they lack the necessary p-orbitals for electron delocalization. Only π electrons and lone-pair electrons can be moved in resonance structures.

The resonance hybrid is a representation of the actual molecule, where the electrons are not in a fixed position, but rather delocalized across multiple atoms. It is essentially an average of all the possible resonance structures.

The more covalent bonds a resonance structure has, the more stable it is. The more covalent bonds, the more the electrons are shared amongst atoms, resulting in a lower energy state.

The energy of the actual molecule is lower than any of the contributing resonance structures due to electron delocalization. The most stable resonance form makes the greatest contribution to the hybrid structure.

Resonance structures can only be drawn if the atoms involved are in the same plane. This is because p-orbital overlap is required for electron delocalization.

A double-headed resonance arrow is used to indicate that the structures are resonance forms, meaning they are different representations of the same molecule, not separate isomers.

A covalent inhibitor binds permanently to its target molecule, preventing it from working.

Amoxycillin is an example of a covalent inhibitor that binds to the active site of an enzyme involved in bacterial cell wall synthesis.

The reaction starts with an electron-rich alcohol (Serine) in the enzyme, and electrons move towards an electron-poor carbon atom (lactam) in the drug.

The lactam ring in amoxycillin converts into an ester and a secondary amine. This ester is stable and doesn't break down easily.

Alkanes are saturated hydrocarbons, containing only single bonds between carbon and hydrogen atoms.

General formula: CnH2n+2. They are very unreactive due to strong sigma bonds.

Alkanes are found in petroleum and are separated by distillation. They are used as fuels and raw materials for plastics.

Alkanes undergo combustion reactions, burning in air to produce carbon dioxide, water, and heat.

Alkanes can react with chlorine or bromine in a radical mechanism, which involves three steps: initiation, propagation, and termination.

The initiation step involves the formation of chlorine radicals due to the absorption of light energy.

The propagation step generates more radicals, where a chlorine radical abstracts a hydrogen atom from the alkane, forming a methyl radical.

The termination step involves the combination of two radicals to form a neutral species.

The stability of a radical determines the products formed in a reaction. More stable radicals form in greater amounts.

Hyperconjugation is the delocalization of electrons from a sigma bond into an adjacent empty p-orbital, stabilizing the radical.

A benzyl radical is a carbon radical attached to a benzene ring - it's unusually stable due to resonance.

An allyl radical is a carbon radical attached to a double bond - it's unusually stable due to resonance and hyperconjugation.