Chemistry Quiz: molecular structure and bonding

The process by which drugs are broken down by the body, usually in the liver. It alters a drug's structure, making it easier to excrete.

The amount of drug that reaches systemic circulation after administration. Determined by the drug's absorption, distribution and metabolism.

The interaction of a drug with its specific target site, often a protein or enzyme, which initiates a chain of events leading to the drug's effect.

The study of how a drug's concentration changes over time in the body. Involves absorption, distribution, metabolism, and excretion.

A chemical bond formed by the sharing of electrons between atoms.

A chemical bond formed by the attraction of oppositely charged ions.

The specific arrangement of atoms in a molecule, which determines its chemical properties and interactions.

A group of atoms within a molecule that confers specific chemical properties.

The amount of substance containing a specific number of elementary entities, defined as 6.02214076 × 10^23 entities (Avogadro's number).

The mass of one mole of a substance. Expressed in grams per mole (g/mol).

The process of calculating the number of moles in a given mass of a substance, using the formula: Moles = Mass / Molecular mass.

An atom's ability to attract electrons towards itself when forming a chemical bond.

Electronegativity increases across a period (left to right) as atoms become smaller and more strongly attract electrons.

A scale used to measure the electronegativity of elements.

Electrons are not confined to fixed positions, but rather exist in regions of space where they are most likely to be found.

A region of space around the nucleus where an electron is most likely to be found.

The spherical region of space around the nucleus where an s-orbital electron is mostly found.

A dumbbell-shaped region of space around the nucleus where a p-orbital electron is mostly found.

A group of orbitals in an atom that have the same principal quantum number, thus having similar energy levels.

The number of covalent bonds an atom forms to achieve a stable noble gas electron configuration.

p orbitals having the same energy level.

A point in an orbital where the probability of finding an electron is zero.

An atom that needs to gain additional electrons to reach a stable electron configuration like a noble gas.

The most stable and lowest-energy configuration of an atom's electrons in their respective orbitals.

Electron pairs in the outer shell of an atom that are not involved in bonding.

A principle that states electrons fill the lowest available energy levels first, starting from the 1s orbital.

The sum of valence electrons minus the number of lone pair electrons and half the number of bonding electrons.

A principle that states each orbital can hold a maximum of two electrons, each with opposite spins.

A species with a single unpaired electron.

A method to determine formal charge that is better for analyzing isolated structures than dynamic chemical reactions.

A rule that states when filling orbitals with the same energy level, electrons occupy each orbital individually with parallel spins before pairing in an orbital.

The process by which atomic orbitals mix together to form new hybrid orbitals with different shapes and energies.

The process of tracking the movement of electrons during bond formation and breakage.

Carbon forms four bonds with other atoms, due to the hybridization of its orbitals.

A neutral atom that gains two electrons becomes negatively charged, and a neutral atom that loses two electrons becomes positively charged.

The outermost electron shell of an atom.

The process of combining atomic orbitals to form new hybrid orbitals with equivalent energy levels.

A measure of the net polarity of a molecule.

A molecule with a separation of electrical charge, resulting in a positive and negative end.

A molecule without a separation of electrical charge, all its atoms are equally electronegative.

A compound that results from the gaining or losing of electrons, resulting in a charged atom.

A chemical bond where one atom donates an electron to another atom, forming oppositely charged ions that then attract.

A neutral collection of atoms held together by covalent bonds.

The ability of an atom to polarize a bond, influencing the distribution of electrons.

A shorthand way of writing chemical structures, where carbon atoms are assumed at intersections of lines.

The electrons in the outermost shell of an atom, determining its bonding behavior.

A bond formed by the direct overlap of atomic orbitals along the line joining the bonded nuclei.

A bond resulting from the sideways overlap of atomic orbitals, creating electron density above and below the bond axis.

A type of orbital hybridization where one s orbital and three p orbitals combine, forming four sp3 hybrid orbitals. These orbitals point towards the corners of a tetrahedron.

A type of orbital hybridization where one s orbital and two p orbitals combine, forming three sp2 hybrid orbitals, leaving one unhybridized p orbital.

A type of orbital hybridization where one s orbital and one p orbital combine, forming two sp hybrid orbitals, leaving two unhybridized p orbitals.

A molecule with a central carbon atom attached to four hydrogen atoms; it is a classic example of sp3 hybridization.

A molecule with two carbon atoms each attached to three hydrogen atoms. The carbon-carbon bond results from the overlap of sp3 orbitals.

A molecule with two carbon atoms each attached to two hydrogen atoms. The carbon-carbon bond results from the overlap of sp2 orbitals.

A molecule with two carbon atoms each attached to one hydrogen atom. The carbon-carbon bond results from the overlap of sp orbitals.

The central carbon atom in the molecule is bonded to three hydrogen atoms, giving it a positive charge.

The central carbon atom in the molecule is bonded to three hydrogen atoms, giving it a single unpaired electron.

Represents the strength of a bond, determined by the energy required to break it. Stronger bonds require more energy to break.

Indicates the distance between two bonded atoms. Shorter bond lengths generally suggest stronger bonds.

Describes the angle formed between two bonds originating from the same atom. Bond angles are influenced by the hybridization of the central atom.