Chemistry Unit 1 and Chemical Bonding Vocabulary

Vocabulary flashcards generated from lecture notes covering chemical bonding types, intermolecular forces, gas laws, and periodic trends.

Hydrogen Bond

An intermolecular attraction occurring when a hydrogen donor attached to fluorine, oxygen, or nitrogen ($\text{F, O, N}$) interacts with an $\text{F, O, N}$ acceptor.

Dipole-Induced Dipole (D-ID)

An intermolecular attraction between a polar molecule with a permanent dipole and a nonpolar molecule in which a dipole is temporarily induced (e.g., $\text{H-Cl}$ and $\text{Cl-Cl}$).

Induced Dipole-Induced Dipole (ID-ID)

An intermolecular attraction occurring between nonpolar molecules due to temporary fluctuations in their electron clouds (e.g., $\text{Cl-Cl}$ and $\text{Cl-Cl}$).

Normal Boiling Point

The temperature at which a liquid transitions into a gas ($\text{L} \rightarrow \text{G}$) under an external pressure of $1\,atm$.

Micelle

A structure formed by soap molecules in water, where hydrophobic nonpolar tails dissolve lipid-based pathogens and hydrophilic polar heads interact with water to wash them away.

Resonance

Molecules that share the same skeletal connectivity of atoms but differ in the placement of bonding pair or lone pair electrons.

Isomers

Molecules that possess the same chemical formula but have different skeletal connectivity of their atoms.

Formal Charge (FC)

A calculation used to assess Lewis structure stability, defined as $FC = \text{\# valence } e^- - (\text{\# bonds} + \text{nonbonds})$.

Electronegativity

A measure of how strongly an atom of a given element pulls on electrons within a chemical bond.

Ideal Gas

A theoretical gas model assuming particles have zero volume and experience no intermolecular interactions, possessing only kinetic energy ($KE$).

Real Gas Parameters ($a$ and $b$)

Corrections to ideal gas behavior where parameter $a$ accounts for intermolecular attractions and parameter $b$ accounts for particle bigness/volume.

Dalton's Law of Partial Pressures

A law stating total pressure is the sum of partial pressures ($P_{\text{total}} = P_A + P_B + \dots$), where the partial pressure of gas $X$ is $P_X = P_{\text{total}} \times X_X$.

Metallic Bonding

Bonding found exclusively in metallic elements that yields malleable, bendable, hard, flexible, and insoluble substances that conduct electricity in the dry state.

Molecular Covalent Bonding

Bonding consisting of nonmetals sharing electrons, producing soft, liquid, or gaseous substances that are soluble but non-conductive.

Ionic Bonding

Bonding formed between metals (cations) and nonmetals (anions) where metals give up electrons and nonmetals steal electrons, creating hard, brittle, soluble substances that conduct in solution.

Extended Covalent Bonding

Bonding composed only of nonmetals in a continuous network that yields hard, rigid, insoluble, non-conductive substances that are difficult to break.

HONC 1234 Rule

A rule indicating the standard number of covalent bonds formed by organic elements: Hydrogen forms $1$, Oxygen forms $2$, Nitrogen forms $3$, and Carbon forms $4$.

Bond Order

The measure of bond strength in resonance structures, calculated as $\text{Sum of bonds} / \text{\# of resonance structures}$.

Effective Nuclear Charge ($Z_{\text{eff}}$)

The net positive charge experienced by valence electrons, calculated using the equation $Z_{\text{eff}} = \text{Protons} - \text{core electrons}$.

Coulomb's Law

An electrostatic principle stating opposite charges attract and like charges repel, where force increases with greater charge and decreases with greater distance (radius).

Isotopes

Atoms of the same element that contain different numbers of neutrons, resulting in different atomic masses.

Cation

A positively charged ion formed when a metal atom loses electrons.

Anion

A negatively charged ion formed when a nonmetal atom gains electrons.