CHM-101 Chapters 3 and 4 Bulk Review

Vocabulary practice flashcards covering electromagnetic radiation, electron configurations, quantum numbers, periodic trends, and chemical bonding from Chapters 3 and 4 review.

Microwaves (Electromagnetic Spectrum)

The form of electromagnetic radiation among gamma rays, visible light, infrared, and microwaves that possesses the longest wavelength and lowest frequency.

Wavelength and Frequency Relationship

The inverse proportional relationship governing electromagnetic radiation traveling through a vacuum, expressed as $c = \nu \times \frac{\text{m}}{\text{s}}$, where waves with shorter wavelengths correspond to higher frequencies.

Photon Energy ($E$)

The quantum of energy carried by a single photon of electromagnetic radiation, given by the relation $E = h\nu$, where radiation with higher frequency possesses higher energy per photon.

Bohr Model Emission Transition

An electron transition from a higher energy level down to a lower principal energy level that emits light; the transition between the largest energy difference (such as from $n = 5$ to $n = 1$) emits light with the shortest wavelength.

Orbital Electron Capacity

The rule based on the Pauli exclusion principle stating that any single atomic orbital can accommodate a maximum of two electrons with opposing spins.

$p_y$ Orbital

A dumbbell-shaped atomic orbital oriented specifically along the y-axis, characterized by the angular momentum quantum number $l = 1$.

Aufbau Principle

The rule stating that electrons fill lower-energy subshells (such as $2s$) completely before occupying higher-energy subshells (such as $2p$).

Potassium Valence Quantum Numbers

The set of quantum numbers representing the single ground-state valence electron of potassium ($K$) in the $4s$ subshell: $n = 4$, $l = 0$, $m_l = 0$, and $m_s = -\frac{1}{2}$ (or $+\frac{1}{2}$).

Electron Configuration of Selenium ($Se$)

The ground-state distribution of electrons for atomic number 34: $1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10} 4p^4$.

Valence Electrons

Electrons occupying the outermost principal energy level ($n$) that determine chemical bonding properties; for arsenic ($[Ar]\text{ }4s^2 3d^{10} 4p^3$), there are 5 valence electrons.

Core Electrons

Electrons in an atom that occupy completed inner energy shells and do not participate directly in bonding, shielding the nucleus from the outer valence electrons.

Isoelectronic Species

Atoms and ions that share the identical ground-state electron configuration; for example, the oxide ion ($O^{2-}$) and neon ($Ne$) both possess 10 electrons ($1s^2 2s^2 2p^6$).

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

The net positive charge experienced by valence electrons from the nucleus, which generally increases across a period from left to right and remains relatively constant down a group.

Atomic Radius Trend

The periodic trend where atom size decreases across a period from left to right due to increased effective nuclear charge, and increases down a group due to added shells (e.g., $Na > Mg > Si > P > Ar$).

Successive Ionization Energies

The progressive energies required to remove electrons one by one; a sharp increase between the 3rd ($2745\,kJ\,mol^{-1}$) and 4th ($11580\,kJ\,mol^{-1}$) ionization energy indicates that the element has three valence electrons and belongs to Group 13 (such as aluminum).

Oxide Ion Lewis Dot Symbol

The Lewis symbol representation for the $O^{2-}$ anion, consisting of the symbol O surrounded by an octet of eight dots and a $2-$ charge designation.

Coulomb Force (Ionic Attraction)

The electrostatic attraction between oppositely charged ions, which increases with higher ion charges ($q_1, q_2$) and smaller ionic radii.

1:1 Binary Ionic Lattice

A crystal lattice structure containing an equal alternating ratio of cations to anions, exemplified by compounds such as $CaO$.

Cobalt(II) Nitrate Hexahydrate

The systematic IUPAC name for the transition metal hydrate salt with the formula $Co(NO_3)_2 \cdot 6H_2O$.

Covalent Bond

A chemical bond formed by the sharing of valence electron pairs between nonmetals, producing discrete molecules.

Bonding and Nonbonding Electron Pairs (Methanol)

In the methanol ($CH_3OH$) molecule, the five covalent single bonds represent five bonding pairs, while the oxygen atom carries two unshared nonbonding (lone) pairs.

Sulfur Tetrafluoride

The systematic molecular name for the binary compound composed of one sulfur atom covalently bonded to four fluorine atoms, having the chemical formula $SF_4$.