Chemistry Review: Redox Reactions, Electron Transitions, Gas Laws, and Chemical Bonding

Vocabulary practice flashcards covering acidic redox balancing, electron energy transitions, gas law formulas and conversions, partial pressure, polarity rules, and chemical bond types based on the lecture notes.

Oxygen Balancing in Acidic Solutions

The step in balancing acidic redox reactions where oxygen atoms are balanced by adding water molecules ($H_2O$).

Hydrogen Balancing in Acidic Solutions

The step in balancing acidic redox reactions where hydrogen atoms introduced by water are balanced by adding hydrogen protons ($H^+$).

Charge Balancing (Redox Half-Reactions)

The procedure of adding electrons to the side with the higher positive charge so that both sides of a half-reaction have equivalent overall charge.

Electron Cancellation

The requirement when combining redox half-reactions to multiply one or both reactions by integers so the number of electrons is equal on both sides and cancels out completely.

Excited State

The state of an electron that has absorbed energy and jumped from its baseline energy level to a higher energy level.

Energy Absorption (Atomic)

The process occurring when an electron moves upward between energy levels, requiring the uptake of a photon.

Photon Emission

The release of light energy occurring when an excited electron falls back down from a higher level toward baseline.

Transition Energy Magnitude

The principle that the electron transition spanning the largest distance between energy levels absorbs or emits a photon with the highest energy and largest frequency.

Boyle's Law

A gas law stating that pressure and volume are inversely proportional at constant temperature, represented by the formula $P_1V_1 = P_2V_2$.

Ideal Gas Law

The central gas equation relating four variables: $PV = nRT$, where $R$ is approximately $0.08$, pressure is typically in atmospheres, and temperature is in Kelvin.

Kelvin Temperature Conversion

The temperature scale conversion determined by adding $273$ to the temperature in degrees Celsius.

Charles's Law

A gas law that relates volume and temperature at constant pressure, in which volume divided by temperature remains constant ($\frac{V_1}{T_1} = \frac{V_2}{T_2}$).

Avogadro's Law

A gas principle comparing volume and the amount of gas in moles ($n$), expressed as $\frac{V_1}{n_1} = \frac{V_2}{n_2}$.

Combined Gas Law

A formula combining Boyle's law, Charles's law, and related gas laws used to solve problems where three variables change simultaneously.

Partial Pressure

The individual pressure exerted by a single gas component within a mixture, which can be found by subtracting all other component pressures from the total pressure.

Electronegativity Trend

The periodic table trend that increases upward and to the right, identifying fluorine as the most electronegative element.

Carbon-Hydrogen Bond ($C-H$)

A chemical bond that is always nonpolar, regardless of whether it is a single, double, or triple bond.

Molecular Symmetry

A structural characteristic where a molecule (such as $CO_2$) possesses a plane of symmetry or mirror image, rendering the overall molecule nonpolar despite having polar bonds.

Covalent Bond

A type of chemical bond formed specifically when two nonmetals are bonded together.

Ionic Bond

A chemical bond formed between a metal (from the left side of the periodic table) and a nonmetal (from the right side).

Metallic Bond

A chemical bond formed when two metals bond together.

Molecular Geometry

The three-dimensional shape of a molecule, determined by the number of atoms attached to the central atom, the number of lone pairs, and the resulting bond angles.