General Chemistry: Gases, Thermochemistry, and Atomic Structure Review

Comprehensive vocabulary flashcards covering pressure units, gas laws, thermodynamics, electromagnetic radiation, quantum mechanics, electron configurations, and periodic trends based on the lecture review.

Pressure Units Equivalence

The standard relationship between atmospheric pressure, torr, and millimeters of mercury: $1\,\text{atm} = 760\,\text{torr} = 760\,\text{mmHg}$.

Gas Laws

The fundamental empirical relationships governing gases, including the laws of Boyle, Charles, Gay Lussac, Avogadero, Dalton, and Graham.

Ideal Gas Equation

The equation of state of an ideal gas expressed as $PV = nRT$.

Combined Gas Equation

The formula relating initial and final states of pressure, volume, amount of gas, and temperature: $\frac{P_1V_1}{n_1T_1} = \frac{P_2V_2}{n_2T_2}$.

Kinetic Molecular Theory (KMT)

A foundational physical model used to explain the behavior, properties, and laws of gases based on particle motion.

Calorie to Joule Conversion

The exact quantitative conversion between calories and joules: $1\,\text{cal} = 4.184\,\text{J}$.

Change in Internal Energy ($\Delta E$ or $\Delta U$)

The change in the total energy of a system, defined mathematically by the first law as $\Delta E = Q + W$ (or $\Delta U = Q + W$), where $Q$ is heat and $W$ is work.

Specific Heat Capacity ($c$)

The amount of heat required to raise the temperature of a given mass of a substance, calculated using the equation $Q = mc\Delta T$.

Heat of Reaction ($\Delta H$)

The enthalpy change associated with a balanced chemical reaction in stoichiometry.

Exothermic and Endothermic

Classifications of chemical processes based on whether heat is released ($\Delta H < 0$, exothermic) or absorbed ($\Delta H > 0$, endothermic).

Speed of Light ($c$)

The speed of electromagnetic radiation, defined by the formula $c = \text{frequency} \times \text{wavelength}$.

Energy of a Photon ($E$)

The quantized energy carried by an individual photon, given by $E = h \cdot v$, where $h$ is Planck's constant and $v$ is frequency.

Nanometer (nm)

A metric unit of length defined as $1\,\text{nm} = 1 \times 10^{-9}\,\text{m}$ (or $1\,\text{m} = 1 \times 10^9\,\text{nm}$).

Neils Bohr Atomic Theory

An atomic model postulating that atomic electrons occupy discrete orbits characterized by the quantization of energy.

Orbital

A mathematical three-dimensional region within atomic subshells and shells where there is a high probability of finding an electron.

Quantum Numbers

The set of four values ($n$, $l$, $m_l$, $m_s$) that specify the shell, subshell, orbital orientation, and spin state of an electron in an atom.

Valence Electrons

The outermost electrons responsible for chemical bonding, determined differently for Main group elements (such as C) and Transition elements (such as Fe).

Paramagnetic and Diamagnetic

Magnetic properties of atoms or ions: paramagnetic materials have unpaired electrons and are attracted to magnetic fields, while diamagnetic materials have all paired electrons and are weakly repelled.

Periodic Table Trends

Systematic predictable patterns observed across periods and groups in the Periodic Table, including Ionization energy (IF), Size (radius), and Metallic character.

Sizes of Ions (Cations and Anions)

The relative dimensions of charged species compared to neutral atoms: cations lose electrons and become smaller than their neutral parent atoms, whereas anions gain electrons and become bigger.