General Chemistry Equations, Constants, and Relationships

Comprehensive vocabulary flashcards covering the key chemistry formulas, variables, and units from the reference sheet.

Density

The relationship given by $d = \frac{m}{V}$, where $d$ is density ($\text{g/cm}^3$ or $\text{g/mL}$), $m$ is mass ($\text{g}$), and $V$ is volume ($\text{cm}^3$ or $\text{mL}$).

Temperature (Kelvin Conversion)

The conversion formula $T_K = T_{^\circ\text{C}} + 273.15$, where $T_K$ is temperature in Kelvin and $T_{^\circ\text{C}}$ is temperature in Celsius.

Atomic Mass

The weighted average formula $\text{Avg Mass} = \sum (f_i \times m_i)$, where $f_i$ represents fractional abundance and $m_i$ represents isotopic mass ($\text{amu}$).

Mole Conversions

The particle conversion formula $N = n \times N_A$, where $N$ is particle count, $n$ is amount in moles ($\text{mol}$), and $N_A = 6.022 \times 10^{23}$.

Wave Mechanics

The fundamental wave equation $c = \lambda \nu$, where $c$ is the speed of light, $\lambda$ is wavelength ($\text{m}$), and $\nu$ is frequency ($\text{s}^{-1}$ or $\text{Hz}$).

Photon Energy

The relationship $E_{\text{photon}} = h\nu = \frac{hc}{\lambda}$, where $E$ is energy ($\text{J}$), $h$ is Planck's constant, and $\nu$ is frequency ($\text{Hz}$).

Photoelectric Effect

The energetic relationship $h\nu = \Phi + KE_{\text{electron}}$, where $\Phi$ is the work function ($\text{J}$) and $KE$ is the kinetic energy of the ejected electron ($\text{J}$).

Hydrogen Energy

The energy level formula $E_n = -2.18 \times 10^{-18}\,\text{J}\left(\frac{1}{n^2}\right)$, where $n$ is the principal quantum number ($n = 1, 2, 3, \dots$).

Hydrogen Transition Energy

The energy change during an electron transition given by $\Delta E = -2.18 \times 10^{-18}\,\text{J}\left(\frac{1}{n_f^2} - \frac{1}{n_i^2}\right)$, where $n_i$ and $n_f$ are the initial and final quantum states.

Rydberg Wavelength

The formula $\frac{1}{\lambda} = R_H\left(\frac{1}{m^2} - \frac{1}{n^2}\right)$, where $R_H = 1.097 \times 10^7\,\text{m}^{-1}$ and $m < n$.

de Broglie Wavelength

The matter wavelength relationship $\lambda = \frac{h}{mv}$, where $m$ is mass ($\text{kg}$), $v$ is velocity ($\text{m/s}$), and $h$ is Planck's constant.

Uncertainty Principle

Heisenberg's principle expressed as $\Delta x \cdot m\Delta v \ge \frac{h}{4\pi}$, where $\Delta x$ is position uncertainty ($\text{m}$) and $\Delta v$ is velocity uncertainty ($\text{m/s}$).

Effective Charge

The formula $Z_{\text{eff}} = Z - S$, where $Z$ is the atomic number and $S$ is the number of core shielding electrons.

Empirical Multiplier

The integer ratio $n = \frac{\text{Molar Mass}}{\text{Empirical Mass}}$, where $n$ serves as the multiplier to convert an empirical formula into a molecular formula.

Percent Yield

The yield ratio given by $\text{\% Yield} = \frac{\text{Actual Yield}}{\text{Theoretical Yield}} \times 100\%$, where actual and theoretical yields are expressed in grams or moles.

Molarity

The concentration relationship $M = \frac{n_{\text{solute}}}{V_{\text{solution}}}$, where $M$ is molarity ($\text{mol/L}$), $n$ is moles of solute, and $V$ is liters of solution.

Dilution

The volumetric dilution relationship $M_1V_1 = M_2V_2$, where $M_1$ and $M_2$ are initial and final molarities, and $V_1$ and $V_2$ are initial and final volumes.

Ideal Gas Law

The equation of state $PV = nRT$, where $P$ is pressure ($\text{atm}$), $V$ is volume ($\text{L}$), $n$ is moles, and $T$ is temperature ($\text{K}$).

Gas Density

The density formula for an ideal gas $d = \frac{PM}{RT}$, where $P$ is pressure ($\text{atm}$), $M$ is molar mass ($\text{g/mol}$), and $T$ is temperature ($\text{K}$).

Partial Pressures

Dalton's relationships given by $P_i = \chi_i P_{\text{total}}$ and mole fraction $\chi_i = \frac{n_i}{n_{\text{total}}}$, where $P_i$ is partial pressure and $\chi_i$ is mole fraction.

Gas RMS Speed

The root-mean-square speed equation $u_{\text{rms}} = \sqrt{\frac{3RT}{M}}$, where $R = 8.314\,\text{J/(mol}\cdot\text{K)}$, $T$ is temperature in $\text{K}$, and $M$ is molar mass in $\text{kg/mol}$.

Average Kinetic Energy

The relationship $KE_{\text{avg}} = \frac{3}{2}RT$, which depends only on temperature $T$ (in $\text{K}$) and is independent of gas mass.

Graham's Effusion

The rate relationship $\frac{\text{Rate}_1}{\text{Rate}_2} = \sqrt{\frac{M_2}{M_1}}$, stating that the effusion rate of a gas is inversely proportional to the square root of its molar mass.

van der Waals Gas

The real gas equation $\left[P + a\left(\frac{n}{V}\right)^2\right][V - nb] = nRT$, where $a$ is the correction for attractive forces and $b$ is the correction for particle volume.