AP Chemistry Bridge Review Flashcards

This flashcard set covers essential vocabulary and concepts from the AP Chemistry bridge review, including periodic trends, stoichiometry, gas laws, and chemical bonding.

Isotopes

Atoms of the same element that exist naturally with different masses, such as $X-35$ ($34.97\,amu$) and $X-37$ ($36.97\,amu$).

Average Atomic Mass

The weighted average of the masses of naturally occurring isotopes; for element $X$ with $75.8\%$ $X-35$ and $24.2\%$ $X-37$, it is approximately $35.45\,amu$.

First Ionization Energy

The energy required to remove the outermost electron from an atom; for example, Mg has a higher first ionization energy than Na.

Atomic Radius

The distance from the nucleus to the outer boundary of the electron cloud, which decreases across a period due to increasing effective nuclear charge.

Ground-state Electron Configuration

The most stable, lowest-energy arrangement of electrons; for sulfur, it is $1s^22s^22p^63s^23p^4$.

Ionic Compound Formula

The ratio of ions in a neutral compound; for aluminum and sulfate ions, the correct formula is $Al_2(SO_4)_3$.

Linear Molecular Geometry

A molecular shape where atoms are arranged in a straight line ($180^\circ$), such as in carbon dioxide ($CO_2$).

Nonpolar Molecule

A molecule with an even distribution of charge, such as $CO_2$, which contains polar bonds that cancel out due to its linear geometry.

Limiting Reactant

The reactant that is completely consumed in a reaction and determines the maximum amount of product that can be formed.

Molarity (M)

A measure of concentration defined as the number of moles of solute per liter of solution ($mol/L$).

Catalyst

A substance that lowers the activation energy of a reaction without changing $\Delta H$ or being consumed by the reaction.

pH

A measure of the acidity or basicity of a solution; a $0.010\,M$ $HCl$ solution has an approximate pH of $2$.

Resonance Structures

Multiple valid Lewis structures used to represent a single molecule or ion, such as the nitrate ion ($NO_3^-$), where the actual structure is an average of these forms.

Formal Charge

The charge assigned to an atom in a Lewis structure, calculated to determine the most plausible arrangement of electrons.

Theoretical Yield

The maximum amount of product that can be produced from a given amount of reactant based on stoichiometric calculations.

Percent Yield

The ratio of the actual yield obtained in an experiment to the theoretical yield, calculated as $(\text{actual yield} / \text{theoretical yield}) \times 100\%$.

Ideal Gas Constant (R)

The constant used in the ideal gas law equation, given here as $0.08206\,L \cdot atm \cdot mol^{-1} \cdot K^{-1}$.

Specific Heat

The amount of heat required to raise the temperature of one gram of a substance by one degree Celsius; for water, this is $4.184\,J/g^\circ C$.

Collision Theory

A model used to explain reaction rates, stating that reactant particles must collide with sufficient energy and Proper orientation to react.

Equivalence Point

The stage in a titration where the number of moles of titrant added is stoichiometrically equal to the number of moles of analyte present.