Chemistry Final Exam Review Guide Flashcards

These flashcards cover key vocabulary, chemical reaction types, thermochemistry, gas laws, and solution chemistry based on the final exam review guide.

Atom

A fundamental vocabulary term from the chemistry units representing the basic unit of a chemical element.

Synthesis Reaction

A reaction type where two or more substances combine to form a new compound, such as $P(s) + O_2(g) \rightarrow P_4O_{10}(s)$.

Decomposition Reaction

A reaction type where a single compound breaks down into two or more simpler substances, such as $Hg_2Cl_2(s) \rightarrow Hg(l) + Cl_2(g)$.

Single Displacement Reaction

A reaction where one element takes the place of another element in a compound, such as $Zn(s) + HCl(aq) \rightarrow ZnCl_2(aq) + H_2(g)$.

Double Displacement Reaction

A reaction where two compounds exchange ions to form two new compounds, such as $AgNO_3(aq) + CaCl_2(aq) \rightarrow Ca(NO_3)_2(aq) + AgCl(s)$.

Combustion Reaction

A reaction type where a substance reacts with oxygen, often releasing heat and producing $CO_2$ and $H_2O$, like the combustion of methanol ($2CH_3OH(l) + 3O_2(g) \rightarrow 2CO_2(g) + 4H_2O(l)$).

Molar Mass

The mass in grams of one mole of a substance, such as for $C_6H_{12}O_6$, $N_2O_5$, or $CaCl_2$.

Stoichiometry

The section of chemistry involving calculations of quantities in chemical reactions using balanced equations, such as converting grams of aluminum to grams of aluminum bromide.

Theoretical Yield

The maximum amount of product that can be produced in a chemical reaction from a given amount of reactant, determined through stoichiometric calculations.

Exothermic Reaction

A reaction that releases energy, such as the combustion of methanol which releases $1454\,kJ$ of heat.

Endothermic Reaction

A reaction that absorbs energy from its surroundings.

Specific Heat

The amount of heat energy required to raise the temperature of a substance, calculated using heat ($J$), mass ($g$), and temperature change ($^{\circ}C$).

Calorimeter

An apparatus, such as a Styrofoam cup, used to measure the amount of heat involved in a chemical or physical process.

Orbital Notation

A way of representing the electron configuration of an atom using boxes or lines for orbitals and arrows for electrons in ascending filling order.

Electron Configuration

The distribution of electrons of an atom or molecule in atomic or molecular orbitals, such as for Rubidium, Xenon, or Antimony.

Short Hand Notation

An abbreviated way to write electron configurations using noble gases, applied to elements like Tellurium, Arsenic, and Strontium.

VSEPR Theory

Valence Shell Electron Pair Repulsion theory; a model used to predict the geometry or shape of individual molecules.

Intermolecular Forces (IMF)

The forces of attraction or repulsion which act between neighboring particles (atoms, molecules, or ions).

Polar Bond

A type of chemical bond where a pair of electrons is unequally shared between two atoms.

Non-polar Molecule

A molecule that has no net dipole moment, determined by its shape and the polarity of its bonds.

Kinetic Molecular Theory

A theory that explains the states of matter based on the idea that matter is composed of tiny particles that are always in motion.

STP

Standard Temperature and Pressure, used as a reference point for gas calculations, such as determining that a $3.00\,mol$ sample of hydrogen gas occupies a specific volume.

Molarity

The concentration of a solution expressed as the number of moles of solute per liter of solution.

Dilution

The process of reducing the concentration of a solute in a solution, often by adding more solvent.

Like Dissolves Like

An expression used in solution chemistry to explain the dissolving process based on the similarity of polarities between solute and solvent.

Conjugate Acid/Base Pairs

Two substances related by the loss or gain of a single hydrogen ion ($H^+$), such as $HCN$ and $CN^-$.

pH

A numeric scale used to specify the acidity or basicity of an aqueous solution, where a concentration of $[H_3O^+] = 1.0 \times 10^{-7}$ results in a neutral value of $7$.

pOH

A measure of hydroxide ion ($OH^-$) concentration, related to pH such that their sum equals $14$ in aqueous solutions.

Hydronium Ion

The ion $H_3O^+$, often used interchangeably with $H^+$ to represent the acidity of a solution.

Hydroxide Ion

The diatomic anion with chemical formula $OH^-$.