Final Exam Theory Review: Chemistry Fundamentals

This set of vocabulary flashcards covers essential chemistry concepts including chemical bonding, gas behavior and laws, solution chemistry, stoichiometry, and acid-base theories based on the exam review transcript.

Ionic Bonding

A type of chemical bonding that involves the transfer of electrons from one atom to another, typically between a metal and a non-metal, leading to the formation of positive and negative ions.

Molecular (Covalent) Bonding

A type of chemical bonding characterized by the sharing of electron pairs between atoms, typically occurring between non-metal atoms.

Electronegativity

A measure of the tendency of an atom to attract a bonding pair of electrons within a covalent bond.

Kinetic Molecular Theory (KMT)

A theory describing gas particles as being in constant, random motion, where the kinetic energy of the particles is directly proportional to the temperature.

Boyle’s Law

A gas law stating that the pressure of a given mass of an ideal gas is inversely proportional to its volume at a constant temperature ($P \times V = k$).

Charles Law

A gas law stating that the volume of an ideal gas is directly proportional to its absolute temperature at a constant pressure ($\frac{V}{T} = k$).

Ideal Gas

A hypothetical gas whose molecules occupy negligible space and have no interactions, perfectly following the gas laws under all conditions of temperature and pressure.

Real Gas Behavior

The behavior of gases that most significantly deviates from ideal behavior under conditions of high pressure and low temperature.

Saturated Solution

A solution in which no more solute can be dissolved in the solvent at a specific temperature.

Unsaturated Solution

A solution that contains less than the maximum amount of solute that can be dissolved in the solvent at a given temperature.

Supersaturated Solution

A solution that contains more dissolved solute than is normally possible at a given temperature, often prepared by cooling a saturated solution made at a higher temperature.

Neutralization

A chemical reaction in which an acid and a base react quantitatively with each other to produce water ($H_2O$) and a salt.

Solubility

The maximum amount of a substance that can be dissolved in a given amount of solvent at a specific temperature and pressure.

Balanced Equation

A chemical equation in which the number of atoms for each element in the reaction and the total charge are the same for both the reactants and the products.

Ionic Equation

A chemical equation that shows all the soluble ionic species as dissociated ions.

Net Ionic Equation

A chemical equation that includes only those species participating in the reaction, omitting spectator ions that do not change during the reaction.

Limiting Reactant

The reactant in a chemical reaction that is completely consumed first, thereby determining the maximum amount of product that can be formed.

Excess Reactant

The reactant that remains in the reaction mixture after the limiting reactant is entirely consumed.

Tetrahedral

A VSEPR molecular shape occurring when there are four bonding pairs and zero lone pairs around a central atom, such as in methane ($CH_4$).

Pyramidal

A VSEPR molecular shape occurring when there are three bonding pairs and one lone pair around a central atom, such as in ammonia ($NH_3$).

Arrhenius Theory

A theory defining acids as substances that dissociate in water to produce hydrogen ions ($H^+_{(aq)}$) and bases as substances that produce hydroxide ions ($OH^-_{(aq)}$).

Modified Arrhenius Theory

An updated theory suggesting that acids react with water to produce hydronium ions ($H_3O^+_{(aq)}$) rather than just dissociating.

Monoprotic

A substance, like $HCl$, that is capable of donating or accepting only one proton ($H^+$) per molecule.

Polyprotic

A substance, like $H_2SO_4$ or $H_3PO_4$, that is capable of donating more than one proton ($H^+$) per molecule.

Predicted Yield

The maximum amount of product that can be generated by a chemical reaction based on stoichiometric calculations (also known as theoretical yield).

Experimental Yield

The actual amount of product obtained from a chemical reaction performed in a real-world setting, which is often less than the predicted yield.