Lab Final Chemistry Flashcards

Vocabulary practice flashcards covering colligative properties, kinetics, chemical equilibrium, titrations, redox/electrochemistry, and basic organic terminology from the chemistry lab final study outline.

Colligative Properties

Properties of solutions that depend on the number of dissolved solute particles, not the identity of the solute.

Vapor Pressure

The pressure produced by vapor above a liquid at equilibrium.

Boiling Point

The temperature at which the vapor pressure of a liquid equals atmospheric pressure.

Boiling-Point Elevation Equation

$$\Delta T_b = i K_b m$$

Freezing-Point Depression Equation

$$\Delta T_f = i K_f m$$

van 't Hoff Factor ($i$)

The number of dissolved particles produced per formula unit of solute.

Molality ($m$)

The concentration unit used in colligative-property equations representing moles of solute per kilogram of solvent.

Osmosis

movement of solvent through semipermeable membrane, less concentrated solution to more concentrated solution

Semipermeable Membrane

A membrane that allows certain particles, usually solvent molecules, to pass while restricting others.

Osmotic Pressure

The pressure required to stop osmosis, given by the equation $\Pi = iMRT$.

Reaction Rate

How quickly reactants disappear or products form in a chemical reaction.

Catalyst

A substance that lowers activation energy and increases reaction rate without being consumed.

Kinetics

The branch of chemistry describing how fast a reaction occurs.

Thermodynamics

The branch of chemistry describing whether a reaction is energetically favorable or spontaneous.

Rate Law

The general equation describing reaction rate as $\text{Rate} = k[A]^m[B]^n$.

Rate Constant ($k$)

The proportionality constant in the rate law equation.

Reaction Orders ($m$ and $n$)

Exponents in the rate law determined experimentally that indicate the dependence of reaction rate on reactant concentrations.

Dynamic Equilibrium

A state in which forward and reverse reactions continue occurring at equal rates.

Reaction Quotient ($Q$)

The value describing the product-to-reactant ratio at any point in time using the equilibrium constant expression.

Le Chatelier's Principle

The principle stating that when an equilibrium system is disturbed, it shifts in the direction that opposes the disturbance.

Equivalence Point

The point in a titration where reactants have reacted in their exact stoichiometric ratio.

Endpoint

The point in a titration where the indicator changes color.

EDTA

A compound that binds metal ions such as $Ca^{2+}$ and $Mg^{2+}$ in a $1:1$ mole ratio.

Water Hardness

presence of dissolved Ca and Mg ions, ppm units, CaCO₃

Oxidation

The loss of electrons, resulting in an increase in oxidation number.

Reduction

The gain of electrons, resulting in a decrease in oxidation number.

Reducing Agent

The reactant that donates electrons and becomes oxidized.

Oxidizing Agent

The reactant that accepts electrons and becomes reduced.

Activity Series

A scale ranking metals by their tendency to lose electrons and undergo oxidation.

Anode

The electrode in an electrochemical cell where oxidation occurs.

Cathode

The electrode in an electrochemical cell where reduction occurs.

Salt Bridge

A cell component that carries ions between half-cells to maintain electrical neutrality and complete the circuit.

Standard Cell Potential Equation

$$E^\circ_{\text{cell}} = E^\circ_{\text{cathode}} - E^\circ_{\text{anode}}$$

Single-Displacement Reaction

A reaction of the general form $A + BC \rightarrow AC + B$ where one element replaces another in a compound.

Double-Displacement Reaction

A reaction of the general form $AB + CD \rightarrow AD + CB$ where two ionic compounds exchange partners.

Structural Isomers

Compounds with the same molecular formula but different connectivity of atoms.

Chain Isomers

Structural isomers with the same molecular formula but a different carbon skeleton.

Positional Isomers

Structural isomers with the same molecular formula, carbon skeleton, and functional group, but with the group in a different location.

Functional Isomers

Structural isomers with the same molecular formula but different functional groups.