Honors Chemistry Final Review

Physical Properties

Characteristics of a substance that can be observed or measured without changing its identity.

Intensive Properties

Properties that do not depend on the amount of substance present (e.g., density, boiling point).

Extensive Properties

Properties that depend on the amount of substance present (e.g., mass, volume).

Chemical Properties

Characteristics of a substance that describe its ability to change into different substances.

Chemical Changes

Changes that result in the formation of new chemical substances.

Physical Changes

Changes that affect one or more physical properties but do not change the substance's chemical identity.

Types of Reactions

Different classifications of chemical reactions, including synthesis, decomposition, and combustion.

Predicting Products

The process of determining the products of a given chemical reaction based on reactants.

Writing Chemical Equations

The method of representing a chemical reaction using symbols and formulas.

Reactants

Substances that undergo a chemical change in a reaction.

Products

Substances formed as a result of a chemical reaction.

Symbols in Chemistry

Notation that represents elements, compounds, and reactions (e.g., H for hydrogen, O for oxygen).

Balancing Chemical Equations

The process of ensuring that the number of atoms of each element is the same on both sides of a chemical equation.

Stoichiometry

The calculation of reactants and products in chemical reactions.

Mole Ratio

The ratio of moles of one substance to moles of another substance in a balanced equation.

Limiting Reagents

The reactant that is completely consumed in a reaction, limiting the amount of product that can be formed.

Percent Yield

The ratio of the actual yield to the theoretical yield, expressed as a percentage.

Kinetic Theory

Theory that explains the behavior of gases in terms of particles in motion.

Phases of Matter

The different states in which matter can exist, including solid, liquid, gas, and plasma.

Phase Changes

Transitions between the different states of matter.

Specific Heat

The amount of heat required to raise the temperature of a unit mass of a substance by one degree Celsius.

Heat of Fusion

The amount of energy required to change a substance from solid to liquid at its melting point.

Heat of Vaporization

The amount of energy required to change a substance from liquid to gas at its boiling point.

Enthalpy

A measure of the total energy of a thermodynamic system.

Entropy

A measure of the disorder or randomness in a system.

Gibb’s Free Energy

The energy associated with a chemical reaction that can be used to do work.

Hess’ Law

The total enthalpy change for a reaction is the sum of the enthalpy changes for each step of the reaction.

Exothermic Reaction

A reaction that releases energy in the form of heat.

Endothermic Reaction

A reaction that absorbs energy from the surroundings.

Activation Energy

The minimum energy required for a reaction to occur.

Catalyst

A substance that increases the rate of a chemical reaction without being consumed.

Gas Laws

Equations that describe the behavior of gases in relation to pressure, volume, and temperature.

Boyle’s Law

States that pressure and volume are inversely related when temperature is held constant.

Charles’ Law

States that the volume of a gas is directly proportional to its temperature when pressure is held constant.

Ideal Gas Law

An equation of state for a gas that relates pressure, volume, temperature, and number of moles: $PV=nRT$.

Solutions

Homogeneous mixtures of two or more substances.

Solute

The substance that is dissolved in a solution.

Solvent

The substance in which the solute is dissolved.

Colloid

A mixture in which one substance of microscopically dispersed insoluble particles is suspended throughout another substance.

Electrolyte

A substance that dissociates into ions in solution and conducts electricity.

Dissociation

The process by which an ionic compound separates into its ions in solution.

Suspension

A heterogeneous mixture in which solute-like particles settle out of a solvent-like phase.

Precipitate

A solid that forms from a solution during a chemical reaction.

Solubility

The ability of a substance to dissolve in a solvent.

Saturated Solution

A solution that cannot dissolve any more solute at a given temperature.

Unsaturated Solution

A solution that can dissolve more solute at a given temperature.

Molarity

A measure of concentration defined as moles of solute per liter of solution.

Molality

A measure of concentration defined as moles of solute per kilogram of solvent.

Determining Precipitates

The process of predicting the formation of a solid when two solutions are mixed.

Net Ionic Equations

Equations that show only the particles that participate in a reaction.

Redox Reactions

Reactions involving the transfer of electrons between two species.

Reduction

The gain of electrons or decrease in oxidation state by a substance.

Oxidation

The loss of electrons or increase in oxidation state by a substance.

Oxidation States

The hypothetical charges that atoms would have if all bonds were purely ionic.

Half Reactions

Reactions that show either the oxidation or reduction process separately.

Balancing Redox Reactions

The process of ensuring that the number of electrons lost equals the number of electrons gained.

Acids

Substances that donate protons (H+) in a chemical reaction.

Bases

Substances that accept protons or donate hydroxide ions (OH-) in a chemical reaction.

Neutralization Reaction

A reaction between an acid and a base that produces salt and water.

pH

A measure of the acidity or basicity of a solution.

Titration

A technique used to determine the concentration of a solution by reacting it with a standard solution.

Polyprotic Acids

Acids that can donate more than one proton per molecule.

Significant Figures

The number of meaningful digits in a measurement.

Criss Cross Method

A method used to write the formulas of ionic compounds.

Ionic Compounds

Compounds composed of ions held together by ionic bonds.

Covalent Compounds

Compounds formed by the sharing of electrons between atoms.

Balancing Chemical Reactions

Ensuring that the same number of each type of atom appears in both the reactants and products.

what is the specific heat of ice

2.05 J/g·°C

what is the spicific heat of whater

4.18 J/g·°C

what is the spesifc heat of whater vaper

2.01 J/g·°C

mole fraction equation

mole present equation

molarity equation

molarity equation

Gibs free energy eqation

$${G}={H}-{S}T$$