Chemistry Lecture Notes on Balancing Equations and Reactions

Flashcards covering significant chemical concepts and reactions such as balancing equations, precipitation reactions, and yields.

Balancing Equations

The process of ensuring the number of atoms for each element in reactants is equal to that in products.

Decomposition of Water

A reaction where water (H2O) breaks down into hydrogen (H2) and oxygen (O2).

Precipitation Reaction

A type of reaction resulting in the formation of an insoluble solid, or precipitate, when two aqueous solutions react.

Limiting Reactant

The reactant that is completely consumed in a chemical reaction, limiting the amount of products formed.

Strong Acid

An acid that completely dissociates in water, releasing all of its hydrogen ions.

Weak Acid

An acid that partially dissociates in water, releasing only some of its hydrogen ions.

Neutralization Reaction

A reaction between an acid and a base resulting in the formation of water and a salt.

Oxidation

The loss of electrons or an increase in oxidation state by a molecule, atom, or ion.

Reduction

The gain of electrons or a decrease in oxidation state by a molecule, atom, or ion.

Percent Yield

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

Combustion Analysis

A method for determining the composition of a compound by burning it in oxygen and analyzing the resulting gases.

Titration

An analytical technique used to determine the concentration of a solute in a solution by adding a titrant of known concentration.

Solubility Table

A table that shows the solubility of various compounds in water, typically used to predict the formation of precipitates.

Hydroxide Ion (OH-)

A diatomic ion consisting of oxygen and hydrogen, commonly produced by bases in aqueous solutions.

Molarity (M)

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