Chemistry Study Guide: Rates of Chemical Reactions – Vocabulary Flashcards

A vocabulary set covering key terms from the lecture notes on rates of chemical reactions and related chemistry concepts.

Law of Conservation of Mass

Mass cannot be created or destroyed during a chemical reaction; the total mass of reactants equals the total mass of products.

Balanced Equation

An equation in which the number of atoms of each element is the same on both sides, reflecting conservation of mass.

Word Equation

A chemical equation written using chemical names in words (e.g., Sodium hydroxide + hydrochloric acid → sodium chloride + water).

Combination (Synthesis) Reaction

Two or more reactants combine to form one product; pattern A + B → AB (e.g., 2Ca + O2 → 2CaO).

Decomposition Reaction

A single compound breaks down into two or more products; pattern AB → A + B (e.g., BaCO3 → BaO + CO2).

Oxidation

Loss of electrons; historically also described as a substance reacting with oxygen.

Reduction

Gain of electrons; oxidation state decreases (often described as the opposite of oxidation).

OILRIG

Mnemonic: Oxidation Is Loss (of electrons); Reduction Is Gain (of electrons).

Redox Reaction

A reaction involving transfer of electrons between species, encompassing both oxidation and reduction.

Metal Displacement Reaction

A single redox reaction where a more reactive metal displaces a less reactive metal from solution.

Metal Activity Series

A ranking of metals by reactivity; helps predict which metals can displace others and which can be reduced.

Carbon Reduction (Smelting)

Extraction of metals from metal oxides using carbon; example: Fe2O3 + 3CO → 2Fe + 3CO2.

Precipitation Reaction

Two soluble ionic solutions mix to form an insoluble solid (precipitate).

Acid

Substance that releases H+ ions in water; typically has pH < 7 and conducts electricity.

Base

Substance that releases OH- ions in water; typically has pH > 7 and conducts electricity; alkali if soluble.

pH Scale

A scale from 0 to 14 measuring acidity/basicity; 7 is neutral;

Neutralization

An acid reacts with a base to form a salt and water.

Acid + Metal Reaction

Acid reacts with a metal to produce a salt and hydrogen gas.

Acid + Metal Hydroxide Reaction

Acid reacts with a metal hydroxide to produce a salt and water.

Acid + Metal Oxide Reaction

Acid reacts with a metal oxide to produce a salt and water.

Acid + Metal Carbonate Reaction

Acid reacts with a metal carbonate to produce a salt, water, and carbon dioxide.

Acid + Metal Hydrogen Carbonate Reaction

Acid reacts with a metal hydrogen carbonate to produce a salt, water, and carbon dioxide.

Rate of Reaction

The speed at which a chemical reaction occurs.

Temperature (Rate Factor)

Raising temperature generally increases reaction rate by giving particles more energy.

Concentration (Rate Factor)

Higher concentration typically increases rate due to more frequent particle collisions.

Surface Area (Rate Factor)

Larger surface area increases rate by exposing more area for reaction.

Agitation (Rate Factor)

Stirring or mixing raises collision frequency and reaction rate.

Catalyst

A substance that increases reaction rate by lowering the activation energy and is not consumed.

Hydrolysis

Reaction with water that breaks bonds in a molecule; used in processes like detoxifying certain compounds.

Calcination

Heating a substance to drive a chemical change or change its composition (often to remove water or drive off CO2).

Fermentation

Microbes convert sugars to ethanol and CO2; used in production of alcoholic beverages.

Pyrolysis

High-temperature decomposition of materials in the absence of oxygen.

Combustion

Fuel reacts with oxygen to produce heat and light; common in torches, engines, and fires.

Hydrocarbon

An organic compound composed mainly of hydrogen and carbon.

Hydrocarbon Combustion

Combustion of a hydrocarbon with oxygen to form CO2 and H2O.