Chemistry Exam Review

Flashcards for reviewing key vocabulary and concepts for the upcoming chemistry exam.

Synthesis Reaction

A reaction where two different things combine to become one.

Decomposition Reaction

A reaction where there is only one reactant, the only thing that can happen is for it to break apart.

Double Replacement Reaction

A compound plus a compound gives you two different compounds; positive ions swap.

Combustion Reaction

A reaction that always involves a substance burning in oxygen, yielding carbon dioxide and water.

Surface Area

The smaller the particle size, the greater the surface area, the faster the reaction rate.

Temperature's Effect on Reaction Rate

The higher the temperature, the faster the reaction due to increased kinetic energy and particle collisions.

Concentration's Effect on Reaction Rate

The higher the concentration, the faster the reaction rate; more particles in the solution lead to more collisions.

Catalyst

A substance that speeds up the reaction rate by lowering the activation energy; it isn't changed by the reaction.

Pressure's Effect on Reaction Rate

Only involved in gases; the higher the pressure, the faster the reaction rate due to smaller volume and more particle collisions.

Acids

Compounds that break up in water to give off H+ ions.

Bases

Compounds that accept electron pairs (or H+ ions).

pH

A measurement of the hydrogen ion concentration; less than seven is an acid, greater than seven is a base, and seven is neutral.

Acidic pH

The lower the pH (less than 7), the substance is acidic

Basic pH

The higher the pH (greater than 7), the substance is basic.

Salt

Any positive and negative ion that forms a compound (not just sodium chloride).

Exergonic Reactions

Chemical reactions that release energy.

Exothermic Reactions

Chemical reactions that release energy in the form of heat.

Endergonic Reactions

Chemical reactions that absorb energy.

Endothermic Reactions

Chemical reactions that absorb energy in the form of heat.