Chemical Reactions Test Review

Chemical Reaction

Consists or reactants and products; it is the process that involves rearrangement of molecular or ionic structures

Law of Conservation of Mass

Mass can niether be created nor destroyed

Reactants

A substance that takes part in the change of a chemical reaction; before the arrow

Products

The result of a chemical reaction after a change has occurred; after the arrow

Chemical Equation

a representation of a chemical reaction; the formulas of the reactants (on the left) are connected by an arrow with the formulas of the products (on the right).

Balanced Chemical Equation

each side of the equation has the same number of atoms of each element and mass is conserved.

Chemical Potential Energy

The energy stored in the chemical bonds of a substance

Law of Conservation of Energy

The total energy of an isolated system remains constant; energy can neither be created nor destroyed

Endothermic Reaction

When more energy is required to break bonds than is released in the formation of new bonds, energy will need to be absorbed from the surroundings.

Exothermic Reaction

When more energy is released during the formation of new bonds than required for breaking bonds, the net energy will be released to the surroundings.

Activation Energy

The minimum quantity of energy which the reacting species must possess in order to undergo a specified reaction

Collision Theory

To take place the particles have to collide with each other. Particles must have enough kinetic energy to break bonds.

How does temperature affects the collision rate?

An increase of temperature typically increases the rate of reaction. An increase of temperature will raise the average kinetic energy.

Synthesis Reaction

A chemical reaction in which two or more substances produce one product

Combustion Reaction

Oxygen combines with a substance (CxHx) and releases energy in the form of heat and light.

Decomposition Reaction

One reactant breaks down into two or more substances

Single Replacement

One element replaces the atoms of another element in a compound

Double Replacement

Ions exchange between two compounds; happens when dissolved in water

Types of decomposition reactions

Binary Compounds (AB→A+B); Carbonates (XCO3→XO+CO2); Chlorates (XClO3→XCl+O2); Hydroxides (XOH→XO+H2O)

Activity Series

A list of elements in decreasing order of their reactivity.

Precipitate

A substance that is in solid form after the change of a chemical reaction

Aqueous Solution

Contains one or more dissolved substances in water

Solvent

The most plentiful substance in a
solution.

Dissociation

When ionic compounds dissolve in water, their ions
separate

Complete Ionic Equation

Ionic equations that show all the particles in a solution as they actually exist

Net Ionic Equations

Ionic equations that show only the particles that participate in the formation of a precipitate, a gas or water

Solute Interactions

Intermolecular attractions between solute particles

Solvent Interactions

Intermolecular attractions between solvent particles

Solute-Solvent Interactions

Intermolecular attractions between a solute particle and a solvent particle