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Atomic mass unit
A unit of mass to express atomic + molecular weights
Law of conservation of mass
States that the mass of all substances present before a chemical change equals the mass of all the substances remaining after the change
Formula mass
The sum of the atomic weights of the atoms in the empirical formula of the compound
Stoichiometry
The relationship between the relative quantities of substances taking part in a reaction or forming a compound, typically a ratio of whole integers
Base
A substance that produces hydroxide ions (OH-) when dissolved in a water solution
Neutralization
Chemical reaction that occurs when the H3O+ ions from an acid react with the OH- ions from a base to produce water molecules and a salt
Avogadro’s number
The number of atoms/molecules in one mole, equal to 6.023 x 10^23
Endothermic
Chemical reaction that requires thermal energy in order to proceed
Products
In a chemical reaction, the new substance or substances formed
Acid
A substance that produces hydrogen ions in a water solution
Hydronium ion
H3O+ ion, forms when an acid dissolves in water and H+ ions interact with water
pH
A measure of the concentration of the hydronium ions in a solution using a scale ranging from 0 to 14 being the most basic
Chemical equation
Shorthand method used to describe chemical formulas and other symbols
Exothermic
Chemical reaction in which energy is primarily given off in the form of thermal energy
Reactants
In a substance, the substance that reacts
Acid base reaction
A solution that has a high concentration of Hydrogen ions (H+) greater than the concentration of water
Neutral solution
A solution that is neither acidic or basic, it has equal amounts of Hydrogen ions (H+) and Hydroxide (OH-)
Salt
Compound formed when negative ions from an acid combine with positive ions from a base
Note 
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