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Chemical Reaction
A process in which reactants react chemically and convert into products by chemical transformation. It is also a rearrangement of atoms in which some of the original bonds are broken and new bonds are formed to give different chemical structures.
Reactants
These are the starting substances.
Products
New substances that result from chemical reactions.
Chemical Equation
Shorthand way of describing a reaction.
(s)
symbol for solid in a chemical reaction
(l)
symbol for liquid in a chemical reaction.
(g)
Symbol for gases in a chemical reaction.
(aq)
Symbol for aqueous solution in a chemical reaction.
Law of Conservation of Mass
Total mass of the products of a reaction is equal to the total mass of the reactants.
Antoine Lavoisier
Established the law of conservation of mass.
Same
A balanced chemical equation has the _________ number of each type of atom on the product side and the reactant side.
Synthesis Reaction
Two or more substances combine to for a new compound.
Polymerization
The process of creating large molecules from small ones is called ___________.
Decomposition Reaction
A chemical reaction in which a single compound is broken down to produce two or more smaller compounds.
Single Displacement Reaction
One element replaces a similar element in a compound.
Double Displacement
Ions from two compounds in solution exchange places to produce two new compounds. The compounds formed is usually a precipitate that settles out of the solution.
Precipitate
It is a new solid product that comes out of a solution in a chemical reaction.
Soluble Compounds
These compounds break down when put in water.
Insoluble Compounds
These compounds do NOT break down when put in water.
Surface Area
The more ___________ that is exposed, the faster the reaction will occur.
Temperature
The higher the ________________ the faster the particles move.
Concentration
The amount of substance in a given volume.
Catalyst
Material that increases the rate of reaction by lowering activation energy.
Enzymes
Cells in your body that acts as catalysts.
Inhibitor
material used to decrease the rate of a reaction.
Exothermic
Chemical reactions that emit thermal energy when they occur.
Endothermic
Chemical reactions that absorb thermal energy when they occur.
Enthalpy
The amount of thermal energy emitted or absorbed by a chemical reaction, under conditions of a constant pressure, can be quantified with a function called ____________________.
Enthalpy of reaction
The amount of thermal energy that flows when a reaction occurs at constant pressure.
Stoichiometry
Section of chemistry that involves using relationships between reactants and/or products in a chemical reaction to determine desired quantitative data.
Stoikhein
Greek word meaning “element'“.
Metron
Greek word meaning “pressure”.
Mole
The amount of substance that contains the same number of entities .
Molar Mass
The mass per mol of its entities.
Empirical Formula
Shows the lowest number of moles and gives the relative number of atoms of each element present.
Molecular Formula
Shows the actual number of atoms of each element in a molecule of the compound.
Solution
Homogenous mixture of 2 or more substances evenly distributed throughout a single phase.
Solute
Substance that is dissolved
Solvent
Dissolving Medium
Solubility
The ability of a substance to be dissolved.
Saturation
The solubility of a solute in a solvent relative to the amount used.
Unsaturated
Contains less solute than the maximum amount of solute a solvent can design.
Saturated
Contains equal amount of solute to the maximum amount of solute a solvent can dissolve.
Supersaturated
Contains more solute than the maximum amount of solute a solvent can dissolve.
Concentration
The amount of solute dissolved in a given amount of solvent.
Dilute Solution
Has relatively low concentration.
Concentrated Solution
Has relatively high concentration.
Parts per million
The number of grams of solute in a million grams of solution. This is used when the solution is very dilute.
Molarity
The number of moles so solute per liter of solution
Molality
The number of moles so solute per kilogram of solvent.
Mixture
a substance made by combining two or more different materials in such a way that no chemical reaction occurs.
Suspension
A heterogenous mixture containing solid particles that are sufficiently large for sedimentation.
Colloid
A homogenous solution with intermediate particle size between a solution and a suspension.
Aqueous
Describes a solution in which the solvent is water.
Filtration
can be used to separate a solid from a liquid.
Evaporation
Can be used to separate a dissolved solute from a solution.
Distillation
is a method of separating chemical substances based on differences in their volatilities in a boiling liquid mixture.
Chromatography
a physical method of separation in which the components to be separated are distributed between two phases.
Polar solvents
Dissolve polar compounds
Nonpolar solvents
Dissolve nonpolar compounds
Miscible
Indicates that liquids will dissolve each other
Immiscible
Indicates that liquids will not dissolve appreciably each other.
Conductivity
is a measure of water’s ability to conduct electrical current.
Electrical Conductivity
is a measure of a material’s ability to conduct an electric current.
Electrolytes
are substances that become ions in solution and acquire the capacity to conduct electricity.
Non electrolyte
a substance that does not dissociate into ions and so in a solution it is a nonconductor of electricity.
Dissociation
A process in which a compound separated intro fragments.
Hydration
The process by which water molecules surround each ions as it moves into solution.
Polarity
Indicates that a solute will dissolve best in a solvent that has a similar _______________ to itself.
Colligative Properties
These are properties that depend upon the concentration of solute molecules or ions, but not upon the identity if the solute.
Emulsion
is a mixture of two immiscible substances. One substance is dispersed in the other.
Emulsification
is the process which emulsions are prepared.
Acid
is a solution with an excess of H+ ions. These substances taste sour.
Base
A solution that has an excess of OH- ions. These substances taste bitter.
Alkali
Another word for bases.
Neutralization
A reaction between an acid an a base.
pH
measures how acidic or basic a solution is.
Acidic Solutions
have pH values below 7
Neutral solution
a solution with a pH of 7
Basic Solution
a solution with pH values above 7.
Force
Holds particles together.
Intermolecular force
the attractions between molecules
Intramolecular force
is the force that keep a molecule together.
Kinetic Energy
Particles can move apart only if they have enough _____________ to overcome this force of attraction.
Atmospheric pressure
The gas molecules in the atmosphere are pulled toward due to gravity exerting pressure.
Barometer
measures atmospheric pressure.
Standard Atmospheric Pressure
SAP
Standard Temperature and Pressure
STP
Boyle’s Law
The pressure and volume of gas are inversely proportional ( as one increases the other decreases.)
Charles’ Law
The volume and absolute temperature of a gas are directly proportional.
Gay-Lussac’s Law
The pressure and absolute temperature (K) of a gas are directly proportional ( as temperature rises, so does pressure.)
22.4
constant value of mol in gases.
