students took the second test of the 4th marking period.
Neutralization reaction
a reaction in which an acid reacts with a base to form an water and a salt
titration
addition of a known amount of solution of a known concentration to determine the concentration of an unknown salt
May 28, 2014
Students reviewed for test and performed an equilibrium lab
May 23, 2014
Rate of reaction the change in concentration of reaction or product per unit time
Collision Theory In order for atoms, ions or molecules to react they must: a) collide b) collide with the proper orientation c) collide with the minimun activation energy
Factors that affect reaction rate
a) nature of the reactants b) concentration c) surface area d) temperature e) catalyst or inhibitor
catalyst a substance that accelerates the rate of a chemical reaction by lowering the activation energy of the reaction. A catalyst does not change the enthalpy of reaction.
Enthalpy (H) heat content of a system at constant pressure
activation energy
the minimum energy colliding particles must have in order to react
reversible reaction a chemical reaction that can occur in both the forward and reverse directions
Chemical equilibrium state at which the forward reaction is equal to the reverse reaction
Equilibrium postiion The concentrations of the reactants and products at equilibrium
At a given temperature a chemical system will reach a state in which a specific ratio of the reactants and products is a constant.
Equilibrium constant The ratio of the product concentration to the reactant concentration raised to the power of the moles of the substance from a balanced chemcial equation.
Factors that affect chemical equilibrium
Le Chatelier's Principle If a stess is applied to a system at equilibrium, the system shifts in the direction that relieves the stress
Changes in concentration a) Adding reactant causes the reaction to shift to the right b) Adding product causes the reaction to shift to the left c) Removing reactant causes the reaction to shift to the left d) Removing product causes the reaction to shift to the right
Changes in pressure (only affects gaseous reactions) a) increases the pressure causes the raction to shift in the direction of less moles. b) decreasing the pressure causes the reaction to shift in the direction of more moles.
Changes in temperature a) increasing the temperature of an exothermic reaction causes the reaction to shift to the left b) increasing the temperature of an endothermic reaction causes the reaction to shift to the right c) decreasing the temperature of an exothermic reaction causes the reaction to shift to the right d) decreasing the temperature of an endothermic reaction causes the reaction to shift to the left
May 15, 2014
calorimeter
a device used to measure heat change
Energy the ability to do work or produce heat
Thermochemistry The study of heat changes that accompany chemical reactions and phase changes
exothermic a reaction or process in which heat is released by the system
endothermic a reaction or process in which heat is absorbed by the system
Law of conservation of energy energy can neither be created or destroyed in ordinary chemical or physical processes.
Universe = system + surrounds
Potential energy
the energy an object has due to it's position or makeup
Chemical potential energy energy stored within the bonds of chemical compounds.
kinetic energy
the energy an object has because of it's motion
Heat (q) energy that flows from a warmer substance to a cooler substance
Temperature
a measure of the kinetic energy of the molecules (how fast they are moving)
calories (cal) the quantity of heat that raises the temperature of one gram of water one degree celsius.
joule(j) unit of energy.
4.18 joules equal one calorie.
specific heat the amount of heat needed to raise one gram of a specific substance by one degree Celsius.
Formula for calculating heat energy that is released or absorbed by a system
Q=mC t
May 9, 2014
Electrolyte compounds that conduct an electric current when dissolved in water or melted.
nonElectrolyte compounds that do not conduct an electric current when dissolved in water or melted.
strong electrolyte compounds that dissociate near 100% when dissolved in water.
weak electrolyte compounds that dissociate near only partially when dissolved in water.
spectator ions ions that do not participate in the chemical reaction
complete ionic equation an equation for a reaction in solution showing all the ions
Net ionic equation an equation for a reaction in solution showing only the particles that are involved in the chemical change.
May 5, 2014
Reviewed for test
complete a freezing point depression lab.
May 1, 2014
Colligative properties physical properties of solutions that depend only on the number of dissolved particles.
Vapor pressure lowering adding a solute to a solvent lowers the solvents vapor pressure.
Boiling point elevation adding a solute to a solvent will raise the boiling point
Freezing point depression adding a solute to a solvent will decrease the freezing point
complete ionic equation
an equation for a reaction in solution showing all the ions
Net ionic equation
an equation for a reaction in solution showing only the particles that are involved in the chemical change.
May 28, 2013
Complete ionic equation An equation that shows all the particles in solution as they exist
Net ionic equation
An equation that includes only the particles that participate in the reaction
Spectator ions Ions that do not participate in the reaction
May 23,2013
students completed an acid -base titration lab
May 17, 19 2013
Strong acids or bases dissociate completely
Weak acids or bases dissociate only partially
Ka The measure of the degree of dissociation of a weak acid
Kb The measure of the degree of dissociation of a weak acid
Bronsted-Lowery an acid is a hydogen ion donor a base is a hydrogen ion accepter
monoprotic an acid that can donate only one hydrogen ion
polyprotic an acid that can donate more than one hydrogen ion.
Neutralization reaction a reaction in which an acid reacts with a base to form a salt (ionic compound) and water.
Titration a method of determining the concentration of a solution by reacting a know volume of that solution with a solution of known concentration (the titrant)
equivalence point point at which the moles of hydrogen ion equal the moles of hydroxide ion.
end point point at which the indicater used in a titration changes colors
May 15, 2013
Students completed the acid base lab they started on monday. They used the remainder of the period to answer the questions on the lab packet with their lab partner.
May 13,2013
Acidic solution A solution that contains more hydrogen ions (H+)than hydroxide ions(OH-)
Basic Solution A solution that contains more hydroxide ions than hydrogen ions.
Kw The ion product for water
May 9, 2013
Students took the first test of the 4th marking period
May 3, 2013
Solubility product constant (Ksp) The equilibrium constant for the dissolving of a slightly soluble compound
Acidic solution A solution that contains more hydrogen ions than hydroxide ions
Basic Solution A solution that contains more hydroxide ions than hydrogen ions.
May 1, 2013
Factors that affect chemical equilibrium
Le Chatelier's Principle If a stess is applied to a system at equilibrium, the system shifts in the direction that relieves the stress
Changes in concentration a) Adding reactant causes the reaction to shift to the right b) Adding product causes the reaction to shift to the left c) Removing reactant causes the reaction to shift to the left d) Removing product causes the reaction to shift to the right
Changes in pressure (only affects gaseous reactions) a) increases the pressure causes the raction to shift in the direction of less moles. b) decreasing the pressure causes the reaction to shift in the direction of more moles.
Changes in temperature a) increasing the temperature of an exothermic reaction causes the reaction to shift to the left b) increasing the temperature of an endothermic reaction causes the reaction to shift to the right c) decreasing the temperature of an exothermic reaction causes the reaction to shift to the right d) decreasing the temperature of an endothermic reaction causes the reaction to shift to the left
Solubility product constant (Ksp) The equilibrium constant for the dissolving of a slightly soluble compound