Unit 1:

• A chemical reaction is the rearrangement of atoms due to the formation and breaking of chemical bonds.
• The fact that atoms are conserved, together with knowledge of the chemical properties of the elements involved, can be used to describe and predict chemical reactions.
• Balance Chemical Equations
• Calculate the mass of any component of a reaction, given any other component
• Using molar mass in a balanced equation, support the claim that atoms and therefore mass, are conserved during a chemical reaction
• Given the reactants of a chemical reaction, students can predict the products of five basic reaction types (synthesis, decomposition, single replacement, double replacement, and combustion)

Unit 2:

• When energy transfers into the system, the process is endothermic
• When energy transfers out of a system, the process is exothermic
• Phase changes are endothermic when enough energy is absorbed to overcome the IMFA between particles (i.e.,melting, vaporization).
• Phase changes are exothermic when enough energy is released and IMFA between particles strengthen (ie freezing, condensation).
• As a substance heats up or cools down (prior to a phase change), the particles are changing KE.
• During the phase change, KE remains the same and PE changes as IMFAs are overcome/strengthened.
• Heating/Cooling Curves and Phase Diagrams are useful models to represent phases and phase change
• Energy flows from warm to cold until both substances reach thermochemical equilibrium (rate of particle motion (kinetic energy) is equal)
• Conservation of energy means that the total change of energy in any system is always equal to the total energy transferred into or out of the system
• Kinetic Molecular Theory provides a model for the behavior of gas particles
• The amount of energy released by a system is absorbed by the surroundings (q = -q).
• Energy cannot be created or destroyed, but it can be transported from one place to another and transferred between systems

Unit 3:

• Water has a high specific heat capacity.
• Water is a polar molecule that has strong electrostatic attractions which form strong hydrogen bonds.  These bonds give water unique properties (such as expansion upon freezing and formation of cages to dissolve like solutes).
• Mechanical (such as abrasion, glacial, crushing, dissolving, frost wedging) and chemical (chemical reactions such as the formation of iron oxides) weathering are two important processes that break down rock
• Water transports materials (erosion) and is responsible for the formation of the Great Lakes and the Grand Canyon.
• Model the chemical attributes of a solution, including the recognition of solute and solvent, and the understanding of what it takes for two things to dissolve in one another (like dissolves like).
• Explain water’s exceptional ability as a solvent and the limitations to this ability (it’s inability to dissolve nonpolar molecules, saturation).
• Explain how the freezing and boiling point of an aqueous solution compares to that of pure water.  This has practical applications in the treatment of ice on the roads.
• As temperature increases, the solubility of gases decreases.  This inverse relationship is due to the effects of temperature on the behavior of gases (KMT).
• Using the knowledge and understandings from the above DCI…
  • Model the formation of potholes

Unit 4:

• Three things must be true for a chemical reaction to occur (collision theory):
  • Atoms/molecules must collide in order to react
  • When they collide, they must have enough energy to react
  • Molecules must collide in the proper orientation
• The rate of a chemical reaction can be affected by temperature, surface area/particle size, concentration, and the presence/absence of a catalyst
• Energy is neither created nor destroyed, it can only change form
• When energy is released from a system, it is released in the form of light, heat, and/or sound
• In chemical reactions, it requires energy to break a chemical bond
• In chemical reactions, energy is released when new chemical bonds are formed
• Endothermic and exothermic potential energy graphs represent the change in enthalpy within a system during a chemical reaction.  This represents the change in bond energy during a reaction.
• In chemical reactions, matter is neither created nor destroyed, it is only rearranged
• Label the parts of a chemical reaction (reactants, products)
• Model energy changes in a chemical reaction (endothermic and exothermic potential energy diagrams)In a chemical system, energy is transferred via particle collisions
• Chemical reactions can move in both directions (forward and reverse)
• Equilibrium is reached when the forward reaction and the reverse reactions are occurring at the same rate
• The concentration of reactants and products is not necessarily equal at equilibrium.  At equilibrium, some reactions will produce more products than reactants and some reactions will produce more reactants than products.
• Solid and liquid reactants and products do not affect equilibrium, only aqueous solutions and gases impact the reaction rate.
• If a condition changes (concentration, temperature, volume/pressure), the reaction direction will shift until equilibrium is reestablished (le chatelier's principle)
• Predict what will happen to  chemical equilibrium in a system when a condition is changed

Unit 5:

• pH is a scale used to measure/indicate of the strength of an acid and represents the concentration of hydrogen ions in solution.
• Recognizing simple acid/base reactions using Bronsted Lowry definitions (donation of H+ makes something an acid. Accepting a H+ makes something a base)
• Acids and bases react together to form water and a neutral salt.
• The strength of an acid or a base depends on the level of dissociation in solution
• Using the knowledge and understandings from the above DCI…
  • Model the positive feedback mechanisms of decreasing gas solubility as the atmosphere warms