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  • Topics
    • Lab - Measurement >
      • Measurement Lesson 1
      • Measurement Lesson 2 Scientific Measurements
      • Measurement Lesson 3 Significant Figures
      • Measurement Lesson 4 Units
      • Measurement Lesson 5 Skills
    • 1. Matter & Energy >
      • Matter Lesson 1 Types of Matter
      • Matter Lesson 2 Mixtures and Separation
      • Matter Lesson 3 Properties and Changes
      • Matter Lesson 4 Phases of Matter
      • Energy Lesson 5 Heating and Cooling Curves
      • Energy Lesson 6 Heat Definitions
      • Energy Lesson 7 Calculating Heat
    • 2. Gas laws >
      • Gas Laws Lesson 1 Gas Laws
      • Gas Laws Lesson 2 Combined Gas Law
    • 3. Atomic Theory & Periodic Table >
      • Lesson 1 Atomic Theory
      • Lesson 2 Subatomic Particles
      • Lesson 3 Foundations of PT
      • Lesson 4 Types of Elements
      • Lesson 5 Electrons
      • Lesson 6 Atoms vs Ions
      • Lesson 7 Oxidation Numbers
      • Lesson 8 Electron Dot Diagrams
      • Lesson 9 Isotopes
      • Lesson 10 Periodic Trends
    • 4. Bonding >
      • Bonding Lesson 1 Basics
      • Bonding Lesson 2 Ionic Bonds
      • Bonding Lesson 2b Stock System
      • Bonding Lesson 3 Covalent Bonds
      • Bonding Lesson 3b Naming Covalent Bonds
      • Bonding Lesson 3c Multiple Bonds and Bond Strength
      • Bonding Lesson 4 Metallic Bonds
      • Bonding Lesson 5 Symmetry
      • Bonding Lesson 6 IMF
    • 5. Nuclear >
      • Nuclear Lesson 1 Transmutation
      • Nuclear Lesson 2 Radioisotope Uses
      • Nuclear Lesson 3 Radiation Penetration
      • Nuclear Lesson 4 Artificial Transmutation
      • Nuclear Lesson 5 Half Life
    • 6. Formulas and Equations >
      • Formulas & Equations Lesson 1 Types of Formulas
      • Formulas & Equations Lesson 2 Types of Reactions
      • Formulas & Equations Lesson 3 Balancing Equations
    • Semester 2 >
      • 10. Math & Moles >
        • Math Lesson 1 Mass
        • Math Lesson 2 Percent Composition
        • Math Lesson 3 Avogadro
        • Math Lesson 4 Molecular Formula from Empirical
        • Math Lesson 5 Mole Ratios
      • 11. Solutions >
        • Solutions Lesson 1 Solutions
        • Solutions Lesson 2 Solubility
        • Solutions Lesson 3 Concentration
        • Solutions Lesson 4 Colligative Properties
      • 12. Acids & Bases >
        • Acids and Bases Lesson 1 Properties
        • Acids and Bases Lesson 2 Naming
        • Acids and Bases Lesson 3 Reactions
        • Acids and Bases Lesson 4 pH Scale
        • Acids and Bases Lesson 5 Indicators
      • 13. Kinetics & Equilibrium >
        • Kinetics & Equilibrium Lesson 1 Collision Theory and Factors
        • Kinetics & Equilibrium Lesson 2 PE Diagrams
        • Kinetics & Equilibrium Lesson 3 Equilibrium
        • Kinetics & Equilibrium Lesson 4 LeChateliers Principle
        • Kinetics & Equilibrium Lesson 5 Entropy and Enthalpy
      • 14. Oxidation Reduction >
        • RedOx Lesson 2 RedOx Reactions
        • RedOx Lesson 3 Half Reactions
        • RedOx Lesson 4 Spontaneous Reactions
        • RedOx Lesson 5 Electrochemical Cells
      • 15. Organic >
        • Organic Lesson 1 Intoduction
        • Organic Lesson 2 Hydrocarbons
        • Organic Lesson 3 Functional Groups
        • Organic Lesson 4 Reactions
  • Review Material
    • Textbook Unit Review Sheets
  • NYS Chemistry Curriculum

Matter & Energy

Learning Targets Matter
1.  I can classify matter as either a pure substance (element or compound) or a mixture.
2.  I can differentiate substances as having definite and constant composition while proportions of mixtures may vary.
3.  I can restate the Law of Conservation of Matter to state that matter cannot be created or destroyed – only transferred in a system (whatever is on the left side of the equation must equal what is on the right side of the equation).
4.  I can identify compounds as two or more elements chemically combined that can be broken down (H2O, NH3).
5.  I understand that elements cannot be broken down by ordinary chemical means (Ar, C, Na).
6.  I comprehend that elements, compounds and solutions are homogeneous meaning that the composition is uniform throughout.
7.  I understand that mixtures can also be heterogeneous meaning that the composition is not uniform throughout (ex: salad, chex mix, soil).
8.  I can differentiate between a physical change (when particles are rearranged but still the same H2O(s) and H2O(l) and a chemical change (when particles are rearranged to form new products 2H2(g) + O2(g) = 2(H2O)(l).
9.  I can name phase changes:     
s to l = fusion/melting                           l to s = solidification/freezing
l to g = vaporization/evaporation         g to l = condensation
s to g = sublimation                             g to s = deposition
10. I can identify different ways to physically separate mixtures such as filtration, distillation and chromatography.

Learning Targets Energy
  1. I can define temperature as the average Kinetic Energy in a system.
  2. I can extend that definition to highest temperature = highest KE = fastest moving particles.
  3. I can differentiate between Kinetic Energy (energy of motion) and Potential Energy (stored energy – distance between particles).
  4. I can identify types of energy as: CEMENT (Chemical, Electrical, Mechanical, Electromagnetic, Nuclear, Thermal).
  5. I can comprehend that heat (thermal energy) is always transferred from high temperature to low temperature.
  6. I can restate the Law of Conservation of Energy to state that energy cannot be created or destroyed only transferred in a system (ex: electrical energy can be transferred to thermal energy when a heater is plugged into the wall).
  7. I can use a heating or cooling curve to explain the difference in potential energy and kinetic energy during phase changes.
    1. If the temperature is not changing the KE is not changing, all energy is going into the phase change.
    2. If the temperature is changing the KE is changing which means that the energy is going in to speed up (or slow down) the particles.
    3. ONLY ONE ENERGY CAN MOVE AT A TIME.
  8. I can use the heat formulas to calculate the amount of energy absorbed (endothermic) or released (exothermic) in reaction.
    1. q=mC∆T can be used only if there is a change in temperature (KE is changing)
    2. q=mHf can only be used during the s-l phase changes
    3. q=mHv can only be used during the l-g phase changes
 
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