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Chemistry
Apply the Laws of Conservation of Matter and Energy to what is observed and
measured in this course.
Individual Unit Priority Standards
1. Observation of Matter and Lab Skills
A. Accurately observe and quantify matter. (SCLE 7A, B, C)
1. Use quantitative and qualitative data as support for reasonable
explanations. (MOCLE 7C)
2. Use volume, mass, density, time, and temperature appropriately with
correct units. (MOCLE 7B)
3. Express a quantity in various units using metric prefixes and dimensional
analysis.
4. Determine the most appropriate instrument(s) to observe the length, area,
volume, mass, density, time, and temperature of a sample (ex. buret)
(MOCLE 7B)
5. Record a measurement to the correct number of significant figures (one
estimated digit), based on the measuring device used. (MOCLE 7B)
6. Calculate a quantity and round answer appropriately using significant
figures.
B. Conduct and communicate the procedures and results of a scientific
investigation to observe the nature of matter. (SCLE 7A, B, C)
1. Construct and/or interpret an appropriate graphical representation of
experimental data. (MOCLE 1.D.a)
2. Analyze experimental data to determine patterns & relationships. (MOCLE
7.1.C.b)
3. Analyze whether evidence (data) and scientific principles support proposed
explanations. (MOCLE 7.1.C.d)
4. Identify the possible effects of errors in observations, measurements, and
calculations, on the validity and reliability of data and resultant explanations
(conclusions). (MOCLE 7.1.C.c)
2. History and Structure of the Atom
A. Describe the structure of an atom and/or ion (proton, electron, and neutron).
1. Calculate the number of protons, neutrons and electrons, given the
mass number and atomic number. (MOCLE 1.1.E.a, b & c)
2. Calculate average atomic mass.
3. Represent an element using nuclear notation.
B. Examine the development and structure of the 20th Century atomic model.
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1. Identify and describe how explanations of the model of the atom have
changed over time as a result of new evidence. (MOCLE 8.1.B.a;
MOCLE 1.1.E.a; MOCLE 8.3.D)
2. Describe the relationship among wavelength, energy, and frequency as
illustrated by the electromagnetic spectrum. (MOCLE 1.2.A.b)
3. Relate the atomic emission spectrum to the position of electrons.
4. Construct an orbital energy diagram and write the corresponding
electron configuration.
5. Draw an electron dot diagram. (MOCLE 1.1.A.c)
3. Periodic Table and Periodicity
A. Determine the rationale for the organization of the Periodic Table.
1. Explain the structure of the periodic table in terms of the elements with
common properties (groups/families) and repeating properties (periods).
(MOCLE 1.1.F.a & 1.1.A.d)
2. Classify elements as metals, nonmetals, metalloids, and noble gases
according to their location. (MOCLE 1.1.F.b)
3. Compare and contrast the common properties of metals, nonmetals, and
metalloids using the periodic table. (MOCLE 1.A.d)
B. Compare and contrast the common properties and major trends in the
Periodic Table.
1. Explain periodic trends: atomic radius, ionization energy,
electronegativity.
2. Predict the chemical reactivity of elements.
4. Chemical Bonding and Nomenclature (MOCLE 1.1.A.c, 1.1.F.c, 1.1.H.a,c)
A. Understand how an ionic bond forms.
1. Predict the number of electrons lost or gained in the formation of an ion.
2. Determine how ions combine to form a neutral compound and write the
appropriate formula.
3. Name ionic compounds (including acids and bases) using IUPAC
standards.
4. Describe characteristics of ionic compounds.
B. Understand how a covalent bond forms.
1. Utilize electron dot diagrams to construct Lewis structures of covalent
compounds.
2. Determine the number of shared pairs and characterize the bond type.
3. Draw and build a model of a molecule.
4. Analyze molecular structure using VSEPR theory to determine polarity.
5. Write the formula for covalent compounds.
6. Name covalent compounds using IUPAC standards.
7. Describe characteristics of covalent compounds (intermolecular forces).
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5. Chemical Reactions
A. Identify a chemical change. (MOCLE 1.1.G.a)
1. Classify the type of chemical reaction as synthesis, decomposition,
single replacement, double replacement, and combustion.
2. Predict the products of a chemical reaction using the activity series of
metals and solubility rules.
B. Apply the Law of Conservation of Mass to writing and balancing chemical
equations. (MOCLE 1.1.I.a, b)
1. Represent a chemical equation in words and formulas.
2. Balance a chemical equation using the Law of Conservation of Mass.
6. The Mole and Stoichiometry (MOCLE 1.1.I.a)
A. Quantify matter using the Mole.
1. Compare the mass, volume, and number of particles for a sample.
2. Calculate molar mass.
3. Use molarity to describe mole quantities in a solution.
B. Synthesize a compound and experimentally determine the ratio of its
elements.
C. Solve stoichiometric problems using mole ratios.
1. Predict the amount of product formed using limiting reagent concept.
2. Compare actual and theoretical yields. (MOCLE 7.1.C.c)
7. Gas Laws
A. Predict gas behavior using Kinetic Molecular Theory. (MOCLE 1.1.D.c)
1. Predict how a gas changes using The Combined Gas Law (Charles’,
Boyle’s, Gay-Lussac’s).
2. Apply Dalton’s Law of Partial Pressures.
B. Apply the mole concept to the Gas Laws.
1. Calculate an unknown variable using the Ideal Gas Law.
(MOCLE 7.1.C.b)
2. Predict experimental results of a reaction involving gas(es) using
stoichiometry.
3. Relate kinetic energy to an object’s mass and its velocity (Graham’s
Law). (MOCLE 1.2.B.a)
8. Thermochemistry: Energy and Matter (MOCLE 1.2.A.a)
A. Distinguish forms of energy as kinetic or potential. (MOCLE 1.2.B.c)
B. Describe energy movement as endothermic or exothermic. (MOCLE 1.2.D.a)
1. Measure the heat flow between a system and surroundings (calorimetry).
C. Describe how energy physically changes matter.
1. Predict how energy will change states of matter (solid, liquid, and gas).
(MOCLE 1.D.a,b)
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2. Label a heating curve with the terms: solid, liquid, gas, melting, freezing,
vaporizing, and condensing.
3. Determine the specific heat of a substance and use it to determine the
amount of energy needed to change its temperature.
4. Calculate the amount of energy involved in a physical change of matter
using Hvap and Hfus.
D. Describe how energy changes accompany chemical reactions. (MOCLE
1.2.D.a)
1. Classify enthalpy values (positive or negative) as endothermic or
exothermic processes. (MOCLE 1.2.D.a)
2. Perform stoichiometric calculations using a thermochemical equation.
3. Produce a progress of reaction graph to illustrate the change in enthalpy.
(MOCLE 1.2.D.a)
9. Solutions
A. Describe the solvation process for both ionic and covalent (polar and
nonpolar) compounds. (MOCLE 1.1.B.c)
1. Describe factors that affect solubility.
2. Describe factors that affect the rate of solution formation.
B. Determine the concentration of a solution.
1. Differentiate between dilute and concentrated solutions.
(MOCLE 1.1.B.a)
2. Express and/or calculate concentration using molarity, molality, percent
by mass and percent by volume. (MOCLE 1.1.B.a)
C. Describe the properties of a solution.
1. Describe the effect of a solute on a solvent.
2. Calculate boiling point elevation and freezing point depression.
10. Acid/Base Properties
A. Compare and contrast the properties of acidic, basic, and neutral solutions.
(MOCLE 1.1.B.b)
B. Identify the meaning of a pH value.
*** Possible Additions and/or Variations for Honors:
 Equilibria
 Nuclear
 Organic
 Elaborate on Acids/Bases (titrations, strong acids/bases)