Chemistry  - List of Units

1. Explain how the properties of matter relate to structure and changes in
structure. (P)
a. Demonstrate the proper use and care of scientific equipment.
b. Observe and practice safe procedures in classroom and laboratory.
c. Define chemistry and matter.
d. Apply the language of chemistry appropriately including terms such as element,
atom, compound, and molecule.
e. Classify a material as element, compound, solution or heterogeneous mixture.
f. Relate symbols to names of common chemical elements.
g. Write the symbol or formula for monatomic and polyatomic ions.

2. Solve numerical chemistry problems using the International System of
Measurement (SI) units, mathematical expressions, and factor labeling. (P)
a. Choose the most appropriate SI unit of mass, length or volume of an object.
b. Define the common SI prefixes used in chemistry and interconvert, using the
factor-label method (dimensional analysis) to obtain the desired unit in solving
problems.
c. Apply the definition of mass, length, volume, time, density, temperature and
pressure.
d. Use scientific notation in chemical calculations.
e. Round values to the proper significant digits.

3. Develop a visual conceptualization of atomic structure based on theory
and a knowledge of fundamental particles. (P)
a. Identify various theories of the atom, including Rutherford, Bohr, and electron
cloud theories by matching the theory to its description.
b. Identify the three fundamental particles of an atom when given the charge,
mass, and location of the particle.
c. Determine the number of protons, electrons, or neutrons in an element when
given the atomic number and the atomic mass of the element, or vice versa.
d. Write the electron configurations of elements.
a. Draw the electron-dot (Lewis) structure of elements.
b. Predict the charge of an ion based on the element’s valence electrons.

4. Analyze patterns and trends in organization of elements in the periodic table.
(P)
a. Identify an element as a metal, nonmetal, metalloid, or noble gas.
b. Locate elements by name and group number (family) or period (series).
c. Compare elements in terms of atomic radius, ionization energy, or
electronegativity using their positions on the periodic table.
d. Predict the charge of monoatomic ions on the basis of position (group number).

5. Compare the properties of compounds according to their type of
bonding. (P, L, E)
a. Describe what determines covalent, ionic, and metallic bonds.
b. Relate bond type between elements on the basis of electronegativity differences.
c. Relate bond type to the position of elements on the Periodic table, electron
configuration, and properties of the compound formed.
a. Draw Lewis electron dot structures and determine the geometric structure of
simple molecules.
b. Identify simple molecules as polar or non-polar on the basis of molecular shape
and bond polarity.
c. Relate bond and molecular polarity to intermolecular forces.

6. Write names and formulas of covalent and ionic compounds. (P)
a. Write chemical formulas of ionic compounds using monatomic and polyatomic
ions.
b. Write chemical formulas of molecular compounds using prefixes.
c. Write names of compounds from their formulas.
a. Given the formula of a compound, identify oxidation states of the elements.
b. Write the names and formulas of common acids and bases.
7. Interpret chemical change in terms of chemical reactions. (P)
a. Write an equation in sentence form (word equation) when given a chemical
equation.
b. Balance a simple chemical equation by inspection when given the
formulas or names of all reactants and products.
c. Classify simple equations as to type: single displacement, double displacement,
synthesis and decomposition.
d. Complete chemical equations when given reactants for reactions, such as
synthesis, decomposition, single displacement, and double displacement.
e. Given a list of solubility rules, predict if a precipitate is formed upon mixing
solutions of known chemicals in a double displacement reaction.
f. Use the activity series to predict single displacement reactions and write
equations of these reactions.
g. Predict products of simple synthesis and decomposition reactions.
h. Identify redox reactions by recognizing the species that are oxidized and
reduced.

8. Explore the relationship between mass and quantity through various
stoichiometric relationships. (P)
a. Calculate the formula/molecular mass of compounds.
b. Define the mole as a quantity of matter.
c. Interconvert among mass, mole, and number of particles.
d. Determine the empirical formula from the percentage composition and the
molecular formula from the empirical formula and molar mass, or vice-versa.
e. Solve stoichiometry problems.
f. Identify the limiting reagent through stoichiometric calculations.

9. Apply understanding of the interactions of matter and energy. (P)
a. Demonstrate understanding by performing calculations relating enthalpy change,
temperature change, mass, and specific heat.
b. Calculate the energy required to change state using mass and heat of
vaporization or heat of fusion.
c. Classify chemical reactions as endothermic or exothermic.

10. Analyze the nature and behavior of gaseous, liquid, and solid
substances using Kinetic Molecular Theory. (P)
a. Describe a gas, liquid or solid in terms of Kinetic Molecular Theory.
a. Describe the relationship among volume, temperature, pressure, and moles
using ideal gas laws.
c. Calculate the partial pressure of a gas in a mixture.

11. Describe and explain the solution process. (P)
a. Describe solutions in terms of solute and solvent; electrolyte or non-electrolyte;
soluble or insoluble; unsaturated, saturated or supersaturated; miscible or
immiscible.
b. Express the concentration of a solution as percent by mass, molarity, molality,
and mole fraction, given appropriate data.
c. Explore the factors that affect solubility.
d. Describe how to make a solution of given molarity in terms of mass needed, or
vice-versa.
e. Describe how to dilute a solution in terms of molarity and volume.

12. Analyze the factors that affect equilibrium with an emphasis on
visualizing its dynamic nature at the macroscopic and molecular levels.
(P)
a. Describe a reversible reaction in terms of a dynamic equilibrium process.
b. Using LeChatelier’s principle, predict the effect upon a reaction at
equilibrium of changing the temperature, concentrations of a reactant or a
product, pressure, or adding a catalyst.

13. Visualize and explain acid-base interactions applying concepts of
chemical bonding and solutions. (P, L)
a. Compare properties of acids and bases, including how they affect indicators and
the relative pH of the solution.
b. Classify species in aqueous solutions according to Arrhenius and Bronsted
definitions, respectively.
c. Predict the product of an aqueous neutralization reaction.
d. Calculate the pH or pOH from the hydrogen or hydroxide ion concentrations of
solutions and vice versa.
e. Describe the role of indicators in experimental prediction of pH.