1. Chemistry Unit Benchmark

2. SPS2 – Students will explore the nature of matter, its classifications, and its system for naming types of matter.

3. Calculate density when given a means to determine a substance’s mass and volume.
Predict formulas for stable binary ionic compounds based on balance of charges.
Use IUPAC nomenclature for transition between chemical names and chemical formulas of
Binary ionic compounds (containing representative elements)

4. Binary covalent compounds (i.e. carbon dioxide, carbon tetrachloride)
Demonstrate the Law of Conservation of Matter in a chemical reaction.
Apply the Law of Conservation of Matter by balancing the following types of chemical equations:
Synthesis, Decomposition, Single replacement, Double replacement

5. Main Concepts To Know Covalent vs. Ionic Bonds Density
Balancing Ionic Compounds
Naming Compounds
Acids, Bases, & Electricity

6. Main Concepts To Know Facts about Acids & Bases (pH scale)
Law of Conservation of Mass (applied to chemical equations)
Balancing Chemical Equations
Interpreting Solubility Curves

7. Main Concepts To Know Types of Reactions Solute vs.Solvent Lab Safety
Hydrocarbon Facts
Counting Atoms of a compound

8. Covalent vs. Ionic Bonds
What types of elements will form a covalent bond?
What types of elements will form an ionic bond?
In which bond are electrons shared?
In which bond are electrons transferred?

9. Density What is the formula?
Be able to determine the density of an object using a chart or displacement information.

10. Balancing Ionic Compounds
Be able to create balanced chemical compounds.
Li & Cl
Al & O
K & N

11. Naming Compounds
Know Prefixes
Name:
P3N5
Ca3O10

12. Acids, Bases, & Electricity
What solutions will conduct electricity well?
Strong Acids & Strong Bases
What property allows the solutions to conduct electricity?
Both contain large amounts of charged ions

13. Acids, Bases, & Electricity
Acids have a pH below 7 & produce H+ ions
Bases have a pH above 7 & produce OH- ions
Be able to read a pH scale and answer questions about it.

14. A chemist is trying to dissolve a large crystal of magnesium sulfate (MgSO4) in water by stirring the solution, but the crystal dissolves very slowly. What can the chemist do to speed up the process?

15. Law of Conservation of Mass (applied to chemical equations)
In a balanced chemical question, the mass of the reactants will equal the mass of the products.

16. This table below shows the reaction of sodium chloride (NaCl) with silver nitrate (AgNO3) and the masses of the compounds involved in the reaction. NaCl +AgNO3→ AgCl +NaNO3
Reaction
NaCl +AgNO3→ AgCl +NaNO3
Mass before
reaction (g)
12.34
15.27
0.00
Mass after x
17.00

17. Balancing Chemical Equations
Be able to balance chemical equations
N2+3H2→2NH3
N2+H2→NH3
N2+H2→2NH3
2N2+3H2→2NH3

18. Interpreting Solubility Curves
Be able to read and interpret a solubility curve.
Example: Be able to tell at what temperature all of the solute would be dissolved.

19. Types of Reactions
AB  A + B
2H2O  2H2 + O2
XA + B  BA + X

20. Concentrated vs. Diluted Saturated vs. Unsaturated
Solute vs.Solvent
Know facts about each
Concentrated vs. Diluted
Saturated vs. Unsaturated

21. General Rules (common sense)
Lab Safety
General Rules (common sense)

22. Saturated vs. Unsaturated
Hydrocarbon Facts
Composition
Saturated vs. Unsaturated

23. Counting Atoms of a compound
C6H12O6
H2O