Week

Chapter

Tasks

Standards

1

1,2

Describe the roll of chemists and procedures used in the study of matter. Measuring and Calculating (SI BASE UNITS) convert metrics, use scientific notation and significant figures in calculating.

Lab #1

S.C.H.2.4.2

1.04, 1.06, 1.07, 1.08

2

3

Matter and Energy

Distinguish between heterogeneous and homogeneous substances, mixtures and solutions. Classify all types of matter. Give examples of elements and compounds. Classify changes as physical or chemical.

Lab #2

S.C.H.2.4.2

S.C.H.2.4.1

2.01, 2.02, 2.03

3

7

Chemical Nomenclature

Demonstrate proficiency in writing chemical formulas. Define oxidation numbers. Demonstrate proficiency in naming compounds.

6.02, 6.03, 6.04

4

8

The Mole

Use Avogardro’s constant to define the mole. Calculate molecular and formula mass. Convert moles and masses. Determine % composition and empirical formulas.

Lab #3

6.05, 6.06, 6.07

5

9

Balancing Equations

Write chemical equations to represent reactions. Use coefficients to balance chemical equations. Differentiate between the five major types of reactions.

Lab #4

S.C.B.1.4.2

7.02, 7.03, 7.04

6

9

Stoichiometry

Determine the mass of reactant or product based on the mass of another reactant or product. Calculate % yield.

6.08, 7.01, 7.02, 7.03, 7.04

7

4

Atomic Structure

Discuss early development in atomic theory. Differentiate among atomic particles. Discuss the development of the modern atomic theory. Calculate average atomic mass and isotopic %.

Lab #5

S.C.A.2.4.1

S.C.A.2.4.3

3.01, 3.02, 3.03

8

5

Electron Clouds and Probability

Describe an electron cloud characterized by the position and velocity of the electron. Characterize the four quantum numbers. Use Pauli’s Exclusion principle, Bohr’s equation, Planck’s equation to calculate the energy of an electron.

S.C.A.2.4.1

S.C.A.2.4.3

S.C.A.2.4.6

3.04, 3.05, 3.06, 3.07, 3.08, 3.09, 3.10

9

6

Periodic Table

Describe early attempts at classifying elements. Identify metals, nonmetals, metalloids. Predict the electron configuration of all elements. Write electron dot diagrams.

Lab #6

S.C.A.2.4.5

4.01, 4.02

10

10

Periodic Properties

Define periodic trends in ionization energy, electron affinity, atomic size, and electronegativity. Use examples to explain periodic properties of elements.

S.C.A.2.4.5

4.02, 4.03

11

12

Identify the type of bonding between two elements given their electronegativities. Differentiate between ionic, covalent, metallic bonding. Determine single, double, and triple covalent bonds. Predict molecular shapes and draw Lewis dot diagrams.

Lab #7

S.C.A.2.4.1

S.C.A.1.4.5

S.C.A.2.4.2

5.01, 5.02, 5.03

12

13

Molecular Structures and Polarity

Differentiate between covalent, ionic, and Van der Waal radii. Discuss polar and nonpolar bonding. Describe hybrid orbitals using bond angles and sigma-pi bonding.

S.C.A.2.4.1

S.C.A.1.4.2

S.C.A.2.4.5

5.04, 5.05, 5.06, 5.07

13

18

Gases

Describe conditions of S.T.P. Relate the laws of Charles, Boyle, and < xml="true" ns="urn:schemas-microsoft-com:office:smarttags" prefix="st1" namespace="">Dalton and perform calculations for volume, pressure, and temperature. Differentiate between an ideal and a real gas. Compute problems using the ideal conditions.

Labs #8, 9

S.C.B.1.4.3

8.01, 8.02, 8.03, 8.04, 8.05

14

20

Solutions

Describe and explain the process of salvation, dissociation, and dissolving. Differentiate and solve problems in molarity, molality, mole fractions, and mass %.

Lab #10

S.C.C.2.4.5

10.01,10.02,10.03, 10.04, 10.7

15

21

Colligative Properties

Calculate the effects of a solute on the boiling point, freezing point, and vapor pressure of a solution. Explain the concept of osmotic pressure.

10.05, 10.06

16

23

Acids/Bases/Salts

Distinguish the definitions of acids and bases according to Arrhenius, Bronsted-Lowry, and Lewis. Name acids and bases. Define anhydrides. Determine pH and calculate hydronium ion concentration.

Lab #11

11.01,11.02,11.03,

11.04, 11.05

17

25

Redox Reactions

Compare the processes of oxidation and reduction. Assign oxidation numbers to elements in a compound. Balance equations using oxidation and reduction electrons.

13.01, 13.02, 13.03

18

Review for FINAL EXAM!!!!!!!!!!!