CHEMISTRY HONORS

Credits: 5

This course differs completely from the nonhonors course in the scope, pace and level of difficulty. Chemistry investigates matter and energy and ways in which these two quantities interact. Over a course of study in chemistry, students should be able to recognize how both matter and energy are both quantified (measured) and qualified (observed) in a variety of contexts. This course also makes connections between matter and the energy transformations and includes the connection to nuclear chemistry. This course exposes students to problemsolving situations that are developed through class discussions, demonstrations, and lab activities. Students will demonstrate understanding through performance expectations. Lab experiences complement the core concepts

Curriculum

Unit 1: Unraveling the Atom: Exploring Atomic Models and Properties in Chemistry Chapter 1-6 & Nuclear

Unit Summary:

In this unit students build on the model of the atom as a foundation for explaining chemical formulas. A study of atomic models is essential to investigate atomic isotopes and radioactivity. The concept of the energy and stability in an atom is dependent on the electron organization. Students will use the periodic table as a tool to explain and predict patterns for electron configurations and use this knowledge to predict the properties of elements. The properties of substances are determined by the interactions between atoms which can be predicted using knowledge of atomic structure. A study of the different kinds of bonds that atoms can make with one another allows students to construct models and explanations about their macroscopic properties. Students learn how to write chemical formulas and to name compounds building on their prior knowledge of atomic structure and bonding. Students are expected to demonstrate proficiency in developing and using models; constructing explanations and designing solutions; using mathematical and computational thinking; and obtaining, evaluating, and communicating information; and they are expected to use these practices to demonstrate understanding of the core ideas. The crosscutting concepts of patterns; energy and matter; scale, proportion, and quantity; and stability and change are called out as organizing concepts for this unit.

Unit 3: Metrics, Moles,Chemical Reactions, Stoichiometry

Unit Summary: Chapters 7,8,9

Chemists use the mole to count atoms, molecules, ions, and formula units. A mole always contains the same number of particles; however, moles of different substances have different masses. The molar mass of a compound can be calculated from its chemical formula and can be used to convert from mass to moles of that compound. A molecular formula of a compound is a whole-number multiple of its empirical formula. Hydrates are solid ionic compounds in which water molecules are trapped. : Millions of chemical reactions in and around us transform reactants into products, resulting in the absorption or release of energy. Chemical reactions are represented by balanced equations. There are four main types of chemical reactions: synthesis, combustion, decomposition, and replacement (single and double) reactions. Double replacement reactions occur between substances in aqueous solutions and produce precipitates, water, or gases The amount of each reactant present at the start of a chemical reaction determines how much product can form. The solution to every stoichiometric problem requires a balanced chemical equation. A chemical reaction stops when one of the reactants is used up. Percent yield is a measure of the efficiency of a chemical reaction.

Unit 4: Energy, Change & States of Matter

Unit Summary: Chapters 10,11,16

Chemical reactions usually absorb or release energy. Energy can change form and flow, but it is always conserved. The enthalpy change for a reaction is the enthalpy of the product minus the enthalpy of the reactants. Thermochemical equations express the amount of heat released or absorbed by chemical reactions. Gases expand, diffuse, exert pressure, and can be compressed because they are in a low-density sate consisting of tiny, constantly-moving particles. The particles in solids and liquids have a limited range of motion and are not easily compressed. Intermolecular forces (dispersion, dipole-dipole, hydrogen bonds) determine a substance’s state at a given temperature. Matter changes phases when energy is added or removed or when pressure changes occur. For a fixed amount of gas, a change in one variable (pressure, temperature, or volume) affects the other two. The ideal gas law relates the number of particles to pressure, temperature and volume. When gases react, the coefficients in the balanced chemical equation represent both molar amounts and relative volumes.

Unit 5: Solutions & Acids & Bases

Unit Summary: Chapters 12,13,14,15

Most everyday matter occurs as mixtures- combinations of two or more substances. Mixtures can be separated by physical means. Common separation techniques include filtration, distillation, and chromatography. Mixtures can be either heterogeneous or homogeneous. Concentration can be expressed in terms of percent (by mass or volume) or in terms of moles (Molarity, molality, and mole fraction). Factors such as temperature, pressure, and polarity affect the formation of solutions. Colligative properties depend on the number of solute particles in a solution (freezing point depression and boiling point elevation)

Acids and bases have real life significance. The human body functions properly only when delicate acid base balances are maintained, crops grow best in soil with proper pH, substances released into the atmosphere as pollutants form acid rain and foods as well as many substances used in the home are acids and bases. This unit focuses on the structure, properties and reactions of acids and bases. Acids and bases are a specific class of molecules which needs to be distinguished by strong acids and bases versus weak acids and bases. Also can be described based on the degree of ionization of the molecules which can be used to calculate the pH, pOH, [H⁺] and [OH^-]. The pH scale shows the degree of ionization. Descriptions of acids and bases fall in three categories: Arrhenius, Brønsted-Lowery, and Lewis. Neutralization reactions are used in titrations to identify concentrations of unknown acids and bases.

Make Up Policy
• When you are absent, you will receive an email from Ms. Paff with what you missed that day
- - Please Check the posted classroom calendar for lesson information.
  - Please watch the notes videos that are included in the email and complete your notes
  - Work on the homework and check your work with the answer keys posted on my website.
- Test: After school on Monday during extra help. Or other afternoons after school in the testing center
•Labs: : You will be sent data and/or video. Please complete the lab and turn in by the due date.

•Quizzes: Next class. unit lunch, after school on Monday

•HW- posted in the google classroom upon request or check your work with the answer keys posted on my website
Accountability Policy

Once Papers are returned to class grade will become & stay a zero

This does not apply to assignments that are graded for completion.

•Completion Assignment (out of 2 pts)

•-0.2pts by end of the period

•-0.75 pts end of day or next day

•add an additional (-0.25) for each subsequent day
•Assignment (out of 50 pts)

•-2pts by end of the period

•-3 pts end of day or next day

•add an additional (-1) for each subsequent day

•Assignment (out of 25 pts)

•-1pts by end of the period

•-2 pts end of day or next day

•-add an additional (-1) for each subsequent day
Grading Policy
Will be updated once District approved

As described in the course proficiency
- Assessments: Major 30%
- Assessments: Minor 60%
- Homework/ Classwork: 10%

Wall High School

PAFF, GALE

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Make Up Policy

Accountability Policy

Grading Policy