Perform a lab experiment safely

Differentiate among element, compound, homogeneous mixture, or heterogeneous mixture. 

Draw and interpret particulate diagrams of matter.

Distinguish between physical and chemical properties and changes. 

Measure and convert measurements using dimensional analysis

Distinguish between reactants and products of a chemical reaction. 

Demonstrate the Law of Conservation of Mass applies to both physical and chemical changes.

Measure quantities using appropriate units for measurement (i.e., grams, meters, liters, second, etc.) and level of precision. 

How does the lens in which we observe matter influence our definition of matter? 

How might our understanding of chemistry change in the absence of measurement?

How does chemistry influence how we view the universe?

Identify and calculate the number of protons, neutrons, and electrons in any atom.

Differentiate between isotopes and ions of elements in terms of the number of subatomic particles present.

Calculate the average atomic mass of an element using isotopic data.

Collect and use information on the Periodic Table, including atomic number, atomic mass, family designation, period number, classification of element (metal, nonmetal, semimetal, or metalloid), and the state of the element at room temperature.

Relate the family/group and period for an elements to their corresponding number of valence electrons and their energy level.

How has atomic theory developed over time?

What determines the structure of an atom? 

How can we determine atomic structure if we can’t see an atom?

How does the periodic table organize and communicate information about atoms?

Distinguish among energy levels, sublevels and orbitals.

Write electron configurations and draw orbital diagrams for elements and ions using the application of Aufbau's Principle, Pauli Exclusion principle, and Hund's Rule.

Determine the number of valence electrons versus core electrons using full and shorthand electron configurations for atoms or ions.

Draw Lewis dot diagrams for atoms utilizing the concept of valence versus core electrons.

Calculate the wavelength, frequency, and energy for a given electron transition. 

How do we explain the properties of matter in terms of the organization of electrons around the nucleus? 

How do we explain the source and common use of the electromagnetic spectrum? 

Describe how atoms interact with one another by transferring and sharing valence electrons

Discover trends and formulate rules about bonds and their physical properties.

Illustrate ionic and covalent bonds utilizing electron dot notation

Use appropriate materials to build adequate models of simple molecules and polyatomic ions representing the shapes of these species

Predict the shape of a molecule from its chemical formula.

Predict the polarity of a molecule given its shape and types of bonds.

Classify a substance as metallic, ionic, or covalent based on data (solubility, melting point, boiling point, conductivity).

Name and write formulas for ionic, covalent, and acidic compounds. 

How do atoms interact to form compounds?

Why is the correct naming and formulating of compounds so important?

How does molecular shape inform our understanding of a compound? 

Write and balance a chemical equation in support of the Law of Conservation of Mass.

Categorize the types of chemical reactions based on the nature of observed changes.

Predict the products of a synthesis, decomposition, single replacement, and double replacement or combustion reaction, for a given combination of reactants. 

Use mole relationships to convert and calculate between different measurements of matter and its particle nature. 

Derive the empirical formula for a compound by using experimentally obtained masses of each element. 

Honors: 

Predict the products of a single replacement reaction with the use of an activity series.

Predict the products of a metathesis or double replacement reaction with the use of solubility rules.

Write complete and net ionic equations for aqueous reactions.

Assign oxidation states and distinguish the patterns for which reactions undergo redox. 

How do we explain and classify the interactions of matter? 

How is the mole used to quantize matter? 

What are the patterns in chemical reactions and how do we utilize them as a tool for prediction? 

Identify stoichiometric ratios from balanced chemical equations. 

Calculate different types of stoichiometry problems. (i.e. mass-mass, mass-volume, volume-volume)

Identify the limiting reactant in a reaction and calculate the theoretical yield of product(s) and the quantity of other reactant(s) consumed or un-reacted. 

Determine percent yield based on experimental/actual yield and expected/theoretical yield. 

How do we interpret a chemical reaction and utilize it as a tool for prediction? 

Explain how dissolving is different from dissociation. 

Define: dilute, concentrated, unsaturated, saturated, and supersaturated.

Explain how stirring, surface area, temperature, and concentration influence the rate of solution formation. 

Apply “like dissolves like” to everyday events. (i.e. actions of detergents and soap)

Interpret a solubility curve. 

Calculate the molarity (concentration) of a solution given the amount of solute and the volume of solvent.

Describe how to create a new solution of a particular molarity from both a solid solute and from an aqueous solution.  

Recognize the difference between concentration and amount, calculating the molarity  of a solution and calculations associated with dilutions. 

Measure acidity levels of common substances using the pH scale.

Differentiate between properties of acids and bases.

Calculate the pH and pOH of different solutions. 

Calculate the molarity of an unknown acid or base from titration data.

How do we describe characteristics of solutions? 

How do we describe factors affecting solubility? 

How do we describe acid-base reactions? 

Explain the effects of temperature, pressure, and volume changes on the behavior of gaseous particles. 

Define kinetic molecular theory and use it to explain differences in real versus ideal gases. 

Apply the gas laws to scenarios involving the temperature, volume, pressure, and amount of a gaseous substance.

Explain how the total pressure in a mixture of gases is equal to the sum of the partial pressures of each gas present. 

Compare the diffusion rates of two gases. 

Calculate the pressure of a dry gas when collected over water. 

How do we describe the behavior of gases and relate the behavior to gas properties? 

Define intermolecular forces and contrast it with intramolecular bonds 

List factors that affect the strength intermolecular forces

Given a covalent molecule, predict what intermolecular forces will be present

Compare the relative strength of London Dispersion forces, dipole-dipole forces, and hydrogen-bonding

Use intermolecular forces to predict physical properties of substances including: melting point, boiling point, solubility, and vapor pressure.

Draw a diagram to show that water is polar and how hydrogen bonding occurs 

Explain why substances with different intermolecular forces do not mix 

How do we explain the structure, properties, and interactions of matter? 

Why are IMFs essential for life?