Chemistry

Unit 1 - ATOMIC STRUCTURE

UNIT 2 - PERIODIC TABLE

UNIT 3 - CHEMICAL BONDING

UNIT 4 - STATES OF MATTER

UNIT 5 - CHEMICAL QUANTITIES

UNIT 6 - CHEMICAL REACTIONS

UNIT 7 - STOICHIOMETRY

UNIT 8 - THERMOCHEMISTRY

Develop models to describe the atomic composition of simple molecules.  

Use evidence to determine whether a physical or chemical change has occurred. 

Describe atomic structure using a model of the atom that includes protons, neutrons, and electrons.  

Compare and contrast atoms of different elements and isotopes of the same element. 

Develop and use Bohr models for atoms, illustrating electron energy levels and the placement of electrons within those levels. 

Use the Bohr model and changes in the electron’s energy to explain why elements have unique atomic emission spectra. 

Describe how elements in the periodic table are arranged by the numbers of protons in atoms.

Identify how the arrangement of the main groups of the periodic table reflects the patterns of outermost electrons. 

Explain how the position of an element in the table can be used to predict some of its chemical properties. 

Use Coulomb’s law to explain effective nuclear charge and why the positive charge exerted by an atomic nucleus is not equal to the charge of its protons. 

Explain patterns of effective nuclear charge across a period of main group elements.

Investigate and explain reactivity patterns in the periodic table using concepts of ionization energy, net effective charge, and atomic radius.   

Use periodic trends to explain some chemical properties of elements.  

Explain that atoms gain or lose electrons to form ions so that they have a full valence shell, which makes them more stable. 

Explain that ionic bonds are electrostatic attractions between cations and anions. 

Describe how the structures of ionic compounds affect their properties.  

Describe the electron sea model and explain how the bonding in metals and alloys affects their properties.  

Explain how nonmetals share electrons to complete their valence shell octet, resulting in the formation of a covalent bond. 

Identify single, double, and triple covalent bonds and draw electron dot diagrams for each. 

Use electronegativity values to determine the type of bond formed. 

Explain how the strength of attractions between particles influence the bulk properties of a material. 

Develop models to explain behavior of gases with changes in temperature, pressure, and volume.

Evaluate models of states of matter and use them to explain differences in the attractive forces between particles.  

Describe how variations in kinetic energy among particles result in constant evaporation and condensation, even without heating or cooling.  

Describe how variations in kinetic energy among particles result in phase changes due to heating and cooling.  

Summarize the mechanisms by which gas bubbles in a heated liquid exert enough pressure to break free of the surface, resulting in boiling. 

Relate phase changes to the strength of attractive forces or bonds between their particles.   

Interpret phase diagrams to determine the state of water at various pressure and temperature points, and apply that understanding to predict the state of carbon dioxide at STP based on its phase diagram.  

Investigate the role of polarity in hydrogen bonding between water molecules.  

Discover how hydrogen bonding affects surface tension, boiling point, and the formation of ice. 

Develop a model that demonstrates the process of solvation within an aqueous solution.  

Diagram and explain why electrolytes conduct electricity and nonelectrolytes do not. 

Analyze the role of pressure in the efflorescence of hydrates. 

Investigate the role of temperature and surface area in the formation of solutions. 

Develop a model to explain how solutions can become supersaturated.  

Construct and interpret graphs depicting solubility curves. 

Use Henry’s law to discover the relationship between the solubility of a gas and pressure. 

Differentiate between solutions, suspensions, and colloids. 

Investigate the three methods used to measure matter – count, mass, and volume.  

Develop models of the mole that encompass atoms, molecules, and formula units. 

Explain the relationship between the mole and Avogadro’s number. 

Use Avogadro’s number to convert from moles to particles and particles to moles. 

Use the periodic table to find the molar mass of elements and compounds.  

Use the mole concept to convert between mass, volume (of a gas), and representative particles.  

Convert mole quantities to masses, and mass quantities to moles.  

Explain the relationship between moles and volumes of gases at STP. 

Calculate the density of a gas at STP, given the molar mass of the gas. 

Explain how to find the percent composition of a compound.  

Develop models to illustrate the law of definite proportion and law of constant composition.  

Find the empirical and molecular formulas for a compound. 

Use subscripts within a chemical formula to represent a mole ratio. 

Find the molarity of a solution.

Investigate how the ratio of solute to solvent affects the concentration of a solution. (Include percentages)  

Devise a method to make a solution of a specific concentration. 

Calculate the percentage of a solution by mass and by volume.

Write balanced equations for chemical reactions.  

Distinguish between endothermic reactions and exothermic reactions. 

Explain what causes chemical reactions (do not include rates).  

Develop a basic conceptual and mathematical model for the generation of energy from the reaction of two substances.  

Develop a model that demonstrates conservation of mass in a chemical equation.  

Identify the five general types of chemical reactions and describe components that are reactants and products in these reactions. ions and describe. 

Predict the outcome of certain reactions based on these components, and make a claim about why the reactants react and why the products are formed. (Non-summative CER) 

Investigate and explain formation of precipitates using knowledge of solubility and intermolecular forces.

Use evidence to make a claim about whether a reaction will form a precipitate in a chemical reaction.

Analyze data on proportionality of reactants and products to predict their stoichiometric ratios in the corresponding chemical equation.

Develop a model that demonstrates conservation of matter of mass in a chemical equation.

Apply mathematical concepts to interpret a chemical equation. 

Use dimensional analysis to determine the mass of reactant required to obtain a given amount of product. 

Use the mole ratio in a chemical reaction to relate amounts of participating substances. 

Develop and use a model of different units of measurement. 

Calculate and communicate data on different units of measurement. 

Explain the concept of limiting reactant and how it affects the amount of product produced in a reaction. 

Explain theoretical and actual yield and why the former is usually larger than the latter.   

Use computational thinking to predict the grams of product given the grams of reactant.   

Explain how molecules must collide with each other with sufficient energy and in the correct orientation for a chemical reaction to take place.  

Represent energy changes in exothermic and endothermic reactions using an enthalpy diagram.  

Calculate enthalpy of reaction from bond energies and molar enthalpy of reaction data.  

Explain how Hess’s law can be used to calculate the change in enthalpy for a chemical reaction using any number of intermediate compounds. 

Calculate the change in enthalpy for a reaction using the sum of a system of chemical equations or a table of enthalpies of formation.  

Calculate the change in enthalpy for a dissolution process using molar enthalpy of a solution.

Understand how and why substances change in enthalpy when transitioning between physical states.  

Calculate the change in enthalpy for state changes between solid, liquid, and gas. 

Describe the link between state change enthalpies and the strength of intermolecular forces.