| C2 | Forms of Energy | |||||
| C2 | P2 | Potential Energy | ||||
| C2 | P2.pl | Potential Energy | essential | P2.p1A | Describe energy changes associated with changes of state in terms of the arrangement and order of the atoms (molecules) in each state. (prerequisite) | |
| C2 | P2.pl | Potential Energy | essential | P2.p1B | Use the positions and arrangements of atoms and molecules in solid, liquid, and gas state to explain the need for an input of energy for melting and boiling and a release of energy in condensation and freezing. (prerequisite) | |
| C2 | C2.1x | Chemical Potential Energy | ||||
| C2 | C2.1x | Chemical Potential Energy | core | C2.1a | Explain the changes in potential energy (due to electrostatic interactions) as a chemical bond forms and use this to explain why bond breaking always requires energy. | |
| C2 | C2.1x | Chemical Potential Energy | core | C2.1b | Describe energy changes associated with chemical reactions in terms of bonds broken and formed (including intermolecular forces). | |
| C2 | C2.1x | Chemical Potential Energy | core | C2.1c | Compare qualitatively the energy changes associated with melting various types of solids in terms of the types of forces between the particles in the solid. | |
| C2 | C2.2 | Molecules in Motion | ||||
| C2 | C2.2 | Molecules in Motion | essential | C2.2A | Describe conduction in terms of molecules bumping into each other to transfer energy. Explain why there is better conduction in solids and liquids than gases. | |
| C2 | C2.2 | Molecules in Motion | essential | C2.2B | Describe the various states of matter in terms of the motion and arrangement of the molecules (atoms) making up the substance. | |
| C2 | C2.2x | Molecular Entropy | ||||
| C2 | C2.2x | Molecular Entropy | core | C2.2c | Explain changes in pressure, volume, and temperature for gases using the kinetic molecular model. | |
| C2 | C2.2x | Molecular Entropy | core | C2.2d | Explain convection and the difference in transfer of thermal energy for solids, liquids, and gases using evidence that molecules are in constant motion. | |
| C2 | C2.2x | Molecular Entropy | core | C2.2e | Compare the entropy of solids, liquids, and gases. | |
| C2 | C2.2x | Molecular Entropy | core | C2.2f | Compare the average kinetic energy of the molecules in a metal object and a wood object at room temperature. | |
| C2 | C2.3x | Breaking Chemical Bonds | ||||
| C2 | C2.3x | Breaking Chemical Bonds | core | C2.3a | Explain how the rate of a given chemical reaction is dependent on the temperature and the activation energy. | |
| C2 | C2.3x | Breaking Chemical Bonds | core | C2.3b | Draw and analyze a diagram to show the activation energy for an exothermic reaction that is very slow at room temperature. | |
| C2 | C2.4x | Electron Movement | ||||
| C2 | C2.4x | Electron Movement | core | C2.4a | Describe energy changes in flame tests of common elements in terms of the (characteristic) electron transitions. | |
| C2 | C2.4x | Electron Movement | core | C2.4b | Contrast the mechanism of energy changes and the appearance of absorption and emission spectra. | |
| C2 | C2.4x | Electron Movement | core | C2.4c | Explain why an atom can absorb only certain wavelengths of light. | |
| C2 | C2.4x | Electron Movement | core | C2.4d | Compare various wavelengths of light (visible and nonvisible) in terms of frequency and relative energy. | |
| C2 | C2.5x | Nuclear Stability | ||||
| C2 | C2.5x | Nuclear Stability | core | C2.5a | Determine the age of materials using the ratio of stable and unstable isotopes of a particular type. | |
| C2 | C2.5x | Nuclear Stability | recommended | C2.r5b | Illustrate how elements can change in nuclear reactions using balanced equations. (recommended) | |
| C2 | C2.5x | Nuclear Stability | recommended | C2.r5c | Describe the potential energy changes as two protons approach each other. (recommended) | |
| C2 | C2.5x | Nuclear Stability | recommended | C2.r5d | Describe how and where all the elements on earth were formed. (recommended) | |
| C3 | Energy Transfer and Conservation | |||||
| C3 | P3.p1 | Conservation of Energy | ||||
| C3 | P3.p1 | Conservation of Energy | prerequisite | P3.p1A | Explain that the amount of energy necessary to heat a substance will be the same as the amount of energy released when the substance is cooled to the original temperature. (prerequisite) | |
| C3 | C3.1x | Hess's Law | ||||
| C3 | C3.1x | Hess's Law | core | C3.1a | Calculate the ?H for a given reaction using Hess | |
| C3 | C3.1x | Hess's Law | core | C3.1b | Draw enthalpy diagrams for exothermic and endothermic reactions. | |
| C3 | C3.1x | Hess's Law | core | C3.1c | Calculate the ?H for a chemical reaction using simple coffee cup calorimetry. | |
| C3 | C3.1x | Hess's Law | core | C3.1d | Calculate the amount of heat produced for a given mass of reactant from a balanced chemical equation. | |
| C3 | P3.p2 | Energy Transfer | ||||
| C3 | P3.p2 | Energy Transfer | prerequisite | P3.p2A | Trace (or diagram) energy transfers involving various types of energy including nuclear, chemical, electrical, sound, and light. (prerequisite) | |
| C3 | C3.2x | Enthalpy | ||||
| C3 | C3.2x | Enthalpy | core | C3.2a | Describe the energy changes in photosynthesis and in the combustion of sugar in terms of bond breaking and bond making. | |
| C3 | C3.2x | Enthalpy | core | C3.2b | Describe the relative strength of single, double, and triple covalent bonds between nitrogen atoms. | |
| C3 | C3.3 | Heating Impacts | ||||
| C3 | C3.3 | Heating Impacts | essential | C3.3A | Describe how heat is conducted in a solid. | |
| C3 | C3.3 | Heating Impacts | essential | C3.3B | Describe melting on a molecular level. | |
| C3 | C3.3x | Bond Energy | ||||
| C3 | C3.3x | Bond Energy | core | C3.3c | Explain why it is necessary for a molecule to absorb energy in order to break a chemical bond. | |
| C3 | C3.4 | Endothermic and Exothermic Reactions | ||||
| C3 | C3.4 | Endothermic and Exothermic Reactions | essential | C3.4A | Use the terms endothermic and exothermic correctly to describe chemical reactions in the laboratory. | |
| C3 | C3.4 | Endothermic and Exothermic Reactions | essential | C3.4B | Explain why chemical reactions will either release or absorb energy. | |
| C3 | C3.4x | Enthalpy and Entropy | ||||
| C3 | C3.4x | Enthalpy and Entropy | core | C3.4c | Write chemical equations including the heat term as a part of equation or using ?H notation. | |
| C3 | C3.4x | Enthalpy and Entropy | core | C3.4d | Draw enthalpy diagrams for reactants and products in endothermic and exothermic reactions. | |
| C3 | C3.4x | Enthalpy and Entropy | core | C3.4e | Predict if a chemical reaction is spontaneous given the enthalpy (?H) and entropy (?S) changes for the reaction using Gibb | |
| C3 | C3.4x | Enthalpy and Entropy | core | C3.4f | Explain why some endothermic reactions are spontaneous at room temperature. | |
| C3 | C3.4x | Enthalpy and Entropy | core | C3.4g | Explain why gases are less soluble in warm water than cold water. | |
| C3 | C3.5x | Mass Defect | ||||
| C3 | C3.5x | Mass Defect | core | C3.5a | Explain why matter is not conserved in nuclear reactions. | |
| C4 | Properties of Matter | |||||
| C4 | P4.p1 | Kinetic Molecular Theory | ||||
| C4 | P4.p1 | Kinetic Molecular Theory | essential | P4.p1A | For a substance that can exist in all three phases, describe the relative motion of the particles in each of the phases. (prerequisite) | |
| C4 | P4.p1 | Kinetic Molecular Theory | essential | P4.p1B | For a substance that can exist in all three phases, make a drawing that shows the arrangement and relative spacing of the particles in each of the phases. (prerequisite) | |
| C4 | P4.p1 | Kinetic Molecular Theory | essential | P4.p1C | For a simple compound, present a drawing that shows the number of particles in the system does not change as a result of a phase change. (prerequisite) | |
| C4 | P4.p2 | Elements, Compounds, and Mixtures | ||||
| C4 | P4.p2 | Elements, Compounds, and Mixtures | essential | P4.p2A | Distinguish between an element, compound, or mixture based on drawings or formulae. (prerequisite) | |
| C4 | P4.p2 | Elements, Compounds, and Mixtures | essential | P4.p2B | Identify a pure substance (element or compound) based on unique chemical and physical properties. | |
| C4 | P4.p2 | Elements, Compounds, and Mixtures | essential | P4.p2C | Separate mixtures based on the differences in physical properties of the individual components. | |
| C4 | P4.p2 | Elements, Compounds, and Mixtures | essential | P4.p2D | Recognize that the properties of a compound differ from those of its individual elements. (prerequisite) | |
| C4 | C4.1x | Molecular and Empirical Formaulae | ||||
| C4 | C4.1x | Molecular and Empirical Formaulae | core | C4.1a | Calculate the percent by weight of each element in a compound based on the compound formula. | |
| C4 | C4.1x | Molecular and Empirical Formaulae | core | C4.1b | Calculate the empirical formula of a compound based on the percent by weight of each element in the compound. | |
| C4 | C4.1x | Molecular and Empirical Formaulae | core | C4.1c | Use the empirical formula and molecular weight of a compound to determine the molecular formula. | |
| C4 | C4.2 | Nomenclature | ||||
| C4 | C4.2 | Nomenclature | essential | C4.2A | Name simple binary compounds using their formulae. | |
| C4 | C4.2 | Nomenclature | essential | C4.2B | Given the name, write the formula of simple binary compounds. | |
| C4 | C4.2x | Nomenclature | ||||
| C4 | C4.2x | Nomenclature | core | C4.2c | Given a formula, name the compound. | |
| C4 | C4.2x | Nomenclature | core | C4.2d | Given the name, write the formula of ionic and molecular compounds. | |
| C4 | C4.2x | Nomenclature | core | C4.2e | Given the formula for a simple hydrocarbon, draw and name the isomers. | |
| C4 | C4.3 | Properties of Substances | ||||
| C4 | C4.3 | Properties of Substances | essential | C4.3A | Recognize that substances that are solid at room temperature have stronger attractive forces than liquids at room temperature, which have stronger attractive forces than gases at room temperature. | |
| C4 | C4.3 | Properties of Substances | essential | C4.3B | Recognize that solids have a more ordered, regular arrangement of their particles than liquids and that liquids are more ordered than gases. | |
| C4 | C4.3x | Solids | ||||
| C4 | C4.3x | Solids | core | C4.3c | Compare the relative strengths of forces between molecules based on the melting point and boiling point of the substances. | |
| C4 | C4.3x | Solids | core | C4.4d | Compare the strength of the forces of attraction between molecules of different elements. (For example, at room temperature, chlorine is a gas and iodine is a solid.) | |
| C4 | C4.3x | Solids | core | C4.5e | Predict whether the forces of attraction in a solid are primarily metallic, covalent, network covalent, or ionic based upon the elements | |
| C4 | C4.3x | Solids | core | C4.6f | Identify the elements necessary for hydrogen bonding (N, O, F). | |
| C4 | C4.3x | Solids | core | C4.7g | Given the structural formula of a compound, indicate all the intermolecular forces present (dispersion, dipolar, hydrogen bonding). | |
| C4 | C4.3x | Solids | core | C4.8h | Explain properties of various solids such as malleability, conductivity, and melting point in terms of the solid | |
| C4 | C4.3x | Solids | core | C4.9i | Explain why ionic solids have higher melting points than covalent solids. (For example, NaF has a melting point of 995 | |
| C4 | C4.4x | Molecular Polarity | ||||
| C4 | C4.4x | Molecular Polarity | core | C4.4a | Explain why at room temperature different compounds can exist in different phases. | |
| C4 | C4.4x | Molecular Polarity | core | C4.4b | Identify if a molecule is polar or nonpolar given a structural formula for the compound. | |
| C4 | C4.5x | Ideal Gas Law | ||||
| C4 | C4.5x | Ideal Gas Law | core | C4.5a | Provide macroscopic examples, atomic and molecular explanations, and mathematical representations (graphs and equations) for the pressure-volume relationship in gases. | |
| C4 | C4.5x | Ideal Gas Law | core | C4.5b | Provide macroscopic examples, atomic and molecular explanations, and mathematical representations (graphs and equations) for the pressure-temperature relationship in gases. | |
| C4 | C4.5x | Ideal Gas Law | core | C4.5c | Provide macroscopic examples, atomic and molecular explanations, and mathematical representations (graphs and equations) for the temperature-volume relationship in gases. | |
| C4 | C4.6x | Moles | ||||
| C4 | C4.6x | Moles | core | C4.6a | Calculate the number of moles of any compound or element given the mass of the substance. | |
| C4 | C4.6x | Moles | core | C4.6b | Calculate the number of particles of any compound or element given the mass of the substance. | |
| C4 | C4.7x | Solutions | ||||
| C4 | C4.7x | Solutions | core | C4.7a | Investigate the difference in the boiling point or freezing point of pure water and a salt solution. | |
| C4 | C4.7x | Solutions | core | C4.7b | Compare the density of pure water to that of a sugar solution. | |
| C4 | C4.8 | Atomic Structure | ||||
| C4 | C4.8 | Atomic Structure | essential | C4.8A | Identify the location, relative mass, and charge for electrons, protons, and neutrons. | |
| C4 | C4.8 | Atomic Structure | essential | C4.8B | Describe the atom as mostly empty space with an extremely small, dense nucleus consisting of the protons and neutrons and an electron cloud surrounding the nucleus. | |
| C4 | C4.8 | Atomic Structure | essential | C4.8C | Recognize that protons repel each other and that a strong force needs to be present to keep the nucleus intact. | |
| C4 | C4.8 | Atomic Structure | essential | C4.8D | Give the number of electrons and protons present if the fluoride ion has a -1 charge. | |
| C4 | C4.8x | Electron Configuration | ||||
| C4 | C4.8x | Electron Configuration | core | C4.8e | Write the complete electron configuration of elements in the first four rows of the periodic table. | |
| C4 | C4.8x | Electron Configuration | core | C4.8f | Write kernel structures for main group elements. | |
| C4 | C4.8x | Electron Configuration | core | C4.8g | Predict oxidation states and bonding capacity for main group elements using their electron structure. | |
| C4 | C4.8x | Electron Configuration | core | C4.8h | Describe the shape and orientation of s and p orbitals. | |
| C4 | C4.8x | Electron Configuration | core | C4.8i | Describe the fact that the electron location cannot be exactly determined at any given time. | |
| C4 | C4.9 | Periodic Table | ||||
| C4 | C4.9 | Periodic Table | essential | C4.9A | Identify elements with similar chemical and physical properties using the periodic table. | |
| C4 | C4.9x | Electron Energy Levels | ||||
| C4 | C4.9x | Electron Energy Levels | core | C4.9b | Identify metals, non-metals, and metalloids using the periodic table. | |
| C4 | C4.9x | Electron Energy Levels | core | C4.9c | Predict general trends in atomic radius, first ionization energy, and electonegativity of the elements using the periodic table. | |
| C4 | C4.10 | Neutral Atoms, Ions, and Isotopes | ||||
| C4 | C4.10 | Neutral Atoms, Ions, and Isotopes | essential | C4.10A | List the number of protons, neutrons, and electrons for any given ion or isotope. | |
| C4 | C4.10 | Neutral Atoms, Ions, and Isotopes | essential | C4.10B | Recognize that an element always contains the same number of protons. | |
| C4 | C4.10x | Average Atomic Mass | ||||
| C4 | C4.10x | Average Atomic Mass | core | C4.10c | Calculate the average atomic mass of an element given the percent abundance and mass of the individual isotopes. | |
| C4 | C4.10x | Average Atomic Mass | core | C4.10d | Predict which isotope will have the greatest abundance given the possible isotopes for an element and the average atomic mass in the periodic table. | |
| C4 | C4.10x | Average Atomic Mass | core | C4.10e | Write the symbol for an isotope, X ZA , where Z is the atomic number, A is the mass number, and X is the symbol for the element. | |
| C5 | Changes in Matter | |||||
| C5 | P5.p1 | Conservation of Matter | ||||
| C5 | P5.p1 | Conservation of Matter | prerequisite | P5.p1A | Draw a picture of the particles of an element or compound as a solid, liquid, and gas. (prerequisite) | |
| C5 | C5.r1x | Rates of Reactions | ||||
| C5 | C5.r1x | Rates of Reactions | core | C5.r1a | Predict how the rate of a chemical reaction will be influenced by changes in concentration, and temperature, pressure. (recommended) | |
| C5 | C5.r1x | Rates of Reactions | core | C5.r1b | Explain how the rate of a reaction will depend on concentration, temperature, pressure, and nature of reactant. (recommended) | |
| C5 | C5.2 | Chemical Changes | ||||
| C5 | C5.2 | Chemical Changes | essential | C5.2A | Balance simple chemical equations applying the conservation of matter. | |
| C5 | C5.2 | Chemical Changes | essential | C5.2B | Distinguish between chemical and physical changes in terms of the properties of the reactants and products. | |
| C5 | C5.2 | Chemical Changes | essential | C5.2C | Draw pictures to distinguish the relationships between atoms in physical and chemical changes. | |
| C5 | C5.2x | Balancing Equations | ||||
| C5 | C5.2x | Balancing Equations | core | C5.2d | Calculate the mass of a particular compound formed from the masses of starting materials. | |
| C5 | C5.2x | Balancing Equations | core | C5.2e | Identify the limiting reagent when given the masses of more than one reactant. | |
| C5 | C5.2x | Balancing Equations | core | C5.2f | Predict volumes of product gases using initial volumes of gases at the same temperature and pressure. | |
| C5 | C5.2x | Balancing Equations | core | C5.2g | Calculate the number of atoms present in a given mass of element. | |
| C5 | C5.3x | Equilibrium | ||||
| C5 | C5.3x | Equilibrium | core | C5.3a | Describe equilibrium shifts in a chemical system caused by changing conditions (Le Chatelier | |
| C5 | C5.3x | Equilibrium | core | C5.3b | Predict shifts in a chemical system caused by changing conditions (Le Chatelier | |
| C5 | C5.3x | Equilibrium | core | C5.3c | Predict the extent reactants are converted to products using the value of the equilibrium constant. | |
| C5 | C5.4 | Phase Change/Diagrams | ||||
| C5 | C5.4 | Phase Change/Diagrams | essential | C5.4A | Compare the energy required to raise the temperature of one gram of aluminum and one gram of water the same number of degrees. | |
| C5 | C5.4 | Phase Change/Diagrams | essential | C5.4B | Measure, plot, and interpret the graph of the temperature versus time of an ice-water mixture, under slow heating, through melting and boiling. | |
| C5 | C54x | Changes of State | ||||
| C5 | C54x | Changes of State | core | C5.4c | Explain why both the melting point and boiling points for water are significantly higher than other small molecules of comparable mass (e.g., ammonia and methane). | |
| C5 | C54x | Changes of State | core | C5.4d | Explain why freezing is an exothermic change of state. | |
| C5 | C54x | Changes of State | core | C5.4e | Compare the melting point of covalent compounds based on the strength of IMFs (intermolecular forces). | |
| C5 | C5.5 | Chemical Bonds - Trends | ||||
| C5 | C5.5 | Chemical Bonds - Trends | essential | C5.5A | Predict if the bonding between two atoms of different elements will be primarily ionic or covalent. | |
| C5 | C5.5 | Chemical Bonds - Trends | essential | C5.5B | Predict the formula for binary compounds of main group elements. | |
| C5 | C5.5x | Chemical Bonds | ||||
| C5 | C5.5x | Chemical Bonds | core | C5.5c | Draw Lewis structures for simple compounds. | |
| C5 | C5.5x | Chemical Bonds | core | C5.5d | Compare the relative melting point, electrical and thermal conductivity and hardness for ionic, metallic, and covalent compounds. | |
| C5 | C5.5x | Chemical Bonds | core | C5.5e | Relate the melting point, hardness, and electrical and thermal conductivity of a substance to its structure. | |
| C5 | C5.6x | Reduction/Oxidation Reactions | ||||
| C5 | C5.6x | Reduction/Oxidation Reactions | core | C5.6a | Balance half-reactions and describe them as oxidations or reductions. | |
| C5 | C5.6x | Reduction/Oxidation Reactions | core | C5.6b | Predict single replacement reactions. | |
| C5 | C5.6x | Reduction/Oxidation Reactions | core | C5.6c | Explain oxidation occurring when two different metals are in contact. | |
| C5 | C5.6x | Reduction/Oxidation Reactions | core | C5.6d | Calculate the voltage for spontaneous redox reactions from the standard reduction potentials. | |
| C5 | C5.6x | Reduction/Oxidation Reactions | core | C5.6e | Identify the reactions occurring at the anode and cathode in an electrochemical cell. | |
| C5 | C5.7 | Acids and Bases | ||||
| C5 | C5.7 | Acids and Bases | essential | C5.7A | Recognize formulas for common inorganic acids, carboxylic acids, and bases formed from families I and II. | |
| C5 | C5.7 | Acids and Bases | essential | C5.7B | Predict products of an acid-base neutralization. | |
| C5 | C5.7 | Acids and Bases | essential | C5.7C | Describe tests that can be used to distinguish an acid from a base. | |
| C5 | C5.7 | Acids and Bases | essential | C5.7D | Classify various solutions as acidic or basic, given their pH. | |
| C5 | C5.7 | Acids and Bases | essential | C5.7E | Explain why lakes with limestone or calcium carbonate experience less adverse effects from acid rain than lakes with granite beds. | |
| C5 | C5.7x | Bronsted-Lowry | ||||
| C5 | C5.7x | Bronsted-Lowry | core | C5.7f | Write balanced chemical equations for reactions between acids and bases and perform calculations with balanced equations. | |
| C5 | C5.7x | Bronsted-Lowry | core | C5.7g | Calculate the pH from the hydronium ion or hydroxide ion concentration. | |
| C5 | C5.7x | Bronsted-Lowry | core | C5.7h | Explain why sulfur oxides and nitrogen oxides contribute to acid rain. | |
| C5 | C5.7x | Bronsted-Lowry | recommended | C5.r7i | Identify the Br | |
| C5 | C5.8x | Carbon Chemistry | ||||
| C5 | C5.8x | Carbon Chemistry | essential | C5.8A | Draw structural formulas for up to ten carbon chains of simple hydrocarbons. | |
| C5 | C5.8x | Carbon Chemistry | essential | C5.8B | Draw isomers for simple hydrocarbons. | |
| C5 | C5.8x | Carbon Chemistry | essential | C5.8C | Recognize that proteins, starches, and other large biological molecules are polymers. |