Standard set
Academic Chemistry
Standards
Showing 79 of 79 standards.
Properties of Matter
Structure of Matter
Matter & Energy
Reactions
Unifying Themes
Science as Inquiry
3.2.10.A1. GRADE 10
3.2.C.A1. CHEMISTRY
3.2.12.A1. GRADE 12
3.2.10.A2. GRADE 10
3.2.C.A2. CHEMISTRY
3.2.12.A2. GRADE 12
3.2.10.A3. GRADE 10
3.2.C.A3. CHEMISTRY
3.2.12.A3. GRADE 12
3.2.10.A4. GRADE 10
3.2.C.A4. CHEMISTRY
3.2.12.A4. GRADE 12
3.2.10.A5. GRADE 10
3.2.C.A5. CHEMISTRY
3.2.12.A5. GRADE 12
3.2.10.A6. GRADE 10
3.2.12.A6. GRADE 12
3.2.10.A1
Predict properties of element using trends of the periodic table.
3.2.10.A1
Identify properties of matter that depend on sample size.
3.2.10.A1
Explain the unique properties of water (polarity, high boiling point, forms hydrogen bonds, high specific heat) that support life on Earth.
3.2.C.A1
Differentiate between physical properties and chemical properties.
3.2.C.A1
Differentiate between pure substances and mixtures; differentiate between heterogeneous and homogeneous mixtures.
3.2.C.A1
Explain the relationship of an element's position on the periodic table to its atomic number, ionization energy, electronegativity, atomic size, and classification of elements.
3.2.C.A1
Use electronegativity to explain the difference between polar and non-polar covalent bonds.
3.2.12.A1
Compare and contrast colligative properties of mixtures.
3.2.12.A1
Compare and contrast the unique properties of water to other liquids.
3.2.10.A2
Compare and contrast different bond types that result in the formation of molecules and compounds.
3.2.10.A2
Explain why compounds are composed of integer ratios of elements.
3.2.C.A2
Compare the electron configurations for the first twenty elements of the periodic table.
3.2.C.A2
Relate the position of an element on the periodic table to its electron configuration and compare its reactivity to the reactivity of other elements in the table.
3.2.C.A2
Explain how atoms combine to form compounds through both ionic and covalent bonding.
3.2.C.A2
Predict chemical formulas based on the number of valence electrons.
3.2.C.A2
Draw Lewis dot structures for simple molecules and ionic compounds.
3.2.C.A2
Predict the chemical formulas for simple ionic and molecular compounds.
3.2.C.A2
Use the mole concept to determine number of particles and molar mass for elements and compounds.
3.2.C.A2
Determine percent compositions, empirical formulas, and molecular formulas.
3.2.12.A2
Distinguish among the isotopic forms of elements.
3.2.12.A2
Explain the probabilistic nature of radioactive decay based on subatomic rearrangement in the atomic nucleus.
3.2.12.A2
Explain how light is absorbed or emitted by electron orbital transitions.
3.2.10.A3
Describe phases of matter according to the kinetic molecular theory.
3.2.C.A3
Describe the three normal states of matter in terms of energy, particle motion, and phase transitions.
3.2.C.A3
Identify the three main types of radioactive decay and compare their properties.
3.2.C.A3
Describe the process of radioactive delay by using nuclear equations and explain the concept of half-life for an isotope.
3.2.C.A3
Compare and contrast nuclear fission and nuclear fusion.
3.2.12.A3
Explain how matter is transformed into energy in nuclear reactions according to the equation E = mc².
3.2.10.A4
Describe chemical reactions in terms of atomic rearrangement and/or electron transfer.
3.2.10.A4
Predict the amounts of products and reactants in a chemical reaction using mole relationships.
3.2.10.A4
Explain the difference between endothermic and exothermic reactions.
3.2.10.A4
Identify the factors that affect the rates of reactions.
3.2.C.A4
Predict how combinations of substances can result in physical and/or chemical changes.
3.2.C.A4
Interpret and apply the laws of conservation of mass, constant composition (definite proportions), and multiple proportions.
3.2.C.A4
Balance chemical equations by applying the law of conservation of mass.
3.2.C.A4
Classify chemical reactions as synthesis (combination), decomposition, single displacement (replacement), double displacement, and combustion.
3.2.C.A4
Use stoichiometry to predict quantitative relationships in a chemical reaction.
3.2.12.A4
Apply oxidation/reduction principles to electrochemical reactions.
3.2.12.A4
Describe the interactions between acids and bases.
3.2.10.A5
MODELS: Describe the historical development of models of the atom and how they contributed to modern atomic theory.
3.2.10.A5
SCALE: Apply the mole concept to determine number of particles and molar mass for elements and compounds.
3.2.C.A5
MODELS: Recognize discoveries from Dalton (atomic theory), Thomson (the electron), Rutherford (the nucleus), and Bohr (planetary model of the atom), and understand how each discovery leads to modern theory.
3.2.C.A5
Describe Rutherford's "gold foil" experiment that led to the discovery of the nuclear atom.
3.2.C.A5
Identify the major components (protons, neutrons, and electrons) of the nuclear atom and explain how they interact.
3.2.12.A5
MODELS/PATTERNS: Use VSEPR theory to predict the molecular geometry of simple molecules.
3.2.12.A5
CONSTANCY AND CHANGE: Predict the shift in equilibrium when a system is subjected to a stress.
3.2.10.A6
Compare and contrast scientific theories.
3.2.10.A6
Know that both direct and indirect observations are used by scientists to study the natural world and universe.
3.2.10.A6
Identify questions and concepts that guide scientific investigations.
3.2.10.A6
Formulate and revise explanations and models using logic and evidence.
3.2.10.A6
Recognize and analyze alternative explanations and models.
3.2.12.A6
Examine the status of existing theories.
3.2.12.A6
Evaluate experimental information for relevance and adherence to science processes.
3.2.12.A6
Judge that conclusions are consistent and logical with experimental conditions.
3.2.12.A6
Interpret results of experimental research to predict new information, propose additional investigable questions, or advance a solution.
3.2.12.A6
Communicate and defend a scientific argument.
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- PA State Standards
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