1.2.a: Summarize the major experimental evidence that led to the development of various atomic models, both historical and current.
1.2.c: Discriminate between the relative size, charge, and position of protons, neutrons, and electrons in the atom.
1.2.d: Generalize the relationship of proton number to the element?s identity.
1.3.a: Use the periodic table to correlate the number of protons, neutrons, and electrons in an atom.
1.3.b: Compare the number of protons and neutrons in isotopes of the same element.
1.3.c: Identify similarities in chemical behavior of elements within a group.
1.3.d: Generalize trends in reactivity of elements within a group to trends in other groups.
2.1.b: Examine evidence from the lab indicating that energy is absorbed or released in discrete units when electrons move from one energy level to another.
2.1.d: After observing spectral emissions in the lab (e.g., flame test, spectrum tubes), identify unknown elements by comparison to known emission spectra.
2.2.b: Interpret graphical data relating half-life and age of a radioactive substance.
2.2.c: Compare the mass, energy, and penetrating power of alpha, beta, and gamma radiation.
2.2.e: After researching, evaluate and report the effects of nuclear radiation on humans or other organisms.
3.1.a: Determine the number of valence electrons in atoms using the periodic table.
3.1.b: Predict the charge an atom will acquire when it forms an ion by gaining or losing electrons.
3.1.c: Predict bond types based on the behavior of valence (outermost) electrons.
3.1.d: Compare covalent, ionic, and metallic bonds with respect to electron behavior and relative bond strengths.
3.2.a: Use a chemical formula to represent the names of elements and numbers of atoms in a compound and recognize that the formula is unique to the specific compound.
4.1.a: Generalize evidences of chemical reactions.
4.1.b: Compare the properties of reactants to the properties of products in a chemical reaction.
4.1.c: Use a chemical equation to describe a simple chemical reaction.
4.1.d: Recognize that the number of atoms in a chemical reaction does not change.
4.1.e: Determine the molar proportions of the reactants and products in a balanced chemical reaction.
4.1.f: Investigate everyday chemical reactions that occur in a student's home (e.g., baking, rusting, bleaching, cleaning).
4.2.a: Using data from quantitative analysis, identify evidence that supports the conservation of mass in a chemical reaction.
4.2.b: Use molar relationships in a balanced chemical reaction to predict the mass of product produced in a simple chemical reaction that goes to completion.
4.2.c: Report evidence of energy transformations in a chemical reaction.
4.2.d: After observing or measuring, classify evidence of temperature change in a chemical reaction as endothermic or exothermic.
5.1.a: Design and conduct an investigation of the factors affecting reaction rate and use the findings to generalize the results to other reactions.
5.1.b: Use information from graphs to draw warranted conclusions about reaction rates.
5.1.c: Correlate frequency and energy of collisions to reaction rate.
5.1.d: Identify that catalysts are effective in increasing reaction rates.
5.2.a: Explain the concept of dynamic equilibrium.
5.2.b: Given an equation, identify the effect of adding either product or reactant to a shift in equilibrium.
6.2.a: Identify the colligative properties of a solution.
6.2.b: Measure change in boiling and/or freezing point of a solvent when a solute is added.
6.3.a: Relate hydrogen ion concentration to pH values and to the terms acidic, basic or neutral.
6.3.b: Using an indicator, measure the pH of common household solutions and standard laboratory solutions, and identify them as acids or bases.
6.3.c: Determine the concentration of an acid or a base using a simple acid-base titration.
Correlation last revised: 1/20/2017