PS: Physical Science

PS.1: Convert metric system units involving length, mass, volume, and time using dimensional analysis (i.e., factor-label method)

Stoichiometry

PS.3: Determine the significant figures based on precision of measurement for stated quantities

Unit Conversions 2 - Scientific Notation and Significant Digits

PS.4: Use scientific notation to express large and small numbers

Unit Conversions 2 - Scientific Notation and Significant Digits

PS.5: Write and name formulas for ionic and covalent compounds

Chemical Equations
Covalent Bonds
Ionic Bonds

PS.6: Write and name the chemical formula for the products that form from the reaction of selected reactants

Chemical Equations
Equilibrium and Concentration

PS.7: Write a balanced symbolic equation from a word equation

Balancing Chemical Equations
Chemical Equations

PS.8: Analyze the development of the modern atomic theory from a historical perspective

Bohr Model of Hydrogen
Bohr Model: Introduction

PS.9: Draw accurate valence electron configurations and Lewis dot structures for selected molecules, ionic and covalent compounds, and chemical equations

Covalent Bonds
Ionic Bonds

PS.10: Differentiate among alpha, beta, and gamma emissions

Nuclear Decay

PS.11: Calculate the amount of radioactive substance remaining after a given number of half-lives has passed

Half-life

PS.13: Identify the number of bonds an atom can form given the number of valence electrons

Covalent Bonds
Electron Configuration
Ionic Bonds

PS.15: Predict the physical and chemical properties of an element based only on its location in the periodic table

Electron Configuration

PS.22: Predict the kind of bond that will form between two elements based on electronic structure and electronegativity of the elements (e.g., ionic, polar, nonpolar)

Ionic Bonds

PS.23: Model chemical bond formation by using Lewis dot diagrams for ionic, polar, and nonpolar compounds

Covalent Bonds
Ionic Bonds

PS.29: Predict the properties of a gas based on gas laws (e.g., temperature, pressure, volume)

Boyle's Law and Charles' Law

PS.30: Solve problems involving heat flow and temperature changes by using known values of specific heat and latent heat of phase change

Calorimetry Lab
Energy Conversion in a System
Phase Changes

PS.31: Describe chemical changes and reactions using diagrams and descriptions of the reactants, products, and energy changes

Chemical Changes
Chemical Equations
Equilibrium and Concentration

PS.32: Determine the concentration of an unknown acid or base by using data from a titration with a standard solution and an indicator

Titration

PS.34: Describe chemical changes by developing word equations, balanced formula equations, and net ionic equations

Chemical Equations

PS.35: Predict products (with phase notations) of simple reactions, including acid/base, oxidation/reduction, and formation of precipitates

Equilibrium and Concentration

PS.37: Predict the direction of a shift in equilibrium in a system as a result of stress by using LeChatalier's principle

Equilibrium and Concentration
Equilibrium and Pressure

PS.38: Relate the law of conservation of matter to the rearrangement of atoms in a balanced chemical equation

Balancing Chemical Equations
Chemical Equations

PS.39: Conduct an investigation in which the masses of the reactants and products from a chemical reaction are calculated

Stoichiometry

PS.41: Apply knowledge of stoichiometry to solve mass/mass, mass/volume, volume/volume, and mole/mole problems

Chemical Equations
Limiting Reactants
Stoichiometry

PS.43: Graph and compute the energy changes that occur when a substance, such as water, goes from a solid to a liquid state, and then to a gaseous state

Calorimetry Lab
Phase Changes

PS.44: Measure and graph energy changes during chemical reactions observed in the laboratory

Chemical Changes

PS.45: Give examples of common chemical reactions, including those found in biological systems

Balancing Chemical Equations
Chemical Equations
Equilibrium and Concentration