General Chemistry Standards

1.1 Identify proper safety procedures in the laboratory
1.2 Identify and use proper tools and equipment in the laboratory
1.3 Differentiate between qualitative and quantitative data
1.4 Convert measurements among the metric units
1.5 Identify the appropriate measuring device for a specific problem and count the number of significant figures in a measurement
1.6 Differentiate between accuracy and precision
1.7 Convert numbers to and from scientific notation maintaining the prevision of the measurement
1.8 Convert measurements using dimensional analysis
1.9 Round numbers to the correct number of significant figures
1.10 Add and subtract numbers maintaining the precision of the measurement
1.11 Multiply and divide numbers maintaining the precision of the measurement
1.12 Identify and differentiate among the seven diatomic molecules
1.13 Differentiate between physical and chemical properties and changes
1.14 Distinguish among a mixture, compound, and a pure substance
1.15 Explain the states of matter in terms of particles
1.16 Classify mixtures as homogeneous or heterogeneous
1.17 Relate the atomic symbols with their correct atomic name
1.18 Calculate the density of a substance
2.1 Compute how heat energy added to a substance will change the substance’s temperature
2.2 Apply the definition of heat to the molecular level
2.3 Identify phase changes and calculate the energy needed to change a phase
2.4 Differentiate among the different types of energy
2.5 Calculate the speed, wavelength, and frequency of electromagnetic radiation
2.6 Differentiate among different types of electromagnetic radiation
2.7 Identify the significance of the various outcomes of Thomson’s and Rutherford’s experiments
2.8 Identify the charge, mass, and location of the three subatomic particles
2.9 Calculate the atomic mass of a given sample with a given percent abundance, and vice versa
3.1 Write the electron configuration of various atoms
3.2 Write the electron configuration of various ions
3.3 Using Aufbau’s Principle and Hund’s Rule, assign electrons to main energy levels and write energy level diagrams for atoms and ions
4.1 Use the modern Periodic Table to predict an element’s chemical and physical properties
4.2 Define atomic radii, ionic radii, ionization energy, electron affinity, and electronegativity in terms of the Periodic Table
4.3 Define valence electrons and determine the number of valence electrons for any main group elements
5.1 Define a chemical bond and calculate the electronegativity difference to determine bond type and polarity
5.2 Use the octet rule to write Lewis structures for compounds
5.3 Determine whether a given chemical is an ionic, covalent, or metallic compound
5.4 Distinguish between ionic and molecular properties
5.5 Identify and describe the metallic properties of conductivity, malleability, ductility, and luster
5.6 Differentiate how electrons behave in ionic, covalent, and metallic compounds
5.7 Use VSEPR theory to describe the geometric shape of molecules
5.8 Differentiate among dipole-dipole forces, ion-dipole forces, hydrogen bonding, and london dispersion forces
5.9 Arrange a group of chemicals in order of increasing freezing or boiling point by considering intermolecular forces
6.1 Identify the oxidation number for an element or polyatomic ion and write the correct formula for the ion and vice versa
6.2 Use the rules for assigning oxidation numbers to determine the formula for an ionic compound from its chemical name
6.3 Name ionic compounds from given chemical formulas
6.4 Write molecular formulas from the names and numbers of the atoms present
6.5 Name molecular compounds from given chemical formulas
6.6 Use oxidation numbers to name compounds and write formulas involving transition ions using the Stock System
6.7 Determine the name of an acid from a formula and derive the formula of an acid from its name
7.1 Use Avogadro’s number to differentiate between number of molecules and a mole of a substance
7.2 Use the Periodic Table to calculate the molar mass of a substance
7.3 Use molar mass to differentiate among mass and a mole of a substance
7.4 Use molar mass to calculate the percent composition of a substance
7.5 Identify a compound’s empirical formula and calculate the molecular formula from the empirical formula and other data
8.1 Correctly write a formula equation from a word equation and vice versa
8.2 Balance chemical equations
8.3 Identify and differentiate among synthesis, decomposition, single-replacement, double-replacement, and combustion reactions
8.4 Predict the products for each type of chemical reaction
8.5 Use mole ratios and dimensional analysis to solve stoichiometry problems
8.6 Use stoichiometry to determine the limiting reactant of a reaction
8.7 Use the limiting reactant to determine the amount of product and calculate percent yield
8.8 Complete net ionic equations and identify spectator ions
8.9 Define and differentiate between exothermic and endothermic chemical reactions
9.1 Use the Kinetic Molecular Theory of Matter to identify behaviors of real and ideal gases
9.2 Relate the pressure of a gas to the force exerted
9.3 Differentiate among various units of pressure
9.4 Use standard temperature and pressure to solve stoichiometric problems
9.5 Use the Combined Gas Law to solve for a gases volume, pressure, or temperature
9.6 Use Dalton’s Law of Partial Pressures to describe different mixed-gas situations
9.7 Using the Ideal Gas Law, calculate a gases volume, pressure, temperature, or amount.
9.8 Define boiling in terms of equilibrium vapor pressure
9.9 Use the ideal gas law and stoichiometry to solve application problems.
10.1 Differentiate between the solute and solvent in a solution and compare electrolytes to nonelectrolytes
10.2 Describe how changing the pressure, temperature, or surface area of a solution/solute will affect the rate of dissolution
10.3 Differentiate among unsaturated, saturated, and supersaturated solutions
10.4 Calculate how many grams of a solute are needed to make a saturated solution
10.5 Calculate the molarity of a solution with given solute and solvent
10.6 Dilute a given solution from one concentration to a weaker concentration
10.7 Calculate other measures of solution concentration, including ppt, ppm, and ppb
10.8 Use molarity to make stoichiometric calculations
11.1 Calculate the equilibrium constant for a reversible chemical reaction
11.2 Calculate the reaction quotient for a given time and a given chemical reaction and compare it to the equilibrium constant
11.3 Predict how specific stresses, including temperature, pressure, and change in concentration, will affect a chemical system at equilibrium according to Le Chatelier’s Principle
12.1 Classify a compound as an Arrhenius Acid or Base
12.2 Classify a compound as a Bronsted-Lowry Acid or Base
12.3 Identify the six strong acids
12.4 Label conjugate acid-base pairs
12.5 Determine the products of an acid-base neutralization reaction
12.6 Calculate the pH of strong acid and strong base solutions
12.7 Calculate the pH of weak acid and weak base solutions
12.8 Identify common indicators and the pH range they are used for
L1 Use Vernier Logger-Pro to make graphs and lines/curves of best fit
L2 Experimentally observe and describe chemical changes
L3 Experimentally determine the density of various objects to at least three signficant figures of precision
L4 Use Vernier Logger-Pro with Temperature Sensors to graph temperature data
L5 Experimentally determine the specific heat of a given substance
L6 Use ball-and-stick models to determine the geometric shape of various molecules
L7 Use experimental procedures (qualitative analysis) to identify various unknown chemical substances
L8 Experimentally create, compare, and contast exothermic and endothermic chemical reactions
L9 Experimentally determine the percent yield for a given chemical reaction
L10 Experimentally determine the heat of fusion for ice
L11 Experimentally determine the value for absolute zero using a Gas Pressure sensor
L12 Experimentally determine the effect of temperature on the solubility of a salt
L13 Experimentally determine the concentration of unknown salt solutions using a titration
L14 Use Vernier Logger-Pro with Colorimeters to graph colorimetry data
L15 Experimentally determine the equilibrium constant for a given reaction using a colorimeter
L16 Experimentally determine how equilibrium and stresses can affect the color of a chemical reaction
L17 Experimentally investigate and describe the titration curves of strong and weak acids and bases
L18 Experimentally and qualitatively determine the difference among solutions of an acid, base, indicator, and water
L19 Apply the methods of Experimental Design to conduct, design, and report the findings of a one-factor experiment

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