Chemistry/PreAP Chem - Grade 10-11

Chemistry/PreAP Chem

Scienfic Inquiry

Mathematics and Measurement in Science

Science in Practice

Mass, Volume, and Density

Elements, Atomic Mass, and Nomenclature

Phases of Matter, Phase Changes, and Physical Changes

The Nature of Gases

Ideal Gas Law

Empirical Formulas, Molecular Formulas, and Percentage Composition

 Mole Concept, Molar Mass, Gram Formula Mass, and Molecular Mass

Chemical Equations and Stoichiometry

Structure of Liquids and Solids

Kinetic Molecular Theory of Gases 

Atomic Theory (Dalton), Atomic Structure, and Quantum Theory 

Periodic Table and Periodicity

Intermolecular Forces and Types of Bonds

 Orbital Theory Applied to Bonding 

Types of Solutions, Concentration, and Solubility

Colligative Properties

Chemical Equilibrium and Factors Affecting Reaction Rates; Le Châtelier’s Principle 

Mechanism, Rate-Determining Step, Activation Energy, and Catalysts

Chemical Processes and Heat; Calorimetry

Enthalpy and Entropy

Acid/Base Theories

Acid/Base Constants and pH; Titration; Buffers 

Nuclear Chemistry

Idenfy and clarify research quesons and design experiments 

Design experiments so that variables are controlled and appropriate numbers of trials are used 

Collect, organize, and analyze data accurately and use techniques and equipment appropriately

Interpret results and draw conclusions, revising hypotheses as necessary and/or formulang addional quesons or explanaons 

Write and speak effecvely to present and explain scienfic results, using appropriate terminology and graphics

Safely use laboratory equipment and techniques when conducting scientific investigaons 

Routinely make predictions and estimates

Disnguish between precision and accuracy with respect to experimental data 

Use appropriate SI units for length, mass, me, temperature, quantity of measure, area, volume, and density; describe the relaonships among SI unit prefixes (e.g., cen-, milli-, kilo-); recognize commonly used non-SI units

Use the correct number of significant figures in reporting measurements and the results of calculaons

Use appropriate statistical methods to represent the results of investigations

Express numbers in scientific notation when appropriate

Solve for unknown equations by manipulating variables

Use graphical, mathematical, and/or statistical models to express patterns and relaonships inferred from sets of scienfic data 

Explain and apply criteria that sciensts use to evaluate the validity of scienfic claims and theories

Explain why experimental replication and peer review are essenal to eliminate as much error and bias as possible in scienfic claims

Explain the criteria that explanations must meet to be considered scientific (e.g., be consistent with experimental/observational evidence about nature, be open to critique and modification, use ethical reportage methods and procedures)

Explain why all scienfic knowledge is subject to change as new evidence becomes available to the scienfic community

Use a variety of appropriate sources (e.g., Internet, scienfic journals) to retrieve relevant informaon; cite references properly

Idenfy and analyze the advantages and disadvantages of widespread use of and reliance on technology

Compare the scienfic definions of fact, law, and theory, and give examples of each in chemistry

Explain why mass is used as a quantity of matter and differentiate between mass and weight

Explain density qualitavely and solve density problems by applying an understanding of the concept of density

Use the IUPAC symbols of the most commonly referenced elements

Compare the characteriscs of elements, compounds, and mixtures

Compare characteriscs of isotopes of the same element 

Compare the definion of matter and energy and the laws of conservation of matter and energy

Describe how matter is classified by state of matter and by composition 

Describe the phase and energy changes associated with boiling/condensing, melting/freezing, sublimation, and crystallization (deposition) 

Explain the difference between chemical and physical changes and demonstrate how these changes can be used to separate mixtures and compounds into their components

Define chemical and physical properties and compare them by providing examples

Define gas pressure and the various pressure units (e.g., torr, kilopascals, mm Hg, atmospheres) 

Describe the use and operation of mercury barometers and manometers to find atmospheric pressure or relative gas pressures

Define the gas laws given by Boyle, Charles, Gay-Lussac, and Dalton and solve problems based on these laws

Predict boiling point changes based on changes in atmospheric pressure

Explain the basis for gaseous diffusion and effusion 

Describe Avogadro’s hypothesis and use it to solve stoichimoetric problems 

Explain the difference between an ideal and real gas, the assumptions made about an ideal gas, and what conditions favor ideal behavior for a real gas

Apply the mathematical relationships that exist among the volume, temperature, pressure, and number of particles in an ideal gas

Compute gas density when given molar mass, temperature, and pressure

Apply the ideal gas law to determine the molar mass of a volatile compound

Solve gas stoichiometry problems at standard and nonstandard conditions

Distinguish between chemical symbols, empirical formulas, molecular formulas, and structural formulas

Interpret the informaon conveyed by chemical formulas for numbers of atoms of each element represented

Use the names, formulas, and charges of commonly referenced polyatomic ions

Provide the interconversion of molecular formulas, structural formulas, and names, including common binary and ternary acids

Calculate the percent composition of a substance, given its formula or masses of each component element in a sample

Determine the empirical formulas and molecular formulas of compounds, given percent composition data or mass composition data

Determine percent composition experimentally and derive empirical formulas from the data (e.g., for hydrates) 

Explain the meaning of mole and Avogadro’s number

Interconvert between mass, moles, and number of particles

Disnguish between formula mass, empirical mass, molecular mass, gram molecular mass, and gram formula mass

Explain how conservation laws form the basis for balancing chemical reactions and know what quantities are conserved in physical, chemical, and nuclear changes 

Write and balance chemical equations, given the names of reactants and products

Describe what is represented, on a molecular and molar level, by chemical equations

Use the appropriate symbols for state (i.e., solid, liquid, gaseous, aqueous) and reaction direction when wring chemical equations

Classify chemical reactions as being synthesis, decomposition, single replacement, or double replacement reacitons

Predict the products of synthesis, combustion, and decomposition reactions and write balanced equations for these reactions

Predict products of single replacement reactions, using the activity series, and write balanced equations for these reactions

Predict the products of double replacement reactions, using solubility charts to identify precipitates, and write balanced equation for these reactions 

Use chemical equation to perform basic mole-mole, mass-mass, and mass-mole computations for chemical reactions 

Identify liming reagents and use this information when solving reaction stoichiometry problems

Compute theorecal yield, actual (experimental) yield, and percent yield

Calculate percent error and analyze experimental errors that affect percent error

Write ionic equations, identifying spectator ions and the net ionic equation 

Describe differences between solids, liquids, and gases at the atomic and molecular levels

Describe and perform common separation techniques (e.g., filtration, distillation, chromatography) 

Use the kinetic molecular theory to explain the states and properties (i.e., microscopic and macroscopic) of matter and phase changes

Explain the basis and importance of the absolute temperature scale and convert between the Kelvin and Celsius scales

Use the kinetic-molecular theory as a basis for explaining gas pressure, Avogadro’s hypothesis, and Boyle’s/Charles’s laws

Describe the importance of models for the study of atomic structure

Describe the crucial contributions of scientists and the critical experiments that led to the development of the modern atomic model

Describe characteriscs of a wave, such as wavelength, frequency, energy, and speed

Describe atomic orbitals (s, p, d, f) and their basic shapes

Apply Hund’s rule and the Aufbau process to specify the electron configurations of the elements 

Describe the historical development of the modern periodic table, including work by Mendeleev and then Moseley 

Describe and explain the organizaon of elements into periods and groups in the periodic table

Use the periodic table to determine the atomic number; atomic mass; mass number; and number of protons, electrons, and neutrons in isotopes of elements 

Calculate the weighted average atomic mass of an element from isotopic abundance, given the atomic mass of each contributor 

Idenfy regions (e.g., groups, families, series) of the periodic table and describe the chemical characteriscs of each

Compare the periodic properties of the elements (e.g., metal/nonmetal/metalloid behavior, electrical/heat conductivity, electronegativity and electron affinity, ionization energy, atomic/covalent/ionic radius) and how they relate to poison in the periodic table 

Use the periodic table to predict and explain the valence electron configuraons of the elements, to idenfy members of configuraon families, and to predict the common valences of the elements

Describe the characteriscs of ionic and covalent bonding 

Explain ionic stability, recognize typical ionic configuraons, and predict ionic configuraons for elements (e.g., electron configuraons, Lewis dot models) 

Describe the nature of the chemical bond with respect to valence electrons in bonding atoms

Explain how ionic and covalent compounds differ

Describe the unique features of bonding in carbon compounds

Compare the different types of intermolecular forces (e.g., van der Waals, dispersion)

Explain and provide examples for dipole moments, bond polarity, and hydrogen bonding

Describe the unique physical and chemical properties of water resulting from hydrogen bonding 

Explain the relationship between evaporation, vapor pressure, molecular kinetic energy, and boiling point for a single pure substance

Explain the relationship between intermolecular forces, boiling points, and vapor pressure when comparing differences in the properties of pure substances

Classify solids as ionic, molecular, metallic, or network

Use Lewis dot diagrams to represent bonding in ionic and covalent compounds

Draw Lewis structures for molecules and polyatomic ions, including those that must be represented by a set of resonance structures

Use VSEPR theory to explain geometries of molecules and polyatomic ions 

Describe how orbital hybridizaon models relate to molecular geometry

Describe the molecular orbital models for double bonds, triple bonds, and delocalized pi electrons

Describe the relaonship between molecular polarity and bond polarity

Define solution, solute, and solvent

Compare properties of suspensions, colloids, and true solution

Define the terms saturated, unsaturated, supersaturated, dilute, and concentrated as they pertain to solution

Give examples of solid, liquid, or gas medium solution

Define and calculate the molarity of a solution

Define and calculate the percent composition of a solution

Describe the preparation and properties of solutions

Solve stoichiometry calculations based on reactions involving aqueous solutions

Describe the relaonship between temperature or pressure and the solubility of gases in liquids

Describe the relaonship between solvent character and solute character and explain miscibility

Apply the general rules of solubility to aqueous salt solutions

Describe the factors affecting the solubility of a solute in a given solvent and its rate of solution

Describe qualitavely the effect of adding solute on freezing point, boiling point, and vapor pressure of a solvent

Define molality and mole fraction 

Calculate changes in the boiling point and freezing point when nonvolale, nonelectrolyte solutes are added to solvents

Explain the collision theory of reactions

Analyze factors (e.g., temperature, nature of reactants) affecng reaction rates in relation to the kinetic theory

Relate reaction mechanism, rate-determining step, activated complex, heat of reaction, and activation energy to reaction kinetics

Interpret potenal energy diagrams for chemical reactions

Describe the conditions that define equilibrium systems on a dynamic molecular level and on a static macroscopic scale

Apply Le Châtelier’s principle to explain a variety of changes in physical and chemical equilibria

Define Ksp and manipulate Ksp to predict solubility

Explain the law of concentration (mass) action and write equilibrium law expressions for chemical equilibrium

Determine solubility product constants from soluibles (and vice versa) for a given solubility equilibrium system 

Relate the rate of a chemical reaction to the appearance of products and the disappearance of reactants

Describe the meaning of reaction mechanism and rate-determining step

Relate collision theory to the factors that affect the rate of reaction

Describe the meaning of activation energy and acvated complex 

Interpret and label a plot of energy versus reaction coordinate

Explain the effects of catalysts on reaction rates (e.g., mechanism, activation energy/activated complex)

Explain the law of conservation of energy in chemical reactions

Describe the concept of heat, and explain the difference between heat energy and temperature.

Explain physical and chemical changes as endothermic or exothermic energy changes

Solve heat capacity and heat transfer problems involving specific heat, heat of fusion, and heat of vaporizaon

Calculate the heat of reaction for a given chemical reaction when given calorimetric data

Define enthalpy and explain how changes in enthalpy determine whether a reaction is endothermic or exothermic

Compute ΔHrxn from ΔHfº values and explain why the ΔHfº values for elements are zero

Explain and apply, mathemacally, the relaonship between ΔHrxnº (forward) and ΔHrxnº (reverse)

Define entropy and explain the role of entropy in chemical and physical changes, and explain the changes that favor increases in entropy

Describe the nature and interacons of acids and bases

Describe the hydronium ion and the concept of amphoterism

Describe Arrhenius and Brønsted-Lowry acids and bases; identify conjugate acids and bases in reactions

Relate solvent interaction to the formation of acidic and basic solutions

Define the water constant, Kw, and the pH scale

Describe characteriscs of strong and weak acids and bases, and idenfy common examples of both

Write and balance a simple equaon for a neutralizaon reaction

Calculate hydrogen ion concentration, hydroxide ion concentration, pH, and pOH for acidic or basic solutions

Explain how the acid-base indicators work

Define percent ionizaon, Ka, and Kb and explain how they relate to acid/base strength

Conduct a titration experiment in order to determine the concentration of an acid or base solutions

Qualitatively understand the behavior of a buffer and explain why buffer solutions maintain pH upon diluon

Describe alpha, beta, and gamma decay, half-life, and fission and fusion

Write appropriate equations for nuclear decay reactions, using particle balance; describe how the nucleus changes during these reactions and compare the resulting radiation with regard to penetrating ability