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Ch 01 Chemical Foundations
1.1 Chemistry: An Overview
1.2 The Scientific Method
list and describe the scientific method; define scientific models (including theory and law)
1.3 Units of Measurement
list the SI units and correlate them with the types of data they measure
1.4 Uncertainty in Measurement
calculate with significant figures; define the types of uncertainty and explain how they affect measurements; calculate with measurement and account for errors including systematic and random errors; differentiate between precision and accuracy
1.5 Significant Figures and Calculations
determine the number of significant figures in a measurement; calculate using significant figures
1.6 Dimensional Analysis
use dimensional analysis to convert between units
1.7 Temperature
use the Kelvin scale to measure temperatures; convert between Celsius and Kelvin
1.8 Density
describe density as a ratio of mass per unit volume; explain that a graph of mass vs. volume is a straight line and the slope is equal to density; calculate the density, mass, or volume using the density equation; explain that density is a ratio and can be used as a conversion factor
1.9 Classification of Matter
explain that pure substances have definite ratios and mixtures have ratios that can vary; describe elements and compounds as pure substances; differentiate between heterogeneous and homogeneous mixtures; describe the methods used to separate mixtures
Ch 02 Atoms, Molecules and Ions
2.1 The Early History of Chemistry
2.2 Fundamental Chemical Laws
law of conservation of mass; law of definite proportions, law of multiple proportions
2.3 Dalton's Atomic Theory
list the postulates of Dalton's atomic theory; explain the modern modifications made to Dalton's atomic theory
2.4 Early Experiments to Characterize the Atom
describe the evidence for modern atomic theory; describe Thomson's cathode ray experiment and the discovery of the electron, Describe Rutherford 's gold foil experiment and the discovery of the nucleus; explain how the model of the atom changed to include a nucleus;describe Chadwicke's experiment and the discovery of the neutron
2.5 The Modern View of Atomic Structure: An Introduction
explain how to determine the atomic number and mass number of an atom; explain the significance of atomic number; define isotope and explain how their properties differ
2.6 Molecules and Ions
describe covalent and ionic bonds; chemical structural formulas;
2.7 An Introduction to the Periodic Table
explain the pattern for common ions for certain groups
2.8 Naming Simple Compounds
explain the rules for naming binary molecular and molecular compounds; describe how to use Roman numerals to indicate the charge of cations of the d-block; describe the correlation between oxidation state and name for polyatomic ions; name binary acids; organization of the periodic table; nomenclature of binary compounds (cations of metals that form one charge; cations of metals that form more than one charge, monatomic and polyatomic anions, or two nonmetals) nomenclature of compounds containing polyatomic ions (per-ate, -ate, -ite, hypo-ite); nomenclature of acids (containing oxygen, not containing oxygen)
Ch 03 Stoichiometry
3.1 Counting by Weighing
3.2 Atomic Masses
3.3 The Mole
3.4 Molar Masses
3.5 Learning to Solve Problems
3.6 Percent Composition of Compounds
3.7 Determining the Formula of a Compound
3.8 Chemical Equations
3.9 Balancing Chemical Equations
3.10 Stoichiometric Calculations
3.11 The Concept of Limiting Reagent
Ch 04 Types of Chemical Reactions and Solution Stoichiometry
4.1 Water Common Solvent
explain how/why water dissolves many ionic and polar substances; describe the process of hydration; relate the water to ion attraction relative to the ion to ion attraction for soluble substances.
4.2 The Nature of Aqueous Solutions
differentiate between solute and solvent; explain why/hoe an electrolyte can conduct electricity and differentiate between strong, weak and nonelectrolytes; describe the dissociation of strong acids; describe the dissociation of strong soluble bases; explain why strong acids and strong bases are strong electrolytes; explain why weak acids and weak bases are weak electrolytes; explain the "dissociation" nonelctrolytes.
4.3 The Composition of Solutions
explain how molarity is used to quantify the concentration of a solution; explain how the process of dilution affects the number of moles of solute.
4.4 Types of Chemical Reactions
list and describe the three main types of chemical reactions.
4.5 Precipitation Reactions
identify the characteristics of a precipitate reaction; write complete ionic equations for double displacement reactions; use the solubility rules to predict the product of a precipitate reaction.
4.6 Describing Reactions in Solutions
differentiate between formula equations and complete ionic equations; write net ionic equations; describe spectator ions.
4.7 Stoichiometry of Precipitation Reactions
use molarity as a ratio to find moles to perform stoichiometric calculations for reactions involving solutions of known concentration.
4.8 Acid-Base Reactions
explain the difference between an acid and a base using the Bronsted-Lowry model; explain how neutralization reactions occur; describe a titration and explain its purpose; explain how to identify the the endpoint of a titration.
4.9 Oxidation-Reduction Reactions
differentiate between a reaction that is redox and one that is not; identify the substance oxidized and the substance reduced; identify the oxidizing agent and the reducing agent; write half reactions for the substance oxidized and the substance reduced; balance redox reactions by balancing the change in electrons
Ch 05 Gases
Ch 06 Thermochemistry
6.1 The Nature of Enegry
Objectives: describe
6.2 Enthalpy and Calorimetry
Objectives: describe
6.3 Hess's Law
Objectives: describe
6.4 Standard Enthalpies of Formation
Objectives: describe
6.5 Present Sources of Energy
Objectives: describe
6.6 New Energy Sources
Objectives: describe
Ch 07 Atomic Structure and Periodicity
7.1 Electromagnetic Radiation
explain the relationship among wavelength, frequency, energy and speed of light
7.2 The Nature of Matter
describe the significance of Planck’s constant; explain that energy is quantized; describe the photoelectric effect and the minimum energy needed to eject an electron
7.3 The Atomic Spectrum of Hydrogen
describe the line emission spectrum of hydrogen;
7.4 The Bohr Model
Bohr model; excited and ground state electrons; (calculation of energy for transitions of hydrogen electron from one level to another)
7.5 The Quantum Mechanical Model of the Atom
describe the quantum mechanical model of the atom and how it is related to the wave function and orbitals; explain the significance of Heisenberg's uncertainty principle;
7.6 Quantum Numbers
determine the four quantum numbers and explain their significance
7.7 Orbital Shapes and Energies
list orbital shapes and energies; explain the effect of nodes; define degenerate orbitals
7.8 Electron Spin and the Pauli Principle
describe electron spin; explain the significance of the electron spin quantum number and how it relates to the Pauli exclusion principle
7.9 Polyelectronic Atoms
explain that the energies of orbitals in a polyelectronic atom are not equal as they are in the hydrogen atom
7.10 The History of the Periodic Table
7.11 The Aufbau Principle and The Periodic Table
use the Aufbau principle to write electron configurations; apply Hund’s rule to degenerate electrons; determine the number of valence and core electrons; relate the quantum mechanical model to the order of the periodic table; describe the periodic trends of atomic properties; determine the energy of first, second, and third ionization and use it to identify the common charge for the element; describe the trend of electron affinity; describe the trend of atomic radius; explain what type of information can be found from the periodic table (by groups); list some properties of alkali metals
Ch 08 Bonding: General Concepts
8.1 Types of Chemical Bonds
relate bond strength to bond energy; define ionic bonding and ionic compounds; define covalent bonding and covalent compounds (molecules); explain how bond length is related to the energy of the system; differentiate between nonpolar and polar covalent bonds
8.2 Electronegativity
define electronegativity; describe the periodic trend
8.3 Bond Polarity and Dipole Moments
relate bond polarity to dipole moment; explain how a molecule can have a dipole
8.4 Ions: Electron Configurations and Sizes
use electron configurations to predict the formula for an ionic compound; compare the size of an ion to its corresponding atom; define isoelectronic and group ions that are isoelctronic
8.5 Energy Effects in Binary Ionic Compounds
define lattice energy
8.6 Partial Ionic Character of Covalent Bonds
describe the percent ionic character of a bond as a relationship between the measure dipole moment and the calculated dipole moment
8.7 The Covalent Chemical Bond: A Model
explain why chemical bonds occur
8.8 Types of Chemical Bonds
relate the energy and length of a bond to its type (single, double, triple); use bond energies to calculate the approximate energy of a reaction; relate breaking and forming bonds to the energy change; use bond energy to calculate the approximate enthalpy change of a reaction
8.9 The Localized Electron Bonding Model
define localized electrons
8.10 Lewis Structures
write Lewis structures for molecules; explain what type of electrons are shown in Lewis structures; explain the duet and octet rules relating both to noble gas configurations; explain that shared electrons form bonds
8.11 Exceptions to the Octet Rule
write Lewis diagrams for incomplete octets using Be and B; write Lewis structures for expanded octets using 3rd row elements and higher
8.12 Resonance
explain that resonance structures occur when more than one correct structure can be drawn for the same molecule; write resonance structures; write Lewis structures that have odd numbers of electrons; apply formal charge to atoms in Lewis structures
8.13 Molecular Structure: The VSEPR Model
apply VSEPR theory to predict the shape of molecules; explain that lone pair electrons require more room and affect the shape of molecules; apply VSEPR theory to resonance structures
Ch 09 Covalent Bonding: Orbitals
9.1 Hybridization & Localized Electron Model
using the localized electron model, explain that the process of hybridization involves the mixing of orbitals; describe the hybrid orbitals designated as sp, sp2, sp3, dsp3, d2sp3
9.2 The Molecular Orbital Model
describe bonding using the molecular orbital model; describe the electron distribution called sigma molecular orbitals; differentiate between bonding and antibonding molecular orbitals; determine the bond order of a molecule and relate it to the stability of the molecule
9.3 Bonding in Homonuclear Diatomic Molecules
describe the bonding in homonuclear diatomic molecules; describe the electron distribution called pi molecular orbitals; explain that paramagnetism is caused by unpaired electrons
9.4 Bonding in Heteronuclear Diatomic Molecules
describe the bonding in heteronuclear diatomic molecules;
9.5 Combining the Localized Electron and molecular Orbital Models
use both the localized electron and molecular orbital models to describe resonance; explain that sigma bonds in a molecule are localized; explain that pi bonds in a molecule are delocalized
Ch 10 Liquids and Solids
10.1 Intermolecular Forces
differentiate between intermolecular forces and intramolecular forces; explain that phase changes involve changes in the forces between different molecules; describe dipole-dipole forces, hydrogen bonding, and London dispersion forces
10.2 The Liquid State
describe surface tension and cohesion and relate them to intermolecular forces; explain that polar liquids exhibit capillary action and involve cohesive and adhesive forces; explain that the structure of liquids is dynamic and involves more disorder than solids
10.3 Intro to the Structures & Types of Solids
distnguish between crystalline and amorphous solids; describe ionic, molecular and atomic solids
10.4 Structure and Bonding in Metals
describe the crystal arrangement called closest packing; explain the bonding of metals using the band model and the molecular orbital model; define alloy; differentiate between substitutional and interstitial alloys
10.5 Carbon and Silicon: Network Atomic Solids
explain that atomic network solids can be viewed as a giant molecule; differentiate between graphite and diamond; explain that ceramics are based on silicates which contain silicon-oxygen anions and a cation; describe the n-type and p-type semiconductors and the application p-n junction
10.6 Molecular Solids
describe the forces that exist between the molecules of molecular solids
10.7 Ionic Solids
describe the closest packing arrangements of ionic solids
10.8 Vapor Pressure and Changes of State
differentiate between vaporization and evaporation; define the vapor pressure of a liquid; explian how vapor pressure changes with temperature; analyze a heating curve; describe the heat of fusion as the enthalpy change that occurs at the melting point
10.9 Phase Diagrams
analyze a phase diagram and label its parts; define the triple point
Ch 11 Properties of Solutions
11.1 Solution Composition
describe the factors that affect solubility; describe solution composition using molarity, mass percent, mole fraction, and molality
11.2 The Energies of Solution Formation
list and describe the steps of the formation of a solution; define the enthalpy of solution;
11.3 Factors Affecting Solubility
Objectives: describe
11.4 The Vapor Pressure of Solutions
Objectives: describe
11.5 Boiling-Point Elevation and Freezing-Point Depression
Objectives: describe
11.6 Osmotic Pressure
Objectives: describe
11.7 Colligative Properties of Electrolyte Solutions
Objectives: describe
11.8 Colloids
Objectives: describe
Ch 12 Chemical Kinetics
12.1 Reaction Rates
define reaction rate in terms of concentration of reactant or product and time; explain how to determine the instantaneous rate of a reaction; account for stoichiometry when describing reaction rate in terms of a product.
12.2 Rate Laws: an Introduction
define and write a rate law for a reaction; define rate constant; explain how the order of a reaction is represented in an equation and how it is determined; explain the difference between integrated and differential rate laws.
12.3 Determining the Form of the Rate Law
describe the method of initial rates; use initial rates and initial concentrations to determine reaction order; determine the overall reaction order from a rate law.
12.4 The Integrated Rate Law
use the integrated rate laws (1st, 2nd, or zero) to determine the order of a reaction; use the slope of a line to calculate rate constant; use the y-intercept to calculate [A]0 ; define and calculate half life; explain how successive half lives vary for 1st, 2nd, and zero order reactions.
12.5 Reaction Mechanisms
define reaction mechanism; describe an intermediate; define molecularity and list the types; explain how molecularity is related to rate law; describe the requirements for a reaction mechanism; write a rate law using the rate determining step.
12.6 A Model for Chemical Kinetics
use kinetic molecular theory to describe the role and limitations of collisions in reaction rates; describe the effects of activation energy on reaction rates; graphically represent the potential energy of a reaction indicating the reactant, Ea, and product energies; describe transition state; explain how energy and molecular orientation affect rate of reaction; use the Arrhenius equation to determine Ea and frequency factor of a reaction; use a derivation of the Arrhenius equation to calculate Ea from various rate constants and their temperatures.
12.7 Catalysis
Objectives: describe
Ch 13 Chemical Equilibrium
13.1 The Equilibrium Condition
Objectives: describe characteristics of equilibrium systems
13.2 The Equilibrium Constant
Objectives: write the equilibrium expression for a reaction; explain the significance of the equilibrium constant
13.3 Equilibrium Expressions Involving Pressures
Objectives: describe equilibrium expressions involving pressure; the relationship between Kp and Kc;
13.4 Heterogeneous Equilibria
Objectives: write equilibrium expressions for heterogeneous systems
13.5 Applications of the Equilibrium Constant
Objectives: describe the relationship of equilibrium constant K and reaction quotient Q
13.6 Solving Equilibrium Problems
Objectives: describe perform calculations to find K from equilibrium concentration data; determining equilibrium concentrations (and pressures) from K and initial concentrations
13.7 Le Chateliers Principle
Objectives: describe Le Chatelier’s principle and the effect of concentration changes, pressure changes, temperature changes on the shift in equilibrium
Ch 14 Acids and Bases
14.1 The Nature of Acids and Bases
Objectives: describe Arrhenius and Bronsted-Lowry models of acids and bases;
14.2 Acid Strength
Objectives: distinguish between conjugate acid-base pairs; use Ka to determine acid strength and equilibrium concentrations; determine the relative strengths of conjugates; compare strong vs. weak acids and bases; describe the amphoterism of water,
14.3 The pH Scale
Objectives: use Kw to calculate pH; use the pH scale; calculate pH and pOH;
14.4 Calculating the pH of Strong Acid Solutions
Objectives: calculate pH of strong and weak acid solutions using ICE tables and equilibrium constants; calculating pH of strong and weak bases, Kb; Percent dissociation H
14.9 The Effect of Structure on Acid-Base Properties
Objectives: describe
14.10 Acid-Base Properties of Oxides
Objectives: describe
14.11 The Lewis Acid-Base Model
Objectives: describe
14.12 Strategy for Solving Acid-Base Problems
Objectives: describe
Ch 15 Acid-Base Equilibria
15.1 Solutionsof Acids or Bases Containing a Common Ion
Objectives: describe
15.2 Buffered Solutions
Objectives: describe
15.3 Buffering Capacity
Objectives: describe
15.4 Titration and pH Curves
Objectives: describe
15.5 Acid-Base Indicators
Objectives: describe
Ch 16 Solubility and Complex Ion Equilibria
Ch 17 Spontaneity, Entropy, and Free Energy
Ch 18 Electrochemistry
Ch 19 The Nucleus: A Chemist's View
19.1 Nuclear Stability and Radioactive Decay
Objectives: define thermodynamic stability and kinetic stability; describe the beta particle and how it is produced; identify the zone of stability in a plot of number of neutrons vs. number of protons; describe an alpha particle and how it is produced; describe gamma rays; explain how positrons are produced; describe the process of electron capture; balance nuclear equations.
19.2 The Kinetics of Radioactive Decay
Objectives: describe and calculate the rate of decay; describe and calculate half-life.
19.3 Nuclear Transformations
Objectives: describe particle accelerators, cyclotrons, and linear accelerators including the transformations that occur in them.
19.4 Detection and Uses of Radioactivity
Objectives: explain how a Geiger-Miller counter works to detect radiation; explain how a scintillation counter works; describe the process of radiocarbon dating (carbon-14 dating); explain how radiotracers are used in medical applications.
19.5 Thermodynamic Stability of the Nucleus
Objectives: describe the effect of mass defect in the formation of matter; explain the significance of and calculate binding energy.
19.6 Nuclear Fission and Nuclear Fusion
Objectives: differentiate between nuclear fission and nuclear fusion; define chain reaction and subcritical, critical and supercritical mass;explain how nuclear reactors work and the purpose for reactor core, moderator, and control rods; explain how a breeder reactor works.
19.7 Effects of Radiation
Objectives: describe the damage of radiation; differentiate between somatic and genetic damage; list the units of radiation.
Ch 20 The Representative Elements
Ch 21 Transition Metals and Coordination Chemistry
Ch 22 Organic and Biological Molecules
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