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TEXT BOOK OBJECTIVES
| Chapter 1 | Chapter 2 | Chapter 3 | Chapter 4 | Chapter 5 |
| Chapter 6 | Chapter 7 | Chapter 8 | Chapter 9 | Chapter 10 |
Chapter 1 Introduction to Chemistry
1.1 The Stories of Two Chemicals
Explain the formation and importance of ozone.
Describe the formation of ozone.
1.2 Chemistry and Matter
Define chemistry and matter.
Compare and contrast mass and weight
Explain why chemists are interested in a submicroscopic description of matter.
1.3 Scientific Methods
Identify the common steps of scientific methods
Compare and contrast types of data
Compare and contrast types of variables
Describe the difference between a theory and a scientific law
1.4 Scientific Research
Compare and contrast pure research applied research and technology.
Apply knowledge of laboratory safety
2.1 Units of Measurement
Define SI base units for time, length, mass, and temperature.
Explain how adding a prefix changes a unit.
Compare the derived units for volume and density.
2.2 Scientific Notation and Dimensional Analysis
Express numbers in scientific notation.
Use dimensional analysis to convert between units.
2.3 How reliable are measurements
Define and compare accuracy and precision
Use significant figures and rounding to reflect the certainty of data.
Use percent error to describe the accuracy of experimental data.
2.4 Representing Data
Create graphs to reveal patterns in data.
Interpret graphs
Chapter 3 Matter-Properties and Changes
3.1 Properties of Matter
Identify the characteristics of a substance
Distinguish between physical and chemical properties
Differentiate among the physical states of matter.
3.2 Changes in Matter
Define physical change and list several common physical changes.
Define chemical change and list several indications that a chemical change has taken place.
Apply the law of conservation of mass to chemical reactions
3.3 Mixtures of Matter
Contrast mixtures and substances
Classify mixtures as homogeneous or heterogeneous
List and describe several techniques used to separate mixtures.
3.4 Elements and Compounds
Distinguish between elements and compounds
Describe the organization of elements on the periodic table
Explain how all compounds obey the laws of definite and multiple proportions.
Chapter 4 The Structure of the Atom
4.1 Early Theories of Matter
Compare and contrast the atomic models of Democritus and Dalton.
Define an atom.
4.2 Subatomic Particles and The Nuclear Atom
Distinguish between the subatomic particles in terms of relative charge and mass.
Describe the structure of the nuclear atom, including the locations of the subatomic particles.
4.3 How Atoms Differ
Explain the role of atomic number in determining the identity of an atom.
Define an isotope and explain why atomic masses are not whole numbers.
Calculate the number of electrons, protons, and neutrons in an atom given its mass number and atomic number.
4.4 Unstable Nuclei and Radioactive Decay
Explain the relationship between unstable nuclei and radioactive decay.
Characterize alpha, beta, and gamma radiation in terms of mass and charge.
5.1 Light and Quantized Energy
Compare the wave and particle models of light.
Define a quantum of energy and explain how it is related to an energy change of matter.
Contrast continuous electromagnetic spectra and atomic emission spectra.
5.2 Quantum Theory and the Atom
Compare the Bohr and quantum mechanical models of the atom.
Explain the impact of de Broglie’s wave-particle duality and the Heisenberg uncertainty principle on the modern view of electrons in atoms.
Identify the relationships among a hydrogen atom’s energy levels, sublevels, and atomic orbitals.
5.3 Electron Configurations
Apply the Pauli exclusion principle, the aufbau principle, and Hund’s rule to write electron configurations using orbital diagrams and electron configuration notation.
Define valence electrons and draw electron-dot structures representing an atom’s valence electrons.
Chapter 6 The Periodic Table and Periodic Law
6.1 Development of the Modern Periodic Table
Trace the development and identify key features of the periodic table.
6.2 Classification of the Elements
Explain why elements in the same group have similar properties.
Identify the four blocks of the periodic table based on electron configuration.
6.3 Periodic Trends
Compare period and group trends of several properties.
Relate period and group trends in atomic radii to electron configuration.
7.1 Properties of s-Block Elements
Explain how elements in a given group are both similar and different.
Discuss the properties of hydrogen.
Describe and compare the properties of alkali metals and alkaline earth metals.
7.2 Properties of p-Block Elements
Describe and compare properties of p-block elements.
Define allotropes and provide examples
Explain the importance to organisms of selected p-block elements.
7.3 Properties of d-Block and f-Block Elements
Compare the electron configurations of transition and inner transition metals.
Describe the properties of transition elements.
Explain why some transition metals form compounds with color and some have magnetic properties.
8.1 Forming Chemical Bonds
Define chemical bond.
Relate chemical bond formation to electron configuration.
Describe the formation of positive and negative ions.
8.2 The Formation and Nature of Ionic Bonds
Describe the formation of ionic bonds.
Account for many of the physical properties of an ionic compound.
Discuss the energy involved in the formation of an ionic bond.
8.3 Names and Formulas for Ionic Compounds
Write formulas for ionic compounds and oxyanions.
Name ionic compounds and oxyanions.
8.4 Metallic Bonds and Properties of Metals
Describe a metallic bond
Explain the physical properties of metals in terms of metallic bonds.
Define and describe alloys.
9.1 The Covalent Bond
Apply the octet rule to atoms that bond covalently.
Describe the formation of single, double, and triple covalent bonds.
Compare and contrast sigma and pi bonds.
Relate the strength of covalent bonds to bond length and bond dissociation energy.
9.2 Naming Molecules
Identify the name of binary molecular compounds from their formulas.
Name acidic solutions.
9.3 Molecular Structures
List five basic steps used in drawing Lewis structures.
Explain why resonance structures.
Explain three exceptions to the octet rule, and identify molecules in which these exceptions occur.
9.4 Molecular Shape
Discuss the VSEPR bonding theory
Predict the shape of and the bond angles in a molecule.
Define hybridization.
9.5 Electronegativity and Polarity
Describe how electronegativity is used to determine bond type.
Compare and contrast polar and nonpolar covalent bonds and polar an non-polar molecules.
Describe the characteristics of compounds that are covalently bonded.
10.1 Reactions and Equations
Recognize evidence of chemical change.
Represent chemical reactions with equations.
10.2 Classifying Chemical Reactions
Classify chemical reactions.
Identify the characteristics of different classes of chemical reactions.
10.3 Reactions in Aqueous Solutions
Describe aqueous solutions
Write complete ionic and net ionic equations for chemical reactions in aqueous solutions.
Predict whether reactions in aqueous solutions will produce a precipitate, water, or a gas.