Chapter 1
Chemistry: The Study of Change
Upon completion of this chapter you should be able to:
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Classify materials in terms of homogeneous and heterogeneous mixtures.
Distinguish between compounds and elements.
Compare physical versus chemical properties.
Recall from memory commonly used prefixes used with SI units.
Solve problems involving density, volume, and mass.
Convert between the Kelvin, Celsius, and Fahrenheit temperature scales.
Apply scientific notation and correct number of significant figures in problem solving.
Discuss the difference between accuracy and precision.
Utilize factor-label method of problem solving.
Chapter 2
Atoms, Molecules, and Ions
Upon completion of Chapter 2 you should be able to:
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Restate the points of Dalton’s atomic theory.
Explain how electrons were discovered and how Milikan’s oil drop experiment determined the
charge of the electron.
Predict the path of alpha particles, beta particles, and gamma rays as they pass between two
oppositely charged electric plates.
Set forth how Rutherford’s experiment concluded that atoms are mostly empty space with very
small central cores, which are known as nuclei.
Predict the path of protons, electrons, and neutrons as they pass between oppositely charged
electrical plates.
Compute the number of electrons, protons, and neutrons in atoms and ions.
Give examples of isotopes.
Predict if an element is a metal, nonmetal, or metalloid.
Classify elements as alkali metals, alkaline earth metals, or noble gases.
List several examples of diatomic molecules.
Classify ions in terms of momatomic ions, polyatomic ions, cations, and anions.
Distinguish between molecular and empirical formulas.
Predict correct formulas for ionic compound
Name common ionic compounds, molecular compounds, binary acids, oxoacids and bases, given
their respective chemical formulas.
Predict the chemical formulas of common ionic compounds, molecular compounds, binary acids,
oxoacids, and bases given their respective names.
Chapter 3
Mass Relationships in Chemical Reactions
This chapter uses the concepts of conservation of mass to assist you in gaining an understanding of
chemical changes. Upon completion of Chapter 3, you should be able to:
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Convert between grams and atomic mass units (AMU’s).
Calculate average atomic mass given the mass and natural abundance of each isotope.
Recall from memory Avogadro’s number.
Determine the number of objects present in a given number of moles.
Convert between mass, number of moles, and number of atoms (molecules) of an element
(compound).
Interpret the meaning of chemical equations in terms of molecules, moles, and masses.
Distinguish between products and reactants in a chemical equation.
Use stoichiometric methods to predict the mass (number of moles) of the products formed given
the mass of each reactant (number of moles of each reactant).
Chapter 4
Reactions in Aqueous Solutions
This chapter introduces you to the concepts of reactions in aqueous solutions. Because water is used so
universally as a solvent, it is important for you to understand basic concepts of reactions that occur in it. Upon
completion of Chapter 4, you will be able to:
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Distinguish between solute, solvent, and solution.
Classify common compounds as strong electrolytes, weak electrolytes, or nonelectrolytes (stron
or weak acids or strong or weak bases.
Compare and contrast the properties of acids and bases.
List common examples of monoprotic, diprotic and triprotic acids.
Predict the products formed by acid-base neutralization reactions.
Assign oxidation numbers to elements in compounds and ions.
Compute the molarity of a solution given the mass (number of moles) of solute and the volume
of solution.
Describe the method of preparing a specific molar solution given the volume of solution required
and solute to be used.
Relate in detail how to prepare a specific dilute solution given a known stock solution using
dilution techniques.
Predict the mass of a precipitate formed using gravimetric analysis methods.
Use the terms titration, standard solution, equivalence point, and indictor to describe quantative
studies of acid-base neutralization reactions.
Determine the concentration of an unknown acid (base) given the results of an acid-base titration
Predict the amount (mass, moles, or volume of solution) of an acid (base) required to neutralize a
base (acid).
Chapter 5
Gases
This chapter examines the properties of gases. Upon completion of Chapter 5 you should be able to:
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Distinguish between the terms gas and vapor.
List four physical characteristics of all gases.
Describe how a simple barometer is constructed and how it functions.
Convert between torr, mmHg, atmospheres, and pascals.
State the difference between open-tube manometers and closed-tube manometers and indicate
how each is used.
Write, explain, and apply each of the following:
• Boyle’s law (P ∝ 1/V and P1V1 = P2V2).
• Charles’ law (P ∝ T and V1/T1 = V2/T2).
• Avogadro’s law (V ∝ n).
• Ideal gas law (PV = nRT).
Describe the Kelvin temperature scale.
Recall from memory the gas constant (R).
State what standard temperature and pressure (STP) are and demonstrate that at STP one mole of
gas occupies 22.4 liters.
Perform calculations involving density, the Ideal gas equation and molar mass.
Use the Ideal gas equation to determine the moles of a gas and use the number of moles in
stoichiometric-based problems.
State Dalton’s law of partial pressures and utilize it in problems involving mixtures of gases
including the collection of gases over water.
Define mole fraction.
Discuss the four assumptions upon which the kinetic molecular theory of gases is based.
Suggest how the kinetic molecular theory of gases qualitatively explains the following:
• The compressibility of gases.
• Boyle’s law.
• Charles’ law.
• Avogadro’s law.
• Dalton’s law of partial pressure
Describe the process of gaseous diffusion.
Argue how a real gas, behaving non-ideally, differs from an ideal gas as described by the four
assumptions in the kinetic molecular theory of gases.
Conclude under what conditions a real gas will approximate an ideal gas.
Chapter 6
Thermochemistry
This chapter develops for you the concepts of thermochemistry. Upon completion of Chapter 6, you
should be able to:
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Define and explain the following terms:
• Radiant energy
• Thermal energy
• Chemical energy
• Potential energy
• Thermochemistry
• Endothermic
• Exothermic
• Heat capacity
• Specific heat
Classify common processes as endothermic or exothermic.
Perform calculations involving specific heat, mass and temperature change.
Chapter 7
Quantum Theory and the Electronic Structure of Atoms
This chapter introduces you to quantum theory and the importance of this theory in describing electronic
behavior. Upon completion of Chapter 7, you should be able to:
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Define wavelength, frequency, and amplitude of waves.
Utilize the relationship between speed, wavelength, and frequency (hertz).
Recall from memory the speed of light (3.00 x 108 m/s).
Apply the metric unit of nano in calculations involving wavelength of light.
Use Planck’s equation to determine energy, frequency, or wavelength of electromagnetic
radiation.
Show how Bohr’s model of the atom explains emission, absorption and line spectra for the
hydrogen atom.
Compare Bohr’s model of the atom and that of the sun and surrounding planets.
Use the terms ground state and excited state to describe electronic transitions.
Recall from memory the four quantum numbers (n,ℓ, mℓ, ms) and their relationships.
Relate the values of the angular momentum quantum number, ℓ, to common names for each
orbital (s, p, d, f) and describe their shapes.
Account for the number of orbitals and number of electrons associated with each value of ℓ, the
angular momentum quantum number.
Categorize orbital energy levels in many-electron atoms in order of increasing energy.
Write the four quantum numbers for all electrons in multi-electron atoms.
Predict the electron configuration and orbital diagrams for multi-electron atoms using the Pauli
exclusion principle and Hund’s rule.
Derive the ground state electron configuration of multi-electron atoms using the Aufbau
principle.
Chapter 8
Periodic Relationships Among the Elements
This chapter presents a qualitative view of the periodic (repeating) relationships of the elements in the
periodic table. Upon completion of Chapter 8 you should be able to:
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Explain the basis of the periodic table as described by Mendeleev and Meyer and indicate the
shortcomings of their methods.
Explain the basis of the periodic table as described by Moseley and how it predicted properties of
“missing” elements.
Identify elements that correspond to each of the following groups:
• representative elements
• noble gas
• transition metals
• lanthanides
• actinides
Describe the electron configuration of cations and anions and identify ions and atoms that are
isoelectronic.
Predict the trends from left to right and top to bottom of the periodic table for each of the
following:
• atomic radius
• ionic radius
• ionization energy
• electron affinity
• metallic character
Identify the metals, nonmetal, and metalloids of Group 4A.
List halides (halogens)
Classify oxides as acidic, basic, or amphoteric.
Chapter 9
Chemical Bonding I: Basic Concepts
Upon completion of Chapter 9 you should be able to:
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Rationalize why alkali metals and alkaline earth metals usually form cations and oxygen and the
halogens form anions using Lewis dot symbols in the discussion.
Use Lewis dot symbols to show the formation of both ionic and molecular compounds.
Identify covalent compounds, the type of covalent bonds present, and the number of lone pairs of
electrons using Lewis structures.
Relate types of bonds to bond length and bond strength.
Compare and contrast various properties expected for ionic compounds versus covalent
compounds.
Identify ionic, polar covalent and (nonpolar) covalent bonds using the concepts of
electronegativity.
Predict the relative changes in electronegativity with respect to position on the periodic table.
Use the concept of electronegativity to rationalize oxidation numbers.
Use Lewis dot and the octet rule to write Lewis structures of compounds and ions.
Chapter 12
Intermolecular Forces and Liquids and Solids
This chapter introduces you to the concepts that are used to explain the properties of liquids and solids.
Upon completion of this chapter you should be able to:
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Characterize the properties of gases, liquids and solids in terms of density, compressibility and motion
of molecules.
Distinguish between intermolecular and intramolecular forces.
Identify and give examples of the following forces.
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ion – ion
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ion – dipole
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ion – induced dipole
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dipole – dipole
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dipole – induced dipole
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induced dipole – induced dipole
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van der Waals
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dispersion
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hydrogen bonding
Suggest why H2O, HF and NH3 do not follow the expected trend as shown by the plot Figure 11.7
Use the concepts of intermolecular forces to explain surface tension, capillary action, cohesion, adhesion
and viscosity.
Describe the structure of water and relate it to why ice is less dense then water.
Distinguish between crystalline and amorphous solids and give examples of each.
Determine the number of atoms contained in a unit cell for simple cubic, face-centered cubic and bodycentered cubic structures.
Characterize ionic, covalent, molecular and metallic crystals including general properties and examples
of each.
Discuss the following:
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evaporation
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condensation
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molar heat of vaporization
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molar heat of fusion
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boiling point
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melting point
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supercooling
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sublimation
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deposition
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molar heat of sublimation
Chapter 13
Physical Properties of Solutions
Upon completion of this chapter, you should be able to:
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Using the terms saturated, unsaturated and supersaturated to describe solutions.
Distinguish between crystallization and precipitation.
Define colligative properties and give four examples (vapor – pressure lowering, freezing – point
lowering, boiling – point elevation and osmotic pressure).
Perform calculations involving boiling-point elevation, freezing-point depression, Kf, Kb and molality.
Use the concepts of osmotic pressure to describe the processes of osmosis and reverse osmosis.
Describe the following terms:
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semi-permeable membrane
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isotonic
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hypertonic
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hypotonic
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crenation
Use the concepts of colligative properties to determine molar mass.
Chapter 15
Chemical Equilibrium
Upon completion of this chapter you should be able to:
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Describe chemical equilibrium using the terms forward and reverse reactions and dynamic process.
Use LeChatelier’s Principle to describe how changing concentration, volume, pressure, or temperature
will shift the reaction so that a equilibrium will be maintained.