Download Chem 20 Final Exam Outline

Chem 20 Final Exam Outline
Molecules and Compounds
Use the formulas and names of compounds fluently
Chapter 2: sections 2-5 to 2-6, 2-9, 2-12, 2-15 to 2-19
Chapter 23: section 23-6
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Recognize the component atoms, simple ions, or polyatomic ions in a molecule.
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Use both the periodic table and a table of common ions to aid in determining the
formulas of binary and other simple compounds.
Use a table of common ions in determining the formulas of compounds containing
one or more polyatomic ions.
Write the formula of an inorganic compound, given its name.
Use the oxidation state notation to describe the valence of polyvalent elements,
e.g. Fe(III).
Write the name of an inorganic compound, given the formula.
Recognize the pattern in the names of the alkane and alkene series.
Apply the general formula CnH2n+2 for alkanes and CnH2n for alkenes to write
formulas for members of those series.
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Discuss the mechanics of bonding between atoms in a molecule.
Chapter 12: sections 12-1 to 12-6, and 12-11
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Recall the structure of the atom.
Understand the importance of the interaction of electrons when two atoms or ions
approach each other.
Contrast the bonding produced by shared pairs of valence electrons and by
transfer of electrons to form ions.
Apply the octet rule to determine the number of covalent bonds which form or the
charge of the ion which forms.
Draw Lewis structures for molecules.
Use VSEPR theory to predict shapes of simple molecules.
Examine the bonding between molecules or atoms in solid and liquid
phases.
Chapter 12: sections 12-12 to 12-14
Chapter 15: sections 15-3 to 15-5, 15-7, 15-9 to 15-11
Chapter 16: section 16-2
Handouts on alcohols from Chemistry a First Course
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Describe the physical properties of ionic, metallic, covalent (molecular), covalent
(network), and van der Waals solids.
Relate the properties of compounds to the uses which those compounds have.
Compare the properties of some alkanes to the properties of their derivative
alcohols, e.g. methane-methanol, propane-propanol, octane-octanol.
Explore the relationship between the strength of the forces holding solids and
liquids together and the magnitude of the melting and boiling points of those
substances.
Investigate the factors which influence solubility.
Chapter 16: sections 16-1 to 16-4
Handouts on alcohols from Chemistry a Second Course
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Recognize the importance of water as a solvent.
Use the terminology related to solubility.
Compare the solubilities of several solute/solvent combinations.
Recognize how the addition of a solute changes the properties of a solvent.
Chemical Reactions
Acquire ability to communicate chemical information through equations
for reactions.
Chapter 5: sections 5-1, 5-3 to 5-11
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Write an equation representing a chemical reaction using chemical formulas for
the species involved.
Recognize that chemical equations need to be balanced for number of atoms and
for charge.
Balance chemical equations for number of atoms and for charge.
Apply the Law of Conservation of Mass to writing balanced chemical equations.
Develop net ionic equations.
Recognize that an energy term is often shown in a chemical equation.
Place the energy term on the correct side of an equation, depending on whether a
reaction is exothermic or endothermic.
Develop a balanced chemical equation from a word equation, experimental
evidence, or a description of a chemical reaction taking place.
Mole Concept
Explore the concepts which relate to Avogadro's number.
Chapter 3: section 3-6
Chapter 4: sections 4-1 to 4-6
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Use an atomic mass (atomic weight) table to compare the relative masses of
atoms.
Realize that the absolute mass of an atom is very small.
Describe how Avogadro's number is obtained.
Explain the concept of a mole.
Calculate the number of moles in a given mass of atoms or molecules.
Calculate the masses of various numbers of moles of atoms and molecules
Apply knowledge about atomic mass to calculations dealing with
molecules.
Chapter 4: sections 4-11 to 4-12
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Calculate the concentrations of solutions in mols×L-1.
Perform stoichiometric calculations.
Chapter 4: sections 4-4 to 4-6, 4-11 to 4-12
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Manipulate the relationship among molar mass, number of moles and mass of
chemicals to solve stoichiometric problems.
Manipulate the relationship among concentration, number of moles and volume of
solution to solve stoichiometric problems.