CHEM 1004
Descriptive Chemistry
Spring 2011 (Buckley)
Learning Objectives
Textbook section references are in parentheses based on Chemistry for Changing Times, John W. Hill, Terry W. McCreary, Doris Kolb, 12th
Edition, Prentice Hall.
Learning Objectives
Problems to
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Consider
Chapter 1 – Chemistry
Distinguish between hypotheses, laws, theories, and models (1.3)
Define and apply the risk-benefit quotient (1.5)
13 - 18
Distinguish between applied research and basic research (1.7)
Identify chemical and physical properties and changes (1.8)
29 - 32
Define and apply the terms solid, liquid, gas, homogeneous mixture, heterogeneous mixture, elements
33 - 44
and compounds (1.9)
State the seven base SI units of measurement (1.10)
Convert measurements within the metric system (1.10) 19-28, 45- 52
You will be responsible for knowing the milli-, centi-, and kilo- prefixes and being able to use
them. If I ask for others I will give you the definition of the prefix.
Work with derived units such as volume and density (1.10 and 1.11)
53 - 64
Given formulas be able to convert between different temperature scales (1.12)
65 - 66
If you are asked to do this I will give you the formulas necessary.
Be able to describe the steps in the FLaReS critical thinking process (1.13)
Apply the FLaReS process (1.13) Critical Thinking Exercises, pp. 33-34
Chapter 2 – Atoms
State the Law of Conservation of Mass (2.2)
15 - 24
State the Law of Definite Proportions (2.3)
25 - 28
State the Law of Multiple Proportions (2.4)
29 - 34
Identify the four basic premises of John Dalton’s Atomic Theory (2.4)
35 - 40
State the historical primary driving force behind arranging the periodic table the way it is (2.5)
CHEM 1004
Descriptive Chemistry
Spring 2011 (Buckley)
Learning Objectives
Textbook section references are in parentheses based on Chemistry for Changing Times, John W. Hill, Terry W. McCreary, Doris Kolb, 12th
Edition, Prentice Hall.
Learning Objectives
Problems to
Got it?
Need work?
Consider
Chapter 3 – Atomic Structure
Describe two of the electrical experiments and their conclusions regarding atomic structure (3.1)
Identify the composition of alpha particles, beta particles, and gamma rays (3.3)
Describe Rutherford’s experiment and the conclusions it leads to regarding atomic structure (3.4)
Write isotopic symbols and interpret isotopic symbols to determine numbers of protons and neutrons
15 – 18
in a nucleus (3.5)
Describe Bohr’s application of line spectra (3.6)
Write electron configurations for elements in the first three periods (3.7)
19 – 26
Identify the number of valence electrons in an atom of an element (3.8)
Identify groups (families), periods, main group elements, transition elements, metals, nonmetals, alkali
27 - 32
metals, alkaline earth metals, and halogens on the periodic table (3.8)
Chapter 11 – Nuclear Chemistry
Nuclear Equations
State the atomic number and mass number for the three fundamental types of radiation – alpha, beta, 12
and gamma (11.2)
Provide missing pieces of information in nuclear equations (11.2) 19-30
Half-Life
Use half-life information to determine quantities of material remaining after specific lengths of time 31-42
(11.3)
CHEM 1004
Descriptive Chemistry
Spring 2011 (Buckley)
Learning Objectives
Textbook section references are in parentheses based on Chemistry for Changing Times, John W. Hill, Terry W. McCreary, Doris Kolb, 12th
Edition, Prentice Hall.
Learning Objectives
Problems to
Got it?
Need work?
Consider
Chapter 4 – Chemical Bonds
Identify isoelectronic species (4.1)
Draw Lewis symbols for individual atoms (4.2)
7–8
Use Lewis symbols to depict the formation of ionic compounds (4.3-4.4)
9 – 10
Write formulas for and name binary ionic compounds (4.5)
11 – 20
You will be given a periodic chart that includes the names.
Write Lewis structures for simple covalently bonded compounds (4.6)
25 - 30
Write names for simple covalently bonded compounds
31 – 34
Draw Lewis structures for simple polyatomic molecules (4.8)
Know the formulas, charges, and names of a select group (to be distributed) of polyatomic ions (4.9)
Your list of polyatomic ions includes: ammonium (NH4+), hydroxide (OH-), nitrate (NO3-),
sulfate (SO42-), and phosphate (PO43-)
Use polyatomic ions to write formulas of and names of compounds (4.9)
21 - 24
If you need polyatomic ions other than those you are responsible for in the line above I will give
you the name, formula, and charge for the polyatomic ion.
Draw Lewis structures for more complicated molecules and ions (4.10 – 4.11) 35 – 38, 55 58
Chapter 5 – Chemical Accounting
Balance a given chemical equation (5.1)
13 – 16
Interconvert between Avogadro’s number, moles, and mass (5.3 – 5.4)
23 – 32
Apply mass and mole relationships in chemical equations (5.4)
33 – 38
Work with molarity and percent relationships (5.5)
39 – 50
Know the definition of molarity – (M = #mol/#liters)
CHEM 1004
Descriptive Chemistry
Spring 2011 (Buckley)
Learning Objectives
Textbook section references are in parentheses based on Chemistry for Changing Times, John W. Hill, Terry W. McCreary, Doris Kolb, 12th
Edition, Prentice Hall.
Learning Objectives
Problems to
Got it?
Need work?
Consider
Chapter 6 – Gases, Liquids, Solids, and Intermolecular Forces
Identify at the molecular level the differences between solids, liquids, and gases (6.1)
Define the terminology associated with phase transitions – melting point, boiling point, condensation,
freezing, and sublimation (6.1)
State key physical differences between ionic and molecular compounds (6.2)
Identify the types of compounds exhibiting dipole-dipole forces, dispersion forces, and hydrogen
7 – 10
bonding (6.3)
Identify key forces that determine solubility of substances in liquids (6.4)
11 – 12
Identify the five key postulates in the kinetic molecular theory (6.5)
Apply Boyle’s Law and Charles’s Law to gases (6.6)
13 – 26
Know the combined gas law – (P1V1/T1 = P2V2/T2)
Apply the ideal gas law (6.7)
27 – 34
Know the ideal gas law (PV = nRT); I will give you R
Chapter 7 – Acids and Bases
Define and give properties for acids and bases (7.1)
Identify acids and bases using the Arrhenius theory (7.2)
13 – 16
Identify acids and bases using the Bronsted-Lowry Acid-Base Theory (7.2)
17 – 22
Classify oxides as either acidic or basic (7.3)
29 – 30
Describe the difference between a strong acid and a weak acid (7.4)
31 – 42
List the three most common strong acids – hydrochloric, sulfuric, and nitric acid (7.4 and Table 7.1)
Identify and write the equation for neutralization reactions (7.5)
43 – 46
Recognize key aspects of the pH scale – logarithmic, low pH is acidic, 7 is neutral, high pH is basic
47 – 56
(7.6)
Estimate pH from hydrogen concentration and vice versa (7.6)
47 – 54
Identify conjugate acid-base pairs (7.7)
55 – 56
CHEM 1004
Descriptive Chemistry
Spring 2011 (Buckley)
Learning Objectives
Textbook section references are in parentheses based on Chemistry for Changing Times, John W. Hill, Terry W. McCreary, Doris Kolb, 12th
Edition, Prentice Hall.
Learning Objectives
Problems to
Got it?
Need work?
Consider
Chapter 8 - Oxidation and Reduction
State and apply three approaches to considering oxidation-reduction reactions (8.1)
13 -16
Given an oxidation-reaction, identify the oxidizing agent and reducing agent (8.2)
17 – 36
Separate an oxidation-reduction into half reactions and identify each as oxidation or reduction (8.2)
23-26
Identify the functions of different parts of an electrochemical cell (8.3)
Describe the process of corrosion (8.4)
Chapter 9 – Organic Chemistry
Identify characteristics of carbon that result in it being a part of millions of compounds (9.1)
15
Identify and write formulas for simple hydrocarbons (9.2)
17 – 26
Define the terms saturated, alkanes, homologous series and isomers and give examples (you will be
41 - 44
expected to know the formulas and names for the alkanes methane through octane) (9.2)
Draw structures for and name simple cyclic hydrocarbons (9.3)
Define the terms unsaturated, alkene, and alkyne (9.4)
45 - 46
Given a table of functional groups, classify some compounds as alcohols, esters, ethers, etc. (9.7) 27-40, 47 - 50
Remaining topics will be chosen from:
Polymers (Chapter 10)
Environmental Topics selected from Chemistry of the Earth (Chapter 12), Air (Chapter 13), Water
(Chapter 14), and Energy (Chapter 15)
Health selected from Biochemistry (Chapter 16), Food (Chapter 17), and Drugs (Chapter 18)