CHEM 1004 – Descriptive Chemistry
Learning Objectives
Textbook References are to: Chemistry for Changing Times, 12th Ed., John W. Hill, Terry W. McCreary, and Doris K. Kolb, Prentice Hall, 2010
Numbers in parentheses refer to sections of the textbook
Objective #
Objective
Problems to Practice
Chapter 1 - Chemistry
Define chemistry (Chapter 1 Intro)
Distinguish between applied and basic research (1.7)
Define the terms matter, mass, and weight (1.8)
Identify properties as either physical or chemical (1.8)
Distinguish between physical changes and chemical changes (1.8)
Give the three widely recognized states of matter – gas, liquid, or solid and distinguish between their
properties (1.9)
Classify substances as pure, mixtures, heterogeneous, homogeneous, elements, and/or compounds (1.9)
List the seven base units of measurement in the SI system (1.10)
Interchange metric prefixes with power of ten notation (1.10, Appendix A.2)
Relate the liter to the m3 (1.10)
Conduct straightforward unit conversions using the unit conversion method (1.10, Appendix A.3)
Identify significant figures in a measured quantity and carry them properly through a calculation
(Appendix A.4)
Define density (1.11)
Solve density problems for missing information (1.11)
Given the appropriate formulas, convert between the Fahrenheit, Celsius, and Kelvin temperature scales
(1.12)
Chapter 2 - Atoms
Recount briefly the historical development of the concept of the atom dating back to Leucippus and
Democritus (2.1)
State the Law of Conservation of Mass and attribute it to Lavoisier (2.2)
State the Law of Definite Proportions and attribute it to Proust (2.3)
Give Dalton’s four principles in his atomic theory and compare to modern theory (2.4)
Discuss the rationale for the arrangement of elements in the first periodic table by Mendeleev (2.5)
Chapter 3 – Atomic Structure
Describe Thomson’s explanation of the cathode ray tube as the first evidence of a substructure of atoms
(3.1)
CHEM 1004 – Descriptive Chemistry
Learning Objectives
Textbook References are to: Chemistry for Changing Times, 12th Ed., John W. Hill, Terry W. McCreary, and Doris K. Kolb, Prentice Hall, 2010
Numbers in parentheses refer to sections of the textbook
Objective #
Objective
Problems to Practice
Recognize Goldstein’s experiment as the first evidence for a positively charged subatomic particle (3.1)
Describe the discovery of radioactivity (3.2)
State the three types of radiation (3.3)
Give the symbols, masses, and charges of the three types of radiation (3.3)
Describe the conclusions drawn from Rutherford’s experiment (3.4)
Identify the nucleus of the atom as the location of protons and neutrons (3.5)
Define isotope (3.5)
Write the symbol for an element including its number of protons and nucleons (3.5)
Link emission spectra to the atomic model (3.6)
State the colors of the visible spectrum in order from low energy to high, or vice versa (3.6)
State the definition of an orbital in terms of probability (3.7)
Identify the shapes of s and p orbitals (3.7)
Use an order-of-filling chart to write electronic structures for atoms through calcium (3.7)
Identify the number of electrons in an atom of an element based on its location in the periodic table (3.8)
Define the terms groups and periods as related to the periodic table (3.8)
Identify the location and members of main group elements, transition elements, alkali metals, alkaline
earth metals, halogens, metals, and nonmetals on the periodic table (3.8)
Chapter 4 – Chemical Bonds
Recognize the stability of noble gas configurations as important in the formation of ions (4.1)
Determine the most likely ion formed from key elements in the periodic table based on location (4.1)
Draw Lewis symbols for main group elements (4.2)
Describe an ionic bond as the result of nearly complete electron transfer (4.3)
Identify elements on the periodic table likely to enter into ionic compounds (4.4)
Write formulas for compounds entering into ionic compounds (4.4)
Name binary ionic compounds (4.5)
Identify elements most likely to form covalent bonds (4.6)
Name covalent compounds (4.6)
Define electronegativity (4.7)
Rank given elements in terms of increasing electronegativity or vice versa (4.7)
Identify which elements form nonpolar covalent and polar covalent bonds (4.7)
CHEM 1004 – Descriptive Chemistry
Learning Objectives
Textbook References are to: Chemistry for Changing Times, 12th Ed., John W. Hill, Terry W. McCreary, and Doris K. Kolb, Prentice Hall, 2010
Numbers in parentheses refer to sections of the textbook
Objective #
Objective
Problems to Practice
State the name, charge, and formula for specified polyatomic ions (4.9)
Write Lewis formulas for given compounds (4.10)
Write Lewis formulas for odd-electron species (4.11)
Identify the molecular shape of a species based on its Lewis formula (4.12)
Identify molecules as being polar or nonpolar based on the Lewis formulas (4.13)
Chapter 5 – Chemical Accounting