Download Detailed list of class Objectives and Lecture Outline

CHM101
Lecture Outline and Objectives
Dr. Miroslav Rezac
Lecture Outline and Objectives
Unit #1
Chapter 1 – Introduction to Chemistry

Nature of Chemistry
Be able to define the nature of chemistry as studying characteristics, composition and
transformation of matter. Be able to describe scientific method/process.
Chapter 2 – Standards for measurement

Measurement systems
Be able to describe a measurement as a determination of a quantifiable property. Be able
to recognize or provide a result of a measurement as a number and unit. Generate larger
and smaller units in metric system using metric prefixes. Memorize, recognize and be
able to provide metric units for mass, length, volume, density, temperature. Be able to
describe in simple terms how we measure each variable. Be able to interconvert
temperatures in Celsius and Kelvin scale. Be able to convert measurements in different
units using conversion factors (conversion equation).

Scientific notation
Be able to convert a given number from decimal to scientific notation and vice versa. Be
able to perform simple mathematical operations with numbers in scientific notation.

Uncertainty and Precision
Determine the number of significant figures in a given number. Be able to provide a
result of a measurement with the correct number of significant figures. Determine the
correct number of significant figures for a result of simple mathematical operations:
operational rules and rounding.

Density
Define density as the mass of a volume unit. Write the equation defining density, linking
density, mass and volume. Using this equation, from known two propensities calculate
unknown one.
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CHM101
Lecture Outline and Objectives
Dr. Miroslav Rezac
Chapter 3 – Classification of Matter

Description of matter
Define matter. Describe three physical states.

Classification of matter - mixtures
Be able to explain difference between pure substance and mixture. Be able to describe
and recognize homogeneous and heterogeneous mixture in term of their properties.

Classification of matter – pure substances
Explain the difference between an element and a compound. Be able to recognize either
from their properties. Explain the term “molecule”. Be able to classify a sample of matter
from provided properties. Know relationship between name and symbol of an element.
Memorize symbols of selected elements. Explain difference between metals and nonmetals.

Chemical formulas
Be able to interpret a chemical formula and interrelate formulas and number of atoms
present. Be able to describe formula as an element or a compound based on its
composition.
Chapter 4 – Properties of Matter

Properties and changes of matter
Be able to point out differences between physical and chemical properties. Be able to
give examples of both. Be able to define a physical change and give examples. Define
chemical change and give examples. Explain law of conservation of mass.

Energy
Define energy. Describe potential and kinetic energy. Explain difference between “heat”
and “temperature”. Be able to link E and T using specific heat. Law of conservation of
energy
Exam #1
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CHM101
Lecture Outline and Objectives
Dr. Miroslav Rezac
Unit #2
Chapter 5 – Early Atomic Theory and Structure

Atoms and Molecule
Describe Greco-Daltonian atom. Explain how atoms aggregate to form molecules. Know
properties of electric charge. Explain the term “ion”. Please name the three subatomic
particles. Describe Thompson (“raisin muffin”) model of atom. Describe Rutherford
model of atom.

Atomic mass
Explain the term “atomic number”. Explain the term isotope in terms of atomic
composition. Explain the term “atomic mass” and “average atomic mass”. Name the
instrument which can measure mass of an atom or of a molecule.
Chapter 10 – Modern Atomic Theory and the Periodic Table

Bohr model of atom
Relate structure of atom to that of solar system. Explain the term quantum; ground state.

Quantum mechanical model of atom
Explain terms “shell”, “subshell” and “orbital” in terms of geometry and energy. Relate
orbital and energy of an electron. Define electron spin. Describe s and p orbital. Write an
electron configuration and orbital diagram for a given number of electrons. Recognize
valence electrons in orbital diagram and know their role.

Periodic table
Define “group” and “period”. Locate regions of the Periodic Table (PT) populated by
representative and transition elements, by metals and non-metals. Use PT to obtain
atomic number and average atomic mass for any element. Determine number of valence
electrons and valence shell number of any representative element from its location in
MPT. Using MPT, write orbital diagram of any representative element.
Chapter 11 - Chemical Bonding

Octet rule
Use Lewis “dot” notation to show valence electrons. For representative elements, be able
to predict the most stable ion formed.
Page 3 of 6
CHM101
Lecture Outline and Objectives
Dr. Miroslav Rezac

Formation of ionic compounds
Be able to describe ionic compound formation as a transfer of valence electrons between
two atoms. Derive chemical formula of ionic compound formed by two ions of a give
charge. Recognize ionic compound by simultaneous presence of metal and non-metal.

Covalent bond
Discuss covalent bond as an overlap of orbitals, resulting in electron octet. Explain
difference between  and  bonds. Draw Lewis structures of molecules; be able to
interpret the “hyphen” as a bonding orbital containing two electrons. In a Lewis structure
be able to correctly count the number of bonding and non-bonding electrons. Describe
multiple bond in terms of multiple bonding orbitals between two atoms.

Polarity
Explain polar bond in terms of asymmetric electron distribution. Explain
electronegativity as the ability of an atom to attract electrons. Relate non-polar covalent
and ionic bond as two extremes.

Polyatomic ions
Memorize names and formulas of selected polyatomic ions. Derive formulas of ionic
compounds containing polyatomic ions and name them.

VSEPR theory
Distinguish between bonding and non-bonding electron pairs as “occupants” of space
around the central atom. Be able to deduct shape of molecule applying the requirement
for “maximum spatial separation” thereof.
Exam #2
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Unit #3
Chapter 6 – Nomenclature

Binary compounds
Name ions derived from representative elements. Name binary ionic compounds formed
from these ions. For ionic compounds of transition elements: from a known name derive
formula and ionic charge, from known ionic charge derive name and formula, from
known formula derive name and ionic charge. Name binary compounds formed of two
non-metals.
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CHM101

Lecture Outline and Objectives
Dr. Miroslav Rezac
Polyatomic ions
Memorize names and formulas of selected polyatomic ions. Generate formulas of
compounds containing polyatomic ions. Name compounds containing polyatomic ions.
Chapter 7 - Quantitative Composition of Compounds

Formula mass
Be able to calculate formula mass of any molecule when given its formula and MPT.

The mole
Be able to define a mole. Be able to calculate number of molecules in one mole of a
substance. Be able to interconvert number of moles and number of objects.

Molar mass
Be able to calculate molar mass of any substance given its formula and MPT.

Percent composition of compounds
For any give compound be able to calculate its percent elemental composition.

Empirical Formula
Explain difference between empirical and molecular formula. Calculate empirical
formula from known elemental composition. Calculate molecular formula from known
empirical formula and molar mass.
Chapter 8 – Chemical Equations

Chemical equations
Be able to recognize reactants and products in any given chemical equation. Be able to
balance a chemical equation. Be able to interpret chemical equation in terms of single
molecules and in terms of moles.

Types of chemical equations
Distinguish four basic types of reactions. Recognize neutralization.

Chemical reactions and energy
Interpret chemical equation with heat included. Define “heat of reaction”. Explain term
“activation energy”. Interpret reaction energy diagrams.
Exam #3
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Page 5 of 6
CHM101
Lecture Outline and Objectives
Dr. Miroslav Rezac
Unit #4
Chapter 8 – Calculation from Chemical Equations

Calculations using chemical equations
Calculate the amount of product formed or reagent needed. Be able to recognize a
limiting reagent and apply this information to calculation of amount of product.
Chapter 12 – Gaseous State of Matter

Kinetic molecular theory of matter
Be able to explain how the average speed of particles of a gas depends on temperature.

Gas Law Variables
Explain pressure of a gas in terms of particles impacting container wall. Memorize
different units of pressure.

Boyle Law
Be able to calculate a new pressure resulting from changing volume and vice versa.

Charles’s and Gay-Lussac Laws
Be able to calculate changes of volume and pressure resulting from changes of
temperature

Combined Gas Law
For p, V and T, be able to calculate changes of the third variable when the two other are
known.

Ideal Gas Law
Be able to relate n, p, V, T by ideal gas law and calculate the fourth variable when three
are provided.

Gas stoichiometry.
Memorize the volume of 1 mole of ideal gas under normal conditions. Apply to reaction
stoichiometry. .
Exam 4
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