B.C.'s Energy College

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Programs

CHEM 040 - Advanced Chemistry

CHEM 040

This course satisfies the requirements for a general or academic science. It meets entrance requirements for further academic or technical training. The advanced level covers the fundamental concepts and topics in chemistry with a qualitative approach to lab work.

Hours:

Total Hours: 120
Lecture Hours: 80
Laboratory Hours: 40

Total Weeks: 16

This course is offered online: No

Prerequisites:

Math 030 Intermediate Mathematics
Science 030 Intermediate Science or equivalent, or permission of the instructor
Math 040 Advanced Algebraic Mathematics is recommended

Learning Outcomes:

Upon successful completion of this course, learners will be able to:

Module 1- The Basics
Lab Safety

Check lab supplies in the course package
List safety precautions taken in storing lab items
Identify symbols used on hazardous products
Describe WHMIS and HHPS
Name hazardous products in the home and outbuildings
Describe first aid treatment for the hazardous products
Demonstrate when and how to use specific pieces of equipment

Measurement

Describe standards used in measurements
Define accuracy, density, heat, precision, significant figure, uncertain figure
Perform SI unit conversions
Measure mass, volume (of solution), and temperature
Investigate the density of solids
Measure heat gain and heat loss in a calorimeter
Describe the imprecise nature of measurements
Describe the uncertainty in a measurement
Determine the number of significant figures in a measured quantity
Round off calculated results to the correct number of significant figures
Compare the calculated value to the true or accepted value
Communicate results and data in an organized form

Chemistry

Describe chemistry as the study of elements and compounds, the atomic structure, and the physical and chemical properties
Identify chemistry as a pathway to a variety of career choices
Identify seven branches of chemistry

Scientific Method

Describe Scientific Method as a three-part process
List three steps of observation, hypothesis, and testing in the Scientific Method
Describe natural law and theory as tested hypotheses
Name three scientific laws

Model 2: – Earth (Part I)
Matter

Define matter
Classify pure substances and mixtures
Contrast pure substances with mixtures
Classify homogeneous and heterogeneous mixtures
Define and give examples of solutions
Define and give examples of suspensions
Identify gel, aerosol, sol, and emulsion as colloidal dispersions

Physical Properties

Define physical properties
Describe three states of matter in terms of kinetic molecular theory
Define melting point, boiling point, solubility, miscibility, and magnetism
Test solubility of some compounds in water
Test miscibility of oil in water
List some additional physical properties, such as hardness, conductance of electricity and heat, density, odour, and taste
Observe and describe physical properties of a few metals, e.g. aluminum, copper, and lead
Identify physical properties of a) salt, b) sand, and c) a mixture of salt and sand
Describe distillation
Describe filtration
Describe principals involved in the separation of mixtures
Devise and perform separation of salt from sand in a mixture
Perform separation of primary colors in food dye by paper chromatography

Chemical Properties

Describe chemical properties
Describe chemical tests
Identify flame test, spot test, and acid test
Describe the difference between chemical changes and physical changes
Identify whether a change is physical or chemical
Perform, observe and describe the reaction of sodium carbonate solution with iron II sulphate solution
Perform, observe and describe the reaction of sodium bicarbonate with acetic acid

Periodic Table

Define elements
Fill elements in a blank Periodic Table and classify them into metals, metalloids, and non-metals
Identify some common elements in the earth and in the human body
Write chemical symbols for elements

Module 3: - Earth (Part II)
Atoms and Isotopes

Describe early models of the atom
Describe modern atomic theory
Describe nucleus, neutrons, protons, and electrons of an element
Use a table to identify the atomic number for an element
Calculate the number of neutrons, protons and electrons in an atom or ion
Define isotopes in terms of protons, neutrons and electrons
Calculate the number of neutrons, protons, and electrons, given the mass number of an isotope
Write electron configurations for the first twenty elements
Define valence electrons, ground state, and excited state
Draw the Bohr diagram for the first twenty elements

Electron Configuration

Identify families of elements
Identify Groups 1 – 2 and 13 –18 as representative elements
Describe the similarities and periodic trends among elements in terms of
electronegativity, atomic radius, ionization energy, valence electrons and ion charge
Identify the following families of elements: the alkali metals, the alkaline earth metals, the halogens, and the noble gases

Describe some properties of the alkali metals, alkaline earth metals, halogens and noble bases
Relate chemical properties to the electron configuration of an element
Relate stability of noble gases to electron arrangement within the atom
Define ion, cation, anion
Predict electron gain or electron loss in forming stable octet of electrons
Identify the member of each period having
Explain the change in atomic size within a period
Identify the member of each period having

Module 4 – Fire (Part I)
Chemical Bonds

Demonstrate a knowledge of the electronic nature of chemical bonding
Name two types of chemical bonding: ionic and covalent
Define ionic bonds
Define covalent bonds
Compare and contrast ionic bonds with covalent bonds

Compounds

Define ionic compounds
Define crystals
Write chemical formulae for ions given a table of common ions
Write the chemical formula given the name of ionic compound, and vice versa
Name eight ionic compounds in home products
Write the molecular formula given the name of covalent compound, and vice versa
Name eight covalent compounds in home products
Determine the polarity of covalent bonds by using a chart of electronegativities

Lewis Structures

Draw Lewis structural formulae of simple ionic compounds
Draw Lewis structural formulae of covalent compounds
Construct models of molecules using the Lewis structure as a guide

Molecular shapes

Define symmetric and asymmetric molecular structures
Determine polar and non-polar molecules on the basis of molecular structure and polarity of bonds
Describe linear, bent, trigonal pyramidal, and tetrahedral molecules
Predict and draw the shape of a molecule given the formula

Module 5 – Fire (Part II)
Introduction to Mole Concept

Identify the mole as the unit for counting atoms, molecules and ions
Relate Avogadro’s number to 1 mole of “particles”
Review scientific notations
Calculate the number of moles from the number of molecules and atoms, and vice versa

Molar Mass

Define molar mass of an element
Define molar mass of a compound
Calculate the molar mass of elements and compounds
Solve problems involving the formula: mass = molar mass x number of moles

Percent Composition

Define Law of Definite Composition
Define percent composition as the percentage by mass of an element in a compound
Calculate the percent composition of each element in a compound

Chemical Reactions

Define precipitate, catalyst, reactants, products
Identify observable changes in chemical reactions such as permanent color change, a gas is produced, or a precipitate is formed
Identify factors that affect the rate of chemical reactions, such as heat, solvent, and catalyst
Classify chemical reactions into the following types:
Use Activity Series Table to predict single replacement reaction
Use Table of Solubility of Ionic Compounds in Water to predict formation of a precipitate in a reaction
Identify endothermic and exothermic reactions
Define photosynthesis as an endothermic reaction which requires light energy and a green pigment
Define Law of Conservation of atoms
Define chemical equations, coefficients, subscripts and postscripts
Predict products of simple reactions
Balance chemical equations
Perform experiments on

Stoichiometric Calculations

Relate the coefficients in a balanced chemical equation to the relative number of moles of reactants and products
Determine the amount of reactant and / or product measured in moles or grams that are involved in a chemical reaction

Module 6 - Water
Introduction to water

Identify some unique properties of water such as hydrogen bond, “universal solvent," and maximum density at 4º C
Describe the use of water in the treatment of sewage; and in making non polar products soluble, e.g. latex paint, and soluble chitin
used in sutures
Define melting point, boiling point of water
Define and give examples of hydrates
Describe high polarity of water due to its bent and asymmetric molecular shape
Describe hydrogen bonding between water molecules
Identify the effects of hydrogen bonding on the relatively high boiling point and heat of vaporization of water
Investigate the relative density of cold water, warm water and ice

Solutions

Define solvent, solute, solution, and aqueous solution
Search for five aqueous solutions in the home, and name the use of each
Compare the solubility of compounds in water in terms of molecular polarities
Dissolve various compounds and list them in increasing order of solubility
Investigate the miscibility of food coloring liquid and water

Water Pollution

Define pollution
Name two major sources of water pollution in the twentieth century
List three sources of water pollution around the home, developing a plan that students will follow to reduce pollution
Investigate and compare the amount of residue in distilled water and tap water
Define molarity, and parts per million (ppm)
Calculate the concentration of a solution in moles / L, g /L and ppm
Calculate the mass of solute dissolved in a given volume of solution
Name sources of toxic heavy metals that pollute drinking water
Describe Safe Drinking Water Act

Acids, Bases and Salts

Define acids, binary acid, oxyacids, organic acids
Name some sources of acid rain
Define bases, alkaline and polyatomic ions
Name some properties of acids and bases
Name products of an acid and a base reaction
Classify compounds as an acid, a base, or a salt
Relate pH measurements to strong acid, weak acid, weak base and strong base
Name compounds used to increase and decrease the soil pH
Describe the function of a buffer
Measure, record and compare pH values for some acids and bases
Investigate, record and compare the pH of fruits, vegetables and house hold chemicals
Investigate and observe changes in pH values in a neutralization reaction

Module 7 – Air
Introduction

Define atmosphere
Describe two layers of atmosphere: - troposphere and stratosphere
Identify physical properties of gases
Define diffusion, contraction, expansion, pressure and standard pressure

Gas Laws

Describe:
Apply gas laws to solve numerical problems

“The Precious Envelope” - Earth’s Atmosphere

Describe the composition of gases in the atmosphere
Describe the function of an “invisible shield”
Describe “fixing of nitrogen”, nitrogen cycle and uses of nitrogen
Describe the importance of ozone layer in the upper atmosphere
Describe ozone depletion
Identify three industrial and / or domestic products containing halo-hydrocarbons and suggest alternatives to halo-hydrocarbon products
Describe oxygen cycle and uses of oxygen
Describe carbon dioxide cycle and uses of carbon dioxide
Describe greenhouse effect and global warming

Carbon Dioxide

Prepare and collect carbon dioxide by:
Test for the presence of carbon dioxide: -
Balance equations for reactions involving carbonates and acids
Balance equations for different types of reactions including subscripts for the
state of a substance
Investigate the presence of carbon dioxide in the exhaled air from lungs

Module 8 – Carbon

Introduction

Define allotropes
Name four allotropes of carbon
Identify unique properties of carbon: -
Name first synthetic organic compound
Contrast organic compounds with inorganic compounds

Hydrocarbons

Define hydrocarbons, alkanes, alkenes, alkynes, cyclic-, and aromatic hydrocarbons
Define resonance bonding
Write general formulae for alkanes, alkenes and alkynes
Classify hydrocarbons as saturated or unsaturated
Name and draw alkanes, alkenes and alkynes up to C10
Draw and name structural isomers of alkanes, alkenes and alkynes
Recognize restricted rotation about double-bonded carbons in alkenes
Identify geometric isomers of alkenes

Functional Groups

Define the functional group.
Identify functional groups in alkenes, alkynes, alcohols, halo-hydrocarbon, halocarbon, aldehydes, ketones, carboxylic acids, esters, amines, amides
Name and draw structures of functional groups

Polymerization

Define polymerization, monomers, polymers and petrochemical industry
Identify two natural polymers
Name five common products made from polymer
Identify petrochemical industry as a major source of industrial air pollution
Suggest ways to reduce industrial pollutions

Knowledge:
An understanding of the fundamentals of Chemistry is vital to understanding the applications in health, the environment and industry.

Grading System: Letters

Passing Grade: D (50%)

Number of Assignments: 8

Nature of Participation: lab work

Percentage of Individual Work: 90

Percentage of Group Work: 10

Course Offered in Other Programs: No

Textbooks: Textbooks are subject to change. Please contact the bookstore at your local campus for current book lists.