CHM 112 Lecture Outline and ObjectivesDr. Miroslav Rezac

Chemistry 112: Lecture Outline and Objectives

Unit #1

Chapter 1 – Basic Concepts about Matter

  • Chemistry: Study of matter

Be able to define the field of chemistry as studying characteristics, composition and transformation of matter. Be able to define matter. Be able to name three physical states and list their mutual differences.

  • 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 process and give examples. Define chemical process and give examples.

  • Classification of matter

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. Explain the difference between an element and a compound. Be able to recognize either from their properties. 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.

  • Atoms and Molecule

Be able to define atom and molecule. Be able to explain relationship between identity of atoms and elements. Explain the terms homoatomic and heteroatomic molecules. Be able to interpret a chemical formula and interrelate formulas and number of atoms present. Be able to describe a molecule as an element or a compound based on its composition.

Chapter 2 – Measurements in Chemistry

  • 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 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.

  • Heat

Explain difference and relationship between heat and temperature. Apply equation linking heat, mass, temperature change and specific heat: from known three calculate the unknown one.

Chapter 3 – Atomic Structure and the Periodic Table

  • Composition of atom

List particles contained in atoms and their charges. Explain terms nucleus and electron cloud. Explain terms atomic and mass number and relate them to number of subatomic particles. Define atomic mass and explain how it is different from mass number. Isotopes. Average atomic mass.

  • Bohr model of atom

Relate structure of atom to that of solar system.

  • Quantum mechanical model of atom

Define orbital. Describe s and p orbital. Explain terms “shell”, “subshell” and “orbital”. Relate orbital and energy of an electron. Define electron spin. 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 PT. Using PT, write orbital diagram of any representative element.

Exam #1

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Unit #2

Chapter 4 - Chemical Bonding: The Ionic Model

  • Octet rule

Use Lewis “dot” notation to show valence electrons. For representative elements, be able to predict the most stable ion formed.

  • 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.

  • Nomenclature

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.

  • Polyatomic ions

Memorize names and formulas of selected polyatomic ions. Derive formulas of ionic compounds containing polyatomic ions and name them.

Chapter 5 - Chemical Bonding: The Covalent Model

  • Definition of 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.

  • Octet

Be able to determine the number of covalent bonds an atom will form from its number of valence electrons. Generate correct Lewis structures from chemical formulas of simple compounds.

  • Expanded octet

Apply the concept of expanded octet in elements of 3rd row and below to generate structures of where central atom forms a high number of covalent bonds.

  • Polyatomic ions

Link a charge of polyatomic ion to the number of “extra” electrons present. Generate correct Lewis structures from know location of charges (= which atom carries the charge) within polyatomic ions and vice versa.

  • VSEPR theory

Students will be able to distinguish between bonding and non-bonding electron pairs as “occupants” of space around the central atom. They will be introduced to the concept of repulsion between such occupants. Hybridization will be introduced only as needed as a way of maximizing the distance between occupants. Students will be able to deduct shape of molecule applying the requirement for “maximum spatial separation” thereof.

  • Electronegativity and polarity

Concept of electronegativity will be introduced. Students will be able to link polarity of a bond to an uneven distribution of electrons within a bonding orbital.

  • Polarity of molecules

Students are expected to differentiate between a polar bond and a polar molecule. They will be able to apply this concept and predict polarity of simple molecules from the electronegativities of bound atoms and VSEPR theory

Chapter 6 - Chemical Calculations: Formula Masses, Moles and Chemical Equations

  • Formula mass

Be able to calculate formula mass of any molecule when given its formula and PT.

  • 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 periodic table.

  • Chemical calculations

Be able to calculate the mass of element present in a given amount of a compound.

  • Chemical equations

Be able to recognize reactants and products in any given chemical equation. Be able to balance a chemical equation. Be able to apply chemical equation in terms of single molecules and in terms of moles.

  • Chemical calculations using chemical equations

Be able to calculate the amount of product formed. Be able to recognize a limiting reagent and apply this information to calculation of amount of product.

Exam #2

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Unit #3

Chapter 7 – Gases, Liquids and Solids

  • Kinetic molecular theory of matter

Be able to explain the terms “kinetic energy”, “potential energy” and be able to distinguish between the two. Be able to differentiate between elastic and inelastic collision. Be able to distinguish three different physical states based on constancy of volume shape. Be able to rank three physical states by their respective contents of kinetic energy and degree of disorder.

  • Changes of state

Be able to name the change of state between solid, liquid and gas (6 total). Be able to recognize which changes absorb and which release energy.

  • Gas Law Variables

Be able to calculate pressure as a force exerted on a unit area. Be able to convert between °C and K.

  • 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.

  • Dalton Law of partial pressures.

Be able to calculate total pressure from partial pressures. Be able to calculate partial pressure from known composition and total pressure.

  • Vapor pressure and boiling

Be able to describe evaporation. Be able to name factors determining vapor pressure. Be able to describe boiling. Name factors influencing boiling point. Be able to explain relationship between vapor pressure and boiling point.

  • Intermolecular forces in liquids.

Be able to name and describe the three principal intermolecular forces: dipole-dipole, hydrogen bond, London interactions. Be able to recognize molecules capable of these attractive interactions.

Chapter 8 - Solutions

  • Characteristics of solution

Be able to define solution as a homogeneous mixture composed of solvent and solute(s). Be able to explain difference between solvent and solute. Be able to describe different types of solutions. Be able to describe solution formation on molecular level.

  • Solubility

Saturated solution. Solubility. Be able to define solubility of a solute and saturated solution. Be able to explain factors influencing solubility. Describe diluted vs. concentrated solutions. Be able to describe solvation. Be able to apply simple solubility rules to estimate solubility of substances in water.

  • Concentration of solutions.

Be able to calculate and express concentration of solutions in percent and molarity. Apply this concept to calculating amounts of solutes needed to prepare solution of specified concentration. Be calculate concentration of solution after dilution. Be able to calculate total particle concentration of dissolved ionic substances.

  • Colloidal dispersions

Be able to define a colloidal dispersion. Be able to describe properties of dispersed particles

  • Colligative properties

Name three most important colligative effects and be able to give an example. Be able to name factors influencing the magnitude of colligative effects. Be able to calculate osmotic pressure. Be able to describe isotonic, hypotonic and hypertonic solutions and their effect on immersed cells.

Exam #3

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Unit #4

Chapter 9 - Chemical reactions

  • Types of chemical reactions

Be able to recognize combination, decomposition, single and double exchange.

  • Redox reactions

Be able to calculate oxidation number for atoms within a compound. Be able to recognize a redox reaction. Be able to describe oxidation as a loss of electrons and reduction as a gain of electrons. Be able to identify oxidizing and reducing reagent in a reaction.

  • Collision theory

Be able to describe a chemical reaction in terms of molecular collisions: activation energy, orientation. Be able to analyze graph for energy of exothermic and endothermic reaction: be able to recognize and describe activation energy and energy of chemical reaction.

  • Rates of chemical reactions

Be able to name three major factors influencing reaction rate in solution: concentration, temperature, activation energy, presence of catalyst. Be able to explain relationship of reaction rate, activation energy and temperature. Be able to describe action of a catalyst.

  • Chemical equilibrium

Be able to explain dynamic equilibrium as a result of steady state of forward and back reaction. Be able to write expression for equilibrium constant from a given reaction. Be able to explain relationship between the value of equilibrium constant and completeness of a reaction.

  • Le Chatelier principle

Be able to estimate effect of temperature on equilibrium constant. Be able to predict the effect of concentration changes on reaction extent (= “degree of completion”) – effects of “addition” of reactant and “removal” of product. Be able to estimate effect of pressure changes on equilibrium. Be able to estimate effect of temperature on equilibrium constant. Be able to predict the effect of concentration changes on reaction extent (= “degree of completion”) – effects of “addition” of reactant and “removal” of product. Be able to estimate effect of pressure changes on equilibrium

Chapter 10 – Acids, Bases and Salts

  • Arrhenius theory of acids and bases

Define acids as sources of H+ and bases as sources of OH-.

  • Bronsted-Lowry theory

Define acids as donors of H+ and bases as its acceptors. Explain relationship between “H+” of Arrhenius and hydronium ion. For a given acidobasic reaction, identify conjugate pairs. For a given species, be able to generate the corresponding conjugate acid / conjugate base.

  • Proticity of Acids

Estimate proticity of acids from their formulas. Be able to draw stepwise acidobasic reactions involving polyprotic acids. Explain amphoteric substance as a species which can act as a base in once reaction and as an acid in another.

  • Neutralization

Define neutralization as a reaction between acid and base. From given acid and base, be able to write balanced neutralization equation. Define “salt” as the product of a neutralization reaction.

  • Ionization constant of acids

Explain ionization of acids in water in terms of Bronsted-Lowry theory. Correctly identify conjugate pairs. Define strong acids as those completely transferring proton onto water. Define weak acids as those which transfer proton incompletely, causing large amounts of acid to be present in resulting equilibrium mixture. Be able to write expression for Ka for a given ionization equilibrium. Define pKa as –log(Ka). Be able to rank acids by their strength from known values of their pKa’s.

  • Self-ionization of water

Write chemical equation for self-ionization of water. Write equation defining ionic product of water. Mathematically relate [H+] and [HO-] for any aqueous solution. Define pH as –log [H+]. Recognize aqueous solution as being acidic, neutral or basic from known pH. Calculate [H+], [HO-] and pH of a solution of strong acid or strong base of known concentration.

  • Buffers

Be able to define a buffer. Give examples of biologically important buffers. Use Henderson-Hasselbach equation to calculate pH of a buffer of known composition.

  • Titrations

Be able to calculate mass of unknown sample of acid or base from known consumption of titrating agent.

Chapter 11 - Radioactivity

  • Nature of radioactivity

Describe radioactivity as a stream of fast particles and electromagnetic radiation resulting from nuclear decay. Name three types of radioactive particles.

  • Rate of radioactive decay

Apply known half-life to calculate residual amount of a nuclide.

  • Biochemical effect of radiation

Describe and explain some effects radiation has on a living organisms.

Exam #3

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