Principle of Moments Worksheet by gqk65242

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```									Professor Susan B. Piepho                                                                                January 2006
Chemistry 131 Daily Schedule

Chemistry 131, Principles of Chemistry I
Daily Schedule, Spring 2006

Readings are from the text, Chemistry, 8th Edition by Raymond Chang. Answers to the even-
numbered problems are given near the back of the book beginning on page AP-1. Complete
solutions to the even-numbered problems are given in the Student Solutions Manual by B. J.
Cruickshank and R. Chang. In the list of assigned problems below, numbers are in italics if no
answer is provided; most of these are Review Questions (which are usually answered in the
reading).

Worksheets are available on the web (http://spiepho.sbc.edu/worksheets/). Please print these out
and bring them to class on the day they are assigned.

NOTE: Unless otherwise indicated, Challenge Problems may be worked as a group of students
from our class (but with no help or assistance of any type from non-class members). Challenge
Problems should be handed in at the beginning of the class period in which they are due. Each
member of a group should turn in their own paper; the names of all members of the group must
be listed on each paper that involves group work.

Daily Assignments

Th 1/19
Read: Guided Tour, Media, A Note to the Student; Chapter 1. The Study of Change, 1.1 – 1.8 (The scientific
method, hypothesis, law, theory, substances, mixture, elements, compounds, physical and chemical properties,
measurement, SI units and prefixes, scientific notation, significant figures).
Worksheet: Chapter 1, Scientific Notation, Significant Figures, and the Factor-Label Method of Solving Problems.

F 1/ 20
Read: Chapter 1. The Study of Change: 1.9 (Dimensional analysis in solving problems).
Problems: The Scientific Method: 1.4; Classification and Properties of Matter: 1.12, 1.14, 1.16, 1.52; Measurement :
1.17, 1.18, 1.22, 1.26; Handling Nu mbers: 1.28, 1.30, 1.32, 1.34, 1.36; Dimensional Analysis: 1.38, 1.40, 1.42(c),
1.46, 1.50, 1.54.

M 1/23
Read: Chapter 2. Ato ms, Molecules, and Ions: 2.1 – 2.5 (Origins of atomic theory, ato mic structure, radioactivity,
Rutherford experiment, atomic nu mber, mass number, isotopes, molecules, ions).
Problems: Structure of the Atom: 2.1, 2.8; Atomic Nu mber, Mass Number, and Isotopes: 2.10, 2.11, 2.12, 2.14,
2.16, 2.18, 2.72; The Periodic Tab le: 2.20, 2.21, 2.22, 2.24, 2.26, 2.74, 2.78, 2.80.

W 1/25
Read: Chapter 2. Ato ms, Molecules, and Ions: 2.6 – 2.7 (Chemical formu las, naming ionic co mpounds, naming
mo lecular co mpounds, naming acids and bases, hydrates).
Problems: Molecu les and Ions: 2.28, 2.30, 2.32, 2.34, 2.36, 2.60, 2.62; Chemical Formu las: 2.39, 2.40, 2.42, 2.44,
2.46, 2.64, 2.66.

Page 1 of 7
Professor Susan B. Piepho                                                                                    January 2006
Chemistry 131 Daily Schedule

Th 1/26
Quiz #1: Chapter 1 (see syllabus for format).
Worksheet: Chapter 2, Naming Inorganic Compounds.
Problems: Naming Inorganic Co mpounds: 2.49, 2.52, 2.53, 2.56, 2.58, 2.84(a)(c)(d)(f).
Read: Chapter 3. Mass Relat ionships in Chemical Reactions: 3.1 – 3.5 (Molar mass of atoms and molecules,
Avogadro’s number, the mass spectrometer, % co mposition).

F 1/ 27
Read: Chapter 3. Mass Relat ionships in Chemical Reactions: 3.6 – 3.8 (Experimental determination of emp irical
formulas, chemical reactions and equations, chemical react ion problems).
Worksheet: Chapter 3, Mole Definitions.
Problems: Ato mic Mass: 3.1, 3.2, 3.6, 3.8; Avogadro’s Number and Molar Mass: 3.9, 3.10, 3.16, 3.20, 3.22;
Molecular Mass: 3.24, 3.26, 3.30; Percent Co mposition and Chemical Formu las: 3.36, 3.38, 3.40, 3.46, 3.48.

M 1/30
Challenge Problems due (group work allowed) : Set 1.
Worksheet: Chapter 3, Empirical and Molecular Formulas.
Problems: Percent Co mposition and Chemical Formu las: 3.44, 3.50, 3.114; Chemical Reactions and Chemical
Equations: 3.57, 3.58, 3.60; A mounts of Reactants and Products: 3.70, 3.72, 3.76.

W 2/1
Read: Chapter 3. Mass Relat ionships in Chemical Reactions: 3.9 – 3.10 (Limiting reagent problems, reaction yield).
Worksheet: Chapter 3, Chemical Stoichiometry Problems.

Th 2/2
Quiz #2: Chapter 2, and Chapter 3 through Section 3.5 and the problems on the previous Friday’s assignment. You
will need to know the names of ions given in Tables 2. 2 and 2.3 on page 60, and the names of co mmon acids and
bases as specified in class.
Problems: Limit ing Reagents: 3.82, 3.83 (Ans.: 0.886 mol NO2 ), 3.84; Reaction Yield : 3.87, 3.88, 3.89 (Ans.:
92.9%), 3.90, 3.92.

F 2/ 3
Read: Chapter 4. Reactions in Aqueous Solutions: 4.1 – 4.4 (to p. 131) Electro lytic properties, hydration,
precipitation reactions, solubility rules; writ ing molecular, ionic, and net ionic equations; acid -base reactions,
Bronsted definition of acids and bases, oxidation-reduction reactions, use of oxidation numbers).
Worksheet: Chapter 4, Types of Chemical Reactions: Writing Balanced Ionic Equations.

M 2/6
Worksheet: Chapter 4, Oxidation-Reduction Reactions.
Problems: Properties of Aqueous Solutions: 4.1, 4.2, 4.3, 4.4, 4.5, 4.6, 4.7 (Ans.: strong, non, weak), 4.8, 4.10, 4.12,
4.14; Precipitation Reactions: 4.15, 4.16, 4.17, 4.18, 4.20, 4.22, 4.24; Acid-Base Reactions: 4.25, 4.26, 4.27, 4.28,
4.29, 4.30, 4.32, 4.33, 4.34; Su mmary questions: 4.120, 4.128.

W 2/8
Read: Chapter 4. Reactions in Aqueous Solutions: 4.4 (pp. 130 – 139) (Types of redo x reactions: co mbination,
decomposition, displacement react ions, disproportionation reactions; activity series (see Figure 4.15, p. 134)).

Th 2/9
Hour Test I
(This will be on Chapters 1, 2, and 3.)

F 2/ 10
Problems: Oxidation-Reduction Reactions: 4.35, 4.36, 4.37, 4.38, 4.39, 4.40, 4.41, 4.42, 4.46, 4.48, 4.50, 4.52, 4.54,
4.56, 4.122, 4.148.

Page 2 of 7
Professor Susan B. Piepho                                                                                    January 2006
Chemistry 131 Daily Schedule

M 2/13
Challenge problems due (group work allowed): Set 2.
Worksheet: Chapter 4, Working with Solutions.
Read: Chapter 4. Reactions in Aqueous Solutions: 4.5 – 4.6 (Molarity, making up solutions, dilution of solutions,
gravimetric analysis).
Problems: Concentration of So lutions: 4.57, 4.58, 4.60, 4.62, 4.64(a)(b), 4.66(a)(c), 4.136; Dilut ion of Solut ions:
4.67, 4.68, 4.70, 4.72, 4.74; Grav imetric analysis: 4.78.

W 2/15
Worksheet: Chapter 4, pH and Titrations.
Read: Chapter 4. Reactions in Aqueous Solutions: 4.7 – 4.8 (Acid-base titrations, redo x titrat ions).

Th 2/16
Quiz #3: Chapter 4 as announced in class.
Problems: Acid-Base titrations: 4.81, 4.82, 4.83, 4.84, 4.86, 4.88; Redo x t itrations: 4.89, 4.90, 4.92, 4.144.

F 2/ 17
Worksheet: Chapter 5, Ideal Gases.
Read: Chapter 5. Gases: 5.1 – 5.5 (Un its of pressure measurement, baro meter, Boyle’s Law, Charles’ and Gay -
Lussac’s Law, Avogadro’s Law, Ideal Gas Equation, gas stoichiometry).
Problems: Substances That Exist as Gases: 5.1, 5.2; Pressure of a Gas: 5.3, 5.4, 5.5, 5.8, 5.9, 5.14; The Gas Laws:
5.15, 5.16, 5.18, 5.20, 5.22, 5.24, 5.26.

M 2/20
Worksheet: Chapter 5, Ideal Gas Mixtures.
Read: Chapter 5. Gases: 5.6 – 5.7 (Dalton’s Law of Part ial Pressures, kinetic mo lecular theory of gases, root-mean-
square speed of a gas).
Problems: The Ideal Gas Equation: 5.27, 5.28, 5.29, 5.30, 5.32, 5.34, 5.36, 5.38, 5.40, 5.42, 5.44, 5.46, 5.48, 5.50;
Gas Stoichio metry: 5.54, 5.58, 5.60.

W 2/22
Read: Chapter 5. Gases: 5.8 (Dev iation fro m ideal gas behavior).
Problems: Dalton’s Law of Partial Pressures: 5.61, 5.62, 5.64, 5.66, 5.68, 5.102; Kinetic Molecular Theory of Gases:
5.71, 5.72, 5.73, 5.76, 5.78; Deviat ion fro m Ideal Behavior: 5.81, 582, 5.83, 5.88.

Th 2/23
Challenge problems due (group work allowed): Set 3.
Catch up on Chapter 5 prob lems.
Read: Chapter 6. Thermochemistry: 6.1 – 6.4 (Types of energy, energy changes in chemical reactions, introduction
to thermodynamics, First Law of Thermodynamics, state functions and path functions, enthalpy changes ( H) o f
chemical reactions, thermochemical equations).
Problems: Defin itions: 6.1, 6.2, 6.3, 6.5; Energy Changes in Chemical Reactions: 6.7, 6.8, 6.9; First Law of
Thermodynamics: 6.11, 6.12, 6.18; Enthalpy of Chemical React ions: 6.21, 6.22, 6.24(a)(b), 6.26.

F 2/ 24
Read: Chapter 6. Thermochemistry: 6.5 – 6.7 (Calorimet ry, specific heat and heat capacity, calorimetry at constant
volume and at constant pressure, standard enthalpy of formation, calculat ion of standard enthalpy of reaction, Hess’s
Law, heat of solution and dilution).
Worksheet: Chapter 6, Calorimetry Exercises.
Problems: Calorimetry : 6.29, 6.30, 6.31, 6.32 (Ans. is (d)), 6.34, 6.36, 6.38, 6.96.

Page 3 of 7
Professor Susan B. Piepho                                                                                   January 2006
Chemistry 131 Daily Schedule

M 2/27
Catch up with Chapter 6.

W 3/1
Worksheet: Chapter 6, The Enthalpy of Chemical Change: Calculations using Hess’s Law and Heats of Formation.

Th 3/2
Quiz #4: Chapters 4, 5, and 6 as announced in class.
Problems: Standard Enthalpy of Formation and Reaction: 6.39, 6.40, 6.41, 6.42, 6.43, 6.44, 6.46, 6.48, 6.54, 6.58,
6.60, 6.62, 6.64; Heat of Solution and Dilution: 6.65, 6.66, 6.67, 6.68, 6.70.

F/3/3
Catch up on Chapter 6 prob lems.

M 3/6
Read: Chapter 7. Quantum Theory and the Electronic Structure of Ato ms: 7.1 – 7.3 (Electro magnetic radiation,
photoelectric effect, photons, dual nature of light, emission spectrum of the H atom, Bohr model of the H atom).
Worksheet: Chapter 7, Electromagnetic Radiation and the Spectrum of Atomic Hydrogen.
Problems: Quantum Theory and Electro magnetic Radiation: 7.1, 7.2, 7.3, 7.4, 7.5, 7.6, 7.8, 7.10, 7.12, 7.110; The
Photoelectric Effect: 7.13, 7.14, 7.16, 7.18, 7.20.

W 3/8
Read: Chapter 7. Quantum Theory and the Electronic Structure of Ato ms: 7.4 – 7.6 (Dual nature of particles, de
Broglie equation, quantum mechanical model of the H atom, Heisenberg uncertainty principle, quantum numbers).
Worksheet: Chapter 7, Quantum Numbers, Orbitals, and Electron Configurations.
Problems: Bohr’s Theory of the Hydrogen Atom: 7.21, 7.22, 7.23, 7.24, 7.26, 7.28, 7.29 † , 7.32, 7.34, 7.120;
Particle-Wave Duality: 7.35, 7.36, 7.37, 7.38, 7.40, 7.98; Quantum Mechanics: 7.43, 7.44, 7.46, 7.47, 7.49, 7.52,
7.94.
†
Answers to 7.29: (a) 14x10-19 J,  = 140 n m; (b) 5x10-19 J; (c) Ephoton = 10x10-19 J; = 200 n m.

Th 3/9
Hour Test II
(This will be on Chapters 4, 5, and 6 as announced in class.)

F 3/ 10
Read: Chapter 7. Quantum Theory and the Electronic Structure of Ato ms: 7.7 – 7.9 (Ato mic orbital plots, energies
of the orbitals, electron configurat ions of mu lti-electron ato ms, Pauli exclusion principle, paramagnetism, , shielding
effect, Hund’s rule, building up principle).
Problems: Quantum Mechanics: 7.54, 7.56, 7.58, 7.62, 7.66, 7.68; Atomic Orb itals: 7.69, 7.70; Electron
Configurat ion: 7.71, 7.72, 7.73, 7.74, 7.75, 7.76, 7.77, 7.78, 7.80, 7.82, 7.84, 7.86, 7.124; The Aufbau Princip le:
7.87, 7.88, 7.89, 7.92.

Spring Break

M 3/20
Challenge problems due (group work allowed) : Set 4.
Catch up on Chapter 7 prob lems.
Read: Chapter 8, Periodic Relationships Among the Elements: 8.1 – 8.2 (Develop ment of Periodic Table,
representative or main group elements, valence electrons, electron configurations of cations and anions).

Page 4 of 7
Professor Susan B. Piepho                                                                                    January 2006
Chemistry 131 Daily Schedule

W 3/22
Worksheet: Chapter 8, Periodic Trends.
Read: Chapter 8, Periodic Relationships Among the Elements: 8.3 – 8.5 (Effective nuclear charge, periodic varia -
tion in atomic radius, trends in ionic radius, isoelectronic series, periodic trends in ioniza tion energy, trends in higher
ionization energies, electron affinities).

Th 3/23
Quiz #5: Chapters 6 and 7 as announced in class.
Problems: Develop ment of the Periodic Table: 8.1, 8.3, 8.4; Periodic Classification of the Elements: 8.5, 8.7, 8.8,
8.11, 8.12, 8.13, 8.14, 8.15, 8.16, 8.18, 8.20, 8.22, 8.24, 8.26, 8.28, 8.32, 8.76, 8.90; Periodic Variation in Physical
Properties: 8.33, 8.34, 8.35, 8.36, 8.38, 8.40, 8.42, 8.44, 8.46.

F 3/ 24
Read: Chapter 8, Periodic Relationships Among the Elements: 8.6 (Chemical properties of the representative or
main group elements).
Problems: Ionization Energy: 8.49, 8.50, 8.54, 8.56, 8.78, 8.118, 8.128; Electron Affinity: 8.62.

M 3/27
Problems: Variation in Chemical Properties of the Representative Elements: 8.65, 8.66, 8.68, 8.70, 8.72, 8.74, 8.92,
8.94.

W 3/29
Catch up on Chapter 8.
Read: Chapter 9. Chemical Bonding I: Basic Concepts: 9.1 – 9.4 (Lewis dot symbols, the ionic bond, lattice energy
of ionic co mpounds, Born-Haber cycle, the covalent bond).

Th 3/30
Quiz #6: Chapter 8 as announced in clas s.
Problems: Lewis Dot Sy mbols: 9.1, 9.2, 9.3; The Ionic Bond: 9.6, 9.7, 9.9, 9.11, 9.13, 9.14, 9.16, 9.18, 9.20; Lattice
Energy of Ionic co mpounds: 9.21, 9.22, 9.23, 9.26.

F 3/ 31
Chapter 9. Chemical Bonding I: Basic Concepts: 9.5 – 9.6 (Electronegativity, relation of electronegativity to
oxidation numbers, drawing Lewis structures in simple cases).
Problems: The Covalent Bond: 9.27, 9.28, 9.29, 9.30, 9.31, 9.74, 9.78; Electronegativity and Bond Type: 9.33, 9.34,
9.36, 9.38, 9.40; Lewis Structure and the Octet Rule: 9.41, 9.44, 9.48.

M 4/3
Chapter 9. Chemical Bonding I: Basic Concepts: 9.7 – 9.8 (Formal charge and Lewis structure, the concept of reso-
nance).
Problems: Lewis Structure and the Octet Rule: 9.42, 9.46; The Concept of Resonance: 9.49, 9.50, 9.54, 9.56, 9.90,
9.100, 9.114.

W 4/5
Chapter 9. Chemical Bonding I: Basic Concepts: 9.9 – 9.10 (Exceptions to the octet rule, bond energy).
Problems: Exceptions to the Octet Rule: 9.57, 9.58, 9.60, 9.62, 9.64, 9.66, 9.96; Bond Energy: 9.67, 9.70; Su mmary
question: 9.86.

Th 4/6
Hour Test III
(This will be on Chapters 7 and 8, and on Chapters 6 and 9 as announced in class)

Page 5 of 7
Professor Susan B. Piepho                                                                                January 2006
Chemistry 131 Daily Schedule

F 4/ 7
Catch up on Chapter 9.
Worksheet : Molecular Geometry Summary Chart.
Read: Chapter 10. Chemical Bonding II: Molecular Geo met ry and Hybrid ization of Atomic Orb itals: 10.1 (Use of
VSEPR theory to predict molecular geo metry).
Problems: Mo lecular Geo metry : 10.2, 10.3, 10.4, 10.5, 10.6, 10.10, 10.12, 10.14.

M 4/10
Challenge problems due (group work allowed) : Set 5.
Read: Chapter 10. Chemical Bonding II: 10.2 (Dipole mo ments and polar mo lecules).
Problems: Dipole Mo ments: 10.16, 10.18, 10.20, 10.22, 10.24.

W 4/12
Worksheet: Hybridization of Carbon Diagram.
Read: Chapter 10. Chemical Bonding II: 10.3 – 10.5 (Valence bond theory, hybridization of ato mic orbitals, sig ma
and pi bonds).
Problems: Valence Bond Theory: 10.25; Hybrid ization: 10.29, 10.30, 10.31, 10.32, 10.34, 10.36, 10.38, 10.42,
10.44, 10.84.

Th 4/13
Quiz #7: Chapter 9, and Chapter 10 as announced in class.
Read: Chapter 10. Chemical Bonding II: 10.6 – 10.7 (Molecular orbital theory, MO configurations for the first and
second row diato mics).
Worksheet: Molecular Orbital Diagrams for the First and Second Rows.
Problems: Mo lecular Orbital Theory: 10.45, 10.46, 10.47, 10.48, 10.52, 10.54, 10.56, 10.58.

F 4/ 14
Read: Chapter 10. Chemical Bonding II: 10.8 (MO theory applied to polyatomic mo lecules: benzene and carbonate
ion; structure of C60 , the buckyball).
Problems: Delocalized Molecular Orbitals: 10.62, 10.64, 10.66, 10.68.

M 4/17
Catch up on Chapter 10.

W 4/19
Read: Chapter 11. Intermo lecular Forces and Liquids and Solids: 11.1 – 11.3 (Types of intermo lecular forces,
hydrogen bonding, properties of liquids).
Problems: Intermolecu lar Forces: 11.1, 11.2, 11.3, 11.4, 11.5, 11.6, 11.10, 11.12, 11.14, 11.16, 11.18, 11.108;
Properties of Liquids: 11.22, 11.23, 11.24, 11.25, 11.27, 11.28, 11.29, 11.30, 11.32.

Th 4/20
Quiz #8: Chapter 10 as announced in class.
Worksheet: Chapter 11, Intermolecular Forces.
Read: Chapter 11. Intermo lecular Forces and Liquids and Solids: 11.4 – 11.7 (Crystalline solids, X-ray diffraction
by crystals, ionic, covalent, mo lecular, and metallic crystals, amorphous solids).
Problems: Crystal Structure: 11.36; X-Ray Diffraction of Crystals: 11.45; Types of Crystals: 11.49, 11.50, 11.51,
11.52, 11.53, 11.54, 11.56; A morphous Solids: 11.57, 11.58.

F 4/ 21
Read: Chapter 11. Intermo lecular Forces and Liquids and Solids: 11.8 – 11.9 (Phase changes, normal boiling point,
liquid -solid and solid vapor equilibria, phase diagrams).
Problems: Phase Changes: 11.59, 11.60, 11.61, 11.62, 11.63, 11.64, 11.65, 11.66, 11.68, 11.69, 11.71, 11.72, 11.73,
11.75, 11.76, 11.78, 11.84; Phase Diagrams: 11.89, 11.90, 11.94; Additional Problems: 11.96, 11.98, 11.100,
11.112, 11.126.

Page 6 of 7
Professor Susan B. Piepho                                                                                 January 2006
Chemistry 131 Daily Schedule

M 4/24
Challenge problems due (group work allowed): Set 6.
Read: Chapter 12. Physical Propert ies of Solutions: 12.1 – 12.3 (Saturated, unsaturated, and super-saturated
solutions, a mo lecular view of the solution process, concentration units).
Problems: Types of Solutions: 12.1, 12.2; A Molecular View of the Solution Process; 12.3, 12.4, 12.5, 12.7, 12.10,
12.12, 12.116; Concentration Units; 12.13, 12.16(a), 12.20, 12.106.

W 4/26
Read: Chapter 12. Physical Propert ies of Solutions: 12.4 – 12.6 (Effect of temperature and pressure on solubility,
colligative properties, vapor-pressure lowering, boiling point elevation, freezing point depression).
Problems: The Effect of Temperature on So lubility: 12.25; Gas So lubility: 12.30, 12.31, 12.33, 12.34, 12.36;
Colligative Propert ies of Nonelectrolyte solutions: 12.39, 12.43, 12.44, 12.45, 12.49, 12.58, 12.92.

Th 4/27
Hour Test IV
(This will be on Chapters 9, 10, and 11.)

F 4/ 28
Read: Chapter 12. Physical Propert ies of Solutions: 12.6 – 12.8 (Os motic pressure, collo ids, hydrophilic and
hydrophobic colloids).
Problems: Co lligative Properties of Nonelectrolyte Solutions: 12.46, 12.50, 12.87; Colligative Properties of
Electrolyte So lutions: 12.69, 12.74, 12.76; Colloids: 12.83, 12.84.

M 5/1
Catch up on Chapter 12.
Questions about final exam.

W 5/3
Review for final exam.

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