The Physical Science Lines I and II
General Chemistry 1st year
3 perods per week
Textbook: Chemistry; The Central Science
by T.L. Brown, H.E. LeMay Jr., B.E. Bursten, and C.J Murphy,
Chapters: 1 – 4
Ch. 1 Matter and Measurements
Classification and properties of matter, SI and derived SI units, precision and accuracy,
significant figures in calculations, dimensional analysis.
Ch. 2 Atoms, molecules, and ions
Atomic theory, atomic and mass numbers, isotopes, atomic and average atomic masses,
molecular and empirical formulas, predicting ionic charges and ionic compounds,
nomenclature of ionic and binary molecular compounds, alkanes and some simple
derivatives of alkanes.
Ch. 3 Calculations with Chemical Formulas and Equations
Balancing equations, states of reactants and products, formula and molecular weights, mole,
molar mass, interconverting mass, moles and number of particles. Empirical formulas from
elemental analysis, stoichiometry and quantitative information from balanced equations,
limiting reactants and theoretical yields.
Ch. 4 Aqueous Reactions and Solution Stoichiometry
General properties of aqueous solutions: electrolytic properties, ionic and molecular
compounds in water, strong and weak electrolytes.
Precipitation reactions: Solubility guidelines for ionic compounds, metathesis reactions,
ionic equations.
Acid-base reactions: strong and weak acids and bases, neutralization reactions and salt
formation.
Oxidation-reduction reactions: oxidation numbers, oxidation of metals by acids and metal
salts, activity series.
Concentration of solutions: molarity, interconverting molarity, moles and volume. Dilution,
solution stoichiometry and chemical analysis by titrations.
General Chemistry 2nd year
3 perods per week
Textbook: Chemistry; The Central Science
By T.L. Brown, H.E. LeMay Jr., B.E. Bursten, and C.J Murphy
Chapters: 5-11
Ch. 5 Thermochemistry
Nature and units of energy, the first law of thermodynamics, relating internal energy change
to heat and work, endo- and exothermic processes, enthalpy and enthalpies of reactions,
calorimetry, Hess´s law, enthalpies of formation.
Ch. 6 Electronic Structure of Atoms
The wave and particle nature of light, photon energy, line spectra and Bohr hydrogen
model, quantum mechanics and atomic orbitals, electron configuration of many-electron
atoms, electron configuration and the Periodic table.
Ch. 7 Periodic Properties of the Elements
Effective nuclear charge and trends in properties: sizes of atoms and ions, ionic energy,
electron affinities.
Metals, nonmetals and metalloids, group trends in alkali and earth alkali metals, oxygen
group, halogens and nobel gases.
Ch. 8 Basic Concepts of Chemical Bonding
Ionic and covalent bonds, octet rule, bond polarity and electronegativity, Lewis structures,
formal charges, resonance structures, exceptions to the octet rule, bond enthalpies and
enthalpies of reactions.
Ch. 9 Molecular Geometry and Bonding Theories
Molecular shapes and the VSEPR model, molecular polarity, a short introduction to
covalent bonding and orbital overlap.
Ch. 10 Gases
Pressure, barometer, the gas laws of Boyle, Charles and Avogadro. The ideal-gas equation
and its application in chemical reactions, gas mixtures and partial pressures, kineticmolecular theory.
Ch. 11 Intermolecular Forces, Liquids and Solids
A molecular comparison of gases, liquids and solids.
Intermolecular forces: ion-dipole, dipole-dipole, London dispersion, hydrogen bonding,
comparison of intermolecular forces, viscosity and surface tension of liquids.
Vapor pressure: effect of intermolecular forces, temperature dependence, boiling point.
Structure of solids: simple, body-centered and face-centered cubic unit cells, NaCl(s)structure.
Bonding in solids: molecular, covalent-network, ionic and metallic solids.
Ch. 25 The Chemistry of Life: Organic and Biological Chemistry
Hybridizations, sp3-, sp2- and sp3-orbitals, - and - bonds, structural isomers,
nomenclature, structural and physical properties of: alkanes, cycloalkanes, and alkenes.
Laboratory experiments: 2x40 min. every other week
The chemistry experiments are largely bases on:
Chemistry with Computers using Logger ProTM and Vernier Sensors,
by D.D. Holmquist and D. L. Volz
1.
Formation and reactions of carbon dioxide
2.
Planning and preparations of solutions
3.
Endo- and exothermic reactions
4.
Additivity of heats of reaction: Hess´s Law
5.
Analysis of FeSO4•nH2O by permanganate titration
6.
Determination of the stoichiometry of the iodometric reaction
7.
Conductivity of solutions: The effect of concentration
8.
Determining the concentration of a solution: Beer´s Law
9.
Pressure-temperature relationship of a gas
10 Reaction of magnesium in hydrochloric acid: collecting and determining the amount
of a hydrogen gas
11. Evaporation and intermolecular forces
12. Structures and nomenclature of organic molecules: an exercise using the program
ChemSketch.
General Chemistry 3rd year
4 perods per week
Textbook: Chemistry; The Central Science
By T.L. Brown, H.E. LeMay Jr., B.E. Bursten, and C.J. Murphy
Chapters: 13-17. 19-20 and 25
Ch. 15 Chemical Equilibrium
The law of equilibrium, equilibrium constants Kc and Kp, heterogeneous equilibria,
calculating equilibrium constants. Application of equilibrium constants: reaction quotient
and direction of a reaction, calculating equilibrium concentrations.
Le Chatelier principle: effect of change in concentrations, volume, pressure and
temperature. The effect of catalysts.
Ch. 16 Acid-Base Equilibria
Brönsted-Lowry acids-base definition, autoionization of water, pH scale, strong and weak
acids and bases, calculating pH of weak acid and weak base solutions and solutions of their
salts, polyprotic acids, acid-base properties of salt solutions, acid-base behavior and
chemical structure, Lewis acids and bases.
Ch. 17 Additional Aspect of Aqueous Equilibria
Common-ion effect, buffered solution, calculating the pH-curve for a acid-base titration:
strong acid–strong base, weak acid-strong base, weak base-strong acid.
Solubility equilibria, solubility product constant (Ksp), solubility (g/L) and molar solubility.
The effect of common-ion, pH and complex formation on solubility. Precipitation and
separation of ions.
Ch. 14 Chemical Kinetics
Reaction rate, determining a rate law from initial rates, temperature and rate, collision
model, orientation factor and activation energy, Arrhenius equation, determining activation
energy. Reaction mechanism: elementary reactions and their rate laws, rate-determining
step, deriving a rate law for few simple multistep mechanism. Catalysis: homogenous and
heterogenous catalysis, enzymes.
Ch. 19 Chemical Thermodynamics
Spontaneous processes, entropy and the second law of thermodynamics, a short introduction
to the molecular interpretation of entropy, entropy change in chemical reactions, Gibbs free
energy, free energy and temperature, free energy and the equilibrium constant.
Ch. 20 Electrochemistry
Balancing oxidation-reduction reactions, voltaic cells, cell electromotive force (EMF), free
energy and EMF, Nernst equation, concentration cells, batteries, corrosion, electrolysis.
Ch. 25 The Chemistry of Life: Organic and Biological Chemistry
Hybridizations, sp3-, sp2- and sp3-orbitals, - and - bonds, structural isomers, stereo
isomers, chirality.
Nomenclature, structural and physical properties of: alkanes, alkenes, alkynes, alcohols,
ethers, aldehydes, ketones, carboxylic acids and derivatives. Biochemistry: amino acids,
peptides and proteins, protein structure, carbohydrates, disaccharides and polysaccharides,
nucleic acids, DNA.
Ch. 13 Properties of Solutions
Solution formation: energy change, spontaneity, chemical reaction. Unsaturated, saturated
and supersaturated solutions.
Factors effecting solubility: solute-solvent interactions, pressure effects, Henry´s law,
temperature effects.
Ways of expressing concentration: mass percentage, ppm, mole fraction, molality,
conversion of concentration units.
Colligative properties: Boiling-point elevation, freezing-point depression
Laboratory experiments: 2 periods every other week
The chemistry experiments are largely bases on:
Chemistry with Computers using Logger ProTM and Vernier Sensors,
by D.D. Holmquist and D. L. Volz
1.
Using conductivity to find the equivalence point for the reaction between saturated
Ba(OH)2 and H2SO4
2.
Colorimetric determination of Kc for: Fe3+ + SCN-  FeSCN2+
3.
The temperature dependence of the vapor pressure of methanol.
4.
Titration curve of a weak acid measured with a computer-interfaced pH electrode.
5.
Titration curve of a Na2A salt measured with a computer-interfaced pH electrode.
6.
Separation of a mixture of Ni2+, Co2+ and Fe3+ with an ion-exchange column.
7.
Determination of the composition of Cu(NH3)n2+ complex by HCl titration of aqueous
and chloroform solutions.
8.
Determination of the rate law of:
S2O82- + 2I-  2SO42- + I2
9.
Electrochemical cell: establishing a table of reduction potential and application of
Nernst equation.
10. Electrolysis of potassium iodide solution: identification of products and halfreactions.
11. EDTA-titration analysis of calcium in milk.
12. Determination of molecular weight by freezing-point depression.
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