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2 basic concepts of chemistry 2 3 Chemical formulas and terms Relationship between configuration of valence electrons and chemical reactivity,
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26449_8contentsgenchem.pdf
1. Introduction
2. basic concepts of chemistry
2.1 Classification of matter
States of matter: solid, liquid, gas
Phase transitions, phase diagrams
Pure substances: elements, compounds
Mixtures: heterogeneous and homogeneous mixtures
Separation methods
2.2 Structure of matter, atomic theory
Matter is discontinuous, Dalton's atomic theory, law of conservation of mass, law of mul- tiple proportions, law of constant proportions
2.3 Chemical formulas and terms
Analysis (decomposition), synthesis (production), reaction (metathesis: transformation), reaction equation.
3. atomic structure and periodic table
Structure of atoms, size and mass of atoms
Atomic nucleus, electron shell, Bohr's atomic model, spectral lines, size of atom and atomic nucleus Subatomic particles
Electrons, protons, neutrons
Structure of the electron shell
s, p, d, f - orbitals, quantum numbers, Pauli's principle, Hund's rule, electron configurati- on, noble gas configuration, stability with half or completely filled shells, valence elec- trons
Periodic table of the elements
Relationship between configuration of valence electrons and chemical reactivity, similar behavior of elements of a group, tendencies in periods, ionization potential, electron affi- nity, electronegativity
3. atomic structure and periodic table
Structure of atoms, size and mass of atoms
Atomic nucleus, electron shell, Bohr
' s atomic model, spectral lines, size of atom and atomic nucleus Subatomic particles
Electrons, protons, neutrons
Structure of the electron shell
s, p, d, f - orbitals, quantum numbers, Pauli principle, Hund's rule, electron configurati- on, noble gas configuration, stability with half or completely filled shells, valence elec- trons, Periodic table of the elements Relationship between configuration of valence electrons and chemical reactivity, similar behavior of elements of a group, tendencies in periods, ionization potential, electron affi- nity, electronegativity
4. chemical bonding and chemical formulas
Atomic orbitals, molecular orbitals, molecular formulae
Ionic bond: Cation, anion, crystal lattice,
Metallic bond, Metal lattice, free electron gas, band model, electrical conductivity due to mobile charge carriers Covalent bonds: single bond, multiple bond, hybridization, mesomeric formulas, formal charges
Spatial structure of molecules
VSEPR model, free electron pairs, Lewis formulas, structural formula, structural isome- rism Structure of solids: ionic crystal lattice, metallic crystal lattice, solids of covalently bon- ded molecules
5 Reaction and reaction equation
5.1 Reaction equations: Balancing reaction equations, stoichiometry, redox reactions,
reduction and oxidation equations, oxidation numbers, combustion of hydrocarbons
5.2 Quantity of substances
Number of particles (atoms, molecules) in matter, Avogadro's constant, mass fraction,
5.3 Driving force of reactions; Why do reactions occur?
6. reaction kinetics
6.1 Basic concepts: Definition of the reaction rate and a rate constant, dependence of
the reaction rate on the concentrations of the reactants.
6.2 2nd order reaction
6.3 1st order reaction
6.4 Temperature dependence of the rate constant 6.6 Temperature dependence of the
equilibrium constant in the MWG
7 Chemical equilibrium
7.1 Mass action law
Mass action constant, dynamic equilibrium
7.2 Principle of the smallest constraint (Le Chatelier)
external constraints (pressure, concentration, temperature)
7.3 Solubility product: Solubility of salts
7.4 Autoprotolysis of water: Ionic product
8 Aqueous solutions
Concentration data, calculation of mixtures
8.1 Definition of pH value
8.2 Acids, bases, salts
Acid-base concept according to Arrhenius (proton donors, proton acceptors)
8.3 Strong and weak acids
8.4 Salts of weak acids
8.5 Buffers
9. thermochemistry
9.1 Definitions
9.2 Heat of reaction, energy of reaction, enthalpy of reaction
9.3 Standard enthalpies of formation
9.4 Theorem of Hess
9.5 Born-Haber circular process
10. gases
10.1 ideal gas law
10.2 partial pressure
11. solutions
11.1 phase diagram
11.2 Interactions in liquids
11.3 Temperature dependence of solubility
11.4 Vapor pressure of solutions
11.5 Distillation
12. liquids, phase equilibria
12.1 State diagram
12.2 Temperature dependence of vapor pressure
12.3 Boiling point of liquids
13. electrochemistry
13.1 Electrical conductivity in solutions
13.2 Electrolysis
13.3 Electromotive force of a cell
13.4 Nernst equation
14. organic chemistry