TAILIEUCHUNG - Ebook Instant notes - Inorganic chemistry (2nd edition): Part 2

(BQ) Part 2 book "Instant notes - Inorganic chemistry" has contents: Chemistry of nonmetals, chemistry of non-transition metals, chemistry of transition metals, lanthanides and actinides, environmental, biological and industrial aspects. | SECTION E—CHEMISTRY IN SOLUTION 147 Fig. 2. Frost diagram for Mn at pH=0 (solid line) and pH=14 (dashed line). The equilibrium constant of this reaction can be calculated by noting that it is made up from the half reactions for MnO2/Mn3+ and Mn3+/Mn2+ each with n=1, and has from Fig. 1. giving K=2×109. The V and MnVI are similarly unstable to disproportionation at pH=0, whereas at pH=14, also shown in Fig. 2. states Mn only MnV will disproportionate. Latimer and Frost diagrams display the same information but in a different way. When interpreting electrode potential data, either in numerical or graphical form, it is important to remember that a single potential in isolation has no meaning, Kinetic limitations Electrode potentials are thermodynamic quantities and show nothing about how fast a redox reaction can take place (see Topic B3). Simple electron transfer reactions (as in Mn3+/Mn2+) are expected to be rapid, but redox reactions where covalent bonds are made or broken may be much slower (see Topics F9 and H7). For example, the potential is well above that for the oxidation of water (see O2/H2O in Table 1), but the predicted reaction happens very slowly and aqueous permanganate is commonly used as an oxidizing agent (although it should always be standardized before use in volumetric analysis). Kinetic problems can also affect redox reactions at electrodes when covalent substances are involved. For example, a practical hydrogen electrode uses specially prepared platinum with a high surface area to act as a catalyst for the dissociation of dihydrogen into atoms (see Topic J5). On other metals a high overpotential may be experienced, as a cell potential considerably larger than the equilibrium value is necessary for a reaction to occur at an appreciable rate. Section F— Chemistry of nonmetals F1 INTRODUCTION TO NONMETALS Key Notes Covalent chemistry Ionic chemistry Acid-base chemistry Redox chemistry Related topics Hydrogen and boron stand out in their

• Hoá học
• Inorganic chemistry
• Chemistry of nonmetals
• Chemistry of non transition metals
• Chemistry of transition metals
• Biological and industrial aspects
• Industrial aspects
• Structural Inorganic Chemistry
• Ebook Structural Inorganic Chemistry
• Structural formulae
• Inorganic compounds
• Symmetry elements
• Regular solids
• Chemistry in solution
• Atomic structure
• Inorganic substances
• Bonding in molecules
• Bonding in solids
• Handbook of inorganic chemistry
• Ammonium phosphate
• Barium hydroxide
• Argon hydroquinone clathrate
• Varium nitrate boron
• Bismuth nitrate pentahydrate
• The transition elements
• Advanced inorganic chemistry
• The electronic structures
• Organometallic compounds
• Homogeneous catalytic reactions
• Transition matal complexes
• Summetry and structure
• Ionic solidsm ther extended arrays
• The nature of chemical bonding
• Concise inorganic chemistry
• The periodic table
• Introduction to bonding
• The ionic bond
• The covalent bond
• General properties of the elements
• Coordination compounds
• The hydrides
• Group I The alkali matals
• Descriptive inorganic chemistry
• Covalent bonding
• Ionic bonding
• Solvent systems
• Acid base behavior
• Oxidation and reduction
• The pnictogens
• The group 18 elements
• The noble gases
• Transition metal complexes
• The group 12 elements
• Nomenclature of inorganic chemistry
• Compositional nomenclature
• Parent hydride names
• Substitutive nomenclature
• Describing the configuration
• Coordination entities
• Final remarks
• rganometallic compoundsc
• Reactions and mechanisms
• Coordination chemistry IV
• Organometallic chemistry
• Parallels between main group
• The group 17 elements
• The second and third row metals
• d Block metal chemistry
• General considerations
• simple bonding theory
• Symmetry and group theory
• Coordination chemistry I
• The crystalline solid state
• Summary of Thesis will Advanced Science Education
• Theory and Methods of Teaching Chemistry
• Self study ability of students
• General Inorganic Chemistry
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• Summary of chemistry doctoral thesis
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• metals
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• Ebook Inorganic Chemistry
• Hóa học vô cơ
• Sách hóa vô cơ
• Cấu trúc hóa học
• Some basic concepts
• Nuclear properties
• Bonding in polyatomic molecules
• Polyatomic molecules
• Ionic solids
• Ions in aqueous solution
• Đề cương môn học
• Hóa vô cơ
• Các chất vô cơ
• Tính acid – base
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• A guidebook to mechanism in organic chemistry
• Nucleophilic substitution
• Aromatic systems
• Elimination reactions
• Linear free energy relationships
• Symmetry controlled reactions
• Nickel carbonate
• Niobium pentafluoride
• Palladium dichloride
• Palladium nitrate
• Phosphonium iodide
• Phosphorus trichloride