Redox reactions - презентация, доклад, проект скачать

Нажмите для полного просмотра!

Содержание ▲

Вы можете ознакомиться и скачать презентацию на тему Redox reactions. Доклад-сообщение содержит 20 слайдов. Презентации для любого класса можно скачать бесплатно. Если материал и наш сайт презентаций Mypresentation Вам понравились – поделитесь им с друзьями с помощью социальных кнопок и добавьте в закладки в своем браузере.

Слайды и текст этой презентации

Слайд 1

Описание слайда:

Redox reactions

Слайд 2

Описание слайда:

The concept of redox reactions Redox reactions - chemical reactions that occur with a change in the oxidation state of the elements included in the reactants

Слайд 3

Описание слайда:

Oxidation - the process of recoil electrons an atom, molecule or ion. Atoms are converted into positively charged ion: Zn0 – 2e → Zn2+ negatively charged ion becomes neutral atom: 2Cl- -2e →Cl20 S2- -2e →S0 The value of the positively charged ion (an atom) is increased accordingly the number of electron donating: Fe2+ -1e →Fe3+ Mn+2 -2e →Mn+4

Слайд 4

Описание слайда:

Recovery - the process of accession of electrons an atom, molecule or ion. Recovery - the process of accession of electrons an atom, molecule or ion. Atom converted to a negatively charged ion S0 + 2e → S2− Br0 + e → Br − The value of the positively charged ions (atoms) reduced by the number of electrons attached: Mn+7 + 5e → Mn+2 S+6 + 2e → S+4 − or it can go into a neutral atom: Н+ + е → Н0 Cu2+ + 2e → Cu0

Слайд 5

Описание слайда:

Recovery - atoms, molecules, or ions donate electrons. They are in the process redox reaction oxidized Recovery - atoms, molecules, or ions donate electrons. They are in the process redox reaction oxidized Typical reductants: ● metal atoms with high atomic radii (I-A, II-A group), as well as Fe, Al, Zn ● simple substances, non-metals: hydrogen, carbon, boron; ● negative ions: Cl−, Br−, I−, S2−, N−3. We are reducing the fluoride ion F−. ● metal ions in lower oxidation states: Fe2+,Cu+,Mn2+,Cr3+; ● complex ions and molecules containing atoms with intermediate oxidation state: SO32−, NO2−; СО, MnO2 and others.

Слайд 6

Описание слайда:

Oxidants - atoms, molecules or ions, electrons join. They are in the process of oxidation-reduction reactions are restored Oxidants - atoms, molecules or ions, electrons join. They are in the process of oxidation-reduction reactions are restored Typical oxidizers: ● nonmetal atoms VII-A, VI-A, VA group consisting of simple substances ● metal ions in the higher oxidation state: Cu2+, Fe3+,Ag+ … ● Complex ions and molecules containing atoms with the highest and lowest oxidation state:с.о.: SO42−, NO3−, MnO4−, СlО3−, Cr2O72-, SO3, MnO2 and others

Слайд 7

Описание слайда:

On the display of the redox properties of the effect of such factors as the stability of the molecule or ion. The stronger the particle, the less it shows the redox properties

Слайд 8

Описание слайда:

The degree of oxidation of sulfur: -2,0,+4,+6 Н2S-2 - reductant 2Н2S+3O2=2H2O+2SO2 S0,S+4O2 – oxidant and reductant S+O2=SO2 2SO2+O2=2SO3 (reductant) S+2Na=Na2S SO2+2H2S=3S+2H2O (oxidant) Н2S+6O4 - oxidant Cu+2H2SO4=CuSO4+SO2+2H2O

Слайд 9

Описание слайда:

Определение степеней окисления атомов химических элементов The oxidation state of atoms of chemical elements in the simple substance = 0 The algebraic sum of oxidation states of all elements in the ion is the ion charge The algebraic sum of oxidation states of all elements in the composite material is 0.

Слайд 10

Описание слайда:

Classification of redox reactions Intermolecular oxidation reactions 2Al0 + 3Cl20 → 2Al+3 Cl3-1 Intramolecular oxidation 2KCl+5O3-2 →2KCl-1 + 3O20 Disproportionation, dismutation (repair itself, autoxidation): 3Cl20 + 6KOH (гор.) →KCl+5O3 +5KCl-1+3H2O 2N+4O2+ H2O →HN+3O2 + HN+5O3

Слайд 11

Описание слайда:

The value of redox reactions Redox reactions are very common. They linked the metabolic processes in living organisms, respiration, rotting, fermentation, photosynthesis. Redox reactions provide the cycling of matter in nature. They can be seen from the combustion and smelting of metal corrosion. With their help prepared alkalis, acids and other valuable chemicals. Redox reactions underlie energy conversion interacting chemicals in eclectic energy in the battery cell.

Слайд 12

Описание слайда:

Corrosion of metals Methods corrosion protection

Слайд 13

Описание слайда:

CORROSION - spontaneous destruction of metals and alloys as a result of chemical and electrochemical interactions with their environment. CORROSION - spontaneous destruction of metals and alloys as a result of chemical and electrochemical interactions with their environment. This redox reaction in which the metal atoms become ions. The more active the metal, so it is more susceptible to corrosion. In the role of an oxidant act atmospheric oxygen and hydrogen cations.

Слайд 14

Описание слайда:

Oxygen and atmospheric moisture Oxygen and atmospheric moisture Carbon and sulfur gases contained in the atmosphere Sea water Groundwater

Слайд 15

Описание слайда:

Слайд 16

Описание слайда:

CHEMICAL - a failure of metals and alloys as a result of their chemical interactions with the substances of the environment. CHEMICAL - a failure of metals and alloys as a result of their chemical interactions with the substances of the environment. The protective oxide film on the aluminum surface Loose film on the iron surface, leading to destruction of metal

Слайд 17

Описание слайда:

Electrochemical - a failure of metals, which is accompanied by the appearance of an electric current in water or another electrolyte medium. Electrochemical - a failure of metals, which is accompanied by the appearance of an electric current in water or another electrolyte medium. Chemical processes - this oxidation metal recoil electrons. Electrical processes - transfer of electrons from one site to another product.

Слайд 18

Описание слайда:

The position of the metal in a series of activity of metal: the farther they are from each other, the faster corrosion. The position of the metal in a series of activity of metal: the farther they are from each other, the faster corrosion. The purity of the metal: the impurity accelerate corrosion. Irregularities in the metal surface cracks. Ground water, sea water, the environment of the electrolyte. Temperature increase. The action of microorganisms (fungi, bacteria, lichens to metals with high corrosion resistance).

Слайд 19

Описание слайда:

The application of protective coatings (paints, varnishes, enamels); The application of protective coatings (paints, varnishes, enamels); Covering other metals (gold-plated, silver, chrome, zinc plating); Creation and use of corrosion-resistant alloys Introduction to the inhibitors reduce aggressive environment; Sacrificial protection