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1、高中化学资料（High school chemistry）The first part is basic concept and basic theory1. Oxidation - reduction reaction1. How to determine the oxidation-reduction reactionAppearance: valence lifting essence: electron transferNote: the reaction must be oxidizing - reducing reaction2. Related conceptsOxidation
2、 (oxidative) oxidizing product (oxidation)Reductive (reducible) reductive (reducible) reductive product (performance reductive)Note: (1) in the same reaction, oxidation and reduction reactions occur simultaneously(2) use the shunt-slip to remember rise and loss of oxygen, drop to return, if the agen
3、t is opposite, oxidation corresponds to the oxidation product, and the reduction corresponds to the reduction product.3. Analysis of oxidation - reduction reaction methodSingle bridge:Double bridge:Note: (1) the valence of the common elements must be remembered. If you are not familiar with the anal
4、ysis, you can use the coordinate method to analyze it.(2) in the same REDOX reaction, the total amount of the oxidant is equal to the total number of electrons lost.4. The judgment of oxidation and reducingOxidizing agent: the element that is at the highest price is only oxidized.The most high price
5、 elements (KMnO4, HNO3, etc.) most non-metallic single materials (Cl2, O2, etc.)Reductant (reducibility) : all elements that are in the lowest price are only reductive.The lowest price element (H2S, I - etc.) metal single matterA substance that is both oxidized and reductive: an element in an interm
6、ediate stateNote: (1) the general oxidation reduction reaction can be expressed as: oxidant + reducing agent = oxidizing product + reduction productOxidative strong peroxidation of oxidants, reducing the reductive property of reductants.(2) when there are multiple elements in a substance that are si
7、gnificantly oxidizing or reducing, remember that the strong dominant (zinc and nitric acid reaction cant produce hydrogen?)(3) remember that strong and weak interactions (that is, the easier it is to have electrons, the harder it is to lose electrons, and vice versa) remember (1) the sequence of met
8、al activities(2) the law of gradual change of the same period and the nature of the elements of the main group(3) non-metallic activity sequenceElements: O F Cl Br N I S P Si C HElemental: F2 Cl2 O2 Br2 I2 S n P C Si H2(4) relationship between oxidation and reducingF2 KmnO4 (H +) Cl2 thin HNO3 thick
9、 H2SO4 Br2 Fe3 + Cu2 + I2 H + 0 Fe2 +F - Mn2 + Cl - NO2 Br - Br - I - I - Fe5. Balance of REDOX reaction equationPrinciple: in the same reaction, the total amount of the oxidant is equal to the total number of electrons lostStep: change the column, find the multiple, and the coefficientNote: in the
10、equation, if a certain element has multiple atomic variations, the number of atoms in the valence element can be balanced first, and the calculation of valence fluctuation is calculated as a whole.Type: general filling and vacancy filling (general water shortage, acid and alkali)Ion reaction, ion eq
11、uation1. Judgment of ion reaction: the reaction that is carried out in aqueous solution is ion reaction2. Writing steps of the ion equation: write, remove, delete, and checkNote: (1) which substances should be dismounted into ionic forms and which should be retained. It is important to remember that
12、 the strong acid, strong alkali, soluble salt salt is to be removed as ionic mode, and the remaining molecular formula should be retained. The special treatment method of concentrated sulfuric acid and microlysote is also required(2) (2) check the method of positive error of ion equation, three chec
13、ks (charge conservation, conservation of mass, coincidence of reaction facts)3. Coexistence of ionsNo one of the following situations can coexist(1) formation of refractory productsCommon AgBr, AgCl, AgI, CaCO3, BaCO3, CaSO3, BaSO3, etc(2) produce volatile substancesCommon NH3, CO2, SO2, HCl, etc(3)
14、 formation of difficult ionizing substancesCommon water, ammonia, weak acid, weak base and so on(4) oxidation reduction reaction occursFe3 + and S2 -, ClO - and S2 -Iii. Atomic structure1. RelationshipNuclear charge = proton number = nuclear number = atomic number = atomic number (Z)Mass number (A)
15、= proton number (Z) + neutron number (N)Note: chemical reactions only change the number of electrons in the outermost shell, soThe number of electrons in the anionic nucleus is equal to the number of protons + | and |Cationic electron number = proton number - BBB 02. What it means3. IsotopesAtoms of
16、 the same atom with the same number of protons and different neutrons.Note:(1) isotopes refer to atoms, not ones or compounds(2) must mean the same element(3) the chemical properties are almost identicalThe arrangement of electrons outside the nucleus(1) characteristics of sports:(2) describe the me
17、thod of electronic movement:(3) configuration of the electron outside the nucleus:Symbol K L M N O P Q1, 2, 3, 4, 5, 6, 7(4) master the writing of atomic structure schematicFour rules to be observed in off-core electron configurationIv. Periodic table of elements and periodic table1. What is the per
18、iodic law?What is atomic number? What is the periodic law? The essence of the periodic law? Who discovered the periodic law?2. The structure of the periodic table(1) the period ordinal = the number of primary number of the electron layer = the outer electron number = highest positive valence(2) reme
19、mber seven cycles, three long, three short and one not all, eighteen and sixteen, and seven of the seven are still zero and eight.(3) periodic ordinal number: one, two, three, four, five, sixNumber of elements: 2, 8, 8, 18, 18, 32(4) order of the nationalities (from left to right), A and B , B, , B,
20、 B , , B, B, B A and A, A, , A, O ANote: A cycle with A element does not necessarily adjacent3. Determination of the nature of elementsIts easy to react with water or acidGold propertyThe alkalinity of hydroxide is weakIts not easy to react with hydrogenThermal stability of non-metallic hydridesThe
21、highest price oxygenate acidityNote: the above is also true.4. Gradual change of elements(1) the change rule of the same period and the nature of the elemental elementsNote: gold attribute (i.e., the property of the lost electron, which is reductive), non-metallic (the property of the electron, is o
22、xidized(2) judgment of atomic radius size: firstly, analyze the number of the electron layer and then analyze the atomic number (the more the general layer, the larger the radius, the larger the number of the same atomic number, the smaller the radius)5. ValenceValence electrons are the peripheral e
23、lectrons (the primary family element is the outermost electron)Main number = maximum number of electrons = highest positive price | negative | + maximum positive value = 8Note: number of atomic number, number of groups, valence, number of outermost electrons6. The application of the periodic table:
24、position, structure and sex5. Molecular structureTo master one force, two keys, three crystals1. BondsRemember concepts, types of bonds (ionic bonds, covalent bonds, metal bonds)2. Ionic bonds(1) remember the definition(2) the formation of ionic bond conditions: lively metal elements ( A, A) and liv
25、ely nonmetallic elements ( A, A) chemical combination between (3) the comparison of ionic radius size: (shell) compared with A rare elements of the same ionic radiusThe electron layer has the same ion, the radius increases with the atomic number and the radius decreases3. Covalent bonds(1) definitio
26、n(2) the type of covalent bond: non polar bond between (atomic element) covalent bond polar bond between (atomic element) (3) a few parameters of covalent bond, bond length, bond energy, bond Angle) :4. Electronic formula(1) definition(2) the similarities and differences between the covalent bonds and the electronic equivalent of ionic bonds5, crystal(1) ionic crystals, molecular crystals, atomic crystals(2) comparison of three crystals (bonding particles, interaction between particles and physical properties)(3) notice the structural characteristics of several common crystals