Chapter I Periodic Law of Material Structure Elements
I. Atomic structure
Proton (z)
Nuclear comments:
Mass number of neutrons (n) (a) = proton number (z)+ neutron number (n)
1. atom (A X) atomic number = nuclear charge number = proton number = extranuclear electron number of atom.
extranuclear electron
★ Learn the first 20 elements by heart, and be familiar with the arrangement of electrons outside the nucleus of element 1 ~ 20:
Li He is a member of Canada.
2. The arrangement law of electrons outside the nucleus: ① The electrons are always arranged in the lowest energy electron layer first; ② The maximum number of electrons contained in each electron layer is 2n2；; ③ No more than 8 electrons in the outermost layer (no more than 2 electrons in the K layer), no more than 18 electrons in the second outer layer and no more than 32 electrons in the penultimate layer.
Electron layer: one (lowest energy) two three four five six seven
Corresponding symbol: K L M N O P Q
3. Elements, nuclides and isotopes
Element: A general term for atoms of the same kind with the same nuclear charge number.
Nuclide: An atom with a certain number of protons and a certain number of neutrons.
Isotope: Different atoms of the same element have the same number of protons but different numbers of neutrons, which are called isotopes. (for atoms)
Second, the periodic table of elements.
1. Arrangement principle:
① Arranged from left to right in the order of increasing atomic number.
② Arrange the elements with the same number of electron layers in a row from left to right. (Number of cycles = number of electron layers of atoms)
③ Arrange the elements with the same number of electrons in the outermost layer in a vertical line from top to bottom in the order of increasing number of electron layers.
Main group ordinal number = outermost electron number of atom
2. Structural features:
Element types of extranuclear electron shell
1 two elements in the first phase
A short period of 8 elements in the second period.
3 Eight elements in the third cycle
Yuan (Line 7) 4 18 Element Phase IV
Element (7 cycles) 5 18 Element in the fifth cycle
Six hundred and thirty-two elements in the sixth period of the period length period.
Period 7 is not filled (there are 26 elements).
Main subjects: 7 main subjects: ia ~ ⅶ a * * *.
Clan subfamily: Ⅲ b ~ ⅶ b ~ ⅶ b, Ⅰ b ~ Ⅱ b ~ Ⅱ b, ***7 subfamily.
(18 vertical row) the eighth family: three vertical rows, located between ⅶ b and Ⅰ b.
(16 family) zero family: rare gas.
Third, the periodic law of elements.
1. periodic law of elements: the properties of elements (extranuclear electron configuration, atomic radius, valence, metal and nonmetal) change periodically with the increase of nuclear charge. The periodic change of element properties is essentially the inevitable result of the periodic change of electron configuration outside the nucleus of elements.
2. The gradual change law of elements in the same period.
The third periodic element11na12mg13al14si15p16s17cl18ar.
The number of electron layers in (1) electronic configuration is the same, and the number of electrons in the outermost layer increases in turn.
(2) The atomic radius decreases in turn.
—
(3) Main price+1+2+3+4
-4 +5
-3 +6
-2 +7
- 1 —
(4) The performance of metals and nonmetals is weakened, while the performance of nonmetals is enhanced.
—
(5) It is difficult to replace cold water with water or acid.
Strong hot water and
Acid resistance and acid resistance reversal
It should be slow-
(6) Chemical formula of hydride-SiH4pH3 H2HCl-
(7) the difficulty of combining with H2-from difficult to easy.
—
(8) stability of hydride-stability enhancement
—
(9) The chemical formula of the highest valence oxide is Na2O MgO Al2O3 SiO 2 P2O5 SO3 Cl2 O7-
The highest valence oxide corresponds to the hydrate (10) chemical formula NaOH mg (oh) 2al (oh) 3H2SiO3PO4H2SO4 HCLO4-
Amphoteric hydrogen in (1 1) alkaline base
Strong oxide weak acid
Strong acid is very strong.
Acid—
(12) The alkalinity is weakened and the acidity is enhanced.
—
Group ia alkali metal element: Li Na K Rb Cs Fr (Fr is the most metallic element, located at the lower left of the periodic table).
Group ⅶ A halogen element: F Cl Br I At (F is the most nonmetallic element, located at the upper right of the periodic table).
★ Method for judging the strength of metal and nonmetal elements:
(1) Strong (weak) metallicity-① Simple substance is easy (difficult) to react with water or acid to generate hydrogen; (2) Strong (weak) alkalinity of hydroxide; ③ Mutual substitution reaction (forced weak) Fe+CuSO4 = FeSO4+Cu.
(2) Strong (weak) nonmetal-① Simple substance is easy (difficult) to react with hydrogen; ② The generated hydride is stable (unstable); ③ The hydrate (oxyacid) of the highest valence oxide has strong (weak) acidity; ④ substitution reaction (forced weak) 2nab r+Cl2 = 2nac+br2.
(1) Compared with the same period:
Metal: sodium > magnesium > aluminum.
Reaction with acid or water: from easy to difficult
Alkalinity: NaOH > Mg (OH) 2 > Al (OH) 3.
Non-metal: silicon I (halogen element)
Reaction of simple substance with hydrogen: from easy to difficult
Hydride stability: HF > HCl > HBR > Hi.
(Ⅲ)
Metallic color: Li < na < k < Rb < cs.
Reducibility (ability to lose electrons): Li < na < k < Rb < cs.
Oxidizability (ability to acquire electrons): Li+> Na+> K+> r b+ > Cs+ nonmetallic: F > Cl > Br > I.
Oxidation: F2 > Cl2 > BR2 > I2.
Reducibility: f-< cl-< br-< I-
Acidity (anaerobic acid): HF < HCl < HBR < hi.
Method of comparing the radii of particles (including atoms and ions): (1) Compare the number of electron layers first, and the radius with more electron layers is larger.
(2) When the number of electron layers is the same, the radius with more nuclear charges is smaller.
Fourth, chemical bonds.
A chemical bond is a strong interaction between two or more adjacent atoms.
Comparison between ionic bond and valence bond of 1.* *
Ionic bond * * * valence bond
The concept of electrostatic interaction between anions and cations to form compounds is called ionic bond, and the interaction between atoms through electron pairs is called * * * valence bond.
Bonding method realizes stable structure by gaining and losing electrons, and realizes stable structure by forming * * * electron pairs.
Anionic and cationic atoms that bind particles.
Bonding elements between active metals and active nonmetallic elements (especially ammonium salts such as NH4Cl and NH4NO3 are only composed of nonmetallic elements, but contain ionic bonds).
Ionic compounds: Compounds composed of ionic bonds are called ionic compounds. (There must be ionic bonds, and there may also be valence bonds of * * *).
* * * Valence compounds: Compounds that form molecules through * * * electron pairs between atoms are called * * * valence compounds. (* * * price key only)
Polar valence bond (polar bond for short): formed by different kinds of atoms, A-B type, such as H-Cl.
* * * Valence bond
Nonpolar valence bond (nonpolar bond for short): formed by the same atom, A-A type, such as Cl-Cl.
2. Electronic:
The difference between the material structure formed by the electronic representation of ionic bond and the material structure formed by the valence bond of * * * is: (1) charge: the charge of cation and anion should be marked when the material structure formed by the electronic representation of ionic bond; However, the material structure representing the formation of valence bonds cannot be marked by charges. (2)[] (square brackets): Anions in substances formed by ionic bonds need to be enclosed in square brackets, and substances formed by valence bonds cannot be enclosed in square brackets.
Chapter II Chemical Reaction and Energy
Section 1 Chemical Energy and Thermal Energy
1 is always accompanied by energy changes in any chemical reaction.
Reason: When substances react chemically, breaking chemical bonds in reactants will absorb energy, while forming chemical bonds in products will release energy. The fracture and formation of chemical bonds are the main reasons for the energy change in chemical reactions. Whether a chemical reaction absorbs or releases energy in the process depends on the relative size of the total energy of reactants and the total energy of products. The total energy of reactant E > the total energy of product E is an exothermic reaction. The total energy of E reactant is less than that of E product, which is an endothermic reaction.
2. Common exothermic and endothermic reactions
Common exothermic reactions: ① complete combustion and slow oxidation. ② Acid-base neutralization reaction. ③ The metal reacts with acid to produce hydrogen.
④ Most chemical reactions (special: C+CO2 2co is endothermic reaction).
Common endothermic reactions: ① redox reactions with C, H2 and CO as reducing agents, such as C (S)+H2O (G) Co (G)+H2 (G).
(2) the reaction between ammonium salt and alkali, such as Ba(OH)2? 8H2O+NH4Cl = bacl 2+2n H3 ↑+ 10H2O
③ Most decomposition reactions such as KClO3, KMnO4, CaCO3, etc.
3, the classification of energy:
Forming conditions and utilizing historical nature
primary energy source
Conventional energy renewable resources hydropower, wind energy and biomass energy.
Non-renewable resources, such as fossil energy such as coal, oil and natural gas.
New energy renewable resources solar energy, wind energy, geothermal energy, tidal energy, hydrogen energy and biogas.
Non-renewable resource nuclear energy
Secondary energy (the energy obtained after processing and conversion of primary energy is called secondary energy)
Electric energy (hydropower, thermal power, nuclear power), steam, industrial waste heat, alcohol, gasoline, coke, etc.
[Thinking] Generally speaking, most combination reactions are exothermic reactions, and most decomposition reactions are endothermic reactions. The exothermic reaction needs no heating, while the endothermic reaction needs heating. Is this correct? For example.
Tap: This statement is wrong. For example, the reaction of C+O2 = CO2 is exothermic, but it needs to be heated, but it doesn't need to be heated after the reaction starts, and the heat released by the reaction can let the reaction continue. Ba(OH)2？ The reaction between 8H2O and NH4Cl is endothermic, but the reaction does not need heating.
Chemical energy and electric energy in the second quarter
1, chemical energy is converted into electrical energy:
electric energy
(Electric power) Thermal power (thermal power generation) Chemical energy → thermal energy → mechanical energy → electric energy Disadvantages: it pollutes the environment and has low efficiency.
The advantages of direct conversion of chemical energy into electrical energy by primary batteries are cleanliness and high efficiency.
2. The principle of galvanic cell
(1) concept: The device that directly converts chemical energy into electrical energy is called a galvanic cell.
(2) Working principle of primary battery: Chemical energy is converted into electrical energy through redox reaction (electron transfer).
(3) Conditions for forming a primary battery: (1) electrodes are conductors with different reactivity; (2) Two electrodes are in contact (wire connection or direct contact); (3) Insert two interconnected electrodes into the electrolyte solution to form a closed loop.
(4) electrode name and reaction:
Negative electrode: the metal with high activity is used as the negative electrode, and the negative electrode undergoes oxidation reaction.
Electrode reaction formula: more active metal -ne-= metal cation.
Negative electrode phenomenon: the negative electrode dissolves and the mass decreases.
Positive electrode: metal or graphite with low activity is used as the positive electrode, and the positive electrode undergoes reduction reaction.
Electrode reaction formula: cation in solution +ne-= simple substance.
Positive electrode phenomenon: generally, there is gas release or the quality of positive electrode increases.
(5) Method for judging the anode and cathode of primary battery:
(1) According to the material of the primary battery electrode:
More reactive metals are used as negative electrodes (potassium, calcium and sodium are too reactive to be used as electrodes);
Metal or conductive nonmetal (graphite) and oxide (MnO2) with low activity are used as the positive electrode.
② According to current direction or electron flow direction: (external circuit) current flows from the positive electrode to the negative electrode; Electrons flow from the negative electrode to the positive electrode of the primary battery through an external circuit.
③ According to the migration direction of ions in the internal circuit: cations flow to the positive electrode of the primary battery, and anions flow to the negative electrode of the primary battery.
(4) According to the reaction type in the primary battery:
Negative electrode: loss of electrons and oxidation reaction, usually the electrode itself is consumed and its mass is reduced.
Positive electrode: electrons are obtained and reduction reaction occurs, which is usually accompanied by precipitation of metal or release of H2.
(6) Writing method of galvanic cell electrode reaction:
(1) The chemical reaction principle of galvanic cell reaction is redox reaction, the negative electrode reaction is oxidation reaction and the positive electrode reaction is reduction reaction. Therefore, the method of writing electrode reaction can be summarized as follows:
① Write the total reaction equation. ② According to the gain and loss of electrons, the total reaction is divided into oxidation reaction and reduction reaction.
(3) The oxidation reaction takes place at the negative electrode and the reduction reaction takes place at the positive electrode. When the reactants and products are in proper positions, attention should be paid to the participation of acid-base medium and water.
(2) The total reaction formula of a primary battery is generally obtained by adding the positive and negative reaction formulas.
(7) Application of primary battery: ① Accelerate the chemical reaction rate, for example, the hydrogen production rate of crude zinc is faster than that of pure zinc. ② Compare the activity of metals. ③ Design a primary battery. ④ Corrosion of metals.
2. The basic types of chemical power supply:
① Dry battery: Active metal is used as the negative electrode, which is corroded or consumed. Such as copper-zinc primary battery and zinc-manganese battery.
(2) Rechargeable battery: The primary battery with two poles participating in the reaction can be recharged and recycled. Such as lead battery, lithium battery, silver-zinc battery, etc.
③ Fuel cell: The materials of both electrodes are inert electrodes, and the electrodes themselves do not react, but the substances introduced into the two electrodes react, such as H2 and CH4 fuel cells, and the electrolyte solution is often alkaline reagent (KOH, etc.). ).
The rate and limit of chemical reaction in the third quarter
1, the rate of chemical reaction
(1) concept: chemical reaction rate is usually expressed by the decrease of reactant concentration or the increase of product concentration per unit time (both positive values). Calculation formula: v (b) = =
① Unit: mol/(liter? S) or mol/(L? Minimum)
②B is a solution or a gas. If B is a solid or a pure liquid, the rate is not calculated.
(3) The above is the average rate, not the instantaneous rate.
④ Important laws: (1) rate ratio = equation coefficient ratio (2) change ratio = equation coefficient ratio.
(2) Factors affecting the chemical reaction rate:
Internal cause: (the main factor) is determined by the structure and properties of the substances involved in the reaction.
External factors: ① temperature: increase the temperature and speed.
② Catalyst: generally, the reaction speed is accelerated (positive catalyst).
③ Concentration: increase the concentration of reactant C and increase the rate (only solution or gas can have concentration).
④ Pressure: increase the pressure and speed (applicable to the reaction with gas).
⑤ Other factors, such as light (ray), solid surface area (particle size), reactant state (solvent), galvanic cell, etc. , will also change the chemical reaction rate.
2, the limit of chemical reaction-chemical equilibrium
(1) Under certain conditions, when a reversible reaction proceeds until the positive reaction rate is equal to the reverse reaction rate, the concentrations of reactants and products will not change and reach a seemingly static "equilibrium state", which is the limit that this reaction can reach, that is, the chemical equilibrium state.
The movement of chemical equilibrium is influenced by temperature, reactant concentration, pressure and other factors. The catalyst only changes the chemical reaction rate and has no effect on the chemical equilibrium.
Under the same conditions, reactions that proceed in both positive and negative directions at the same time are called reversible reactions. The reaction from reactant to product is usually called positive reaction. The reaction from product to reactant is called reverse reaction.
In any reversible reaction, the forward reaction should be carried out simultaneously with the reverse reaction. The reversible reaction can't go through to the end, that is, no matter how far the reversible reaction goes, the amount of any substance (reactant and product) can't be zero.
(2) Characteristics of chemical equilibrium state: inverse, dynamic, equal, constant and variable.
① Inverse: The research object of chemical equilibrium is reversible reaction.
② Dynamic: dynamic equilibrium, when the equilibrium state is reached, the positive and negative reactions continue.
3 and so on. When the equilibrium state is reached, the positive reaction rate and the reverse reaction rate are equal, but not equal to 0. That is, v is positive = v is negative ≠0.
④ Determination: When the equilibrium state is reached, the concentration of each component remains unchanged and the content of each component remains certain.
⑤ Change: When conditions change, the original balance will be destroyed and a new balance will be established under new conditions.
(3) Marks for judging the state of chemical equilibrium:
① VA (positive direction) = VA (negative direction) or nA (consumption) = NA (generation) (comparison of the same substance in different directions)
(2) The concentration or percentage content of each component remains unchanged.
(3) Judging by color invariance (there is a substance that is colored)
(4) The amount or total volume or total pressure or average relative molecular weight of the total substance remains unchanged (provided that the amount of the total substance of the gas before and after the reaction is not equal, that is, for the reaction XA+YbZC, X+Y ≠ Z).
Chapter III Organic Compounds
Most carbon-containing compounds are called organic compounds, or organic compounds for short. Some compounds, such as carbon monoxide, carbon dioxide, carbonic acid and carbonate, have always been regarded as inorganic compounds because their composition and properties are similar to inorganic compounds.
I. Hydrocarbons
1. Definition of hydrocarbons: Organic substances containing only carbon and hydrogen are called hydrocarbons, also known as hydrocarbons.
2, the classification of hydrocarbons:
Saturated hydrocarbon → alkane (such as methane)
Aliphatic hydrocarbon (chain)
Hydrocarbon unsaturated hydrocarbon → olefin (such as ethylene)
Aromatic hydrocarbon (containing benzene ring) (such as benzene)
3. Comparison of properties of methane, ethylene and benzene:
Organic alkanes, olefins, benzene and their homologues.
General formula CnH2n+2cnh 2n——
Representative methane (CH4), ethylene (C2H4) and benzene (C6H6).
Structural formula CH4 CH2 = CH2 or
(functional group)
Structural characteristics of C-C single bond,
Chain, saturated hydrocarbon c = c double bond,
The only bond between a single bond and a double bond, cyclic.
Spatial structure regular tetrahedron hexaatom plane regular hexagon
A colorless and odorless gas with physical properties, lighter than air, slightly soluble in water, lighter than air, slightly soluble in water, colorless and odorless liquid, lighter than water, slightly soluble in water.
High-quality fuel, chemical raw materials, petrochemical industrial raw materials, plant growth regulator, ripening agent solvent, chemical raw materials.
Main chemical properties of organic matter
Alkanes:
Methane ① oxidation reaction (combustion)
CH4+2O2-→ CO2+2H2O (light blue flame, no black smoke)
② Substitution reaction (note that light is the main reason for the reaction, and there are five kinds of products).
CH4+Cl2―→CH3Cl+HCl CH3Cl+Cl2―→ch2cl 2+HCl
CH2Cl2+Cl2―→CHCl3+HCl
Under the illumination condition, methane can also be replaced by bromine vapor.
Methane cannot discolor acidic KMnO4 solution, bromine water or bromine carbon tetrachloride solution.
Olefin:
Ethylene ① Oxidation Reaction (Ⅰ) Combustion
C2H4+3O2-→ 2co2+2h2o (bright flame and black smoke)
(2) Oxidation of acidic potassium permanganate solution will make acidic potassium permanganate solution fade.
② Addition reaction
CH2 = CH2+BR2-→ CH2BR-CH2BR (can make bromine water or bromine carbon tetrachloride solution fade)
Under certain conditions, ethylene can also react with H2, Cl2, HCl and H2O.
CH2 = CH2+H2―→ch3ch 3
CH2 = CH2+HCl-→ ch3ch2cl (chloroethane)
CH2 = CH2+H2O ―→ ch3ch2oh (ethanol production)
③ addition polymerization reaction NC H2 = CH2 ―→- CH2-CH2-n (polyethylene)
Ethylene can discolor acidic KMnO4 solution, bromine water or bromine carbon tetrachloride solution. This reaction is usually used to identify alkanes and olefins, such as methane and ethylene.
Benzene ① oxidation reaction (combustion)
2c6H6+15o2 -→12co2+6H2O (bright flame with smoke)
② substitution reaction
The hydrogen atom on the benzene ring is replaced by bromine atom and nitro group.
+Br2 ―→+ HBr
+nitric acid-―→ +H2O
③ Addition reaction
+3H2――→
Benzene cannot discolor acidic KMnO4 solution, bromine water or bromine carbon tetrachloride solution.
4. Comparison of homologues, isomers, allotropes and isotopes.
Concept homologue isomer allotrope isotope
One or several CH2 groups in the molecular composition are used to define the mutual names of substances with similar structures and different molecular formulas. Different simple substances composed of the same element have the same mutual names, but different atoms of the same element have different mutual names.
Different molecular formulas are the same, the symbols of the same elements are the same, and the molecular formulas can be different-
Similar structure, different, different—
The simple atom of the research object compound
6. Naming of alkanes:
(1) Common nomenclature: alkanes are generally called "some alkanes", and some refer to the number of carbon atoms in alkanes. 1- 10 uses Party A, Party B, Party C, Party D, Party E, Party A, Party G, Party A, Party B, Party B, Party C, Party C, Party B, Party C, Party C, Party C, Party C, Party C, Party C, Party C, Party C.
N-butane, isobutane; N-pentane, isopentane, neopentane.
(2) System terminology:
① Naming step: (1) Find the main chain-the longest carbon chain (determine the mother name); (2) Number-near one end of the branch chain (small but many);
(3) Write the name-simplify first and then complicate, please merge the same base.
② Name composition: substituent position-substituent name mother name
(3) Arabic numerals indicate the positions of substituents, and chinese numerals indicates the number of identical substituents.
CH3-CH-CH2-CH3
2- methylbutane
7. Compare the boiling points of similar hydrocarbons:
① At first glance, there are many carbon atoms and high boiling point.
② The number of carbon atoms is the same. Second, the boiling point of branched chain is low.
At room temperature, hydrocarbons with 1-4 carbon atoms are all gases.
Second, derivatives of hydrocarbons.
Comparison of properties of 1, ethanol and acetic acid
Organic saturated monohydric alcohol saturated monohydric aldehyde saturated monocarboxylic acid
The general formula cnh2n+1oh-cnh2n+1cooh.
Representative ethanol acetaldehyde acetic acid
Simple molecular formula CH3CH2OH
Or C2 H5 ohch 3 choch 3 cooh.
Hydroxyl functional group: -oh
Aldehyde group:-CHO
Carboxyl:-COOH
A colorless liquid with special fragrance, commonly known as alcohol, is easily soluble in water and volatile.
(Non-electrolyte)-Colorless liquid with strong pungent smell, commonly known as acetic acid, easily soluble in water and ethanol, and anhydrous acetic acid is also called glacial acetic acid.
Used as fuel, beverage and chemical raw materials; Used for medical disinfection, the mass fraction of ethanol solution is 75%-an organic chemical raw material, which can be made into acetate fiber, synthetic fiber, perfume, fuel and so on. , is the main component of vinegar.
Main chemical properties of organic matter
Reaction of ethanol with sodium
2CH3CH2OH+2Na―→2CH3CH2ONa+H2↑
The reaction between ethanol and Na (compared with water): ① Similarity: both of them generate hydrogen, and the reaction is exothermic.
② Difference: It is slower than the reaction between sodium and water.
Conclusion: Hydrogen atoms on hydroxyl groups in ethanol molecules are more active than those in alkanes, but not as active as those in water molecules.
(2) oxidation reaction (I) combustion
CH3CH2OH+3O2―→2CO2+3H2O
(ii) Under the catalysis of copper or silver, it can be oxidized by O2 to acetaldehyde (CH3CHO).
2ch 3 ch 2 oh+O2―→2ch 3 CHO+2H2O
③ Elimination of reaction
ch 3c H2 oh―→CH2 = CH2 ↑+ H2O
Oxidation Reaction of Acetaldehyde: Properties of Aldehyde Group (-CHO) —— Reaction with Silver Ammonia Solution and Newly Prepared Cu(OH)2
ch 3c ho+2Ag(NH3)2OH―→ch 3c oonh 4+H2O+2Ag↓+3nh 3↓
(silver ammonia solution)
ch 3c ho+2Cu(OH)2―→ch 3c ooh+Cu2O↓+2H2O
(brick red)
Examination of aldehyde group: Methods 1: Silver mirror was formed by water bath heating with silver ammonia solution.
Method 2: Add the newly prepared alkaline suspension of Cu(OH)2, and heat it until it boils, with brick red precipitate.
Acetic acid ① has the general character of acid: ch3cooh ≒ ch3coo-+h+
Make the purple litmus test solution turn red;
React with active metals, alkali and weak acid salts, such as CaCO3 and Na2CO3.
Comparison of acidity: CH3COOH > H2CO3.
2ch3cooh+CaCO3 = 2 (ch3coo) 2ca+CO2 =+H2O (forced weak)
② esterification reaction
CH3COOH+C2H5OH CH3COOC2H5+H2O
Dehydrogenation of acidic dehydrogenated alcohols
Three. Basic nutrients
Nutrients in food include sugar, oil, protein, vitamins, inorganic salts and water. People used to call sugar, oil and protein the basic nutrients in animal and plant foods.
Species elements represent molecules.
Carbohydrate monosaccharide C H O Glucose C6H 12O6 Glucose and fructose are isomers of each other.
Monosaccharide cannot be hydrolyzed.
fructose
Disaccharide C H O sucrose C 12 H 22 O 1 1 sucrose and maltose are isomers of each other.
Hydrolysis will occur.
maltose
Polysaccharide C H O starch (C6H 10O5) N starch and cellulose can't be called isomers because of their different N values and molecular formulas.
Hydrolysis will occur.
cellulose
Unsaturated higher fatty acid glycerides of oil, oil, C·H·O and vegetable oil contain C = C bonds, which can undergo addition reaction.
Hydrolysis will occur.
C-c bond of animal fat saturated higher fatty acid glyceride,
Hydrolysis will occur.
Protein C H2O
Neurotrophic proteins and other enzymes, muscle,
Polymers formed from amino acids such as hair can undergo hydrolysis reaction.
The main idea is to change the nature of learning.
glucose
Simple structure: CHOH CHOH CHOH CHOH CHOH Choh Choh Town
Or CH2OH(CHOH)4CHO (containing hydroxyl and aldehyde groups)
Aldehyde group: ① The newly prepared Cu(OH)2? Brick red sediment-determination of the condition of diabetic patients
② react with silver ammonia solution to produce silver mirror-industrial mirror and glass bottle liner.
Hydroxyl: Esterification with carboxylic acid to form ester.
Sucrose hydrolysis reaction: glucose and fructose are produced.
starch
Hydrolysis of cellulose starch and cellulose: producing glucose.
Starch characteristics: Starch turns blue when it meets iodine.
Oil hydrolysis reaction: higher fatty acids (or higher fatty acid salts) and glycerol are produced.
Protein Hydrolysis: The final product is amino acid.
Color reaction: protein will turn yellow when it encounters concentrated nitric acid (a part of identifying protein).
The burning protein smells of burnt feathers (identify protein)