What equipment does the paper mill in Xihu District, Nanchang City have?

Junior Middle School Chemistry Book Review Outline

Chemistry to Chemistry World Review Outline The first unit consists of scientific research on matter, structure, properties and their changing laws.

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Principles for accessing medicines

Safety principles: Do not touch medicines directly with your hands, do not taste medicines that cannot be smelled with nostrils close to the mouth of the container. Taste of any medicine

Storage principles: The dosage should be strictly in accordance with the laboratory's. If you do not specify the amount, generally admit the minimum amount, which requires 1-2 ml of liquid, as long as the solid covers the tube. bottom.

Principle: Leftover medicines cannot be put back into the original bottles and should not be thrown away. Those that cannot be taken out of the laboratory should be placed in designated containers.

If the experimental drug solution splashes into the eyes, wash them immediately with water.

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Lumpy or dense solid particles. Solid drugs are generally held with tweezers, "two at an angle, three slowly and vertically"

Powdered or granular drugs A key (or library) of "one horizontal delivery three upright"

Use tweezers or the key should be cleaned immediately with a clean paper towel

Liquid medicine (stored in a small jar). Obtain a small amount of liquid medicine---a glue-tip dropper (pinch two "suction empty drops")

The dropper should be suspended directly above the instrument vertically, so that the liquid droplets can flow. Do not let the dropper touch the wall of the instrument that absorbs the liquid. Make the dropper flat on a bench or other place to avoid contaminating the dropper. Do not use an uncleaned dropper before sucking other reagents (do not cross-use drip bottle droppers , no need to rinse)

For test solutions from narrow-mouth bottles, cork wins, place on the table to pour the liquid, with the label toward the palm of your hand, close to the mouth of the vial or instrument, to prevent corrosion of the label left The liquid in the bottle ran down.

To access a certain amount of liquid medicine, use a graduated cylinder.

The reading of the measuring cylinder must be maintained steadily between the line of sight of the liquid meniscus and the lowest level in the measuring cylinder. Overlooking the high reading, look for the bottom of the reading section.

B. Liquid volume operation: First dump the liquid measuring cylinder off the required scale and drip to the amount marked with a dropper row.

Note: The graduated cylinder is a pressure gauge and can only be used to measure liquids and cannot be used as a reaction vessel for long-term storage without drugs. Do not use hot or cold liquids in quantities and should not be heated.

C. Reading a book, when you look up, the reading is lower than the actual volume. If you look down, the reading is higher than the actual volume.

Use an alcohol lamp

1. Alcohol lamp flame: three different outer flames, inner flames and flame cores. The outer flame has the highest temperature and the inner flame temperature is the lowest, so the hot material on the outer flame should be heated.

Notes on the alcohol lamp:

A. The alcohol in the alcohol lamp does not exceed 2/3 of the volume;

B. After the alcohol lamp is used up, the lamp cap must be capped instead of blowing it out with your mouth;

C It is absolutely prohibited to add alcohol to a burning alcohol lamp;

e It is absolutely forbidden to use a burning alcohol lamp to light another alcohol lamp lights to avoid causing fire.

E. Alcohol-free lamps are covered with caps to prevent alcohol from evaporating.

Tools that can be heated directly include: tubes, evaporating dishes, burning spoons, crucibles, tools that can be heated, but must be padded with asbestos mesh beakers, flask instruments: unheated cylinders, glass rods, gas bottles.

To heat the medicine, put the dry instrument before preheating, and then fix the medicine at the bottom for heating; to heat the solid medicine, the medicine is laid, and the tube mouth should be slightly tilted downward to prevent water from flowing back into the tube from breaking. test tube; when heating liquid medicine, the liquid volume cannot exceed 1/3 of the volume of the test tube. It is necessary to tilt the test tube upward at an angle of 45°, and do not put the test tube mouth facing yourself or others

Wash tools :

Use a tube scrubber, a rotating or ascending and descending tube brush to scrub, but not too fast to prevent tube damage.

Clean sign: The water attached to the inner wall of the glassware neither gathers into water droplets nor falls.

Activities to explore

Characteristics of green chemistrylt;

An investigation of candle burning to explore the gases/agt in inhaled and exhaled air;

Unit 2: Basic Concepts of the Contour of the Air Around Us

Physical Change: No change creates new matter. Such as melting paraffin, evaporating water

Chemical change: a change that produces new substances. Antirust of steel, such as the essential characteristics of burning substances

Chemical changes: to produce new materials. Must be accompanied by physical changes, chemical changes Physical changes are not accompanied by chemical changes.

Physical properties: Nature does not require chemical changes. Such as color, state, odor, density, solubility, volatility, hardness, melting point, boiling point, electrical conductivity, thermal conductivity, ductility.

Chemical properties: Properties of substances that manifest chemical changes (flammability, combustion, oxidation, reduction, stability). Like rust, oxygen supports combustion.

Pure substance: A substance. Such as N2 O2 CO2 P2O5.

Mixture: A mixture of two or more substances. Air, sucrose and water (each component maintains its original properties inside)

Elements composed of the same elements: pure substances. N2 O2 S P.

Compounds: pure substances composed of various elements. CO2 potassium chlorate SO2.

Oxide: A pure substance that is a compound of two elements, one of which is the element oxygen. Such as CO2 SO2.

Combining reaction: A reaction in which two or more substances produce another substance. A B AB

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Decomposition reaction: A reactant produced in the reaction of two or more other substances. AB A B

Oxidation reaction: the reaction between a substance and oxygen. (Slow oxidation is also an oxidation reaction)

Catalyst: A substance that can change the rate, quality, and chemical properties of other substances in chemical reactions that do not change before and after the reaction. (Also called a catalyst) It should be said that the substance is a catalyst. If they cannot speak, say that the manganese dioxide catalyst is a manganese dioxide catalyst for the potassium chlorate decomposition reaction]

Catalytic reaction under the action of the catalyst.

Secondly, the properties of oxygen

The physical properties of oxygen: a colorless, odorless gas with a density slightly greater than that of air and easily soluble in water. Under certain conditions, it can liquefy into a light blue liquid and solidify into a light blue solid.

Chemical properties of oxygen: chemically active, oxidizing, and a common oxidizing agent.

Support Burning: Wood Revival of Wooden Strip Test Paper with Sparks.

Reactions of oxygen substances: (sulfur, carbon, iron wire, phosphorus)

Reaction conditions with oxygen

Phenomena of reactions with oxygen

Name of products and chemicals

Expression of chemical reactions

Third air

Determination of the oxygen content of the composition that is - excessive red phosphorus combustion Experiment

Composition of air: N2: Oxygen content 78%: 21% inert gas 0.94% CO2: 0.03% other gases and impurities 0.03%

Oxygen uses: An inert gas that supplies breathing and supports combustion

nitrogen utilization

nature and purpose

Air pollution (air quality daily forecast)

The main sources of pollution are fossil fuels (combustion of coal and oil, etc.) and exhaust emissions from factories and automobile exhaust emissions.

(2) Pollutant gases and dust. Such as: sulfur dioxide, CO, nitrogen oxide, etc.

Oxygen produced in the laboratory

Drugs include: hydrogen peroxide and manganese dioxide or potassium permanganate or potassium chlorate and manganese dioxide

/gt; Reaction principle:

(1) Hydrogen peroxide oxygen water

(2) Potassium permanganate, permanganate manganese dioxide oxygen

(3 )Potassium chlorate, potassium chloride, oxygen

3. Experimental device

Collection method:

Densier than air - upward air exhaust method (the conduit opening enters the cylinder and is The bottom of the body, easy to set up the cylinder to catch up with the best)

Insoluble in water or easily soluble in water and does not react with water - Drainage method (the air in the container or conduit cannot be collected immediately after the bubbles start to escape the bubbles continuously and evenly) The collection begins only when the edges of the bubbles glow from the cylinder mouth of the group, indicating that the gas has been collected). The collected gas is pure.

Steps:

(1) Check the air tightness of the device.

(2): Put the drug into the test tube, and insert the single-hole rubber stopper and catheter into the test tube.

(3): Tube stage

(4) A kerosene lamp is fixed on the metal frame and lit. The first test tube is evenly arranged and heated by the external heating part.

(5): Collect oxygen by drainage method

(6): After collection, the first conduit is evacuated from the water tank. Extinguish the alcohol lamp.

6. Test method: The wood in the Mars gas bottle is recovered, and the gas in the bottle is oxygen.

7. Full experience:

(1) Exhaust the air upward to collect the wooden bottle with Mars, the wood will revive, and the oxygen on the bottle will be sufficient.

(2) Collection drainage method: When bubbles emerge from the edge of the cylinder mouth group, it indicates that the oxygen cylinder is full.

8. Precautions:

(1) The test tube mouth is slightly tilted downward (solid drug heating) to prevent the heat of the drug in the water from converting into steam and then condensing the page back into the tube to the bottom, leaving the test tube broken into water droplets.

(2) The catheter cannot be inserted into the test tube if it is too long. Exposing the rubber plug only a little bit can promote the discharge of gas.

(3) The tube at the bottom of the in vitro drug tile is heated evenly.

(4) Place the iron clip onto the upper half of the test tube (about 1/3 from the test tube mouth).

(5) Move the lower part of the alcohol lamp back and forth to heat the first test tube evenly and then align the drug parts with the outer flame of the alcohol lamp to heat and align the drug parts; heat the test tube.

(6) Drainage and gas collection method: Fill the collection bottle with water and pour it into the sink (under the bottle of water). If the conduit extends to the bottle, you can use the exhaust air collection cylinder to bring the conduit opening close to the bottom of the gas collection bottle.

(7) In the method of water drainage and gas collection, it should be noted that when the bubbles are continuously and evenly released from the conduit port during collection, use air or gas collection and mixing. The foam at the mouth of the gas collection bottle is proven to be intact.

(8) To stop the reaction, first withdraw the catheter and shift the alcohol lamp (to prevent water from flowing back into the test tube in the sink and causing the embassy to rupture) BR /gt;

(9) Set to collect the complete oxygen bottle by the bottle mouth and cover it with a glass plate.

(10) Use the oxygen nozzle of the potassium permanganate system and a small group of cotton fortresses.

5 Oxygen Industrial Production Methods - Separated Liquid Air Method

At low pressure, air is fed into liquid air and then evaporates. Since the boiling point of liquid nitrogen is lower than the boiling point of liquid oxygen, the nitrogen evaporates first from the liquid air, leaving mostly liquid nitrogen.

Water Review Outline Properties of Water in Composition

Electrolysis of Water Unit 3: Experiment: Electrolysis of water is a chemical reaction caused by the action of direct current. Water molecules form hydrogen atoms and oxygen atoms, and the two atoms, respectively, form two components into hydrogen molecules and oxygen molecules, specifically hydrogen molecules, and oxygen molecules aggregate into hydrogen and oxygen.

Cathode oxygen, negative hydrogen

The volume ratio of positive and negative gases is 1:2.

Negative gas burning wood cathode gas can be revived with Mars.

Water Oxygen Hydrogen (decomposition reaction)

2H2O O2 2 H2

Composition of water: Water is a pure substance and a chemical compound.

From a macroscopic analysis, water is a composition composed of hydrogen, oxygen, and water compounds.

Microscopic analysis shows that water is composed of water molecules, which are formed of hydrogen atoms and oxygen atoms. Properties of water

Physical properties: Colorless, odorless, tasteless liquid with a boiling point of 100°C, a freezing point of 0°C, and a density of 1g/cm3. It can dissolve substances that form solutions.

Chemical properties: decomposed into hydrogen and oxygen, water can also react with water of many elements (metals, non-metals), oxides (metal oxides, non-metal oxides), under the condition of electricity, salt reactions with other substances.

Hydrogen

Physical properties: Colorless, odorless gas, insoluble in water, less dense than air, and has the smallest gas density under the same conditions. 2. Chemical properties - flammability.

Burning air (or oxygen) is released with a large amount of heat, a light blue flame, and the only product is water.

Note: In the case of fire, a mixture of hydrogen and air (or oxygen) may explode, so be sure to check whether the hydrogen is pure before igniting it. (Experience the pure method: collect the hydrogen in the test tube, cover the mouth of the bottle with your thumb, move the alcohol lamp flame downward, release your thumb to ignite, there will be a sharp explosion, the hydrogen is impure, need to collect and retest; say enough loudly Compared to pure hydrogen)

Molecule

Definition: The smallest particle of molecular materials and chemical properties.

Characteristics of molecules:

Molecules are very small, with very small weight and volume

The molecules are constantly moving, and the higher the temperature, the higher the energy. The molecules move faster.

(3) Intermolecular forces and intervals. After mixing the liquid volumes of several different liquids, the total volumes are usually not equal by simple addition because of intermolecular forces and spacing. (Expansion and contraction)

Atom

Definition: The smallest particle in the chemical change of an atom

The essence of chemical change: the differentiation of molecules and the recombination of atoms.

Comparison of molecules and atoms:

Atoms and molecules

Similar points: The form of particles of matter is independent microscopic particles. Differences:

molecules can be divided into chemical changes and atoms in chemical changes cannot be subdivided.

Contact: Molecules can be split into atoms, and atoms form molecules.

Classification and composition of matter

Substance particles composed of material elements: molecules, atoms, ions

/ agt;

Classification of matter A mixture of pure substances (elements, compounds)

Water

Water purification and purification, adding flocculants to absorb impurities, adsorption and precipitation

Disinfection (adding chlorine and carbon monoxide Dichlorine)

Activated carbon water purifier filter

: It has a porous structure, gas, vapor or colloidal solid, and has strong adsorption capacity. The adsorbed pigment leaves the liquid and becomes colorless, deodorizing.

Classification of substances Filters separate mixtures of soluble and insoluble substances (note: "low", "depending")

Distillation: separate mixtures of substances with different boiling points

Taking care of water resources

Water resources owned by humans

China’s water resources and water resource pollution: Sources of water pollution: industrial pollution, agricultural pollution, domestic pollution.

3. Take good care of water resources

- The water-saving mark saves water and improves water utilization. On the one hand, it saves water and prevents waste of water. On the other hand, it uses new technologies. Reform processes and change their habits to reduce large amounts of industrial, agricultural and domestic water use and improve water utilization.

Prevention and control of water pollution:

Reduce the production of pollutants

B Treat contaminated water to comply with discharge standards that promote the use of agricultural fertilizers, and Use chemical fertilizers and pesticides rationally

D. Centralized sewage treatment can be used before discharge.

Units, chemical equation review outline

Definition: chemical changes in formulas, chemical equations

1, 2 H 2 022 H 2 O hydrogen in air Burning into H 2 O water

↑The reactants on the left are the products of the above reaction conditions.

gt; identify the chemical changes produced and see if there are New materials

Inside laboratory chemical reactions

Preparation of oxygen from potassium chlorate: 2KCl032KCl 3 O2↑lt; br/Hydrogen peroxide to produce oxygen 2H202 2H20 02↑

Chemical equation writing

(1) Write the reactants and products

2. Every tweak around the equal sign means that the atoms on the left side have equal rights

List generation formula for water hydrogen combustion in air H20H2↑ O2↑It is clear that it does not end if the number of all atoms in the reactants leaves only one O in it, but there are two on the right

The water decorated in the front plus 2 plus 2 becomes the backward generated H2 front 2H202H2 O2

Please note that there is no gas in the back, if you want to add ↑ it should be the final equation 2H202H2↑ O2↑

Four types of reactions, the most basic type

The compound decomposition substitution metathesis

① Two compounds of materials two or more substances To produce one substance, such as Ca(OH)2 for CaO H 2 O

(2) The decomposed substance reacts to produce two or more substances, for example: 2KmnO4K2Mn04 MN02 02↑

③Replace a simple element with other substances to replace iron H2SO4 ferrous sulfate H2↑

Calculate BR /gt;

①Things established, You asked about p>

The equation listed in ⑤, the result

⑥A

/gt; example topic How many grams of water is produced when 4G of hydrogen burns in air?

Solution: Let us generate >2mol Xmol/agt;

X = 2mol

M = 2mol Burns to produce 36 grams of water.

Unit 5, Chemical Properties of Carbon and Review Outline of Carbon Oxides

Carbon

Physical Properties

Graphite, diamond, Physical Properties of Carbon 60

Uses of each substance.

Chemical Properties

Stable

Flammable

Carbon burns entirely in oxygen: C O2 CO2

BR /gt; reduce charcoal Reduced copper oxide: C 2CuO 2CU CO2↑

Coke reduced iron oxide: 3C 2Fe2O3 4FE 3CO2↑

The coal stove performs three reactions: (some combination reactions)

Bottom of the coal stove: C O2, CO2

In the coal stove: CO2 C 2CO

Generation of blue flame on the coal stove: 2CO O2 2CO2

Laws and properties of the carbon dioxide system:

Legal system of principles: reaction of marble with dilute hydrochloric acid (laboratory homemade carbon dioxide): calcium carbonate 2HCl calcium chloride H2O CO2↑

Properties

Physical properties: Colorless, odorless gas with a density greater than that of air, easily soluble in water

Chemical properties

Carbon dioxide is easily soluble in water : H2O CO2 H2CO3

High temperature calcined limestone (industrial production of carbon dioxide): CaCO3 calcium CO2↑

Reaction of lime water with carbon dioxide (identified carbon dioxide) Ca(OH)2 CaCO3↓H2O of CO2

lt;/Uses: photosynthesis, natural gas, chemical fertilizers, chemical raw materials

Carbon monoxide properties:

Carbon monoxide reduction copper oxide: CO CO2 Copper of CuO

BR /gt; flammability of carbon monoxide: 2CO O2 2CO2

Uses: fuel, metal smelting

Other reactions: sodium carbonate and dilute hydrochloric acid Reaction (Fire Extinguisher Principle) Sodium Carbonate 2HCl 2NaCl H2O CO2↑

Unit 6,

Combustion and Fire Extinguishing Substances Fuel Combustion Utilization Review Outline Conditions

, Combustible

Oxygen

Principles and methods of fire extinguishing when reaching the ignition point

BR /gt; Energy changes in fossil fuels and chemical reactions

p>

Fuel on the environment

Methane burns in the air: CH4 2O2 CO2 2H2O

Impact

Alcohol burns in the air: C2H5OH 3O2 2CO2 3H2O

Hydrogen Combustion in Air: 2H2 O2 2H2O

Unit 7, Review Outline of Dissolution of Substances

Solution Features: Uniform, stable mixture.

Basic properties of solutions: (1) A solution in which a small amount of solid matter is dissolved in water (the proportion of water) increases the boiling point and lowers the freezing point;

So you can sprinkle Salt melts snow

②Acid, alkali, and salt are dissolved in water, and the conductivity of the solution (because of ionization to generate ions). Sucrose and alcohol are non-conductive when dissolved in aqueous solution;

③ Sodium hydroxide solid, concentrated sulfuric acid dissolved in aqueous solution increases the temperature (the temperature of the reaction solution of CaO and water rises), dissolved in aqueous solution

The temperature of NH4 NO3 solid decreases.

Emulsification: Initially, two immiscible substances form an emulsion under the action of some substances. In detergents, cooking oils are emulsified in water, so you can use the oil to wash clothes.

①②With water temperature

Cool solute ②③Evaporated solvent

①Three saturated solutions with abnormal increase in temperature Unsaturated solution Unsaturated solution Unsaturated solution The hydrated lime solvent evaporation method is used to increase the mass fraction of the solute and continuously cool the mass fraction of the solute.

The method of

saturated lime water and unsaturated lime water is:

① add water ② cool the solution with solute, at the same temperature, a certain proportion of the unsaturated solution is saturated The solution is concentrated.

20℃, the solubility of soluble substances gt; 10g, the solubility of water-soluble substances, the solubility of insoluble substances 0.01g 1g, the solubility of insoluble substances lt; 0.01g 1g-10g, .

3. The solubility of solid substances and changes in temperature can be divided into three categories: (1) The solubility of most solid substances (2) The solubility of a few substances increases with temperature, such as nitric acid Potassium; NaCl, which is not affected much by temperature; (3) The solubility of very few substances decreases with the increase of temperature and Ca(OH)2.

4. Separation and filtration of KCl and manganese dioxide, and the following steps: dissolution, filtration, and evaporation.

Separation of NaCl and potassium nitrate is crystallized, and the steps are: dissolution, Cooling and crystallization. (Cooling thermal saturated solution method)

Small temperature changes in the solubility of substances in the solvent used are evaporated to obtain crystals (such as NaCl).

Comparatively large change in temperature, the solubility in the hot saturated solution is cooled, and crystals (such as KNO3 and CuSO4) are obtained.

The substance that cools the saturated copper sulfate solution precipitates into crystals with the chemical formula CuSO4·5H2O of.

5. The solute is iodine, iodine, and alcohol solvent. Hydrochloric acid, the solute is HCl gas, a solute of lime is Ca(OH)2, the solute of brine is NaCl, the solute of calcium oxide is dissolved in water is Ca(OH)2, sulfur trioxide is dissolved in the solute of water is H2SO4, The solute copper sulfate of hydrocholine CuSO4·5H2O dissolved in water, and the solute C2H5OH of medical alcohol. Brine is a 0.9% sodium chloride solution.

6. Mass fraction of solute = mass of solute ÷ mass of solution × 100% = mass of solute ÷ (mass of solute solvent) × 100%

Water diluted by solution or evaporation of water Concentrated solute remains unchanged: Minutes ago Half the mass of the solution; the mass fraction of the solute is halved, and adding water equals the mass of the original solution.

7. Notes: (1) Solute, the mass of the solution when the solute is added to the solution; ② The complete solubility of the added solid (solubility size); ③ The reaction of water (such as CaO copper sulfate, The relationship between the water consumed by the reaction), the solubility (S) in the saturated solution and the mass fraction (C%) (independent of the mass fraction and solubility of the solute in the unsaturated solution) Solute

①Sgt; C②C% = S÷ (100 S) × 100%

9, A g, 100 g of water The formation of the substance dissolved in this solution and its solute Mass fraction: equal to and may be greater than A% A%, or may be smaller than A%.

Unit 8 The miraculous outline of matter composition

Atomic composition

1. There are three particles that make up atoms: protons, neutrons and electrons. However, not all atoms are made of the three types of particles. If there is a hydrogen atom, there are only protons and electrons, and neutrons.

In an atom, the number of positive charges (nuclear charge) brought is the nuclear charge of protons (neutrons have no charge). Each proton carries one unit of positive charge. Such nuclear charge = Number of nuclear protons in ER Nuclear charge number of electrons outside the nucleus = Number of protons = Number of electrons outside the nucleus is equal to.

There are charged particles in atoms, so the entire atom has no significant electricity?

Atoms are composed of protons and neutrons living in a positively charged nucleus and negatively charged electrons. In turn, positively charged protons and uncharged neutrons carry a positive charge outside the nucleus. The electrons outside the nucleus (the nuclear charge at the center of the atom) are electrically negatively charged equal but in opposite directions, so the entire atom is not significantly dynamic.

Relative atomic mass: - The ratio of 1/12 of the atomic mass of a standard carbon atom to the mass of other atoms, and the resulting statement is the relative atomic mass of this atom.

Relative atomic mass of element atoms = actual mass/atom of element (actual mass of carbon atom × 1/12)

Please note:

agt;

Relative atomic mass is just a ratio, not the actual atomic mass. Its unit is omitted.

In the calculation of relative atomic mass, the choice of a carbon atom is carbon atom 12, which contains 6 protons and 6 neutrons. 1/12 of its mass is approximately equal to 1.66×10 -27 kg.

Element:

Definition: A general term for a class of atoms with the same number of protons (nuclei) having the same nuclear charge.

The order of content of each element in the earth's crust: O, silicon, aluminum and iron

The most abundant non-metallic elements, differences and connections between molecules and atoms

/gt; Elements And

Atomic concept is a collective group of atoms with the same nuclear charge. Chemical changes in the smallest particles.

Talking about the difference between types does not allow for the meaning of counting. That is, the meaning of quantity that emphasizes the number of species spoken.

A description of the substance to which the macro composition is applied. this.