(1) diamond, graphite: C (2) mercury, mercury: Hg (3) quicklime, calcium oxide: CaO (4) dry ice (solid carbon dioxide): CO2 (5) hydrochloric acid, hydrochloric acid: HCl (6) sulfurous acid: H2SO3 (7) hydrosulphuric acid: H2S (8) hydrated lime, slaked lime: Ca (OH)2 (9) Caustic soda, caustic soda, caustic soda: NaOH (10) Soda ash: Na2CO3 Sodium carbonate crystals, soda ash crystals: Na2CO3?10H2O (11) Sodium bicarbonate, acidic sodium carbonate: NaHCO3 (also known as baking soda) (12) Cholagogic alum, blue alum, copper sulfate crystals: CuSO4?5H2O (13) Copper green, malachite: Cu2(OH)2CO3 (decomposition of the generate three oxides of substances) (14) methanol: CH3OH toxic, blindness, death (15) alcohol, ethanol: C2H5OH (16) acetic acid, acetic acid (16.6 ° C glacial acetic acid) CH3COOH (CH3COO- acetate ions) with the generality of the acid (17) ammonia: NH3 (alkaline gas) (18) ammonia, ammonia monohydrate: NH3?H2O (for the common alkali, with the general nature of alkali, is a base that does not contain metal ions) (19) sodium nitrite: NaNO2 (industrial salt, toxic)
Two, the state of the color of the common substances
1, white solids: MgO, P2O5, CaO, NaOH, Ca (OH) 2, KClO3, KCl, Na2CO3, NaCl, anhydrous CuSO4; iron, magnesium is silver-white (mercury is silver-white liquid)
2, black solids: graphite, charcoal powder, iron powder, CuO, MnO2, Fe3O4 ▲ KMnO4 is violet-black
3, red solids: Cu, Fe2O3 , HgO, red phosphorus ▲ Sulfur: yellowish ▲ Cu2(OH)2CO3 green
4, solution The color of the solution: Where the solution containing Cu2+ is blue; Where the solution containing Fe2+ is light green; Where the solution containing Fe3+ is brownish yellow, the rest of the solution is generally not colorless. (Potassium permanganate solution is purplish red)
5, precipitation (i.e., insoluble in water salts and bases): ① salt: white ↓: CaCO3, BaCO3 (dissolved in acid) AgCl, BaSO4 (also insoluble in dilute HNO3), etc. ② alkali: blue ↓: Cu (OH) 2 reddish brown ↓: Fe (OH) 3 white ↓: the rest of the alkali.
6, (1) with irritating gases: NH3, SO2, HCl (all colorless)
(2) colorless and odorless gases: O2, H2, N2, CO2, CH4, CO (highly toxic)
▲Note: with irritating odors of liquids: hydrochloric acid, nitric acid, acetic acid. Alcohol is a liquid with a special gas.
7, toxic, gas: CO Liquid: CH3OH Solid: NaNO2 CuSO4 (can be used as a fungicide ,mixed with slaked lime to form a sky-blue sticky substance - Bordeaux liquid)
Three, the solubility of substances
1, the solubility of salt
substances containing potassium, sodium, nitrate, ammonium are soluble in water
Cl-containing compounds only AgCl is not soluble in water, the other are soluble in water;
SO42-containing compounds only BaSO4 is not soluble in water, the other are soluble in water.
Only K2CO3, Na2CO3, (NH4)2CO3 are soluble in water, others are insoluble in water
2, the solubility of alkali
The bases that are soluble in water are: barium hydroxide, potassium hydroxide, calcium hydroxide, sodium hydroxide and ammonia, and other bases are not soluble in water. Refractory bases in Fe (OH) 3 is a reddish-brown precipitate, Cu (OH) 2 is a blue precipitate, other refractory bases are white. (Including Fe(OH)2) Note: AgCl and BaSO4 are insoluble in dilute nitric acid in the precipitates,
other precipitates are soluble in acid. Such as: Mg (OH) 2 CaCO3 BaCO3 Ag2 CO3, etc.
3, most of the acid and acidic oxides can be dissolved in water, (acidic oxides + water → acid) most of the alkaline oxides are insoluble in water, can be soluble in: barium oxide, potassium oxide, calcium oxide, sodium oxide (alkaline oxides + water → alkali)
Four, the most of the chemical
1, the Earth's crust. The most abundant metallic element is aluminum. 2、The most abundant non-metallic element in the earth's crust is oxygen.
3. The most abundant substance in the air is nitrogen. 4、The hardest naturally occurring substance is diamond.
5. The simplest organic substance is methane. 6、The most active metal in the order of activity table of metals is potassium.
7. The oxide with the smallest relative molecular mass is water. The simplest organic compound, CH4
8. The gas with the lowest density under the same conditions is hydrogen.
9. The most conductive metal is silver.
10. The atom with the smallest relative atomic mass is hydrogen.11. The metal with the lowest melting point is mercury.
12. The most abundant element in the human body is oxygen. 13. The element that makes up the largest variety of compounds is carbon.
14, daily life in the most widely used metal is iron. 15, the earliest use of natural gas is China; China's largest coal base in: Shanxi Province; the earliest use of wet copper refining is China (the Western Han Dynasty, found [Liu An "Huainan Wanbi technology" "Zeng Qing get iron is transformed into copper"], the Song Dynasty application); the earliest discovery of the electron is the British Thomson; the earliest use of the electron is the British Thomson; the earliest use of the electron is the British Thomson; the earliest use of the electron is the British Thomson. The first to discover the electron was Thomson of England; the first to conclude that air is composed of N2 and O2 was Lavoisier of France.
Fifth, junior high school chemistry in the "three"
1, the composition of the three particles of matter are molecules, atoms, ions.
2, reduce copper oxide commonly used three reducing agents hydrogen, carbon monoxide, carbon.
3, hydrogen as a fuel has three major advantages: abundant resources, high heat, the product of combustion is water does not pollute the environment. 4, the composition of atoms generally have three kinds of particles: protons, neutrons, electrons. 5, there are only three ferrous metals: iron, manganese, chromium. 6, the composition of the elements of matter can be divided into three categories that is (1) the metal elements, (2) non-metallic elements, (3) the elements of the rare gases. 7, the iron There are three types of oxides whose chemical formulae are (1) FeO, (2) Fe2O3, and (3) Fe3O4.
8, There are three characteristics of solutions (1) homogeneity, (2) stability, and (3) mixtures.
9, chemical equations have three meanings: (1) that what substances to participate in the reaction, the result of what substances; (2) that the reactants, products of each substance asked the molecules or atoms of the number of particles than; (3) that the reactants, the products of the mass ratio between. Chemical equations have two principles: based on objective facts; follow the law of conservation of mass.10, pig iron is generally divided into three kinds: white iron, gray iron, ductile iron.
11, carbon steel can be divided into three kinds: high carbon steel, medium carbon steel, low carbon steel.
12, commonly used in ironmaking iron ore are three: (1) hematite (the main component of Fe2O3); (2) magnetite (Fe3O4); (3) rhodochrosite (FeCO3).
13, there are three kinds of steelmaking equipment: converter, electric furnace, flat furnace.
14, the three reaction conditions often associated with temperature are ignition, heating, and high temperature.
15, saturated solution into an unsaturated solution there are two ways: (1) warming, (2) add solvent; unsaturated solution into a saturated solution there are three ways: lowering the temperature, add solute, constant temperature evaporation of solvent. (Note: solubility with temperature and become smaller substances, such as: calcium hydroxide solution from a saturated solution into an unsaturated solution: lowering the temperature, add solvent; unsaturated solution into a saturated solution there are three ways: warming, add solute, thermostatic evaporation of solvent).
16, there are generally three ways to collect gases: drainage method, upward emptying method, downward emptying method.
17, the three main causes of water pollution: (1) industrial production of waste residue, waste gas, waste water; (2) the arbitrary discharge of domestic sewage; (3) agricultural production of pesticides and fertilizers applied with rainwater into the river.
18, there are three kinds of fire extinguishers usually used: foam fire extinguishers; dry powder fire extinguishers; liquid carbon dioxide fire extinguishers.
19, the solubility of solid substances with the temperature can be divided into three categories: (1) most of the solubility of solid substances with the increase in temperature and increase; (2) a small number of substances solubility by the temperature is very small; (3) a very small number of substances solubility with the increase in temperature and decrease. 20, CO2 can be extinguished for three reasons: can not be combusted, can not support the combustion, the density of larger than air. 21, monomers can be divided into three categories: metallic monomers; non-metallic monomers; rare gases monomers. 22, the world's three most important fossil fuels today are: coal, oil, natural gas.
23, the three black oxides that should be remembered are: copper oxide, manganese dioxide, and iron tetraoxide.
24, hydrogen and carbon monomers have three similar chemical properties: stability at room temperature, flammability, and reducibility.
25, three pale blue color appearing in the textbook: (1) liquid oxygen is pale blue (2) sulfur burns in air with a faint pale blue flame, (3) hydrogen burns in air with a pale blue flame.
26, with the copper element related to the three blue: (1) copper sulfate crystals; (2) copper hydroxide precipitate; (3) copper sulfate solution. 27, filtration operation in the "three against": (1) the lower end of the funnel is close to the inner wall of the beaker; (2) the end of the glass rod is lightly against the three layers of the filter paper; (3) the beaker edge is close to the glass cupped to be filtered. beaker rim rests against the glass cupped drain.
28, the three major gaseous pollutants: SO2, CO, NO2
29, the flame of the alcohol lamp is divided into three parts: the outer flame, the inner flame, the center of the flame, of which the outer flame has the highest temperature.
30, access to medicines have "three no" principle: (1) no hands in contact with medicines; (2) do not put your nose to the mouth of the container to smell the odor of gas; (3) do not taste the flavor of drugs. 31, the ancient three major chemical processes: papermaking, gunpowder, burning porcelain 32, industrial waste: wastewater, slag, exhaust
34, can be directly heated three instruments: test tubes, crucibles, evaporating dishes (in addition to combustion spoons)
35, the conservation of mass explains the atomic three invariant: the type does not change, the number of unchanged, the quality of the mass does not change
36, mixed with air may explode the three kinds of combustion. Mixed with air may explode three gases: H2, CO, CH4 (actually any flammable gas and dust). 37, the three products of coal distillation (chemical change): coke, coal tar, coke oven gas
38, concentrated sulfuric acid three characteristics: water absorption, dehydration, strong oxidation
39, the use of alcohol lamps three prohibitions: on the combustion, to the combustion of the lamp in the addition of alcohol, blowing out the mouth
40, the use of alcohol lamps: the three prohibitions: on the combustion, to the combustion of the lamp in the addition of alcohol, mouth blowing <
40, three steps in the preparation of solutions: calculation, weighing (measure), dissolution
41, biological cells in the most abundant of the first three elements: O, C, H
42, the atom in the three equations: the number of nuclear charge = the number of protons = the number of electrons outside the nucleus = the number of atomic number
43, the composition of three kinds of particles of matter: molecules, atoms, and away from
43, the three particles of matter: molecules, atoms, and away from
Chemical mnemonics
1, the basic types of reactions:
Chemical reaction: more than one decomposition reaction: a change more than one
Replacement reaction: a single for a single Complex decomposition reaction: reciprocal ions
2, common elements of the chemical valence (positive price):
One-valent potassium, sodium, hydrogen, and silver, two calcium, magnesium, barium, and zinc, the three-valent metal elements aluminum;
One-five-seven variable chlorine, two-four-five nitrogen, sulfur four-six, three-five with phosphorus, two-four carbon;
One-two copper, two-three iron, two-four-six-seven manganese special.
3, the laboratory steps to produce oxygen:
"Tea (check), Zhuang (loaded), fixed, point, collection, Li (away), interest (quench)"
"Check" check the device tightness "Fill" to contain the medicine and connect the device
"Fix" to fix the test tube on the iron stand "Point" to ignite the alcohol lamp to heat
"collect" to collect the gas "away" to move the catheter away from the water
"off" to extinguish the alcohol lamp and stop heating.
4, the experimental steps to reduce copper oxide with CO:
"one pass, two points, three extinguish, four stop, five processing"
"one pass" first hydrogen, "two points
"One pass" is to pass the hydrogen gas first, "two pass" is to light the alcohol lamp for heating;
"Three extinguish" is to extinguish the alcohol lamp after the experiment is finished, "four stop" is to wait until the room temperature before stopping to pass the hydrogen gas; "five handle" is to deal with the exhaust gas and prevent the hydrogen gas from being used. "Handle the tail gas to prevent CO pollution of the environment.
5, the experimental phenomenon of electrolysis of water:
"Oxygen positive and hydrogen negative, oxygen and hydrogen two": the positive electrode releases oxygen, the negative electrode releases hydrogen; the volume ratio of oxygen to hydrogen is 1:2.
6, the elements that make up the earth's crust: adoptive daughter (oxygen, silicon, aluminum)
7, the outermost layer of the atom Relationship with the formation of ions and valence:
"Loss of Yang positive, get anion negative, the value is unchanged": the outermost layer of the atom after the loss of electrons to form a cation, the element's valence is positive; the outermost layer of the atom after the gain of electrons to form an anion, the element's valence is negative; the number of electrons gained or lost = the number of charges = the value of the valence.
8, the basic operation of chemical experiments mnemonic:
Solid need a spoon or paper slot, a send two vertical three bullet bullet; block solid or tweezers good, a horizontal two put three slow vertical.
Liquid should be in a bottle with a thin mouth, hand labeled and then poured. The readings should be level with the cut surface, and the elevated view should be low and the elevated view should be low and the elevated view should be low.
The dropper should be pinched, suspended vertically without staining, not flat, not poured and not put in a mess, and do not forget to clean it after use.
Tray balance must be put flat, the traveling code spinning screw needle in the center; left put the object to the right to put the code, tweezers clamp big and then clamp small;
Test paper to measure the liquid first cut small, the best glass rod dipped in liquid measurement. The test paper is first moistened and stuck on the stick to the gas.
The wine lamp is heated with the outer flame, two-thirds of the limit. Sulfuric acid into the water stirring, slowly injected into the anti-boiling splash.
Experiment first check the airtightness, heat the cup and bottle through the net. Drainage of gas collection is complete, first withdraw the catheter and then move the lamp.
9, the order of metal activity:
Metal activity order from strong to weak: K Ca Na Mg Al Zn Fe Sn Pb (H) Cu Hg Ag Pt Au (recite in order) potassium calcium sodium magnesium aluminum zinc iron tin lead (hydrogen) copper mercury silver platinum
10, the "crisscross method forget.
12, experiments in the law:
① Where the solid heating gas are selected potassium permanganate O2 device (solid-solid heating type);
Where the solid and the liquid reaction and do not need to be heated to make gas are selected hydrogen peroxide O2 device (solid-liquid not heating type).
② Where the test tube solid heating, should be preheated, the mouth of the test tube should be slightly downward sloping.
③Where the gas produced is insoluble in water (does not react with water), it can be collected by the drainage method.
Where the gas is denser than air, can be collected by upward air displacement method.
Any gas that is less dense than air can be collected by the downward air displacement method.
④ Whenever a gas is made, the gas tightness of the device should be checked first, the conduit should be exposed to the rubber stopper for 1-2 ml, and the iron clamp should be clamped 1/3 of the way from the mouth of the tube.
⑤ Whenever a long-necked funnel is used for gas production experiments, the end of the long-necked funnel should be inserted under the liquid surface.
6 Whenever a flammable gas is ignited, its purity must first be tested.
⑦Whenever using toxic gases in experiments, always dispose of the exhaust gas at the end.
8 Where the use of reducing gases to reduce metal oxides, it must be "one pass, two points, three extinguished, four stops"
13, the laws of the reaction: substitution reaction:
(1) metal monomers + acid → salt + hydrogen
(2) metal monomers + salt (solution) → another metal + another salt
(2) salt (solution) → another metal + another salt
(2) salt (solution) → another metal + another metal + another salt
(2) salt (solution) → another metal + another metal + another salt A metal + another salt
(3) metal oxides + charcoal or hydrogen → metal + carbon dioxide or water
Complex decomposition reactions:
① basic oxides + acid → salt + H2O ② alkali + acid → salt + H2O
③ acid + salt → new salt + new acid ④ salt 1 + salt 2 → new salt 1 + new salt 2
⑤ salt + base → new salt + new base
5 salt + base → new salt + new base
5 salt + base → new salt + new base
5 salt + base → new salt + new salt + new base
5 salt + base → new salt + new salt + new salt + new salt + new salt + new salt + new salt + new salt + new salt + new salt + new salt + new base New base
14, metal + acid → salt + H2 ↑ in:
① equal mass of the metal reacts with a sufficient amount of acid, the release of hydrogen from the more at least the order: Al>Mg>Fe>Zn
② equal mass of the different acids reacts with a sufficient amount of the metal, the smaller the relative molecular mass of the acid, the more hydrogen is released.
3) The same acid of equal mass reacts with a sufficient amount of a different metal to give out the same amount of hydrogen.
④After the reaction metal + acid → salt + H2↑, the solution becomes heavier in mass and the metal becomes lighter.
In metal + salt solution → new metal + new salt:
①When the relative atomic mass of the metal > the relative atomic mass of the new metal, the mass of the solution becomes heavier and the metal becomes lighter after the reaction.
② When the relative atomic mass of the metal < the relative atomic mass of the new metal, the mass of the solution becomes lighter and the metal becomes heavier after the reaction.
15, catalyst: a change of two unchanged (change the rate of reaction of a substance, its own chemical properties and the quality of the unchanged substance is a catalyst)
Oxidizing agent and reducing agent: gain oxygen return, loss of oxygen oxygen (the substance that captures the elemental oxygen is a reducing agent, loss of the elemental oxygen is an oxidizing agent)
16, the connection of the gas-washing cylinders with the removal of impurities: long in and short out
16, with a gas-washing cylinder drainage gas collection connection: short in long out
with a gas-washing cylinder exhaust air collection gas connection: dense small is short in long out, dense large is long in short out
17, experiments in addition to impurities principle: first in addition to the other, and then in addition to the water vapor
experiment test principle: the first test of water, and then test the other
CaO Calcium hydroxide quicklime
Ca (OH)2 Calcium hydroxide Hydrated lime, slaked lime
NaOH Sodium hydroxide Soda ash, caustic soda, caustic soda
Na2CO3 Sodium carbonate Soda ash, soda
NaHCO3 Sodium bicarbonate Soda baking soda
Diamonds, graphite: C
Hydrochlorite, mercury: Hg
Lime, calcium oxide: CaO
Dry ice (solid carbon dioxide): CO2
Hydrochloric acid, hydrochloric acid: HCl(6) Sulfurous acid: H2SO3
Hydrogen sulfuric acid: H2S
Sliquid lime, slaked lime: Ca(OH)2
Caustic soda, caustic soda, caustic soda: NaOH
Soda ash: Na2CO3 Sodium carbonate crystal, soda ash Crystals: Na2CO3?10H2O
Sodium bicarbonate, acidic sodium carbonate: NaHCO3 (also called baking soda)
Chole alum, blue alum, copper sulfate crystals: CuSO4?5H2O
Copper green, malachite: Cu2(OH)2CO3 (decomposes to form a triple oxide of the substance)
Methanol: CH3OH Toxic, blindness, death
Alcohol, ethanol: C2H5OH
Ammonia: NH3 (alkaline gas)
Acetic acid, acetic acid (16.6 ℃ glacial acetic acid) CH3COOH (CH3COO- acetate ions) With the generality of the acid
Ammonia: NH3 (alkaline gas)
Ammonia, ammonia monohydrate: NH3?H2O (for the common alkali, with the generality of alkali, is a kind of alkali does not contain metal ions)
Sodium nitrite: NaNO2 (industrial salt, poisonous) Answer: fine rain§ fluttering | Level 5 | 2011-3-25 21:38
A. Common substances, scientific names, common names and chemical formulas
Common name Scientific name Chemical formula
Diamond, graphite C
Alcohol Ethanol C2H5OH
Lime, slaked lime Calcium hydroxide Calcium hydroxide Ca(OH)2
Lime Calcium oxide CaO
Acetic acid (melting point 16.6 ℃, the solid state is called glacial acetic acid) Acetic acid CH3COOH
Wood alcohol, wood alcohol Methanol CH3OH
Dry ice Solid CO2 CO2
Copper green, malachite Copper alkali carbonate Cu2(OH)2CO3
Choleum, blue alum Copper sulfate crystals CuSO4-5H2O
Hydrogen sulfuric acid H2S
Sulfurous acid H2SO3
Salt acid water (industrial name) Hydrochloric acid, hydrochloric acid HCl
Mercury Hg <
Soda ash, soda, soda pop Sodium carbonate Na2CO3
Soda ash crystals Sodium carbonate crystals Na2CO3-10H2O
Acidic sodium carbonate, baking soda Sodium bicarbonate NaHCO3
Caustic soda, caustic soda, caustic soda Sodium hydroxide NaOH
Poisonous salts, nitrate salts (industrial name) Sodium nitrite NaNO2
Ammonia Monohydrate Ammonia NH3-H2O Answer: yangjiang yaozhu | Level 1 | 2011-3-25 21:41
Soda ash, soda, natural alkali , mouth alkali: Na2CO3 Baking soda: NaHCO3 Limestone, marble: CaCO3 Lime: CaO Table salt: NaCl Slippery lime, slaked lime: Ca(OH)2 Caustic soda, caustic soda, Caustic soda: NaOH Dry ice: CO2 Bile alum, blue alum: CuSO4?5H2O Hydrogen peroxide: H2O2 Iron red, iron ore: Fe2O3 Copper green, malachite: Cu2 (OH)2CO3 Bordeaux: Ca (OH)2 and CuSO4 Natural gas, biogas, pit gas (the main ingredient): CH4 Hydrogas: CO and H2 Urea: CO(NH2) 2
Organic fraction:
C2H2 (acetylene) Alcohol, ethanol: C2H5OH
Acetic acid: glacial acetic acid, vinegar CH3COOH
Glucose: C6H12O6