Can the chemicals in the displacement reaction be other What are they? Except for oxide acids or sa

Na and water can be regarded as a displacement reaction...

Group IA IIA (hot water) reacts with water to produce hydroxides and hydrogen.

F2 reacts with water...

Al reacts with a base *****

Active metals are replaced with water to produce hydrogen.

The non-metallic element replaces the oxygen-free compound 2H2+SiCl4=Si+4HCl

Of course you can, the example is the same upstairs, -

1) Dry displacement The displacement reaction of a solid with a solid or a solid with a gas under heating or high temperature conditions.

2) Wet displacement The reaction of the substitution in an aqueous solution.

The replacement of metal with acid is the reaction between metal atoms and hydrogen ions in an acid solution. Such as:

zn+2hcl===zncl2+h2↑

2Al+3H2SO4(dilute)==Al2(SO4)3+3H2 The replacement of metal atoms with the cations of less active metals in the salt solution is the replacement of metal atoms with cations of less active metals in the salt solution. Such as:

Cu+Hg(NO3)2===Hg+Cu(NO3)2 wet mold is a faction displacement that follows the order of metal activity.

The displacement reaction must be a redox reaction, but the redox reaction is not necessarily a displacement reaction.

The reaction of one elemental substance and one compound to produce another elemental substance and another compound. It is one of the basic types of chemical reactions, and displacement refers to the substitution of elements that make up elemental elements for certain elements in a compound.

Displacement reaction, take you into the world of displacement reaction, chemistry!

Elemental metals. Sour.

Salt. Hydrogen. displacement reaction) zinc and dilute sulfuric acid zn

h2so4znso4

The H2 phenomenon has bubbles that produce metal dissolution.

Iron and dilute Fe sulfate

h2so4feso4

H2 phenomenon: There are bubbles that produce metal dissolution and the solution turns light green.

Magnesium and dilute sulfate mg

h2so4mgso4

The H2 phenomenon has bubbles that produce metal dissolution.

Aluminium and dilute sulfuric acid 2Al

3h2so4

al2(so4)3

The H2 phenomenon has bubbles that produce metal dissolution.

Zinc and dilute hydrochloric acid Zn2HCl

zncl2h2↑

Phenomenon: There are bubbles that produce metal dissolution.

Iron and dilute hydrochloric acid Fe2HCl

FeCl2H2 phenomenon has bubbles to produce metal dissolution.

Magnesium and dilute hydrochloride mg + 2HCl

mgcl2h2↑

Phenomenon: There are bubbles that produce metal dissolution.

Aluminum and dilute hydrochloric acid 2Al6HCl

2alcl3

The H2 phenomenon has bubbles that produce metal dissolution.

Elemental metals. Salt (solution).

New metals. New salt.

Iron and copper sulfate solution reaction: fecuso4

feso4cu

There is red substance production.

Zinc and copper sulphate solution reaction: Zn

cuso4=znso4

Cu has red substance production.

Copper and mercury nitrate solution reaction: Cu

hg(no3)2

cu(no3)2

HG has a red substance production.

Hydrogen or carbon reduces metal oxides at high temperatures.

3c+2fe2o3===3co2+4fe

c+2cuo===co2+2cu

2c+fe3o4===2co2+3fe

3h2+fe2o3===3h2o+2fe

h2+cuo===h2o+2cu

4h2+fe3o4===4h2o+3fe

Other. Magnesium bars are burned in carbon dioxide.

2mg+co2===2mgo+c

In high school, there is also the replacement of metals with metal oxides, the replacement of non-metals with non-metal oxides, and the replacement of non-metals with non-metal hydrides.

Elemental metals. Sour.

Salt. Hydrogen. displacement reaction) zinc and dilute sulfuric acid zn

h2so4znso4

H2 iron and dilute Fe sulfate

h2so4feso4

H2 magnesium and dilute sulfate mg

h2so4mgso4

H2 aluminium and dilute sulfuric 2al

3h2so4

al2(so4)3

H2 zinc and dilute hydrochloric acid Zn2HCl

zncl2h2↑

Iron and dilute hydrochloric acid Fe2HCl

fecl2h2↑

Magnesium and dilute hydrochloride mg + 2HCl

mgcl2h2↑

Aluminum and dilute hydrochloric acid 2Al6HCl

2alcl3

H2 Elemental Metal. Salt (solution).

New metals. New salt.

Iron and copper sulfate solution reaction: fecuso4

feso4cu

Zinc and copper sulphate solution reaction: Zn

cuso4=znso4

Cu copper and mercury nitrate solution reaction: Cu

hg(no3)2

Cu(NO3)2Hg acid.

Alkali. Salt. Water (neutralization reaction).

Hydrochloric acid and caustic soda react: HCLnaoh

naclh2o

Hydrochloric acid and calcium hydroxide reaction: 2HCl

ca(oh)2

cacl22h2o

Aluminum hydroxide drug ** Hyperacidity: 3HCl

al(oh)3

alcl33h2o

Sulfuric acid and caustic soda reaction: H2SO42NaOH

na2so4

2H2O acid. Salt.

Another acid. Another salt.

Marble reacts with dilute hydrochloric acid: CaCO32HCl

cacl2h2o

Sodium CO2 carbonate reacts with dilute hydrochloric acid:

na2co32hcl

2naclh2o

Sodium CO2 bicarbonate reacts with dilute hydrochloric acid: NaHCO3HCl==NaCl

h2oco2↑

Sulfuric acid and barium chloride solution reaction: H2SO4BAC2BASO4

Chemical properties of 2HCl base.

Alkali. Non-metallic oxides.

Salt. Water. Caustic soda deteriorates when exposed to air: 2NaOHCO2

na2co3

H2O caustic soda absorbs sulfur dioxide gas: 2NaOHSO2NA2SO3

H2O caustic soda absorbs sulfur trioxide gas: 2NaOH3Na2SO4

H2O slaked lime deteriorates in air: Ca(OH)2CO2CaCO3

H2O slaked lime absorbs sulfur dioxide: Ca(OH)2SO2CASO3H2O base.

Acids --- salts.

Water (neutralization reaction, see above for equation) base. Salt.

Another alkali. Another salt.

The reaction phenomenon is inferred from the product.

1) Metal (before H) +

Acid (hydrochloric acid or dilute sulfuric acid) - salt. Hydrogen.

displacement reaction) zinc and dilute sulfuric acid ZnH2SO4

ZNSO4H2 continuously produces bubbles and the zinc particles gradually dissolve, making it suitable for laboratory hydrogen production.

Iron and dilute sulfuric acid FeH2SO4

FeSO4H2 slowly emits gas, the metal gradually dissolves, and the solution turns light green.

Magnesium and dilute sulfate Magh2SO4

MgSO4H2 rapidly produces a large number of bubbles and the metal gradually dissolves.

Zinc and dilute hydrochloric acid Zn2HCl

ZnCl2H2 continuously produces bubbles, making it suitable for laboratory hydrogen production.

Iron and dilute hydrochloric acid Fe2HCl

FeCl2H2 slowly emits gas and the metal gradually dissolves.

Magnesium and dilute hydrochloride mg + 2HCl

MgCl2H2 rapidly produces a large number of bubbles and the metal gradually dissolves.

Aluminum and dilute hydrochloric acid 2Al6HCl

2alcl3

3H2 has a large number of bubbles and the metal gradually dissolves.

2) Metals. Salt (solution).

Another metal.

Another salt. displacement reaction).

Iron and copper sulfate solution reaction: fecuso4

feso4cu

The surface of the iron is covered with a red substance, and the solution changes from blue to light green.

9.Reaction of aluminum and copper sulfate solution: alcuso4

al2(so4)3

The surface of the Cu silvery-white metal is covered with a layer of red substance, and the solution changes from blue to colorless.

Copper and silver nitrate solution reaction: Cu+2AGno3

2ag+cu(no3)2

The red metal surface is covered with a layer.

Silvery-white metal, the solution changes from colorless to blue.

According to the book, it's the following: (with a little expansion).

The reaction of one element and one compound to produce another element and another compound is called displacement reaction. Such as:

Reaction Expression:

a+bc=ac+b

Categories of substances before and after the reaction:

1) Elemental (a and b): can be metallic or non-metallic (carbon or hydrogen); (2) Compounds (BC and AC): can be acids or salts (solutions) or oxides.

Reaction conditions: 1) room temperature; (2) Heating or high temperature.

General principles for judging whether a reaction can occur or not:

1) If a is a metal, whether the displacement between metals or between metals and hydrogen can occur is generally judged by the order of metal activity, and the knowledge that needs to be mastered is: a

from, it can be displaced with water at room temperature; b.

From, the metals in front are generally able to displace the metals in the back from their salt solution; c.

The metal that comes before the hydrogen can displace the hydrogen in the acid. (2) if A is a non-metal (C or H2), only the metal between can be displaced; Carbon can also displace hydrogen in water at high temperatures.

Displacement reaction, take you into the world of displacement reaction, chemistry!

Because the chemical properties of inorganic and organic substances are inconsistent. So the classification of reaction types is different.

But it can also be blended:

Image: 2C2H5OH + 2NA --2C2H5ONA + H2 This is the reaction of organic matter, which belongs to the "displacement reaction".The reaction of acetic acid with sodium is even more so.

Substitution reactions, addition reactions themselves are defined as "reactions between organic matter", even if they have this characteristic in inorganic chemistry, they cannot be called "substitution reactions" or "addition reactions".

As a reminder, if there is a compound that can reduce magnesium ions to magnesium element, then magnesium sulfate will definitely be reduced to sulfide.

Moreover, for magnesium and other active metal salts to reduce the metal element, the reaction must be carried out in the non-aqueous system, and these salts are usually solid, and the solid is not good to react, if you want to melt, you generally need a higher temperature, and there is also the problem of atmosphere protection, otherwise the prepared metal element will be oxidized by the air immediately.

If you want to simply prepare some less active metals, it is best to divide the situation, so that it is not easy to cause waste.

It is a reaction between a metal atom and a hydrogen ion in an acid solution. Such as:

zn+2hcl====zncl2+h2↑

2AL+3H2SO4 (dilute) ====AL2 (SO4)3+3H2

Replacement of metal with salt solution:

a+bc→b+ac

The displacement relationship is when an element that makes up a compound is replaced by an element that makes up an element.

First, there are the following 4 situations of displacement reaction, and displacement reaction is one of the basic types of inorganic chemical reactions, such as:

fe+cuso4=cu+feso4

zn+2hcl=h2↑+zncl2

The more reactive non-metals are replaced by the less reactive non-metals, according to the type of elemental matter in the reactants and products:

The more reactive metal replaces the less reactive metal or hydrogen.

1. According to the type of reaction environment, there are two types of displacement reactions.

1) Dry replacement.

Solid-to-solid or solid-to-gas displacement reactions under heating or high temperature conditions, e.g

cl2+2nabr=br2+2nacl

o2+2h2s=2s↓+2h2o

The displacement reaction that occurs in the solution or between gases is carried out at room temperature, and the displacement reaction between gases and solids or two solids generally needs to be carried out at high temperatures.

2) Wet replacement.

Displacement reactions that are carried out in aqueous solutions, but redox reactions are not necessarily displacement reactions.

The replacement of metal with acid is the displacement of metal atoms with cations of less active metals in salt solution. Such as:

cu+hg(no3)2====hg+cu(no3)2

Wet displacement adheres to the order of metal activity.

The displacement reaction must be a redox reaction, which refers to the reaction of one element and one compound to produce another element and another compound, which can be expressed as.

Chemical-compulsory di-halogen substitution reaction.

(1) Metal (pre-H) + acid (hydrochloric acid or dilute sulfuric acid) - salt + hydrogen (displacement reaction).

1.Zinc and dilute sulfuric acid Zn + H2SO4 == ZnSO4 + H2 continue to produce bubbles, zinc particles gradually dissolve, suitable for laboratory hydrogen production.

2.Iron and dilute sulfuric acid Fe + H2SO4 == FeSO4 + H2 slowly release gas, the metal gradually dissolves, and the solution turns light green.

3.Magnesium and dilute sulfuric acid mg + h2SO4 == mgSO4 + H2 quickly produce a large number of bubbles and the metal gradually dissolves.

4.Zinc and dilute hydrochloric acid Zn + 2HCl === ZNCL2 + H2 continuously produce bubbles, which is suitable for laboratory hydrogen production.

5.Iron and dilute hydrochloric acid Fe + 2HCl === FeCl2 + H2 slowly release gas, and the metal gradually dissolves.

6.Magnesium and dilute hydrochloric acid Mg+ 2HCl === MgCl2 + H2 quickly produce a large number of bubbles, and the metal gradually dissolves.

7.Aluminum and dilute hydrochloric acid 2AL + 6HCl == 2ALCL3 + 3H2 There are a large number of bubbles produced and the metal is gradually dissolved.

2) Metal + Salt (Solution) – Another Metal + Another Salt (Displacement Reaction).

8.Iron and copper sulfate solution reaction: Fe + CuSO4 === FeSo4 + Cu The surface of iron is covered with a layer of red substance, and the solution changes from blue to light green.

9.Reaction of aluminum and copper sulfate solution: Al+CuSO4 === Al2(SO4)3 + Cu The silvery-white metal surface is covered with a layer of red substance, and the solution changes from blue to colorless.

10.Reaction of copper and silver nitrate solution: Cu+2AGnO3 === 2AG+ Cu(NO3)2 The surface of the red metal is covered with a layer.

Silvery-white metal, the solution changes from colorless to blue.