"Ionization of Electrolytes and Ion Reactions" Elements and the World of Matter PPT Courseware (Lesson 2 Ion Reactions)

"Ionization of Electrolytes and Ion Reactions" Elements and the World of Matter PPT Courseware (Lesson 2 Ion Reactions)

Part One: Literacy Goals

1. Understand the essence of ion reactions through experiments and experimental facts; understand the conditions and applications of ion reactions with changing ideas, and gradually improve scientific inquiry and innovation capabilities. Increase your interest in learning chemistry and experience the fun of inquiry.

2. Understand ionic reactions and the conditions for their occurrence through experimental facts, and learn to write general ionic equations. Able to understand the steps of writing ionic equations through model cognition.

3. Through induction and summary, learn the detection methods of SO_4^2"-" and Cl- plasma.

Ionization ion reaction of electrolyte PPT, part 2 content: knowledge foundation

1. The solubility formula of salt

Potassium sodium ammonium nitrate is soluble in tetrasalt, potassium sodium ammonium barium is soluble in tetraalkali.

Lead and barium sulfate are difficult to dissolve, while calcium salt and silver salt are only slightly soluble.

The normal salt of carbonate is less soluble, but the magnesium salt is slightly soluble in water.

Most of the hydrochloride is soluble, while silver salt is insoluble and lead is slightly soluble.

2. The four common strong bases: NaOH, KOH, Ba(OH)2, Ca(OH)2. Three strong acids: H2SO4, HCl, HNO3.

3. Common weak acids: H2CO3, HClO, CH3COOH, etc. Common weak bases: NH3·H2O, etc.

PPT on the ionization reaction of electrolytes, part three: preview of new knowledge

1. Ion reaction

1. Explore the essence of electrolyte reaction in aqueous solution

2.Definition

A chemical reaction involving ions in a solution.

3. Substance

The concentration of one or more ions decreases.

4. Conditions for ion exchange type ion reaction to occur

It produces substances that are difficult to dissolve, substances that are difficult to ionize, and substances that are volatile.

2. Ionic equation

1. Express

Ionic reactions can be expressed by ionic equations. For example, the ionic equation for the reaction between NaOH solution and hydrochloric acid is H++OH- === H2O.

2. Meaning

It not only represents a chemical reaction, but also represents a type of chemical reaction. For example, SO_4^2"-" +Ba2+ BaSO4↓ can not only represent the reaction of two solutions of Na2SO4 and BaCl2, but also represent the reaction between soluble sulfate (or sulfuric acid) and soluble barium salt. reaction in solution.

[Micro Thought 1] Can the ionic equation H++OH- === H2O represent all neutralization reactions that occur between strong acids and strong bases?

Tip: No. H++OH- === H2O only represents the reaction between a strong acid and a strong base that does not react between the acid ion in the acid and the cation in the base, such as the reaction between NaOH and hydrochloric acid, Ba(OH)2 and The reaction between H2SO4 cannot be expressed by this ionic equation.

3. Application of ionic reactions

Ion reactions can be used to test the presence of certain ions.

Ionization reaction of electrolyte PPT, part 4: independent testing

1. Judge whether it is right or wrong (mark “√” if it is correct and “×” if it is wrong).

(1) Any reaction that generates gas is an ionic reaction. ()

(2) Chemical reactions involving ions in the solution are all ionic reactions. ()

(3) When an ionic reaction occurs, the ion concentration in the solution will definitely decrease. ()

(4) Adding BaCl2 solution to a certain solution produces a white precipitate, indicating that the solution must contain _____. ()

(5) When checking Cl- in the solution, you can first add hydrochloric acid and then add AgNO3 solution. ()

Answer: (1)× (2)√ (3)× (4)× (5)×

2. When hydrochloric acid is dropped into the following solutions, which one will not undergo ionic reaction ()

A.AgNO3 B.NaOH

C.Na2CO3 D.KNO3

Answer:D

Analysis: When hydrochloric acid and KNO3 solution are mixed, no precipitation, gas or difficult-to-ionize substances are generated.

3. After adding NaOH, the following ions in the solution will be greatly reduced ()

A.CO_3^2"-" B.K+

C.SO_4^2"-" D.H+

Answer:D

Analysis: OH- reacts with H+ to form water, which reduces the number of H+. D is correct.

Ionization ion reaction of electrolyte PPT, part 5 content: exploration

Writing ionic equations

Question exploration

1. Can all chemical reactions be written as ionic equations?

Hint: No. Reactions that are not carried out in solution and are not reactions between freely moving ions cannot be written as ionic equations, such as calcining calcium carbonate to produce calcium oxide, etc.

2. Most salt substances are strong electrolytes. When writing ionic equations, do salt substances have to be broken down into ionic forms?

Hint: No. Only soluble salts can be broken down into ionic form.

3.What are the main categories of weak electrolytes?

Tips: Weak acid, weak base and water, etc.

Knowledge induction

1. Steps for writing ionic equations

Write a chemical equation—break easily soluble and easily ionizable substances into ionic forms—delete unreacted ions—check whether they are balanced.

2. The key to writing ionic equations

The key to writing an ionic equation is whether the "splitting" of the substance is reasonable.

(1) Strong acids, strong bases and soluble salts are rewritten into ionic forms.

(2) Weak acids, weak bases, insoluble salts, gases, elements, oxides, etc. are all written in chemical formulas.

3. "Six Looks" to determine whether the ionic equation is correct or incorrect

(1) Check whether it conforms to the objective facts of the reaction, such as the reaction between iron and dilute sulfuric acid.

(2) Check whether it complies with the principle of splitting and writing, such as the reaction between calcium carbonate and hydrochloric acid.

(3) See whether it conforms to mass conservation, such as the reaction between sodium and water.

Ionization reaction of electrolytes PPT, Part 6: In-class testing

1. Among the following reactions, which one is an ionic reaction ()

A.H2 and O2 react to form water

B. Put the zinc flakes into dilute sulfuric acid

C. Charcoal reacts with CO2 at high temperature to generate CO

D.2KClO3 2KCl+3O2↑

Answer:B

Analysis: Ionic reaction is a chemical reaction in which ions participate in the solution, B is consistent.

2. Which of the following ionic equations is written correctly ()

A.Na put into water: Na+2H2O Na++OH-+2H2↑

B. Calcium carbonate is dissolved in acetic acid (CH3COOH, monobasic weak acid): CaCO3+2H+ Ca2++H2O+CO2↑

C. Add copper powder to the silver nitrate solution: 2Ag++Cu Cu2++2Ag

D. Reaction of Ba(OH)2 solution and dilute sulfuric acid: Ba2++OH-+H++SO_4^2"-" BaSO4↓+H2O

Answer:C

3. In a colorless and transparent acidic solution, the ion group that can coexist in large amounts is ()

A.Na+, K+, SO_4^2"-", OH-

B.Na+, K+, Cl-, NO_3^"-"

C.Fe3+, K+, Na+, NO_3^"-"

D.Ag+, K+, SO_4^2"-", Cl-

Answer:B

Analysis: In item A, OH- can react with H+ in the acidic solution to form water; in item B, the four ions do not react with H+ and can coexist in large amounts; in item C, Fe3+ is brown and does not meet the meaning of the question; in item D, Ag+ and Cl- can react to form AgCl precipitation and cannot coexist in large amounts.

4. The reaction of substances in the following groups in solution can be expressed by the same ionic equation ()

A.Sodium hydroxide and hydrochloric acid; sodium hydroxide and carbonic acid

B.BaCl2 solution and Na2SO4 solution; Ba(OH)2 solution and H2SO4 solution

C.Na2CO3 solution and hydrochloric acid; CaCO3 and hydrochloric acid

D. Copper oxide and nitric acid; Copper oxide and hydrochloric acid

Answer:D

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