"Ionization of Electrolytes" Ion Reaction PPT Courseware

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"Ionization of Electrolytes" Ion Reaction PPT Courseware

Part One: Literacy Goals

1. Through experiments, understand the concept of ionization with changing thoughts, thereby mastering the connotation and extension of the electrolyte concept, and gradually improving scientific inquiry and innovation capabilities.

2. By understanding the concepts of electrolytes and ionization, we can re-understand the concepts of acids, alkalis, and salts from a combination of macro and micro perspectives.

3. Through induction and summary, learn to use ionization equations to express the ionization of certain acids, bases, and salts, and cultivate evidence reasoning and model cognitive awareness.

PPT on the ionization of electrolytes, part 2: independent preview before class

Knowledge foundation

1. Conductivity experiments prove that aqueous solutions of NaCl, NaOH, and H2SO4 can conduct electricity, while aqueous solutions of sucrose and alcohol do not.

2. Common acids include HCl, H2SO4, HNO3 (write chemical formula), and common bases include NaOH, KOH, Ba(OH)2 and Ca(OH)2.

3.NaCl, Na2SO4, etc. are normal salts, while NaHSO4 is an acid salt.

Preview of new knowledge

1. Electrolyte

1.Definition

A compound that conducts electricity in an aqueous solution or in a molten state. Such as HCl, H2SO4, NaOH, Ca(OH)2, NaCl, KNO3, etc.

Warm reminder: Compounds that cannot conduct electricity in aqueous solution or in the molten state are called non-electrolytes. Such as sucrose, alcohol, etc.

2. The reason why electrolyte solution or molten electrolyte conducts electricity (taking NaCl as an example)

(1) The conditions necessary for electrolyte to conduct electricity: there are freely moving ions.

(2) NaCl is an electrolyte, and the solid contains charged particles Na+ and Cl-, but these ions cannot move freely, so the sodium chloride solid does not conduct electricity.

(3) When NaCl solid is dissolved in water, Na+ and Cl- enter the water under the action of water molecules, forming charged particles that can move freely, so the NaCl solution can conduct electricity.

(4) When sodium chloride solid melts when heated, the movement of ions accelerates as the temperature increases, overcoming the interaction between ions and producing Na+ and Cl- that can move freely, so molten NaCl can also conduct electricity.

[Micro Thought 1] (1) NaCl solution can conduct electricity. Is NaCl solution an electrolyte?

(2) Pure H2SO4 does not conduct electricity in the molten state. Isn’t H2SO4 an electrolyte?

Tips (1) NaCl solution is a mixture, not an electrolyte.

(2) H2SO4 can conduct electricity in aqueous solution, so H2SO4 is an electrolyte.

2. Ionization of electrolytes

1.Definition

The process in which an electrolyte forms free-moving ions when it is dissolved in water or melted by heat.

2. Expression method - ionization equation

(1) Ionization of acid (such as H2SO4): H2SO4 2H++SO_4^2"-".

(2) Ionization of base (such as NaOH): NaOH Na++OH-.

(3) Ionization of salt (such as CuSO4): CuSO4 Cu2++SO_4^2"-".

3. Understand acids, bases and salts from the perspective of ionization:

(1) Acid: A compound in which all cations generated during ionization are hydrogen ions (H+);

(2) Base: a compound in which all the anions generated during ionization are hydroxide ions (OH-);

(3) Salt: a compound composed of metal cations or ammonium ions (N) and acid anions.

Autonomous testing

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

(1) Compounds that can conduct electricity in aqueous solutions and in the molten state are electrolytes. ()

(2) Compounds that can conduct electricity in water must be electrolytes. ()

(3) The ionization of the electrolyte requires electricity. ()

(4) Electrolytes are compounds, and electrolyte solutions are mixtures. ()

(5) An electrolyte that can ionize to produce H+ when dissolved in water must be an acid. ()

(6) Sodium chloride crystals cannot conduct electricity because they do not contain ions. ()

Answer(1)×　(2)×　(3)×　(4)√　(5)×　(6)×

2. The following substances are available: ① Nitrogen ② Liquid CO2 ③ Hydrogen chloride gas ④ Copper sheet ⑤ Barium sulfate crystal ⑥ Sucrose ⑦ Alcohol ⑧ Melted KNO3 ⑨ NaOH solution

Please answer the following questions (fill in the serial numbers):

(1) The above substances that can conduct electricity are __________.

(2) Among the above substances, the electrolyte is __________.

(3)③⑧The ionization equations of the two substances are

③__________,

⑧__________.

Answer (1)④⑧⑨　(2)③⑤⑧　(3)③HCl=H++Cl-　⑧

Ionization of electrolytes PPT, part 3 content: classroom exploration and learning

Electrolytes and their conductivity

Question exploration

(1) The device shown in the picture above is a device for testing the conductivity of substances. Add the following substances to a dry beaker in sequence and observe whether the light bulb becomes brighter? Is the substance added to the beaker an electrolyte?

(2) Through the above experiments, discuss: Is the electrolyte itself necessarily conductive? What is the general environment in which the electrolyte conducts electricity?

(3) If absolute alcohol or alcohol aqueous solution is put into the beaker above and the light bulb does not light up, is alcohol an electrolyte?

Deepen and expand

Judgment of electrolytes

(1) From the perspective of substance classification: electrolytes and non-electrolytes both belong to compounds. Elements and mixtures are neither electrolytes nor non-electrolytes.

Common acids (common strong acids HCl, H2SO4, HNO3, HI, HBr, HClO4, etc.; common weak acids H2CO3, H2S, H2SO3, CH3COOH, etc.), bases - common strong bases NaOH, KOH, Ca(OH)2, Ba (OH)2, etc.; common weak bases NH3·H2O, Fe(OH)3, Cu(OH)2, etc., salts, most metal oxides, and water are electrolytes, while most non-metal oxides, most Organic matter, NH3, etc. are non-electrolytes.

(2) From the perspective of material properties: electrolytes conduct electricity under certain conditions. The condition for electrolyte to conduct electricity is that the electrolyte is dissolved in water or in a molten state, and one of the two is sufficient. Some electrolytes conduct electricity when dissolved in water, but do not conduct electricity in the molten state, such as HCl gas; some electrolytes can only conduct electricity in the molten state, such as BaSO4.

(3) Whether a compound is an electrolyte or not has nothing to do with its solubility. For example, sucrose can be dissolved in water, but sucrose is a non-electrolyte; salts that are insoluble in water, such as BaSO4 and CaCO3, are electrolytes.

(4) Compounds that can conduct electricity when dissolved in water are not necessarily electrolytes. For example, CO2 aqueous solution can conduct electricity, but it is not the CO2 molecules themselves that ionize to produce ions, but the H2CO3 generated by its reaction with water ionizes to produce freely moving ions, so H2CO3 is an electrolyte, and CO2 is not an electrolyte.

Su Neng application

Example 1 Which of the following statements is correct ()

A. Liquid hydrogen chloride cannot conduct electricity, but hydrogen chloride is an electrolyte

B. Aqueous solutions of Cu and Cl2 can both conduct electricity, so Cu and Cl2 are both electrolytes.

C. If an aqueous solution of a certain compound can conduct electricity, the compound must be an electrolyte

D.BaSO4 is difficult to dissolve in water, so BaSO4 is not an electrolyte

Answer A

Analyzing item A, the aqueous solution of HCl can conduct electricity, so HCl is an electrolyte; item B, Cu and Cl2 are both simple substances and do not belong to electrolytes; item C, the aqueous solution of CO2 can conduct electricity, but CO2 is not an electrolyte; item D, although BaSO4 is difficult It dissolves, but the dissolved part is all ionized, and BaSO4 can conduct electricity in the molten state, so BaSO4 is an electrolyte.

Error-prone reminder: There are two conditions for electrolyte ionization: in aqueous solution or molten state, no electricity is required; ionization is a prerequisite for electrolyte conduction.

Variation training 1 Electrolytes not only occupy an important position in industrial and agricultural production, but also play an important role in various life activities. Which of the following statements about electrolytes is correct ()

A. Compounds are all electrolytes

B. Pure water has poor electrical conductivity, but water is also an electrolyte

C. Electrolytes must be able to conduct electricity in water, and compounds that conduct electricity in water must be electrolytes.

D. NaNO3 solid does not conduct electricity, so NaNO3 is not an electrolyte

Answer B

Analysis: Compounds that can conduct electricity in an aqueous solution or in a molten state are electrolytes. Item A is wrong. Water is an electrolyte. Item B is correct. There are conditions for electrolytes to conduct electricity. Electrolytes may not be able to conduct electricity in water, such as barium sulfate, which conducts electricity in water. The compound is not necessarily an electrolyte, such as carbon dioxide, item C is wrong; NaNO3 solution can conduct electricity, so NaNO3 is an electrolyte, item D is wrong.

Ionization of electrolytes PPT, Part 4: In-class testing

1. Electrolyte refers to a compound that can conduct electricity in an aqueous solution or in a molten state. Several students expressed the following understandings or opinions on the key words in this definition. Which one do you think is incorrect ()

A. The word "or" means that only one of the two conditions in the aqueous solution or in the molten state is required.

B. "Able to conduct electricity" means that the substance itself can ionize to produce ions and conduct electricity, rather than the product of its reaction to ionize to produce ions and conduct electricity.

C. "Compound" indicates that the substance cannot be a single substance, let alone a mixture.

D. A poorly soluble compound like barium sulfate cannot be an electrolyte.

AnswerD

Analysis of item D is wrong. Barium sulfate can conduct electricity in the molten state and is an electrolyte.

2. Which of the following statements is correct ()

A. Graphite has good electrical conductivity, so graphite is an electrolyte

B. It can be seen from experiments that the aqueous solution of NH3 has a certain conductivity, so NH3 is an electrolyte

C. Neither liquid HCl nor solid NaCl can conduct electricity, so neither HCl nor NaCl are electrolytes.

D. Sucrose cannot conduct electricity in an aqueous solution or in a molten state, so sucrose is not an electrolyte.

AnswerD

Analytical graphite is a simple substance, not a compound, so it does not belong to an electrolyte. Item A is incorrect; an aqueous solution of NH3 can conduct electricity because NH3 reacts with H2O to form NH3·H2O. NH3·H2O ionizes to produce freely moving ions and conducts electricity. Item B is incorrect. Correct; although liquid HCl and solid NaCl do not conduct electricity, their aqueous solutions can conduct electricity, so both are electrolytes. Item C is incorrect.

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For more information about the "Ionization of Ion Reaction Electrolytes" PPT courseware, please click on the Ionization of Ion Reaction ppt Electrolyte ppt tab.

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Update Time: 2024-11-26

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