"End of Chapter Review Lesson" Matter and its Changes PPT

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"End of Chapter Review Lesson" Matter and its Changes PPT

Special topic summary and practice

True or False Judgment of Ionic Equations

1. Check whether it is consistent with objective facts. For example, if Fe reacts with dilute sulfuric acid, it is wrong to write 2Fe＋6H＋===2Fe3＋＋3H2↑.

2. Check whether the chemical formula is written correctly. For example, the reaction between NaHCO3 and dilute hydrochloric acid is written as 2H++CO2-3===CO2↑+H2O, which is wrong.

3． See if conservation of mass and charge are followed. For example, Zn＋Ag＋===Zn2＋＋Ag charge is not conserved.

4． See if some ion reactions are missed. For example, for the reaction between H2SO4 solution and Ba(OH)2 solution, it is wrong to write Ba2++SO2-4===BaSO4↓ or H++OH-===H2O.

Thematic sparring

1. Iron, dilute hydrochloric acid, clarified lime water, and copper chloride solution are common substances in middle school chemistry. As shown in the figure, the wrong ionic equation for the reaction between the four substances is ()

A. OH－＋H＋===H2O

B． 2OH－＋Cu2＋===Cu(OH)2↓

C． Fe＋Cu2＋===Cu＋Fe2＋

D． Fe＋2H＋===Fe3＋＋H2↑

2. The correct ionic equation for the following reaction is ()

A. Use dilute hydrochloric acid to remove calcium carbonate in scale: Ca2＋＋CO2-3＋2H＋===Ca2＋＋H2O＋CO2↑

B． Use dilute hydrochloric acid to remove magnesium hydroxide from scale: Mg(OH)2＋2H＋===Mg2＋＋2H2O

C． Use sodium bicarbonate as an antacid to neutralize gastric acid: 2H++CO2-3===H2O+CO2↑

D． Use H2SO4 to neutralize alkaline wastewater: H2SO4+2OH-===2H2O+SO2-4

Determine whether ions can coexist in large quantities in aqueous solution

The key to whether ions can coexist in large amounts in a solution is to see whether the ions meet the conditions for ionic reactions to occur. If they react, they cannot coexist in large amounts.

1. See if insoluble or slightly soluble substances can be generated between ions. Be proficient in memorizing the solubility of acids, bases, and salts, especially insoluble salts.

2. See if the ions can react to form gas. There are two types of gases: acidic gases and alkaline gases. Specifically, volatile weak acidic acid radicals and H+ cannot coexist in large amounts; ammonium salts and strong bases cannot coexist in large amounts.

3． See if the ions can react to form difficult-to-ionize substances (weak acids, weak bases, water, etc.). Hydrochloric acid, sulfuric acid and nitric acid among acids are easy to ionize, and other acids are generally difficult to ionize; sodium hydroxide, potassium hydroxide, calcium hydroxide, and barium hydroxide among alkali are easy to ionize, and other alkali are considered to be difficult to ionize.

4． See if redox reactions can occur between ions, etc.

5. Pay attention to the restrictive conditions attached to the question

(1) In a colorless and transparent solution, colored ions cannot exist, such as Cu2+ (blue), Fe3+ (brown), Fe2+ (light green), MnO-4 (purple), etc.

(2) In strongly acidic solutions, ions that react with H+ cannot coexist in large quantities.

(3) In a strongly alkaline solution, ions that react with OH- cannot coexist in large quantities.

Redox reactions

1. Clarify the relationship between concepts

2. Associative memory keywords

(1) Memorize the formula: "When it rises, it loses oxygen, and when it falls, it regains oxygen." Its meaning is: the valence increases → loses electrons (electron pair deviation) → is oxidized → reducing agent → has reducing properties (electron losing ability); the valence decreases → gains electrons (electron pair deviation) → is reduced → oxidizing agent → has oxidizing properties (Get electronic abilities).

(2) Memory formula: "The dosage properties are the same, and the others are opposite." Its meaning is: the oxidizing agent has oxidizing properties and the reducing agent has reducing properties; the "other opposite" means that the oxidizing agent is reduced, a reduction reaction occurs, and a reduction product is obtained; the reducing agent is oxidized, an oxidation reaction occurs, and an oxidation product is obtained.

3． Learn the correct analysis method

Valence changes are the premise and basis for analyzing all redox reactions. Correctly marking the valence of each element is the key and breakthrough for analyzing redox reactions. The specific method is to find the variable price and determine the type (whether it is a redox reaction); classify the increase or decrease and determine the others (the valence increases, electrons are lost, an oxidation reaction occurs, the valence decreases, electrons are gained, and a reduction reaction occurs).

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For more information about the "End-of-Chapter Review Lesson Substances and Their Changes" PPT courseware, please click the "End-of-Chapter Review Lesson PPT Substances and Their Changes" PPT courseware.

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Update Time: 2024-07-03

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