"Diversity of Iron" PPT courseware on the properties and transformation of substances (Lesson 1 Ferrous Salts and Iron Salts)

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"Diversity of Iron" PPT courseware on the properties and transformation of substances (Lesson 1 Ferrous Salts and Iron Salts)

Part One: Literacy Goals

1. Based on application examples in production and life or through experimental exploration, be able to understand the main properties of iron and its important compounds from a combination of macro and micro perspectives.

2. Be able to complete experiments independently or in cooperation with classmates, record experimental phenomena and data, complete experimental reports, and actively communicate, gradually improving scientific inquiry and innovation capabilities.

3. Apply the principles of redox reactions and experiments to study the transformation relationships between important iron compounds, master the tests of Fe3+ and Fe2+, and cultivate awareness of evidence reasoning and model cognition.

Diversity of Iron PPT, Part 2: Knowledge Padding

1. Common valences of iron include 0, +2 and +3. Give an example and write down the chemical formulas of the corresponding substances Fe, FeCl2 and FeCl3.

2. Generally speaking, an element has oxidizing properties when it is in a high valence state, it only has reducing properties when it is in the lowest valence state, and it has both oxidizing and reducing properties when it is in an intermediate valence state. Please determine what the behavior of iron in the following reactions is. Oxidizing or reducing.

(1)Fe2O3+3CO 2Fe+3CO2: Oxidizing property.

(2)Fe+2H+ Fe2++H2↑　Reducibility.

(3)2Fe2++Cl2 2Fe3++2Cl- Reducibility.

Diversity of Iron PPT, Part 3: Preview of New Knowledge

1. The existence of iron element

1. Content

The content of iron in the earth's crust is second only to oxygen, silicon and aluminum.

2. Existence form

(1) Free state: Found in meteorite.

(2) Compound state: mainly exists as +2 and +3 valent iron compounds. Such as pyrite (FeS2), hematite (Fe2O3), magnetite (Fe3O4), siderite (FeCO3), etc.

2. Properties of Fe2+ and Fe3+

1. Experimental predictions and hypotheses

2. Experimental operations and phenomena

[Micro Thought 1] In the laboratory, some iron filings or nails are usually added to the reagent bottles containing FeSO4 solution. Why is this?

Tip: Fe2+ has strong reducing properties and is easily oxidized and deteriorated. Therefore, the purpose of adding elemental iron to the reagent bottle containing the ferrous salt solution is to prevent Fe2+ from being oxidized.

[Micro Thought 2] How to remove the impurity FeCl2 mixed in the FeCl3 solution?

Tip: Pour in Cl2 or add chlorine water dropwise or add "green" oxidant H2O2 solution:

Diversity of Iron PPT, Part 4: Independent Testing

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

(1) Iron is the third most abundant element in the earth’s crust. ()

(2) There is no free iron in nature. ()

(3) Industrial ironmaking requires the addition of reducing agents. ()

(4) Steel and pig iron are both alloys of iron. Steel is not easy to rust, while pig iron is easy to rust. The main component of rust is Fe3O4. ()

Answer: (1)× (2)× (3)√ (4)×

Analysis: Iron is the fourth most abundant element in the earth’s crust. Free iron is found in meteorites. The general process of industrial ironmaking is Fe2O3==Fe. The main component of rust is Fe2O3.

2. (1) When Cl2 is introduced into the FeCl2 solution, the phenomenon is: the solution changes from ______ to ______.

(2) The chemical equation for the reaction between sufficient Cl2 and Fe is ______,

The ionic equation for the reaction of Fe with dilute sulfuric acid is ______.

Answer: (1) light green brown

Diversity of Iron PPT, Part 5: Exploration

Properties of Fe2+ and Fe3+

Question exploration

In a mixed solution of FeCl3 and CuCl2, an excess of iron powder is added. After full reaction, what are the metal ions in the solution?

Knowledge induction

(1) Fe2+ has both reducing and oxidizing properties, and can be oxidized to Fe3+ or reduced to Fe.

① When Fe2+ encounters a strong oxidizing agent, it is oxidized to Fe3+, such as 2Fe2++Cl2 2Fe3++2Cl-.

② When Fe2+ encounters reducing agents such as C, Al, Zn, and CO, it can be reduced to Fe, such as Fe2++Zn Zn2++Fe, FeO+CO Fe+CO2.

(2) Fe3+ has strong oxidizing property and can be reduced to Fe2+ or Fe.

①Fe3+ is reduced to Fe by C, CO, Al, etc., such as Fe2O3+3CO 2Fe+3CO2, Fe2O3+2Al 2Fe+Al2O3.

②Fe3+ is reduced to Fe2+ by Fe, Cu, etc., such as 2Fe3++Cu 2Fe2++Cu2+.

Analysis of typical cases

Example 1 It is known that chemical reactions can occur in the following three experiments:

①Put the bright iron nails into the copper sulfate solution; ②Put a few drops of hydrogen peroxide into the ferrous sulfate solution; ③Put the copper wire into the ferric chloride solution. Which of the following is correct ()

A. In experiment ①, iron nails are used as oxidants.

B. Fe2+ has reducing properties in experiment ②

C. What occurred in experiment ③ was a displacement reaction

D. The above experiments prove that oxidizing Fe3+>Fe2+>Cu2+

Answer:B

Analysis: A substitution reaction occurs between iron and copper sulfate to form copper and ferrous sulfate. Iron is a reducing agent. Item A is wrong. Add a few drops of hydrogen peroxide to the ferrous sulfate solution, and the ferrous ions are oxidized to form ferrous ions, reflecting the ferrous ions. The reducibility of , item B is correct; putting copper wire into a ferric chloride solution produces ferrous chloride and copper chloride, which is not a replacement reaction, item C is wrong; the oxidizing property of the oxidizing agent is stronger than the oxidizing property of the oxidation product, then oxidation The property is Fe3+>Cu2+>Fe2+, item D is wrong.

Method rules: Coexistence rules of iron, copper and their compounds in solutions

(1) Fe can react with Fe3+ and Cu2+, so when there is Fe powder remaining in the solution, it is impossible for Fe3+ and Cu2+ to exist in large amounts in the solution. Since the oxidizing Fe3+>Cu2+, iron powder is added to the mixed solution of Fe3+ and Cu2+, and the iron reacts with Fe3+ first; since the reducing Fe>Cu, the Fe and Cu mixture is added to the Fe3+ solution, and Fe reacts first.

(2) Cu can react with Fe3+, so when Cu precipitates, there cannot be a large amount of Fe3+ in the solution.

(3) Fe2+ can coexist with Fe3+, Cu2+, Fe, and Cu in large amounts.

Point training 1-1 After the reaction of the following substances, +3 valent iron must be produced ()

①Excess Fe reacts with Cl2; ②After Fe reacts with excess dilute sulfuric acid, add H2O2 solution to it; ③Add a small amount of hydrochloric acid to the Fe(NO3)2 solution; ④The mixture of Fe and Fe2O3 is dissolved in hydrochloric acid.

A. Only ① B. Only ①② C. Only ①②③ D. All

Answer:C

Analysis: Cl2 in ① is highly oxidizing and can oxidize iron to +3. Since it does not react in solution, excess iron will not reduce ferric chloride. ② The reaction between Fe and dilute sulfuric acid can only generate Fe2+. After adding H2O2 solution to it, since H2O2 is a common oxidizing agent, it can oxidize Fe2+ into Fe3+. ③On the surface, no reaction will occur, but in fact, Fe2+ is oxidized by nitric acid. In ④, Fe reacts with hydrochloric acid first to form FeCl2, and Fe2O3 reacts with hydrochloric acid to form FeCl3. However, the relative quantity relationship between the reactants is not given in the question. If iron is sufficient, all the FeCl3 generated can be reduced to FeCl2.

Iron Diversity PPT, Part Six: In-class Testing

1. Put iron powder into a mixed solution composed of hydrochloric acid, MgCl2 solution, FeCl3 solution, and CuCl2 solution. After full reaction, if there is remaining iron powder, then the large number of cations contained in the solution at this time is ()

A.Cu2+ and Fe2+ B.Fe2+ and Mg2+

C.Fe3+ and Fe2+ D.H+ and Cu2+

Answer:B

Analysis: The following reaction occurs when iron powder is added to the mixed solution: 2H++Fe Fe2++H2↑, iron and MgCl2 solutions cannot react, 2Fe3++Fe 3Fe2+, Cu2++Fe Fe2++Cu, because there is remaining iron powder, Therefore, the cations in the solution at this time mainly include Mg2+ and Fe2+.

2. Which of the following reactions can ultimately produce compounds containing Fe3+ ()

①Excess Fe and dilute nitric acid; ②Iron wire burning in sulfur vapor; ③Pour Cl2 into FeBr2 solution; ④Reaction of iron and CuCl2 solution

⑤Fe(OH)2 is exposed in the air

A.①②③ B.①③⑤

C.③④ D.③⑤

Answer:D

Analysis: ①Fe reacts with dilute nitric acid to form ferric nitrate, and Fe3+ reacts with excess Fe to form Fe2+, so it is not selected; ②The iron wire burns in sulfur vapor to form FeS, so it is not selected; ③Pour Cl2 into the FeBr2 solution, and due to the reduction of Fe2+ Stronger than Br-, chlorine first oxidizes Fe2+ to Fe3+, so it is selected; ④ Iron reacts with CuCl2 solution to generate ferrous chloride and copper, so it is not selected; ⑤ Fe(OH)2 is exposed to the air and reacts with oxygen and water The reaction produces Fe(OH)3, so it is selected.

3. In order to verify the properties of Fe3+, a chemical interest group designed a set of experiments as shown in the figure. Among them, the wrong experimental plan design is ()

A.④ B.③ C.③④ D.①②③④⑤

Answer:C

Analysis: ③ No reaction, the experimental plan and phenomenon are wrong; ④ What is tested is Cl-, which has nothing to do with the properties of Fe3+.

Keywords: Free download of PPT courseware for compulsory course 1 of high school chemistry in Lu Ke version, PPT download of diversity of iron, PPT download of properties and transformation of matter, PPT download of ferrous salts and iron salts, .PPT format;

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