"Diversity of Iron" PPT courseware on the properties and transformation of matter (lesson 2 iron, iron oxides and iron hydroxides)

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"Diversity of Iron" PPT courseware on the properties and transformation of matter (lesson 2 iron, iron oxides and iron hydroxides)

Part One: Literacy Goals

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

2. Able to master the properties and typical experimental phenomena of elemental iron, FeO, Fe2O3, Fe(OH)2, Fe(OH)3 through experimental exploration and communication and discussion, and be able to write major chemical equations and ionic equations. Be able to proactively communicate and gradually improve scientific inquiry and innovation capabilities.

3. Understand the application of iron-containing substances in production and life, establish the connection between the properties, experimental phenomena and applications of iron-containing substances, and strengthen the scientific attitude and social responsibility.

Diversity of Iron PPT, Part 2: Knowledge Padding

1. Metal elements can react with non-metals and can react with water or acid to produce H2. Can undergo displacement reactions with certain salt solutions. And the more active the metal, the more violent it will react with water or acid.

2. Alkaline oxides are metal oxides that can react with acids to form salts and water. For example, Na2O+2HCl === 2NaCl+H2O, iron oxides can also react with acids.

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

1. Properties of elemental iron

1.Physical properties

Iron is a bright silver-white metal with a high density and a melting point of 1538°C. Pure iron has strong corrosion resistance. It has good ductility and thermal conductivity. Its electrical conductivity is worse than that of copper and aluminum, and it can be attracted by magnets.

2. Chemical properties

2. Comparison of the properties of iron oxides - FeO, Fe2O3 and Fe3O4

3. Comparison of properties of iron hydroxides - Fe(OH)2 and Fe(OH)3

[Micro Thought 1] Given that 2Fe+3Cl2 2FeCl3 and Fe+S FeS, please determine the oxidizing properties of Cl2 and sulfur?

Tip: Cl2 can oxidize Fe to +3 valence, while elemental sulfur can only oxidize Fe to +2 valence, indicating that Cl2 is more oxidizing than elemental sulfur.

[Micro Thinking 2] Point out the reaction between iron and water vapor, and the oxidants and reducing agents in the thermite reaction.

Tip: In the reaction between iron and water vapor, iron acts as a reducing agent and water acts as an oxidizing agent, indicating that iron has reducing properties. In the thermite reaction, aluminum acts as the reducing agent and iron oxide acts as the oxidizing agent, indicating that iron oxide has oxidizing properties.

Diversity of Iron PPT, Part 4: Independent Testing

1. The physical properties of pure iron are ()

①Bright silvery white ②Black ③Easily corroded in humid air

④ It is ductile ⑤ It can conduct electricity and heat ⑥ It is hard and brittle ⑦ It can be attracted by magnets and is easily magnetized ⑧ Its density is smaller than aluminum

A.①③④⑤⑦B.①④⑤⑦

C.①③⑤⑦ D.All

Answer:B

2. Which of the following statements about iron and its compounds is correct ()

A. Hematite is reddish brown and its main component is FeO

B. Pig iron and steel are both iron alloys, containing iron elements and no non-metallic elements.

C. Iron is more susceptible to corrosion than aluminum, indicating that iron is more active than aluminum

D.Fe(OH)2 is unstable and will be quickly oxidized to Fe(OH)3 in solution

Answer:D

Analysis: The main component of hematite is Fe2O3, item A is wrong; Pig iron and steel contain carbon elements, item B is wrong; Aluminum is more active than iron, because aluminum surface easily forms a dense oxide film to resist corrosion, item C is wrong; Fe (OH)2 is very reducible and easily oxidized, so option D is correct.

Diversity of Iron PPT, Part 5: Exploration

properties of iron

Question exploration

During the class group experiment, Xiao Ming accidentally mixed a small amount of iron powder into copper powder. Classmate Xiao Ming wanted to discard the mixture, but was stopped by classmate Xiao Bing. Xiao Bing used the knowledge he had learned to successfully remove a small amount of iron powder. Can FeCl3 solution be used to remove iron powder mixed in copper powder? If not, what reagent can be used? What other methods can be used?

Tip: Since FeCl3 not only reacts with Fe, but also with Cu, FeCl3 solution cannot be used to remove iron powder mixed in copper powder; H2SO4 and CuSO4 solutions both react with Fe but not with Cu, so H2SO4 or CuSO4 can be used The solution removes the iron powder mixed in the copper powder. In addition, iron can be attracted by magnets but copper cannot, so magnets can also be used to suck out iron powder.

Knowledge induction

(1) Fe and H2O do not react at room temperature. However, Fe is easily corroded under the combined action of water and O2 in the air. Iron cannot react with hot water, but at high temperatures, Fe can

React with H2O(g) 3Fe+4H2O(g) Fe3O4+4H2.

(2) The valence of the iron element in the iron element is 0. The iron element has reducing properties and can react with oxidizing substances.

(3) Fe only has reducing properties and can be oxidized to Fe2+ and Fe3+ by oxidants.

①Fe can be oxidized to Fe2+ by weak oxidants such as I2, S, Fe3+, Cu2+, H+, such as Fe+S FeS, Fe+2Fe3+ 3Fe2+.

②Fe can be oxidized to Fe3+ by strong oxidants such as Cl2, such as 2Fe+3Cl2 2FeCl3.

Analysis of typical cases

Example 1: Put iron pieces into each of the following solutions. After the reaction, the mass of the solution increases and no gas is produced. ()

A.CuCl2 solution B.AgNO3 solution

C.Fe2(SO4)3 solution D.Dilute sulfuric acid

Answer:C

Analysis: Fe reacts with CuCl2 solution. Every time 56 g Fe is dissolved, 64 g Cu is generated. The quality of the solution is reduced. Item A is wrong. Fe reacts with AgNO3 solution. For every 56 g of Fe dissolved, 216 g of Ag are generated. The quality of the solution is reduced, and item B is incorrect. Fe reacts with Fe2(SO4)3 solution, Fe dissolves, the solution mass increases and no gas is released, item C is correct. Fe reacts with dilute sulfuric acid. For every 56 g of Fe dissolved, 2 g of H2 is generated. The mass of the solution increases, but gas is released, which is an error.

Point training 1-1 Which of the following substances reacts with iron to only produce +3-valent iron compounds ()

A.Cl2 B. Hydrochloric acid C.O2 D.CuSO4

Answer:A

Analysis: The transformation of Fe→Fe3+ requires a strong oxidant. Iron burns in O2 to produce Fe3O4. Hydrochloric acid, CuSO4 and Fe undergo a displacement reaction to produce +2-valent iron compounds.

Point-to-Point Training 1-2 Which of the following statements about the reaction between metals and water is correct ()

A. Sodium can sink to the bottom and react violently with water

B. Since aluminum pots can be used to boil water, aluminum cannot react with boiling water.

C. Iron and cold water can react to produce ferric oxide and hydrogen.

D. The weaker the reactivity of the metal, the more stringent the conditions required to react with water.

Answer:D

Analysis: The density of sodium is smaller than that of water. So it is impossible for sodium to sink to the bottom of the water and react violently with water, so item A is wrong. Aluminum pots can be used to boil water because there is a dense oxide film on the surface of the aluminum to prevent the internal metal from continuing to react, so Item B is incorrect; iron and water vapor can react to form iron ferric oxide and hydrogen, so item C is incorrect; the weaker the reactivity of the metal, the worse its reducibility, and the harsher the conditions required when reacting with water, so item D is correct.

Iron Diversity PPT, Part Six: In-class Testing

1. Which of the following substances cannot be produced by direct combustion of the corresponding elemental substances in air ()

A.MgO B.CO2 C.CO D.Fe3O4

Answer:D

Analysis: MgO can be generated by the combustion of magnesium ribbons in the air; CO2 and CO can be generated by the complete combustion and incomplete combustion of carbon in the air respectively; and Fe3O4 can only be generated by the combustion of iron wire in pure oxygen.

2. Which of the following solutions cannot obtain Fe3O4 ()

A. Place FeO in the air and heat it at high temperature

B. Burn the Fe wire in oxygen

C. Place the Fe wire in water vapor and heat it at high temperature

D. Place the Fe wire in humid air to slowly rust

Answer:D

Analysis: Rust appears reddish brown and its composition is Fe2O3.

3. Which of the following statements is correct ()

①Iron can be attracted by magnets ②Hemoglobin in the human body contains iron

③Fe can be burned in pure oxygen to obtain Fe2O3 ④Fe2O3 cannot react with water to obtain Fe(OH)3, so Fe(OH)3 cannot be produced through chemical reactions

⑤Fe(OH)2 is heated in air to obtain FeO

A.①② B.②④ C.②③④⑤ D.①②⑤

Answer:A

Analysis: ① Iron can be attracted by magnets, ② Human hemoglobin contains iron, ③ Iron can be burned in pure oxygen to obtain Fe3O4; ④ Fe(OH)3 can be obtained through the reaction 4Fe(OH)2+O2+2H2O === 4Fe(OH )3 is prepared; ⑤Fe(OH)2 is heated in air, and the final product is Fe2O3.

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Update Time: 2024-10-02

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