What are the guidelines for preparing the lesson "Redox Equations" under the 10th-grade Chemistry curriculum? What are the academic topics of the 10th-grade Chemistry curriculum in Vietnam?
What are the guidelines for preparing the lesson "Redox Equations" under the 10th-grade Chemistry curriculum in Vietnam?
Redox Equations
I. Oxidation Number
- Definition: The oxidation number is a value used to express the oxidation state of each element in a compound or ion.
- An element in its elemental state has an oxidation number of 0.
- In compounds, the oxidation number is governed by a set of rules as follows:
+ The oxidation number of O in most compounds is -2 (except in H2O2).
+ The oxidation number of H is usually +1 (except in compounds with metals).
- Rules for calculating oxidation numbers:
+ The sum of oxidation numbers of all elements in a neutral molecule is 0.
+ The sum of oxidation numbers in an ion equals the charge of that ion.
II. Redox Reactions
- Definition:
- A redox reaction is a reaction in which there is a transfer of electrons between substances.
- A reducing agent is a substance that donates electrons.
- An oxidizing agent is a substance that receives electrons.
- Oxidation process: Substance loses electrons.
- Reduction process: Substance gains electrons.
- Example:
Zn + CuSO4 → ZnSO4 + Cu
Zn loses electrons (defined as being oxidized).
Cu2+ gains electrons (defined as being reduced).
III. Formulating Chemical Equations for Redox Reactions
- Steps to perform:
- Step 1: Determine the oxidation numbers of the elements in the equation.
- Step 2: Identify the oxidizing agent and the reducing agent.
- Step 3: Write the oxidation and reduction processes, balance the electrons.
- Step 4: Balance the equation according to the number of moles of transferred electrons.
Example:
Formulate the reaction equation: Fe + Cl2 → FeCl3
The oxidation number of Fe increases from 0 to +3: oxidation.
The oxidation number of Cl decreases from 0 to -1: reduction.
Complete equation: 2Fe + 3Cl2 → 2FeCl3.
IV. Common Redox Equations
Reactions between metals and acid solutions:
Zn + 2HCl → ZnCl2 + H2
Fe + 2HCl → FeCl2 + H2
Reactions in an alkaline medium:
2MnO4- + 5H2O2 + 6OH- → 2MnO2 + 5O2 + 8H2O
Reduction of SO2 reaction:
SO2 + Br2 + 2H2O → H2SO4 + 2HBr
Oxidation of organic compounds:
CH3CHO + [O] → CH3COOH
See more commonly encountered redox equations:
Cu + HNO3 → Cu(NO3)2 + NO2 + H2O
FeO + HNO3 → Fe(NO3)3 + NO + H2O
H2S + Cl2 + H2O → H2SO4 + HCl
Fe3O4 + HNO3 → Fe(NO3)3 + NO + H2O
FeCO3 + H2SO4 → Fe2(SO4)3 + SO2 + CO2 + H2O
FeSO4 + NaOH → Fe(OH)2 + Na2SO4
Al + HNO3 → Al(NO3)3 + NO + H2O
Zn + HNO3 → Zn(NO3)2 + NO2 + H2O
H2S + FeCl3 → S + FeCl2 + HCl
FeSO4 + H2SO4 → Fe2(SO4)3 + SO2 + H2O
FeSO4 + HNO3 → Fe(NO3)3 + H2SO4 + NO2 + H2O
Fe(OH)2 + H2SO4 → Fe2(SO4)3 + H2S + H2O
Al + HNO3 → Al(NO3)3 + H2O + NO2
Ag + HNO3 → AgNO3 + NO + H2O
Fe3O4 + HNO3 → Fe(NO3)3 + NO + H2O
Al + HNO3 → Al(NO3)3 + N2O + H2O
Fe + HNO3 → Fe(NO3)3 + NO2 + H2O
Cu + HNO3 → Cu(NO3)2 + N2O + H2O
Fe3O4 + H2SO4 → Fe2(SO4)3 + SO2 + H2O
Mg + HNO3 → Mg(NO3)2 + NO + H2O
Fe + H2SO4 → Fe2(SO4)3 + SO2 + H2O
KMnO4 + HCl = KCl + MnCl2 + Cl2 + H2O
C2H4 + KMnO4 + H2O → C2H4(OH)2 + MnO2 + KOH
Fe + HNO3 → Fe(NO3)3 + NO+ H2O
Cu + H2SO4 → CuSO4 + SO2 + H2O
Al + HNO3 → Al(NO3)3 + N2 + H2O
Mg + HNO3 → Mg(NO3)2 + NO2 + H2O
Zn + HNO3 → Zn(NO3)2 + NH4NO3 + H2O
Al + H2O + NaOH → NaAlO2 + H2
K2Cr2O7 + HCl → CrCl3 + KCl + Cl2+ H2O
C6H12O6 + KMnO4 + H2SO4 → MnSO4+ H2O + K2SO4 + CO2
Mg + HNO3 → Mg(NO3)2 + NO + H2O
Fe(NO3)2 + HCl → Fe(NO3)3 + FeCl3 + NO + H2O
Fe3O4 + HNO3 → Fe(NO3)3 + NO2 + H2O
H2S + O2 → SO2 + H2O
Fe + HNO3 → Fe(NO3)3 + N2O + H2O
Fe(OH)2+ HNO3 → Fe(NO3)3 + NO2 + H2O
NO + K2CrO7 + H2SO4 → HNO3 + K2SO4 + H2O + Cr2(SO4)3
FeSO4 + K2Cr2O7 + H2SO4 → Fe2(SO4)3 + Cr2(SO4)3 + K2SO4 + H2O
Mg + HNO3 → Mg(NO3)2 + N2O + H2O
SO2 + KMnO4 + H2O → MnSO4 + K2SO4 + H2SO4
Fe3O4 + H2SO4 → Fe2(SO4)3 + SO2 + H2O
Ag + HNO3 → AgNO3 + NO + H2O
Zn + HNO3 → Zn(NO3)2 + NO + H2O
H2S + H2SO4 → SO2 + H2O + S
Al + HNO3 → Al(NO3)3 + NO + H2O
Cu + HNO3 → Cu(NO3)2 + NO+ H2O
Fe3O4 + H2SO4 → Fe2(SO4)3 + SO2 + H2O
FeO + H2SO4 → Fe2(SO4)3 + SO2 + H2O
C2H2 + KMnO4 + H2O → (COOH)2 + MnO2 + KOH
H2S + KMnO4 → KOH + MnO2+ S + H2O
Zn + H2SO4 → ZnSO4 + SO2 + H2O
Fe3O4 + HNO3 → Fe(NO3)3+ NO2 + H2O
Mg + HNO3 → Mg(NO3)2 + N2 + H2
Zn + HNO3 → Zn(NO3)2 + N2 + H2O
H2S + CuSO4 → CuS + H2SO4
Ag + HNO3 → AgNO3 + NO2 + H2O
What are the guidelines for preparing the lesson "Redox Equations" under the 10th-grade Chemistry curriculum? What are the academic topics of the 10th-grade Chemistry curriculum in Vietnam? (Image from Internet)
What are the academic topics of the 10th-grade Chemistry curriculum in Vietnam?
Under the general education program of Chemistry issued together with Circular 32/2018/TT-BGDDT, there are 3 academic topics in the 10th-grade Chemistry curriculum:
Topic 10.1: CHEMICAL BASIS
- Chemical bonding
- Nuclear reactions
- Activation energy of chemical reactions
- Entropy and Gibbs Free Energy Variability
Topic 10.2: CHEMISTRY IN FIRE PREVENTION AND FIGHTING
- A Brief Introduction to Fire and Explosion Reactions
- Flashpoint (Flash temperature), self-ignition temperature and fire temperature
- Chemistry of fire and explosion reactions
Topic 10.3: CHEMISTRY AND INFORMATION TECHNOLOGY PRACTICE
- Drawing molecular structures
- Practice virtual chemistry experiments
- Structural and energy parameterization
What is the method of forming and developing the key traits of the 10th-grade Chemistry curriculum in Vietnam?
Under Subsection 2, Section 6 of the General Education Program in Chemistry promulgated together with Circular 32/2018/TT-BGDDT, the method of forming and developing the key traits of the 10th-grade Chemistry curriculum in Vietnam is as follows:
Through the organization of learning activities, teachers help students form and develop a scientific worldview, practice honesty, love of work, and a sense of responsibility;
Based on experimental and practical activities, especially visits and practices in laboratories, production facilities, and different areas to contribute to raising students' awareness of the protection and rational use of natural resources, the sense of responsibility of workers, and the principle of ensuring safety in production labor, especially in chemical-related disciplines
Teachers apply diverse forms of learning to foster students' interest and confidence in learning, scientific exploration, appreciation for the fruits of scientific labor, and the ability to apply scientific knowledge to life.
