Untitled Flashcards Set

Unit Title: Action Reaction - Chemical Reaction

Quarter 3

Unit Concept

• Chemical Reactions: Understanding the processes where substances transform and interact to form new products, emphasizing the importance of balancing and understanding reaction equations.

• Valency: The measure of bonding capacity of elements, indicating how many atoms of each element can combine.

• Equations: Representations of chemical reactions that show the relationships between reactants and products.

• Changes: Differentiating between physical changes (where substances remain the same) and chemical changes (where new substances are formed).

• Acids and Bases: Properties, interactions, and applications of acids and bases in various contexts.

• Applications: Real-world examples demonstrating the practical uses of chemical reactions in daily life and industries.

• Reaction Types: Understanding various types of chemical reactions including synthesis, decomposition, single replacement, double replacement, and combustion.

Global Context

• Globalization and Sustainability: Investigating how chemical reactions play a crucial role in creating sustainable solutions in the chemical industry.

Key Concept

• Change: Focusing on the transformations that matter undergoes through different reactions.

Related Concept

• Interactions: Emphasizing how substances interact to create new materials and the implications of those interactions for sustainability.

Statement of Inquiry

• The chemical industry can provide sustainable solutions through various changes brought by the interactions of matter.

Sciences Criteria to be Assessed

Quarter 3 A, B, C & D

Criteria D: Research and Inquiry

• Research Paper: The significance of understanding chemical reactions is paramount in developing sustainable chemical processes. This research paper explores recent advancements in chemical manufacturing that focus on reducing waste and enhancing energy efficiency. For instance, catalytic processes that improve the speed and yield of reactions are being investigated to minimize resource consumption. Furthermore, the paper delves into bio-chemicals, highlighting breakthroughs in using biological materials for creating chemicals, which further supports the concept of sustainability.

• Balancing Chemical Equations: This is essential for understanding the conservation of mass in chemical reactions.

Sample Balancing Equations

1. Combustion Reaction:

   • Unbalanced Equation: C₃H₈ + O₂ → CO₂ + H₂O

   • Balanced Equation: C₃H₈ + 5 O₂ → 3 CO₂ + 4 H₂O

   • This equation illustrates the combustion of propane, showing the ratio of reactants to products necessary to conserve the number of atoms.

2. Synthesis Reaction:

   • Unbalanced Equation: N₂ + H₂ → NH₃

   • Balanced Equation: N₂ + 3 H₂ → 2 NH₃

   • This demonstrates the formation of ammonia from nitrogen and hydrogen gases.

3. Decomposition Reaction:

   • Unbalanced Equation: 2 H₂O → H₂ + O₂

   • Balanced Equation: 2 H₂O → 2 H₂ + O₂

   • This shows how water can be broken down into hydrogen and oxygen gas.

4. Double Replacement Reaction:

   • Unbalanced Equation: AgNO₃ + NaCl → AgCl + NaNO₃

   • Balanced Equation: AgNO₃ + NaCl → AgCl + NaNO₃

   • In this reaction, silver nitrate and sodium chloride exchange ions to form silver chloride and sodium nitrate.

Unit Content

1. Chemical Reactions: In-depth study of reactions, including the role of energy changes, catalysts, and inhibitors in chemical processes.

2. Valency and Chemical Formula: Understanding through the criss-cross rule, including complex ions and their charges.

3. Balancing Chemical Equations: Techniques for balancing various types of equations, including oxidation-reduction reactions.

4. Physical and Chemical Change: Methods for detecting and identifying physical versus chemical changes in experiments.

5. Acids, Bases, and Salts: Exploring reactions of acids with bases (neutralization) and the resultant salt and water.

6. Applications of Acids, Bases, and Salts: Real-life applications such as in food preservation, cleaning agents, and pH regulation.

7. Types of Chemical Reaction: Analyzing complex reaction types and their real-world implications.

Periodic Table and Valency

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### Unit Concept: Chemical Reactions 

Chemical reactions involve the process in which substances (reactants) transform into different substances (products). These changes are driven by the interaction between atoms, molecules, or ions. Chemical reactions play a fundamental role in various chemical processes, both in nature and industry. 

### Key Concepts 

1. Chemical Reactions: Reactions are processes where substances interact to form new substances with different properties. 

2. Valency: The combining power of an element, indicating how many atoms of another element it can bond with. It is determined by the number of electrons in the outer shell. 

3. Equations: A chemical equation represents a chemical reaction using symbols of elements and compounds. It shows the reactants and products, and the process of transformation. 

4. Changes: Chemical reactions can result in physical or chemical changes. 

   - Physical Change: A change in the state or appearance of a substance without changing its chemical composition. 

   - Chemical Change: A change that results in the formation of new substances with different chemical compositions. 

5. Acids and Bases: Acids release hydrogen ions (H⁺) in solutions, while bases release hydroxide ions (OH⁻). Acids and bases interact to form salts and water in neutralization reactions. 

6. Applications: Chemical reactions have practical applications in everyday life, such as in cleaning, medicine, food preservation, and energy production. 

7. Reaction Types: Chemical reactions can be classified into different types, such as synthesis, decomposition, displacement, and redox reactions. 

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### Global Context 

- Globalization and Sustainability: Chemical processes are vital for producing sustainable solutions to global challenges. Sustainable chemistry aims to minimize waste and use renewable resources, while chemical industries contribute to areas such as clean energy, food production, and environmental protection. 

### Key Concept 

- Change: In chemistry, change refers to the transformation that occurs when substances undergo chemical reactions, resulting in new substances with different properties. 

### Related Concept 

- Interactions: Interactions occur when atoms, molecules, or ions combine or react, leading to new products or changes in the structure and properties of matter. 

### Statement of Inquiry 

- The chemical industry can provide sustainable solutions through various changes brought about by the interactions of matter. 

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### UNIT CONTENT (Detailed) 

1. Chemical Reactions:  

   - Involves the rearrangement of atoms or molecules during a reaction. 

   - Examples include combustion, rusting, fermentation, and photosynthesis. 

2. Valency and Chemical Formula (Criss-Cross Rule): 

   - Valency: The number of electrons an atom can gain, lose, or share to form bonds.  

   - Criss-Cross Rule: Used to write chemical formulas for ionic compounds. The valency of one ion is crossed over to become the subscript of the other ion. 

     - Example: For Na (Valency 1) and Cl (Valency 1), the formula is NaCl. 

3. Balancing Chemical Equations: 

   - Chemical equations must be balanced to follow the law of conservation of mass, meaning the number of atoms on the reactant side must equal the number on the product side. 

     - Example: Unbalanced: \( H_2 + O_2 \rightarrow H_2O \) 

     - Balanced: \( 2H_2 + O_2 \rightarrow 2H_2O \) 

4. Physical and Chemical Change: 

   - Physical Changes: Do not involve the formation of new substances. Examples: melting, freezing, dissolving. 

   - Chemical Changes: Involve the creation of new substances. Examples: rusting of iron, combustion, and digestion. 

5. Acids, Bases, and Salts: 

   - Acids: Substances that release hydrogen ions (H⁺) in water. 

   - Bases: Substances that release hydroxide ions (OH⁻) in water. 

   - Salts: Formed when acids and bases react. Example: NaCl (sodium chloride) from NaOH (sodium hydroxide) and HCl (hydrochloric acid). 

6. Applications of Acids, Bases, and Salts: 

   - Acids: Used in cleaning products, batteries, and food preservation. 

   - Bases: Used in soaps, detergents, and as antacids. 

   - Salts: Essential for human nutrition, food preservation, and industrial processes. 

7. Types of Chemical Reactions: 

   - Synthesis: Two or more substances combine to form a new compound (e.g., A + B → AB). 

   - Decomposition: A compound breaks down into simpler substances (e.g., AB → A + B). 

   - Single Displacement: One element replaces another in a compound (e.g., A + BC → AC + B). 

   - Double Displacement: Two compounds exchange ions to form new compounds (e.g., AB + CD → AD + CB). 

   - Redox Reactions: Involve the transfer of electrons between substances (oxidation and reduction). 

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### Ions and Cations 

- Cations: Positively charged ions formed when an atom loses electrons. 

- Anions: Negatively charged ions formed when an atom gains electrons. 

#### Examples of Common Cations and Anions: 

- Cations:  

  - Na⁺ (Sodium ion) 

  - Ca²⁺ (Calcium ion) 

  - Fe²⁺ (Iron(II) ion) 

  - K⁺ (Potassium ion) 

- Anions:  

  - Cl⁻ (Chloride ion) 

  - SO₄²⁻ (Sulfate ion) 

  - NO₃⁻ (Nitrate ion) 

  - OH⁻ (Hydroxide ion) 

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• | Element | Symbol | Atomic Mass | Valency | Electronic Configuration | 

• |------------     -|------------|-----------------|-------------|-----------------------------| 

• | Hydrogen    | H          | 1.008           | 1           | 1s¹                        | 

• | Carbon        | C          | 12.011          | 4           | 1s² 2s² 2p²                 | 

• | Oxygen        | O          | 15.999          | 2           | 1s² 2s² 2p⁴                 | 

• | Nitrogen       | N          | 14.007          | 3           | 1s² 2s² 2p³                 | 

• | Sodium        | Na         | 22.990          | 1           | 1s² 2s² 2p⁶ 3s¹             | 

• | Chlorine       | Cl         | 35.45           | 1           | 1s² 2s² 2p⁶ 3s² 3p⁵         | 

• | Potassium   | K          | 39.098          | 1           | 1s² 2s² 2p⁶ 3s² 3p⁶ 4s¹     | 

• | Calcium       | Ca         | 40.078          | 2           | 1s² 2s² 2p⁶ 3s² 3p⁶ 4s²     | 

• | Iron              | Fe         | 55.845          | 2, 3        | [Ar] 3d⁶ 4s²                 | 

• | Sulfur           | S          | 32.065          | 2           | 1s² 2s² 2p⁶ 3s² 3p⁴         | 

• | Phosphorus | P          | 30.974          | 3, 5        | 1s² 2s² 2p⁶ 3s² 3p³         | 

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Chemical Reactions and Related Concepts 

This note provides a comprehensive overview of the unit concept focusing on chemical reactions, valency, equations, changes, acids and bases, applications, and reaction types. It also explores the global context of globalization and sustainability, emphasizing the key concept of change and the related concept of interactions. 

Unit Content 

• Chemical Reactions: The process in which substances (reactants) undergo a transformation to form new substances (products). 

• Valency and Chemical Formula: Valency refers to the combining capacity of an element, often determined by the number of electrons in its outer shell. The criss-cross rule is used to determine the formula of ionic compounds. 

• Balancing Chemical Equations: The process of ensuring that the number of atoms for each element is the same on both sides of a chemical equation. 

• Physical and Chemical Change: Physical changes affect the form of a chemical substance, while chemical changes result in the formation of new substances. 

• Acids, Bases, and Salts: Acids are substances that donate protons (H+ ions), bases accept protons, and salts are formed from the neutralization reaction between an acid and a base. 

• Applications of Acids, Bases, and Salts: These substances have various applications in industries, laboratories, and everyday life. 

• Types of Chemical Reactions: Includes synthesis, decomposition, single replacement, double replacement, and combustion reactions. 

Global Context 

The unit emphasizes the importance of globalization and sustainability in the chemical industry. The statement of inquiry highlights how the chemical industry can provide sustainable solutions through various changes brought about by the interactions of matter. 

Cations and Ions 

Cations are positively charged ions formed when an atom loses one or more electrons. Anions are negatively charged ions formed when an atom gains electrons. The periodic table lists elements along with their symbols, atomic mass, electronic configuration, and valency. 

Periodic Table Overview 

Element Symbol Atomic Mass Valency Electronic Configuration Hydrogen H 1.008 1 1s1 Helium He 4.0026 0 1s2 Lithium Li 6.94 1 [He] 2s1 Beryllium Be 9.0122 2 [He] 2s2 Boron B 10.81 3 [He] 2s2 2p1 

symbols of the cation (positive ion) and anion (negative ion). 

• Determine the valency of each ion. 

• Cross the valencies to become the subscripts of the other ion. 

• Simplify the subscripts if necessary. 

Balancing Chemical Equations 

To balance a chemical equation, follow these steps: 

1. Write the unbalanced equation. 

2. Count the number of atoms of each element on both sides. 

3. Add coefficients to balance the number of atoms for each element. 

4. Ensure that the coefficients are in the simplest ratio. 

5. Double-check to confirm that the equation is balanced. 

This comprehensive note serves as a foundational guide to understanding chemical reactions, their applications, and the principles governing them. 

Periodic Table Elements and Their Properties 

The periodic table consists of 118 known elements, each with unique properties, including their symbols, valence, electronic configurations, electron masses, cation lists, and anion lists. Below is a comprehensive overview of these elements and their characteristics. 

Elements Overview 

• Symbol: The one or two-letter abbreviation for each element. 

• Valence: The combining capacity of an element, often determined by the number of electrons in the outer shell. 

• Electronic Configuration: The distribution of electrons in an atom's orbitals. 

• Electron Mass: The mass of an electron, approximately 9.109 x 10-31 kg. 

• Cations: Positively charged ions formed when an atom loses electrons. 

• Anions: Negatively charged ions formed when an atom gains electrons. 

Sample Elements 

Here are a few examples of elements from the periodic table along with their properties: 

• Hydrogen (H) 

• Valence: 1 

• Electronic Configuration: 1s1 

• Cations: H+ 

• Anions: None 

• Oxygen (O) 

• Valence: 2 

• Electronic Configuration: 1s2 2s2 2p4 

• Cations: None 

• Anions: O2- 

• Sodium (Na) 

• Valence: 1 

• Electronic Configuration: 1s2 2s2 2p6 3s1 

• Cations: Na+ 

• Anions: None 

• Chlorine (Cl) 

• Valence: 1 

• Electronic Configuration: 1s2 2s2 2p6 3s2 3p5 

• Cations: None 

• Anions: Cl- 

hemical Reactions & Valency

Chemical reactions involve the transformation of substances into new products

Valency represents the combining capacity of atoms with other elements

The criss-cross rule helps determine chemical formulas by exchanging valencies

Understanding valency is crucial for writing correct chemical formulas Key concepts include:

Reactants and products

Conservation of mass

Proper formula writing

Element combinations

Physical & Chemical Changes

Physical changes alter appearance without changing substance identity

Chemical changes create new substances with different properties

Examples include:

Physical: melting, freezing, evaporation

Chemical: rusting, burning, digestion Change indicators include:

Color changes

Gas formation

Temperature changes

Precipitate formation

Acids, Bases & Salts

Acids are substances that donate hydrogen ions

Bases are substances that accept hydrogen ions

Salts form from acid-base neutralization reactions Common properties:

Acids taste sour, turn litmus red

Bases taste bitter, turn litmus blue

Salts are neutral compounds Applications include:

Food preservation

Cleaning products

Industrial processes

Types of Chemical Reactions

Combination/Synthesis reactions (A + B → AB)

Decomposition reactions (AB → A + B)

Single displacement (A + BC → AC + B)

Double displacement (AB + CD → AD + CB) Key features:

Mass conservation

Energy changes

Reaction conditions

Product formation