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    Chemistry 101 for Teens

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    • Introduction to Chemistry
      • 1.1Overview of Chemistry
      • 1.2Importance of Chemistry
      • 1.3Branches of Chemistry
    • The Periodic Table
      • 2.1History of the Periodic Table
      • 2.2Major Groups of the Periodic Table
      • 2.3Periods and Groups
    • Atomic Structure
      • 3.1Atomic Theory
      • 3.2Atomic Components
      • 3.3Atomic Models
    • Chemical Bonding
      • 4.1Ionic Bonds
      • 4.2Covalent Bonds
      • 4.3Metallic Bonds
    • Chemical Reactions
      • 5.1Reaction Types
      • 5.2Balancing Equations
      • 5.3Stoichiometry
    • Solutions and Solubility
      • 6.1Types of Solutions
      • 6.2Solubility Rules
      • 6.3Concentration Calculations
    • Acids, Bases, and pH
      • 7.1Defining Acids and Bases
      • 7.2Acid-Base Reactions
      • 7.3pH and pOH
    • Energy in Chemistry
      • 8.1Endothermic and Exothermic Reactions
      • 8.2Thermodynamics
      • 8.3Energy and Chemical Change
    • The Gas Laws
      • 9.1Boyle's Law and Charles' Law
      • 9.2The Ideal Gas Law
      • 9.3Real Gases
    • Organic Chemistry Basics
      • 10.1Introduction to Organic Chemistry
      • 10.2Carbon and Hydrocarbons
      • 10.3Functional Groups
    • Nuclear Chemistry
      • 11.1Radioactivity
      • 11.2Nuclear Equations
      • 11.3Applications of Nuclear Chemistry
    • Biochemistry Basics
      • 12.1Introduction to Biochemistry
      • 12.2Proteins, Carbohydrates, and Lipids
      • 12.3Nucleic Acids
    • Chemistry in Our Daily Life
      • 13.1Household Chemistry
      • 13.2Chemistry in Industry
      • 13.3Environmental Chemistry

    Chemical Reactions

    Balancing Chemical Equations

    scientific law that a closed system's mass remains constant

    Scientific law that a closed system's mass remains constant.

    Balancing chemical equations is a fundamental concept in chemistry that illustrates the law of conservation of mass. This law states that matter cannot be created or destroyed, only transformed. In the context of chemical reactions, this means that the number of atoms for each element must be the same on both sides of the equation.

    Understanding Chemical Equations

    A chemical equation represents a chemical reaction. It includes the reactants (substances that are combined or broken apart) on the left side and the products (new substances formed) on the right side. The two sides are separated by an arrow (→) which indicates the direction of the reaction.

    For example, the chemical equation for the reaction of hydrogen and oxygen to form water is:

    2H2 + O2 → 2H2O

    This equation tells us that two molecules of hydrogen (H2) react with one molecule of oxygen (O2) to form two molecules of water (H2O).

    Steps to Balance a Chemical Equation

    Balancing a chemical equation involves adjusting the coefficients (the numbers in front of the chemical formulas) to ensure that the number of atoms for each element is the same on both sides of the equation.

    Here are the basic steps:

    1. Write the unbalanced equation, which includes the formulas of the reactants and products.
    2. Count the number of atoms for each element on both sides of the equation.
    3. Adjust the coefficients to balance the atoms for one element at a time. Start with an element that appears in only one compound on each side.
    4. After balancing the atoms for one element, move on to another element and repeat the process.
    5. Check your work. The number of atoms for each element should now be the same on both sides of the equation.

    Practice Problems on Balancing Chemical Equations

    To solidify your understanding, try balancing the following chemical equations:

    1. H2 + O2 → H2O
    2. CH4 + O2 → CO2 + H2O
    3. Fe + O2 → Fe2O3

    Remember, practice is key to mastering the skill of balancing chemical equations. It not only helps you understand the stoichiometry of reactions but also lays the foundation for further studies in chemistry.

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    Next up: Stoichiometry