Balancing Chemical Equations with Polyatomic Ions

Melissa Maribel
10 Sept 201804:00
EducationalLearning
32 Likes 10 Comments

TLDRIn this educational video, Melissa Maribel, a personal tutor, shares essential tips for effortlessly balancing chemical equations involving polyatomic ions. She demonstrates the process step-by-step, emphasizing the importance of keeping polyatomic ions intact and adjusting coefficients to ensure equal representation of elements on both sides. The video also addresses a common scenario where OH and H2O are on opposite sides, suggesting a change to HOH for easier balancing. By following these methods, viewers are encouraged to practice and stay determined in mastering the skill of chemical equation balancing.

Takeaways
  • 🔬 Keep polyatomic ions together if they are the same on both sides of the equation to simplify the balancing process.
  • 📝 List all single elements and polyatomic ions on each side in the same order to make it easier to count and compare quantities.
  • 📚 Pay attention to subscripts; they indicate the number of atoms or ions present, such as 2 irons or 3 sulfate ions (SO4).
  • 🌐 Understand the difference between polyatomic ions in parentheses (indicating multiple instances) and those not in parentheses (indicating a single instance).
  • 🧩 Start balancing the equation by addressing elements with the highest subscripts first, such as iron in iron hydroxide.
  • ⚖️ Balance each element and polyatomic ion one at a time, ensuring that the entire equation is balanced after each step.
  • 💧 When OH and H2O are on opposite sides of the equation, rewrite H2O as HOH to simplify the balancing process.
  • 🔄 After rewriting H2O as HOH, re-count and list all elements and polyatomic ions to ensure accurate balancing.
  • ✅ Always balance aluminum and sulfate (SO4) last, as they often require adjustments based on the balance of other elements.
  • 🛠️ Remember to balance individual elements of hydrogen or oxygen at the end of the process to achieve a fully balanced equation.
  • 💪 Stay determined and keep practicing; balancing chemical equations with polyatomic ions is a skill that improves with practice.
Q & A

  • What is the first tip Melissa Maribel gives for balancing chemical equations with polyatomic ions?

    -Keep polyatomic ions together if they are the same on both sides of the equation.

  • Why is it helpful to keep polyatomic ions together when balancing chemical equations?

    -It simplifies the balancing process by treating the polyatomic ion as a single unit rather than balancing each element individually.

  • How do you count the number of polyatomic ions in a compound with a subscript?

    -If the polyatomic ion is inside parentheses followed by a subscript, multiply the number of ions by the subscript.

  • In the example given, how many SO4 ions are on the reactant side if the subscript is 3?

    -There are three SO4 ions on the reactant side.

  • How do you balance the number of irons when there are two irons on the reactant side and only one on the product side?

    -Place a 2 in front of the entire compound containing iron on the product side.

  • What happens to the number of OH ions when you place a 2 in front of iron hydroxide on the product side?

    -The number of OH ions becomes 2 times 3, which equals six OH ions.

  • Why should you rewrite H2O as HOH when OH and H2O are on opposite sides of the equation?

    -Rewriting H2O as HOH makes it easier to balance the hydrogen and hydroxide ions separately.

  • How do you balance the aluminum atoms in the given example when there are two aluminum atoms on the product side and one on the reactant side?

    -Place a 2 in front of aluminum hydroxide on the reactant side.

  • What is the final step to balance the SO4 ions when you have three SO4 ions on the product side and one on the reactant side?

    -Place a 3 in front of H2SO4 on the reactant side.

  • What is Melissa Maribel's final advice for those learning to balance chemical equations?

    -Stay determined, and keep practicing more examples.

Outlines
00:00
🔍 Balancing Chemical Equations with Polyatomic Ions

This paragraph introduces a chemistry tutorial focused on simplifying the process of balancing chemical equations that include polyatomic ions. The speaker, Melissa Maribel, presents herself as a personal tutor and offers a step-by-step guide to balance equations efficiently. The key points involve keeping polyatomic ions intact when they are the same on both sides of the equation, listing all elements and ions in the same order for clarity, and counting each element or ion to determine the coefficients needed for balance. The example given illustrates the process of balancing an equation involving iron, potassium, sulfur, and hydroxide ions, emphasizing the importance of recognizing the number of polyatomic ions and adjusting the equation accordingly. The tutorial also addresses the special case of OH and H2O, suggesting a method to rewrite H2O as HOH for easier balancing.

Mindmap
Keywords
💡Balancing chemical equations
Balancing chemical equations is the process of ensuring that the number of atoms for each element is the same on both sides of a chemical reaction. This is crucial for adhering to the law of conservation of mass. In the video, this concept is the central theme, with the focus on how to balance equations that include polyatomic ions, such as SO4 and OH.
💡Polyatomic ions
Polyatomic ions are groups of atoms that act as a single charged unit in a chemical reaction. They are an integral part of the balancing process discussed in the video. For example, SO4 (sulfate) and OH (hydroxide) are kept together when they are the same on both sides of the equation, simplifying the balancing process.
💡Reactant
A reactant is a substance that participates in a chemical reaction and is consumed or transformed to form products. In the script, reactants are listed with their respective polyatomic ions and single elements to facilitate the balancing process.
💡Product
Products are the substances formed as a result of a chemical reaction. In the video, the script details how to balance the chemical equation so that the number of products matches the reactants, ensuring the equation is balanced.
💡Subscript
In chemistry, a subscript number indicates the quantity of atoms or groups of atoms in a molecule. The video script uses subscripts to denote the number of iron atoms or OH groups, which is essential for balancing the equation.
💡Parentheses
Parentheses in a chemical formula indicate the repetition of the enclosed group of atoms. In the script, the presence of parentheses around a polyatomic ion signifies that there is more than one of that ion, which is a key factor in balancing the equation.
💡Iron hydroxide
Iron hydroxide is a compound that contains iron and hydroxide ions. In the video, it is used as an example to illustrate the process of balancing the iron atoms on both sides of the chemical equation.
💡Potassium sulfate
Potassium sulfate is a compound consisting of potassium, sulfur, and oxygen. The script uses it to demonstrate how to balance the sulfate ions and potassium atoms in a chemical equation.
💡Potassium hydroxide
Potassium hydroxide is a strong base made of potassium and hydroxide ions. The video script uses it to explain how to balance the hydroxide ions and potassium atoms in the equation.
💡H2O to HOH
In the script, the tutor suggests rewriting H2O (water) as HOH to balance OH and H2O on opposite sides of the equation. This is a strategy to simplify the balancing process by ensuring that the number of hydrogen and hydroxide ions are equal.
💡Aluminum hydroxide
Aluminum hydroxide is a compound used in the script as an example to demonstrate the balancing of aluminum atoms. It illustrates the process of adjusting the coefficients in front of compounds to achieve a balanced equation.
💡H2SO4
H2SO4, or sulfuric acid, is used in the script to show how to balance the hydrogen and sulfate ions. It is an example of how individual elements can be balanced at the end of the process if they are not part of a polyatomic ion.
Highlights

Introduction to the process of balancing chemical equations with polyatomic ions by Melissa Maribel.

Tip 1: Keeping polyatomic ions together if they are the same on both sides of the equation.

Explanation of how to handle polyatomic ions like SO4 and OH when they are identical on both reactant and product sides.

Listing all single elements and polyatomic ions in the same order for easier balancing.

Counting elements and polyatomic ions, with special attention to subscripts and parentheses indicating multiples.

Balancing iron by adjusting the coefficient in front of the iron hydroxide compound.

Balancing SO4 by placing a coefficient of 3 in front of potassium sulfate.

Balancing K and OH by adjusting the coefficient in front of potassium hydroxide.

Tip 2: Changing H2O to HOH when OH and H2O are on opposite sides of the equation.

Rewriting the chemical equation with the new representation of water (HOH).

Counting and balancing aluminum hydroxide by placing a coefficient of 2 in front of it.

Balancing OHs on the product side by adjusting the coefficient in front of water (HOH).

Balancing individual elements of hydrogen or oxygen at the end of the process.

Final step of balancing the equation by adjusting the coefficient in front of H2SO4.

Achieving a balanced chemical equation through the application of the provided tips.

Encouragement to practice more examples and stay determined in the learning process.

Transcripts

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