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Ionic equations and formulae

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Intros
Lessons
  1. Balancing ionic equations
  2. Metathesis reactions
  3. Ways to write a metathesis reaction equation.
  4. Writing net ionic equations.
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Examples
Lessons
  1. Write the products and balanced equations for metathesis reactions:
    Write the balanced equation (including state symbols) for the metathesis reaction between:
    1. AgNO3 reacting with NaBr
    2. CaCl2 reacting with K2CO3
    3. Na3PO4 reacting with MgSO4
      1. Write net ionic equations from descriptions of metathesis reactions.:
        Write the net ionic equation for the metathesis reaction between:
        1. Pb(NO3)2 reacting with CuSO4
        2. MgCl2 reacting with Na2CO3
        3. CuCl2 reacting with K3PO4
      Topic Notes
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      Introduction to Ionic Equations and Formulae

      Welcome to the fascinating world of ionic equations and formulae! These concepts are essential in understanding chemical reactions and the behavior of ions in solution. Our introduction video serves as a perfect starting point, offering a clear and concise explanation of these fundamental ideas. As we dive into this topic, you'll discover how ionic equations help us visualize the actual particles involved in reactions, while formulae provide a shorthand way to represent compounds. The video will guide you through the basics, making it easier to grasp these sometimes challenging concepts. Remember, mastering ionic equations and formulae is crucial for success in chemistry, so pay close attention! Don't worry if it seems complex at first with practice and patience, you'll soon become comfortable working with these important tools. Let's begin this exciting journey together, exploring the world of ions and their interactions!

      Understanding Metathesis Reactions

      Metathesis reactions, also known as double replacement reactions, are a fundamental concept in chemistry that involves the exchange of ions between two compounds. These reactions are essential to understand as they occur frequently in various chemical processes and have numerous applications in industry and everyday life.

      To comprehend metathesis reactions, it's crucial to first understand what a salt is. A salt is an ionic compound formed by the neutralization reaction between an acid and a base. It consists of a positively charged cation and a negatively charged anion. Common examples include sodium chloride (table salt) and potassium nitrate.

      In a metathesis reaction, two compounds exchange their ions to form two new compounds. The general formula for a metathesis reaction is:

      AB + CD AD + CB

      Where A and C are cations, while B and D are anions. To identify a metathesis reaction, look for two reactants that are both ionic compounds and result in two new ionic compounds as products.

      Balancing equations for metathesis reactions is crucial to ensure that the law of conservation of mass is followed. Here's a step-by-step guide to balancing these equations:

      1. Write the correct formulas for all reactants and products.
      2. Count the number of atoms of each element on both sides of the equation.
      3. Add coefficients in front of compounds to balance the number of atoms.
      4. Double-check that all elements are balanced on both sides.

      For example, let's balance the equation for the reaction between silver nitrate and sodium chloride:

      AgNO + NaCl AgCl + NaNO

      In this case, the equation is already balanced as there is an equal number of atoms on both sides.

      Predicting product formulas in metathesis reactions involves understanding the charges of ions and how they combine. Follow these steps:

      1. Identify the ions present in the reactants.
      2. Determine which ions will combine in the products.
      3. Write the formulas of the new compounds, ensuring charge balance.

      For instance, in the reaction between barium chloride and sodium sulfate:

      BaCl + NaSO BaSO + 2NaCl

      The barium ion (Ba²) combines with the sulfate ion (SO²) to form barium sulfate, while the sodium ions (Na) combine with the chloride ions (Cl) to form sodium chloride.

      It's important to note that not all combinations of ionic compounds will result in a metathesis reaction. Some key factors that determine whether a metathesis reaction will occur include:

      • The solubility of the products
      • The formation of a gas
      • The formation of a weak electrolyte or molecular compound

      Understanding these factors helps predict whether a reaction will proceed and what products will form. For example, if one of the potential products is insoluble in water, it will likely precipitate out of solution, driving the reaction forward.

      Metathesis reactions have numerous practical applications, including water treatment, qualitative analysis in chemistry labs, and the production of various industrial chemicals. By mastering the concepts of metathesis reactions, balancing equations, and predicting product formulas, students can develop a strong foundation for more advanced chemical concepts and problem-solving skills in chemistry.

      Writing Full Molecular Equations

      Writing full molecular equations for ionic reactions is a crucial skill in chemistry that requires attention to detail and a solid understanding of chemical principles. This process involves determining the correct formulas for reactants and products, and then balancing the equation to ensure conservation of mass. Let's explore this step-by-step, emphasizing the importance of maintaining neutrality in ionic compounds.

      Step 1: Identify the reactants and products. In an ionic reaction, you'll typically have two ionic compounds reacting to form two new ionic compounds. It's essential to recognize the ions involved in the reaction.

      Step 2: Write the correct formulas for each compound. For ionic compounds, ensure that the overall charge is neutral. This means the positive charges from cations must balance the negative charges from anions. For example, in sodium chloride (NaCl), the Na+ ion balances the Cl- ion.

      Step 3: Write the initial equation using the full molecular formulas. At this stage, don't worry about balancing; focus on getting the correct formulas for all compounds.

      Step 4: Balance the equation. Adjust the coefficients in front of each compound to ensure that the number of atoms of each element is the same on both sides of the equation. Remember, you can't change subscripts in formulas as this would alter the compound's identity.

      Step 5: Double-check that the equation is balanced and that all ionic compounds are neutral.

      Let's walk through an example to illustrate this process:

      Suppose we want to write the full molecular equation for the reaction between aqueous solutions of silver nitrate and sodium chloride.

      Step 1: Identify reactants and products
      Reactants: Silver nitrate (AgNO3) and sodium chloride (NaCl)
      Products: Silver chloride (AgCl) and sodium nitrate (NaNO3)

      Step 2: Write correct formulas
      AgNO3, NaCl, AgCl, NaNO3 (all are already neutral)

      Step 3: Write initial equation
      AgNO3 + NaCl AgCl + NaNO3

      Step 4: Balance the equation
      In this case, the equation is already balanced as there's one of each atom on both sides.

      Step 5: Final check
      AgNO3 + NaCl AgCl + NaNO3
      The equation is balanced, and all compounds are neutral.

      Maintaining neutrality in ionic compounds is crucial because it reflects the fundamental nature of ionic bonding. In nature, large-scale separation of charges is energetically unfavorable. By ensuring neutrality, we accurately represent the stable forms of ionic compounds as they exist in reactions.

      Remember, when writing full molecular equations for ionic reactions, always start by identifying the ions involved, write out the full formulas of compounds ensuring neutrality, and then balance the equation. This methodical approach will help you accurately represent ionic reactions in their full molecular form.

      Full Ionic Equations

      Full ionic equations are a crucial concept in chemistry that provide a more detailed representation of chemical reactions compared to molecular equations. These equations show the complete dissociation of ionic compounds in aqueous solutions, offering a comprehensive view of all species present in a reaction. Understanding how to write full ionic equations is essential for grasping the intricacies of chemical reactions, particularly those involving aqueous solutions and precipitates.

      To write a full ionic equation, we start with a molecular equation and then break down the ionic compounds into their constituent ions. This process involves recognizing which compounds are soluble and will dissociate in water. Compounds that are soluble in water exist in an aqueous state, denoted by (aq) after the formula. In contrast, insoluble compounds form precipitates, indicated by (s) for solid.

      Aqueous states are crucial in full ionic equations as they represent the dissociation of compounds into ions. For example, when sodium chloride (NaCl) is dissolved in water, it separates into Na+ and Cl- ions. This dissociation is represented in the full ionic equation, showing each ion as a separate entity in the solution.

      Precipitates, on the other hand, are insoluble products formed when certain ions combine in a solution. These are represented as solid compounds in full ionic equations and do not dissociate further. Recognizing which compounds form precipitates is key to accurately writing these equations.

      An important concept in full ionic equations is that of spectator ions. These are ions that remain unchanged throughout the reaction and appear on both sides of the equation. Identifying spectator ions is crucial as they can be canceled out in the net ionic equation, which focuses only on the species that actively participate in the reaction.

      Let's walk through an example to illustrate the transition from a molecular equation to a full ionic equation:

      Consider the reaction between silver nitrate and sodium chloride:

      Molecular equation: AgNO3 (aq) + NaCl (aq) AgCl (s) + NaNO3 (aq)

      To convert this to a full ionic equation, we dissociate the aqueous compounds:

      Full ionic equation: Ag+ (aq) + NO3- (aq) + Na+ (aq) + Cl- (aq) AgCl (s) + Na+ (aq) + NO3- (aq)

      In this full ionic equation, we can see that Na+ and NO3- appear on both sides unchanged. These are the spectator ions. AgCl is the precipitate formed and remains as a solid compound.

      Writing full ionic equations requires a solid understanding of solubility rules and the behavior of ions in aqueous solutions. It's important to remember that only strong electrolytes (like strong acids, strong bases, and soluble ionic compounds) should be fully dissociated in these equations. Weak electrolytes and nonelectrolytes are typically left in their molecular form.

      Practicing with various reactions and becoming familiar with common ionic compounds will improve your ability to write these equations accurately. Full ionic equations provide a more complete picture of chemical reactions, helping to visualize the actual species present in solution and the formation of precipitates. This deeper understanding is invaluable in fields such as analytical chemistry, environmental science, and chemical engineering.

      Net Ionic Equations

      Net ionic equations are a crucial concept in chemistry that provide a simplified representation of chemical reactions in aqueous solutions. Unlike full ionic equations, which show all ions present in a reaction, net ionic equations focus solely on the species that undergo a chemical transformation. This concise approach allows chemists to highlight the essential components of a reaction and better understand the underlying chemical processes.

      The key difference between net ionic equations and full ionic equations lies in the treatment of spectator ions. Spectator ions are ions that remain unchanged throughout the reaction and do not participate in the chemical transformation. In a net ionic equation, these spectator ions are omitted, leaving only the reactive species. This simplification helps chemists concentrate on the actual chemical change taking place.

      Identifying and removing spectator ions is crucial for several reasons. Firstly, it streamlines the equation, making it easier to interpret and analyze. Secondly, it emphasizes the true nature of the reaction by focusing on the species that actually undergo change. Lastly, it allows for a more accurate prediction of reaction outcomes and products.

      To write a net ionic equation from a full ionic equation, follow these steps:

      1. Write the balanced molecular equation for the reaction.
      2. Dissociate all strong electrolytes (strong acids, strong bases, and soluble ionic compounds) into their constituent ions.
      3. Identify the spectator ions by comparing the reactant and product sides of the equation.
      4. Cancel out the spectator ions on both sides of the equation.
      5. Write the remaining ions and molecules as the net ionic equation.

      Let's illustrate this process with an example:

      Consider the reaction between silver nitrate and sodium chloride:

      AgNO3 (aq) + NaCl (aq) AgCl (s) + NaNO3 (aq)

      Step 1: This is already the balanced molecular equation.

      Step 2: Dissociate the strong electrolytes:

      Ag+ (aq) + NO3- (aq) + Na+ (aq) + Cl- (aq) AgCl (s) + Na+ (aq) + NO3- (aq)

      Step 3 & 4: Identify and cancel out spectator ions (Na+ and NO3-):

      Ag+ (aq) + Cl- (aq) AgCl (s)

      Step 5: This is the net ionic equation, showing only the species involved in the chemical transformation.

      By mastering net ionic equations, chemists can more effectively analyze and predict the outcomes of chemical reactions in aqueous solutions, focusing on the essential chemical transformations while disregarding the non-reactive spectator ions.

      Practical Applications and Problem Solving

      Ionic equations play a crucial role in various chemical processes and have numerous practical applications in both industry and everyday life. Understanding how to write and balance these equations is essential for chemists, engineers, and students alike. In this section, we'll explore the practical applications of ionic equations, problem-solving strategies, and provide practice problems with step-by-step solutions to reinforce your understanding.

      Practical Applications of Ionic Equations

      1. Water Treatment: Ionic equations are used to understand and optimize water purification processes. For example, the removal of hard water ions through ion exchange can be represented by ionic equations.

      2. Battery Technology: The chemical reactions in batteries, such as lead-acid batteries used in cars, can be described using ionic equations. This helps in understanding and improving battery performance.

      3. Corrosion Prevention: Ionic equations help explain the process of metal corrosion and guide the development of corrosion prevention techniques.

      4. Environmental Science: Ionic equations are used to study and mitigate acid rain effects, as well as understand the chemistry of ocean acidification.

      Problem-Solving Strategies

      When writing and balancing ionic equations, follow these steps:

      1. Write the balanced molecular equation.
      2. Break down the compounds into their constituent ions.
      3. Identify and cancel out spectator ions.
      4. Balance the remaining ions and charges.

      Practice Problems

      Problem 1: Write the net ionic equation for the reaction between silver nitrate and sodium chloride.

      Solution:

      1. Molecular equation: AgNO + NaCl AgCl + NaNO
      2. Ionic breakdown: Ag + NO + Na + Cl AgCl + Na + NO
      3. Cancel spectator ions (Na and NO)
      4. Net ionic equation: Ag + Cl AgCl

      Problem 2: Balance the following ionic equation: Fe³ + I Fe² + I

      Solution:

      1. Identify the changes in oxidation states: Fe³ is reduced to Fe², I is oxidized to I
      2. Balance the electron transfer: 2Fe³ + 2I 2Fe² + I
      3. Verify charge balance: (+6) + (-2) = (+4) + (0)

      Real-World Examples

      1. Swimming Pool Maintenance: The addition of chlorine to pool water can be represented by the ionic equation: Cl + HO HOCl + H + Cl. This helps pool owners understand the chemistry behind water treatment.

      2. Antacid Action: The neutralization of stomach acid by antacids can be described using ionic equations. For example, Mg(OH) + 2H Mg² + 2HO shows how magnesium hydroxide neutralizes excess stomach acid.

      3. Soil pH Adjustment: Farmers use ionic equations to understand how lime (CaCO) neutralizes acidic soil: CaCO + 2H Ca² + HO + CO

      4. Wastewater Treatment: The precipitation of heavy metals in wastewater treatment can be

      Conclusion

      In summary, this article has delved into the crucial aspects of ionic equations and formulae, providing a comprehensive overview of these fundamental chemical concepts. We've explored the key points, including the formation of ions, balancing ionic equations, and understanding spectator ions. The introduction video for ionic equations serves as an invaluable resource, offering a visual and interactive approach to grasping these sometimes challenging ideas. By watching and engaging with the video, learners can reinforce their understanding and see these concepts in action. To further your knowledge and proficiency in ionic equations and formulae, we encourage you to explore additional resources, practice problems for ionic equations, and engage in hands-on experiments. Remember, mastering these concepts is essential for success in chemistry and related fields. Continue to challenge yourself, ask questions, and apply what you've learned to real-world applications of ionic equations. Your journey in understanding ionic equations and formulae is just beginning, and the possibilities for further exploration are endless.

      Balancing ionic equations is a skill that can be honed with practice. The introduction video for ionic equations provides a solid foundation for beginners. Additionally, practice problems for ionic equations are available to test your knowledge. Real-world applications of ionic equations demonstrate their importance in various fields.

      Balancing Ionic Equations and Metathesis Reactions

      Balancing ionic equations Metathesis reactions

      Step 1: Understanding Metathesis Reactions

      Metathesis reactions, also known as double replacement reactions, occur when two salts react in solution to form new products. These reactions involve the exchange of ions between the reactants. A salt, in general terms, is any compound composed of two oppositely charged ions or groups that dissolve in solution in a ratio that makes the compound neutral overall. For example, when potassium phosphate (K3PO4) reacts with calcium sulfide (CaS), the ions involved are K+, Ca2+, S2-, and PO43-.

      Step 2: Identifying the Ions and Their Charges

      To balance the ionic equation, it is crucial to identify the charges of the ions involved. For instance, potassium (K) is in group 1 of the periodic table and forms a K+ ion. Phosphate (PO4) is a polyatomic ion with a 3- charge (PO43-). Calcium (Ca) is in group 2 and forms a Ca2+ ion, while sulfide (S) forms an S2- ion. Understanding these charges helps in predicting the products of the reaction.

      Step 3: Predicting the Products

      In a metathesis reaction, the ions exchange partners. For example, when potassium phosphate reacts with calcium sulfide, the potassium ions (K+) will pair with the sulfide ions (S2-), and the calcium ions (Ca2+) will pair with the phosphate ions (PO43-). This results in the formation of potassium sulfide (K2S) and calcium phosphate (Ca3(PO4)2).

      Step 4: Writing the Unbalanced Equation

      The unbalanced equation for the reaction between potassium phosphate and calcium sulfide is:
      K3PO4 + CaS K2S + Ca3(PO4)2
      At this stage, the equation is not balanced because the number of atoms of each element on the reactant side does not equal the number on the product side.

      Step 5: Balancing the Equation

      To balance the equation, we need to ensure that the number of atoms of each element is the same on both sides. Start by balancing the polyatomic ions as a whole unit if they appear unchanged on both sides of the equation. For example, balance the phosphate (PO4) groups first. In the products, there are two phosphate groups, so we need two phosphate groups in the reactants:
      2 K3PO4 + CaS K2S + Ca3(PO4)2
      Next, balance the calcium atoms. There are three calcium atoms in the products, so we need three calcium atoms in the reactants:
      2 K3PO4 + 3 CaS K2S + Ca3(PO4)2
      Finally, balance the potassium and sulfur atoms. There are six potassium atoms in the reactants (2 K3PO4), so we need six potassium atoms in the products:
      2 K3PO4 + 3 CaS 3 K2S + Ca3(PO4)2

      Step 6: Verifying the Balanced Equation

      Verify that the equation is balanced by counting the number of atoms of each element on both sides. The balanced equation should have the same number of each type of atom on both sides:
      Reactants: 6 K, 2 PO4, 3 Ca, 3 S
      Products: 6 K, 2 PO4, 3 Ca, 3 S
      The equation is now balanced.

      Step 7: Writing the Net Ionic Equation

      To write the net ionic equation, we need to show only the ions that participate in the reaction. Spectator ions, which do not change during the reaction, are omitted. For the reaction between potassium phosphate and calcium sulfide, the net ionic equation focuses on the formation of the precipitate (calcium phosphate):
      3 Ca2+ (aq) + 2 PO43- (aq) Ca3(PO4)2 (s)
      This net ionic equation shows the formation of the insoluble product, calcium phosphate, from the calcium and phosphate ions in solution.

      FAQs

      1. What is the difference between a full ionic equation and a net ionic equation?

        A full ionic equation shows all ions present in a reaction, including spectator ions. A net ionic equation, on the other hand, only includes the ions and molecules that actively participate in the reaction, omitting spectator ions. Net ionic equations provide a simplified view of the essential chemical changes occurring in a reaction.

      2. How do you identify spectator ions in an ionic equation?

        Spectator ions are ions that appear unchanged on both sides of the equation. To identify them, compare the ions present in the reactants and products. Any ions that remain in the same form on both sides are spectator ions. These ions do not participate in the chemical reaction and can be canceled out when writing a net ionic equation.

      3. Why is it important to balance ionic equations?

        Balancing ionic equations is crucial to ensure that the law of conservation of mass is followed. It ensures that the number of atoms and the total charge are equal on both sides of the equation. Balanced equations accurately represent the stoichiometry of the reaction and are essential for quantitative analysis and predictions in chemistry.

      4. What are some common applications of ionic equations in everyday life?

        Ionic equations have numerous practical applications, including water treatment processes, understanding battery chemistry, explaining metal corrosion, and analyzing environmental issues like acid rain. They are also used in swimming pool maintenance, antacid action in the stomach, soil pH adjustment in agriculture, and wastewater treatment.

      5. How can I improve my skills in writing and balancing ionic equations?

        To improve your skills, practice regularly with a variety of problems. Start by writing molecular equations, then convert them to full ionic equations, and finally to net ionic equations. Familiarize yourself with solubility rules and common ion charges. Use online resources, textbooks, and practice problems to test your understanding. Additionally, try to relate the equations to real-world applications to better grasp their significance.

      Prerequisite Topics for Ionic Equations and Formulae

      Understanding ionic equations and formulae is a crucial aspect of chemistry, but to truly grasp this concept, it's essential to have a solid foundation in certain prerequisite topics. Two key areas that serve as building blocks for mastering ionic equations and formulae are the introduction to chemical reactions and balancing chemical equations.

      Let's start with the importance of understanding chemical reactions. This fundamental concept is crucial because ionic equations are essentially a more detailed representation of chemical reactions involving ions. By grasping the basics of how substances interact and transform during a reaction, students can better comprehend the behavior of ions in solution and how they participate in chemical processes. The chemical reactions visualization techniques learned in this prerequisite topic help in mentally picturing the movement and interactions of ions, which is invaluable when working with ionic equations.

      Moving on to the second prerequisite, balancing chemical equations is absolutely critical for working with ionic equations and formulae. This skill ensures that the law of conservation of mass is upheld in chemical reactions, including those involving ions. When dealing with ionic equations, the ability to balance charges becomes just as important as balancing atoms. The techniques learned in balancing chemical equations provide a strong foundation for this more advanced balancing act.

      The relationship between these prerequisites and ionic equations is clear when we consider the process of writing and interpreting ionic equations. Students must first identify the reactants and products, much like in basic chemical reactions. Then, they need to apply their balancing skills to ensure that both mass and charge are conserved. Finally, understanding how to visualize these reactions helps in distinguishing between spectator ions and those actively participating in the reaction.

      By mastering these prerequisite topics, students build a strong conceptual framework that makes learning ionic equations and formulae much more manageable. The skills developed in understanding chemical reactions and balancing equations serve as a bridge to more complex ionic concepts. They provide the necessary tools to analyze, interpret, and predict the behavior of ions in various chemical contexts.

      In conclusion, a solid grasp of these prerequisite topics is not just helpful but essential for success in understanding ionic equations and formulae. By investing time in mastering these foundational concepts, students set themselves up for a deeper, more intuitive understanding of ionic chemistry, paving the way for success in more advanced chemical studies.

      In this lesson, we will learn:

      • To recall the definition of a metathesis (double replacement) reaction.
      • Different methods to write metathesis reactions involving precipitate products.
      • How to construct balanced net ionic equations from full formula equations.

      Notes:

      • Recall that when ionic species react, salts are produced. If two salts react, a metathesis reaction occurs. This is also known as a double replacement reaction.
        • You can spot these reactions; look for two salts as the reactants. Salts can be spotted by using a table of common ions and charges. Most chemistry textbooks have back page for this; a salt has two oppositely charged ions or groups in a ratio that makes the compound neutral overall.
          For example the reaction of potassium phosphate, K3PO4 and calcium sulfide, CaS:
          • The potassium ion has a single positive charge (formula K+) and the phosphate ion has a 3- charge (formula PO43-). To balance, the formula of potassium phosphate is K3PO4 to give an overall neutral compound.
          • The calcium ion has a double positive charge (formula Ca2+) and the sulfide ion has a double negative charge (formula S2-). As such, the formula of calcium sulfide is CaS which gives an overall neutral compound.
          So four ions that make up the two salts have been identified: K+, Ca2+, S2- and OH-. In a metathesis reaction, ions are exchanged between the two salts reacting together. The products can be predicted by swapping the anions:

          K3PO4 + CaS \enspace → \enspace K S + CaPO4


          As with before, the formula of the molecule will allow charges to balance and give a neutral molecule. To find this formula you can ‘cross’ the charges of the ions that make the compound.

          With the formulae found, we just need to balance the equation now.
          When balancing you can treat polyatomic ions as one combined entity; counting the individual atoms in the ions isn’t necessary as the ratio of atoms within the group should not change when balancing equations anyway:

          K3PO4 + CaS \enspace → \enspace K2 S + Ca3(PO4)2


          There are 3 Ca atoms in the products to 1 in the reactants, and 2 PO4 groups in the products to 1 in the reactants. Balancing for these:

          2K3PO4 + 3CaS \enspace → \enspace K2 S + Ca3(PO4)2


          There are now 6 K atoms in the products to 2 in the reactants and 3 S atoms in the reactants to 1 in the products.
          Balancing for these gives the full equation:

          2K3PO4 + 3CaS \enspace → \enspace 3K2 S + Ca3(PO4)2
      • When metathesis reactions occur, sometimes one of the products formed is an insoluble solid, and comes out of solution. This is called a precipitate. In a real chemistry experiment spotting a precipitate is easy because the solution turns cloudy; the precipitate is blocking light passing through the solution. Because metathesis reactions normally use solutions, we assume the reactants and products are aqueous so if a precipitate is formed, you MUST make it clear with an (s) state symbol. There are a few ways to write metathesis reaction equations:
        • A formula equation, or full equation, involves writing all reactants and products of the reaction in their neutral molecular form. This is the normal way of writing an equation, like we did above with K3PO4 and CaS reacting.

        • A full ionic equation is written by displaying all the dissolved species – the dissolved ions! Full ionic equations include spectator ions; these are the ions still in an aqueous state in the products (which did not react). For example in the reaction with silver nitrate, AgNO3 and sodium chloride, NaCl.
          We assume aqueous state unless given otherwise:

          Ag+ + NO3- + Na+ + Cl- \enspace → \enspace AgCl(s) + Na+ + Cl-

        • A net ionic equation is an ionic equation where only the reacting ionic species are included; spectator ions are ignored and stoichiometry is in its simplified form. This is a simplified version of the equation that can be written after the balanced full equation has been determined.

          Ag+ + Cl- \enspace → \enspace AgCl(s)