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In the study of chemistry, chemical equations are used to represent the various chemical reactions that occur between substances. These equations serve as essential tools for understanding the nature and scope of these reactions. However, in some cases, the full balanced equation can be overwhelming and unnecessarily complex. This is where net ionic equations come into play. A net ionic equation focuses on the species that undergo a change in charge during the reaction, providing a simplified representation of the reaction. In this guide, we will explore the step-by-step process of writing a net ionic equation, enabling us to better understand and analyze chemical reactions.
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The net ionic equation is an important part of chemistry because it represents only the elements that are changed in a chemical reaction. They are most commonly used in oxidation-reduction reactions, exchange reactions, and acid-base neutralization reactions. [1] X Research Source There are three basic steps to writing a net ionic equation: balancing the molecular equation, converting it to a full ionic equation (according to how each substance exists in solution), and finally Write the net ionic equation.
Steps
Learn the components of the ionic equation
- Ionic compounds can be formed between metals and nonmetals, metals and polyatomic ions, or many polyatomic ions.
- If you’re not sure what a compound it is, you can find the elements in that compound on the periodic table. [4] X Research Sources
- Implement these rules in the order outlined below:
- All salts Na + , K + , and NH 4+ are soluble.
- All salts NO 3– , C 2 H 3 O 2– , ClO 3– , and ClO 4– are soluble.
- All salts Ag + , Pb 2+ , and Hg 22+ are soluble.
- All salts Cl – , Br – , and I – are soluble.
- All salts CO 32- , O 2- , S 2- , OH – , PO 43- , CrO 42- , Cr 2 O 72- , and SO 32- are soluble (with a few exceptions). .
- All SO 42- salts are soluble (except in a few cases).
- For example, in NaCl, Na is the positively charged cation because it is a metal, and Cl is the negatively charged anion because it is a nonmetal.
- If you are studying general chemistry it is often asked to memorize some common polyatomic ions.
- Some common polyatomic ions are CO 32- , NO 3– , NO 2– , SO 42- , SO 32- , ClO 4– and ClO 3– . [8] X Research Sources
- Also you can find many other ions in chemistry books or on the internet. [9] X Research Source
Write the net ionic equation
- Write the number of atoms that form each compound on both sides of the equation.
- Add coefficients before elements other than oxygen and hydrogen to balance each side.
- Hydrogen atom balance.
- Oxygen atom balance.
- Count the number of atoms on each side of the equation to make sure they are balanced.
- For example, Cr + NiCl 2 –> CrCl 3 + Ni is balanced to 2Cr + 3NiCl 2 –> 2CrCl 3 + 3Ni.
- If the state of the element is not provided, use the state found on the periodic table.
- If the compound is called a solution, you can write it as aqueous or ( dd ).
- If there is water in the equation, you must determine if the ionic compound is water soluble by using the solubility worksheet. [11] X Research Source If the solubility is high, the compound will be in the aqueous state ( dd ), if the solubility is low, the compound will be in the solid state ( r ).
- In the absence of water, the ionic compound is solid ( r ).
- If the problem is written as an acid or a base, then the compound is aqueous ( dd ).
- For example, 2Cr + 3NiCl 2 –> 2CrCl 3 + 3Ni. Elemental forms of Cr and Ni are in the solid state. NiCl 2 and CrCl 3 are ionic compounds, so they are aqueous. Rewrite the equation as: 2Cr ( r ) + 3NiCl 2( dd ) –> 2CrCl 3( dd ) + 3Ni ( r ) .
- Solids, liquids, gases, molecular compounds, ionic compounds with low solubility, polyatomic ions and weak acids will not dissociate.
- Ionic compounds with high solubility (use solubility worksheet) and strong acids will ionize 100% (HCl ( dd ) , HBr ( dd ) , HI ( dd ) , H 2 SO 4( dd ) , HClO 4( dd ) ) , and HNO 3( dd ) ). [12] X Research Source
- Note, although polyatomic ions do not dissociate further, if they are constituents of the compound they will dissociate from the compound.
- In this example, NiCl 2 dissociates into Ni 2+ and Cl – while CrCl 3 dissociates into Cr 3+ and Cl – .
- Ni has a charge of 2+ because Cl has a charge of negative one but has 2 atoms. So we have to balance 2 negative Cl ions. Cr has a charge of 3+, so we have to balance 3 negative Cl ions.
- Remember that polyatomic ions have a charge of their own. [13] X Research Source
- Solids, liquids, gases, weak acids and ionic compounds with low solubility do not change state or separate into ions. We keep these substances intact.
- The molecules will be dispersed in solution so their state will change to ( dd ). The three exceptions that don’t become ( dd ) are: CH 4( k ) , C 3 H 8( k ) , and C 8 H 18( l ) .
- Continuing with the above example, the full ionic equation would look like this: 2Cr ( r ) + 3Ni 2+( dd ) + 6Cl –( dd ) –> 2Cr 3+( dd ) + 6Cl –( dd ) + 3Ni ( r ) . When Cl is not present in the compound, it is not a diatomic substance, so we multiply the factor by the number of atoms in the compound to get 6 Cl ions on both sides of the equation.
- After completing the example, we have 6 equilibrium Cl ions – cancelable on each side. The net ionic equation is 2Cr ( r ) + 3Ni 2+( dd ) –> 2Cr 3+( dd ) + 3Ni ( r ) .
- If you write it correctly then the total charge on the reactant side should be equal to the total charge on the product side in the net ionic equation.
Advice
- Write the states of all substances in the equation, otherwise you will lose points.
This article is co-authored by a team of editors and trained researchers who confirm the accuracy and completeness of the article.
The wikiHow Content Management team carefully monitors the work of editors to ensure that every article is up to a high standard of quality.
There are 9 references cited in this article that you can view at the bottom of the page.
This article has been viewed 172,647 times.
The net ionic equation is an important part of chemistry because it represents only the elements that are changed in a chemical reaction. They are most commonly used in oxidation-reduction reactions, exchange reactions, and acid-base neutralization reactions. [1] X Research Source There are three basic steps to writing a net ionic equation: balancing the molecular equation, converting it to a full ionic equation (according to how each substance exists in solution), and finally Write the net ionic equation.
In conclusion, writing a net ionic equation is a crucial skill for chemistry students. It allows them to focus on the important ions and molecules involved in a chemical reaction, simplifying the overall equation. By following the steps outlined in this guide, students can easily convert a balanced chemical equation into a net ionic equation. By removing the spectator ions, the net ionic equation helps to highlight the actual chemical changes occurring in the reaction. This simplification allows for a clearer understanding of the core reactions taking place. The net ionic equation is an essential tool for chemists, providing a concise representation of chemical reactions and facilitating further analysis and understanding.
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