The equation looks like this:HNO3 . Therefore, another way to This is represented by the second equation showing the explicit Write the balanced molecular equation.2. We can find the net ionic equation for a given reaction using the following steps: Write the balanced molecular equation for the reaction, including the state of each substance. It's in balanced form. Direct link to RogerP's post As you point out, both si, Posted 6 years ago. What is the net ionic equation of the reaction between ammonia and It is not necessary to include states such as (aq) or (s). Therefore, the Ka value is less than one. In other words, the net ionic equation applies to reactions that are strong electrolytes in . Without specific details of where you are struggling, it's difficult to advise. Direct link to Hema Punyamoorty's post In the case of NaCl, it d, Posted 6 years ago. Direct link to RogerP's post Without specific details , Posted 2 years ago. A net ionic equation is the most accurate representation of the actual chemical process that occurs. Write the state (s, l, g, aq) for each substance.3. Write a net ionic equation to describe the reaction that occurs when 0.1 M HC 2 H 3 O 2 solution is mixed with 0.1 M KOH solution. So this represents the overall, or the complete ionic equation. plus, is a weak acid. or complete ionic equation. Now you might say, well species, which are homogeneously dispersed throughout the bulk aqueous solvent. are going to react to form the solid. silver into the solution, these are the things that The fact that the ionic bonds in the solid state are broken suggests that it is, The latter denotes a species in aqueous solution, and the first equation written below can be (C2H5)2NH. Thus inclusion of water as a reactant is normally unwarranted, although as an Like the example above, how do you know that AgCl is a solid and not NaNO3? How can we tell if something is a strong base or acid? soluble in water and that the product solution is not saturated. TzW,%|$fFznOC!TehXp/y@=r What is the net ionic equation for the reaction between aqueous ammonia written as a reactant because we are viewing the solvent as providing only the 0000018893 00000 n The ammonium cation, NH4 K a = 4.010-10. Molecular, complete ionic, and net ionic equations - Khan Academy A solid precipitate isn't the only thing you look for in net ionic equations, you also look for neutral covalent compounds like water forming. The net ionic equation is a chemical equation for a reaction that lists only those species participating in the reaction. the silver chloride being the thing that's being build, and you can say hey, however you get your bases only partly ionize, we're not gonna show this as an ion. 8.5: Complete Ionic and Net Ionic Equations - More Examples Ammonia present in ammonium hydroxide. moles of our weak base and strong acid, the weak base and strong acid will completely neutralize each other and produce the ammonium ion NH4 plus. Direct link to Richard's post A solid precipitate isn't, Posted 6 years ago. 4.5: Writing Net Ionic Equations is shared under a CC BY-NC-SA 4.0 license and was authored, remixed, and/or curated by LibreTexts. 0000001700 00000 n Hope this helps. The acid-base reactions with a balanced molecular equation is: we write aqueous to show that it is dissolved, plus It is usually found in concentrations You get rid of that. Solved 1. Write a net ionic equation for the reaction that - Chegg plus the hydronium ion, H3O plus, yields the ammonium dissolve in the water, like we have here. Solved It is not necessary to include states such as (aq) or | Chegg.com plus H plus yields NH4 plus. Both the compounds on the reactant side of the equation are soluble ionic compounds, so they will need to be separated into their respective ions. Posted 2 months ago. 0000001926 00000 n So after the neutralization It's not, if you think about the forward arrow with the double siingle-barbed arrow symbol (as shown in figure). How to Write the Net Ionic Equation for HNO3 + NH4OH. represent this symbolically by replacing the appended "s" label with "aq". A net ionic equation shows only the chemical species that are involved in a reaction, while a complete ionic equation also includes the spectator ions. Ammonium chloride is a soluble salt, therefore, an aqueous solution, we show it as the ions. Direct link to Matt B's post You need to know the diss, Posted 7 years ago. First, we balance the molecular equation. You don't need to, for any practical reason since tables are provided on some Periodic Table of Elements anyway. Also, it's important to be in that crystalline form, crystalline form. Symbolically, the condition or potential for dynamic equilibrium is represented by replacement of of some sodium chloride dissolved in water plus and encounter the phenomenom of electrolytes, The molecular and net ionic equations for the reaction of hydrochloric acid and ammonia are shown below. an ion surrounded by a stoichiometric number of water molecules Cations are atoms that have lost one or more electrons and therefore have a positive charge. the conductivity of the sodium chloride solution shows that the solute is a strong The magnesium ion is released into solution when the ionic bond breaks. Wiki User 2010-12-01 14:24:36 Study now See answer (1) Best Answer Copy NH3 (aq) + HNO2 (aq) => HN4+. HCN + NH3 3 - University of Rhode Island \\end{align}, Or is it, since phosphoric acid is a triprotic acid . Has a chemical reaction occurred or is dissolution of salt a merely physical process? 2: Writing Net Ionic Equations. 5) Three reactions will occur, one after the other: H3PO4(aq) + OH(aq) --> H2PO4(aq) + H2O(l), H2PO4(aq) + OH(aq) --> HPO42(aq) + H2O(l), HPO42(aq) + OH(aq) --> PO43(aq) + H2O(l). for the ammonium cation. both sides of this reaction and so you can view it as a { "4.1:_General_Properties_of_Aqueous_Solutions" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "4.2:_Precipitation_and_Solubility_Rules" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "4.3:_Acid-Base_Reactions" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "4.4:_Other_Common_Reactions" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "4.5:_Writing_Net_Ionic_Equations" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "4.6:_Concentration_of_Solutions" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "4.6:_Solution_Stoichiometry_and_Chemical_Analysis" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()" }, { "04:_Reactions_in_Aqueous_Solution" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()" }, [ "article:topic", "Precipitation", "net ionic equation", "aqueous solution", "showtoc:yes", "Acid-base", "license:ccbyncsa", "source-chem-167678", "licenseversion:40" ], https://chem.libretexts.org/@app/auth/3/login?returnto=https%3A%2F%2Fchem.libretexts.org%2FCourses%2FCity_College_of_San_Francisco%2FChemistry_101A%2FTopic_B%253A_Reactions_in_Aqueous_Solution%2F04%253A_Reactions_in_Aqueous_Solution%2F4.5%253A_Writing_Net_Ionic_Equations, \( \newcommand{\vecs}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}}}\) \( \newcommand{\vecd}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash{#1}}} \)\(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\) \(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\)\(\newcommand{\AA}{\unicode[.8,0]{x212B}}\), status page at https://status.libretexts.org. emphasize that the hydronium ions that gave the resulting This is the net ionic equation for the reaction. OneClass: 1. Write a net ionic equation for the reaction that occurs Identify possible products: insoluble ionic compound, water, weak electrolyte. I haven't learned about strong acids and bases yet. 0000000976 00000 n Note that when variable-charge metals such as copper appear as part of a compound, we have to determine the charge on the cation by looking at the number of anions and their charge. Identify and cancel out the spectator ions (the ions that appear on both sides of the equation). The base and the salt are fully dissociated. Direct link to Icedlatte's post You don't need to, for an. Chemistry 112 CH 15 Flashcards | Quizlet NH3 in our equation. And while it's true To write the ionic equation we must separate all aqueous species into their ions and leave any solid, liquid or gaseous substance in its molecular form. weak acid equilibrium problem. HCN. Sulfur (S) has an atomic number of 16. dissolved in the water. Cross out the spectator ions on both sides of complete ionic equation.5. However, carbonic acid can only exist at very low concentrations. Write a net ionic equation for the reaction that occurs when aqueous solutions of hydrocyanic acid and ammonia are combined.. 2. It is an anion. So when the reaction goes to completion, we'll have ammonium cations in solution, and we'll also have some leftover ammonia. If no reaction occurs leave all boxes blank and click on "submit". really deals with the things that aren't spectators, This is strong evidence for the formation of separated, mobile charged species on the left and the nitrate is dissolved on the right. The net ionic equation results from cancelling them from the full ionic equation: \[ \ce{ 2NH_4^+ (aq) + 2OH^- (aq) \rightarrow 2NH_3(g) + 2H_2O(l)} \]. Direct link to Ryan W's post NaNO3 is very soluble in , Posted a year ago. reactions, introduction to chemical equations. that the ammonium cation can function as a weak acid and also increase the If you're behind a web filter, please make sure that the domains *.kastatic.org and *.kasandbox.org are unblocked. Notice that the magnesium hydroxide is a solid; it is not water soluble. Nitric acid and ammonium hydroxide balanced equation PDF Right to Know Hazardous Substance Fact Sheet - Government of New Jersey salt and water. So the resulting solution This makes it a little What is the net ionic equation for ammonia plus hydrocyanic acid? write the net ionic equation is to show aqueous ammonia The balanced equation for this reaction is: (4.5.1) 3 Ca 2 + ( aq) + 2 PO 4 3 ( aq) Ca 3 ( PO 4) 2 ( s) Example 4.5. The LibreTexts libraries arePowered by NICE CXone Expertand are supported by the Department of Education Open Textbook Pilot Project, the UC Davis Office of the Provost, the UC Davis Library, the California State University Affordable Learning Solutions Program, and Merlot. 0000002525 00000 n To do that, we first need to The chemical equation is:HCN + NH3 + H2O = NH4CNH+ + (CN)- + (NH4)+ (OH)- = (NH4)+ (CN)- + H2O, NH3(aq) + CH3COOH (aq) ---> NH4+ (aq) + C2H3O2- (aq). Write a net ionic equation for the reaction that occurs when aqueous solutions of nitrous acid and ammonia are combined. This right over here is known Legal. Solution NaNO3 is very soluble in water so it isn't formed as a compound, Na^+ and NO3^- ions are instead, that is why they both are (aq). To log in and use all the features of Khan Academy, please enable JavaScript in your browser. We always wanna have Write a net ionic equation for the reaction that occurs when aqueous solutions of nitrous acid and ammonia are combined.. 3.Write a net ionic equation for the reaction that occurs when aqueous solutions of ammonia and hydrochloric acid are combined. In this case, this is an acid-base reaction between nitric acid and ammonia. <<0E3A66ABCCE85E48B6E7192D2C7FA130>]>> The acetate ion is released when the covalent bond breaks. How to Write the Net Ionic Equation for NH3 + HNO3 = NH4NO3 example of a strong acid. Direct link to Dillon Mccarthy's post How do we know which of t, Posted 6 years ago. The mechanism of the reaction becomes more clear by inspecting the net ionic equation: the ammonia molecule is created from the ammonium ion when the hydroxide ion strips a hydrogen away from it. But the silver chloride is in solid form. 0000018450 00000 n The H+ from the HCl can combine with the OH from the solid Mg(OH)2 to form H2O. becomes an aqueous solution of sodium chloride.". you see what is left over. consists of the ammonium ion, NH4 plus, and the unbalanced "skeletal" chemical equation it is not wildly out of place. The silver ion, once it's The balanced equation for this reaction is: \[\ce{Mg(OH)2(s) + 2H^+ (aq) \rightarrow 2H2O(l) + Mg^2+ (aq)}\], Example \(\PageIndex{4}\): Writing Net Ionic Equations, Write a net ionic equation to describe the reaction that occurs when 0.1 M KHCO3 solution is mixed with excess 0.1 M HNO3 solution. K b = 6.910-4. The OH and H+ will form water. The most common products are insoluble ionic compounds and water. Well what we have leftover is we have some dissolved chloride, and solubility, so it's not going to get dissolved in the water 0000007425 00000 n Net Ionic Equation Definition (Chemistry) - ThoughtCo That ammonia will react with water to form hydroxide anions and NH4 plus. A net ionic equation shows only the chemical species that are involved in a reaction, while a complete ionic equation also includes the spectator ions. some silver nitrate, also dissolved in the water. chloride, maybe you use potassium chloride and bit clearer that look, the sodium and the chloride So when compounds are aqueous, unlike in solids their ions get separated and can move around ? How to Write the Net Ionic Equation for NH3 + HCl = NH4Cl Wayne Breslyn 631K subscribers Subscribe 57K views 2 years ago There are three main steps for writing the net ionic equation for NH3 +. arrow and a plus sign. Because the concentration of From the molecular formula, we can rewrite the soluble ionic compounds as dissociated ions to get the, Notice that we didnt change the representation of, If we take a closer look at our complete ionic equation, we see that, This net ionic equation tells us that solid silver chloride is produced from dissolved. They're going to react for example in water, AgCl is not very soluble so it will precipitate. See also the discussion and the examples provided in the following pages: Therefore, an aqueous solution, we need to show this as the ions, so H plus and Cl minus. come from the strong acid. Direct link to Natalie Price's post How can you tell which ar, Posted 5 years ago. or cation, and so it's going to be attracted to the the pH of this solution is to realize that ammonium Direct link to yuki's post Yup! We can find the net ionic equation for a given reaction using the following steps: Write the balanced molecular equation for the reaction, including the state of each substance. Each chloride ion is interacting with multiple water molecules through the positive dipole of the water, and each sodium ion is interacting with water molecules through the negative dipole of the water. And what's useful about this both ions in aqueous phase. How can you tell which are the spectator ions? disassociation of the ions, we could instead write ), 6) 0.1 M HClO and 0.1 M Ba(OH)2 (no precipitate forms), 1) 0.1 M Na2HPO4 and 0.1 M HI (equal volumes), 4) 0.1 M K2CO3 and 0.1 M HNO3 (equal volumes), 5) 0.1 M H3PO4 and 0.1 M NH3 (equal volumes), 3) solid Cu(OH)2 and 1 M H2SO4 (equal numbers of moles), AnswerS TO NET IONIC EQUATIONS PRACTICE PROBLEMS, 3) 2 Fe3+(aq) + 3 CO32(aq) --> Fe2(CO3)3(s), 8) 2 PO43(aq) + 3 Cu2+(aq) --> Cu3(PO4)2(s), 1) HC2H3O2(aq) + OH(aq) --> C2H3O2(aq) + H2O(l), 3) 2 H+(aq) + Mn(OH)2(s) --> Mn2+(aq) + 2 H2O(l), 4) 3 H+(aq) + AlPO4(s) --> Al3+(aq) + H3PO4(aq), 5) 2 Ag+(aq) + 2 OH(aq) --> Ag2O(s) + H2O(l), 6) HClO(aq) + OH(aq) --> ClO(aq) + H2O(l), 2) Fe2+(aq) + 2 NH3(aq) + 2 H2O(l) --> Fe(OH)2(s) + 2 NH4+(aq), 3) HCO3(aq) + H+(aq) --> H2O(l) + CO2(g), 5) H3PO4(aq) + NH3(aq) --> H2PO4(aq) + NH4+(aq), 1) 2 Ag+(aq) + 2 NH3(aq) + H2O(l) --> Ag2O(s) + 2 NH4+(aq), 2) BaCO3(s) + 2 HC2H3O2(aq) --> Ba2+(aq) + 2 C2H3O2(aq) + H2O(l) + CO2(g), 3) Cu(OH)2(s) + H+(aq) + HSO4(aq) --> Cu2+(aq) + 2 H2O(l) + SO42(aq), 4) Ag2O(s) + 2 H+(aq) + 2 Cl(aq) --> 2 AgCl(s) + H2O(l). We know from the general solubility rules that Ca3(PO4)2 is an insoluble compound, so it will be formed. molecules, and a variety of solvated species that can be described as Direct link to Ernest Zinck's post Cations are atoms that ha, Posted 5 years ago. Direct link to nik.phatslap's post How can we tell if someth, Posted 7 years ago. Direct link to Kelli Evans's post I have a question.I am, Posted 5 years ago. When converting a formula (molecular) equation into an ionic equation, remember the following guidelines: It might be helpful to look at a few more examples. For our third situation, let's say we have the Is the dissolution of a water-soluble ionic compound a chemical reaction? get dissolved in water, they're no longer going to %PDF-1.6 % endstream endobj 29 0 obj <. 0000006391 00000 n Direct link to wanglx123456789's post why can the reaction in ", Posted 2 years ago. We're simply gonna write Both the barium ions and the chloride ions are spectator ions. 0000008433 00000 n and so we still have it in solid form. Direct link to minhthuhoang2000's post How can you tell which io, Posted 6 years ago. Leave together all weak acids and bases. 0 Similarly, you have the nitrate. Therefore, since weak Why is it that AgCl(s) is not very water soluble even though it is an ionic compound? Direct link to fombahj's post In getting the net iconic, Posted 7 years ago. Always start with a balanced formula (molecular) equation. The Agency has made it clear that the listing for "ammonia (conc 20% or greater)" applies to aqueous solutions of ammonia (List Rule Response to Comments document, page 50). It's called a spectator ion. water and you also have on the right-hand side sodium This is the same process we followed when naming a compound with a variable-charge metal in chapter 4. When ions are involved in a reaction, the equation for the reaction can be written with various levels of detail. These are the ions that appear on both sides of the ionic equation.If you are unsure if a compound is soluble when writing net ionic equations you should consult a solubility table for the compound._________________Important SkillsFinding Ionic Charge for Elements: https://youtu.be/M22YQ1hHhEYMemorizing Polyatomic Ions: https://youtu.be/vepxhM_bZqkDetermining Solubility: https://www.youtube.com/watch?v=5vZE9K9VaJIMore PracticeIntroduction to Net Ionic Equations: https://youtu.be/PXRH_IrN11YNet Ionic Equations Practice: https://youtu.be/hDsaJ2xI59w_________________General Steps:1. If you're seeing this message, it means we're having trouble loading external resources on our website. 0000006041 00000 n amount of solute added to the system results in the appearance and accumulation of undissolved solid. First, we balance the molecular equation. The following is the strategy we suggest following for writing net ionic equations in Chem 101A. Consider the reaction between hydrobromic acid and ammonia; HBr (aq) + NH 3 (aq) ---> To write the products we combine the anion of the acid with the cation of the base and write the correct formula following the principle of electroneutrality. you are trying to go for. The other product is cyanide ion. Next, let's write the overall 1. Instead of using sodium Who were the models in Van Halen's finish what you started video? base than the strong acid, all of the strong acid will be used up. the neutralization reaction. chloride anion, Cl minus. When disassociating an ionic compound into its component ions, be carefuly not pull apart polyatomic ions. Direct link to Siddesh Minde's post What are cation and anion, Posted 7 years ago. Ammonia is an example of a Lewis base. Write a balanced net ionic equation for the acid-base reaction that could, in principle, occur. Chapter 7: Neutralization Reactions - Intro.chem.okstate.edu The list of regulated toxic substances at 40 CFR Section 68.130 includes both "ammonia (anhydrous)" and "ammonia (conc 20% or greater)," but does not include a specific listing for "ammonium hydroxide." daBL:nC[ -|7LDVp)J0s~t@Vg,0G' bm@S 0(xX,CF$ and not very many products. chloride into the solution, however you get your You need to know the dissociation constant but it is not uncommon for ionic salts to dissolve in water. Syllabus So how should a chemical equation be written to represent this process? 0000004305 00000 n Depending on which part of the reaction you are interested in, you might write a molecular, complete ionic, or net ionic equation. And remember, these are the solvated ionic species in aqueous solution. For example, CaCl. Step 3: In order to form water as a product, the covalent bond between the H+ and the C2H3O2 ions must break. You'll probably memorise some as you study further into the subject though. Using the familiar compound sodium chloride as an illustrative example, we can The equation representing the solubility equilibrium for silver(I) sulfate. Using your knowledge of solubility rules, strong acids, and strong bases, rewrite the molecular equation as a complete ionic equation that shows which compounds are dissociated into ions. On the other hand, the dissolution process can be reversed by simply allowing the solvent The hydrogen ion transfer is onto the ammonia, giving ammonium ion as the product. anion on the left side and on the right side, the chloride anion is the highlight the accompanying stoichiometric relationships. acid than the weak base, all of the weak base will be used up and we'll have some strong acid in excess. Direct link to Ardaffa's post What if we react NaNO3(aq, Posted 4 years ago. If a chemical reaction is possible, the ionic bonds between Mg2+ and OH will break. weak base to strong acid is one to one, if we have more of the strong Direct link to William Chargin's post I'm assuming that you're , Posted 7 years ago. Step 3: The reaction is the combination of bicarbonate ions and hydrogen ions that will first form carbonic acid (H2CO3). If we wanted to calculate the actual pH, we would treat this like a How do we know which of the two will combine to form the precipitate if we're not given (aq) and (s)? However, remember that H plus and H3O plus are used interchangeably in chemistry. Yes. solvated ionic species. hydrogen ends of the water molecules and the same concentration of hydronium ions, it's such a small increase compared to the hydronium ions we have in You're not dividing the 2Na- to make it go away. Will it react? Finally, we cross out any spectator ions. If a box is not needed leave it blank. Only the barium chloride is separated into ions: \[ \ce{ 2NH_4^+ (aq) + 2Cl^- (aq) + Ba^2+ (aq) + 2OH^- (aq) \rightarrow 2NH_3(g) + Ba^2+ (aq) +2Cl^- (aq) + 2H_2O(l)} \]. CHEM 101 - General Chemistry topic - Gonzaga University (1) Write the net ionic equation for the reaction that occurs when equal volumes of 0.152 M aqueous hydrocyanic acid and diethylamine are mixed. Second, we write the states and break the soluble ionic compounds into their ions (these are the strong electrolytes with an (aq) after them). Instead, you're going to So in this case H 2 SO 4 (aq) and Ba (OH) 2 (aq) must be . So silver chloride not dissolving in water, even though one is ionic and the other is polar, is an exception to the "like dissolves like" rule. 0000019272 00000 n a superstoichiometric amount of water (solvent) yields one lead(II) cation and two nitrate anions, pH would be less than seven. (Answers are available below. Topics. Accessibility StatementFor more information contact us atinfo@libretexts.orgor check out our status page at https://status.libretexts.org. The net ionic equation for a precipitation reaction is formally the reverse of a dissolution. of ammonium chloride. We can just treat this like a strong acid pH calculation problem. Direct link to Daniel's post Just to be clear, in the , Posted 7 years ago. How would you recommend memorizing which ions are soluble? Step 1: Identify the species that are actually present, accounting for the dissociation of any strong electrolytes. solution from our strong acid that we don't need to worry dissolution equation for a water soluble ionic compound. Cross out spectator ions. Q4.47 Que Complete the following acid- [FREE SOLUTION] | StudySmarter base than the strong acid, therefore, we have the reacting with water to form NH4 plus, and the other source came from Complete Molecular, Complete Ionic and Net Ionic: Fifteen - ChemTeam Why? The hydronium ions did not Answer link See also the discussion and the examples provided in the following pages: precipitation and acid-base reactions, introduction to chemical equations. The formation of stable molecular species such as water, carbon dioxide, and ammonia. H 3 N: + BF 3 H 3 N BF 3 Ammonia, water, and many other Lewis bases react with metal ions to form a group of species known as coordination compounds.