Double Displacement Reactions

in this video we will be looking at double displacement reactions and do some examples that illustrate double displacement reactions first we want to talk about what a double displacement reaction is in very very general terms so sometimes we call these double displacement reactions precipitation reactions as a solid will sometimes form as well another name these double displacement reactions sometimes go by our metathesis reactions so in a double displacement reaction you're looking at a reaction between two ionic compounds that's your key that you're dealing with a double displacement reaction what will happen in these double displacement reactions is the ionic compounds will switch partnerships in the reaction this follows a very predictable pattern so we're going to look at this pattern so I did this in a very general way and then we'll look at some specific examples later so I have ionic compound a B with a B and the positive on B being the negative line now I'm going to react that with compound CD also an ionic compound with C being the positive ion D being the negative ion so what I'm going to do is I'm going to mix and match partnerships and take the positive a is currently paired with the negative B and I need to pair this with the other negative ions so my new partnerships going to be a d the other two that are left over I still have negative B left over and positive C I need to pair those as well so my other compound will be C B the C has to come first because that's a positive I'm we always write ionic compounds with the positive ion first for these double displacement reactions we no longer need to be told what the product is we can figure it out from the reactants that we have previously anytime you had a reaction you had to be given the entire reaction reactants and products here we're now at the stage for these type of double displacement reactions where you're not going to be given what the products are you're going to have to figure those out so now that we've seen the general pattern let's look at some specific examples so aqueous solutions of lead nitrate and potassium chloride are mixed we want to write out the complete molecular ionic and net ionic equations for these so what we're really doing is we are going to mix and match these ions so we want to figure out what's going to be produced what are we going to make out of this so the first step is to predict the products we need to take our ions and mix and match those so the first step is looking at what you have so the lead nitrate I have a lead iron at plus 2 and I also have nitrate ions the nitrate ions are going to be minus 1 it doesn't matter that I have two of those at this point we just need to list what type of ions we have present we can deal with the exact numbers later when we don't and bounce the equation so for the lead nitrate I have lead plus 2 s and I have nitrate ions for the KCl what do I have I have potassium plus 1 and chloride minus 1 now I need to mix these ions I need to pair the lead who is currently with the nitrate with a new ionic partnership that's going to be the negative chloride I I need to pair the lead and the chloride well how do I pair those well I can't just randomly throw them together I still need to achieve charge balance blebs plus 2 the chlorides minus 1 so what I'm really going to need is I'm going to need two chloride ions from that in order to have charge balance so my new formula is going to be P bcl-2 now for my other partnership I'm pairing negative nitrate ions with the positive potassium ions matrix minus one potassium plus one so to have charge Mouse I just need one of each so my other compound is going to be K no.3 so on I kind of the stage that we're at here we were able to successfully predict the products next up we have to decide whether those products are soluble or not soluble and to do that we need to use the solubility rules to the side of these are going to be soluble or not so you have to memorize these solubility rules so our solubility rules for chloride say chlorides generally soluble except when paired with let and here we're paired with let so being we are paired with lead that's going to be a solid here that's not going to be soluble for our other compound things in Group one a potassium is in Group one a those ions are always soluble also nitrate is always soluble so the other products definitely going to be soluble so our precipitate is going to be the PB CL 2 our last step is to balance the equation just like all of our other equations have to be balanced these double displacement reaction equations have to be balanced as well so here you can go ahead and use a tally chart sometimes you don't need to sometimes you just kind of quickly look and see what you need we need to successfully balance us so getting those two coefficients in there to get everything balanced what we just wrote is sometimes called the Molecular equation that's our standard form there's a couple other different forms of this that we can write that we're going to see but we generally start with this molecular equation it's going to quickly go through the steps again first predict the products mix and match the ions you are not worried about balancing in terms of balancing equation at this state you first have to just get correct formula of the products once you have that hearing you solubility rules to decide those products of soluble and lastly you're going to balance that equation so molecular equations are considered the standard form the equation but what the molecular equations doesn't do a good job of is it doesn't do a good job of showing those ions that are actually in solution so we sometimes do is sometimes we write an ionic equation from that Molecular equation because the ionic equation does a little bit better job of showing exactly what you have in that solution I just rewrote our Molecular equation that we ended with and then here are the steps we're going to do to go from this molecular equation to the ionic equation we're in take soluble Ana compounds remember soluble ionic compounds will be strong electrolytes they're going to have charges they're going to dissolve we're gonna show how they really look in the solution as ions if we have a precipitate we're going to leave the precipitate as written we're not going to make any changes to that so we're going to take our Molecular equation and write the ionic equation from this so here's how we do the lead nitrate is soluble PB no3 2 is soluble so what kind of ions do we have well these aren't really together so the aq means these not really the Taylor is to split up in the I so we're showing that in the psionic equation what do I have I have one wet ion with a plus two charge what do I also has I have two night straight lines they're not linked together they're actually separate so I need to show them as having two in quantity but not actually being bound together so that's how we're going to write our main straight ions out like that they're not together the top we're showing them kind of together what it's really happening though is they are not together in that same thing with the potassium chloride to KCl that is soluble that's a strong electrolyte as well that's going to split up into its ion so I'm really going to have two potassium ions and two chloride ions now for the product side the lead chloride that we have here the PB CL - that's a solid that's our precipitate that's not dissolved in solution that hasn't been dissolved by the water that hasn't split up into individual ions letting the chloride are still together we leave that together when we write our ionic equation for the two can O three what do we have well this is soluble so we need to show those ions two potassium ions soluble two nitrate ions that are soluble one key thing you want to make sure you do and sometimes people get sloppy and don't do this you need to show charges for all of your eyes you can't get sloppy this is an ionic equation after all if you're not showing those charges you didn't write an ionic equation so you have to make sure you're doing that it's kind of easy to get careless and sloppy and not quite do that you have to make sure you're still doing that you also have to make sure you're writing the states of matter in whether it's a solid whether it's a cute you kind of be easy to kind of forget to do that for a couple of them you have to do that for everything so what we just wrote is the ionic equation and the ionic equation does a little bit better job showing all the individual ions that we have present there's one last equation we can write from this and it's called the net ionic equation so lob ionic equation clearly shows all the I's in place it can be a little bit long and cumbersome sometimes we can write a more condensed way of showing that so sometimes the net ionic equation is written but the net ionic equation does is the net ionic equation simplifies equation - just showing the things that end up changing in this it shows the action for what happened in the reaction so we want to look at how do we take our ionic equation write a net ionic equation from that so we're going to do is we're going to look for things that appear on each side of the equation and cancel them off these things that we're going to cancel off we call spectator ions chemistry sometimes called the science of change we often care about how things are changing what changed in the reaction and that's what this net ionic equation is going to do is going to get rid of any piece that wasn't directly involved in the change so let's kind of look at our ionic equation now what we're doing is we're looking for things that appear on both sides of the equation very similar to what you may do in math if you have the same thing on the left that you do on the right you cancel those things off so what do we have here I see two nitrate ions on the left two nitrate ions on the right we can cancel those off I see two potassium ions on the reactant side on the left two potassium ions on the product side on the right we could cancel those off now when you cancel in math it's a little bit different than what we're showing when we're cancelling here when you cancel off something in math you completely got rid of it it doesn't exist anymore that's not what's happening here when we're canceling here when we're cancelling we're not getting rid of it there are still nitrate ions present there are still potassium ions present by us cancelling them off though what that is showing is that they didn't take part in the change they weren't part of the change in this they were part of the action they were watching they were spectating they were seeing what was happening but they weren't a part of it that's why we called me spectator ions they're there but they're not actually involved in the reaction our last step is we just kind of bring down just like in math bring down what we didn't cancel so let ions let ions chloride ions chloride ions our precipitate un-- chloride our precipitated what we have is a net ionic equation and the net ionic equation just shows those things that actually change in the equation just like the ionic equation is important to remember to write charges in where it's appropriate as well as to write in whether things are aqueous or solids this was one example let's look at another example that kind of goes through this in this one we're going to be looking at equus solutions of fecl3 and NaOH our mix we're gonna write out the complete molecular ionic and net ionic equations from me so what are we looking to do we're gonna react fecl3 and I NaOH and we're gonna try to figure out what in the world those are going to produce so again just like before the first step is to predict the products we need to mix and match the positive and negative sign so I wrote out again the items that we have in place fecl3 well that means I have Fe plus 3 times I'm also going to have CL minus i but look at that NaOH what am I going to have I'm going to have sodium plus ions and hydroxide ions so now I need to mix and match right now the iron is paired with the chloride so to mix and match the ions I need to pair the iron with the hydroxide so the iron is plus 3 the hydroxides minus 1 so in order to pair those up I'm going to need three hydroxides for everyone iron in order to achieve charge balance need to do a similar proud suss with the other ionic pair now I'm going to pair the chloride ions with the sodium ion chlorides minus one sodium is plus one so what's my formula going to be NaCl remember positive mine always comes first so now I've successfully predicted the products fe co 3 plus NaOH will produce FeO x3 and NaCl our next step is to use solubility rules to decide of the products are soluble again you have to have these solubility rules memorize so let's look at the FeO a ch3 the FeO a ch3 if you look on your solubility rules you're going to find that the hydroxide ions are generally not soluble unless they're paired with something else that's very very soluble here this is going to be our precipitate iron is not going to allow the iron to be able sorry iron is not going to allow the hydroxide to be soluble here this is going to form a precipitate this would not be one of the exceptions so here's going to be our precipitate NaCl well we kind of recognize salt soluble in water but kind of using the rules anytime you have sodium ions they're almost always going to be soluble chloride is going to be soluble unless it's paired with certain specific things that would make it insoluble so we're gonna have NaCl be soluble the FE oh3 not be soluble last step is we would balance the equation same techniques we've been using before remember you don't necessarily have to split apart the polyatomic i'm you can balance them as whole units you can use a tally chart sometimes you don't need to but after you balance the equation remember we've done this lots and lots of times already I'm not showing the specifics of this you need to just quickly then balance that equation so then we would have our Molecular equation next up would be to write out that ionic equation now so for the ionic equation remember like Euler equation did a good job of being kind of concise as being a standard form but it doesn't show the ions that we know actually exist so we're gonna write that ionic equation from the Molecular equation when do the same thing we did in the previous example and take our soluble ionic compounds those strong electrolytes and show how they really look in the solution as ions just like before we're going to leave the precipitate as written we're just gonna bring that down as written so to start this off the fecl3 is soluble so what are we going to do we're going to have iron plus three AIIMS and three chloride ions remember these chlorine ions aren't together anymore they're separated each chloride is now individually surrounded by water molecules that's what this means when we say fecl3 aq we really mean we have separate iron ions and three separate chloride hinds we're do the same thing for the sodium hydroxide three NaOH that soluble so I need to split that up and show how that actually dissolved three sodium ions eq3 hydroxide ions aq4 the FE o h3 this is our solid thus our precipitate this has not dissolved this is not split up into individual ions these ions are still all together I need to show that I'm just gonna bring that down as is the NaCl though is soluble so the NaCl being soluble I need to split this up into three sodium ions and three chloride ions so here we have our ionic equation kind of quickly go back and double check we have charges for things you gotta remember to do that we have states of matter for everything so now we have this ionic equation now we're ready to move on and write the net ionic equation so for the net ionic equation although the ionic equation shows all the ions in place as we see it's kind of long so we can shorten that up with a net ionic equation remember this is showing just the things that are changing in the reaction so how do we do that we're looking for those spectator ions we're looking for those lines that appear on each side of the equation and we're gonna cancel them off these are those spectator ions these are things that are not going to be involved in the actual change they're still present but they're not involved in the actual change so when we're looking for these spectator ions I see three chloride ions on the reactant side and three chloride ions on the product side I'm seeing three sodium ions on the reactant side and three sodium ions on the product side we can cancel those off after you found those spectator ions that have canceled those off it's really just a matter of bringing down things you didn't cancel off yet that iron plus three soluble the hydroxide ions soluble and then our precipitate so now we have our net ionic equation just showing those things that change the actual change that happened here were iron ions reacting with hydroxide ions to produce that solid Fe o h3 we have states of matter for everything we show charges where appropriate so here we have our net equation so being able to write these molecular ionic and non-ionic equations for these double displacement reactions takes some practice this isn't something you're going to be able to do just by looking at it you have to practice doing some of these to make sure you're comfortable doing these by yourself

in this video we will be looking at double displacement reactions and do some examples that illustrate double displacement reactions first we want to talk about what a double displacement reaction is in very very general terms so sometimes we call these double displacement reactions precipitation reactions as a solid will sometimes form as well another name these double displacement reactions sometimes go by our metathesis reactions so in a double displacement reaction you&#39;re looking at a reaction between two ionic compounds that&#39;s your key that you&#39;re dealing with a double displacement reaction what will happen in these double displacement reactions is the ionic compounds will switch partnerships in the reaction this follows a very predictable pattern so we&#39;re going to look at this pattern so I did this in a very general way and then we&#39;ll look at some specific examples later so I have ionic compound a B with a B and the positive on B being the negative line now I&#39;m going to react that with compound CD also an ionic compound with C being the positive ion D being the negative ion so what I&#39;m going to do is I&#39;m going to mix and match partnerships and take the positive a is currently paired with the negative B and I need to pair this with the other negative ions so my new partnerships going to be a d the other two that are left over I still have negative B left over and positive C I need to pair those as well so my other compound will be C B the C has to come first because that&#39;s a positive I&#39;m we always write ionic compounds with the positive ion first for these double displacement reactions we no longer need to be told what the product is we can figure it out from the reactants that we have previously anytime you had a reaction you had to be given the entire reaction reactants and products here we&#39;re now at the stage for these type of double displacement reactions where you&#39;re not going to be given what the products are you&#39;re going to have to figure those out so now that we&#39;ve seen the general pattern let&#39;s look at some specific examples so aqueous solutions of lead nitrate and potassium chloride are mixed we want to write out the complete molecular ionic and net ionic equations for these so what we&#39;re really doing is we are going to mix and match these ions so we want to figure out what&#39;s going to be produced what are we going to make out of this so the first step is to predict the products we need to take our ions and mix and match those so the first step is looking at what you have so the lead nitrate I have a lead iron at plus 2 and I also have nitrate ions the nitrate ions are going to be minus 1 it doesn&#39;t matter that I have two of those at this point we just need to list what type of ions we have present we can deal with the exact numbers later when we don&#39;t and bounce the equation so for the lead nitrate I have lead plus 2 s and I have nitrate ions for the KCl what do I have I have potassium plus 1 and chloride minus 1 now I need to mix these ions I need to pair the lead who is currently with the nitrate with a new ionic partnership that&#39;s going to be the negative chloride I I need to pair the lead and the chloride well how do I pair those well I can&#39;t just randomly throw them together I still need to achieve charge balance blebs plus 2 the chlorides minus 1 so what I&#39;m really going to need is I&#39;m going to need two chloride ions from that in order to have charge balance so my new formula is going to be P bcl-2 now for my other partnership I&#39;m pairing negative nitrate ions with the positive potassium ions matrix minus one potassium plus one so to have charge Mouse I just need one of each so my other compound is going to be K no.3 so on I kind of the stage that we&#39;re at here we were able to successfully predict the products next up we have to decide whether those products are soluble or not soluble and to do that we need to use the solubility rules to the side of these are going to be soluble or not so you have to memorize these solubility rules so our solubility rules for chloride say chlorides generally soluble except when paired with let and here we&#39;re paired with let so being we are paired with lead that&#39;s going to be a solid here that&#39;s not going to be soluble for our other compound things in Group one a potassium is in Group one a those ions are always soluble also nitrate is always soluble so the other products definitely going to be soluble so our precipitate is going to be the PB CL 2 our last step is to balance the equation just like all of our other equations have to be balanced these double displacement reaction equations have to be balanced as well so here you can go ahead and use a tally chart sometimes you don&#39;t need to sometimes you just kind of quickly look and see what you need we need to successfully balance us so getting those two coefficients in there to get everything balanced what we just wrote is sometimes called the Molecular equation that&#39;s our standard form there&#39;s a couple other different forms of this that we can write that we&#39;re going to see but we generally start with this molecular equation it&#39;s going to quickly go through the steps again first predict the products mix and match the ions you are not worried about balancing in terms of balancing equation at this state you first have to just get correct formula of the products once you have that hearing you solubility rules to decide those products of soluble and lastly you&#39;re going to balance that equation so molecular equations are considered the standard form the equation but what the molecular equations doesn&#39;t do a good job of is it doesn&#39;t do a good job of showing those ions that are actually in solution so we sometimes do is sometimes we write an ionic equation from that Molecular equation because the ionic equation does a little bit better job of showing exactly what you have in that solution I just rewrote our Molecular equation that we ended with and then here are the steps we&#39;re going to do to go from this molecular equation to the ionic equation we&#39;re in take soluble Ana compounds remember soluble ionic compounds will be strong electrolytes they&#39;re going to have charges they&#39;re going to dissolve we&#39;re gonna show how they really look in the solution as ions if we have a precipitate we&#39;re going to leave the precipitate as written we&#39;re not going to make any changes to that so we&#39;re going to take our Molecular equation and write the ionic equation from this so here&#39;s how we do the lead nitrate is soluble PB no3 2 is soluble so what kind of ions do we have well these aren&#39;t really together so the aq means these not really the Taylor is to split up in the I so we&#39;re showing that in the psionic equation what do I have I have one wet ion with a plus two charge what do I also has I have two night straight lines they&#39;re not linked together they&#39;re actually separate so I need to show them as having two in quantity but not actually being bound together so that&#39;s how we&#39;re going to write our main straight ions out like that they&#39;re not together the top we&#39;re showing them kind of together what it&#39;s really happening though is they are not together in that same thing with the potassium chloride to KCl that is soluble that&#39;s a strong electrolyte as well that&#39;s going to split up into its ion so I&#39;m really going to have two potassium ions and two chloride ions now for the product side the lead chloride that we have here the PB CL - that&#39;s a solid that&#39;s our precipitate that&#39;s not dissolved in solution that hasn&#39;t been dissolved by the water that hasn&#39;t split up into individual ions letting the chloride are still together we leave that together when we write our ionic equation for the two can O three what do we have well this is soluble so we need to show those ions two potassium ions soluble two nitrate ions that are soluble one key thing you want to make sure you do and sometimes people get sloppy and don&#39;t do this you need to show charges for all of your eyes you can&#39;t get sloppy this is an ionic equation after all if you&#39;re not showing those charges you didn&#39;t write an ionic equation so you have to make sure you&#39;re doing that it&#39;s kind of easy to get careless and sloppy and not quite do that you have to make sure you&#39;re still doing that you also have to make sure you&#39;re writing the states of matter in whether it&#39;s a solid whether it&#39;s a cute you kind of be easy to kind of forget to do that for a couple of them you have to do that for everything so what we just wrote is the ionic equation and the ionic equation does a little bit better job showing all the individual ions that we have present there&#39;s one last equation we can write from this and it&#39;s called the net ionic equation so lob ionic equation clearly shows all the I&#39;s in place it can be a little bit long and cumbersome sometimes we can write a more condensed way of showing that so sometimes the net ionic equation is written but the net ionic equation does is the net ionic equation simplifies equation - just showing the things that end up changing in this it shows the action for what happened in the reaction so we want to look at how do we take our ionic equation write a net ionic equation from that so we&#39;re going to do is we&#39;re going to look for things that appear on each side of the equation and cancel them off these things that we&#39;re going to cancel off we call spectator ions chemistry sometimes called the science of change we often care about how things are changing what changed in the reaction and that&#39;s what this net ionic equation is going to do is going to get rid of any piece that wasn&#39;t directly involved in the change so let&#39;s kind of look at our ionic equation now what we&#39;re doing is we&#39;re looking for things that appear on both sides of the equation very similar to what you may do in math if you have the same thing on the left that you do on the right you cancel those things off so what do we have here I see two nitrate ions on the left two nitrate ions on the right we can cancel those off I see two potassium ions on the reactant side on the left two potassium ions on the product side on the right we could cancel those off now when you cancel in math it&#39;s a little bit different than what we&#39;re showing when we&#39;re cancelling here when you cancel off something in math you completely got rid of it it doesn&#39;t exist anymore that&#39;s not what&#39;s happening here when we&#39;re canceling here when we&#39;re cancelling we&#39;re not getting rid of it there are still nitrate ions present there are still potassium ions present by us cancelling them off though what that is showing is that they didn&#39;t take part in the change they weren&#39;t part of the change in this they were part of the action they were watching they were spectating they were seeing what was happening but they weren&#39;t a part of it that&#39;s why we called me spectator ions they&#39;re there but they&#39;re not actually involved in the reaction our last step is we just kind of bring down just like in math bring down what we didn&#39;t cancel so let ions let ions chloride ions chloride ions our precipitate un-- chloride our precipitated what we have is a net ionic equation and the net ionic equation just shows those things that actually change in the equation just like the ionic equation is important to remember to write charges in where it&#39;s appropriate as well as to write in whether things are aqueous or solids this was one example let&#39;s look at another example that kind of goes through this in this one we&#39;re going to be looking at equus solutions of fecl3 and NaOH our mix we&#39;re gonna write out the complete molecular ionic and net ionic equations from me so what are we looking to do we&#39;re gonna react fecl3 and I NaOH and we&#39;re gonna try to figure out what in the world those are going to produce so again just like before the first step is to predict the products we need to mix and match the positive and negative sign so I wrote out again the items that we have in place fecl3 well that means I have Fe plus 3 times I&#39;m also going to have CL minus i but look at that NaOH what am I going to have I&#39;m going to have sodium plus ions and hydroxide ions so now I need to mix and match right now the iron is paired with the chloride so to mix and match the ions I need to pair the iron with the hydroxide so the iron is plus 3 the hydroxides minus 1 so in order to pair those up I&#39;m going to need three hydroxides for everyone iron in order to achieve charge balance need to do a similar proud suss with the other ionic pair now I&#39;m going to pair the chloride ions with the sodium ion chlorides minus one sodium is plus one so what&#39;s my formula going to be NaCl remember positive mine always comes first so now I&#39;ve successfully predicted the products fe co 3 plus NaOH will produce FeO x3 and NaCl our next step is to use solubility rules to decide of the products are soluble again you have to have these solubility rules memorize so let&#39;s look at the FeO a ch3 the FeO a ch3 if you look on your solubility rules you&#39;re going to find that the hydroxide ions are generally not soluble unless they&#39;re paired with something else that&#39;s very very soluble here this is going to be our precipitate iron is not going to allow the iron to be able sorry iron is not going to allow the hydroxide to be soluble here this is going to form a precipitate this would not be one of the exceptions so here&#39;s going to be our precipitate NaCl well we kind of recognize salt soluble in water but kind of using the rules anytime you have sodium ions they&#39;re almost always going to be soluble chloride is going to be soluble unless it&#39;s paired with certain specific things that would make it insoluble so we&#39;re gonna have NaCl be soluble the FE oh3 not be soluble last step is we would balance the equation same techniques we&#39;ve been using before remember you don&#39;t necessarily have to split apart the polyatomic i&#39;m you can balance them as whole units you can use a tally chart sometimes you don&#39;t need to but after you balance the equation remember we&#39;ve done this lots and lots of times already I&#39;m not showing the specifics of this you need to just quickly then balance that equation so then we would have our Molecular equation next up would be to write out that ionic equation now so for the ionic equation remember like Euler equation did a good job of being kind of concise as being a standard form but it doesn&#39;t show the ions that we know actually exist so we&#39;re gonna write that ionic equation from the Molecular equation when do the same thing we did in the previous example and take our soluble ionic compounds those strong electrolytes and show how they really look in the solution as ions just like before we&#39;re going to leave the precipitate as written we&#39;re just gonna bring that down as written so to start this off the fecl3 is soluble so what are we going to do we&#39;re going to have iron plus three AIIMS and three chloride ions remember these chlorine ions aren&#39;t together anymore they&#39;re separated each chloride is now individually surrounded by water molecules that&#39;s what this means when we say fecl3 aq we really mean we have separate iron ions and three separate chloride hinds we&#39;re do the same thing for the sodium hydroxide three NaOH that soluble so I need to split that up and show how that actually dissolved three sodium ions eq3 hydroxide ions aq4 the FE o h3 this is our solid thus our precipitate this has not dissolved this is not split up into individual ions these ions are still all together I need to show that I&#39;m just gonna bring that down as is the NaCl though is soluble so the NaCl being soluble I need to split this up into three sodium ions and three chloride ions so here we have our ionic equation kind of quickly go back and double check we have charges for things you gotta remember to do that we have states of matter for everything so now we have this ionic equation now we&#39;re ready to move on and write the net ionic equation so for the net ionic equation although the ionic equation shows all the ions in place as we see it&#39;s kind of long so we can shorten that up with a net ionic equation remember this is showing just the things that are changing in the reaction so how do we do that we&#39;re looking for those spectator ions we&#39;re looking for those lines that appear on each side of the equation and we&#39;re gonna cancel them off these are those spectator ions these are things that are not going to be involved in the actual change they&#39;re still present but they&#39;re not involved in the actual change so when we&#39;re looking for these spectator ions I see three chloride ions on the reactant side and three chloride ions on the product side I&#39;m seeing three sodium ions on the reactant side and three sodium ions on the product side we can cancel those off after you found those spectator ions that have canceled those off it&#39;s really just a matter of bringing down things you didn&#39;t cancel off yet that iron plus three soluble the hydroxide ions soluble and then our precipitate so now we have our net ionic equation just showing those things that change the actual change that happened here were iron ions reacting with hydroxide ions to produce that solid Fe o h3 we have states of matter for everything we show charges where appropriate so here we have our net equation so being able to write these molecular ionic and non-ionic equations for these double displacement reactions takes some practice this isn&#39;t something you&#39;re going to be able to do just by looking at it you have to practice doing some of these to make sure you&#39;re comfortable doing these by yourself

Transcript for:Double Displacement Reactions

Transcript for:
Double Displacement Reactions