Pirate Chemistry Forming Ionic Compounds We now know how many reactive or valence (outer) electrons each element has. Because of that, we can figure out what charge ions like to go to. Armed with this information, we should be able to figure out the formulae of any ionic compound. Let’s look at one we already did: Sodium atom: Na Chlorine atom: Cl When these two ions combine, the sodium gives up its valence electron to the chlorine to become a +1 charge while the chlorine takes the electron to become a –1 charge: Sodium ion: Na+1 Chloride ion: Cl-1 The +1 charge of the Na cancels out the –1 charge of the Cl and the two become a new compound: Na+1Cl-1 The charges are still there internally but since they cancel each other out we typically don’t include them in the overall formula so we just end up with: NaCl We see that any ionic compound will be made of two parts; a positive ion and a negative ion. Remember that metals tend to go to positive ions and non-metals tend to go to negative ions. These ions have special names: Cation: an ion with a positive charge Anion: an ion with a negative charge In the above example, sodium is the cation because it is positive and chlorine is the anion because it is negative. Let’s examine the chart below for more examples: Metal Non-metal Cation Anion Combination Formula Na Cl Na+1 Cl-1 Na+1Cl-1 NaCl K I K+1 I-1 K+1I-1 KI Ca O Ca+2 O-2 Ca+2O-2 CaO Mg S Mg+2 S-2 Mg+2S-2 MgS Al N Al+3 N-3 Al+3N-3 AlN But what happens if the charges aren’t equal? All text copyright Chris Smith 2009. All pictures obtained from internet and are copyright of their owners but assumed to be public accessible. If you are the owner of a picture and want it removed, email csmith@d211.org, and it will be. Pirate Chemistry Combining Ions of Different Charges What would happen if we tried to combine calcium with chloride? Remember that: Calcium atom Chlorine atom 20 electrons (unstable number) 2 in the first shell 8 in the second shell 8 in the third shell 2 in the fourth (valence) shell Calcium will lose 2 electrons in valence shell 17 electrons (unstable number) 2 in the first shell 8 in the second shell 7 in the third (valence) shell Chloride will gain 1 electron in valence shell Chloride ion: Calcium ion: 18 electrons (stable number) 2 in the first shell 8 in the second shell 8 in the third shell (octet rule satisfied) 18 electrons (stable number) 2 in the first shell 8 in the second shell 8 in the third shell (octet rule satisfied) Chloride ion 2, 8, 8 -1 https://cornellchem.wikispaces.com/file/view/ Electron_shell_020_calcium.png/47421581 http://www.bbc.co.uk/schools/gcsebitesize/ science/images/diag_calcium_2.gif http://upload.wikimedia.org/wikipedia/ commons/thumb/9/96/ Electron_shell_017_Chlorine.svg/558pxElectron_shell_017_Chlorine.svg.png Calcium is giving up two electrons but chloride only needs one. If we tried to put them together we would end up with an overall charge of +1: Calcium ion: Ca+2 Chloride ion: Cl-1 Ca+2Cl-1 CaCl+1 ????? All compounds need to be neutrally charged so this cannot be. Plus, where did that other electron go? Calcium has lost 2 but chloride has only gained 1. The solution is that Calcium has the ability to satisfy two chloride ions! Instead of trying to force two electrons on one atom of chlorine, calcium gives one electron to two different chlorines: All text copyright Chris Smith 2009. All pictures obtained from internet and are copyright of their owners but assumed to be public accessible. If you are the owner of a picture and want it removed, email csmith@d211.org, and it will be. Pirate Chemistry http://www.green-planet-solar-energy.com/images/ eletron-shell-filling.gif 7 Ca Calcium gives up one electron to two different chlorides Cl Two different chlorines accept one electron each 7 Cl Calcium chloride is formed from 1 calcium atom and 2 chlorine atoms http://www.bbc.co.uk/schools/gcsebitesize/science/images/diag_calcium_chloride.gif So the formula for calcium chloride is: Calcium ion: Ca+2 Chloride ion: Cl-1 Ca+2Cl-1 Cl-1 CaCl2 Note that this 2 here in subscript form indicates that there are 2 chlorine atoms in the formula Calcium chloride is a white crystal. It has a variety of uses as a dessicant, ice control on roads, and as an addiAll text copyright Chris Smith 2009. All pictures obtained from internet and are copyright of their owners but astive in many applications. http://img.en.china.cn/0/0,0,145,15811,640,480,a308c609.jpg sumed to be public accessible. If you are the owner of a picture and want it removed, email csmith@d211.org, and it will be. Pirate Chemistry All we need to do, then, is to make sure there are as many negative charges as positive charges and vice versa. There are a variety of methods for doing this. The easiest way to do it is to follow these two simple steps: 1. Check to see if the charges are the same. If they are, simply put the cation first and the anion second and you are done. 2. If the charges DON’T cancel each other out, perform the ―criss-cross‖ method. The charge magnitude for the cation becomes the number of the anion atoms present. The charge magnitude for the anion becomes the number of the cation atoms present. Example 1: Strontium and Oxygen Sr+2 O-2 These charges cancel each other out. SrO Final formula Example 2: Strontium and Fluorine Sr+2 F-1 These charges DON’T cancel out. Criss-cross the numbers down. Sr F Sr1F2 Note that we eliminate the + and — signs here. Also, you don’t have to write the ―1‖. It’s implied SrF2 Final formula Example 3: Potassium and Oxygen K+1 O-2 K These charges DON’T cancel out. Criss-cross the numbers down. O K2O1 Note that we eliminate the + and — signs here. Also, you don’t have to write the ―1‖. It’s implied. K2 O Final formula Example 4: Aluminum and Oxygen Al+3 O-2 Al2O3 Final formula All text copyright Chris Smith 2009. All pictures obtained from internet and are copyright of their owners but assumed to be public accessible. If you are the owner of a picture and want it removed, email csmith@d211.org, and it will be. Pirate Chemistry Metal Non-metal Cation Anion Formula Mg Cl Mg+2 Cl-1 MgCl2 Al Br Al+3 Br-1 AlBr3 Na O Na+1 O-2 Na2O K N K+1 N-3 K3N Al O Al+3 O-2 Al2O3 Be P Be+2 P-3 Be3P2 Naming Ionic Compounds Naming ionic compounds is very simple. The name of the cation does not change. The name of the anion changes to an –ide ending. Using the above examples: Formula Cation Anion MgCl2 Magnesium Chloride AlBr3 Aluminum Bromide Na2O Sodium Oxide K3N Potassium Nitride Al2O3 Aluminum Oxide Be3P2 Beryllium Phosphide http://www.homedepot.ca/wcsstore/HomeDepotCanada/ images/catalog/21296b7e-2623-41b9-ad0ca87bbfdf5dc3_4.jpg http://image.hotrod.com/f/11785508/ hrdp_0901_24_z+rust_removal_guide+aluminum_oxide.jpg Aluminum Oxide, Al2O3, is a very hard, abrasive mineral. It is used on devices like a Dremel rotary device. When powdered, it is a major component of the ―chalk‖ used for billiards cues. All text copyright Chris Smith 2009. All pictures obtained from internet and are copyright of their owners but assumed to be public accessible. If you are the owner of a picture and want it removed, email csmith@d211.org, and it will be. http://z.about.com/w/experts/Pool-Billiards-2283/2009/01/MasterChalk-jpg.jpg Pirate Chemistry Questions 1. 2. 3. 4. 5. 6. What is a cation? What is an anion? Do metals tend to become cations or anions? Do non-metals tend to become cations or anions? What charge to all compounds have to be, positive, negative, or neutral? Write the formula for the following ionic compounds: A. Magnesium bromide B. Aluminum fluoride C. Potassium oxide D. Lithium nitride E. Sodium sulfide F. Beryllium nitride G. Aluminum sulfide H. Calcium iodide I. Cesium oxide 7. Write the name for the following ionic compounds: A. NaBr B. K2S C. Ca3N2 D. BaO E. BeCl2 All text copyright Chris Smith 2009. All pictures obtained from internet and are copyright of their owners but assumed to be public accessible. If you are the owner of a picture and want it removed, email csmith@d211.org, and it will be.