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Ionic Compounds

Ionic Compounds. Recall Ions: “+” on the left (metals) because they lose electrons (become less negative) “-” on the right (non-metals) because they gain electrons (become more negative) What is the total charge if you have X +1 and Y -1 ______________________________________.

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Ionic Compounds

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  1. Ionic Compounds Recall Ions: “+” on the left (metals) because they lose electrons (become less negative) “-” on the right (non-metals) because they gain electrons (become more negative) What is the total charge if you have X+1 and Y-1 ______________________________________

  2. Ionic Compounds • Metal and a non-metal combine to form "Ionic Compounds". • The metal atoms loses electrons to form positive ions. • The non-metal gains the electrons to form negative ions. • The two ions join together • ______________________________________ • ______________________________________

  3. Ionic compounds are formed when a metal gives one or more of its electrons to a non metal. When all of the electrons are gone, the metal’s inner orbit of electrons is full. So, the metal is stable. ______ ______ Ca Ionic Compounds Ca+2

  4. The non-metal receives one or more electrons to fill its outer shell and become stable. If we draw the Lewis Structure for a non metal we include the full valence orbit, brackets and a charge Having gained two electrons, the Oxygen is now negative. ____ O -2 O Ionic Compounds

  5. Putting the compound together, we can see that the overall molecule has a neutral charge. This particular example is simple because the Calcium and Oxygen want to exchange the same number of electrons. What would happen if they wanted to exchange different numbers of electrons? -2 O Ionic Compounds Ca+2 +2 – 2 = 0 Try it!

  6. First draw the Lewis structures of the atoms on their own. Now use an arrow to show the electron transferring from the Lithium atom to the Oxygen atom You can see that the Oxygen atom still does not have a complete outer shell. Clearly another Lithium atom is required to complete the compound. Li O Li Using Lewis Structures:Ionic bonding between Lithium and Oxygen

  7. ______________________ ______________________ The final Lewis structure is illustrated here. ______________________ Li+ Li+ -2 O Lithium Oxide continued

  8. Draw the Lewis Structures of the individual atoms. Use arrows to show the transfer of electrons. Aluminum has one electron left, we need another oxygen atom. The oxygen atom now needs more electrons so we need another aluminum atom. The extra electrons on the Aluminum mean we need another Oxygen. Since, we have been able to make both atoms stable, we have hit the correct ratio. Al Al O O O Illustrate the bonding between Aluminum and Oxygen. (Note the ratio here is a little harder to find.)

  9. Having _______3 electrons, the aluminum has a charge of __. Having ________2 electrons, the oxygen has a charge of ___. Now draw the final Lewis Structure. This structure is designed to illustrate the transfer of electrons while bonding. -2 -2 -2 Al+3 Al+3 O O O Aluminum Oxide Continued

  10. Naming Ionic Compounds Naming these compounds is straight forward. • ______________________ • ______________________ Examples – Sodium Chloride, Calcium Oxide

  11. The trick to finding the ratio of atoms in the molecule. The easiest way is to find the number of BONDS the ion will make is to again refer to your period table Writing the formulas for Ionic Compounds

  12. Number the groups 1-3 going from left to right (skip the Tansition Metals) Number the groups 1-3 going from right to left (skip the Nobel Gases) Writing the formulas for Ionic Compounds 1 2 3 2 1 3

  13. ______________________ ______________________ Writing the formulas for Ionic Compounds +1 +2 +3 -3 -2 -1

  14. Write out the atoms with their stable charge Al+3O-2 Cross over the numbers to the opposite atom (Criss-Cross Rule!) Al2O3 ____ Then …

  15. Criss-Cross Rule Example: Aluminum Chloride Step 1: Aluminum Chloride write out name with space Step 2: Al+3 Cl-1 write symbols & valence number Step 3: Al Cl 1 3 criss-cross valence number as subscripts Step 4: AlCl 3 combine as formula unit (“1” is never shown) - Reduce if possible

  16. Criss-Cross Rule Example: Magnesium Oxide Step 1: Magnesium Oxide Step 2: Mg+2 O-2 Step 3: Mg O 2 2 Step 4: Mg2O2 Step 5: MgO

  17. _____ When atoms get larger, their atomic structure can become more complex. This means that some atoms can have different numbers of valence electrons in different situations. For example if we look at the Lewis structure of Copper. It can have one valence electron or two valence electrons. Clearly, this atom can form more than one type of molecule. -2 -2 O O Cu Cu Cu+1 Cu+1 Cu+2 Multivalent Compounds

  18. In terms of naming these compounds, we need a method of distinguishing, CuO and Cu2O ______________________ ______________________ The roman numeral is only included if the metal is one of the atoms that can exhibit more than one charge. This information will be provided! e.g. Write the name for the following compounds, CuF Copper (I) Fluoride PbI2 ______________________ CaF2 ______________________ Multivalent Compounds

  19. How do we know which roman numeral is being used? • CuF • ______________________ • ______________________ • Cu 1 F1 Cu +1 F-1 • Copper (I) Flouride • PbI2 Pb 1 I2 Pb +2 I-1 • Lead (II) Iodide

  20. ________ • ________ • Be careful when you are asked to determine the roman numeral given the formula (e.g. CuS) • This would lead you to answer: Copper (I) Sulfide • However we ALWAYS NEED TO CHECK THAT THE CHARGE ON THE ANION IS CORRECT • In this case it would be -1 however, if we look at the periodic table we know that S is -2 • Therefore we need to multiply both charges by 2 • Copper (II) Sulfide • __________

  21. Ionic Compounds • Many ionic compounds are soluble in water. • When they dissolve, they separate into ions. • Water molecules surround each ion preventing it them from rejoining

  22. Ionic Compounds Properties • ______________________ • Many are also electrolytes which means they conduct electricity when dissolved in water • Pure water is a poor conductor of electricity, dissolved ions improve this property considerably

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