1 / 40

SKILLS Project

SKILLS Project. Naming and Building Ionics (I). What are ionic compounds?. Remember, this unit only applies to the naming and construction of ionic compounds. Ionic compounds are almost always made of a METAL and a NON-METAL.

gabi
Download Presentation

SKILLS Project

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. SKILLS Project Naming and Building Ionics (I)

  2. What are ionic compounds? • Remember, this unit only applies to the naming and construction of ionic compounds. • Ionic compounds are almost always made of a METAL and a NON-METAL. • Remember, you can determine whether something is a metal or non-metal based on their position on the periodic table.

  3. Naming Ionic Compounds • Ionic nomenclature is fairly simple and follows the following steps: • The positive ion or ions are always named first (typically a metal or metals.) • The anion is named second, but drops its suffix and typically ends in –ide. • Polyatomics (larger ions with specific names) do not undergo a change to their names when used in compounds. • Refer to the next slide for a complete list of useful polyatomics and associated charges.

  4. Polyatomic Ions • NO31- - Nitrate • NO21- - Nitrite • SO42- - Sulfate • SO32- - Sulfite • PO43- - Phosphate • PO33- - Phosphite • OH1- - Hydroxide • CO32- - Carbonate • NH41+ - Ammonium • C2H3O21- - Acetate

  5. CN1- - Cyanide • MnO41- - Permanganate • ClO41- - Perchlorate • ClO31- - Chlorate • ClO21- - Chlorite • C2O42- - Oxalate • IO31- - Iodate • BrO31- - Bromate • CrO42- - Chromate • Cr2O7-2 - Dichromate • O22- - Peroxide • N31- - Azide • AsO43- - Arsenate • S2O32- - Thiosulfate

  6. Example 1: Li2S Sulfide Lithium Sulfur Replace the last syllable of the anion with –ide. Remember, we don’t do this for polyatomic ions. Name the non-metal or anion second. Typically, this will be at the end of the compound. Name the metal or positive ion first. These are usually at the beginning of the compound as well.

  7. Example 2: MgO Oxide Magnesium Oxygen Replace the last syllable of the anion with –ide. Remember, we don’t do this for polyatomic ions. Name the non-metal or anion second. Typically, this will be at the end of the compound. Name the metal or positive ion first. These are usually at the beginning of the compound as well.

  8. Example 3: Na3P Phosphide Sodium Phosphorous Replace the last syllable of the anion with –ide. Remember, we don’t do this for polyatomic ions. Name the non-metal or anion second. Typically, this will be at the end of the compound. Name the metal or positive ion first. These are usually at the beginning of the compound as well.

  9. Example 4: Ca2C Carbide Calcium Carbon Replace the last syllable of the anion with –ide. Remember, we don’t do this for polyatomic ions. Name the non-metal or anion second. Typically, this will be at the end of the compound. Name the metal or positive ion first. These are usually at the beginning of the compound as well.

  10. Example 5: Ba3N2 Nitride Barium Nitrogen Replace the last syllable of the anion with –ide. Remember, we don’t do this for polyatomic ions. Name the non-metal or anion second. Typically, this will be at the end of the compound. Name the metal or positive ion first. These are usually at the beginning of the compound as well.

  11. Example 6: (NH4)2S Sulfide Ammonium Sulfur Replace the last syllable of the anion with –ide. Remember, we don’t do this for polyatomic ions. Name the non-metal or anion second. Typically, this will be at the end of the compound. Name the metal or positive ion first. These are usually at the beginning of the compound as well. Note: Even though this compound is made up only of non-metals, the bond between the ammonium and sulfur is actually ionic due to the charges.

  12. Example 7: MgCO3 Magnesium Carbonate We don’t need to replace the ending of the polyatomic “carbonate” with –ide. Remember, we don’t need to change polyatomics when writing ionic names. Name the non-metal or anion second. Typically, this will be at the end of the compound. Name the metal or positive ion first. These are usually at the beginning of the compound as well.

  13. Example 8: NH4C2H3O2 Ammonium Acetate Hint: the challenge with working with polyatomics is recognizing them. As a rule, look for polyatomics when a compound contains 3 or more different elements. We don’t need to replace the ending of the polyatomic “acetate” with –ide. Remember, we don’t need to change polyatomics when writing ionic names. Name the non-metal or anion second. Typically, this will be at the end of the compound. Name the metal or positive ion first. These are usually at the beginning of the compound as well.

  14. Example 9: K2Cr2O7 Potassium Dichromate We don’t need to replace the ending of the polyatomic “dichromate” with –ide. Remember, we don’t need to change polyatomics when writing ionic names. Name the non-metal or anion second. Typically, this will be at the end of the compound. Name the metal or positive ion first. These are usually at the beginning of the compound as well.

  15. Example 10: CsClO4 Cesium Perchlorate We don’t need to replace the ending of the polyatomic “perchlorate” with –ide. Remember, we don’t need to change polyatomics when writing ionic names. Name the non-metal or anion second. Typically, this will be at the end of the compound. Name the metal or positive ion first. These are usually at the beginning of the compound as well.

  16. Practice on Your Own: • Na3PO4 - • BaCl2 - • NaI - • LiIO3 - • Sr(NO3)2 - • NaH - • (NH4)2Se - • MgSO4 - • CsCN - • H3AsO4 - Sodium phosphate Barium chloride Sodium iodide Lithium iodate Strontium nitrate Sodium hydride Ammonium selenide Magnesium sulfate Cesium cyanide Hydrogen arsenate

  17. Building Ionic Compounds • To build your compound, you will need to do five things: • Place the metal or positive ion in front of the non-metal or negative ion. • Use the periodic table or a chart to find the charges of each element. Ionics are made of “ions” or charged particles. • Swap the charges and drop them below the elements or ions they represent. • Remove the plus and minus signs- these numbers are no longer being used as charges. • Simplify, if needed.

  18. Ex. 11: Oxygen and Magnesium O Mg 2- 2+ O Mg MgO Note: We never write “1” as a subscript. The presence of the symbol indicates that at least one is present already. Done! You’ve just built magnesium oxide. Both subscripts may be divided by 2 to simplify. 1 2 1 2 • Simplify, if needed. Place the metal or positive ion in front of the non-metal or negative ion. • Remove the plus and minus signs- these numbers are no longer being used as charges. • Swap the charges and drop them below the elements or ions they represent. • Use the periodic table or a chart to find the charges of each element. Ionics are made of “ions” or charged particles.

  19. Ex. 12: Sodium and Phosphorous Na P 3- 1+ P Na Na3P Note: We never write “1” as a subscript. The presence of the symbol indicates that at least one is present already. Done! You’ve just built sodium phosphide. The subscripts cannot be simplified any further (divided by a common number). 1 3 • Simplify, if needed. Place the metal or positive ion in front of the non-metal or negative ion. • Remove the plus and minus signs- these numbers are no longer being used as charges. • Swap the charges and drop them below the elements or ions they represent. • Use the periodic table or a chart to find the charges of each element. Ionics are made of “ions” or charged particles.

  20. Ex. 13: Iron (III) and Sulfur S Fe 2- 3+ S Fe Fe2S3 Neither subscript may be divided by a common factor. Done! You’ve just built Iron (III) sulfide 2 3 • Simplify, if needed. Place the metal or positive ion in front of the non-metal or negative ion. • Remove the plus and minus signs- these numbers are no longer being used as charges. • Swap the charges and drop them below the elements or ions they represent. • Use the periodic table or a chart to find the charges of each element. Ionics are made of “ions” or charged particles.

  21. Ex. 14: Barium and Fluorine Ba F 1- 2+ F Ba BaF2 Note: We never write “1” as a subscript. The presence of the symbol indicates that at least one is present already. Done! You’ve just built barium fluoride. Neither subscript may be simplified any further. 2 1 • Simplify, if needed. Place the metal or positive ion in front of the non-metal or negative ion. • Remove the plus and minus signs- these numbers are no longer being used as charges. • Swap the charges and drop them below the elements or ions they represent. • Use the periodic table or a chart to find the charges of each element. Ionics are made of “ions” or charged particles.

  22. Ex. 15: Vandium (IV) and Selenium V Se 2- 4+ Se V VSe2 Note: We never write “1” as a subscript. The presence of the symbol indicates that at least one is present already. Both subscripts may be divided by 2 to simplify. Done! You’ve just built vanadium (IV) selenide. 4 1 2 2 • Simplify, if needed. Place the metal or positive ion in front of the non-metal or negative ion. • Remove the plus and minus signs- these numbers are no longer being used as charges. • Swap the charges and drop them below the elements or ions they represent. • Use the periodic table or a chart to find the charges of each element. Ionics are made of “ions” or charged particles.

  23. Practice on Your Own: • Iridium (III) Iodide – • Sodium Silicide – • Calcium Nitride – • Lithium Oxide – • Zinc (II) Phosphide – • Iron (II) Oxide – • Calcium Carbide – • Manganese (VII) Nitride – • Cesium Selenide – • Strontium Bromide – IrI3 Na4Si Ca3N2 Li2O Zn3P2 FeO Ca2C Mn3N7 Cs2Se SrBr2

  24. Working with Polyatomics • Remember, polyatomics are a series of charged particles (ions) made up of more than one atom. Hence poly- (many), -atomic (atoms) means “many atoms.” For Example, Carbonate Ion: (CO3)2- CO32- = The (2-) charge applies to the ENTIRE polyatomic. So, when you “swap and drop,” you will be doing so to the entire thing all at once.

  25. Ex. 16: Ammonium and Carbonate NH41+ CO32- Note: We never write “1” as a subscript. The presence of the symbol indicates that at least one is present already. Also, you can remove the parenthesis in this case. 2- 1+ Done! You’ve just built ammonium carbonate (CO3) (NH4)2CO3 (NH4) Neither subscript may be simplified any further. 2 1 • Simplify, if needed. Place the metal or positive ion in front of the non-metal or negative ion. • Remove the plus and minus signs- these numbers are no longer being used as charges. • Swap the charges and drop them below the elements or ions they represent. • Use the periodic table or a chart to find the charges of each element. Ionics are made of “ions” or charged particles.

  26. Ex. 17 : Lead (III) and Dichromate Pb3+ Cr2O72- 2- 3+ Done! You’ve just built ammonium carbonate (Cr2O7) Pb2(Cr2O7)3 Pb Neither subscript may be simplified any further. 2 3 • Simplify, if needed. Place the metal or positive ion in front of the non-metal or negative ion. • Remove the plus and minus signs- these numbers are no longer being used as charges. • Swap the charges and drop them below the elements or ions they represent. • Use the periodic table or a chart to find the charges of each element. Ionics are made of “ions” or charged particles.

  27. Ex. 18 : Sodium and Oxalate Na C2O42- Note: We never write “1” as a subscript. The presence of the symbol indicates that at least one is present already. Also, you can remove the parenthesis in this case. 2- 1+ Done! You’ve just built sodium oxalate. (C2O4) Na2C2O4 Na Neither subscript may be simplified any further. 2 1 • Simplify, if needed. Place the metal or positive ion in front of the non-metal or negative ion. • Remove the plus and minus signs- these numbers are no longer being used as charges. • Swap the charges and drop them below the elements or ions they represent. • Use the periodic table or a chart to find the charges of each particle. Ionics are made of “ions” or charged particles.

  28. Ex. 19 : Lead (IV) and Sulfate Pb4+ SO42- Note: We never write “1” as a subscript. The presence of the symbol indicates that at least one is present already. Also, you can remove the parenthesis in this case. 2- 4+ Done! You’ve just built lead (IV) sulfate. (SO4) Pb(SO4)2 Pb Both subscripts may be divided by 2. 1 2 2 4 • Simplify, if needed. Place the metal or positive ion in front of the non-metal or negative ion. • Remove the plus and minus signs- these numbers are no longer being used as charges. • Swap the charges and drop them below the elements or ions they represent. • Use the periodic table or a chart to find the charges of each particle. Ionics are made of “ions” or charged particles.

  29. Ex. 20 : Iron (III) and Arsenate Fe3+ AsO43- Note: We never write “1” as a subscript. The presence of the symbol indicates that at least one is present already. Also, you can remove the parenthesis in this case. 3- 3+ Done! You’ve just built iron (III) arsenate. (AsO4) FeAsO4 Fe Both subscripts may be divided by 3. 1 3 1 3 • Simplify, if needed. Place the metal or positive ion in front of the non-metal or negative ion. • Remove the plus and minus signs- these numbers are no longer being used as charges. • Swap the charges and drop them below the elements or ions they represent. • Use the periodic table or a chart to find the charges of each particle. Ionics are made of “ions” or charged particles.

  30. A quick note: • Going from names to formulas follows a fairly easy and consistent pattern. • However, going from formulas to names can prove tricky if transition metals are involved. • REMEMBER: always find the charge of a transition metal (virtually any metal that is NOT in the “s” block (groups 1 and 2) and place it as a roman numeral in your compound’s name.) • Watch out for simplification! You may have to reverse this to find the actual charge of a transition metal.

  31. Quick tip! • When reversing a “swap and drop,” be careful not to accidentally use a subscript that is part of a polyatomic. • For example: FeNO3 You can prevent these mistakes quite easily by putting your polyatomics in parentheses when you see them and before you do any “swapping and dropping” - like this: 3+ 1- 1+ 1- Fe1(NO3)1 Fe (NO) Fe (NO3) FeNO3

  32. Practice on Your Own: • Lead (IV) chlorite - • Cesium phosphate - • Ammonium sulfate - • Ammonium sulfide - • Ammonium sulfite - • La(ClO4)3 - • Fe3PO4 - • Ag2CO3 - • V(C2H3O2)5 - • CuSO3 - Pb(ClO2)4 Cs3PO4 (NH4)2SO4 (NH4)2S (NH4)2SO3 Lanthanum (III) perchlorate Iron (I) phosphate Silver (I) carbonate Vanadium (V) acetate Copper (II) sulfite

  33. Advanced Practice • The slides that follow deal with naming and determining formulas under a variety of conditions. Remember: • Transition metals are given their charges with a roman numeral. This must be shown in naming them. • If you are using names to find formulas, be careful. You may have to reverse simplifications to find the true charges of transition metals. • Polyatomics are given specific names that should not be altered. • These problems are excellent practice and should be worked through carefully.

  34. Example 21: Name Fe2O3 Iron (?) Oxide 2- 3+ FeO Iron (III) Oxide 2 3 Finally, ask yourself if these numbers have been simplified. The oxygen is “-2” as we expect. This means that no simplification has occurred and that we can assume iron has a 3+ charge. After checking our work, we can conclude that the charge on iron is +3 this time, so we use iron (III) in the name. To find the charge of the iron we will have to reverse the “swap and drop” we normally do when creating formulas. First, name the cation and anion, in order. Note that iron, Fe, is a transition metal. We will have to find the original charge of the iron to finish this name. Now that the charges are back, they can be made + and – again.

  35. Example 22: Name FeO Iron (?) Oxide 2- 2+ 1- 1+ FeO Iron (II) Oxide 1 1 Finally, ask yourself if these numbers have been simplified. The oxygen is “-1” while we know it should be “-2”. This means that both charges were divided by 2 to simplify at some point. Multiply by 2 to reverse the simplification and find the original charges that were given to iron and oxygen. To find the charge of the iron we will have to reverse the “swap and drop” we normally do when creating formulas. After checking our work, we can conclude that the charge on iron is +2 this time, so we use iron (II) in the name. First, name the cation and anion, in order. Note that iron, Fe, is a transition metal. We will have to find the original charge of the iron to finish this name. Now that the charges are back, they can be made + and – again.

  36. Example 23: Name Mn(CrO4)2 Manganese (?) Chromate 2- 4+ 1- 2+ Mn(CrO4) Manganese (IV) Chromate 1 2 Finally, ask yourself if these numbers have been simplified. The chromate is “-1” while we know it should be “-2”. This means that both charges were divided by 2 to simplify at some point. Multiply by 2 to reverse the simplification and find the original charges that were given to manganese and chromate. To find the charge of the manganese we will have to reverse the “swap and drop” we normally do when creating formulas. After checking our work, we can conclude that the charge on Mn is +4 this time, so we use manganese (IV) in the name. First, name the cation and anion, in order. Note that manganese, Mn, is a transition metal. We will have to find the original charge of the Mn to finish this name. Now that the charges are back, they can be made + and – again.

  37. Example 24: Name Cu2SO3 Copper (?) Sulfite 2- 1+ Cu(SO3) Copper (I) Sulfite 2 1 Finally, ask yourself if these numbers have been simplified. The sulfite is “-2” while we know it should be “-2”. This means that simplification has not occurred. To find the charge of the copper we will have to reverse the “swap and drop” we normally do when creating formulas. After checking our work, we can conclude that the charge on Cu is +1 this time, so we use copper (I) in the name. First, name the cation and anion, in order. Note that copper, Cu, is a transition metal. We will have to find the original charge of the Cu to finish this name. Now that the charges are back, they can be made + and – again.

  38. Example 25: Name VPO4 Vanadium (?) Phosphate 3- 3+ 1- 1+ V(PO4) Vanadium (III) Phosphate 1 1 First, name the cation and anion, in order. Note that vanadium, V, is a transition metal. We will have to find the original charge of the vandadium to finish this name. Finally, ask yourself if these numbers have been simplified. The phosphate is “-1” while we know it should be “-3”. This means that both charges were divided by 3 to simplify at some point. Multiply by 3 to reverse the simplification and find the original charges that were given to vanadium and phosphate. To find the charge of the vanadium we will have to reverse the “swap and drop” we normally do when creating formulas. After checking our work, we can conclude that the charge on vanadium is +3 this time, so we use vanadium (III) in the name. Now that the charges are back, they can be made + and – again.

  39. Practice on Your Own • Fe3AsO4 - • CuF - • Pb(NO3)2 - • Ir(Cr2O7)3 - • Zr(S2O3)2 - • Ag2C2O4 - • Ti(CN)4 - • Ga2(SO4)3 - • WCrO4 - • (NH4)3PO3 - Iron (I) arsenate Copper (I) fluoride Lead (II) nitrate Iridium (VI) dichromate Zirconium (IV) thiosulfate Silver (I) oxalate Titanium (IV) cyanide Gallium (III) sulfate Tungsten (II) chromate Ammonium phosphite

  40. Excellent! • If you’ve made it this far, you should have virtually complete mastery of chemical nomenclature. • Congratulations!

More Related