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Naming Ionic Compounds

Naming Ionic Compounds. Metals Joining with Nonmetals or Polyatomics. Ionic Compounds. Positive Ion is called a CATION . They are metals. Negative Ion is called an ANION . They are non-metals. Learning Check. Give the names of the following ions: Ba 2+ Al 3 + K +

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Naming Ionic Compounds

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  1. Naming Ionic Compounds Metals Joining with Nonmetals or Polyatomics

  2. Ionic Compounds • PositiveIon is called a CATION. They are metals. • Negative Ion is called an ANION. They are non-metals.

  3. Learning Check Give the names of the following ions: Ba2+ Al3+ K+ _________ __________ _________ N3 O2 F _________ __________ _________ P3 S2Cl _________ __________ _________

  4. Ionic Compounds • Notice the cross over of Charges • The Cation is always written FIRST, Anion Second. • Ionic compounds are made up of metals and non-metals, the metal is written FIRST.

  5. Formation of Ionic CompoundsCrossing Rule Ca+2+ Cl-1 CaCl2 But you MUST make sure to check to see if the whole number ratios can be REDUCED. If they can, you must reduce them.

  6. Example of reducing: • Cr4+ O2- • If you just cross you get Cr2O4 but this would NOT be the correct formula for chromium (IV) oxide. • The correct formula is CrO2

  7. Naming Rules • Step 1: The name of the metal is written first, the same way it is written on the periodic table • Step 2: Write the name of non-metal second, BUTchange the ending of the element to –ide. • Step 3: Remember the crossing rule and remember to reduce!

  8. Examples of Ionic Compounds with Two Elements Formula Ions Name Cation Anion NaCl Na+ Cl– sodium chloride K2S K+ S2– potassium sulfide MgO Mg2+ O2– magnesium oxide CaI2 Ca2+ I– calcium iodide Al2O3 Al3+ S2– aluminum sulfide

  9. Multiple Ionic Charges & Names • Some Transition metals can have more than one charge and therefore more than one name.

  10. How do I know if a metal is multi-valanced (mulitiple ionic charges)? • Look at you table of ions!

  11. Transition Metals Form Positive Ions Most transition metals andGroup 4(14) metals, • Form 2 or more positive ions • Zn2+,Ag+, and Cd2+ form only one ion.

  12. When writing the names • Write the name of the element followed by the Roman numeral. • EX: Cu2+ is written Copper(II) • So, what is the name of Fe3+? • How would you write the name of PbCl4?

  13. Metals with Variable Charge The names of transition metals with two or more positive ions (cations) use a Roman numeral after the name of the metal to identify ionic charge.

  14. Examples of Names of Compounds with Variable Charge Metals

  15. Naming FeCl2 STEP 1 Determine the charge of the cation from the anion. Fe ion + 2 Cl– = Fe ion + 2– = 0 Fe ion = 2+ = Fe2+ STEP 2 Name the cation by the element name, and use a Roman numeral to show its charge. Fe2+ = iron(II) STEP 3Write the anion with an ide ending. chloride STEP 4Name the cation first, then the anion. iron(II) chloride

  16. Naming Cr2O3 STEP 1Determine the charge of cation from the anion. 2Cr ions + 3O2– = 2Cr ions + 3(2–) = 2Cr ions + 6– = 0 2Cr ions = 6+ Cr ion = 3+ = Cr3+ STEP 2Name the cation by the element name, and use a Roman numeral to show its charge. Cr3+ = chromium(III) STEP 3Write the anion with an ide ending.oxide STEP 4Name the cation first, then the anion. chromium (III) oxide

  17. Polyatomic Ionic Compounds What is a polyatomic ion? Polyatomic ions: groups of atoms that tend to stay together and carry an overall ioniccharge. They still need two parts!

  18. Table of Common Polyatomic Ions

  19. Polyatomic Compound Formulas • Formulas for polyatomic compounds is determined the same way as ionic compounds. Cation first, Anion second, cross over rule • But… brackets may be required!!! Al+3 + CO3-2 Al2(CO3)

  20. Ammonium Ion • The only positively charged polyatomic ion. • NH4+ ammonium ion • Ammonium nitrate : ammonium ion NH4+ nitrate ion NO3- • NH4NO3 • Because this ion has a positive charge, it WILL come first.

  21. Naming Polyatomic Compounds • Step 1: Write the name of the metal first. • Step 2: Write the name of the polyatomic ion second. • NaH2CO3 • Sodium hydrogen carbonate or sodium bicarbonate NOT sodium hydrogen carbon oxide!!!!!!!

  22. Hydrates A hydrate is a compound that has a specific number of water molecules within its solid structure. For example, in its normal state, copper(II) sulfate has five water molecules associated with it. Systematic name: copper(II) sulfate pentahydrate Formula: Cu(SO)4 ∙ 5H2O Some other hydrates are BaCl2 ∙ 2H2O LiCl ∙ H2O MgSO4 ∙ 7H2O Sr(NO3)2 ∙ 4H2O

  23. Hydrates When the water molecules are driven off by heating, the resulting compound, Cu(SO)4, is sometimes called anhydrous copper(II) sulfate. Anhydrous means the compound no longer has water molecules associated with it.

  24. Familiar Inorganic Compounds

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