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Naming Ionic Compounds

Naming Ionic Compounds. The Big Idea in Naming Ionic Compounds . Every compound needs to have a unique name. This is accomplished by naming the two ions that make up the compound. By identifying both the metal ion and the non-metal ion, the compound is identified. Identifying metal ions.

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Naming Ionic Compounds

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  1. Naming Ionic Compounds

  2. The Big Idea in NamingIonic Compounds Every compound needs to have a unique name. This is accomplished by naming the two ions that make up the compound. By identifying both the metal ion and the non-metal ion, the compound is identified.

  3. Identifying metal ions The metal ions (or cations) that form the positive ions are given the same name as the atoms they are formed from. When writing the symbol for an ion, it is very important to show the charge to differentiate it from its atom. Example: Na = Sodium atom Na + = Sodium ion

  4. Identifying non-metal ions The non-metal ions (or anions) that are formed when an atom accepts electrons are distinguished from their atoms by the “ide” ending. When writing the symbol for an ion, it is very important to show the charge to differentiate it from its atom. Example: Cl = Chlorine atom Cl - = Chloride ion

  5. When in Rome, do as the Romans do! The elements from “Rome” form ions that do not necessarily follow the octet rule. The charge on a particular ion is indicated using a Roman numeral.

  6. Examples from “Rome” Atoms from Rome can form more than one ion. This requires a way of telling the ions apart. This is done by using Roman numerals to tell the different ions apart. The Roman numeral indicates the charge on the ion. This method of using Roman numerals to indicate the charge is called the Stock system and is used only for atoms that form more than one ion.

  7. Complete the following Table: Mercury (II) Cr 3+ Mn 2+ Manganese (III) Ba 2+ Au 3+ Cobalt (III) K + Lithium Titanium (II)

  8. You Try! Write the formulas for the following: • Chromium (III) chloride • Barium bromide • Iron (III) sulfide • Copper (I) oxide • Potassium oxide Note: atoms that are not from “Rome” do not use Roman numerals.

  9. Finding the charge on the metal ion • In order to use the Stock system we must know the charge on the metal ion. This can be determined by using the charge on the negative ion and remembering that the sum of the charges on all the ions in a compound must be zero.

  10. Naming compounds using the Stock System The Stock system is important in naming compounds formed from elements that form more than one type of ion.

  11. You Try! Write the names for the following compounds: • MnO • NiBr2 • Cu2S • SnCl4 • BaCl2 Manganese (II) oxide Nickel (II) Bromide Copper (I) sulfide Tin (IV) chloride CrCl3 Cu I2 HgCl2

  12. More on Negative ions So far we’ve used “ide” endings to indicate a negative ion. However, there are other kinds of negative ions that have different endings:

  13. Table E – Selected Polyatomic Ions Reference Table E provides a list of the names and formulas for common polyatomic ions.

  14. Complete the following table: Cl - _nitride_ NO3 - sulfide_ sulfate_ SO32- Oxide F - NO2 - Hydrogen carbonate

  15. Use Table E to identify the following polyatomic ions • Nitrate • Sulfate • Phosphate • chlorate • Nitrite • Sulfite • Phosphite • chlorite

  16. Let’s review! • The names of the metal ions are the same as their atoms. • When a metal atom forms more than one ion, a Roman numeral is used to indicate the charge on the ion. • Most monatomic negative ions end in “ide”. • Polyatomic negative ions end in “ate” or “ite”. The names and formulas of these ions can be found in Table E.

  17. The Crossover Rule re-visited Once the ions making up a compound have been identified, the formula for the compound can be easily determined using the crossover rule. For instance: copper (II) acetate is made up of Cu 2+ ions and acetate ions (C2H3O2– ions). Since the atoms in the polyatomic ion are bonded together they will act as a single unit.

  18. Reality check! Write the formulas for the following compounds: • barium nitrate ________ • tin (II) chloride ________ • sodium sulfate ________ • copper (II) oxide ________ • copper (I) oxide ________ • iron (III) sulfide ________ • potassium chlorate ________ • silver (I) nitrate ________ • lead (IV) bromide ________ • sodium phosphate ________

  19. Complete the following: KCl Calcium chloride MnCl2 MnCl3 BaO Sodium sulfate CuSO4 Copper (I) sulfate Mg(NO3)2 Calcium acetate

  20. Things to think about • Why is KCl called potassium chloride when CuCl is called copper (I) chloride? • Why is sodium nitrate written as NaNO3 (no parenthesis) while magnesium nitrate is written as Mg(NO3)2 (with parenthesis)? • Why would it be incorrect to refer to FeO as simply iron oxide? • Most polyatomic ions are negative, but some positive ions exist. See if you can find the positive ions in Table E and list them. K only forms a 1+ ion, while Cu can form a 1+ or a 2+ ion. Therefore you need the Roman numeral to identify which ion is in the compound Parentheses are required when there is more than one polyatomic ion to indicate that are multiple numbers of the whole ion. Fe2O3 and FeO are both iron oxide. Need a unique name. Ammonium NH4+ Hydronium H3O+

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