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Naming and Formulating Ionic Compounds

This guide explains the process of naming and determining the formulas of ionic compounds. For monoatomic anions, drop the suffix and add “-ide”. Cations retain their element name, with the cation named first followed by the anion. Neutrality in ionic compounds is key; the lowest ratio of each ion is required for charge balance. Common ions like sodium (Na+), chloride (Cl-), and polyatomic ions are discussed, with emphasis on recognizing and naming them correctly. Examples, including transition metals with multiple charges, are provided for clarity.

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Naming and Formulating Ionic Compounds

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  1. Naming and determining the formula of ionic compounds

  2. Naming ionic compounds • For monoatomic anions only • drop the ending and add “-ide” • so F- • fluoride • Cl-, O2-, C4- • chloride, oxide and carbide

  3. Continuing… • cations keep the name of the element. • When naming compounds always name the positive (cation) first and the negative (anion) last. • so mixing ions of chlorine and sodium give you • sodium chloride • (positive) (negative)

  4. Determining the formula of ions • Ionic compounds are neutral • You need to find the lowest number of each ion to make it neutral • for example: • Na+ and O2- • 2 sodium for every one oxygen • Na2O

  5. More examples • Al3+ and O2- • Al2O3 • K+ andCl- • KCl • the subscripts don’t effect the name if there is only one possibility • still (cation)(anion) • Aluminum oxide • Potassium chloride

  6. Several atoms can form a couple of different ions. • These are all metals that aren’t in group 1, 2 or aluminum. • for example iron can form Fe2+ or Fe3+ • These are said as iron (II) and iron (III) • Cu+ and Cu2+ is Copper (I) and Copper (II)

  7. Figuring out charge on these elements • If the ion is named, the charge is in the name. • If you have the formula, use the charges of the other ions present to determine the charge. • Remember • Alkali will always be +1 • Alkaline Earth +2, Halogens -1, oxygen group -2 • Aluminum will always be +3

  8. Examples • Copper (II) chloride • CuCl2 • Cobalt (III) sulfide • Co2S3 • NiF2 • Nickel (II) fluoride • Ag2S • Silver (I) sulfide

  9. Polyatomic ions • Polyatomic Ions- many atoms in one ion • You can NOT break these apart in this section. • the “ide” suffix only applies to monoatomic anions

  10. Common polyatomic ions

  11. Don’t worry you don’t have to memorize them!! • They are given to you for tests. • You will however have to be able to recognize them with the list. • You have to look at polyatomic ions like they are one thing. • Don’t alter their formula in anyway

  12. Determining the formula of ions • Ionic compounds are neutral • Remember-- you cannot break a polyatomic ion apart • for example: Ammonium carbonate • NH4+ and CO32- • (NH4)2CO3

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