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Mastering Ionic and Covalent Compound Naming: A Comprehensive Guide

This guide covers the systematic naming of ionic and covalent compounds, including exceptions and special cases involving transition metals and acids. For ionic compounds, we explain how to name Type I compounds using the metal first followed by the nonmetal with an "-ide" suffix, while addressing polyatomic ions. For Type II ionic compounds, we illustrate how to include Roman numerals to denote varying charges of transition metals. Additionally, we delve into naming covalent compounds using prefixes to indicate atom counts, along with clear examples.

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Mastering Ionic and Covalent Compound Naming: A Comprehensive Guide

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  1. Compound names & Formulas Chapter 5

  2. Naming Ionic Compounds(Type I) • The metal is always named first and the nonmetal second • The name of the first symbol takes its name from the name of the element. Example: Na+ is called sodium • The name of the second symbol takes the first part of the element name and adding an –ide. Example: Cl- is called chloride

  3. Naming Ionic Compounds(Type I) • Exceptions!!! • Polyatomic ions already have specific names, so just name them that way. • Example: NH4+ is called ammonium

  4. Name the following • CaCl2: • Al2O3: • BaF2: • Li2O: • CaCO3: • KNO3: • NaF:

  5. Naming Covalent Compounds (Type III) • These contain only NONMETALS • The first element in the formula is named first and the full name is used. • The second element’s name ends in –ide. • Prefixes are used to denote the numbers of atoms present.

  6. Naming Covalent Compounds (Type III) • Prefixes mono 1 hexa 6 di 2 hepta 7 tri 3 octa 8 tetra 4 nona 9 penta 5 deca 10

  7. Name the following • BF3: • N2O4: • H2O: • CO2: • SiI4: • PCl3:

  8. Naming Ionic Compound w/ Transition Metals (Type II) • The metal is always named first and the nonmetal named second • Because the metal can assume more than one charge, is specified by a Roman in parentheses • Example: FeCl2 = Iron(II) chloride HINT: the number after the nonmetal usually becomes the Roman numeral

  9. Name the following • CuCl: • HgO: • Fe2O3: • MnO4: • PbCl4:

  10. Writing Ionic Formulas(swap and drop) • The (+) ion is written first, then the (-) ion • Find the charges of the ions -Look at the group # -Look at the roman numeral after the element (transition metals) • Write ions and their charges • Swap & drop charges, making them subscripts.

  11. Examples • Magnesium chloride • Aluminum oxide

  12. Examples: • Calcium sulfide • Lead (IV) oxide

  13. Examples: • Sodium sulfate • Ammonium carbonate

  14. Naming Acids • Acids contain hydrogen (H+ ions in solution) • ALL compounds beginning with hydrogen are acids • To name acids, you have to look at the anion (negative one!)

  15. Acid contains no oxygen • Acid begins with hydro- • Ends in –ic • The middle contains the base name of the anion Hydro_(anion)_ic • Example: HCl = Hydrochloric acid

  16. Acid contains oxygen • Check the name of the anion (it will be a polyatomic ion) • If it ends in –ite (i.e. nitrite) - use the root name of the polyatomic ion - ends in –ous • Example: HNO2 = Nitrous Acid

  17. Acid contains oxygen • If it ends in –ate (i.e. nitrate) -use the root name of the polyatomic ion -ends in –ic • Example: HNO3 = Nitric Acid

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