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Chemistry I Honors/ACP C101-121 Unit 5: Chemical Nomenclature

Chemistry I Honors/ACP C101-121 Unit 5: Chemical Nomenclature. Objective #1: Classification of Chemical Compounds. Objective #2: Binary Ionic Compounds. Review of common charges:. Objective #2 Binary Ionic Compounds. Naming involves: 1. Name the metal

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Chemistry I Honors/ACP C101-121 Unit 5: Chemical Nomenclature

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  1. Chemistry I Honors/ACP C101-121Unit 5: Chemical Nomenclature

  2. Objective #1: Classification of Chemical Compounds

  3. Objective #2:Binary Ionic Compounds Review of common charges:

  4. Objective #2Binary Ionic Compounds • Naming involves: 1. Name the metal 2. Name the nonmetal, adding -ide ending • Examples: CsF: ___________________ ZnS: ______________________ MgF2: _____________________ Li2O: _________________________ *Note that the subscript in the formula has nothing to do with the name!! • Some traditional transition metal ion names use the suffixes “-ic” and “-ous”

  5. Objective #2 Binary Ionic Compounds What pattern do you notice? Iron (II) ferrous Iron (III) ferric Tin (II) stannous Tin (IV) stannic Lead (II) plumbous Lead (IV) plumbic Copper (I) cuprous Copper (II) cupric -ic is always the suffix of the ion with the highercharge

  6. Objective #2 Binary Ionic Compounds • If the metal ion present is a transition metal, then the charge of the transition metal must be indicated by a Roman Numeral (Stock System) • Special Cases: • Silver and Gold are usually +1 and do not get a Roman Numeral…but always double check!!! ;) • Zinc is always +2, so it does not need a Roman Numeral • Lead and Tin are transition metals “wannabes”, so they need Roman numerals as there are two versions • Mercury (I) ion formula is Hg+2+2 • Mercury (II) ion formula is Hg+2 Mercury I has the 2, Mercury II has no 2!!!

  7. Objective #2 Binary Ionic Compounds • Examples: Fe2S3: ___________________ Cu2O: ___________________ CrCl3 :___________________ SnF2: ____________________ Hg2Cl2: __________________

  8. Writing formulas involves: 1. Write down formula of cation 2. Write down formula of anion 3. Determine charges of ions 4. Use subscripts to balance charges back to zero • Examples:

  9. Objective #3 Binary Molecular Formulas • Binary Molecular Compounds contain 2 nonmetals • “Fake Greek” prefixes are used to indicate the number of each atom present

  10. Objective #3 Binary Molecular Formulas • Naming involves: 1. Name first element normally; prefix used only if more than one atom of element is used 2. Name second element adding ide ending; prefix is always used, regardless of number of atoms present • Examples of naming and writing formulas

  11. Objective #4 Ternary Ionic Compounds • Follow the same pattern as other ionics, BUT make sure the PAI is written in parentheses, so the charge is isolated!! • Examples:

  12. Objective #5: Formulas of Acids • Examples: Hydrofluoric Acid: Sulfurous Acid: Nitric Acid: What do these acids have in common?

  13. Binary acids are named using the prefix hydro- and adding the suffix -ic to the second element • All other acids are named by the polyatomic ion they contain and then changing the ending as follows: - ate becomes –ic - ite becomes –ous • Examples: Something I “ate” made me “sick” Take a “bite” , its “delcious”

  14. Objective #5 Acid-Base Characteristics and Definitions

  15. Objective #5 Acid-Base Characteristics and Definitions Acid-Base Theories • The Arrhenius Definition of Acids and Bases • Arrhenius acid: A substance that increases the number of hydrogenions in water solution • Arrhenius base: A substance that increases the number of hydroxideions in water solution

  16. Objective #5 Acid-Base Characteristics and Definitions • Examples: HCl(aq)H+1 (aq)+ Cl-1 (aq) NaOH(aq)Na+1 (aq)+ OH-1 (aq)

  17. Objective #5 Acid-Base Characteristics and Definitions The Bronsted-Lowery Definition of Acids and Bases • A broader definition for acids and bases • All Arrhenius acids are also Bronsted-Lowery acids • Not all Arrhenius bases are also Bronsted-Lowery bases • A Bronsted-Lowery acid is a substance that accepts protons • A Bronsted-Lowery base is a substance that accepts protons

  18. Objective #5 Acid-Base Characteristics and Definitions • Examples: HCl + H2O H3O+1 (aq)+ Cl-1 (aq) NH3 + H2O NH4+1 (aq)+ OH-1 (aq)

  19. Objective #5 Acid-Base Characteristics and Definitions Bronsted-Lowery Acid/Base Pairs • After an acid donates a proton, the species that remains is referred to as a conjugate base; this designation is given because the new species is now eligible to accept a proton • After a base accepts a proton, the species that remains is referred to as a conjugate acid; this designation is given because the new species is now eligible to donate a proton

  20. Objective #5 Acid-Base Characteristics and Definitions • Example: NH3 + H2O  NH4+1 + OH- acid basecon. acid con. base • A conjugate acid-base pair always differs by a proton

  21. For each of the following acid-base reactions, identify the acid-base pairs: • Examples: • The ability of a substance to act as either an acid, a base, or both depends on the extent that a substance can donate or accept protons (this will be explored further later in the year)

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