Chemical Names

1. Chemical Names H Chemistry I Unit 5

2. Objective #1 Classification of Chemical Compounds

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

4. Objective #2 Binary Ionic Compounds *naming involves: 1. Name the metal 2. Name the nonmetal adding ide ending

5. Objective #2 Binary Ionic Compounds *examples: CsF____________ ZnS____________ MgF2______________ Li2O_______________ *some traditional transition metal ion names:

6. Objective #2 Binary Ionic Compounds Iron (II) ferrous Iron (III) ferric Tin (II) stannous Tin (IV) stannic Lead (II) plumbous Lead (IV) plumbic Copper (I) cuprous Copper (II) cupric

7. Objective #2 Binary Ionic Compounds *if the metal ion present is a transition metal than 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 Zinc is always +2 and does not get a Roman Numeral Lead and Tin are not transition metals but they do get Roman numerals mercury (I) ion formula is Hg2+2 mercury (II) ion formula is Hg+2

8. Examples of Naming Binary Ionic Chemicals Fe2S3 iron sulfide *transition element; needs Roman numeral *charge on iron +3 iron (III) sulfide

9. Cu2O copper oxide *transition element; needs Roman numeral *charge of copper is +1 copper (I) oxide

10. CrCl3 chromium chloride *transition element; needs Roman numeral *charge of chromium is +3 chromium (III) chloride

11. SnF2 tin fluoride *not transition but still needs Roman numeral *charge on tin is +2 tin (II) fluoride

12. Hg2Cl2 mercury (I) chloride

13. Objective #2 Binary Ionic Compounds *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

14. Examples of Writing Binary Ionic Formulas potassium fluoride KF sodium fluoride NaF magnesium iodide MgI2 barium oxide BaO

15. aluminum oxide Al2O3 iron (II) sulfide FeS mercury (II) oxide HgO copper (II) oxide CuO lead (IV) oxide PbO2

16. Objective #3 Binary Molecular Formulas *binary molecular compounds contain 2 nonmetals *Greek prefixes are used to indicate the number of each atom present

17. Objective #3 Binary Molecular Formulas *prefixes:

18. Objective #3 Binary Molecular Formulas *naming involves: • 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)

19. NO nitrogen monoxide NO2 nitrogen dioxide N2O dinitrogen monoxide SF6 sulfur hexafluoride P4O10 tetraphosphorusdecoxide

20. Examples of Writing Binary Molecular Formulas carbon dioxide CO2 carbon monoxide CO Sulfur trioxide SO3 Dinitrogenpentoxide N2O5

21. phosphorus pentachloride PCl5 dichlorineheptoxide Cl2O7

22. Objective #4 Formulas Containing Polyatomic Ions NaNO2 sodium nitrite Fe2(CO3)3 iron (III) carbonate Pb(Cr2O7)2 lead (IV) dichromate NH4OH ammonium hydroxide Ag2CO3 silver carbonate

23. sodium nitrate NaNO3 calcium phosphate Ca3(PO4)2 Ammonium phosphate (NH4)3PO4 Magnesium hydroxide Mg(OH)2

24. Copper (II) acetate Cu(C2H3O2)2 Iron (III) hydroxide Fe(OH)3

25. Objective #5 Formulas of Acids *examples: hydrofluoric acid HF sulfurous acid H2SO3 nitric acid HNO3

26. *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 changing the ending as follows: ate becomes ic ite becomes ous

27. Examples of Acids HCl hydrochloric acid HBr hydrobromic acid HNO2 nitrous acid HClO4 perchloric acid HC2H3O2 acetic acid

28. hydroiodic acid HI phosphorous acid H3PO3 Phosphoric acid H3PO4

29. Objective #5 Acid-Base Characteristics and Definitions

30. Objective #5 Acid-Base Characteristics and Definitions Acid-Base Theories • The Arrhenius Definition of Acids and Bases • an Arrhenius acid is a substance that increases the number of hydrogen ions in water solution • an Arrhenius base is a substance that increases the number of hydroxide ions in water solution

31. Objective #5 Acid-Base Characteristics and Definitions *examples: HCl(aq) › H+1(aq) + Cl-1(aq) NaOH(aq) › Na+1(aq) OH-1(aq)

32. 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 donates protons *a Bronsted-Lowery base is a substance that accepts protons

33. Objective #5 Acid-Base Characteristics and Definitions *examples: HCl + H2O › H3O+1(aq) + Cl-1(aq) NH3 + H2O › NH4+1(aq) + OH-1(aq)

34. 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 eligible to donate a proton

35. Objective #5 Acid-Base Characteristics and Definitions *example: HCN + H2O › CN-1 + H3O+1 acid base con. base con. acid *a conjugate acid-base pair always differs by a proton *for each of the following acid-base reactions, identify the acid-base pairs:

36. Objective #5 Acid-Base Characteristics and Definitions (examples) H2PO4-1 + H2O --› HPO4-2 + H3O+1 HClO4 + H2O --› _______ + ______ (acid) (base) (con. acid) (con. base) HSO4-1 + H2O --› _______ + ______ (acid) (base) (con. base) (con. acid) *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)