1. Classification of Inorganic Compounds Inorganic Chemistry: Non carbon compounds Exceptions: Carbonate and bicarbonate ions Binary ionic Compounds: Contain two elements, one metal and one nonmetal. EX: KCl, MgCl2, AlCl3, Ternary Ionic Compounds: Contain three elements, at least one metal and one nonmetal Ex: KNO3, Ca(NO3)2, Al(NO3)3, Na2CO3 Binary Molecular Compound: Contain two nonmetals Ex: NH3, H2O, H2S

2. Classification of Inorganic Compounds Aqueous Solution: Is produced when a compound dissolves in water Binary Acid: An aqueous solution of a compound containing hydrogen and one other nonmetal Ex: HCl(aq), HBr(aq), H2S(aq) Ternary oxyacid: An aqueous solution of a compound containing hydrogen, a nonmetal, and oxygen Ex: HNO3, H2SO4, H3PO3

3. Classification of Inorganic Compounds and Acids Inorganic Compounds and Acids Ionic Molecular Aqueous Acid Binary ionic Ternary Ionic Binary Binary Ternary Molecular Acid Acid Compound

4. Classification of Ionic Compounds and Acids Practice a) carbon disulfide, CS b)Lithium dichromate, Li2Cr2O7 c) Magnesium iodide, MgCl d) Nitric acid, HNO3(aq) e) Hydrochloric acid, HCl(aq) How do you distinguish binary molecule and binary acid ?

5. Classification of Ions Ions Cations Anions Monoatomic Polyatomic Monoatomic Polyatomic Practice: Ba2+, Cl-, Ni2+, ClO3-, NO3-, CO32-

6. Monoatomic Ions Cations: Metals lose valence electrons to become positively charged cations. Ex: Li+, Na+, Mg2+, Al3+ Anions: Nonmetal atoms gain valence electrons and become negatively charged ions called Anions. Ex: Cl-, O2-, S2-, N3- Naming Metal ions: 1) Name of parent metal followed by ion 2) Transition metals can form more than on cation (Fe2+, Fe3+) In this case, it is necessary to specify the charge. As per IUPAC the cation can be named for the parent metal followed by its charge by Roman numerals in parentheses. Ex: Iron(II) ion for Fe2+, Copper(II) ion for Cu2+ 3) Naming transition metals with their charge in parentheses is called stock system. Naming ofAg+, Zn2+ and Cd2+ are not required to follow the Stock system

7. Naming of Metal cations by Latin system The Latin system of naming involves the Latin name of metal and suffix –ous or –ic If the metal produces two cations, the lower charge ion is received –ous and higher charge ion is received –ic Ex: Latin name of ion is ferrum. Ferrous ion is F2+ and Ferric ion is Fe3+ Latin Name for Copper is Cuprum. Cuprous is for Cu+ and Cupric is for Cu2+ Mercury(I) ion is exception for naming with Latin name (Hydrargyrum is difficult to pronounce) Hg22+ : Mercurous (Hg+ becomes Hg2+ for stability reasons) Hg2+ : Mecuric:

8. Monoatomic Cations

9. Naming Nonmetal ions As per IUPAC rules, the nonmetal ions are named using nonmetal name followed by the suffix –ide.
Anion
IUPAC Name
Br-
Cl- F- I-
N3-
O2-
P3-
S2-
Bromide ion
Chloride ion
Fluoride ion
Iodide ion
Nitride ion
Oxide ion
Phosphide ion
Sulfide ion

10. Formulas of Monoatomic Cations Group number of a metal indicates the charge of Metal
Lithium
Sodium
Potassium
Magnesium
Calcium
Barium
Aluminum
1 or IA
2 or IIA
3 or IIIA + 2+ 3+

11. Formulas of Monoatomic Anions Group VA or 15:. Gains 3 electrons
Formulas of Monoatomic Anions Group VA or 15: Gains 3 electrons N3- Group VIA or 16: Gains 2 electrons O2- Group VIIA or 17: Gains 1 electron F- Requirement of electrons is the key to predict the negative charge on nonmetals The elements in Group VA need 3 electrons, Group VIA need 2 electrons, Group VII need 1 one electron to get isoelectronic structure with the nearest noble gas Predict Charge of Barium ion, Cobalt(II) ion, Choride ion, Phosphide ion, Iodide ion

12. Polyatomic Ions (Anions) 1) Generally one or more elements combine with oxygen to produce ions These oxyions have names ending with –ate Ex: Nitrate ion of NO33-, Sulfate for SO42- 2) Some oxyions have names ending with –ite Ex: Nitrite for NO22-, Sulfite for SO The ions with name ending with -ite, will have one less oxygen atom than the corresponding –ate Chlorate ion ClO Chlorite ion ClO2- (Distinguish between monatomic anion and polyatomic anion)

13. Polyatomic Ions (anions)

14. Writing Chemical Formulas 1) Ionic compound contains positive and negative ions. Ex: NaCl 2) Formula unit is the simplest representative particle of ionic compound 3) Since the formula unit is neutral, the total positive charge must be equal to total negative charge. 4) Sodium Chloride: NaCl is composed of Na+ and Cl- Calcium Chloride: Ca2+, Cl- To have neutral charge, it is necessary to have 2 Cl- ions Therefore, calcium chloride has the formula of CaCl2 (Ca2+ and 2Cl-) Exercise: Copper(I) oxide Cu+ and O Cadmium oxide Cd2+ and O Cobalt(III)oxide Co3+ and O Aluminum oxide Al3+ and O2-

15. Formula Units Containing Polyatomic Ions “The rules apply same as in the case of monoatomic ions” The charge of positive ions and negative ions should be equal NH4+ and SO42- : Two NH4+ ions are needed to give neutral formula. Therefore the formula is (NH4)2SO4 Practice examples: Ca2+ and CO32- Ca2+ and OH- Ca2+ and PO43-

16. Binary Ionic Compounds The net charge must be zero to the ionic compound. This principle applies to every ionic compound including Binary ionic compounds. Practice: Determine the charge of iron in Fe2O3, Cu3P and CoN

17. Naming Binary Ionic Compounds 1) The metal cation is named first followed by nonmetal anion 2) The suffix –ide should be added to the nonmetal anion MgO: Magnesium oxide SnF2: Stock system- Tin(II) fluoride, Latin system: Stannous fluoride Practice: Systematic names of Mn3P and Fe2S3

18. Predicting Formulas of Binary Ionic Compounds 1) Use periodic table to predict the formula 2) Group number is the charge of the metal ion (cation) Practice: Sodium chloride, Aluminum oxide Magnesium chloride Aluminum sulfide Gallium oxide

19. Transition metal in Ternary ionic Compounds 1) Transition metals have variable charges 2) The charge must be determined first before attempting the name Determine the charge and give the correct name for: 1) Fe3(PO4)2 2) Hg(OH)2 3) Co(ClO3)3

20. Naming Ternary Ionic Compounds Name cation first followed by anion CaCO Calcium carbonate CuSO4: Stock system: Copper(II) sulfate Latin System: Cupric sulfate Practice: 1) KMnO4, Ca(NO3)2, Hg(NO3)2, BaCrO4, Cu(NO2)2 2) Write the formula for Mercury(I) nitrite, iron(III) sulfate 3) Identify binary and ternary ionic compounds LiCl, LiClO, LiClO2

21. Predicting Formulas of Ternary Ionic Compounds 1) With the help of Periodic table, predict the charge of the metal 2) If the anion is familiar, use the charge of the anion to predict the formula 3) Take help from the similar formula. Identify the group of the metal or nonmetal and predict formula Examples: Calcium carbonate is CaCO3. Predict a) Barium carbonate and Calcium silicate. Potassium chlorate is KClO3. Predict Lithium chlorate, Potassium bromate and Sodium bromate

22. Binary Molecular Compounds 1) Compounds of two nonmetals 2) Molecule is the simplest representative in a binary molecules 3)Order of writing: C, P, N, H, S, I, Br, Cl, O, F Ex: CH4, PH3, NH3, H2S, HI, HBr, HCl, H2O, HF

23. Naming of Binary Molecular Compounds 1) First element named first followed by second element with suffix –ide. 2) The number of atoms of each element will be indicated by Greek prefixes (mono, di, tri etc) The prefix mono is always omitted unless it is necessary EX: CO and CO2 are named as Carbon monoxide and Carbon dioxide

24. Naming of Binary Molecular Compounds Cl2O5: Dichlorine pentaoxide Practice: P4S3, P4S7, IF6, Br3O8, P4S10
Atoms Prefix Atoms Prefix
mono hexa-
di hepta-
tri octa-
tetra nona-
penta deca-

25. Binary Acids “Aqueous solution of a compound containing hydrogen and a nonmetal” Ex: HCl, HBr Named by prefix hydro- followed by nonmetal stem and adding the suffix –ic acid Muriatic Acid: Aqueous hydrogen chloride Chemical name is hydrochloric acid, HCl(aq) Practice: HF(aq), HBr(aq), H2S(aq)

26. Ternary Oxyacids “An aqueous solution of a compound containing hydrogen and an oxyanion” Naming: Attach –ic acid or -ous acid to the nonmetal stem HNO3 (aq) : Nitr + ic acid HNO2 (aq): Nitr + ous acid SO42-: Sulfate (sodium sulfate) SO32-: Sulfite (sodium sulfite) H2SO4(aq): Sulfuric acid H2SO3(aq): Sulfurous acid

27. Ternary acids and related compounds Exercise: H3PO4(aq), H3PO3(aq), HBr(aq), HBrO2(aq), HBrO3(aq)
Formula
Ternary acid
Ternary compound
HClO
HClO2
HClO3
HClO4
Hypochlorous acid
Chlorous acid
Chloric acid
Perchloric acid
Sodium hypochlorite
Sodium chlorite
Sodium chlorate
Sodium perchlorate
NaClO
NaClO2
NaClO3
NaClO4