Nomenclature

1. Nomenclature C2H3O2- acetate ion HC2H3O2 Acetic Acid

2. Forms of Chemical Bonds • There are 3 forms bonding atoms: • Ionic—complete transfer of 1 or more electrons from one atom to another (one loses, the other gains) • Covalent—some valence electrons shared between atoms • Metallic– holds atoms of a metal together Most bonds are somewhere in between ionic and covalent.

3. NAMING COMPOUNDS • Your ability to name compounds and write formula’s hinges on your ability to recognize whether a compound is Ionic or Molecular.

4. COMPOUNDS FORMED FROM IONS CATION + ANION ---> COMPOUND Na+ + Cl- --> NaCl A neutral compound requires equal number of + and - charges.

5. Naming Monatomic Ions • Monatomic cations are identified simply by the element’s name. • Examples: K+ is called the potassium cation Mg2+ is called the magnesium cation

6. Naming Monatomic Ions • For monatomic anions, the ending of the element’s name is dropped, and the ending –ide is addend to the root name. Examples: F-is called the fluoride anion N3+ is called the nitride anion

7. Monatomic Ions

8. Two Types of Compounds Ionic Molecular Smallest piece Formula Unit Molecule Types of elements Metal and Nonmetal Nonmetals Solid, liquid or gas State solid Melting Point High >300ºC Low <300ºC

9. Naming Binary Ionic Compounds • Binary ionic compounds involve combining the manes of the cation and anion that makes up the compound. • The name of the cation is given first, followed by the name of the anion • Example: Aluminum Oxide Al2O3 Name of anion Oxide Name of cation Aluminum

10. Naming Binary Ionic Compounds • Examples: NaCl ZnI2 Al2O3 sodium chloride zinc iodide aluminum oxide

11. Learning Check nitride Complete the names of the following binary compounds: Na3N sodium __________________ KBr potassium________________ Al2O3 aluminum ________________ MgS _________________________ bromide oxide Magnesium sulfide

12. Writing the formulas of Binary Ionic Compounds 1. Find the charge for each atom. (Remember: if you don’t see a number, then it is implied to be a 1) • Switch the numbers on the elements.(you want to balance the positive charges and the negative charges.) Mg2+ Cl- Mg2+ Cl-

13. Writing the formulas of Binary Ionic Compounds 3. Write your formula. (Remember + and - signs Go away.) There is one catch! If the charges have the same magnitude, then the ions will form a compound with a 1:1 ratio. MgCl2 Mg+2 O2-MgO

14. Learning Check Write the correct formula for the compounds containing the following ions: 1. Na+, S2- a) NaS b) Na2S c) NaS2 2. Al3+, Cl- a) AlCl3 b) AlCl c) Al3Cl 3. Mg2+, N3- a) MgN b) Mg2N3 c) Mg3N2

15. Stock system of Nomenclature • Transition metals (the d-block elements) can form two or more cations with different charges. • These elements REQUIRE Roman Numerals because they can have more than one possible charge: anything except Group 1A, 2A, Ag, Zn, Cd, and Al • Examples: Fe2+ Iron (II) Fe3+ Iron (III)

16. Learning Check Complete the names of the following binary compounds with variable metal ions: FeBr2 iron (_____) bromide CuCl copper (_____) chloride SnO2 ___(_____ ) ______________ Fe2O3 ________________________ Hg2S ________________________ II I oxide Tin IV Iron (III) oxide Mercury (I) sulfide

17. Polyatomic Ions NO3- nitrate ion NO2- nitrite ion

18. Naming Oxyanions • Oxyanion: polyatomic ions that contains oxygen. • Some elements can combine with oxygen to form more than one type of oxyanion. Example: nitrogen can form NO3- or NO2-. The name of the ion with the greater number of oxygen atoms ends in –ate. The name of the ion with the smaller number of oxygen atoms ends in –ite. NO3- NO2- Nitrite Nitrate

19. Naming Oxyanions • In this example, an anion that has one fewer oxygen atom than the –iteanion has is given the prefix hypo-. An anion that has one more oxygen atom that the –ate anion has is given the prefix per-. ClO- ClO2- ClO3- ClO4- perchlorate chlorate chlorite hypochlorite

20. Ternary Ionic Nomenclature(Polyatomic Ions) • Ionic compounds involving polyatomic ions are named in the same way as binary compounds. • The name of the cation is given first followed by the name of the anion • Example Al2(SO4)3 NH4Cl Aluminum sulfate Ammonium chloride

21. Learning Check sodium carbonate Na2CO3 MgSO3 MgSO4 Ca(HCO3)2 CaCO3 Ca3(PO4)2 magnesium sulfite magnesium sulfate calcium bicarbonate calcium carbonate calcium phosphate

22. Ternary Ionic Nomenclature Writing Formulas 1. Find the charge for each atom. (Remember: if you don’t see a number, then it is implied to be a 1. It helps to circle the ions) 2. Switch the numbers on the elements.(you want to balance the positive charges and the negative charges.) K+ SO42- K+ SO42-

23. Ternary Ionic Nomenclature Writing Formulas 3. Write your formula. (Remember + and - signs Go away.) K2SO4 There is one catch! If you need more than one of the polyatomic ions to make the charge neutral, you must enclose it in parenthesis. Ca+2 CH3COO-Ca(CH3OO)2

24. Ternary Ionic Nomenclature Sodium Sulfate Na+ and SO4-2 Na2SO4 Iron (III) hydroxide Fe+3 and OH- Fe(OH)3 Ammonium carbonate NH4+ and CO3–2 (NH4)2CO3

25. Learning Check 1. aluminum nitrate a) AlNO3 b) Al(NO)3 c) Al(NO3)3 2. copper(II) nitrate a) CuNO3 b) Cu(NO3)2 c) Cu2(NO3) 3. Iron (III) hydroxide a) FeOH b) Fe3OH c) Fe(OH)3 4. Tin(IV) hydroxide a) Sn(OH)4 b) Sn(OH)2 c) Sn4(OH)

26. Mixed Practice! Name the following: • Na2O • CaCO3 • PbS2 • Sn3N2 • Cu3PO4 • HgF2 Sodium oxide Calcium carbonate Lead (IV) sulfide Tin (II) nitride Copper (I) phosphate Mercury (II) fluoride

27. Naming Molecular Compounds CO2 Carbon dioxide All are formed from two or more nonmetals. BCl3boron trichloride CH4 methane

28. Molecular (Covalent) Nomenclature • Less electronegative atom comes first. It is given a prefix only it is contributes more than one atom to the molecule. • In general, the order of nonmetals in molecular names and formulas (which one comes first): C, P, N, H, S, I, Br, Cl, O, F

29. Molecular (Covalent)Nomenclature • The second element is named by combining: • a prefix indicating the number of atoms contributed by the element . • The root word of the second element. • The ending changes to –ide.

30. Molecular (Covalent)Nomenclature • The o or a at the end of a prefix is dropped if the main word starts with a vowel. P4O10 tetraphosphorus decoxide

31. Molecular Nomenclature Prefixes PREFIX mono- di- tri- tetra- penta- hexa- hepta- octa- nona- deca- NUMBER 1 2 3 4 5 6 7 8 9 10

32. Learning Check mon CO carbon ______oxide CO2 carbon _______________ PCl3phosphorus_______chloride CCl4 carbon ________chloride N2O _____nitrogen _____oxide dioxide tri tetra di mon

33. Learning Check 1. P2O5 a) phosphorus oxide b) phosphorus pentoxide c) diphosphorus pentoxide 2. Cl2O7a) dichlorineheptoxide b) dichlorine oxide c) chlorine heptoxide 3. NF3a) nitrogen trifluoride b) mononitrogen fluoride c) nitrogen difluoride

34. Acid Nomenclature • Acid: usually refers to a solution in water of an acid compound rather that the acid itself. • Formulas usually begin with ‘H’. • In binary acids, there are only two elements that make up the molecule. Example HF, hydrofluoric acid • In ternary acids are ALL aqueous and are made up of at least one polyatomic ion. Example :H2SO4 – sulfuric acid

35. Acid Nomenclature No Oxygen w/Oxygen An easy way to remember which goes with which for those that contain oxygen… “In the cafeteria, you ATE something ICky”

36. Learning Check • HBr(aq) • H2CO3 • H2SO3 • No oxygen, -ide hydrobromic acid • Has oxygen, -ate  carbonic acid • Has oxygen, -ite  sulfurous acid

37. Learning Check • hydrofluoric acid • sulfuric acid • nitrous acid  HF (aq)  H+ F- • 2 elements  H+ SO42- • 3 elements, -ic  H2SO4  H+ NO2-  HNO2 • 3 elements, -ous

38. The End