Nomenclature : Naming Chemicals

1. Nomenclature: Naming Chemicals PO43- phosphate ion HC2H3O2 Acetic Acid C2H3O2- acetate ion

2. Before naming…. • Some things you MUST know to be successful…. You really need to commit these things to memory

3. Ions: • Atoms or groups of atoms with a _________. • Cations- ________ions - get by losing electron(s). • Anions- ________ ions - get by gaining electron(s). • Ionic bonding- held together by the ______________ (_____________________). • Ionic solids are called ________. • Salts are __________________; they conduct electricity when dissolved in water (aq.)

4. Metals • Conductors of heat and electricity • Make ________(lose e- to become + charged) • Malleable (made into ________) • Ductile (made into ________)

5. Nonmetals • Are a ________ _______ or a _______ • Make ________(gain e- to become - charged) • __________ bond to each other

6. Semi-metals (AKA ________) • Characteristics of _____ metals and nonmetals • More ________ as you go down PT

7. Common Ions of Elements ________ _____

8. Predicting Charges on Monatomic Ions KNOW THESE !!!! +1 +2 -3 -2 -1 0 Variable, always + Cd+2

9. Polyatomic Ions • _______ of covalently bonded atoms that have a charge. * NO3- :___________ * NO2- :___________ • Yes, you have to memorize them. • Listed in your resource handbook: memorize the required list!!!!

10. Patterns for Polyatomic Ions • -ate ion • _________________________________ • -ate ion plus 1 O  same charge, ___- prefix • _________________________________ • -ate ion minus 1 O  same charge, -___ suffix • _________________________________ • -ate ion minus 2 O  same charge, ___- prefix, -___ suffix • _________________________________

11. Polyatomic Ions You can make additional polyatomic ions by adding a __ to the ion! • CO3-2 is carbonate: • HCO3– is ______________________ • PO43- is phosphate: • HPO42- is ______________________ • H2PO4– is ______________________ • SO42- is sulfate • HSO4– is ______________________

12. The 3 types of Chemical Bonds:________, _______ and _________ • Electronegativity and Bond Type • Bond type can be determined by the difference in electronegativity (degree of sharing of e-) between the elements involved • Differences of: • ≥ 2 =_________________ • 0.5-1.9 = ______________________ • ≤ 0.4 = ____________________________ • Metals bonded to other metals are ___________________ bonded, regardless of the difference in electronegativity.

13. Metallic bonds • The atoms of metals are held together when the atom’s _________ ____________________________________________________________________________________________________________ • __________________keep everything together

14. Ionic Bonds • Complete_______of 1 or more electrons from one atom to another (or a _____________________) • one _____ one or more e-, the other ____ those e-s • Atoms involved are • ______________________________________________________________________________ • The cation and anion are attracted to each other by _______________________

15. Ionic compounds are neutral • Ionic compounds are ______________ • That is, they have no __________ charge • This is because the number of electrons _____ ________________________________________________________________________________________________________________________ • Formulas reflect this neutrality- the charges on the individual ions are not written in because they _________________ _____________________________________

16. COMPOUNDS FORMED FROM IONS CATION + ANION ---> COMPOUND Na+ + Cl---> NaCl A neutral compound requires

17. Covalent Bonds • ________________valence electrons that are ______________between atoms • We are going to name only simple covalent compounds that have 2 elements involved

18. Most bonds are somewhere in between ionic and covalent • Because not all atoms __________________________ • The conventions of naming assume _____________ _____________________in bond types • Metals bonded to nonmetals or polyatomic ions are classified as having ionic bonds* • Materials made out of all non-metals are classified as having covalent bonds* • * _____________________________________________ ______________________________________________ ______________________________________________ ______________________________________________. • For more on this, go back to bonding

19. Naming things: • If there is only one element present, ________ ____. Atomic substances do not require “special” naming. • For anything with more than one element, remember that there is ONE MAIN THING to look for: • Is there a ______________________?

20. So… some general help for naming: • Look to see if there is a ________ ______in the formula • Again, semimetals are not a classification in naming; _______________________________________________________________________________________________________________________________________ • If there are only metals, __________________________ • (metallic bonding; nothing else need be done) • If ________the first element is a metal, then the compound is an ________________ compound • Nonmetals _________ signify a _______ compound • There is a flow chart in your handbook to help!

21. Naming ionic compounds: • Remember that those are compounds that have a metal first in the formula*, and then a _______________________________________. • We can handle these as simple types • _______________(2 elements) compounds • ___________(more than 2 element) compounds • Names are always for the smallest whole number ratio of the elements, the ___________ *Two exceptions to this rule: • Compounds that start with either ammoniums (NH4+) or hydronium (H3O+)

22. General information for naming ionic compounds:

23. Specifics for binary ionic compounds: Example: CaCl2, or calcium chloride • Name the cation first, then the anion root with an –idesuffix • For CaCl2, the monatomic cation is Ca2+ , calcium, and the monatomic anion is Cl- , named chloride. • We use chloride because the root for chlorine is chlor, and we use = root + -idefor the second element in binary compounds • CaCl2 = calcium chloride

24. Learning Check Complete the names of the following binary compounds: Na3N KBr Al2O3 MgS

25. If the Metal is a Transition Metal… __________________________are Type II Cations, and are elements that can have ______________ ______________________. They MUST have a __________________________________________________________________________________________________ 1+ or 2+ 2+ or 3+ Cu+,Cu2+ Fe2+, Fe3+ ______________________________________________ ________________________________________________

26. Type II Cations These elements REQUIRE Roman Numerals because they can have more than one possible charge: anything except Group 1A, 2A, Ag, Zn, Cd, and Al (You should already know the charges on these!) Or another way to say it is: Transition metals and the metals in groups 4A and 5A (except Ag, Zn, Cd, and Al) require a Roman Numeral. FeCl3(Fe3+) ____________________ CuCl (Cu+ ) ____________________ SnF4 (Sn4+) ____________________ PbCl2 (Pb2+) ____________________ Fe2S3 (Fe3+) ____________________ You will appreciate this more when we go from names to formulas!

27. Type II Cations Some Type II cations have a name using the “old” system as well as the “new system”. The old system, still widely used, adds to the root or stem of the Latin name of the metal the suffixes –ous and –ic. These represent the lower and higher charges respectively.

28. Examples of Older Names of Cations formed from Transition Metals(you do nothave to memorize these)

29. Learning Check Complete the names of the following binary compounds with variable metal ions: FeBr2 CuCl SnBr4 Fe2O3 Hg2S

30. Writing Formulas for Ionic Compounds from Names Formulas of ionic compounds are determined from the charges on the ions Na + F  Na++ F- NaF Sodium atom + fluoride ion sodium fluoride Charge balance: 1+ + 1- = 0

31. Neutral, you say? • Formulas are written to make the compound have a _____________________________. • You do NOT write the charges in the formula because they MUST cross out to accurately represent the compound. • Ex: NaF2 is INCORRECT for sodium chloride because_________________________________________________________________________________________________________________________________________________

32. Writing the formula… Write the formula for the barium chloride, the compound that will form between Ba2+ and Cl. Solution: 1. Write the ___________, and then the ___________. 2. Balance charge with the number of + and – ions 3. Write the number of ions needed ____________ __________________________:

33. So what if the oxidation numbers aren’t even? • If the oxidation numbers or charges do not balance, you can write the number of ions of each until you get the same number of each charge in total. • Yes. The “___________ ____________” _________. You take the ______ __________from the _________, and you make it the number of _________ (subscript), and take the charge on the anion, and you make that many cations (subscript). Is there an easier way?

34. Criss-Crossing in action: Example: Lead (II) nitrate Pb2+ N3- *the charges do not balance Pb2+ N3- Pb3N2 • The 2 and the 3 are brought down to the opposite element, so that there are now ___________ ions and ___________ions • This means there were _____ transferred from the lead atoms to the nitrogen atoms; the compound is neutral

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

36. Ternary Ionic Compounds: • Contain at least 3 elements • There MUST be at least one polyatomic ion (it helps to ______________) Examples: NaNO3 ____________________________ K2SO4 _____________________________ Al(HCO3)3 ______________________________

37. Specifics for ternary ionic compounds Examples: NaNO3, and Co(NO3)2 • Name the cation first, then polyatomic ion • For NaNO3, the monatomic cation is Na+ , sodium, and the polyatomic anion is NO3- , named nitrate. • NaNO3 is sodium nitrate • For Co(NO3)2, the monatomic cation is Co+2, cobalt (II) and the polyatomic anion is NO3- , named nitrate. • Co(NO3)2 is cobalt (II) nitrate

38. Learning Check Match each set with the correct name: 1.Na2CO3 a) magnesium sulfite MgSO3 b) magnesium sulfate MgSO4 c) sodium carbonate 2 . Ca(HCO3)2 a) calcium carbonate CaCO3 b) calcium phosphate Ca3(PO4)2 c) calcium bicarbonate

39. Writing Formulas for Ternary Ionic Compounds • Write the _______ first, then the _____________. • Overall charge must equal ____________. • If charges cancel, just write symbols. • If not, use ________________ to balance charges. • Use parentheses to ____________________________ ______________________________________________. • Use ______________________ to indicate the ion’s charge when needed (transition metals) • Remember that the final formula should ________ __________________________written in.

40. Writing Formulas, cont’d Example: Cr2+ PO43- *the charges do not balance Cr2+ PO43- ______________ The polyatomic ions is in parentheses _____________________ ________________________________. This is so that we know to count a number of those groups!

41. 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)

42. Ternary Ionic Nomenclature: You Criss-cross these, too. Sodium Sulfate Iron (III) hydroxide Ammonium carbonate

43. Write the Formula: Copper (II) chlorate Calcium nitride Aluminum carbonate Potassium bromide Barium fluoride Cesium hydroxide

44. General naming rules for covalent (molecular) compounds • Names are _______________, __________________. • Prefixes tell you________________________. • First element whole name with the appropriate prefix • ***NEVER use ______ for the first element! • For the second element, use the _________ _____________ and the -ideending with appropriate prefix for that many.

45. never YouNEVER . Since you are sharing electrons, rather than giving them away/ picking them up, the charges _______________ ________________.

46. Covalent Naming Prefixes: PREFIX NUMBER 1 2 3 4 5 6 7 8 9 10

47. Specifics for binary covalent compounds Example: CO2 is carbon dioxide • Name the first element, using a prefix if there is more than one atom of the element present • Name the second element, using the appropriate prefix in all cases • CO2 is carbon dioxide because there is one carbon (no prefix when there is only one atom of the element,) and two oxygens (di- prefix)

48. Learning Check 1. P2O5a) phosphorus oxide b) phosphorus pentoxide c) diphosphoruspentoxide 2. Cl2O7 a) dichlorineheptoxide b) dichlorine oxide c) chlorine heptoxide 3. Cl2 a) chlorine b) dichlorine c) dichloride

49. Learning Check Give the names of following covalent compounds: CO CO2 PCl3 CCl4 N2O

50. More Covalent Examples • arsenic trichloride • dinitrogenpentoxide • tetraphosphorusdecoxide