1. Unit 3 Nomenclature NAMING COMPOUNDS

2. Nomenclature: Naming Compounds There are 2 main types of binary compound: compounds composed of 2 or more elements. 1. Ionic compound: compounds that contain a metal and a non-metal. 2. Covalent molecule: compounds that contain two non-metals. (Write this on the back of your foldable)

3. TYPE I BINARY IONIC COMPOUNDS (Not transitional metals) (write on outside flap)

4. (open flap, write on back side of flap) Forms between 2 ions Cation (+) is always named first and the anion (-) second Cation takes its name from the name of the element End of name (anion) is “ide” The net charge on an ionic compound is always zero.

5. sodium chloride Na + + Cl - NaCl (does the charge add to 0?) ( +1) + (-1) = 0 Use crisscross method to determine # of atoms calcium chloride Ca 2+ + Cl - CaCl 2 (does the charge add to 0?) (+2) + 2(-1) = 0 strontium nitride Sr 2+ + N 3- Sr 3 N 2 3(+2) + 2(-3) = 0 Write on area under the flap, examples

6. Practice Name the following Type I binary compounds: CsF AlCl 3 MgI 2 Rb 2 O SrI 2 K 2 S

7. POLYATOMIC (IONIC) (write on outside of 2 nd flap)

8. (open flap, write on backside of flap) Forms with an ion made of many atoms: Act as a single ion; Mostly anions (exception NH 4 + ) Need to use ( ) when there are multiples of a polyatomic ion Example: Ca(OH) 2 (1 Ca 2+ and 2 OH - ) calcium hydroxide Leave name of polyatomic as is – do not change ending!

9. aluminum hydroxide Al 3+ + (OH) - Al(OH) (check the charge) CRISSCROSS to balance charges. REMEMBER TO PUT ( ) AROUND THE POLYATOMIC Al 3+ + OH - Al(OH) 3 ammonium sulfate (NH 4 ) + + (SO 4 ) 2- (check the charge) (NH 4 ) + + (SO 4 ) 2- (NH 4 ) 2 SO 4 (Write on area under the flap, examples)

10. Common Polyatomic Ions ( copy on back of foldable pg 100 of text book)

11. Practice Name the following compounds: Na 2 CO 3 Na 3 PO 4 (NH 4 ) 2 Cr 2 O 7

12. TYPE II BINARY IONIC COMPOUNDS (TRANSITION METALS) (write on outside flap, 3 rd flap) (Mark on your periodic table where the transitional metals are located)

13. 3-13

14. (open flap, write on backside of flap) Many metals can form more than one type of cations, such as most of the transition metals. The cation name still goes first, and the anion second. Ending is still “ide” Identify the charge of the anion to help determine the cation charge. Use roman numerals to indicate charge – If the roman numeral is I, charge is +1 – If the roman numeral is II, charge is +2 – If the roman numeral is III, charge is +3, etc.

15.  (more notes)  Write the cation name with the charge as Roman numerals in parenthesis.  Ends in “ide”  EXCEPTIONS…: Zn 2+, Cd 2+, Ag 1+ We use Roman Numerals to indicate the charge. I=1 II=2 III=3 IV=4 V=5

16. Common Type II Cations

17. Practice (Write on area under the flap, examples Give the names for each of the following compounds: CuCl What is the charge on the Cl? -1; copper(I)chloride HgO What is the charge on the O? -2; mercury (II) oxide

18. Fe 2 O 3 Undo the crisscross. Fe 2 O 3 Fe 3+ O 2- ; Iron (III) oxide MnO 2 Undo the crisscross. Mn 4+ O 2- Manganese (IV) oxide Practice: PbCl 4 FeO CuCl 2

19. Determine the molecular formula lead (II) oxide Pb 2+ + O 2- PbO(do the charges add to 0?) +2 + -2 = 0 Iron (III) sulfide Fe 3+ + S 2- Fe 2 S 3 (crisscross) Copper (II) Nitride Cu 2+ + N 3- Cu 3 N 2 (crisscross)

20. TYPE III BINARY COMPOUNDS THAT ONLY CONTAIN NONMETALS (MOLECULAR) (write on outside flap, 4 th flap)

21. 1.The first element in the formula is named first 2.The second element is named as though it were an anion. (ends in –ide) 3.Prefixes are used to denote the numbers of atoms present. 4.The prefix mono- is never used for naming the first element. For example, CO is carbon monoxide, never monocarbon monoxide. Rules for naming

22. Forms between 2 or more nonmetals Ionic charges are NOT used Can be multiple combinations of the same atoms ex. CO & CO 2

23. Number of atomsPrefix 1mono- 2di- 3tri- 4tetra- 5penta- 6hexa- 7hepta- 8octa- 9nona- 10deca-

24. Examples: (Write on area under the flap, examples CO= carbon monoxide CO 2 = carbon dioxide N 2 O 5 = dinitrogen pentoxide carbon tetrachloride = CCl 4 dihydrogen monoxide = H2OH2O Memorize: NH 3 = ammonia Remember ammonium? NH 4 +

25. Practice Name these Type III Binary Compounds: BF 3 NO N 2 O 3 CCl 4 IF 5

26. ACIDS (write on outside flap, 5 th flap)

27. A substance that produces a hydrogen ion in solution HINT: look for H in the front of the formula 3 types of names #1- comes from binary compound ending in “-ide” – change to hydro_____ic acid HCl= hydrogen chloride rename as hydrochloric acid H 3 N= trihydrogen nitride rename as hydronitric acid H 2 S= dihydrogen sulfide rename as hydrosulfic acid

28. #2-comes from polyatomic ion ending in “-ite” – Change to “ous” acid HNO 2 =hydrogen nitrite rename as nitrous acid H 2 SO 3 = dihydrogen sulfite rename sulfurous acid

29. #3 comes from polyatomic ion ending in “-ate” – Change to –ic acid HNO 3 = hydrogen nitrate rename as nitric acid H 2 SO 4 = dihydrogen sulfate rename as sulfuric acid

30. Rule # 2 & 3 Examples AcidAnionName H 2 SO 4 SO 4 2- (sulfate) sulfuric acid H 3 PO 4 PO 4 3- (phosphate) phosphoric acid HC 2 H 3 O 2 C 2 H 3 O 2 - (acetate) acetic acid H 2 SO 3 SO 3 2- (sulfite) sulfurous acid HNO 2 NO 2 - (nitrite) nitrous acid

31. Practice Name the following acids HI HBr HCN H 2 S HF HNO 3