Chemical Naming. Burlingame High School

Transcription

1 Chemical Naming 1

2 Ionic Compounds Ion- an atom that has a positive or negative charge. The only particle lost or gained when forming ions is the e -. Cation Positively charged ion (lost an e - ) Anion Negatively charged ion (gained an e - ) 2

3 Naming Ionic Compounds 1. Cation is always written first» In name and in formula 2. Anion is written second.» Change the ending to -ide 3. Balance Charges» Overall charge must equal zero 3

4 Practice with Ionic Naming Elements Balanced Ion Pairs Li + N Mg + Cl Rb + S - 4

5 Write Balanced Ion Pairs Elements Balanced Ion Pairs Li + N 3Li + + N -3 Mg + Cl Mg Cl - Rb + S 2Rb + + S 2-5

6 Write the Elements Balanced Ion Pairs Li + N 3Li + + N -3 Li 3 N Mg + Cl Mg Cl - MgCl 2 Rb + S 2Rb + + S 2- Rb 2 S 6

7 the compound Elements Balanced Ion Pairs Li + N 3Li + + N -3 Li 3 N Lithium Nitride Mg + Cl Mg Cl - MgCl 2 Magnesium Chloride Rb + S 2Rb + + S 2- Rb 2 S Rubidium Sulfide 7

8 Naming Short cut 8

9 More Practice with Ionic Naming Elements Balanced Ion Pairs Al + O Ca + P Ga + F 9

10 Write balanced ion pairs Elements Balanced Ion Pairs Al + O Al +3 + O -2 Ca + P 3Ca P -3 Ga + F Ga F - 10

11 Write the formula Elements Balanced Ion Pairs Al + O Al +3 + O -2 Al 2 O 3 Ca + P 3Ca P -3 Ca 3 P 2 Ga + F Ga F - GaF 3 11

12 the compound Elements Balanced Ion Pairs Al + O Al +3 + O -2 Al 2 O 3 Aluminum Oxide Ca + P 3Ca P -3 Ca 3 P 2 Calcium Phosphide Ga + F Ga F - GaF 3 Galium Flouride 12

13 Naming with Polyatomic Ions Polyatomic ions» Composed of 2 or more elements that act as a unit.» Have a positive or negative charge.» Most are anions (negative charge)» Most end in -ite/-ate the same way as binary ionic compounds, but use the polyatomic ion name. 13

14 Polyatomic Ions 14

15 Naming with Polyatomic Ions Ions Balanced Ion Pairs Na +1 + PO 4-3 Ba +2 + PO

16 Write Balanced Ion Pairs Ions Balanced Ion Pairs Na +1 + PO Na +1 + PO 4-3 Ba +2 + PO 3-3 3Ba PO

17 Write the formula Ions Balanced Ion Pairs Na +1 + PO Na +1 + PO 4-3 Na 3 PO 4 Ba +2 + PO 3-3 3Ba PO 3-3 Ba 3 (PO 3 ) 2 17

18 the compound Ions Balanced Ion Pairs Na +1 + PO Na +1 + PO 4-3 Na 3 PO 4 Sodium Phosphate Ba +2 + PO 3-3 3Ba PO 3-3 Ba 3 (PO 3 ) 2 Barium Phosphite 18

19 Write the formula Aluminum Nitrate Balanced Ion Pairs 19

20 Write the formula Aluminum Nitrate Balanced Ion Pairs 2Al NO 3-2 Al 2 (NO 3 ) 3 20

21 Naming with Transition Metals Transition Metals have various valences. (Refer to chart) Valence (or charge) is indicated by a roman numeral. Iron III = Fe +3 Iron II = Fe +2 21

22 Ion charges 22

23 Naming with Transition Metals The Roman Numeral tells you the charge on the metal ion, not the number of metal ions present. Write balanced ion pairs to determine formula Iron III Oxide Balanced Ion Pairs 2Fe O -2 Fe 2 O 3 Iron II Oxide Fe +2 + O -2 FeO 23

24 Naming with Transition Metals Lead IV Hydroxide Iron III Carbonate Copper II acetate Balanced Ion Pairs 24

25 Naming with Transition Metals Lead IV Hydroxide Iron III Carbonate Copper II acetate Balanced Ion Pairs Pb (OH - ) 2Fe CO 3-2 Cu C 2 H

26 Naming with Transition Metals Lead IV Hydroxide Iron III Carbonate Copper II acetate Balanced Ion Pairs Pb (OH - ) 2Fe CO 3-2 Cu C 2 H Pb(OH) 4 Fe 2 (CO 3 ) 3 Cu(C 2 H ) 2 26

27 More Naming Practice with Transition Metals Balanced Ion Pairs Zn(C 2 H 3 O 2 ) 2 Cu 3 (PO 4 ) 2 CuClO 3 27

28 More Naming Practice with Transition Metals Zn(C 2 H 3 O 2 ) 2 Balanced Ion Pairs Zn C 2 H Cu 3 (PO 4 ) 2 3Cu PO 4-3 CuClO 3 Cu +1 + ClO

29 More Naming Practice with Transition Metals Zn(C 2 H 3 O 2 ) 2 Cu 3 (PO 4 ) 2 CuClO 3 Balanced Ion Pairs Zn C 2 H Cu PO 4-3 Cu +1 + ClO 3-1 Zinc II Acetate Copper II Phosphate Copper I Clorate 29

30 Molecular Compounds Compounds where both elements have negative charges both from right side of the periodic table both are non-metals Electrons are not transferred, they are shared 30

31 Naming Molecular Compounds Rules for naming molecular compounds 1st element has normal name 2nd element has ending changed to -ide use prefixes to say how many of each element Do not use a prefix with the first element if there is only one. 31

32 Molecular Naming Prefixes 1 mono 6 hexa 2 di 7 hepta 3 tri 8 octa 4 tetra 9 nona 5 penta 10 deca 32

33 the compounds CO 2 CO PCl 3 N 2 P 4 SO 4 N 2 O 5 S 4 Cl 9 33

34 the compounds CO 2 CO PCl 3 N 2 P 4 SO 4 N 2 O 5 S 4 Cl 9 Carbon Dioxide Carbon Monoxide Phosphorus Trichloride Dinitrogen Tetraphosphide Sulfur Tetroxide Dinitrogen Pentoxide Tetrasulfur Nonachloride 34

35 Write the formulas 1. dinitrogen monoxide 2. phosphourus trichloride 3. sulfur hexafluroride 4. carbon disulfide 5. carbon tetrabromide 6. dinitrogen tetrahydride 7. boron trichloride 8. diphosphourus trioxide 9. hexaselenium monochloride 35

36 Write the formulas 1. dinitrogen monoxide N 2 O 2. phosphourus trichloride PCl 3 3. sulfur hexafluroride SF 6 4. carbon disulfide CS 2 5. carbon tetrabromide CBr 4 6. dinitrogen tetrahydride N 2 H 4 7. boron trichloride BCl 3 8. diphosphourus trioxide P 2 O 3 9. hexaselenium monochloride S 6 Cl 36

37 Naming Acids Acids are ionic compounds (cation + anion) H + is the cation All acids start with H When acids dissolve into ion pairs, they produce and H + HCl H + + Cl - HNO 3 H + + NO 3-37

38 Naming Acids When the name of the anion ends in ide, the acid name begins with the prefix hydro-, the stem of the anion has the suffix ic and it is followed by the word acid. HCl = hydrochloric acid. When the anion name ends in ite, the acid name is the stem of the anion with the suffix ous, followed by the word acid. HClO 2 = Chlorous acid. When the anion name ends in ate, the acid name is the stem of the anion with the suffix ic, followed by the word acid. HClO 3 = Chloric acid 38

39 Practice Naming Acids Anion Anion S -2 SO 4 2- SO

40 the anion Anion Anion S -2 Sulfide SO 4 2- Sulfate SO 3 2- Sulfite 40

41 Write the Anion Anion S -2 Sulfide H 2 S SO 4 2- Sulfate H 2 SO 4 SO 3 2- Sulfite H 2 SO 3 41

42 the acid Anion Anion S -2 Sulfide H 2 S Hydrosulfuric Acid SO 4 2- Sulfate H 2 SO 4 Sulfuric Acid SO 3 2- Sulfite H 2 SO 3 Sulfurous Acid 42

43 Naming Acids When the name of the anion ends in ide, the acid name begins with the prefix hydro-, the stem of the anion has the suffix ic and it is followed by the word acid. HCl = hydrochloric acid. * When the anion name ends in ite, the acid name is the stem of the anion with the suffix ous, followed by the word acid. H2ClO2. = Chlorous acid. * When the anion name ends in ate, the acid name is the stem of the anion with the suffix ic, followed by the word acid. H2ClO3 = Chloric acid 43

44 Organic Compounds Organic Compounds - any covalently bonded compound containing carbon (except carbonates and oxides) Functional group - a specific arrangement of atoms in an organic compound that is capable of characteristic chemical reactions. 44

45 Hydrocarbons Hydrocarbons are the simplest organic compounds. They contain only carbon and hydrogen They can be straight-chain, branched chain, or cyclic molecules. Carbon must form 4 bonds 45

46 Naming Hydrocarbons Hydrocarbons - Organic compounds that contain only carbon & hydrogen Alkanes - contain only single covalent bonds Alkenes - contain one or more carbon - carbon double bond Alkynes - contain one or more carbon-carbon triple bond 46

47 Organic Prefixes Number of carbon atoms Prefix 1 meth 2 eth 3 pro 4 but 5 pent 6 hex 7 hept 8 oct 9 non 10 dec 47

48 Naming Hydrocarbons C x H (2x-2) Alkyne 48

49 Simple Alkanes 49

50 Functional Groups 50