Nomenclature PO 4. phosphate ion. HC 2 H 3 O 2 Acetic Acid C 2 H 3 O 2. acetate ion. Chemistry 1 Honors: Chapter 7: pp

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Chemistry 1 Honors: Chapter 7: pp218-258

1 Chemistry 1 Honors: Chapter 7: pp PO 4 3- phosphate ion Nomenclature HC 2 H 3 O 2 Acetic Acid C 2 H 3 O 2 - acetate ion SAVE PAPER AND INK!!! When you print out the notes on PowerPoint, print "Handouts" instead of "Slides" in the print setup. Also, turn off the backgrounds (Tools>Options>Print>UNcheck "Background Printing")!

2 Forms of Chemical Bonds Most bonds are somewhere in between ionic and covalent. 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 holds atoms of a metal together

3 Common Names A lot of chemicals have common names as well as the proper IUPAC name. Chemicals that should always be named by common name and never named by the IUPAC method are: H 2 O water, not dihydrogen monoxide NH 3 ammonia, not nitrogen trihydride

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

5 Predicting Charges on Monatomic Ions KNOW THESE!!!! Cd +2

6 Properties of Ionic Compounds Forming NaCl from Na and Cl 2 A metal atom can transfer an electron to a nonmetal. The resulting cation and anion are attracted to each other by electrostatic forces.

7 ammonium chloride, NH 4 Cl IONIC COMPOUNDS NH 4 + Cl -

8 Some Ionic Compounds Ca F - ---> CaF 2 Mg 2+ + N > Mg 3 N 2 magnesium nitride Sn 4+ + O > calcium fluoride SnO 2 Tin (IV) oxide

9 Formulas of Ionic Compounds Formulas of ionic compounds are determined from the charges on the ions atoms ions Na + F : Na + : F : NaF sodium + fluorine sodium fluoride formula Charge balance: = 0

10 Monatomic Ions

11 Writing a Formula Write the formula for the ionic compound that will form between Ba 2+ and Cl. Solution: 1. Balance charge with + and ions 2. Write the positive ion of metal first, and the negative ion Ba 2+ Cl Cl 3. Write the number of ions needed as subscripts BaCl 2

12 Learning Check Write the correct formula for the compounds containing the following ions: 1. Na +, S 2- a) NaS b) Na 2 S c) NaS 2 2. Al 3+, Cl - a) AlCl 3 b) AlCl c) Al 3 Cl 3. Mg 2+, N 3- a) MgN b) Mg 2 N 3 c) Mg 3 N 2

13 Solution 1. Na +, S 2- b) Na 2 S 2. Al 3+, Cl - a) AlCl 3 3. Mg 2+, N 3- c) Mg 3 N 2

14 Naming Compounds Binary Ionic Compounds: 1. Cation first, then anion 2. Monatomic cation = name of the element Ca 2+ = calcium ion 3. Monatomic anion = root + -ide CaCl 2 Cl = chloride = calcium chloride

15 Naming Binary Ionic Compounds Examples: NaCl ZnI 2 Al 2 O 3 sodium chloride zinc iodide aluminum oxide

16 Learning Check Complete the names of the following binary compounds: Na 3 N sodium KBr Al 2 O 3 MgS potassium aluminum

17 Transition Metals Elements that can have more than one possible charge MUST have a Roman Numeral to indicate the charge on the individual ion. 1+ or or 3+ Cu +, Cu 2+ Fe 2+, Fe 3+ copper(i) ion copper (II) ion iron(ii) ion iron(iii) ion

18 Names of Variable Ions 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. FeCl 3 (Fe 3+ ) iron (III) chloride CuCl (Cu + ) copper (I) chloride SnF 4 (Sn 4+ ) tin (IV) fluoride PbCl 2 (Pb 2+ ) lead (II) chloride Fe 2 S 3 (Fe 3+ ) iron (III) sulfide

19 Examples of Older Names of Cations formed from Transition Metals (you do not have to memorize these)

21 Learning Check Complete the names of the following binary compounds with variable metal ions: FeBr 2 CuCl SnO 2 Fe 2 O 3 Hg 2 S iron ( ) bromide copper ( ) chloride ( )

22 NO 3 - Polyatomic Ions nitrate ion NO 2 - nitrite ion

23 Polyatomic Ions You can make additional polyatomic ions by adding a H + to the ion! CO 3-2 is carbonate HCO 3 is hydrogen carbonate H 2 PO 4 is dihydrogen phosphate HSO 4 is hydrogen sulfate

24 Ternary Ionic Nomenclature Writing Formulas Write each ion, cation first. Don t show charges in the final formula. Overall charge must equal zero. If charges cancel, just write symbols. If not, use subscripts to balance charges. Use parentheses to show more than one of a particular polyatomic ion. Use Roman numerals indicate the ion s charge when needed (stock system)

25 Ternary Ionic Nomenclature Sodium Sulfate Na + and SO 4-2 Na 2 SO 4 Iron (III) hydroxide Fe +3 and OH - Fe(OH) 3 Ammonium carbonate NH 4+ and CO 3 2 (NH 4 ) 2 CO 3

26 Learning Check 1. aluminum nitrate a) AlNO 3 b) Al(NO) 3 c) Al(NO 3 ) 3 2. copper(ii) nitrate a) CuNO 3 b) Cu(NO 3 ) 2 c) Cu 2 (NO 3 ) 3. Iron (III) hydroxide a) FeOH b) Fe 3 OH c) Fe(OH) 3 4. Tin(IV) hydroxide a) Sn(OH) 4 b) Sn(OH) 2 c) Sn 4 (OH)

27 Naming Ternary Compounds Contains at least 3 elements There MUST be at least one polyatomic ion (it helps to circle the ions) Examples: NaNO 3 Sodium nitrate K 2 SO 4 Al(HCO 3 ) 3 Potassium sulfate Aluminum bicarbonate or Aluminum hydrogen carbonate

28 Learning Check Match each set with the correct name: 1. Na 2 CO 3 a) magnesium sulfite MgSO 3 b) magnesium sulfate MgSO 4 c) sodium carbonate 2. Ca(HCO 3 ) 2 a) calcium carbonate CaCO 3 b) calcium phosphate Ca 3 (PO 4 ) 2 c) calcium bicarbonate

29 Mixed Practice! Name the following: 1. Na 2 O 2. CaCO 3 3. PbS 2 4. Sn 3 N 2 5. Cu 3 PO 4 6. HgF 2

30 Mixed Up The Other Way Write the formula: 1. Copper (II) chlorate 2. Calcium nitride 3. Aluminum carbonate 4. Potassium bromide 5. Barium fluoride 6. Cesium hydroxide

31 Naming Molecular Compounds CO 2 Carbon dioxide All are formed from two or more nonmetals. CH 4 methane BCl 3 boron trichloride Ionic compounds generally involve a metal and nonmetal (NaCl)

Molecular (Covalent) Nomenclature for two

32 Molecular (Covalent) Nomenclature for two nonmetals Prefix System (binary compounds) 1. Less electronegative atom comes first. 2. Add prefixes to indicate # of atoms. Omit mono- prefix on the FIRST element. Mono- is OPTIONAL on the SECOND element (in this class, it s NOT optional!). 3. Change the ending of the second element to -ide.

33 Molecular Nomenclature Prefixes PREFIX monoditritetrapentahexaheptaoctanonadeca- NUMBER

34 Molecular Nomenclature: Examples CCl 4 carbon tetrachloride N 2 O dinitrogen monoxide SF 6 sulfur hexafluoride

35 More Molecular Examples arsenic trichloride AsCl 3 dinitrogen pentoxide N 2 O 5 tetraphosphorus decoxide P 4 O 10

36 Learning Check Fill in the blanks to complete the following names of covalent compounds. CO carbon oxide CO 2 PCl 3 CCl 4 N 2 O carbon phosphorus chloride carbon chloride nitrogen oxide

37 Learning Check 1. P 2 O 5 a) phosphorus oxide b) phosphorus pentoxide c) diphosphorus pentoxide 2. Cl 2 O 7 a) dichlorine heptoxide b) dichlorine oxide c) chlorine heptoxide 3. Cl 2 a) chlorine b) dichlorine c) dichloride

38 Overall strategy for naming chemical compounds.

39 A flow chart for naming binary compounds.

40 Mixed Review Name the following compounds: 1. CaO a) calcium oxide b) calcium(i) oxide c) calcium (II) oxide 2. SnCl 4 a) tin tetrachloride b) tin(ii) chloride c) tin(iv) chloride 3. N 2 O 3 a) nitrogen oxide b) dinitrogen trioxide c) nitrogen trioxide

41 Solution Name the following compounds: 1. CaO 2. SnCl 4 a) calcium oxide c) tin(iv) chloride 3. N 2 O 3 b) Dinitrogen trioxide

42 Mixed Practice 1. Dinitrogen monoxide 2. Potassium sulfide 3. Copper (II) nitrate 4. Dichlorine heptoxide 5. Chromium (III) sulfate 6. Iron (III) sulfite 7. Calcium oxide 8. Barium carbonate 9. Iodine monochloride

43 Mixed Practice 1. BaI 2 2. P 4 S 3 3. Ca(OH) 2 4. FeCO 3 5. Na 2 Cr 2 O 7 6. I 2 O 5 7. Cu(ClO 4 ) 2 8. CS 2 9. B 2 Cl 4

Acid Nomenclature Acids Compounds that form H +

Ternary acids are ALL aqueous Examples: HCl

44 Acid Nomenclature Acids Compounds that form H + in water. Formulas usually begin with H. In order to be an acid instead of a gas, binary acids must be aqueous (dissolved in water) Ternary acids are ALL aqueous Examples: HCl (aq) hydrochloric acid HNO 3 nitric acid H 2 SO 4 sulfuric acid

45 Acid Nomenclature Review No Oxygen w/oxygen Anion Ending -ide -ate -ite Acid Name hydro-(stem)-ic acid (stem)-ic acid (stem)-ous acid An easy way to remember which goes with which In the cafeteria, you ATE something ICky

46 Acid Nomenclature Flowchart ACIDS start with 'H' 2 elements 3 elements hydro- prefix -ic ending no hydro- prefix -ate ending becomes -ic ending -ite ending becomes -ous ending

47 Acid Nomenclature HBr (aq) 2 elements, -ide hydrobromic acid H 2 CO 3 3 elements, -ate H 2 SO 3 3 elements, -ite carbonic acid sulfurous acid

48 Acid Nomenclature hydrofluoric acid 2 elements sulfuric acid 3 elements, -ic nitrous acid 3 elements, -ous H + F- H + SO 4 2- H + NO 2 - HF (aq) H 2 SO 4 HNO 2

49 Name Em! HI (aq) HCl H 2 SO 3 HNO 3 HIO 4

50 Write the Formula! Hydrobromic acid Nitrous acid Carbonic acid Phosphoric acid Hydrotelluric acid

51 Nomenclature Summary Flowchart

52 Now it s Study Time DONE

53 Rainbow Matrix Game Link on Chemistry Geek.com on Chemistry I page Use [ ] to represent subscripts since you can t enter subscripts into the computer So H 2 O would be H[2]O And Al 2 (SO 4 ) 3 would be Al[2](SO[4])[3] Additional Polyatomic Ions (you do not have to memorize these, but they are in the game!) Borate = BO 3-3 ; Silicate = SiO 4-4 ; Manganate = MnO 4-2 (permanganate is -1)

Nomenclature. Common Names. Common Names COMPOUNDS FORMED FROM IONS. Binary Ionic Compounds

Nomenclature. Common Names. Common Names COMPOUNDS FORMED FROM IONS. Binary Ionic Compounds PO 4 3- phosphate ion C 2 H 3 O 2 - acetate ion World of Chemistry: Chapter 4 Nomenclature HC 2 H 3 O 2 Acetic Acid Common Names Common Names A lot of chemicals have common lot of chemicals have common