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Canton South Chemistry!. Chemical Nomenclature Naming compounds and writing chemical formulas. Predicting Charges on Monatomic Ions. +1 +2 +3 +4 +5 +2 +3 - PowerPoint PPT Presentation
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Chemical Nomenclature
Naming compounds and writing chemical formulas.
Canton South Chemistry!
Predicting Charges on Monatomic Ions
+1 +2 +3 +4 +5 +2 +3
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Nomenclature refers to the process of naming chemicals.
Initially the focus is on the most basic rules and ideas involved in the naming of compounds.
Understanding Nomenclature
I. Binary Compounds A binary compound contains just two element
1. The element with the positive charge ( more metallic ), is written
first.
2. The element with the negative charge( more non-metallic) is written
second
Understanding Nomenclature
• The second word (negative ion) is formed by changing the ending
of the element name to “ide”.
For example: fluorine changes to fluoride, and oxygen to oxide
ex: NaCl sodium chloride
KBr potassium bromide
The first word (metal or positive ion) remains the same word
1. Using the rules given , name the compounds listed below.
1. MgO ____________________ 2. CaI2__________________
3. BaS ____________________ 4. ZnI2
______________________
5. CaO ____________________ 6. Ag2O_____________________
7. K3P ____________________ 8.
AlBr3_____________________
9. Na3N ____________________ 10.
MgS_____________________
Writing proper Chemical formulas.
potassium and chlorine =
1+
K Cl = KCl
1-
= 0
The net charge of the formula must be zero
potassium chloride
Crisscross Methodsimplified method for writing these formulas
Calcium and bromide = calcium bromide Ca2+ Br1-
= 0
Ca2+ Br1-
Ca2+ Br1-
1 2
2+ 2- = 0
1 2
**But we don’t write ones!!! CaBr2
Subscripts
Ca1Br2
Crisscross Methodsimplified method for writing these formulas
aluminum and sulfide = aluminum sulfide Al3+ S2-
= 0
Al3+ S2-
Al3+ S2-
2 3
6+ 6- = 0
2 3
Al2S3
Subscripts
Al2S3
12. sodium chloride ____________13. potassium iodide __________ 14. magnesium sulfide __________15. aluminum bromide__________ 16. strontium oxide ____________ 17. sodium sulfide __________ 18. rubidium phosphide _________19. barium nitride __________
Using the rule given , give the formula for these compounds
Groups/Families
• 23, 24, 23, 23, 23, 12, 2
• 1, 2
• 24, 13, 12
Fe Cu ZnNiCo Zn
Ag
Au HgHg
ZnMnCr
Pt
IA
IIA
I-VIIIB
VIAVIIA
VIIIA
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multiple charges
-4
+3
-3
+2+4
+3+5
Cd
VA
+2+3
+2+4
+2+3
+1+3
+2+1
+2+3
+2+3
+1+2
+2+4
+1+2
+2
Some metallic element are capable of more than one positive charge. We will indicated these with a roman numeral in parenthesis following the name of
the positive element.
Type II Binary Compounds(Stock System)
Roman numeral = the + charge
iron (II) = 2+ and iron (III) = 3+
***Used only when:***
MORE THAN 1 POSITIVE CHARGE
iron and chloride =
Fe Cl 1-
Fe Cl1-
3
iron chloride
=
iron chloride
1 2
(II)
(III)
Compare FeCl2 & FeCl3
iron chloride
2-2+
3+ 3- 0
0
=
Type II Binary Compounds(Stock System)
***Used only when:***
MORE THAN
1 POSITIVE CHARGE
1
4. Name the following compounds.
21. CuO ______________________ 22. PbS ________________________
23. HgCl ______________________ 24. MnO2 _________________________
25. Fe2S3 ______________________ 26. SnBr2 ________________________
27. BiCl3 ______________________ 28. PbCl4 ________________________
Type II Binary Compounds
lead (II) sulfide
Another method of indicating metallic ions with more than one charge is:
Classicalor
“Old School”The "ous"-"ic" System
a suffix
while the suffix -ic is used for the higher ionic charge
The suffix -ous is used for the lower charge.
* Chemistry trivia time:
In the James Bond movie Goldfinger who was the villian?
Auric Goldfinger
What was the license plate number on Goldfinger's Rolls Royce?
AU3 What was the name of Goldfinger's business establishment?
Auric Enterprises
** Mercury's name was changed because hydroargentous and hydroargentic would be just to much to handle
29. ferric chloride ________________________ _____________
30. stannic oxide ________________________ _____________
31. mercuric iodide ________________________ _____________
32. cuprous oxide ________________________ _____________
33. plumbous sulfide ________________________ _____________
34. antimonic bromide _______________________ ____________
35. aurous phosphide ________________________ _____________
“Old School”
The "ous"-"ic" System
(“old school”) (Stock) formula
tin (IV) oxide SnO2
A ternary compound contains three or more different elements.
Ternary compounds usually contain one or more polyatomic ions ( radicals ).
Polyatomic ions ( radicals )are treated just like an ion.
When writing the formula – the basic rules apply.
Ternary CompoundsIt takes “3” or more
Examples: Fe(ClO4)2 ; NaOH : NH4MnO4
Ex: Calcium hydroxide
Calcium and hydroxide = calcium hydroxide Ca2+ OH1-
= 0
Ca2+ OH1-
1 2
Ca OH 2
Subscripts
CaOH2
But OH2 = H2O = water !!!
***Parentheses : need to be used whenever more than a single polyatomic ion is needed to balance the charges
- in other words if you add a subscript put the polyatomic radical in parentheses.
( )
Determining Names and Formulas of Ionic Compounds
Containing Polyatomic Ions
Practice with Polyatomic Ions
NH4OH
Ba(OH)2
Fe(CN)3
Zn(C2H3O2)2
ammonium sulfide
plumbous hydroxide
ammonium hydroxide
barium hydroxide
iron (III) cyanide
zinc acetate
(NH4)2S
Pb(OH)2
... the `ate chart
CO32-CO3
2-
NO3-NO3
-
ClO3-ClO3
-CrO42-CrO4
2-
PO43-PO4
3-
MnO3-MnO3
-
SO42-SO4
2-
-3 -2 -1Polyatomic Ions – they all contain oxygen
... the `ate chart
ChemistryChemistry
NomenclatureNomenclature
ClassClassCrazyCrazy
PleasePlease
Manana ?Manana ?
StudyStudy
-3 -2 -1
... the `ate become… `ites– they all lose an oxygen..
but the charge remains the same
CO22-CO2
2-
NO2-NO2
-
ClO2-ClO2
-CrO32-CrO3
2-
PO33-PO3
3-
MnO2-MnO2
-
SO32-SO3
2-
-3 -2 -1
... the `ate; the `ite; now the hypo-– subtract another oxygen !!
and the charge remains the same
CO 2-CO 2-
NO -NO
-
ClO -ClO -CrO22-CrO2
2-
PO23-PO2
3-
MnO -MnO -
SO22-SO2
2-
-3 -2 -1
– lets add an oxygen … the Per- ... the `ate; the `ite; the hypo..
and the charge remains the same
CO42-CO4
2-
NO4-NO4
-
ClO4-ClO4
-CrO52-CrO5
2-
PO53-PO5
3-
MnO4-MnO4
-
SO52-SO5
2-
-3 -2 -1
ClO2-1
ClO4-1
ClO3-1
ClO-1
perchlorate
chlorate
chlorite
hypochlorite
`ate `ite hypo- per-
Na2CO3CO3-2
HCO3-1
carbonate
bicarbonate
carbonate versus bicarbonate
NaHCO3
sodium carbonate
sodium bicarbonate
add H+ and drop a negative charge
36. AlPO4 ______________________ 37. (NH4)2CO3 _______________________
38. __________ lithium cyanide 39. ___________ copper(II) nitrate 40. KClO ______________________ 41. Zn(C2H3O2)2 ______________________
42. __________ calcium phosphate 43. ___________ ammonium sulfite 44. __________ ammonium acetate 45. NaMnO4 _______________________
Determining Names and Formulas of Ionic Compounds Containing Polyatomic Ions
Naming Covalent Molecular Compounds
Use these Prefixes: Greek prefixes to indicate number (never use mono on first)
mono - 1 di - 2 tri - 3 tetra - 4 penta - 5 hexa - 6 hepta - 7 octa - 8nona - 9 deca – 10
Nonmetal to Nonmetal ( or to the right of the zigzag red line)
Ex: BF3 NO
N2O5
boron trifluoride
dinitrogen pentoxide
nitrogen monoxide
1. CO __________________________ 8. diphosphorus pentoxide _________________ 2. PBr3 ______________________________ 9. carbon dioxide _________________
3. CCl4 ______________________________ 10. selenium trioxide _________________
4. NCl3 ______________________________ 11. sulfur hexafluoride _________________
5. SeO2 ______________________________ 12. phosphorus pentiodide ________________
6. P2O3 _____________________________ 13. sulfur tribromide ________________
7. NH3 ______________________________ 14. phosphorus hexachloride______________
Naming Covalent Molecular Compounds
