1. Common Polyatomic Ions
Names of Common Polyatomic Ions
Ion Name Ion Name
NH ammonium CO carbonate
*NO *nitrite HCO bicarbonate
NO nitrate *IO *iodate
*SO *sulfite *IO *periodate
SO sulfate *ClO *hypochlorite
HSO hydrogen sulfate *ClO *chlorite
OH hydroxide ClO chlorate
CN cyanide *ClO *perchlorate
C2H3O acetate *BrO *bromate
MnO permanganate C2O oxalate
PO phosphate Cr2O dichromate
*PO *phosphite CrO chromate
H2PO dihydrogen phosphate O peroxide
Memorize the BOLD ions
* = you will be responsible for knowing these
Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 100

2. *Charges NEVER change between different forms
Polyatomic Ion Trends
*Charges NEVER change between different forms
+1 oxygen
“Per____ate”
“Normal”
“–ate” form
BrO3-
bromate
ClO3-
chlorate
IO3-
iodate
NO3-
nitrate
CO32-
carbonate
SO42-
sulfate
PO43-
phosphate
-1 oxygen
“-ite” form
-2 oxygens
“hypo___ite”
BrO4-
ClO4-
IO4-
BrO2-
ClO2-
IO2-
NO2-
CO22-
SO32-
PO33-
BrO-
ClO-
IO-
perbromate
bromite
hypobromite
perchlorate
chlorite
hypochlorite
periodate
iodite
hypoiodite
nitrite
carbonite
sulfite
phosphite

3. Atomic Theory Review

4. Electron Cloud Model Orbital (“electron cloud”) instead of “orbits”
Region in space where there is 90% probability of finding an electron
Orbital Shape
Orbital
90% probability of
finding the electron
Electron Probability vs. Distance 40 30
Electron Probability (%) 20 10 50
100
150
200
250
Distance from the Nucleus (pm)
Courtesy Christy Johannesson

5. Shapes of s, p, and d-Orbitals
each holds 2 electrons (s2)
each of 3 orbitals holds 2 e - = 6 total p electrons (p6)
each of 5 orbitals holds 2 e - = 10 total d electrons (d10)

6. s, p, and d-orbitals s orbitals: p orbitals: d orbitals: Each holds 2
electrons
(outer orbitals of
Groups 1 and 2)
p orbitals:
Each of 3 sets holds
2 electrons = 6 electrons
(outer orbitals of
Groups 3 to 8)
d orbitals:
Each of 5 sets holds
2 electrons
= 10 electrons
(found in elements
in third period
and higher)
Orbital Filling Video

7. Orbitals overlap each other as you get farther from the nucleus
Copyright © 2006 Pearson Benjamin Cummings. All rights reserved.

8. f-orbitals
7 f 2 e- each = 14 e-

9. s, p, d and f orbitals
How many g orbitals could exist?

10. theoretical g-orbitals
9 g 2 e- each = 18 e-

11. Periodic Patterns for Electron Config8 1 2 1 2 3 4 5 6 7 3 4 5 6 7 1s 2s 3s 4s 5s 6s 7s 1s 2p 3p 4p 5p 6p 7p d
(n-1) 3d 4d 5d 6d 6 7 f
(n-2) 4f 5f

12. 1s1 Periodic Patterns 1st Period s-block Example - Hydrogen
# of e- in that orbital(s)
1st Period
s-block
Courtesy Christy Johannesson

13. Electron Configuration ReviewS
32.066 16
Electron Configuration Review
Longhand Configuration
S 16e-
1s2
2s2
2p6
3s2
3p4
Core Electrons
Valence Electrons
(Highest energy level)
Shorthand Configuration
S 16e- [Ne] 3s2 3p4
Courtesy Christy Johannesson

14. [Ar] 4s2 3d10 4p2 Periodic Patterns Ge Example - Germanium 32 72.61
Courtesy Christy Johannesson

15. Shorthand Configuration
neon's electron configuration(1s22s22p6) A B
3rd energy level (or 3rd period)
[Ne]
[Ne] 3s1
1 electron in the s orbital C D
orbital shape (s,p,d,f…etc.)
[ ]
Na =
1s22s22p6 3s1
electron configuration

16. Shorthand Configuration Practice
Element symbol
Electron configuration Ca
[Ar] 4s2 V
[Ar] 4s2 3d3 F
[He] 2s2 2p5 Ag
[Kr] 5s2 4d9 I
[Kr] 5s2 4d10 5p5 Xe
[Kr] 5s2 4d10 5p6 Fe
[He] 2s22p63s23p64s23d6
[Ar] 4s23d6 Sg
[Rn] 7s2 5f14 6d4

17. Periodic Patterns Review
energy level
(subtract for d & f)
Group # (1-8…excluding d block)
total # of valence e-
Column within Sublevel block
# of e- in sublevel/orbital
Courtesy Christy Johannesson

18. Periodic Patterns and Charge Trends+1 +2 d 1 2 3 4 5 6 7 +3
- 3
- 2
- 1 1s
NON-METALS
Variable Charge
METALS 6 7 f
(n-2)

19. Electron Configurations for Cations
Metals lose e- to attain a noble gas configuration
Metals form positive ions
Cations are “paws”itive
Metal ions will lose e- from configuration
Na: 1s22s22p63s1
Na+: 1s22s22p6 noble gas configuration

20. Formation of a Cation sodium atom sodium ion Na Na+ [Ne] 3s1 [Ne] 11p+
loss of
one valence
electron
11p+ e- e- e- e- e- e-

21. Electron Configurations for Anions
Non-metals gain electrons to attain a noble gas configuration
They form negative ions
Take a look at the e- configuration
S 1s22s22p63s23p4 (6 valence electrons)
+ 2e-
S2- 1s22s22p63s23p6 (noble gas configuration)

22. Formation of an Anion chlorine atom chloride ion Cl Cl – [Ne]3s23p5
[Ne]3s23p6 or [Ar]
gain of
one valence
electron e- e- e-
17p+ e- e- e- e- e- e-
17p+ e- e- e- e- e- e- e- e- e- e-

23. Stable Electron Configurations
All atoms react to achieve noble gas configuration
Noble gases have two s and six p electrons
Eight valence electrons
Also called the octet rule Ar

24. Bonding Review and Writing Ionic Formulas
Table salt
Bonding Review and Writing Ionic Formulas

25. Formation of Ionic Bond
chloride ion
Cl -
17p+ e-
sodium ion
Na+
11p+ e- - +

26. Ionic Bonding Anions and cations are held together by opposite charges
All ionic compounds are called salts
Simplest ratio is called the formula unit
The bond is formed through the transfer of electrons
Electrons are transferred to fill all available orbitals, or achieve a noble gas configuration

27. K+ e-
Br - e- Br K
potassium atom
bromine atom K+
O2- K+
potassium ion
potassium bromide
bromide ion
potassium oxide
KBr
K2O
Mg2+
Br -
Br -
magnesium bromide
MgBr2

28. ? Bonding Practice NaOH AlN Pb4+ N3- Pb3N4 CaBr2 lead (IV) nitride
Mg2+
OH -
Ca2+ ?
OH -
Pb4+
Pb N3-
Pb3N4
N3-
CaBr2
Mg(OH)2
lead (IV) nitride
Ca(OH)2 or
CaO
plumbic nitride

29. (NH4)3PO4 Ca3(PO4)2 Al2O3 FeO Ca2+ PO43- NH4+ PO43- Al3+ O2- NH4+ Ca2+

30. Subscripts, Superscripts and Coefficients
Mg2+
PO43-
Mg3(PO4 )2 5
coefficient
subscripts
MAGNESIUM PHOSPHATE

31. Writing Formulas of Ionic Compounds
chemical formula:
has neutral charge;
shows types of atoms and how many of each
To write an ionic compound’s formula, we need:
1. the two types of ions
2. the charge on each ion
Na+ and F–
Ba and O2–
Na+ and O2–
Ba and F–
NaF
BaO
Na2O
BaF2

32. The Importance of Parentheses
Calcium hydrox
ide
ide
Ca2+
OH-
Ca - O H
CaOH2
vs.
Ca(OH)2
HO - Ca - OH
The formulas imply two totally different compounds!

33. Writing Formulas w/Polyatomic Ions
Parentheses are required only when you need more
than one “bunch” of a particular polyatomic ion
Ba and SO42–
BaSO4
Mg and NO2–
Mg(NO2)2
NH4+ and ClO3–
NH4ClO3
Sn4+ and SO42–
Sn(SO4)2
Fe3+ and Cr2O72–
Fe2(Cr2O7)3
NH4+ and N3–
(NH4)3N

34. Traditional (OLD) System of Nomenclature
…used historically (and still some today) to name
compounds w/multiple-charge cations
To use:
1. Use Latin root of cation.
2. Use -ic ending for higher charge
“ -ous “ “ lower “
3. Then say name of anion, as usual.
; (“icky” food is good for you!)
; (“delicious” food is not good for you!)
Element Latin root ic ous
gold, Au aur- Au Au1+
lead, Pb plumb- Pb Pb2+
tin, Sn stann- Sn Sn2+
copper, Cu cupr- Cu Cu1+
iron, Fe ferr- Fe Fe2+

35. Write formulas:
Write names:
cuprous sulfide
Pb3P4
3 Pb? 4 P3–
Cu1+
S2–
Cu2S
plumbic phosphide
auric nitride
Pb3P2
3 Pb? 2 P3–
Au3+
N3–
AuN
plumbous phosphide
ferrous fluoride
SnCl4
Sn? 4 Cl1–
Fe2+
F1–
FeF2
stannic chloride

36. Nomenclature - Humor BaNa2 “BaNaNa” “Ferrous Wheel” Fe2+ A KNiFe
What weapon can you make
from the elements nickel,
potassium and iron?
Fe = iron (Latin = ferrum)
Fe2+ = lower oxidation state = ferrous
Fe3+ = higher oxidation state = ferric
A KNiFe

37. Teacher: What is the formula for water?
Student: H, I, J, K, L, M, N, O
Teacher: That’s not what I taught you.
Student: But you said the formula for water was…H to O.
"H-O-H"?! WHAT'S
THAT SPELL?!
WATER?
mis
mis
Website: Dihydrogen monoxide Information Campaign
“Little Johnny took a drink,
Now he shall drink no more.
For what he thought was H2O,
Was H2SO4.”
A sign outside the chemistry hotel reads “Great Day Rates, Even Better NO3-1s”
What do you do with a dead chemist? Barium
Under aged Pb walks into a bar and the bartender turns to the gold
Bouncer and says, “Au, get the lead out!”

38. Four Types of Naming Fixed Charge Ionic Compounds
Variable Charge Ionic Compounds
Acidic Compounds
Covalent Molecules
Contain a metal with a fixed charge and a non-metal (ionic)
Contain a metal with a variable charge and a non-metal (ionic)
Contain H+ with various anions (ionic when aqueous)
Contain 2 or more nonmetals only

39. Variable charge cations Elemental anions
Fixed charge cations
Variable charge cations 1+ H 1 He 2
Elemental anions H 1 1 2+ 3+ 3- 2- 1- Li 3 Be 4 B 5 C 6 N 7 O 8 F 9 Ne 10 2 Na 11 Mg 12 Al 13 Si 14 P 15 S 16 Cl 17 Ar 18 3 K 19 Ca 20 Sc 21 Ti 22 V 23 Cr 24 Mn 25 Fe 26 Co 27 Ni 28 Cu 29 Zn 30 Ga 31 Ge 32 As 33 Se 34 Br 35 Kr 36 4 Rb 37 Sr 38 Y 39 Zr 40 Nb 41 Mo 42 Tc 43 Ru 44 Rh 45 Pd 46 Ag 47 Cd 48 In 49 Sn 50 Sb 51 Te 52 I 53 Xe 54 5 Cs 55 Ba 56 Hf 72 Ta 73 W 74 Re 75 Os 76 Ir 77 Pt 78 Au 79 Hg 80 Tl 81 Pb 82 Bi 83 Po 84 At 85 Rn 86 6 * Fr 87 Ra 88 Rf
104 Db
105 Sg
106 Bh
107 Hs
108 Mt
109 7 W La 57 Ce 58 Pr 59 Nd 60 Pm 61 Sm 62 Eu 63 Gd 64 Tb 65 Dy 66 Ho 67 Er 68 Tm 69 Yb 70 Lu 71 Ac 89 Th 90 Pa 91 U 92 Np 93 Pu 94 Am 95 Cm 96 Bk 97 Cf 98 Es 99 Fm
100 Md
101 No
102 Lr
103

40. Fixed Charge Exceptions
Start with Al
Go backwards down the stairs
Decrease the charge after
each stair 3+ Al 13 3+ Zn 30 2+ Ag 47 +

41. Fixed Charge Compound Nomenclature
Metals (fixed charge) + Nonmetals
Objectives:
To predict the ionic charge on a cation in a binary ionic compound.
To write systematic names and formulas for binary ionic compounds.

42. Fixed Charge Compounds
Compounds that contain a metal with a fixed charge
(group 1, 2, and 3, with Zn2+, Ag+, etc.), and a non-metal
To name these compounds, use the name of metal and the
name of the non-metal with the ending replaced by the suffix –ide
Examples:
NaCl (Na+ Cl-)
sodium chloride
CaS (Ca2+ S2-)
calcium sulfide
AlI3 (Al3+ 3I-)
aluminum iodide

43. Common Simple Cations and Anions
Cation Name Anion Name*
H+ hydrogen H - hydride
Li+ lithium F - fluoride
Na+ sodium Cl - chloride
K+ potassium Br - bromide
Cs+ cesium I - iodide
Be2+ beryllium O 2- oxide
Mg2+ magnesium S 2- sulfide
Al3+ aluminum N 3- nitride
Ag+ silver P 3- phosphide
Zn2+ zinc
*The root is given in color
EXCEPTIONS
Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 86

44. “Perhaps one of you gentlemen would mind telling me just
what is outside the window that you find so attractive..?”
Image courtesy NearingZero.net

45. Fixed Charge Naming Practice
Formula Name
barium oxide
BaO ____________________
________________ sodium bromide
MgI2 ____________________
KCl ____________________
________________ strontium fluoride
________________ cesium fluoride
NaBr
magnesium iodide
potassium chloride
SrF2
CsF

46. Fixed Charge Nomenclature w/Polyatomic Ions
Simply insert the name of the
polyatomic ion into the final name
Ba2+ and SO42–
BaSO4
barium sulfate
Mg2+ and NO2–
Mg(NO2)2
magnesium nitrite
NH4+ and ClO3–
NH4ClO3
ammonium chlorate
Al3+ and SO42–
Al2(SO4)3
alumnium sulfate
Na+ and Cr2O72–
Na2Cr2O7
sodium dichromate
NH4+ and N3–
(NH4)3N
ammonium nitride

47. Polyatomic Ions Quiz PO43- …………… phosphate SO42- …………… sulfate
Cr2O72- …………..
MnO4- …………..
CH3COO- …….
phosphate
sulfate
dichromate
permanganate
acetate

48. Variable Charge Compound Nomenclature
Metals (variable charge) + Nonmetals
Objectives:
To predict the ionic charge on a cation in a binary ionic compound.
To write systematic names and formulas for binary ionic compounds.

49. Roman Numeral Review Greek Number Roman Numeral 1 I 2 II 3 III 4 IV 56 VI 7
VII 8
VIII 9 IX 10 X
Number
Roman Numeral 1 I 5 V 10 X 50 L
100 C

50. Variable charge cations Elemental anions
Single charge cations 1+
Variable charge cations H 1 He 2
Elemental anions H 1 1 2+ 3+ 3- 2- 1- Li 3 Be 4 B 5 C 6 N 7 O 8 F 9 Ne 10 2 Na 11 Mg 12 Al 13 Si 14 P 15 S 16 Cl 17 Ar 18 3 K 19 Ca 20 Sc 21 Ti 22 V 23 Cr 24 Mn 25 Fe 26 Co 27 Ni 28 Cu 29 Zn 30 Ga 31 Ge 32 As 33 Se 34 Br 35 Kr 36 4 Rb 37 Sr 38 Y 39 Zr 40 Nb 41 Mo 42 Tc 43 Ru 44 Rh 45 Pd 46 Ag 47 Cd 48 In 49 Sn 50 Sb 51 Te 52 I 53 Xe 54 5 Cs 55 Ba 56 Hf 72 Ta 73 W 74 Re 75 Os 76 Ir 77 Pt 78 Au 79 Hg 80 Tl 81 Pb 82 Bi 83 Po 84 At 85 Rn 86 6 * Fr 87 Ra 88 Rf
104 Db
105 Sg
106 Bh
107 Hs
108 Mt
109 7 W La 57 Ce 58 Pr 59 Nd 60 Pm 61 Sm 62 Eu 63 Gd 64 Tb 65 Dy 66 Ho 67 Er 68 Tm 69 Yb 70 Lu 71 Ac 89 Th 90 Pa 91 U 92 Np 93 Pu 94 Am 95 Cm 96 Bk 97 Cf 98 Es 99 Fm
100 Md
101 No
102 Lr
103

51. Variable Charge Ionic Compounds
Compounds that contain a metal with variable charge (Pb, Sn, and the transition metals—not including Ag or Zn), and a non-metal
To name, given the formula:
1. Figure out charge on cation
Stock System
of nomenclature
2. Write name of cation
3. Write Roman numerals in ( )
to show cation’s charge

52. Variable charge Naming Practice
4. Write name of anion:
FeO Fe? O2–
Fe2O3 2 Fe? 3 O2–
CuBr Cu? Br –
CuBr2 Cu? 2 Br –
iron(II) oxide
iron(III) oxide
copper(I) bromide
copper(II) bromide

53. Variable Charge Cations
Common Type II Cations
Ion Stock System Traditional System
Fe 3+ iron (III) ferric
Fe 2+ iron (II) ferrous
Cu 2+ copper (II) cupric
Cu 1+ copper (I) cuprous
Co 3+ cobalt (III) cobaltic
Co 2+ cobalt (II) cobaltous
Sn 4+ tin (IV) stannic
Sn 2+ tin (II) stannous
Pb 4+ lead (IV) plumbic
Pb 2+ lead (II) plumbous
Hg 2+ mercury (II) mercuric
Hg2 2+ mercury (I) mercurous
*Mercury (I) ions are always bonded together in pairs to form Hg2 2+
Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 90

54. Variable Charge Ionic Compounds
To find the formula, given the name:
1. Write symbols for the two types of ions
2. Balance charges to write formula
cobalt (III) chloride Co3+ Cl–
tin (IV) oxide Sn4+ O2–
tin (II) oxide Sn2+ O2–
CoCl3
SnO2
SnO

55. Naming Variable Charge Ionic Compounds
Formula Name
mercury (I) oxide
Hg2O ____________________
HgO ____________________
________________ copper (II) fluoride
________________ copper (I) sulfide
Cr2O3 ____________________
________________ lead (IV) oxide
mercury (II) oxide
CuF2
Cu2S
chromium (III) oxide
PbO2

56. Ionic Compounds with Polyatomic Ions
Fe3(PO4) 2
________________ iron (II) phosphate
________________ ammonium carbonate
________________ aluminum sulfate
V2SO3 ____________________
AgCN ____________________
Ba(ClO3)2 ____________________
________________ copper (II) hydroxide
(NH4)2CO3
Al2(SO4)3
vanadium (I) sulfite
silver cyanide
barium chlorate
Cu(OH)2

57. Acidic Compounds
Oxysalts + H2O  Oxyacids

58. Acidic Compounds (Nonmetals Dissolved in Water)
Acids(aq) without oxygen
The prefix hydro- is used to represent hydrogen, followed by the root name of the nonmetal with its ending replaced by the suffix –ic acid.
(aq) = aqueous or dissolved in water
Examples:
*HCl(aq)
HBr(aq)
Hydrochloric acid
Hydrobromic acid
*The name of this gas would be hydrogen monochloride if it was NOT dissolved in water.

59. Acidic Compounds Nonmetals Dissolved in Water
Acids(aq) WITH oxygen (oxyacids)
Start with the name of the polyatomic ion (with oxygen), and change the ending based on the following rule:
If the ion ends in “ate,” change the suffix to –ic acid.
If the ion ends in “ite,” change the suffix to –ous acid.
Retain any prefixes such as “per” or “hypo” in front of the acid name. NEVER use “hydro”!
Examples:
HClO3(aq)
HBrO(aq)
ClO3- = chlorate
Chloric acid
BrO- = hypobromite
Hypobromous acid

60. Oxyacid Naming Rules An ion with a name ending in An acid with a
-ite
-ous
-ate
-ic
Hill, Petrucci, General Chemistry An Integrated Approach 1999, page 60

61. Common Oxyacid Names
The following table lists the most common families of oxy acids.
one more
oxygen atom
HClO4
perchloric acid
most
“common”
HClO3
chloric acid
H2SO4
sulfuric acid
H3PO4
phosphoric acid
HNO3
nitric acid
one less
oxygen
HClO2
chlorous acid
H2SO3
sulfurous acid
H3PO3
phosphorous acid
HNO2
nitrous acid
two fewer
oxygens
HClO
hypochlorous acid
H3PO2
hypophosphorous acid

62. Acid Nomenclature Practice
Formula Name
hydrochloric acid
HCl ____________________
HClO ____________________
________________ sulfuric acid
________________ hydrofluoric acid
H3N ____________________
________________ periodic acid
hypochlorous acid
H2SO4 HF
hydronitric acid
HIO4

63. Covalent Compounds Nonmetal + Nonmetal Objectives:
To write systematic names and formulas for binary molecular compounds.

64. Writing Formulas of Covalent Compounds
contain two or more non-metals (NO METALS!)
Key: FORGET CHARGES
To Name, given the formula:
1. Use Greek prefixes to indicate how many atoms
of each element, but don’t use “mono” on first element (least electronegative, excluding H)
2. Add the suffix –ide to the second element (most electronegative)
1 mono 6 hexa
2 di 7 hepta
3 tri 8 octa
4 tetra 9 nona
5 penta 10 deca
Prefixes to memorize!

65. Covalent Nomenclature Practice
EXAMPLES:
carbon dioxide CO
dinitrogen trioxide
SF6
carbon tetrachloride
NI3
CO2
carbon monoxide
N2O3
sulfur hexafluoride
CCl4
nitrogen triiodide

66. More Practice with covalent compounds…
As2S3
________________ diarsenic trisulfide
________________ sulfur dioxide
P2O5 ____________________
________________ nitrogen trihydride
N2O5 ____________________
H2O ____________________
SO2
diphosphorus pentoxide
NH3
dinitrogen pentoxide
dihydrogen monoxide

67. Naming Simple Chemical Compounds
Ionic (metal and nonmetal)
Covalent (2 nonmetals)
Metal
Nonmetal
First
nonmetal
Second
nonmetal
Forms
only one
positive
ion
Forms
more than
one positive
ion
Single
Negative
Ion
Polyatomic
Ion
Use the
name of
element
Use element
name followed
by a Roman
numeral to
show the charge
Use the name
of the
element, but
end with ide
Use the
name of
polyatomic
ion (ate or
Ite)
Before
element name
use a prefix
to match
subscript
Use a prefix
before
element name
and end
with ide

68. Overall Nomenclature PracticeIr Ca Ti H Ba N3 Zn N Au Na F3 S S2
Cl(aq)
Br2 P2
F(aq) I2
Cl4
2O3 3P
iridium (III)
calcium
titanium (IV)
hydrochloric acid
barium
trinitrogen
hydrofluoric acid
zinc
nitrogen
gold (III)
sodium
fluoride
sulfide
bromide
diphosphide
iodide
tetrachloride
oxide
phosphide
Ionic/variable
Ionic/fixed
Acid
Covalent

69. Ionic Nomenclature Practice
Ir2 Ca H Pt Sr K Zn Mn Au H2
(Cr2O7)3
(OH)2
NO3 (aq)
(CH3COO)2
BrO2(aq)
SO4 CN
(NO2)2
(ClO3)4
PO4
SO3 (aq)
iridium (III)
calcium
nitric
platinum (II)
bromous
strontium
potassium
zinc
manganese (IV)
gold (III)
sulfurous
dichromate
hydroxide
acid
acetate
sulfate
cyanide
nitrite
chlorate
phosphate
Ionic/variable
Ionic/fixed
Acid

70. Covalent Ionic (M + NM) Ionic (M + NM) Two or more NM’s
Variable charge cation
Fixed charge cation
carbon tetrabromide
sulfur dichloride
N2O5
NCl3
vanadium (II) chromate
niobium (V) perchlorate
Mn2S5
Pt(IO3)4
rubidium sulfate
barium oxide
NH4ClO3 KI
Greek prefixes
Roman
numeral
Roman numeral
for name only
Charge
Polyatomic ions OK
Polyatomic ions OK
Where would you file these?
Criss-Cross
Rule
VCrO4
VCrO4
dinitrogen pentoxide
dinitrogen pentoxide
BaO
BaO
platinum (IV) iodate
platinum (IV) iodate
CBr4
CBr4
ammonium chlorate
ammonium chlorate
Roman
numeral
Nb(ClO4)5
Nb(ClO4)5
potassium iodide
potassium iodide
SCl2
SCl2
nitrogen trichloride
nitrogen trichloride
Rb2SO4
Rb2SO4
manganese (V) sulfide
manganese (V) sulfide

71. Suffixes have meaning “-ide” binary compound
sodium chloride (NaCl)
“-ite” or “-ate” polyatomic compound
sulfite (SO32-)
sulfate (SO42-) “-ate” means one more oxygen than “-ite”
“-ol” alcohol
methyl alcohol (methanol)
“-ose” sugar
sucrose
“-ase” enzyme
sucrase

72. Extra Slides H O S

73. Compounds Containing Polyatomic Ions
Insert name of ion where it should go in the compound’s name.
Write formulas:
iron (III) nitrate
ammonium phosphide
ammonium chlorite
zinc phosphate
lead (II) permanganate
Fe3+ 3
NO31–
Fe(NO3)3 3
NH41+
P3–
(NH4)3P
NH41+
ClO21–
NH4ClO2 3
Zn2+ 2
PO43–
Zn3(PO4)2
Pb2+ 2
MnO41–
Pb(MnO4)2

74. Writing Formulas of Ionic Compounds
Write names:
(NH4)2S2O3
AgBrO3
(NH4)3N
U(CrO4)3
Cr2(SO3)3
ammonium thiosulfate
silver bromate
ammonium nitride U ? 6+ 3
CrO42–
uranium (VI) chromate 2 Cr ? 3+ 3
SO32–
chromium (III) sulfite

75. Traditional (OLD) System of Nomenclature
…used historically (and still some today) to name
compounds w/multiple-charge cations
To use:
1. Use Latin root of cation.
2. Use -ic ending for higher charge
“ -ous “ “ lower “
3. Then say name of anion, as usual.
; (“icky” food is good for you!)
; (“delicious” food is not good for you!)
Element Latin root ic ous
gold, Au aur- Au Au1+
lead, Pb plumb- Pb Pb2+
tin, Sn stann- Sn Sn2+
copper, Cu cupr- Cu Cu1+
iron, Fe ferr- Fe Fe2+

76. Write formulas:
Write names:
cuprous sulfide
Pb3P4
3 Pb? 4 P3–
Cu1+
S2–
Cu2S
plumbic phosphide
auric nitride
Pb3P2
3 Pb? 2 P3–
Au3+
N3–
AuN
plumbous phosphide
ferrous fluoride
SnCl4
Sn? 4 Cl1–
Fe2+
F1–
FeF2
stannic chloride

77. BrO41- BrO31- BrO21- BrO1- CO42- CO32- CO22- CO2- ClO41- ClO31- ClO21-
Polyatomic Ion:
a group of atoms that stay together and have a single, overall charge.
BrO41-
Perbromate ion
BrO31-
Bromate ion
BrO21-
Bromite ion
BrO1-
Hypobromite ion
CO42-
CO32-
Carbonate ion
CO22-
CO2-
ClO41-
ClO31-
Chlorate ion
ClO21-
ClO1-
IO41-
IO31-
Iodate ion
IO21-
IO1-
NO41-
NO31-
Nitrate ion
NO21-
NO1-
PO53-
PO43-
Phosphate ion
PO33-
PO23-
SO52-
SO42-
Sulfate ion
SO32-
SO22-
1 more oxygen
“normal”
1 less oxygen
2 less oxygen

78. Multiple-charge cation Everything else
Two nonmetals
Multiple-charge cation
Everything else
carbon tetrabromide
sulfur dichloride
N2O5
NCl3
vanadium (II) chromate
niobium (V) perchlorate
Mn2S5
Pt(IO3)4
rubidium sulfate
barium oxide
NH4ClO3 KI
Greek prefixes
Roman numeral
for name only
Roman
numeral
Charge
Polyatomic ions OK
Polyatomic ions OK
Where would you file this?
Criss-
Cross
Rule
VCrO4
VCrO4
dinitrogen pentoxide
dinitrogen pentoxide
BaO
BaO
platinum (IV) iodate
platinum (IV) iodate
CBr4
CBr4
ammonium chlorate
ammonium chlorate
Roman
numeral
Nb(ClO4)5
Nb(ClO4)5
potassium iodide
potassium iodide
SCl2
SCl2
nitrogen trichloride
nitrogen trichloride
Rb2SO4
Rb2SO4
manganese (V) sulfide
manganese (V) sulfide

79. Multiple-charge cation Everything else
Two nonmetals
Multiple-charge cation
Everything else
Greek prefixes
Roman numeral
for name only
Roman
numeral
Charge
Polyatomic ions OK
Polyatomic ions
Where would you file this?
Criss-
Cross
Rule
VCrO4
dinitrogen pentoxide
BaO
platinum (IV) iodate
CBr4
ammonium chlorate
Roman
numeral
Nb(ClO4)5
potassium iodide
SCl2
nitrogen trichloride
Rb2SO4
manganese (V) sulfide

80. Write the compound formed by the following ions:
1) Al3+ S2-
2) Mg2+ PO43-
When a formula is given…write the proper name.
When a name is given…write the proper formula.
3) BaO
4) lithium bromide
5) Ni2S3
6) triphosphorus heptoxide
7) N2O5
8) molybdenum (VI) nitride
9) trinitrotoluene (TNT)… CH3C6H2(NO2)3
10) phosphoric acid H3PO4
Write the total number of atoms that make up each compound.
Extra credit: What is the formula for plumbic iodide? (Hint: lead is Pb2+ or Pb4+)

81. POP QUIZ Write the compound formed by the following ions: 1) Al3+ S2-
2) Mg2+ PO43-
When a formula is given…write the proper name.
When a name is given…write the proper formula.
3) BaO
4) lithium bromide
5) Ni2S3
6) triphosphorus heptoxide
7) N2O5
8) molybdenum (VI) nitride
9) trinitrotoluene (TNT)… CH3C6H2(NO2)3
10) phosphoric acid H3PO4
Write the total number of atoms that make up each compound.
Extra credit: What is the formula for plumbic iodide? (Hint: lead is Pb2+ or Pb4+)