1. Compounds

2. Binary Compounds NaCl sodium chloride (Na1+ Cl1-)
Binary compounds that contain a metal of fixed oxidation number
(group 1, group 2, Al, Zn, Ag, etc.), and a non-metal.
To name these compounds, give the name of metal followed by the
name of the non-metal, with the ending replaced by the suffix –ide.
Examples:
NaCl sodium chloride (Na1+ Cl1-)
CaS calcium sulfide (Ca2+ S2-)
AlI3 aluminum iodide (Al I1-)

3. Common Simple Cations and Anions
Cation Name Anion Name*
H 1+ hydrogen H 1- hydride
Li 1+ lithium F 1- fluoride
Na 1+ sodium Cl 1- chloride
K 1+ potassium Br 1- bromide
Cs 1+ cesium I 1- iodide
Be 2+ beryllium O 2- oxide
Mg 2+ magnesium S 2- sulfide
Al 3+ aluminum
Ag 1+ silver
*The root is given in color.
Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 86

5. Example: Aluminum Chloride
Criss-Cross Rule
Example: Aluminum Chloride
Step 1:
write out name with space
Al Cl 3+ 1-
Step 2:
write symbols & charge of elements
Al Cl
Step 3: 1 3
criss-cross charges as subsrcipts
Step 4: AlCl 3
combine as formula unit
(“1” is never shown)

6. Example: Aluminum Chloride
Criss-Cross Rule
Example: Aluminum Chloride
Step 1: Aluminum Chloride
Step 2: Al3+ Cl1-
Step 3: Al Cl 1 3
Step 4: AlCl 3

7. Example: Aluminum Oxide
Criss-Cross Rule
Example: Aluminum Oxide
Step 1: Aluminum Oxide
Step 2: Al3+ O2-
Step 3: Al O 2 3
Step 4: Al2O3

8. Example: Magnesium Oxide
Criss-Cross Rule
Example: Magnesium Oxide
Step 1: Magnesium Oxide
Step 2: Mg2+ O2-
Step 3: Mg O 2 2
Step 4: Mg2O2
Step 5: MgO

9. Naming Binary Compounds
Formula Name
barium oxide
BaO ____________________
________________ sodium bromide
MgI2 ____________________
KCl ____________________
________________ strontium fluoride
________________ cesium fluoride
NaBr
magnesium iodide
potassium chloride
SrF2
CsF

10. Ternary Compounds Objectives:
To determine the ionic charge on a cation in a ternary ionic compound.
To write systematic names and formulas for ternary ionic compounds.

11. Ternary Compounds
Ternary compounds are those containing three different elements.
(NaNO3, NH4Cl, etc.). The naming of ternary compounds involves the
memorization of several positive and negative polyatomic ions, (two or
more atoms per ion), and adding these names to the element with which
they combine.
i.e., Sodium ion, Na1+ added to the nitrate ion, NO31-, to give the compound, NaNO3, sodium nitrate.
Binary rules for indicating the oxidation number of metals and for indicating
the numbers of atoms present are followed. The polyatomic ions that should
be learned are listed in a separate handout.

12. Ternary Compounds NaNO2 sodium nitrite KClO3 potassium chlorate
Ca3(PO4)2 calcium phosphate
Fe(OH)3 iron (III) hydroxide
NaHCO3 sodium bicarbonate
‘sodium hydrogen carbonate’

13. Common Polyatomic Ions
Names of Common Polyatomic Ions
Ion Name Ion Name
NH ammonium CO carbonate
NO nitrite HCO hydrogen carbonate
NO nitrate (“bicarbonate” is a widely
SO sulfite used common name)
SO sulfate ClO hypochlorite
HSO hydrogen sulfate ClO chlorite
(“bisulfate” is a widely ClO chlorate
used common name) ClO perchlorate
OH hydroxide C2H3O acetate
CN cyanide MnO permanganate
PO phosphate Cr2O dichromate
HPO hydrogen phosphate CrO chromate
H2PO dihydrogen phosphate O peroxide
Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 100

14. Ternary Compounds Ca3(PO4) 2 ________________ calcium phosphate
________________ ammonium carbonate
________________ aluminum sulfate
Na2SO4 ____________________
LiCN ____________________
Ba(ClO3)2 ____________________
________________ copper (II) hydroxide
(NH4)2CO3
Al2(SO4)3
sodium sulfate
lithium cyanide
barium chlorate
Cu(OH)2

15. Magnesium Phosphate Step 1: Magnesium Phosphate Step 2: Mg2+ PO43-

16. Polyatomic Ions - Memorize
Eight “-ATE’s”
PO43- ……………
SO42- ……………
CO32- …………..
ClO31- …………..
NO31- ………..….
phosphate
sulfate
carbonate
chlorate
nitrate
phosphATE
sulfATE
carbonATE
chlorATE
nitrATE
Exceptions:
ammonium
hydroxide
cyanide
NH41+ ……………
OH1- ……………
CN1- …………..

17. 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

18. 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

19. 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) triphosphorous heptaoxide
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+)

20. 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) triphosphorous heptaoxide
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+)

21. Answer Key
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) triphosphorous heptaoxide
7) N2O5
8) molybdenum (VI) nitride
9) trinitrotoluene (TNT)… CH3C6H2(NO2)3
10) phosphoric acid H3PO4
Al2S3
Mg3(PO4)2
barium oxide
LiBr
nickel (III) sulfide
P3O7
dinitrogen pentaoxide
MoN2
Write the total number of atoms that make up each compound. 21 8
Extra credit: What is the formula for plumbic iodide? (Hint: lead is Pb2+ or Pb4+)
PbI4

22. Polyatomic Ions - Quiz C2O42- …………… oxalate CrO42- …………… chromate
MnO41- …………..
CH3COO1- …….
oxalate
chromate
dichromate
permanganate
acetate

23. Exceptions!
Two exceptions to the simple –ide ending are the diatomic oxide ions,
O22- and O21-.
O22- is called peroxide
O21- is called superoxide.
Note the differences.
barium oxide __________
barium peroxide __________
BaO
BaO2
Ba2+
sodium oxide __________
sodium peroxide __________
Na2O
Na2O2
Na1+
Do Not Reduce to lowest terms!
potassium oxide __________
potassium superoxide __________
K2O
KO2
K1+

24. Ionic Compounds: Polyatomic Ions
Polyatomic Ions Grid to Memorize
Chart of the Ions and Polyatomic Ions
Keys

25. Ionic Binary Compounds: Multiple-Charge Cations
Keys

26. Naming Chemical Compounds
Binary Compound? No
Yes
Polyatomic ions
present?
Use the strategy
summarized
earlier No
Yes
This is a compound
for which naming
procedures have not yet
been considered.
Name the compound
using procedures similar
to those for naming
binary ionic compounds.
Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 102

27. Oxidation Numbers and Ionic Compounds
Keys

28. Names and Formulas of Compounds
Keys

29. Subscripts, Superscripts and Coefficients

30. Electronegativities Period H B P As Se Ru Rh Pd Te Os Ir Pt Au Po At
2.1 B
2.0 P As Se
2.4 Ru
2.2 Rh Pd Te Os Ir Pt Au Po At 1 1 2A 3A 4A 5A 6A 7A
Actinides: Li
1.0 Ca Sc
1.3 Sr Y
1.2 Zr
1.4 Hf Mg La
1.1 Ac
Lanthanides: * y Be
1.5 Al Si
1.8 Ti V
1.6 Cr Mn Fe Co Ni Cu
1.9 Zn
1.7 Ga Ge Nb Mo Tc Ag Cd In Sn Sb Ta W Re Hg Tl Pb Bi N
3.0 O
3.5 F
4.0 Cl C
2.5 S Br
2.8 I 2 2 Na
0.9 K
0.8 Rb Cs
0.7 Ba Fr Ra
Below 1.0 3 3 3B 4B 5B 6B 7B 8B 1B 2B
Period 4 4 5 5 6 6
Linus Pauling ( ) awarded Nobel Prize in chemistry in 1954 for his 1939 text, The Nature of the Chemical Bond,
and also won the Nobel Peace Prize in 1962 for his fight to control nuclear weapons.
The greater the electronegativity of an atom in a molecule, the more strongly it attracts the electrons in a covalent bond. 7
Hill, Petrucci, General Chemistry An Integrated Approach 2nd Edition, page 373

31. Interpretation of a Chemical FormulaS
Sulfuric Acid
H2SO4
Two atoms
of hydrogen
One atom
of sulfur
Four atoms
of oxygen

32. C8H18 Chemical Formulas Subscript indicates that
there are 8 carbon atoms
in a molecule of octane.
Subscript indicates that
there are 18 hydrogen atoms
In a molecule of octane.
Davis, Metcalfe, Williams, Castka, Modern Chemistry, 1999, page 203

33. Stock System of Nomenclature
CuCl2
Name of Roman
cation numeral
indicating
charge
Name of anion +
copper (II)
chloride

34. Al2(SO4)3 Chemical Formulas Subscript 2 refers to 2 aluminum atoms.
4 oxygen
atoms in
sulfate ion.
Subscript 3 refers to
everything inside parentheses.
Here there are 3 sulfate ions,
with a total of 3 sulfur atoms
and 12 oxygen atoms.
Davis, Metcalfe, Williams, Castka, Modern Chemistry, 1999, page 204

35. Naming Binary Ionic Compounds
Al2O3
Name of cation Name of anion
aluminum oxide
Davis, Metcalfe, Williams, Castka, Modern Chemistry, 1999, page 207

36. The Stock System of Nomenclature
CuCl2
Name of Name of anion
cation
Roman
numeral
indicating
charge +
Copper (II) chloride
Davis, Metcalfe, Williams, Castka, Modern Chemistry, 1999, page 208

37. Bonding Activity

38. Common Polyatomic Ions

39. K1+ e- e-
Br1- Br K Br
potassium atom
bromine atom e- K
potassium atom
bromine atom
Br1-
K1+
potassium ion
bromide ion
potassium ion
potassium bromide
bromide ion
KBr
Mg2+
Br1-
K1+
O2-
Br1-
K1+
magnesium bromide
potassium oxide
MgBr2
K2O

40. ? K1+ Br1- Al3+ N3- Pb4+ PO43- K1+ O2- K1+ Ca2+ S2- Mg2+ Br1- OH1-
Cu2+
Br1-
NH41+
NO31-
OH1-

41. Chemical Bonding Activity
Pb4+
N3-
Na1+
OH1-
Al3+
N3-
Pb4+
N3-
N3-
(metal)
M2+
M1+
N2-
Pb4+
(metal)
M1+
(metal)
(nonmetal)
N3-
Ca2+ ?
Pb4+
Mg2+
OH1-
Pb N3-
N3-
Pb3N4
OH1-
lead (IV) nitride or
plumbic nitride

42. Chemical Bonding Activity
          Chemical Bonding Activity (pink/blue)
Chemical Bonding Activity Pieces
          Chemical Bonding Activity (pink/blue)
Chemical Bonding Activity Pieces
Keys

43. 4. Al3+ N3- 5. 1. K1+ Br1- KBr K1+ O2- 2. AlN K1+ 6. OH1- Cu2+ K2O
Key 4.
Al3+
N3-
Pb4+
N3- 5. 1.
K1+
Br1-
KBr
N3-
Pb4+
K1+
O2- 2.
AlN
K1+
N3- 6.
OH1-
Cu2+
K2O
Pb4+
OH1-
N3- 3.
Mg2+
Br1-
Cu(OH)2
Br1- 7.
NH41+
NO31-
Pb3N4
MgBr2
NH4NO3

44. 8. Ca2+ PO43- 9. NH41+ PO43- 10. Al3+ O2- NH41+ Ca2+ NH41+ O2- PO43-
Key 8.
Ca2+
PO43- 9.
NH41+
PO43-
10.
Al3+
O2-
NH41+
Ca2+
NH41+
O2-
PO43-
Al3+
(NH4)3PO4
Ca2+
O2-
11.
Fe2+
O2-
Ca3(PO4)2
Al2O3
FeO

45. 13. Pb4+ S2- 14. Pb2+ S2- 12. Fe3+ O2- PbS O2- 15. Cu2+ O2- Pb4+ S2-
Key
14.
Pb2+
S2-
12.
Fe3+
O2-
PbS
O2-
15.
Cu2+
O2-
Pb4+
S2-
Fe3+
O2-
CuO
16.
Cu1+
O2-
Cu1+
Fe2O3
Cu2O
Pb2S3
Pb2S4
PbS2

46. Molecular Models Activity
Keys

47. Molecular Models Activity
carbon tetrachloride
methane
water
ethane
ethyne
dihydrogen monosulfide
carbon dioxide
ammonia
hydrogen monochloride
trichloromethane
urea
propane
butane
nitrogen triiodide (video)
supplies

48. Bonding and Shape of Molecules
Number
of Bonds
Number of
Unshared Pairs
Covalent
Structure
Shape
Examples 2 3 4 1 2
-Be-
Linear
Trigonal planar
Tetrahedral
Pyramidal
Bent
BeCl2
BF3
CH4, SiCl4
NH3, PCl3
H2O, H2S, SCl2 B C N : O :

49. Carbon tetrachloride Cl Cl C Cl Cl Cl C CCl4 Tetrahedral geometry
Carbon tetrachloride – “carbon tet” had been used as dry cleaning solvent
because of its extreme non-polarity.

50. Methane H H C H H H C Tetrahedral geometry
Methane –The first member of the paraffin (alkane) hydrocarbons series.
a.k.a. (marsh gas, CH4).

51. Water
d(-) .. ..
SO2
Bent
geometry H O
d(+)
Polar molecule

52. Ethane H H H C C H H H C2H4 C = 1s22s22p2 ball-and-stick
Lewis dot notation
C2H4
molecular formula
space-filling molecule

53. Ethane H H H C C H H H C2H4 ball-and-stick Lewis dot notation
molecular formula
space-filling molecule

54. Ethyne H C C H C H C H H C C H C2H2 No octet 6 electrons = triple bond
each C “feels” 6 electrons H C C H C H C H
Stable octet
C2H2 H C C H
each C “feels” 7 carbons
Ethyne – a.k.a. “acetylene”

55. Dihydrogen monosulfide.. ..
SO2 H S
Bent

56. Carbon dioxide O C O O C O O C
Linear
geometry
CO2

57. Ammonia N
107o H .. .. N H N H N H H
NH3 H
Trigonal
Pyramidal
geometry

58. Hydrogen monochlorideCl H H Cl Cl
HCl
d(+)
d(-)
HCl(g) + H2O(l)  HCl(aq)
hydrogen
chloride
water
hydrochloric
acid
Polar molecule

59. Trichloromethane H H Cl C Cl Cl C Cl Cl Cl H C Cl d(+) CHCl3 d(-)
Tetrahedral geometry
Polar molecule

60. Urea H H H H N N O C O C N N H H H H CO(NH2)2 NOT “di-urea”
Urea – The first organic compound to be synthesized (Wohler, 1828).

61. Propane H H H H H H C C C H C C C H H H H H H H H H
C3H8

62. Butane H H H H H C C C C H H H H H H H H H H - C - C - C - C - H

63. Nitrogen triiodide N I I I .. N I NI3 Trigonal Pyramidal geometry
Video clip:
(slow motion)
detonation of NI3

64. Supplies 15 black (carbon) 8 green (chlorine and iodine)
1 yellow (sulfur)
4 blue (oxygen)
4 red (nitrogen)
42 hydrogen (hydrogen)
67 bonds (bonds)

65. C Cl I S N O H Cl H Cl C Cl H C H O C O Cl H S H H C C H H H Cl C Cl
CHCl3
HCl

66. H H H H H H H H C C C C H H C C C H H H H H H H H N N I I H H H I

67. Decomposition of Nitrogen Triiodide

69. Decomposition of Nitrogen Triiodide
Molecules store energy (chemical potential energy) in the bonds that hold them together. When the bonds are broken, energy is released.
2 NI3(s) N2(g) I2(g)

70. N H .. .. C H O .. H H .. O CH4, methane NH3, ammonia H2O, water O
lone pair
electrons O O
O3, ozone

71. The VSEPR Model .. .. .. The Shapes of Some Simple ABn Molecules O S O
Linear
Bent
Trigonal
planar
Trigonal
pyramidal
AB6 F P F S F Cl
Students often confuse electron-domain geometry with molecular geometry.
You must stress that the molecular geometry is a consequence of the electron domain geometry.
The best arrangement of a given number of electron domains is the one that minimizes the repulsions among them. F Xe
T-shaped
Square
planar
Trigonal
bipyramidal
Octahedral
Brown, LeMay, Bursten, Chemistry The Central Science, 2000, page 305