1. Naming Compounds Writing Formulas
Chapters 8 & 9
Naming Compounds
Writing Formulas

2. Systematic Naming
There are too many compounds to remember the names of them all.
Compound is made of two or more elements.
Put together atoms.
Name should tell us how many and what type of atoms.

3. Periodic Table More than a list of elements.
Put in columns because of similar properties.
Each column is called a group.

4. Representative Elements
The group A elements

5. Metals

6. Metals Luster – shiny. Ductile – drawn into wires.
Malleable – hammered into sheets.
Conductors of heat and electricity.

7. Transition Metals
The Group B elements

8. Non-Metals
Dull
Brittle
Nonconductors- insulators

9. Metalloids or Semimetals
Properties of both
Semiconductors

10. Atoms and Ions Atoms are electrically neutral.
Same number of protons and electrons.
Ions are atoms, or groups of atoms, with a charge.
Different numbers of protons and electrons.
Only electrons can move.
Gain or lose electrons.

11. F-1 O-2 Anion A negative ion. Has gained electrons.
Non metals can gain electrons.
Charge is written as a super script on the right.
F-1
Has gained one electron
O-2
Has gained two electrons

12. K+1 Ca+2 Cations Positive ions. Formed by losing electrons.
More protons than electrons.
Metals form cations.
K+1
Has lost one electron
Ca+2
Has lost two electrons

13. Naming Compounds Writing Formulas
Chapters 8 & 9
Naming Compounds
Writing Formulas

14. Compounds Follow the Law of Definite Proportion.
Have a constant composition.
Have to add the same number of atoms every time.
Two types.

15. Two Types of Compounds 1 Ionic Compounds Made of cations and anions.
Metals and nonmetals.
The electrons lost by the cation are gained by the anion.
The cation and anions surround each other.
Smallest piece is a FORMULA UNIT.

16. Crystalline Structure – Ionic Compound

17. Two Types of Compounds 2 Molecular Compounds Made of molecules.
Made by joining nonmetal atoms together into molecules.
H2O, CO2, C6H12O6

18. Chemical Formulas
Shows the kind and number of atoms in the smallest piece of a substance.
Molecular formula- number and kinds of atoms in a molecule.
CO2
C6H12O6

19. Two Types of Compounds Ionic Molecular Smallest Piece Formula Unit
Molecule
Types of Elements
Metal and Nonmetal
Nonmetals
Solid, Liquid or Gas
State
Solid
Melting Point
High >300ºC
Low <300ºC

20. Chemical Formulas More than one atom? –use a subscript (H2O)
There are 7 diatomic elements
Hydrogen (H2), Nitrogen (N2), Oxygen (O2), Fluorine (F2), Chlorine (Cl2), Bromine (Br2), and Iodine (I2)
Remember: “Br I N Cl H O F”

21. Ionic Compounds
This formula represents not a molecule, but a formula unit
The smallest whole number ratio of atoms in an ionic compound.
Ions surround each other so you can’t say which is hooked to which. (p. 140)

22. Charges on Ions
For most of the Group A elements, the periodic table can tell what kind of ion they will form based on their location.
Elements in the same group have similar properties.
Including the charge when they become ions.

23. +1 +2 +3 -3 -2 -1

24. What about the others?
Groups 4A and 8A do not usually form ionic bonds (in fact, Group 8A rarely forms compounds!)
Many transition metals have more than one common ionic charge

25. Systematic Naming
There are too many compounds to remember the names of them all.
Compound is made of two or more elements.
Put together atoms.
Name should tell us how many and what type of atoms.

26. Naming Ions We will use the systematic way.
Cation- if the charge (oxidation #) is always the same, use name of the metal.
Transition metals can have more than one charge or oxidation number.
Therefore, indicate the charge with roman numerals in parenthesis.
Fe+3 is named - iron (III) ion Movie

27. Exceptions: Some of the transition metals have only one ionic charge:
Do not use roman numerals for these:
Silver is always 1+ (Ag1+)
Cadmium and Zinc are always 2+ (Cd2+ and Zn2+)

28. Metals with Multiple Charges
Transition Metals
Here it is easier to list the ones that only have a single common oxidation state.
All Group 3B - 3+
Ni, Zn, Cd - 2+ Ag
Lanthanides and actinides - 3+

29. Name These Ions Na+1 Ca+2 Al+3 Fe+3 Fe+2 Pb+2 Li+1 sodium ion
calcium ion
aluminum ion
iron (III) ion
iron (II) ion
lead (II) ion
lithium ion
Na+1
Ca+2
Al+3
Fe+3
Fe+2
Pb+2
Li+1

30. Write Formulas for These
Potassium ion
Magnesium ion
Copper (II) ion
Chromium (VI) ion
Barium ion
Mercury (II) ion
K+1
Mg+2
Cu+2
Cr+6
Ba+2
Hg+2

31. Naming Anions Anions are always the same.
Change the element ending to – ide
F-1 Fluorine

32. Naming Anions Anions are always the same.
Change the element ending to – ide
F-1 Fluorin

33. Naming Anions Anions are always the same
Change the element ending to – ide
F-1 Fluori

34. Naming Anions Anions are always the same
Change the element ending to – ide
F-1 Fluor

35. Naming Anions Anions are always the same
Change the element ending to – ide
F-1 Fluori

36. Naming Anions Anions are always the same
Change the element ending to – ide
F-1 Fluorid

37. Naming Anions Anions are always the same
Change the element ending to – ide
F-1 Fluoride

38. Name These Ions Cl-1 N-3 Br-1 O-2 Ga+3 Chloride Nitride Bromide Oxide
Gallium (III)
Cl-1
N-3
Br-1
O-2
Ga+3

39. Write These sulfide ion iodide ion phosphide ion strontium ion S-2 I-1
Sr+2

40. Polyatomic Ions Groups of atoms that stay together and have a charge.
Use your reference sheet
Acetate C2H3O2-1
Nitrate NO3-1
Nitrite NO2-1
Hydroxide OH-1
Permanganate MnO4-1
Cyanide CN-1

41. Polyatomic Groups with a Charge

42. Polyatomic Ions Ammonium NH4+1 Sulfate SO4-2 Sulfite SO3-2
Carbonate CO3-2
Chromate CrO4-2
Dichromate Cr2O7-2
Phosphate PO4-3
Phosphite PO3-3

43. Common Polyatomic Ions

44. We’ve named the ions, so now it is time to name the compounds!
Ionic Compounds
We’ve named the ions, so now it is time to name the compounds!

45. Naming Binary Ionic Compounds
Binary Compounds - 2 elements.
Ionic - a cation and an anion.
To write the names just name the two ions.
Easy with Representative elements.
NaCl = Na+ Cl- = sodium chloride
MgBr2 = Mg+2 Br- = magnesium bromide

46. Naming Binary Ionic Compounds
The problem comes with the transition metals.
Need to figure out their charges.
The compound must be neutral.
Same number of + and – charges.
Use the anion to determine the charge on the positive ion.

47. Balancing Charge Na+ & O-2 Na+x O-2y x(+1) + y(-2) = 0
find the smallest common factor
Na2O
Ca+2 & N-3 x(+2) + y(-3) = 0
Ca3N2

48. Balancing Charges
How many zinc +2 charges are needed to balance phosphide’s -3 charge?
What subscripts must be placed on the line?
The numbers used must always be whole numbers.

50. Naming Ionic Compounds
Many metals form more than one compound with some anions.
For these, roman numerals are used in the name to indicate the charge on the metal.
Cu O2- = Cu2O
copper(I) oxide copper(I) oxide
Cu O = CuO
copper(II) oxide copper(II) oxide

51. More Examples FeCl2 iron(II) chloride FeCl3 iron(III) chloride
SnS tin(II) sulfide
SnS2 tin(IV) sulfide
AgCl silver chloride
CdS cadmium sulfide
Note
Some transition metals only have a single state
so the roman numeral may be omitted.
Some main group metals, with high atomic number
have more than one state, roman numbers are used.

52. Naming Binary Ionic Compounds
Write the name of CuO
Need the charge of Cu
O is -2
Copper must be +2
Copper (II) oxide
Name CoCl3
Cl is -1 and there are three of them = -3
Co must be +3 Cobalt (III) chloride

53. Naming Binary Ionic Compounds
Write the name of Cu2S.
Since S is -2, the Cu2 must be +2, so each one is +1.
copper (I) sulfide
Fe2O3
Each O is x -2 = -6
2 Fe must = +6, so each is +3.
iron (III) oxide

54. Naming Binary Ionic Compounds
Write the names of the following
KCl
Na3N
CrN
Sc3P2
PbO
PbO2
Na2Se
Potassium Chloride
Sodium Nitride
Chromium (III) Nitride
Scandium (II) Phosphide
Lead (II) Oxide
Lead (IV) Oxide
Sodium Selenide

55. Ternary Ionic Compounds
Will have polyatomic ions
At least three elements
Name the ions
NaNO3
CaSO4
CuSO3
(NH4)2O
Sodium Nitrate
Calcium Sulfate
Copper (II) Sulfite
Ammonium Oxide

56. Ternary Ionic Compounds
LiCN
Fe(OH)3
(NH4)2CO3
NiPO4
Lithium Cyanide
Iron (III) Hydroxide
Ammonium Carbonate
Nickel (III) Phosphate

57. Writing Formulas The charges have to add up to zero.
Get charges on pieces.
Cations from name of table.
Anions from table or polyatomic.
Balance the charges by adding subscripts.
Put polyatomics in parenthesis.

58. Writing Formulas Write the formula for calcium chloride.
Calcium is Ca+2
Chloride is Cl-1
Ca+2 Cl-1 would have a +1 charge.
Need another Cl-1
Ca+2 Cl2-1

59. Write the Formulas for These
Li2S
SnO
SnO2
MgF2
CuSO4
FeP
GaNO3
Fe2S3
lithium sulfide
tin (II) oxide
tin (IV) oxide
magnesium fluoride
copper (II) sulfate
iron (III) phosphide
gallium (I) nitrate
iron (III) sulfide

60. Write the Formulas for These
ammonium chloride
ammonium sulfide
barium nitrate
NH4Cl
(NH4)2S
Ba(NO3)2

61. Things To Look For
If cations have (roman #), the number is their charge.
If anions end in -ide they are probably off the periodic table (Monoatomic)
If anion ends in -ate or -ite it is polyatomic

62. Writing Names and Formulas
Molecular Compounds
Writing Names and Formulas

63. Molecular Compounds made of just nonmetals
smallest piece is a molecule
can’t be held together because of opposite charges
can’t use charges to figure out how many of each atom

64. Easier Ionic compounds use charges to determine how many of each.
Have to figure out charges.
Have to figure out numbers.
Molecular compounds name tells you the number of atoms.
Uses prefixes to tell you the number

65. Prefixes 1 mono- 2 di- 3 tri- 4 tetra- 5 penta- 6 hexa- 7 hepta-
8 octa-

66. Prefixes
9 nona-
10 deca-
To write the name write two words

67. Prefixes Prefix name Prefix name -ide 9 nona- 10 deca-
To write the name, write two words with
Prefix
name
Prefix
name
-ide

68. Prefixes Prefix name Prefix name -ide 9 nona- 10 deca-
To write the name write two words
One exception is we don’t write mono- if there is only one of the first element.
Prefix
name
Prefix
name
-ide

69. Prefixes Prefix name Prefix name -ide 9 nona- 10 deca-
To write the name write two words
One exception is we don’t write mono- if there is only one of the first element.
No double vowels when writing names (oa oo)
Prefix
name
Prefix
name
-ide

70. Name These N2O NO2 Cl2O7 CBr4 CO2 BaCl2 Dinitrogen Monoxide
Nitrogen Dioxide
Dichlorine Heptoxide
Carbon Tetrabromide
Carbon Dioxide
Barium Chloride

71. Write Formulas for These
diphosphorus pentoxide
tetraiodine nonoxide
sulfur hexafluoride
nitrogen trioxide
carbon tetrahydride
phosphorus trifluoride
aluminum chloride
P2O5
I4O9
SF6
NO3
CH4
PF3
AlCl3

72. Nomenclature Flowchart
Is a metal present
as the first element? No
Use prefixes
(mono, di, tri ...)
Yes
Can the metal have
more than one
oxidation state? No
Roman numerals
are not needed.
Yes
Use Roman numerals

73. Helpful to remember...
1. In an ionic compound, the net ionic charge is zero (criss-cross method)
2. An -ide ending generally indicates a binary compound
3. An -ite or -ate ending means there is a polyatomic ion that has oxygen
4. Prefixes generally mean molecular; they show the number of each atom

74. Helpful to remember...
5. A Roman numeral after the name of a cation shows the ionic charge of the cation.

75. Writing Names and Formulas
Acids
Writing Names and Formulas

76. Acids Compounds that give off hydrogen ions when dissolved in water.
Must have H in them.
Will always be an H next to an anion.
The anion determines the name.

77. Typical Acids and Bases
HCl HNO3 H2SO4 H3PO4
Base
NaOH KOH Ba(OH)2 Al(OH)3

78. Naming Acids
If the anion attached to hydrogen ends in -ide, use the prefix hydro- and change -ide to -ic acid
HCl - hydrogen ion and chloride ion
hydrochloric acid
H2S hydrogen ion and sulfide ion
hydrosulfuric acid

79. Naming Acids If the anion has oxygen in it, no hydro
It ends in -ate or -ite
Change the suffix -ate to -ic acid
HNO3 Hydrogen and nitrate ions
Nitric acid
Change the suffix -ite to -ous acid
HNO2 Hydrogen and nitrite ions
Nitrous acid

80. Oxyanion and Oxyacids An ion with oxygen in it is called an oxyanion.
An acid with an oxyanion in it is called an oxyacid.

81. Acids
If the second element ends in -ide, name the acid hydro - root - ic acid
HCN = hydrogen cyanide = hydrocyanic acid
If the second element ends in -ite, name the acid root - ous acid
H2SO3 = hydrogen sulfite = sulfurous acid

82. Name These HF H3P H2SO4 H2SO3 HCN H2CrO4 H3PO4 Hydrofluoric acid
Hydrophosphoric acid
Sulfuric acid
Sulfurous acid
Hydrocyanic acid
Chromic acid
Phosphoric acid

83. Writing Formulas Hydrogen will always be first
Name will tell you the anion
Make the charges cancel out
Starts with hydro- no oxygen, -ide
No hydro, -ic comes from -ate, -ous comes from -ite

84. Write Formulas for These
hydroiodic acid
acetic acid
carbonic acid
phosphoric acid
hydrobromic acid HI
HC2H3O2
H2CO3
H3PO4
HBr

85. More Acid Practice
Name and Formula

86. Name the Formula H2S H2CrO4 HClO3 H2CO3 HSCN H2SO3 H3PO4
Hydrosulfuric acid
Chromic acid
Chloric acid
Carbonic acid
Thiocyanic acid
Sulfurous acid
Phosphoric acid

87. Write the Formula Hydroiodic acid Hydrobromic acid Perchloric acid
Sulfuric acid
Hydrophosphoric acid
Hydroselenic acid
Chlorous acid HI
HBr
HClO4
H2SO4
H3P
H2Se
HClO2