-Periodic-Naming-and-Formula-Writing.ppt

Notes

1. 1
Nomenclature of
Inorganic Compounds

2. 2
Chapter Outline
6.1 Common and Systematic
Names
6.2 Elements and Ions
6.3 Writing Formulas from
Names of Compounds
6.4 Binary Compounds
6.5 Naming Compounds
Containing Polyatomic Ions
6.6 Acids

3. 3
Common and Common and
Systematic NamesSystematic Names

4. 4
Chemical nomenclature is the system of
names that chemists use to identify
compounds. Two classes of names exist:
common names and systematic names.

5. 5
–They are not based on the composition
of the compound.
–They are based on an outstanding
chemical or physical property.
•Chemists prefer systematic names.
–Systematic names precisely identify the
chemical composition of the compound.
–The present system of inorganic
chemical nomenclature was devised by
the International Union of Pure and
Applied Chemistry (IUPAC).
•Common names are arbitrary names.

6. 6

7. 7
Elements and IonsElements and Ions

8. 8
The formula for most elements
is the symbol of the element.
Sodium Na
PotassiumK
ZincZn
Argon Ar
Mercury Hg
Lead Pb
Calcium Ca

9. 9
Hydrogen H
2
NitrogenN
2
Oxygen O
2
Fluorine F
2
ChlorineCl
2
Bromine Br
2
Iodine I
2
These 7 elements are found
in nature as diatomic molecules.

10. 10
SulfurS
8
Phosphorous P
4
Two elements are commonly polyatomic.

11. 11
IonsIons

12. 12
→
remove e
-
neutral atom
A charged particle known as an ion can
be produced by adding or removing one
or more electrons from a neutral atom.
If one or more electrons are removed
from a neutral atom a positive ion is
formed. A positive ion is called a cation.

13. 13
Na  Na
+
+

e
-

Ca  Ca
2+
+

2e
-
Al  Al
3+
+

3e
-
Positive Ion Formation:
Loss of Electrons From a Neutral Atom

14. 14
Naming CationsNaming Cations

15. 15
Cations are named the same
as their parent atoms

16. 16

Atom

Cation
Name of
Cation
sodium (Na)
Na
+
sodium ion

17. 17

Atom

Cation
Name of
Cation
calcium (Ca)
Ca
2+
calcium ion

18. 18

Atom

Cation
Name of
Cation
lithium (Li)
Li
+
lithium ion

19. 19

Atom

Cation
Name of
Cation
magnesium (Mg)
Mg
2+
magnesium ion

20. 20

Atom

Cation
Name of
Cation
strontium (Sr)
Sr
2+
strontium ion

21. 21
→
neutral atom
A charged particle known as an ion can
be produced by adding or removing one
or more electrons from a neutral atom.
If one or more electrons are added
to a neutral atom a negative ion is
formed. A negative ion is called an
anion.
add e
-

22. 22
Naming AnionsNaming Anions

23. 23
An anion consisting of one element has
the stem of the parent element and an –
ide ending

24. 24

Atom

Anion
Name of
Anion
fluorine (F)
F
-
fluoride ion
stem

25. 25

Atom

Anion
Name of
Anion
chlorine (Cl)
Cl
-
chloride ion
stem

26. 26

Atom

Anion
Name of
Anion
bromine (Br)
Br
-
bromide ion
stem

27. 27

Atom

Anion
Name of
Anion
nitrogen (N)
N
3-
nitride ion
stem

28. 28

Atom

Anion
Name of
Anion
phosphorous (P)
P
3-
phosphide ion
stem

29. 29

Atom

Anion
Name of
Anion
oxygen (O)
O
2-
oxide ion
stem

30. 30
Ions are always formed by adding or
removing electrons from an atom.

31. 31
Most often ions are formed when metals
combine with nonmetals.

32. 32
The charge on an ion can be predicted
from its position in the periodic table.

33. 33
elements of
Group IIA have a
+2 charge
elements of Group
IA have a +1 charge
elements of
Group VA have a
-3 charge
elements of
Group VIA have a
-2 charge
elements of
Group VIIA have a
-1 charge

34. 34
Writing Formulas From Writing Formulas From
Names of CompoundsNames of Compounds

35. 35
A chemical formula is a shorthand way
of writing the name of a compound.
It is composed of the symbols of the
elements and the number of atoms each
element is present in the compound.
The number of atoms of an element is
written as a subscript.

36. Guidelines in writing the formulas of
inorganic compounds:
1. Represent by symbols the fragments of the
compound in the sequence that they occur in the
given name. In most cases, the positive fragment
(cation) comes first before the negative fragment
(anion). Enclose the radicals in parenthesis. A
radical is a group of elements that behaves as a unit
with a charge that can either be a positive or
negative. Refer to the list of common ions and their
charges.
36

37. Example:
Sodium chlorideNa
+
Cl
-
Aluminum oxideAl
+3
O
-2
Plumbic carbonatePb
+4
(CO
3)
-2
Calcium sulfate Ca
+2
(SO
4)
-2
37

38. Guidelines in writing the formulas of
inorganic compounds:
2. Cross indicate (crisscross) the charge as
subscript (exclude the signs). In cases where
the sum of the positive and negative charges
is equal to zero, cross indication is not
necessary.
38

39. Example:
Sodium chlorideNa
+
Cl
-
NaCl
Aluminum oxideAl
+3
O
-2
Al
2O
3
Plumbic carbonatePb
+4
(CO
3)
-2
Pb
2(CO
3)
4
Calcium sulfate Ca
+2
(SO
4)
-2
CaSO
4
39

40. Guidelines in writing the formulas of
inorganic compounds:
3. Observe the following:
•In the final form, omit writing “1” if it is the
subscript.
•Reduce the subscript derived from cross
indication into the smallest whole number.
However, do not change the subscripts which
appear in the radical(s).
•Eliminate the parenthesis of the radicals when
the subscript is “1”.
40

41. Example:
Mg
+2
Cl
-
---Mg
1Cl
2---MgCl
2
Pb
+4
(CO
3)
-2
---Pb
2(CO
3)
4 ---Pb(CO
3
)
2
Na
+1
(S
2O
3)
-2
---Na
2(S
2O
3)
1 ---Na
2
S
2
O
3
41

42. Guidelines in writing the formulas of
inorganic compounds:
4. In some cases, two nonmetallic elements
combine to form more than one kind of
compounds. Examples of nonmetallic elements
are carbon, sulfur, oxygen, nitrogen, chlorine,
etc. These compounds are named with different
prefixes to designate the number of atoms of
one element that combine. If the prefix ends in
a or o and the word that follows starts with a or
o, drop the last vowel of the prefix.
42

43. 43
PrefixesPrefixes

44. 44
A Greek prefix is placed before the name
of each element to indicate the number
of atoms of the element that are present.

45. 45
• di = 2
• tri = 3
• tetra = 4
• penta = 5
•hexa = 6
•hepta = 7
• octa = 8
• nona = 9
•deca = 10
• mono = 1
Mono is rarely used when
naming the first element.

46. 46
ExamplesExamples

47. 47
N
2
O
3
dinitrogen trioxide
indicates two
nitrogen atoms
indicates three
oxygen atoms

48. 48
PCl
5
phosphorous pentachloride
indicates one
phosphorous atom
indicates five
chlorine atoms

49. 49
Cl
2
O
7
dichlorine heptoxide
indicates two
chlorine atoms
indicates seven
oxygen atoms

50. 50
CO carbon monoxide
Carbon dioxide CO
2

51. 51
Nomenclature of Nomenclature of
Inorganic CompoundsInorganic Compounds

52. Inorganic compounds are classified into
oxides, bases, acids, and salts. Each class is
distinguished from the others by their
chemical formulas (composition), properties,
and names.
52

53. Oxides
The oxides are binary compounds (two
elements) consisting of oxygen which is the
anion and another element which may be a
metal or a nonmetal. Thus, oxides are either
metallic or nonmetallic. The name of a
metallic oxide consists of the name of the
cation followed by the term “oxide”
53

54. Examples
Aluminum oxideAl
2O
3
Ferric oxide Fe
2O
3
54

55. Oxides
In naming nonmetallic oxides, refer to #4.
guidelines in writing the formula of inorganic
compound.
55

56. Bases
The inorganic bases are compounds of a
metallic element with one or more hydroxyl
(OH
-
) groups. The name of a base consists of
the name of the cation followed by the term
“hydroxide”
56

57. Examples
Ferrous hydroxide Fe(OH)
2
Aluminum hydroxide Al(OH)
3
57

58. Acids
The inorganic acids are those compounds
consisting of hydrogen and a negative ion
(except O
-2
) or a negative radical whose water
solution changes the color of litmus paper
from blue to red. There are two kinds of
inorganic acids: binary acid and ternary acid.
58

59. Binary Acids
A binary acid is one in which the H is
combined with a nonmetal such as Cl, Br, S,
etc. Its name consists of prefix “hydro”
connected to the root word of the nonmetal
with the suffix “ic” and the word “acid”.
Sulfur is an exception to the rule where its full
name is used.
•General formula: hydro root word ic acid
59

60. Examples
HCl hydrochloric acid
H
2S hydrosulfuric acid
60

61. Ternary Acids
A ternary acid is composed of three elements:
hydrogen, a nonmetal, and oxygen. The
nonmetal and oxygen, as a group, is called a
radical and carries a negative charge.
61

62. Ternary Acids
Name of Radical Name of Acid
 
hypo______ite
______ite
______ate
per______ate
 
 
hypo__________ous acid
__________ous acid
__________ic acid
per_________ ic acid
62

63. Examples
Radical Acid Name Acid Formula
Hypochlorite ClO
-
Hypochlorous acid HClO
Chlorite ClO
2
-
Chlorous acid HClO
2
Chlorate ClO
3
-
Chloric acid HClO
3
Perchlorate ClO
4
-
Perchloric acid HClO
4
63

64. Salts
The salts are compounds consisting of a metal
combined with a nonmetal or a negative
radical except OH
-
­
. They are formed by the
reaction between a base an acid which is
called neutralization reaction. The cation
comes from the base while the anion comes
from the acid.
64

65. Salts
NaOH + HCl NaCl + HOH
base acid salt water
65

66. 66
A chemical compound must have a
net charge of zero.

67. 67
If the compound contains ions,
then the charges on all of
the ions must add to zero.

68. 68
The Stock SystemThe Stock System

69. 69
The metals in the center of the periodic
table (including the transition metals)
often form more than one type of
cation.

70. 70
Each ion of iron forms a different
compound with the same anion.
Fe
2+
Fe
3+
FeS
Fe
2
S
3

71. 71
IUPAC devised the Stock System of
nomenclature to name compounds of
metals that have more than one type of
cation.
Cation
Charge
+1 +2 +3 +4 +5
Roman
Numeral
I II III IV V
In the Stock System the charge on the cation
is designated by a Roman numeral placed in
parentheses immediately following the name
of the metal.
The nonmetal name ends in -ide.

72. 72
Stock System
Lower Charge Higher Charge
Element Formula Name Formula Name
Copper Cu
+
copper (I) Cu
2+
copper (II)
Iron Fe
2+
iron(II) Fe
3+
iron(III)
Lead Pb
2+
lead (II) Pb
4+
lead(IV)
Mercury Hg
2
2+
mercury(I) Hg
2+
mercury(II)
Tin Sn
2+
Tin(II) Sn
4+
Tin (II)
Stock System
Higher Charge
Element Formula Name Formula Name
Lower Charge

73. 73
ExamplesExamples

74. 74
ion chargeion name
FeCl
2
iron(II) chloride
+2-1
chlorideiron(II)
FeCl
3
iron(III) chloride
-1+3
iron(III)chloride
compound name

75. 75
ion chargeion name
SnBr
2
tin(II) bromide
+2-1
bromidetin(II)
SnBr
4
tin(IV) bromide
-1+4
tin(IV)bromide
compound name

76. 76
The Classical SystemThe Classical System

77. 77
In the Classical System the name of the metal
(usually the Latin name) is modified with the
suffixes -ous and ic.

78. 78
-ous lower charge
-ic higher charge
Metal name ends in
nonmetal name ends in
-ide

79. 79
Examples

80. 80
ion chargeion name
FeCl
2
ferrous chloride
+2-1
chlorideferrous
FeCl
3
ferric chloride
-1+3
ferricchloride
compound name

81. 81
ion chargeion name
SnBr
2
stannous bromide
+2-1
bromidestannous
SnBr
4
stannic bromide
-1+4
stannicbromide
compound name

82. 82
Lower Charge Higher Charge

Element Formula Name Formula Name
Copper Cu
+
cuprousCu
2+
Cupric
Iron Fe
2+
ferrousFe
3+
ferric
Lead Pb
2+
plumbousPb
4+
plumbic
MercuryHg mercurousHg
2+
mercuric
Tin Sn
2+
stannousSn
4+
stannic
Ion Names: Classical System

83. 83