1. Chemical Names and Formulas
Chapter 9
What's in a name? that which we call a rose By any other name would smell as sweet

2. Introduction
Naming of ionic and molecular compounds require memorization and knowledge of some basic rules.
Deriving formulas from chemical names also require memorization and knowledge of some basic rules.
Acids and bases are unique compounds that are named using simple rules.
Two laws express how elements come together to form compounds.

3. Naming Ions Section 9.1
Monatomic Ions
Polyatomic Ions

4. Review: What is an ionic bond?
Ionic bonds: The electrostatic forces that hold ions together in ionic compounds.
One atom gives up electrons and the other picks up electrons.
Na+ Cl-
Na Cl → Na Cl-
(1s22s22p63s1) (1s22s22p63s23p5 ) (1s22s22p6) (1s22s22p63s23p6 )

5. I.) Monatomic Ions
These are ions that consists of a single atom with a positive or a negative charge.
Naming these ions is fairly straight forward.
Exception: The transition metals.

6. Cations of Representative Metals
Use the name of the metal followed
by the word “ion” or “cation.”
Group 1A,2A, and aluminum from 3A loses the same number of electrons as given by their group number.

7. Monatomic Anions Start with the stem of the element name
and add –ide to the end.
Only nonmetals form anions.
The charge of any anion of the representative elements is determined by subtracting 8 from the group number.

8. Transition Metals
Many of these transition metals form more than one cation with different ionic charges.
Two naming systems used to name these transition metals:
Stock system
An older system

9. The Stock System A Roman numeral is place in
parentheses and placed after the name
of the element to indicate the numerical
value of the charge on the ion.
This is the preferred method for naming cations of transition metals.
No space is left between the element name and the Roman numeral.
All this is followed by the word “ion.”

10. The Older System
It makes use of the “classical” names of the elements.
Uses two suffixes:
ous: Used with the cation with the lower charge. (Ferrous = Fe2+)
ic: Used with the cations with the higher charge (Ferric = Fe3+)

11. II.) Polyatomic Ions
These are ions that are composed of more than one atom.
The atoms of these ions are covalently bonded together.
These ions are treated as one unit.
Most are anions and we need to know only one cation. (NH4+ = ammonium)

12. Naming Polyatomic Anions
The names of most polyatomic anions
end with the suffix –ite or –ate.
Most of these ions you will need to memorize. (See Table 9.3 p. 257)
-ite: One less oxygen (SO32- = Sulfite)
-ate: One more oxygen (SO42- = Sulfate)

13. Naming & Writing Formulas for Ionic Compounds Section 9.2
Binary Ionic Compounds
Compounds with Polyatomic Ions
Sodium chloride
NaCl
Sodium
Bicarbonate
NaHCO3

14. I. ) Binary Ionic Compounds
Binary compound:
A compound composed of only
two elements and can be either
ionic or molecular.
Sodium chloride
NaCl

15. Naming Binary Ionic Compounds
First verify that the compound is binary.
Place the name of the cation ion first followed by the anion.
For transition metals include the Roman numerals.
Let’s work through some samples.

16. Name the following compound: CaS.
Is the compound binary?
Name of cation:
Is cation derived from a transition metal?
Name of anion:
Name of compound:

17. Name the following compound: SnF2.
Is the compound binary?
Name of cation:
Is cation derived from a transition metal?
Name of anion:
Name of compound:

18. Name the following compound: SnO2.
Is the compound binary?
Name of cation:
Is cation derived from a transition metal?
Name of anion:
Name of compound:

19. Writing Formulas for Binary Ionic Compounds
If you know the name of a binary ionic compound you can write its formula.
First, write the symbols for the cations and anions.
Second, use subscripts to balance out the charges.
Use the “crisscross” method.
No charges should be seen in the final answer.

20. Give the formula for the following compound: potassium chloride.
Is this a binary compound?
What is the cation?
Symbol for cation:
What is the anion?
Symbol for anion:
Does one cation and one anion balance each other out?
If not, how many of each are needed to balance the charges?

21. Give the formula for the following compound: iron(III) oxide.
Is this a binary compound?
What is the cation?
Symbol for cation:
What is the anion?
Symbol for anion:
Does one cation and one anion balance each other out?
If not, how many of each are needed to balance the charges?

22. Give the formula for the following compound: calcium sulfide.
Is this a binary compound?
What is the cation?
Symbol for cation:
What is the anion?
Symbol for anion:
Does one cation and one anion balance each other out?
If not, how many of each are needed to balance the charges?

23. II.) Compounds with Polyatomic Ions
These ionic compounds have at least one polyatomic ion.
Naming these compounds is similar to naming binary compounds, if we treat the polyatomic ion as one unit.
Sodium
Bicarbonate
NaHCO3

24. Naming Compound with Polyatomic Ions
Write the name for the cation ion
followed by the name of the anion,
remembering that the anions will
end in –ate or –ite.
The key to naming these compounds is to have the polyatomic ions memorized.

25. Name the following compound: LiCN.
Is the compound binary?
Name of cation:
Is cation derived from a transition metal?
Name of anion:
Name of compound:

26. Name the followingcompo und: NaClO.
Is the compound binary?
Name of cation:
Is cation derived from a transition metal?
Name of anion:
Name of compound:

27. Name the following compound: NH4C2O4.
Is the compound binary?
Name of cation:
Is cation derived from a transition metal?
Name of anion:
Name of compound:

28. Writing Formulas for Polyatomic Ionic Compounds
The process for writing the formulas for polyatomic ionic compounds is the same as for binary ionic compounds.
First, write the symbols for the cation and anion.
Second, balance the charges treating the polyatomic ions as one unit.
Or simply use the crisscross method.

29. Give the formula for the following compound: potassium sulfate.
Is this a binary compound?
What is the cation?
Symbol for cation:
What is the anion?
Symbol for anion:
Does one cation and one anion balance each other out?
If not, how many of each are needed to balance the charges?

30. Give the formula for the following compound: sodium nitrate.
Is this a binary compound?
What is the cation?
Symbol for cation:
What is the anion?
Symbol for anion:
Does one cation and one anion balance each other out?
If not, how many of each are needed to balance the charges?

31. Give the formula for the following compound: calcium nitrate.
Is this a binary compound?
What is the cation?
Symbol for cation:
What is the anion?
Symbol for anion:
Does one cation and one anion balance each other out?
If not, how many of each are needed to balance the charges?

32. Naming & Writing Formulas for molecular Compounds Section 9.3
Naming Binary Compounds
Writing Formulas for Binary Molecular Compounds
Carbon
dioxide
CO2
Carbon
monoxide CO

33. Review: What is an covalent bond?
Covalent bonds: The sharing of electrons between two atoms.
One atom gives up electrons and the other picks up electrons.

34. I.) Naming Binary Molecular Compounds
Use prefixes to distinguish between the different binary molecular compounds.
Prefixes tell us how many of each atom is present in a molecule of a binary compound.
Look at prefixes in Table 9.4 (p.269)
All binary molecular compounds end with –ide.

35. Rules for Naming Binary Molecular Compounds
ID that the compound is molecular
Name the elements in the order listed in the formula
Use prefixes to indicate the number of each atom in the molecule.
Omit mono- if the 1st element has only 1 atom
Drop the “o” from mono- if the 1st atom begins with a vowel.
The name of the second element ends with –ide.

36. Name the following binary compound: CO2.
Is the compound molecular?
Name of 1st atom:
How many?
Prefix for 1st atom:
Name of 2nd atom:
Prefix for 2nd atom:
Name of compound:

37. Name the following binary compound: N2O.
Is the compound molecular?
Name of 1st atom:
How many?
Prefix for 1st atom:
Name of 2nd atom:
Prefix for 2nd atom:
Name of compound:

38. Name the following binary compound: Cl2O8.
Is the compound molecular?
Name of 1st atom:
How many?
Prefix for 1st atom:
Name of 2nd atom:
Prefix for 2nd atom:
Name of compound:

39. II.) Writing Formulas of Binary Molecular Compounds
Simply use the prefixes in the name to tell you the number of each atom of each element.
Write the correct symbol for each element and include the number of atoms using a subscript.

40. Give the formula for the following compound: silicon dioxide.
Is this a molecular compound?
What is the 1st atom?
What is its prefix:
How many of the 1st atoms?
What is the 2nd atom?
What is its prefix?
What is the formula?

41. Give the formula for the following compound: Arsenic pentachloride.
Is this a molecular compound?
What is the 1st atom?
What is its prefix:
How many of the 1st atoms?
What is the 2nd atom?
What is its prefix?
What is the formula?

42. Give the formula for the following compound: Iodine tribromide.
Is this a molecular compound?
What is the 1st atom?
What is its prefix:
How many of the 1st atoms?
What is the 2nd atom?
What is its prefix?
What is the formula?

43. Naming & Writing Formulas for Acids & bases Section 9.4
Naming Acids
Writing Formulas for Acids
Names and Formulas for Bases
Sulfuric acid
H2SO4
Sodium hydroxide
NaOH

44. Acids A compound that contains one or more
hydrogen atom and produces hydrogen
ions (H+) when dissolved in water.
This is a group of ionic compounds with special properties.
Acids have many natural and synthetic uses.
More on acids in chapter 19.

46. I.) Naming Acids
Treat acids as if they were anions combined with enough hydrogen ions to make a neutral compound.
Acids will have the basic formula HnX, where “n” is the number of hydrogens and “X” is a monatomic or polyatomic ion.
Three rules for dealing with the naming of acids.

47. Rule #1: Compounds That End in -ide
Acid name begins with prefix hydro-
Drop –ide and add –ic
Add the word “acid” at the end
These compounds are often binary molecular compounds that do not have oxygen as a component.

48. Give the name of the following acid: HCl.
Is this a binary compound?
What is the prefix?
What is the anion?
Name of anion:
How does the suffix of the anion change?
What is the complete name of the acid?

49. Give the name of the following acid: H2S.
Is this a binary compound?
What is the prefix?
What is the anion?
Name of anion:
How does the suffix of the anion change?
What is the complete name of the acid?

50. Rule #2: Compounds That End in –ite
Drop –ite and add –ous.
Add the word “acid” at the end.
The anions of these compounds have oxygen as a component.
All of these are polyatomic acids.
Do not use the prefix “hydro-”.

51. Give the name of the following acid: H2SO3.
Is this a binary compound?
What is the prefix?
What is the anion?
Name of anion:
How does the suffix of the anion change?
What is the complete name of the acid?

52. Give the name of the following acid: H3PO3.
Is this a binary compound?
What is the prefix?
What is the anion?
Name of anion:
How does the suffix of the anion change?
What is the complete name of the acid?

53. Rule #3: Compounds That End in –ate
Drop –ate and add –ic.
Add the word “acid” at the end.
Again these acids are derived from compounds that have polyatomic anions with oxygen as a component.
Do not use the prefix “hydro-”.

54. Give the name of the following acid: H3PO4.
Is this a binary compound?
What is the prefix?
What is the anion?
Name of anion:
How does the suffix of the anion change?
What is the complete name of the acid?

55. Give the name of the following acid: H2SO4.
Is this a binary compound?
What is the prefix?
What is the anion?
Name of anion:
How does the suffix of the anion change?
What is the complete name of the acid?

56. II.) Writing Formulas from Acid Names
Simply use the reverse process to obtain the formulas from the names of the acids.
Make sure that you include enough hydrogen ions (H+) to balance the charges of the anions.

57. Give the formula for the following compound: hydrochloric acid.
Is this a binary compound?
How do you know?
Symbol for cation:
What is the anion?
Symbol for anion:
Does one cation and one anion balance each other out?
If not, how many of each are needed to balance the charges?

58. Give the formula for the following compound: nitric acid.
Is this a binary compound?
How do you know?
Symbol for cation:
What is the anion?
Symbol for anion:
Does one cation and one anion balance each other out?
If not, how many of each are needed to balance the charges?

59. Bases An ionic compound that produces
hydroxide ions (OH-) when dissolved
in water.
Like acids, these are a special group of ionic compounds with many natural and synthetic uses.
More on these compounds in chapter 19.

60. III.) Names and Formulas for Bases
Bases are named in the same way as other ionic compounds – the name of the cation followed by the name of the anion.
The key to identifying bases is to look for the OH- ion.

61. Give the formula for the following compound: potassium hydroxide.
Is this a binary compound?
What is the cation?
Symbol for cation:
What is the anion?
Symbol for anion:
Does one cation and one anion balance each other out?
If not, how many of each are needed to balance the charges?

62. Give the formula for the following compound: Iron(III) hydroxide.
Is this a binary compound?
What is the cation?
Symbol for cation:
What is the anion?
Symbol for anion:
Does one cation and one anion balance each other out?
If not, how many of each are needed to balance the charges?

63. Name the following binary compound: NaOH.
Is the compound binary?
Name of cation:
Is cation derived from a transition metal?
Name of anion:
Name of compound:

64. Name the following binary compound: Fe(OH)3.
Is the compound binary?
Name of cation:
Is cation derived from a transition metal?
Name of anion:
Name of compound:

65. The laws governing formulas and names Section 9.5
The Laws of Definite and Multiple Proportions
Practicing Skills: Naming Chemical Compounds
Practicing Skills: Writing Chemical Formulas

66. I.) The Laws of Definite and Multiple Proportions
Elements combine to form compounds in very predictable ways.
Thus we can describe the way they form compounds with two laws:
The Law Definite Proportions
The Law of Multiple Proportions

67. Law of Definite Proportions
In samples of any compound, the masses
of the elements are always in the same
proportions.
The ratios of atoms in a compound correlates to the ratio of masses of each element in that compound.
This law is very important in stoichiometry and chemical equations (chapter 12).

68. Example of The Law of Definite Proportions
Let’s examine this law using MgS.
The ratio of atoms is 1:1
The mass ratio will also be 1:1
Let’s see this for a 100g. sample of MgS.

69. Law of Multiple Proportions
Whenever the same two elements form
more than one compound, the different
masses of one element that combine with
the same mass of the other are in the
ratio of small whole numbers.
This law relates the mass of one element in a compound to the mass of another element in the same compound.
This law is also important for stoichiometry.

70. Example of The Law of Multiple Proportions
Let’s examine this law using H2O and H2O2.
Let’s see what the ration of oxygen is for the two compounds.

71. Sample Problem
Carbon reacts with oxygen to form two compounds. Compound A contains
2.41 g. of carbon for each 3.22 g. of oxygen. Compound B contains 6.71 g. of carbon for each 17.9 g. of oxygen. What is the lowest whole number mass ratio of carbon that combines with a given mass of oxygen?

72. Practicing Skills: Naming Chemical Compounds
Use this chart to help you write
chemical names.

73. Practicing Skills: Writing Chemical Formulas
Use this chart to help you write
chemical formulas.

74. Chemical Names and Formulas
Chapter 9
The End
What's in a name? that which we call a rose By any other name would smell as sweet

75. Naming acids Acids are ionic compounds where hydrogen is the cation.
These are the oxygen
containing acids, or oxo acids.
These are the binary acids

76. Naming bases We name bases as we name all other ionic compounds.
Name the following acids or bases: HF
HNO2
H3PO4
NaOH
Give the formula for the following acids or bases:
Lithium hydroxide
Carbonic acid
Hydrobromic acid
Barium hydroxide
Bases are ionic
compounds in which the
anions are mostly hydroxide.