Chapter 9 Notes
Honors Chemistry
Chapter 9: Chemical Names and Formulas
Section 1: Naming Ions
(read pages 252-259)
Monatomic Ions


Ions that consist of a _______________ atom with a _______________ or _______________
charge resulting from the ________ or ________ of ______ or more _______________ electrons
Two Types
 Positive Ions
o _______________
 Negative Ions
o _______________
Cations



_______________ charged ions
Metal atom _______________ _______________
Name _______________ the _______________
Naming Cations Practice
Element
Sodium
# of valence electrons
……………………
Ion formed
Name of cation
…………… ……………………………
Ca2+
Magnesium
Anions



_______________ charged ions
Nonmetal atom _______________ _______________
Name changes to _______________ ending
Naming Anions Practice
Element
Nitrogen
# of valence electrons Ion formed
………………
……
Name of anion
………………………..
S2Fluoride
1
Chapter 9 Notes
Honors Chemistry
Note

Groups _______________ and _______________ usually ________ _______ form ions
Ions of Transition Metals



Many of the _______________ metals form _______________ than _______________ cation
with _______________ ionic charges
Not _____________ transition metals have ______________ than ____________ charge
_______________ must be determined from the _______________ of _______________
_______________
Two Methods to Name Transition Metal Ions
1. _______________ _______________
2. _______________ _______________
Stock System


_______________ method of _______________
A _______________ _______________ in _______________ is placed _______________ the
name of the element to indicate the _______________ _______________ of the
_______________
Number
Roman Numeral
1
2
3
4
5
Stock System Naming Practice
Ion Formed # of Electrons Lost
Cu+
1
Stock Name
Copper (I) ion
Cu2+
Lead (II) ion
Pb4+
2
6
Chapter 9 Notes
Honors Chemistry
Classical Method

In the past, scientists used the _______________ names of elements.
Example:
Ferrum is Latin for Iron.
Ferr- is the root of this word.
2+
3+
Iron forms two ions: Fe and Fe
Ion names:
2+
Fe is the ferrous ion
3+
Fe is the ferric ion
Practice Problems
Name the ions formed by these elements and classify them as anions or cations.
a) Selenium ______________________________
b) Barium ______________________________
c) Phosphorous ______________________________
Polyatomic Ions





What does the prefix poly mean? _______________
Polyatomic ions are _______________ of _______________ than _______________ atom
_______________ bound _______________ of atoms that behave as a _______________ and
carry a _______________
The names of most polyatomic ions end in _______________ or _______________
Different Endings
o Ammonium  _______________
o _______________  CNo _______________  OH-
A Closer Look at a Polyatomic Ion
Name: _______________
_______________: shows the _______________ on the polyatomic ion
PO43_______________: shows the _______________ of atoms of that element
Book Work - Page 258 #3-9
3
Chapter 9 Notes
Honors Chemistry
Section 2: Naming and Writing Formulas for Ionic Compounds
(read pages 260-266)
Binary Ionic Compounds


What does the prefix bi mean? _______________
A binary _______________ compound is composed of _______________ elements - a
_______________ and a _______________
Naming Binary Ionic Compounds


If you know the formula of the ionic compound, you can write the name
To name any binary ionic compound, place the _______________ name _______________,
followed by the _______________ name.
Naming Binary Ionic Compounds - Examples
1. Naming a Simple Ionic Compound (1 _______________ + 1 _______________)
a. CaCl2 ____________________________
2. Naming an Ionic Compound containing a Transition Metal with only ONE possible charge (1
_______________ + 1 _______________)
a. ZnS ______________________________
3. Naming an Ionic Compound containing a Transition Metal with only ONE possible charge (1
_______________ + 1 _______________)
a. Cu2O ____________________________
b. CuO ____________________________
Try It!
Name the following binary ionic compounds:
1. NaF _________________________________________
2. FeCl3 _________________________________________
3. FeCl2 _________________________________________
Writing Binary Ionic Formulas



If you know the name of a binary ionic compound, you can write the formula!
Write the ____________ of the ____________ and then the ____________. Then, add the
____________ that are needed to ____________ the ____________.
The _______________ charge of the _______________ must balance the _______________
charge of the _______________ so that the net ionic charge of the compound is
_______________.
4
Chapter 9 Notes
Honors Chemistry
Remember the Crisscross Method?
1. __________________________________________________________________
2. __________________________________________________________________
3. __________________________________________________________________
4. __________________________________________________________________
Writing Binary Ionic Formulas - Examples
1. Simple Ionic Compounds:
a. Sodium Bromide _______________
2. Ionic Compounds with Transition Metals:
a. Iron (III) Oxide _______________
Writing Formulas for Binary Ionic Compounds
Write formulas for these binary ionic compounds.
a. Copper (II) sulfide _________________________________________
b. Potassium nitride _________________________________________
11. Write formulas for these compounds
a. Sodium iodide _________________________________________
c. Potassium sulfide _________________________________________
d. Calcium iodide _________________________________________
What is a polyatomic ion?

_________ bound groups of _________ that behave as a ___________ and carry a ___________
Polyatomic Ions behave as a UNIT.

You _______________ change the _______________ or the _______________ of
_______________ of each _______________ in a polyatomic ion or you will change the
_______________ of that ion!!
Naming Compounds with Polyatomic Ions



To name a compound containing a polyatomic ion, state the _______________
_______________, and then the _______________.
Just like naming binary _______________ compounds!
Except you _______________ _______________ change the anion name!
5
Chapter 9 Notes
Honors Chemistry
Naming Compounds with Polyatomic Ions Example
1.
2.
3.
4.
CaSO4 ______________________________
AlPO4 ______________________________
NaC2H3O2 ______________________________
CuSiO3 ______________________________
Writing the Formula of a Compound containing a Polyatomic Ion



Remember: Polyatomic ions _______________ as a _______________.
You _______________ change the assigned _______________.
Write the ____________ for the ____________, followed by the ____________ for the
____________ ion, then ____________ the charges. Use _____________.
Writing Formulas with Polyatomic Ions Example
1.
2.
3.
4.
5.
6.
Aluminum chromate _______________
Ammonium sulfide _______________
Ammonium sulfate _______________
Tin (II) cyanide _______________
Magnesium hydroxide _______________
Potassium sulfate _______________
Try It!
Write the formulas of the following binary ionic compounds:
1.
2.
3.
4.
Tin (IV) sulfide ______________________________
Magnesium nitrate ______________________________
Calcium bromide ______________________________
Sodium hydroxide ______________________________
Book Work - Page 266 #14-19
Section 3: Naming and Writing Formulas for Molecular Compounds
(read pages 268-270)
Binary Molecular Compounds


A binary _______________ compound is composed of _______________ elements –
_______________ are _______________
Binary molecular compounds do not contain _______________ – they are made of…
_______________
6
Chapter 9 Notes
Honors Chemistry
Naming Binary Molecular Compounds


Use _______________
The _______________ in the name of a binary molecular compound tells how many
_______________ of each _______________ are present in each _______________ of the
_______________
Number
Prefix
1
2
3
4
5
6
7
8
9
10
Steps for Naming a Binary Molecular Compound
1. _______________ that the compound is a binary _______________ compound.
2. _______________ the elements in the _______________ that they appear in the
_______________
a. Use _______________ to indicate the _______________ of each kind of atom.
b. The name of the _______________ element _______________ the _______________.
The _______________ of the _______________ element changes to _______________
Special Rules

If there is only _______________ atom of the _______________ element in the formula, drop
the _______________
Example: CCl4 is called ___________________, NOT monocarbon tetrachloride.

If the element _______________ with a _______________, drop the _______________ on the
end of the _______________.
Example: CO is called _________________________, NOT carbon monooxide.
Naming Binary Molecular Compounds - Examples
1. N2O ______________________________
2. Cl2O8 ______________________________
Try It!
1.
2.
3.
4.
CBr4 ______________________________
N2H4 ______________________________
PCl5 ______________________________
S2F10 ______________________________
7
Chapter 9 Notes
Honors Chemistry
Writing Formulas for Binary Molecular Compounds

Use the _______________ in the name to tell you the _______________ of each
_______________ in the _______________. Then, write the correct _______________ for the
two elements with the appropriate _______________.
Writing Formulas for Binary Molecular Compounds – Examples
1. Dinitrogen trioxide _______________
2. Iodine heptafluoride _______________
Try It!
a.
b.
c.
d.
Carbon disulfide ______________________________
Tribromine octoxide ______________________________
Silicon monocarbide ______________________________
Dihydrogen monoxide ______________________________
Book Work - Page 270 #20-25
Section 4: Naming and Writing Formulas for Acids and Bases
(read pages 271-273)
Naming Acids



Acid – a _______________ that contains _______________ or more _______________ atoms
and produces _______________ ions (_____________) when _______________ in
_______________
_______________ is most commonly listed _______________ in the compound
Formula: _______________
o NOTE: Acids _______________ _______________ have to have _______________
first, but _______________ do.
Rules for Naming Acids


_______________ rules
Dependent of the _______________ (the non _______________ part)
8
Chapter 9 Notes
Honors Chemistry
Rule #1



When the name of the _______________ ends in _______________, the _______________
name begins with _______________. The _______________ of the _______________ has the
suffix _______________ and is followed by _______________.
Simply – if there is no _______________ in the acid formula, the formula for the name is
______________________________ _______________
Example
o HCl
 Cation – _______________
 Anion – _______________
 Name of Acid – _______________ _______________
Rule #2



When the _______________ name ends in _______________, the _______________ name is
the stem of the anion with the suffix _______________ followed by the word
_______________.
Formula for name: ___________________ _______________
Example
o HClO2
 Cation – _______________
 Anion – _______________
 Name of Acid – _______________ _______________
Rule #3



When the anion name _______________ in _______________, the _______________ name is
the _______________ of the anion with the suffix _______________ followed by the word
_______________.
Formula for name: _______________ _______________
Example
o HClO3
 Cation – _______________
 Anion – _______________
 Name of Acid – _______________ _______________
Practice Problems
1.
2.
3.
4.
H2SO3 ______________________________
HNO3 ______________________________
HBr ______________________________
H3PO3 ______________________________
9
Chapter 9 Notes
Honors Chemistry
Writing Formulas for Acids


Use the _______________ in _______________
Example:
o Write the formula for hydrocyanic acid.
o Hydro-root-ic acid means the anion ends in –ide.
 The cation is _______________ (__________).
 The anion is _______________ (__________).
 The formula for the acid is _______________.
Practice Problems
Write the formulas for the following acids:
1.
2.
3.
4.
Hydroiodic acid ______________________________
Carbonic acid ______________________________
Carbonous acid ______________________________
Acetic acid ______________________________
Names and Formulas of Bases



Base – a _______________that produces _______________ions (____________) when
_______________in _______________
Named the _______________way as an _______________compound: Name of
_______________, then name of _______________.
o __________ is usually _______________ (_____) but it does not have to be.
Example:
o NaOH
 Cation: _______________
 Anion: _______________
 Name of Base: _______________ _______________
Try It!
Provide the appropriate name or formula of the following bases:
1.
2.
3.
4.
Potassium hydroxide ______________________________
Be(OH)2 ______________________________
RbOH ______________________________
Aluminum hydroxide ______________________________
Book Work – Page 273 #26-33
10
Chapter 9 Notes
Honors Chemistry
Section 5: The Laws Governing Formulas and Names
(read pages 274-279)
The Law Governing Formulas and Names


The _______________ for naming and writing _______________ are _______________
because elements form compounds in _______________ ways.
Two Important _______________
o The Law of _______________ Proportions
o The Law of _______________ Proportions
The Law of Definite Proportions


1.
2.
3.
4.
States that in samples of any chemical _______________, the _______________ of the elements
are always in the _______________ _______________.
So what does that mean?
What is the formula for water? _______________
What is the atomic mass of Oxygen? _______________
What is the atomic mass of Hydrogren? _______________
What is the mass ratio of Oxygen to Hydrogen in water? _______________
1. What is the formula for Hydrogen Peroxide or Dihydrogen Dioxide? ___________
2. What is the mass ratio of Oxygen to Hydrogen in hydrogen peroxide? __________
The Law of Multiple Proportions

Whenever the _______________ two elements form _______________ than one
_______________, the different _______________ of one element that combine with the
_______________ mass of the other element are in the _______________ of small
_______________ numbers.
Guidelines for Writing the Chemical Formula of a Compound
1. An _______________ ending generally indicates a _______________ compound.
2. An _______________ or _______________ ending means a _______________ ion that contains
_______________ is in the formula.
3. _______________ in a name generally indicate that the compound is _______________.
4. A _______________ _______________ after the name of a _______________ shows the
_______________ of the _______________.
11
Chapter 9 Notes
Honors Chemistry
Naming Review
Naming Practice
Formula
Name
Sodium chloride
BrF3
LiNO3
Dinitrogen tetrahydride
Potassium hydroxide
Rb2O
Hydrofluoric acid
Book Work - Page 279 #35, 39-41
12
Ionic or Molecular?