CHEMISTRY-CP, CHAPTER 9
CHEMICAL FORMULAS AND BONDING
OBJECTIVES
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Describe the development of the periodic table
Define periodic table and periodic law
Identify and define groups and periods
Name the groups on the periodic table
Identify an element as either a solid, liquid, or gas based on the periodic table.
Determine if an element is radioactive or synthetic based on its position on the periodic table
Describe the following periodic properties of the periodic table: energy levels, valence electrons, and
Lewis Dot Diagrams
Define the octet rule
Determine the oxidation numbers of the elements and describe the pattern of oxidation numbers found
on the periodic table
Distinguish between metals, nonmetals and metalloids
State the octet rule
Define ion, monatomic ion, polyatomic ion, cation and anion
Name anions and cations
Write ion symbols
Identify and name the polyatomic ions
Illustrate how ionic bonds form
Define ionic and covalent bonds
Define binary ionic compound & ternary ionic compound and give examples of each
Name ionic compounds
Determine the empirical formula of an ionic compound
State the prefixes used in naming
Name and write the chemical formulas for molecular compounds
Define hydrate and anhydrous
Name and write the chemical formulas for hydrates
Describe how to tell a compound is a hydrate
Name and write the chemical formulas for acids
CHAPTER VOCABULARY (VOCABULARY QUIZ ON THURSDAY, OCTOBER 25)
Acid
Element
Molecule
Alkali Metal
Empirical Formula
Monatomic Ion
Alkaline Earth Metal
Formula Unit
Noble Gas
Anion
Group
Nonmetal
Binary Compound
Halogen
Octet Rule
Cation
Hydrate
Monatomic Ion
Chemical Formula
Inner Transition Metal
Oxidation Number
Chemical Symbol
Ion
Period
Compound
Ionic Bond
Periodic Law
Covalent Bond
Ionic Compound
Periodic Table
Diatomic Molecule
Metal
Polyatomic Ion
Electron
Metalloid
Precipitate
Electron Dot Structure
Molecular Compound
Transition Metal
Transuranium Element
Unshared Pair
Valence Electron
In 1860, ___________________ elements had been discovered
 J.W. Dobereiner (early 1800’s):
Triads had:
Examples of triads:
Important because:

Dmitri Mendeleev (1869):
Listed the elements according to __________________________________________.
Important because:
Periodicity:
Examples of Periodicity:
Allowed him to:

Henry Moseley:
Listed the elements according to ________________________________________.
Important because:
The modern periodic table is listed in order of _____________________________.
Periodic Law:
Periodic Table:
Element Key:
Groups(Families):
There are _______________ groups labeled with the numbers ______________________.
Group Number/Location
1
2
3-12
13
14
15
16
17
18
Atomic #57-70
Atomic #89-102 (bottom row)
Group Name
Periods:
There are _________________ periods labeled with the numbers __________________.
Practice Problems
Identify the element with the following designation:
a) Group 2, Period 2
____________________
b) Group 18, Period 6
___________
c) Group 14, Period 5
____________________
d) Group 3, Period 6
___________
e) Alkali Metal in Period 2
____________________
f) Noble gas in Period 4
___________
g) First Lanthanide
____________________
h) Halogen in Period 5
___________
States of Matter:
Solids:
Liquids:
Gases:
Practice Problems
Identify each of the following as either a solid, a liquid or a gas.
a) Arsenic
___________________
b) neon
c) Halogen in Period 4
___________________
d) element in period 5, Group 12________
Types of Elements
1) Metals:
Properties of Metals:
Luster:
_________________
Malleable:
Ductile:
Location of Metals:
Exception:
2) Nonmetals:
Properties of Nonmetals:
Location of Nonmetals:
Exception:
3) Metalloids:
Properties of Metalloids:
Location of Metalloids:
Exception:
Practice Problems
Identify each of the following elements as a metal, a nonmetal or a metalloids.
a) Potassium _______________________
b) Antimony ______________________
c) Carbon
d) Boron
_______________________
______________________
Identify each of the following elements.
a) An element in Period 6 that does not conduct electricity and is a gas
__________________
b) An element in Group 13 that has some metallic properties & some nonmetallic properties______________
c) A liquid that conducts electricity
________________________
Radioactive Elements:
Radioactivity:
Elements are radioactive because they have too many or too few ____________________________.
Synthetic Elements:
Synthetic elements are __________________________.
Electrons are located __________________________________in _______________________________.
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Energy Level 1 can hold a maximum of ____________ electrons
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Energy Level 2 can hold a maximum of ____________ electrons
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Energy Level 3 can hold a maximum of ____________ electrons
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Energy Level 4 can hold a maximum of ____________ electrons
Valence Electrons:
o Pattern for the # of valence electrons within the representative elements
Group
1
2
13
14
15
16
17
18
o Transition Metals:
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Exceptions
 Silver is always _________________
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Zinc is always __________________
o Inner Transition Metals:
Practice Problems
How many valence electrons does each of the following elements have?
a) phosphorus____________________
b) calcium
_____________________
c) zinc
d) fluorine
_____________________
____________________
e) uranium ____________________
Lewis Dot Diagrams:
f) germanium _____________________
Practice Problems
Draw the Lewis Dot Diagram for each of the following elements.
a) Iodine
__________________________
b) Aluminum ________________________
c) Xenon
__________________________
d) Silver
________________________
Oxidation Number:
o Ion:
o Octet Rule:
 If an element loses electrons, its oxidation # is a ___________________ number
because:

Cation:
o Elements with 1-3 valence electrons:
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If an element gains electrons, its oxidation # is a __________________ number because:
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Anion:
o Elements with 5-8 valence electrons:
o Elements with 4 valence electrons:
 Pattern for the oxidation #s of elements within the representative elements:
Group
1
2
13
14
15
16
17
18
o Transition Metals:
Exceptions
Zinc is always _________________
Silver is always ________________
o Inner Transition Metals:
Monatomic Ions:
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Cation:
o To Name a Cation:
 Transition Metals:
o To Name a Transition Metal:
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Except:
Anion:
o To Name:
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Ion Symbol:
Example: Write the ion symbol for the ions formed from the following elements.
a) Lithium
b) Aluminum
c) Silver
d) Phosphorus

e) Selenium
g) Bromine
Example: Name the following ions.
a) Fe2+
b) Cl-
c) N3-
d) K+
f) P3-
e) Zn2+
Polyatomic Ions:
-Names typically end in:
-The only positively charged polyatomic ion is:
-Where should you look to find the polyatomic ions?
Example: Name the following ions.
a) PO4 3-

b) O2-
Example: Write the symbols for the following ions.
a) nitride
b) nitrate
Ionic Compound:
o Binary Ionic Compound:
c) NH4+
c) nitrite
o Ternary Ionic Compound:
o Ionic Bond:
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An ionic bond is formed between an ______________________ and
a __________________________ because:

Therefore, ionic bonds form between ___________________
and ______________________________ because:
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Electrons are ________________________________ in an ionic bond because:
Empirical Formula:
o Subscripts:
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Shows:
Three different ways to determine the empirical formula (all get the same result):
To illustrate an ionic bond to determine the empirical formula:
Examples:
a) Show how an ionic bond forms between sodium and iodine.
b) Show how an ionic bond forms between calcium and chlorine.
c) Show how an ionic bond forms between aluminum and oxygen.
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To use charges to determine the empirical formula:
Examples: Write the chemical formulas for the compounds formed from the following two
ions.
a) Potassium and chloride
b) Ammonium and sulfide
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The Crisscross method of determining the Empirical Formula
Example: Use the crisscross method to determine the empirical formulas for the
compounds formed from the following two ions.
a) zinc and oxide
b) Sodium and hydroxide
To Name an Ionic Compound
1)
Ex. 1—CaCl2
Ex. 2—Fe2O3
Ex. 3--NaOH
2)
3)
Ionic Compound Examples:
1) Name the following compounds:
a) MgS
b) CaSO4
2) Write the chemical formulas for the following compounds.
 Cobalt(II) chloride
b. potassium bromide
c) Cu(C2H3O2)2
c. manganese(IV) oxide
Covalent Compound (Molecular Compound):
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Covalent Bond:
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A covalent bond is formed between 2 or more __________________
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Electrons are ________________________________ in a covalent bond because:
Molecule:
1. Diatomic Molecules:
a. The 7 Diatomic Molecules:

Molecular Substance:
Naming Molecular Compounds
-Numerical Prefixes
1
2
3
4
5
6
7
8
9
10
-To Name a Molecular Compound:
Examples--Name the following molecular compounds:
a) N2O4
b) PCl5
c) NO2
-To Write the Chemical Formula of a Molecular Compound:
Example—Write the chemical formulas for the following molecular compounds.
a) nitrogen trifluoride
b) diphosphorus pentoxide
c) carbon tetrachloride
Other Types of Compounds:
-Hydrates:
-Anhydrous:
-To Name a Hydrate:
Example: Name the hydrate MgSO4  2H2O.
-To Write the Chemical Formula of a Hydrate:
Example: Write the chemical formula for copper(II) pentahydrate.
-Acid:
-start with:
-To Name a Binary Acid:
Example: HCl
To name a ternary acid:
Example: Name HNO3
Other Common Acids:
HNO3 = nitric acid
H2CO3 = carbonic acid
H2SO4 = sulfuric acid
H3PO4 = phosphoric acid
HC2H3O2 = acetic acid