Chapter 7 and 8 Notes
Honors Chemistry
Chapter 7: Ionic and Metallic Bonding
Section 1: Ions
(read pages 187-193)
Valence Electrons
 electrons in the _______________ energy level
 involved in _______________
 Pattern on the periodic table (page 188, Table 7.1)
o
o
o
o
o
o
o
o
o
Group _____ = _____ Valence Electron
Group _____ = _____ Valence Electrons
Groups __________ = __________ in Valence Electrons
Group _____ = _____ Valence Electrons
Group _____ = _____ Valence Electrons
Group _____ = _____ Valence Electrons
Group _____ = _____ Valence Electrons
Group _____ = _____ Valence Electrons
Group _____ = _____ Valence Electrons
 exception: _______ only has _____ valence electrons
Electron Dot Structures
 _______________ that shows the _______________ electrons as dots
 ________ dot (electron) on each side __________ start _______________ up
Practice:
Octet Rule
 atoms want to acquire 8 electrons in their _______________ energy level to become
_______________
o Again, the idea of _______________ s and p _______________
 atoms will _______________ with each other in some _______________ way to obtain these
_____ valence electrons
 Exceptions: _____ and _____ only need _____ valence electrons
Cation



atom _______________ electrons, _______________
a _______________ charged ion
name _______________ the _______________
1
Chapter 7 and 8 Notes
Honors Chemistry
Example
Na (atom) structure
Na )2e- )8e- )1e What does Na need to become stable (happy)? __________________
 Is it easier for Na to lose its 1 ve- or gain 7 electrons? _____________
So the Na atom becomes Na ion:
 __________ (ion – cation) Na )2e- )8e- (lost the outer e-)
 Now Na is stable and the name stays _______________
 Looks like __________ but still has Na properties
Anion
 atom _______________ electrons, _______________
 a _______________ charged ion
 name _______________ to _______________ _______________
Example
Cl (atom) structure
Cl )2e- )8e- )7e What does Cl need to become stable (happy)? __________________
 Is it easier for Chlorine to lose its 7 ve- or gain 1 electron? _________
So the Cl atom becomes Cl ion:
 __________ (ion – anion)
Cl )2e- )8e- )8e- (gained 1 e-)
 Now Cl is stable and the name changes to _______________
 Looks like __________ but still has Cl properties
Practice Problems
Give the name and symbol of the ion formed when:
a. a nitrogen atom gains three electrons - ________________________
b. a calcium atom loses two electrons - _________________________
c. a fluorine atom gains one electron - __________________________
d. An arsenic atom gains three electrons - _______________________
e. A beryllium atom loses two electrons - _______________________
Charges Based on Groups
 Group _____ = Ions with a _____ charge ( _______ 1 electron)
 Group _____ = Ions with a _____ charge ( _______ 2 electrons)
 Groups __________ = Ions with ____________ charges (all ______________)
 Group _____ = Ions with a _____ charge ( _______ 3 electrons)
 Group _____ = Ions with a _____ charge ( _______ or ___________ 4 electrons)
 Group _____ = Ions with a _____ charge ( ___________ 3 electrons)
 Group _____ = Ions with a _____ charge ( ___________ 2 electrons)
 Group _____ = Ions with a _____ charge ( ___________ 1 electron)
 Group _____ = Does ________ form _________ (already ______________)
Book Work – Page 193 #3-10
2
Chapter 7 and 8 Notes
Honors Chemistry
Section 2 – Ionic Bonds and Ionic Compounds
(Read pages 194-199)
Ionic Bonds
 _______________ charges attract
 _______________ of electrons
 between a _______________ and a _______________
 called a _______________
Example: Sodium and Chlorine
**
Na
*Cl**
**
Example: Sodium and Oxygen
Example: Magnesium and Oxygen
Formula Unit
 __________ whole-number ratio of __________ in an __________ compound
Practice Problems
Use electron dot structures to determine chemical formulas (and names) of the ionic compounds formed
when the following elements combine:
a) Potassium reacts with Iodine
b) Aluminum reacts with Oxygen
c) What is the formula of the ionic compound composed of calcium cations and chloride anions?
3
Chapter 7 and 8 Notes
Honors Chemistry
Short Cut – Crisscross Method
1. __________________________________________________________________
2. __________________________________________________________________
3. __________________________________________________________________
4. __________________________________________________________________
Example: Barium and Nitrogen
Ba2+
N3-
Practice Problems
Determine the chemical formulas and names of the ionic compounds formed when the following
elements combine:
a) Magnesium and Chlorine ___________________________________
b) Aluminum and Sulfur ______________________________________
Ionic Compounds Properties
 _______________ solids
 _______________ melting points
 conduct _______________ when _______________ in water
Let’s Review
1. Write the correct chemical formula for the chemical compounds formed from each pair of ions.
Name the compound that is formed.
a. Rb+, O2- ___________________________________
b. Ca2+, N3- ___________________________________
c. Fr+, F- ___________________________________
d. Al3+, P3- ___________________________________
2. Write the formulas for each compound.
a. Strontium iodide ___________________________________
b. Lithium boride ___________________________________
c. Beryllium sulfide ___________________________________
d. Potassium selenide ___________________________________
4
Chapter 7 and 8 Notes
Honors Chemistry
3. Decide whether or not the following pairs of elements will form ionic bonds. If not, explain.
a. Na and Ne ___________________________________
b. K and Br ___________________________________
c. N and S ___________________________________
d. Rb and Be ___________________________________
Book Work – Page 199 #14-20, 22
Section 3 – Bonding in Metals
(Read pages 201-203)
Metallic Bond
 attraction of the _______________valence electrons
o “______________________________”
 between a _______________ and a _______________
Metallic Bond Properties
 good _______________ of electricity
 ductile - _____________________________________________
o example: _______________ wire
 malleable - _____________________________________________
o example: _______________ foil
 atoms are _______________ with an orderly _______________
Alloy
 _______________ of metals
 _______________ are _______________ to those of their _______________ elements
Book Work – Page 203 #23-26
Chapter 8: Covalent Bonding
Section 1 – Molecular Compounds
(Read pages 213-216)
Covalent Bond
 _______________ of electrons
o _______________ is _______________!
 between a _______________ and a _______________
 called a _______________
o _______________ molecule – consists of the same __________ atoms
 examples:
5
Chapter 7 and 8 Notes
Honors Chemistry
Covalent Compounds Properties
 _______________ or _______________
 _______________ melting points
 do __________ conduct _______________ when _______________ in water
Molecular Formula
 _______________ formula for the molecular (_______________) compound
 Shows how many _______ of each element are in a compound - does not show ______________
Book Work – Page 216 #1-6
Section 2 – The Nature of Covalent Bonding
(Read pages 217-222)
Structural Formula
 represents the covalent bonds by _______________ and _______________
 single bond
o sharing of _____ electrons
o __________ dash line
 unshared pair
o _______________ pair or electrons
Practice Problems
The following covalent molecules have only single covalent bonds. Draw an electron dot structure for
each.
1. NF3
2. SBr2
6
Chapter 7 and 8 Notes
Honors Chemistry
Double Vs. Triple Bonds
 Double Bond
o _______________ of _______________ electrons
o _______________ dash lines
 Triple Bond
o _______________ of _______________ electrons
o _______________ dash lines
Coordinate Covalent Bond
 A _______________ bond in which _______________ atom contributes _______________
_______________ electrons
 Example:
Bond Dissociation Energies
 _______________ required to _______________ the _______________ between two
_______________ bonded atoms
 A _______________ bond _______________ energy means the bond is _______________ to
break
Resonance Structure
 A _______________ that occurs when it is possible to draw _______________ or
_______________ valid _______________ _______________ structures that have the
_______________ number of _______________ _______________ for a _______________ or
_______________
 Example:
Exceptions to the Octet Rule
 _______________ and _______________ octets can occur
 _______________ Octet example:
o _______________
o Draw it:
7
Chapter 7 and 8 Notes

Honors Chemistry
_______________ Octet example:
o _______________ and _______________
o Draw it:
Book Work: Page 229 #14, 16, 17, 20, and 21
Section 3 – Bonding Theories
(Read pages 230-236)
Molecular Orbitals
 _______________ atomic _______________ form _______________ orbitals
 Remember the atomic orbitals: _____________________ from Chapter 5?
Sigma Bonds
 Formed when _______________ atomic _______________ combine to form a
_______________ orbital that is _______________ around the _______________ connecting
the _______________ atomic _______________
 Simply – a _______________ _______________ of orbitals _______ to _______
 _______________ bonds
 Symbol is Greek letter _______________ (σ)
Pi Bonds
 When _______________ atomic _______________ combine to form a molecular
_______________ by _______________ _______________ by ______________
 Simply: an _______________ of _______________ __________ by __________
 _______________ than _______________ bonds because of ___________ overlap
 Symbol is Greek letter _______________ (π)
8
Chapter 7 and 8 Notes
Honors Chemistry
Comparison of Sigma vs. Pi bonds in a P orbital
VSEPR Theory
 _______________ _______________ _______________-_______________
_______________ Theory
 States that because _______________ pairs _______________, _______________ adjust their
_______________ so that _______________ electron pairs are as _______________
_______________ as possible
 Helps _______________ the _______________ _______________ of an atom
There are multiple different shapes that a molecule can have:
 _______________ the shape by looking at _______________ of the _______________ atom.
o Characteristics include:
 How many _______________ pairs
 How many _______________ pairs
 See chart on next page (you only need to know the few in the chart that we talk about!)
Practice Problems
Determine the molecular shape of the following molecules:
1. SBr2
2. HCl
3. SiF4
Book Work – Page 236 #24 and 27
9
Chapter 7 and 8 Notes
Honors Chemistry
Codes for Molecular Geometry
Remember – you’re looking at the central atom!
All 2 atom molecules are LINEAR!
Shape
and
Example
Linear
#Bonded
Pairs
Angular
2
#Lone
Pairs
Draw It
Name of
Shape
#Bonded
Pairs
#Lone
Pairs
4
1
4
2
5
0
5
1
6
0
Tetrahedral
1
See-Saw
(Disphenoidal)
O3
SF4
Bent
Square Planar
XeF4
Trigonal
Planar
3
0
Trigonal
Bipyramidal
BeF3
Trigonal
Pyramidal
PCl5
3
1
Square
Pyramidal
NH3
T-Shape
BrF5
3
2
Octahedral
ClF3
SeCl6
Solid Line – Same Plane
Triangle – In Front of Plane
Dotted Line – Behind Plane
10
Draw It
Chapter 7 and 8 Notes
Honors Chemistry
Section 4 – Polar Bonds and Molecules
(Read pages 237-241)
Nonpolar Covalent Bond
 atoms _______________ the electron _______________
 consists of the _______________ 2 _______________
 _______________ molecules
Polar Covalent Bond
 atoms _______________ the electron _______________
 one atom has a _______________ electronegativity than the another and _______________ onto
the electron _______________
 REMINDER: What is electronegativity? The _______________ of an atom to
_______________ electrons
Dipole
 each atom is _______________ charged
 one atom is partially _______________, written as _____
 one atom is partially _______________, written as _____
Beside properties, we can _______________ determine if a compound will be Ionic, Polar Covalent, or
Nonpolar Covalent.
What number are we interested in? ______________________________
Find this number on your periodic table.
We want the electronegativity _______________ between the two atoms, what math are we going to
do? _______________
Nonpolar Covalent
Polar Covalent
Ionic
Do this notation on your periodic table!
Practice Problems
30. Identify the bonds between each pair of elements as nonpolar covalent, moderately polar
covalent, very covalent, or ionic.
a. H and Br _____________________________________________________
a. K and Cl _____________________________________________________
b. C and O _____________________________________________________
c. Cl and F _____________________________________________________
d. Li and O _____________________________________________________
e. Br and Br _____________________________________________________
11
Chapter 7 and 8 Notes
Honors Chemistry
31. Place the following covalent bonds in order from least to most polar:
a. H – Cl
b. H – Br
c. H – S
d. H – C
Hydrogen Bond
 includes _______________
 _______________ bonds
 holds _______________ together
Book Work - Page 244 #32, 37
Overall Review
Make a REVIEW chart, mind map (web), or foldable comparing the 3 types of bonds (Ionic, Metallic,
Covalent). Be sure to include:
1. types of elements (metal, nonmetal)
2. physical state of matter (solid, liquid, gas)
3. what the electrons do (transferred, shared, free-flowing)
4. melting points (high or low)
5. conductivity (yes or no)
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