Unit 5 - Bonding
Lesson 1 – Ionic Bonds
Lewis Dot Diagrams Review
A way of showing atoms and ________________________
Atoms are represented by an atomic symbol with its __________________
Valence electrons depend on _______________
The Octet Rule
Atoms are most stable when ___________________________________________
Level 1 = ______________
All other shells = __________
Noble gases have _________________________ so they don’t bond with anyone
Other atoms __________________________ electrons to get a full outer shell
Ionic Bonding
___________________________ between ______________ and ________________.
___________________electrons are __________ by _____________ , ______________ by
_________________.
Diagram:
Metals _______________________ to get a stable outer shell (revert back to 8)
Nonmetals _______________________ electrons to get a stable outer shell (add as many as
needed until 8)
Diagram:
Properties of Ionic Compounds
Most have high __________________________________________________.
Many ___________________________________. Most are ________________________.
Good conductors of electricity if _________________________________________________.
Form ___________________________________________.
Ionic bonds are usually __________________________. If stressed, the bonds will break along a
______________________________.
Metal Cations
Type I

metals whose ions can only have __________ possible charge
 IA, IIA, (Al, Ga, In, Zn, Cd, Ag)

determine charge by _________________ on the Periodic Table
 IA = 1+, IIA = 2+, (Al, Ga, In = 3+; Zn & Cd = 2+; Ag = 1+)
Type II

metals whose ions can have ____________________________ possible charge (mostly
____________________________________________________)
Polyatomic Ions
Polyatomic ions are made of _____________________. Polyatomic ions are ______________________
that travel together—____________________. The given charge is on the _________________________,
not on ________________________ within the polyatomic ion.
A list can be found on page 7 of your reference packet. You are responsible for knowing:
_____________________________________________________________________________________
You will have a quiz on the ___________________________________________ of these polyatomic ions.
Naming Type I Metals Ionic Compounds
All names are composed of a ________________ (positive metal ion) and an ____________
(negative nonmetal ion or polyatomic ion)
Cation (metal) is _________________
Anion (nonmetal) is element name with ___________ on the end or name of polyatomic ion.
Examples – Name the following
NaCl
MgO
Li3PO4
NH4Cl
Formulas for Ionic Compounds
_____________the ions so the compound has a charge of______________
Magnesium Fluoride
Silicon Sulfide
Examples – Find the formulas of:
Calcium Oxide
Aluminum Chloride
Magnesium Nitrate
Extra Rules for naming Ionic Compounds with a Type II metal ions:
_____________________ are named like normal but with a _____________________ to
indicate___________________________________________.
FeCl3
Examples – Naming Ionic Compounds with Type II metal ions:
CuSO4
VCl5
FeO
Strong and Weak Electrolytes
 An aqueous solution that is a ______________________ of electricity is a
______________________(complete ____________________________________ of ions).
 An aqueous solution that is a poor conductor of electricity is a _______________________.
 The greater the __________ of ionization or dissociation, the _______________________
of the solution.
Lesson 2 - Metallic Bonding
Metallic bond
Occurs between atoms with ________________________________________.
Metal atoms pack ______________________________, like oranges in a box.
Creates a _____________________ lattice formation
Diagram:
Many metals have an ___________________________
In an effort to be ______________, their outer electrons become __________________
amongst _________________.
No valence electrons belong to one atom, ________________________.
______________________ move around throughout the piece of metal.
Metallic bonds are not ________________, but nuclei with ____________________.
Electron Sea Model
Metals can be thought of as ______________ suspended in “sea” of
________________________.
Attractions hold __________________________________, but not so tightly as to impede
their flow.
This explains many of the properties of metals, like ___________________________________
Physical Properties
Conductivity
Delocalized electrons are ___________________ so when a potential difference is applied
they can carry the _______________________ along
Mobile electrons also mean they can transfer _______________well
Ductility
Delocalized electrons allow metals to be __________________________________________.
Luster
The interaction between the ________________ with light makes them shiny (luster)
Malleability
The electrons are attracted to the nuclei and are __________________________________.
The layers of the metal atoms can ___________________________________________
without the need to ______________________ in the metal
______________is so extremely malleable that 1 gram can be hammered into a sheet that is
only 230 atoms thick (70 nm)
Diagram:
______________________ allow atoms to slide by without breaking
Melting/Boiling points
Metals melt at a ________________________ temperatures
Metals boil at an _________________________________ because it requires the ________
____________________________to break away from the others, which takes a ton of energy.
Gallium can melt in your hand at __________________, but it boils at ___________________!
Alloys
Alloy = ______________________________________
Mixing one metal with other metal(s) or non metal(s) often __________________ its properties
Steel is _________________ than pure ________________because the ______________
prevents the delocalised electrons to move so readily.
If too much ________________ is added then the metal is _________________.
Alloys are generally less _______________ and ________________ than the original metal(s)
Some alloys are made by melting and mixing two or more metals
Bronze =
Stainless Steel =
Carbide =
Lesson 3 - Covalent bonding
Covalent Bonding
Takes place between two ____________________
Electrons are _____________ by both nuclei to help each attain _________ valence electrons.
There are several ____________________________ in these bonds:
Attractions between _____________________________
Repulsions between ________________________
Repulsions between ________________________
A _______________ is formed when two or more atoms bond _______________
Polar and Non-polar Covalent Bonds
Though atoms often form compounds by ______________________, the electrons are not always
shared ___________________.
If the electrons are shared ____________ it is a _______________ covalent bond
If the electrons are ______ shared equally it is a _______________ covalent bond
Properties of Covalent Compounds
1.
2.
3.
4.
Lewis Structures
Using an atoms _________________________ we can predict how different atoms will bond
covalently to form ___________________
Each __________________between atoms requires each atom to share _____________ with
the other atom.
Example:
Dot Diagram Steps
Draw out atoms with ________________________________
Connect ________________ to share until _______________ have full shells
_________________ with ______________________ as the bond
______________ any _____________ of electrons not involved with bonding
Example: NH3
Double and Triple bonds
Sometimes _____________________________ of electrons are shared to meet the octet rule
Double Bonds= _________________ of electrons shared between two atoms.
These bonds are _________________ and ________________ than _______________bonds.
Triple Bonds= __________________of electrons shared between two atoms
These bonds are _________________ and ________________ than _______________bonds.
Some Clues for Drawing Dot Diagrams
Put the ________________ in the ___________ of the dot diagram (the one that will have the
most bonds)
________________ is never in the middle of the dot diagram
A dash represents____________________________
Practice Drawing
Draw dot diagrams for the following:
CH4
PCl3
COH2
Exceptions to the Octet Rule
The Lewis structure for NO (with odd number of electrons)
SH2
The Lewis structure for boron (B): Boron shares ________ electrons to form ______________
bonds.
The Lewis structures of SF4 and PCl5 (for elements in Period 3 or greater)
Some common bonding patterns:
C = ___ bonds & ___ lone pairs, different bonding combinations:
___ single bonds
___ double bonds
___ single + ___triple bond
___single + ___double bond
N = ___ bonds & ___ lone pair
O = ___bonds & ___ lone pairs
H and halogen = ___ bond
B = ___ bonds & ___ lone pairs
Naming Covalent Bonds
Write names of _________________________
Add __________________ to the last name
Add _________________ at beginning of each word to indicate how many of each element.
Exception- do not use _____________ in front of the ___________ element
Covalent Bonding Prefixes
1=
2=
3=
4=
5=
6=
7=
8=
9=
10=
Practice Naming
Name the following:
CCl4
PCl3
SH2
CO2
NO3
Moleular Elements
 Certain elements occur as 2 atom molecules
 Rule of 7’s
 there are 7 common ______________ elements
 find the element with _____________________ 7, N
 make a _______________ by going over to Group 7A, then down
 don’t forget to include ____________________
Common Covalent Compounds:
Know the names of:
Water
Ammonia
Methane
Acid Nomenclature
How to identify an acid:
The formula of an acid starts with _____________ (for now)
HCl =
HNO3 =
H3PO4 =
Two types of acids:
1.
(Two elements, one of which is _______________________)
Examples:
2.
(contain ________________, usually a ____________________ bonded to hydrogen)
Examples:
If it is a binary acid:
Prefix =
root =
Suffix =
HCl =
HBr=
H2S =
If it is an oxyacid:
Prefix =
root =
Suffix =
If anion ends in _____________replace with _______________
If anion ends in _____________ replace with _______________
Example: HNO3
Example: HNO2
*Sulfate/ite root goes to sulfur (sulphuric and sulphurous acid). Same is true for phosphate
For Example
Examples
1. HNO2
3. H3PO4
5. HCl
2. H2SO3
4. HNO3
6. H2SO4
Try on your own
1. HCl
5. H2CO3
9. H2CrO4
2. HBr
6. HC2H3O2
10. H2Cr
3. H2SO4
7. H3PO4
4. H2S
8. H3P
Try writing the formulas:
1. Sulfuric acid
2. Nitric acid
3. Hydrochloric acid
4. Acetic acid
5. Hydrofluoric acid
6. Phosphorous acid
7. Carbonic acid
8. Nitrous acid
9. Phosphoric acid
10. Hydrosulfuric acid
Lesson 4 – Molecular Geometry. VSEPR, and Polarity
VSEPR Theory
VSEPR =
Electrons ____________ each other in a molecule
The structure around a _________________________ is determined by _______________
electron-pair repulsions (getting pairs of electrons as far apart as possible)
Think about 300 students in the gym, and everyone swinging their arms to make sure they have space on all
sides in every direction
Helps to predict the ________________ of molecules
Steps For Determining Shape
Draw the dot diagram for the _____________________
Most compounds follow _________________ but not all of them (note: only the central atom
can break the octet rule. _______________ breaks the rule)
Determine how many _______________ of electrons are on the _________________ atom
Determine how many _____________ the central atoms is involved in. (each bond, whether
single, double or triple, counts as ______________shared pair)
Look at number of bonds (_________________) versus unshared (___________) pairs of
electrons and assign the correct shape
Linear
Total Pairs =
Shared pairs =
Unshared (lone) pairs =
Trigonal Planar
Total Pairs =
Shared Pairs =
Unshared (lone) Pairs =
Tetrahedral
Total Pairs =
Shared Pairs =
Unshared (lone) Pairs =
Trigonal Pyramidal
Total Pairs =
Images
Shared pairs =
Unshared (lone) pairs =
Bent
Total Pairs =
Shared Pairs =
Unshared (lone) pairs =
Bond Angles
Bond angles are determined by the number of ___________________ pairs of electrons which
push the _____________________ closer together
Linear =
Tetrahedral =
Trigonal Planar
Trigonal
pyramidal=
Bent =
Polar Covalent Bonds
Covalent Bonding
A covalent bond is a _______________________ of electrons electrostatically attracted to the
_______________nuclei of two atoms.
The atoms achieve a stable outer _________________________ (a noble gas arrangement)
by __________________ electrons.
Both _______________ try to pull the electrons towards _________________
This is like a _________________ where both sides are pulling on the _________________.
It creates a ___________________ between the two atoms.
Picture a tug-of-war:
If both teams pull with the ________________ the mid-point of the rope will not move.
Pure Covalent Bond
This __________________ of the rope can be compared to a ________________________,
where the bonding pair of electrons are held at the _________________ between the nuclei of
the bonding atoms.
Polar Covalent Bond
What if it was an _____________ tug-of-war?
The team on the right are __________________, so will pull the rope harder and the
____________________ of the rope will move to the right.
A __________________________________ is a bond formed when the shared pair of
electrons in a covalent bond are not shared ________________.
This is due to different elements having different __________________________.
If _____________________ contained a ____________________ bond, the electrons would
be shared equally as shown above.
However, ______________________ has a higher electronegativity and pulls the bonding
electrons towards __________________
e.g. Hydrogen Iodide
This makes iodine ____________________ and hydrogen ___________________. This is known
as a __________________.
In general, the electrons in a covalent bond are _________________________.
________________ indicates where the bonding electrons are most likely to be found.
Although all covalent bonds involve ___________________, they differ widely in the
____________________________
We divide covalent bonds into _______________________________________________
Bonds are polarized along a ______________ from covalent to ionic depending on the difference
in __________________. A polar covalent bond has some amount of _______________________
charges at either end.
Consider the polarities of the following bonds:
Bond
Electronegatvities
Difference
Polar Vs. Non Polar Properties
Polar Covalent
Pure (non-polar) Covalent
Like Dissolved Like
 Polar solvents ___________________ in one another.

Nonpolar solvents ________________ in one another.

This is the ____________________________________________.

Methanol dissolves in water, but hexane __________________ dissolve in water.

Hexane dissolves in toluene, but ______________ does not dissolve in toluene.
Network Solids
A compound with _________________________ bonds.
Highest ___________________________ of all substances.
Examples:
Diamond structures consists of ______________ carbons in a ____________________ array
Graphite structures consist of _______________________ carbons in a ______________ array.
The layers in graphite are able to _____________________________________________.
Fullerenes consist of ______________________________ fused into icosahedral spheres of at
least ____ carbons
Nanotubes are long hollow tubes constructed of ________________________
Other examples include
_________________: covalent atomic solids of ___________________; includes
_________________________________________________
_______________: metalloid almost always found in compounds _______________
•
borax = Na2[B4O5(OH)4]8H2O
•
kernite = Na2[B4O5(OH)4]3H2O
•
colemanite = Ca2B6O115H2O
•
Pyrex
Molecular Solids
A crystalline molecular solid has molecules arranged ________________________________
held together by ____________________________________.
In water, molecules are arranged in a ____________________________________ for ice.
Other examples.
Polymers & Proteins
Substances composed of ______________ characterized by the
____________________ of one or more species of atoms or groups of atoms
_____________________________ to each other in amounts sufficient to provide a
_____________________ that do not vary markedly with the addition of
__________________________ of the repeating units.
Common Polymers
Polymers are common in nature. __________________________________________________
are all examples of polymers
A wide variety of ________________________ have been produced, largely from
________________________________. These include _____________________________
Polymer & Protein Structure
Molecular Mass:
High ________________________ structures
Extremely large molecular weights are to be found in ___________________________ with
very long chains.
Molecular Shape:
Chain molecules are usually _________________________________
These chains may _______________________________, leading to extensive intertwining
and entanglement of neighboring chain molecules.
These random coils and molecular entanglements are responsible for many of the important
characteristics of such as _________________________________________.
Molecular structure and function are ____________________________.