General Chemistry
Bonding- Chapters 7-8
Mr. Hines
Part A – The Octet Rule
1
Identify the various families on the periodic table and describe their properties.
2
Interpret the octet rule
3
Define Lewis dot structure and be able to write them.
4
Explain the easiest path for an atom to achieve an octet and give examples.
5
Determine which elements violate the octet rule and explain why.
6
Identify charges on Subatomic particles and explain the effects.
7
Explain charges on Elements
8
Label the charge above each group on the periodic table and explain where it comes from.
9
Evaluate the placement of hydrogen and helium on the periodic table
Part B – Ionic Bonds
10 Explain how Ionic Bonds form
11 Explain how ionic compounds are formed.
12 Distinguish between a Superscript and Subscript
13 Predict the formula of an Ionic compound
Part C – Covalent Bonds
14 Explain How Covalent Bonds Form.
15 Use classical models of the atom and Lewis dot structures to explain Covalent bonding.
16 Define Lone pair electrons, unpaired electrons, and how they influence covalent bonding.
17 Identify the 3 kinds of covalent bonds
18 Identify the 2 ways of drawing covalent bonds
19 Draw individual elements with proper Lewis dot structures and stick drawings.
20 Draw single covalent bonds with proper Lewis dot structures and stick drawings.
21 Draw double covalent bonds with proper Lewis dot structures and stick drawings.
22 Draw Triple covalent bonds with proper Lewis dot structures and stick drawings.
23 Compare and Contrast ionic bonds and covalent bonds.
Part D – Metallic Bonds
24 Define metallic bonding, explain how it works, and give examples
25 Define alloys, indicate reasons for creating alloys, and give examples
26 Describe properties of metals and alloys
PART A – THE OCTET RULE
Vocabulary
Bonding
Subatomic
particle
Properties
Easiest path
Attract
Overall charge
Atom
Valence
electron
Octet rule
Family
Repel
Metalloid line
Element
Lewis dot
structure
Ion
Lawn mower
Cation
Salt
Proton
Negative
charge
Noble gas
Positive charge
Anion
Energy level
Neutron
Chemistry
Electron
Period
Oct
Group
Metal
Stable
Neutral charge
Non-metal
Objective 1 - Identify the various families on the periodic table and describe their
properties – Go to the periodic table if families.
Objective 2 - Interpret the octet rule
A. Noble gases – Family of elements on the periodic table in ________________________.
B. The noble gases all have their outermost energy levels ______________ with electrons.
C. When an atom’s outermost energy level is filled, it is called “stable.”
D. Stable is a condition where change is ______ likely.
E. All of the elements on the periodic table will try to become stable like the Noble gases.
F. In other words, ____ other elements will try to get 8 electrons in their outermost energy level.
G. It can also be phrased that elements will try to get 8 valence electrons.
H. In order to achieve this, elements will _____________________ electrons from other atoms.
I. This is known as the “OCTET RULE.”
J. Octet rule – atoms will gain or lose electrons in order to obtain the electron structure of a noble gas
– usually eight electrons (oct=8)
 Questions
1. What is meant by the term “stable?” _______________________________________________
2. What is something in your life that is stable? ________________________________________
3. What is meant by the term “unstable?” ________________________________________________
4. What is something in your life that is unstable? ________________________________________
5. How many electrons on the outermost energy level will create a stable atom? _________
6. How many valence electrons will create a stable atom? _________
7. What will atoms do to get 8 valence electrons? _______________________________________
8. What is the octet rule?
_______________________________________________________________________________
9. What number does “oct” represent? ________
Objective 3 – Define Lewis dot structure and be able to write them.
A. Lewis Dot Structure – Abbreviated diagram of an atom showing only the valence electrons.
B. Why write Lewis dot structures? A large part of chemistry involves the understanding of how
atoms bond together – ____________________________- alone - are responsible for bonding.
Writing Lewis dot structures is a shortcut to drawing atoms and their electrons
C. ______________________________________ are best learned by doing them.
Draw a Lewis Dot Structure for the following Elements.
H
He
Li
Be
B
C
N
O
F
Ne
Na
Mg
Al
Si
P
S
Cl
Ar
K
Ca
Objecive 4 – Explain the easiest path for an atom to achieve an octet and give examples.
A. If you were given the choice of using a pair of scissors or a lawnmower to cut the grass in your
yard, which would you choose and why?
B. To achieve an octet, elements will naturally choose the _______________________.
C. For example 1: Magnesium has 2 valence electrons. It is easier for Magnesium to lose its 2
valence electrons to achieve an octet than to gain 6.
Notes
D. Example 2: Chlorine has 7 valence electrons. It is easier for Chlorine to gain 1 electron to achieve
an octet rather than lose 7.
Notes
Symbol
O
P
Ca
Element
Valence
electrons
Gain or Lose
How many?
Noble gas
Lewis structure
Na
Al
F
K
N
Sr
 Questions
1. What family on the periodic table does every element want to be like? _____________________
2. In terms of electrons, what is meant by the easiest path?
________________________________________________________________________________
3. Why does Aluminum lose 3 electrons instead of gaining 5? ______________________________
4. Why does Phosphorus gain 3 electrons instead of losing 5? ______________________________
5. What is the octet rule? ___________________________________________________________
6. What is special about the Noble gas family? ___________________________________________
Objective 5 -Determine which elements violate the octet rule and explain why.
A. Some elements violate the octet rule.
B. This is because the 1st energy level can only hold 2 electrons (not 8)
C. In order for some atoms to become stable, they only need 2 valence electrons.
1
Symbol
2
H
3
Li
4
B
5
C
6
Be
Element
Valence Gain or Lose
electrons
How many?
Noble gas Lewis
structure
 Questions
1. What is the octet rule? _________________________________________________________________
2. Which elements violate the octet rule? ____________________________________________________
3. How many valence electrons does Boron have when it is stable? ____
4. How many valence electrons does Lithium have when it is stable? ____
5. Why are some elements stable without 8 valence electrons? ___________________________________
Objective 6 – Identify charges on Subatomic particles and explain the effects.
A. Charges on subatomic particles
1. Proton = ______________________________(+)
2. Neutron = ______________________________ (zero)
3. Electron = _______________________________(-)
B. Important fact *** Opposite charges attract***
C. Charges on protons
1. Each proton will carry a charge of +1
2. Therefore, 2 protons will have a charge of ____ and 3 protons will have a
charge of ___
D. Charges on electrons
1. Each electron will carry a charge of -1
2. Therefore, 2 electrons will have a charge of ___and 3 electrons will have a
charge of ___
 Questions
1. What is the charge on 1 proton? ______
2. What is the charge on 2 protons? ______
3. What is the charge on 7 protons? ______
4. What is the charge on 1 electron? ______
5. What is the charge on 2 electrons? ______
6. What is the charge on 7 electrons? ______
7. What is true about opposite charges? _________________________________________________
Objective 7 – Explain charges on Elements
A. If protons have a positive charge and electrons have a negative charge, then what is the charge on the element?
B. To determine the charge on the element, you must add the total charge of the protons to the total
charge of the
electrons.
C. If Sodium atom has 11 protons and 11 electrons, then the overall charge on the element will be 0
(zero)
D. If a Sodium ion has 11 protons and 10 electrons, then the overall charge on the element will be +1
E. If an element has a charge of zero, it is called an atom.
F. If an element has a charge other than zero, it is called and ion.
G. If an element has a positive charge, it is called a cation.
H. If an element has a negative charge, it is called an anion.
 Questions
1. What is the overall charge on an element that has 19 protons and 19 electrons? _______
2. What is the overall charge on an element that has 19 protons and 18 electrons? _______
3. What is the overall charge on an element that has 17 protons and 18 electrons? _______
4. What is an element called if it has charge other than zero? ___________
5. What is an element called if it has a positive charge? __________
6. What is an element called if it has a charge of zero? __________
7. What is an element called if it has a negative charge? __________
Objective 8 - Label the charge above each group on the periodic table and explain where it
comes from.
A. Each group on the periodic Table will have a specific charge – Label the charge above each group.
B. Where does the charge for each group come from?
Notes
Objective 9 - Evaluate the placement of hydrogen and helium on the periodic table
Notes
PART B – IONIC BONDS
Bond
Formula
Ionic Compound
Tree
Ionic bond
Binary compound
Superscript
Criss Cross method
Subscript
Objective 10 - Explain how Ionic Bonds form
A. If you remember from earlier, elements can have a positive or negative charge based on the
number of _________________________________________.
B. One important fact about charges is that opposite charges will ________________ each other.
C. Therefore, a positively charged _____________will attract a negatively charged anion.
D. When atoms stick together, it is called bonding.
E. The force that holds different ions together ___ similar to the force that holds 2 magnets together.
F. Ionic bond – force of attraction that holds ions together due to opposite charges.
G. For example, Sodium will have a ____charge and Chlorine will have a ___ charge – This will
cause 1 atom of Sodium to bond with 1 atom of Chlorine. Formula - NaCl – Name Sodium Chloride.
H. When metals (positive charge) bond with non-metals (negative charge), the compound is called a
___________.
Objective 11 - Explain how ionic compounds are formed.
A. When 2 or more ions are bonded together, it is called an ________________________.
B. Ionic compounds will always have a charge of ________________.
C. For example; NaCl: the +1 and the -1 charge adds up to ZERO.
D. Another example: Potassium and Oxygen.
Notes
Objective 12 – Distinguish between a Superscript and Subscript
A. A superscript is a number that is written above and to the right of a character.
B. Ionic charges are written as superscripts. Example: Na+1
C. A subscript is a number that is written below and to the right of a character.
D. The number of atoms is written as a subscript. Example: O2
Objective 13 – Predict the formula of an Ionic compound
Notes: Criss Cross
Practice
Cation
Charge Anion
Sodium
Fluorine
Lithium
Fluorine
Potassium
Oxygen
Potassium
Nitrogen
Aluminum
Sulfur
Calcium
Oxygen
Boron
Fluorine
Charge
Symbols
Formula
 Questions
1. What causes an ionic bond? ____________________________________________________
2. What is a cation? ___________________________________
3. What is an anion? ___________________________________
4. What is a superscript? ________________________________
5. What is a subscript? _________________________________
6. What is the overall charge on an ionic compound? _________
Overall
charge
PART C – COVALENT BONDS
Covalent
bond
Lone pair
electrons
Unpaired
electrons
Single
bond
Double
bond
Triple bond Stick
Stick
drawing
Objective 14 – Explain How Covalent Bonds Form.
A. Compounds are not limited to bonds formed by the attraction of elements of positive and negative
charges (_________________________________).
B. On many occasions, non-metals will bond with other non-metals.
C. How can this be since non-metals do not give up electrons in order to complete the octet?
D. In a covalent bond, atoms will _____________ electrons so that the octet is filled.
E. Covalent Bond – A bond formed by the sharing of electrons between atoms – usually non-metals.
F. For example, ______________has 6 valence electrons and ____________________ has 7.
Notes
Objective 15 - Use classical models of the atom and Lewis dot structures to explain
Covalent bonding.
Example 1 - Hydrogen has 1 valence electron and Fluorine has 7 valence electrons.
Classical model
Lewis dot structure
H
F
H
F
A. In order for these elements to be stable, they both must gain electrons – but neither of them
is willing to give up any electrons.
B. Since both Hydrogen and Fluorine need 1 electron, they can each share 1 electron.
C. When this happens, Hydrogen and Fluorine will form a covalent bond – electrons are shared
Example 2 – Hydrogen and Oxygen
Classical model
H
O
Lewis dot structure
H
O
Formula =
Objective 16 - Define Lone pair electrons, unpaired electrons, and how they
influence covalent bonding.
A. Lone pair electrons – valence electrons that are paired (2).
B. Unpaired electrons – valence electrons that are not paired (2)
C. Lone pair electrons ___________________form covalent bonds *
D. Unpaired electrons _______________ form covalent bonds
Examples
H
Unpaired electrons =
Lone pair electrons =
F
O
N
Unpaired electrons =
Lone pair electrons =
Unpaired electrons =
Lone pair electrons =
Unpaired electrons =
Lone pair electrons =
Objective 17 - Identify the 3 kinds of covalent bonds
A. We will study 3 kinds of covalent bonds.
1. Single bonds – 1 covalent bond between atoms
2. Double bonds – 2 covalent bonds between atoms
3. Triple bonds – 3 covalent bonds between atoms
Objective 18 - Identify the 2 ways of drawing covalent bonds
A. Lewis dot structures – dots represent valence electrons.
B. Stick drawings – sticks represent covalent bonds involving 2 shared electrons.
Questions 
1. What is a lone pair electron? _________________________________________________
2. What is an unpaired electron? ______________________________________________
3. What are the 3 kinds of covalent bonds? _______________________________________
4. Hydrogen is in group one. What other group could it be placed in? __________________
5. How many valence electrons will cause Hydrogen to become stable? ________________
Objective 19 - Draw individual elements with proper Lewis dot structures and stick drawings.
**Important Fact: Non-metals will always have the same number of sticks as unpaired electrons.
Section A
Non metal
element
1. Fluorine
2.
Bromine
3.. Sulfur
4.
Tellurium
5.
Arsenic
6.
Carbon
7.
Nitrogen
8.
Silicon
Lewis dot structure
Valence
electrons
Unpaired
electrons
Stick drawing
Objective 20 - Draw single covalent bonds with proper Lewis dot structures and stick drawings.
1.
Lewis dot structure
H
Lewis dot structure
F
Unpaired =
2.
Unpaired =
H
3.
Unpaired =
H
4.
Unpaired =
H
Cl
Unpaired =
O
Unpaired =
S
Unpaired =
5.
Unpaired =
H
6.
Unpaired =
H
7.
Unpaired =
H
H
Unpaired =
Unpaired =
N
Unpaired =
P
Unpaired =
Covalent bond (Lewis)
Stick drawing
8.
C
H
9.
Unpaired =
S
Unpaired =
Cl
Unpaired =
10. S
Unpaired =
F
Unpaired =
11. N
Unpaired =
F
Unpaired =
Unpaired =
12. P
Unpaired =
Cl
Unpaired =
 Questions
1. What is a covalent Bond? _____________________________________________________________
2. What family of elements are usually involved in a covalent bond? _______________________________
3. How is a covalent bond different from an ionic bond?
__________________________________________________________________________________
4. What does 1 stick represent in a stick drawing? ____________________________________________
5. How many electrons are involved in a single covalent bond? _______
6. How many electrons does phosphorus need to complete its octet? ________
7. How many sticks must be drawn on a phosphorus atom? _______
Objective 21 - Draw double covalent bonds with proper Lewis dot structures and
stick drawings.
A. Remember – covalent bonds share electrons – they do not give and take like ionic bonds.
B. Also remember that unpaired electrons will form covalent bonds.
1.
Lewis dot structure
O
Lewis dot structure
O
2.
Unpaired =
O
Unpaired =
S
3.
Unpaired =
C
Unpaired =
O
4.
Unpaired =
C
Unpaired =
S
5.
Unpaired =
C
Unpaired =
Se
6.
Unpaired =
S
Unpaired =
S
7.
Unpaired =
Si
Unpaired =
Te
8.
Unpaired =
Si
Unpaired =
O
Unpaired =
Unpaired =
Covalent bond
Stick drawing
Objective 22 - Draw Triple covalent bonds with proper Lewis dot structures and
stick drawings.
1.
Lewis dot
structure
N
Lewis dot
structure
N
2.
P
N
3.
As
P
Covalent bond
Stick drawing
Objective 23 – Compare and Contrast ionic bonds and covalent bonds.
A. How are they alike?
________________________________________________________________________
B. How are they different?
________________________________________________________________________
Part D – Metallic Bonding
Metallic Bond
Stainless Steel
Bronze
Malleable
Ductile
Alloy
Objective 24 - Define metallic bonding, explain how it works, and give examples
A. Ionic bonding occurs between metals _______________________________.
B. Metals ____ bond with other metals – this is called metallic bonding
C. Metallic bond – bond between 2 or more metals.
D. What causes metals to bond if they are all positively charged atoms – like charges repel!
E. Metallic bonding occurs as the ________________________of free floating valence
electrons for the positively charged nuclei.
F. Aluminum is used for many products such as ________. What holds the aluminum atoms
together? metallic bonds
Objective 25 - Define alloys, indicate reasons for creating alloys, and give examples
A. Alloy - mixture of 2 or more metals
B. For example: Stainless steel is a mixture of Iron, Cromium, Carbon, and Nickel. Also notice
that ____________ is not on the periodic table – steel is an alloy.
C. Chemists create alloys because their ________________ are often superior to those of their
component elements.
D. Example 1: ___________________ (Cu) is soft and malleable while __________ (Sn) is
hard and sturdy. If you mix copper and tin, you get an alloy that is hard and malleable.
E. An alloy of copper and tin is known as _______________.
F. Example 2. _____________ (Au) is a soft metal that is very shiny. People like to wear gold
jewelry because it is very shiny. However, Gold is too soft to hold its shape and can bend
easily like a wire. Gold is therefore sold as alloys of other metals to give it more strength.
Objective 26 - Describe properties of metals and alloys
A. Strong conductors of electricity
B. Strong conductors of heat
C. Malleable
D. Ductile
 Questions
1. What is a metallic bond? ____________________________________________________
2. What holds metals together since they are all positively charged?
___________________________________________________________________________
3. What is an alloy? ___________________________________________________________
4. Give an example of an alloy. _________________________
5. List 3 properties of metals and alloys.
______________________________
______________________________
______________________________