APPLIED CHEMISTRY
CHEMICAL BONDS
P.A. STATE STANDARDS:
CHEM.A.1.1.4 Relate the physical properties of matter to its atomic or molecular structure.
CHEM.A.1.2.1 Compare properties of solutions containing ionic or molecular solutes (e.g., dissolving, dissociating).
CHEM.A.1.2.3 Describe how factors (e.g., temperature, concentration, surface area) can affect solubility.
CHEM.A.1.2.4 Describe various ways that concentration can be expressed and calculated (e.g., molarity, percent by mass, percent by volume).
CHEM.A.1.2.5 Describe how chemical bonding can affect whether a substance dissolves in a given liquid.
CHEM.B.1.3.2 Classify a bond as being polar covalent, non‐polar covalent, or ionic.
CHEM.B.1.3.3 Use illustrations to predict the polarity of a molecule.
CHEM.B.1.4.1 Recognize and describe different types of models that can be used to illustrate the bonds that hold atoms together in a compound
(e.g., computer models, ball‐and‐stick models, graphical models, solid‐sphere models, structural formulas, skeletal formulas, Lewis dot structures).
CHEM.B.1.4.2 Utilize Lewis dot structures to predict the structure and bonding in simple compounds.
OBJECTIVES


























State the octet rule
Define ion, monatomic ion, polyatomic ion, cation and anion
Name anions and cations
Illustrate how ionic bonds form
Define ionic and covalent bonds
Determine the empirical formula of an ionic compound
Describe the properties of ionic compounds
Explain the dissociation of ionic compounds
Define molecule, molecular substance, molecular formula and structural formula
Draw Lewis Structures for molecular compounds
Define and identify single, double and triple covalent bonds
Students will state VSEPR Theory
Students will determine the molecular geometry of molecules
Students will state the number of bonds and lone pairs associated with each molecular shape
Students will state the bond angle associated with each molecular shape
Students will describe general trends in bond length
Describe and identify exceptions to the octet rule
Describe the properties of covalent compounds
State the reality of bonding.
Describe periodic trends in electronegativity and use periodic table to determine an element’s electronegativity.
Explain the shielding effect.
Calculate EN
Use EN to determine if a bond is ionic, polar covalent or nonpolar covalent.
Label dipoles using both vectors and the symbols - and +
Distinguish between the properties of ionic bonds, polar covalent bonds and nonpolar covalent bonds.
Use Lewis Structures and Molecular Geometries to determine the polarity of a molecule.
APPLIED CHEMISTRY
CHEMICAL BONDING
DAILY PLANNER
DAY
1
Fri., 3/15
2 and 3
CLASSWORK
Intro to Ionic & Covalent Bonding WebTutorial (10 Points)
Properties of Ionic vs. Covalent Compounds
(25 Points)
4
5
6
7
8
9
10
11
12
13
14
15
Tent. Fri, 4/5
HOMEWORK
Finish today’s Review Sheet
Finish for Homework
Finish Lab
Define Vocabulary Terms
Notes: Ionic Bonding
Notes: Metallic Bonding
Alloy Lab (10 Points)
Notes: Covalent Bonding, Lewis Structures
Notes: N-A method for Lewis Structures
Start Molecular Modeling Activity (Draw the Lewis
Structures)
Molecular Modeling Lab (15 Points)
Finish Vocabulary Term Definitions
Notes: VSEPR Theory
Continue Working on Molecular Modeling Lab
Notes: EN and Types of Bonds
Finish Molecular Modeling Lab
HW5: Worksheet E
HW6: Worksheet F
Notes: Polarity of Molecules/Intermolecular Forces
Homework & Extra Credit Due (25 Points +)
Begin Polarity Lab
Go over Homework & Extra Credit
Complete Polarity Lab (25 Points)
Bonding Test (100 Points)
HW7: Worksheet G
Work on Polarity Lab
HW1: Worksheet A
HW2: Worksheet B
HW3: Worksheet C
HW4: Worksheet D
Finish today’s lab
Finish today’s lab
Top Pairs for the Periodic Trends Unit:
Period 1: Amber Grace & Kennymac Durante
Period 2: Luke Miller & Jordan Rodriguez
HOMEWORK GRADE
EXTRA CREDIT
A
35/35
B
32/25
C
29/35
D
25/35
F
22/35
No Grade
0/35
4 Points: Worksheet H
3 Points: Worksheet I
5 Points: Create a poster
illustrating 5 different metals and
their crystal structures.
8 Points: Write a 3 page essay
detailing the importance of water
in our lives.
7/7
Homeworks Complete
6/7
Homeworks Complete
5/7
Homeworks Complete
4/7
Homeworks Complete
3.5/7
Homeworks Complete
Less than ½ of
Homework Complete
(<3.5/7)
VOCABULARY TERMS
Allotrope:
Alloy:
Anion:
Ball-and-Stick Model:
Bond Angle:
Cation:
Compound:
Covalent Bond:
Covalent-Network Solid:
Crystalline Solid:
Diamond:
Dipole:
Dipole-dipole force:
Dispersion Force:
Double-Covalent Bond:
Electronegativity:
Graphite:
Hydrogen Bond:
Intermolecular Force:
Intramolecular Force:
Ion:
Ionic Bond:
Ionic Compound:
Lewis Structure:
Molecular Substance:
Molecule:
Nonpolar:
Octet Rule:
Polar:
Single-Covalent Bond:
Structural Formula:
Structural Isomer:
Triple Covalent Bond:
Unshared Pair:
Valence Electron:
VSEPR Theory:
The OCTET RULE states that atoms tend to gain, lose or share electrons in order to acquire a full set of valence electrons. For most elements, this
is _____________ valence electrons.

However, Hydrogen & Helium only require _____________________ valence electrons.

Therefore, the elements are all trying to be like the Group 18 elements, the ________________________________________.

Atoms form ________________________________________________________ to become stable.
There are 3 main types of chemical bonds:
1)
2)
3)
Important Definitions
Ion:
Ionic Compound:
Ionic Bond:
Empirical Formula:
Types of Elements in an Ionic Compound:
How do ionic bonds form?
Using Lewis Dot Diagrams to determine the Empirical Formula of an Ionic Compound:
1) Draw the Lewis Dot Diagrams for each element
2) Use arrows to show the transfer of electrons between atoms
Practice Problems:
1) Show how an ionic bond forms between sodium and oxygen. What is the empirical formula of this compound?
2) Use Lewis Dot Diagrams to determine the empirical formula of the ionic compound formed between aluminum and sulfur.
Properties of Ionic Compounds:
Definition:
Types of Elements in a Metallic Bond:
How do Metallic Bonds Form?
Properties of Metallic Bonds (Metals):
1.
Malleable:
2.
Ductile:
3.
Conductivity:
4.
Interparticle Forces:
5.
Other Properties:
Practice Problems
_____ 1. Metals are good conductors of electricity because they
a. form crystal lattice
b. contain positive ions
c. contain mobile valence electrons
d. form ionic bonds
_____ 2. A metallic bond is a bond between
a.
valence electrons and positively charged metal ions
b. the ions of two different metals
c.
a metal and nonmetal
d. none of the above
Important Definitions
Covalent Bond:
Molecular (Covalent) Compound:
Molecule:
Types of Elements in a Molecular Compound:
How do covalent bonds form?
Properties of Covalent (Molecular Compounds):
Important Definitions
Structural Formula:
Lewis Structure:
Based On:
Dash:
Single Covalent Bond ():
Double Covalent Bond ():
Triple Covalent Bond ():
Lone Pair ():
There are 2 ways to determine the Lewis Structure for a Molecular Compound
1) Using Lewis Dot Diagrams (works 95% of the time).
Practice Problems:
1) Draw the Lewis Structure for F2.
2) Draw the Lewis Structure for CH4.
3) Draw the Lewis Structure for O2.
2) The mathematical way to determine the Lewis Structure of a Compound (Works all the time)
N-A = # of bonds
2
N = # of electrons needed to be stable
Most elements need 8 electrons
H and He need 2 electrons
A = # of valence electrons available
N-A = The number of electrons that need to be shared between the atoms
*You divide this number by two to determine the # of bonds since each bond consists of 2 electrons
Practice Problems:
Draw the Lewis Structures for the following compounds:
1) NH3
b) Cl2
c) CF4
d) H2CO
f) NH4+
e) C2H2
Resonance Structures:
Example: Draw the Resonance Structures of Ozone (O3)
Coordinate Covalent Bond:
Exceptions to the Octet Rule:
1) Atoms with Less than an Octet
2) Atoms with More than an Octet
3) Molecules with Odd Numbers of Electrons
Important Definitions
VSEPR Theory:
Ball-and-Stick Model:
Bond Angles:
Molecular Shapes are on the back of your periodic tables
Practice Problems:
For each of the following molecules, draw the Lewis Structure, determine the appropriate shape and then draw the ball-and-stick model of the
molecule.
1) CO2
b) PF3
c) CBr4
Lewis Structure:
Lewis Structure:
Lewis Structure:
Molecular Shape:
Molecular Shape:
Molecular Shape:
Ball-and-Stick Model
Ball-and-Stick Model:
Ball-and-Stick Model:
Electronegativity:
The difference between two atoms electronegativities determines the type of bond formed between those two atoms
EN = EN1 –EN2
 is the Greek letter _____________________ and means __________________________
EN is always a ____________________________ number
Example: Calculate the EN between cesium and fluorine.
You can think of bonding as a __________________________________________________________ for __________________________
between atoms.
Ionic Bond:
EN is ____________________________________________________________________
Nonpolar Covalent Bond:
EN is __________________________________________________________________
Polar Covalent Bond:
EN is between ___________________________ & _____________________________
EN CHART
Practice Problems: Identify each of the following bonds as either IONIC, POLAR COVALENT, or NONPOLAR COVALENT
a) C-O
b) C-H
c) I-I
d) P-I
Polar bonds have ________________________________________________________ atoms due to the _________________________ sharing of
electrons.
Dipoles:
:
Two ways to label the dipoles (partial charges) on a polar bond.
1) Vectors
2) -and +
Example: Label the dipoles on a C-Cl bond.
To Determine the Polarity of an entire Molecule:
1) Draw the Lewis Structure of the Molecule
2) Determine the Molecular Geometry of the Molecule
3) Determine they types of bonds in the Molecule (do EN for each bond in the molecule)
 If you find a polar bond and the geometry is trigonal planar, trigonal pyramidal or bent or unsymmetrical: the molecule is Polar
 If you find polar bonds but it is completely symmetrical tetrahedral or linear: the polar bonds cancel each other out and the molecule is
NONPOLAR
PRACTICE PROBLEMS:
Determine whether each of the following compounds is IONIC, POLAR COVALENT or NONPOLAR COVALENT
a) CO2
b) NH3
c) H2O
WORKSHEET A
A. Using Lewis Dot Diagrams or charges, illustrate how the following elements form ionic compounds
1. KBr
2. Sodium & Nitrogen
3. Ca & P
4. Magnesium and Oxygen
5. AlN
6 Lithium and Sulfur
7. Barium and Chlorine
8. CaS
9. Zn and Cl
B. Write the chemical formulas for each of the following binary ionic compounds. You may use the crisscross method or
you may draw the Lewis Structures to determine the formulas!
1. sodium nitride
______________________
6. Aluminum fluoride
______________________
2. lead (IV) iodide
______________________
7. Tin (IV) bromide
______________________
3. strontium oxide
______________________
8. Manganese (IV) oxide______________________
WORKSHEET B
True/False
_____ 1. Metals that are good conductors of electricity are said to be ductile.
_____ 2. Drifting valence electrons insulate cations from one another and contribute to the malleability of a metal
_____ 3. Metals are good conductors of electricity because electrons flow freely in them.
_____ 4. Most of the metals you encounter on a daily basis are in their pure elemental form.
_____ 5. Metals are crystalline.
MATCHING
_____ 6. Ductile
A. The attraction of valence electrons for positive metal ions
_____ 7. Metallic Bonds
B. A negatively charged ion
_____ 8. Ionic Bonds
C. Electrons in the outermost energy level
_____ 9. Malleable
D. A solid in which the atoms, ions or molecules are arranged in an orderly, repeating, 3dimensional pattern
_____ 10. Anion
E. A mixture of 2 or more elements, at least one of which is a metal
_____ 11. Cation
F. A depiction of valence electrons around the symbol of an element
_____ 12. Alloy
G. Can be drawn into wires
_____ 13. Crystalline Solid
H. The electrostatic attraction that binds oppositely charged ions together
_____ 14. Lewis Dot Diagram
I. Atoms typically require 8 valence electrons to be stable
_____ 15. Valence Electron
J. Can be hammered or forced into shapes
_____ 16. Octet Rule
K. A positively charged ion
MULTIPLE CHOICE
_____ 17. Ionic bonds typically form between
a. members of the same family
b. a metal and a nonmetal
c. all nonmetals
d. all metals
_____ 18. Metals are good conductors of electricity because they
a. form crystal lattice
b. contain positive ions
c. contain mobile valence electrons
d. form ionic bonds
_____ 19. An ionic compound is
a. electrically neutral
b. composed of anions and cations
c. held together by ionic bonds
d. all of the above
_____ 20. A metallic bond is a bond between
a.
valence electrons and positively charged metal ions
b.
the ions of two different metals
c.
a metal and nonmetal
d.
none of the above
_____ 21. Which element when combined with chlorine would most likely form an ionic compound?
a. lithium
b. carbon
c. phosphorus
d. bromine
WORKSHEET C
A. Determine which of the following compounds contain covalent bonds. Circle all of the compounds that contain only
covalent bonds.
KCl
C6H8O6
HNO3
Mg3N2
LiClO4
Br2
N2H4
B. MULTIPLE CHOICE
_____ 1. A group of atoms united by covalent bonds is a(n)
a) cation
b) ionic compound
c) molecule
d) octet
c) inner-level electrons
d) valence electrons
_____ 2. To form a bond, atoms share
a) neutrons
b) protons
_____ 3. Molecular compounds
a) have high melting points
b) are good conductors in their liquid state
c) have weak interparticle forces
d) are crystalline solids
_____ 4. Which of the following compounds is formed through the sharing of electrons?
a) CH4
b) CaCl2
c) MgF
d) Al2O3
_____ 5. What type of bond exists in O2 molecule?
a) an ionic bond
b) a metallic bond
c) a single covalent bond
d) a double covalent bond
C. Draw Lewis Structures for the following covalently bonded compounds.
a. HCl
b. CCl4
c. Cl2O
WORKSHEET D
A. Draw Lewis Structures for the following covalently bonded compounds.
a. HCl
b. CCl4
c. Cl2O
d. I2
e. H2O
f. PI3
g. C2H4
h. N2
i. CH4
j. HCN
k. H2S
l. SCl2
m. C2H2
n. CCl2Br2
o. NF3
A. Determine which of the following compounds contain covalent bonds. Circle the compounds that contain only covalent bonds.
KCl
C6H8O6
HNO3
Mg3N2
LiClO4
Br2
N2H4
WORKSHEET E
A. On the line at the left, write the term from the list that matches each description below.
Trigonal planar
VSEPR theory
ball-and-stick model
symmetry
Unshared pair
bond angle
hybrid orbital
___________________________ 1. a visual model of molecular geometry
___________________________ 2. the geometric angle between two adjacent bonds
___________________________ 3. a pair of valence electrons not involved in a bond
___________________________ 4. the theory that states that the pairs of valence electrons are
arranged as far apart as possible in small molecules.
___________________________ 5. name for a triangular flat molecule
B. For each of the following compounds:
1) Draw the Lewis Structure.
2) Determine the geometry of the molecules.
3) Draw the ball-and-stick model with the proper geometry
1. PCl3
2. H2S
3. CBr4
4. CO
WORKSHEET F
A. Find the electronegativity difference between each of the following pairs of elements and to predict the kind
of bond that will be formed.
Element Pairs
Electronegativity Difference
Type of Bond
calcium and fluorine
carbon and silicon
beryllium and sulfur
hydrogen and germanium
zinc and bromine
B. MULTIPLE CHOICE
Write the letter of the correct answer on the line. If you do not write the letter on the line, I will not count it as
complete!
____1. An atom of which element has the greatest attraction for the electrons in a bond with a hydrogen atom?
a) chlorine
b) silicon
c) phosphorus
d) sulfur
____2. When the atoms within molecules have different electronegativities, the electrons are shared unequally
and the bonds are
a) nonpolar
b) ionic
c) polar
d) metallic
____ 3. What is the electronegativity difference between carbon and oxygen?
a) 1
b) 2
c) 3
d) 0
____ 4. Which of the following elements is the most electronegative?
a) aluminum
b) arsenic
c) nitrogen
d) fluorine
____ 5. Which element is more likely to give up an electron?
a) radium
b) bromine
c) gold
d) phosphorus
____ 6. What kind of bond forms between sulfur and fluorine?
a) nonpolar
b) ionic
c) polar
d) metallic
c) chlorine
d) fluorine
____ 7. Which element has the highest electronegativity?
a) bromine
b) oxygen
WORKSHEET G
A. The line below represents the range of differences in electronegativity that are possible between any two elements in
the periodic table. The smallest difference is represented by the left end of the line, and the greatest difference by the right
end of the line. In the space at the left below, write the letter of the labeled parts from this line that corresponds to the
descriptions. Some of the letters may be used more than once.
a
0.0
b
c d
0.4
1.0
1.5
e
f
2.0
2.5
g
3.0
1. ______ The lowest possible value of EN.
2. ______ The bond of greatest possible ionic character.
3. ______ A pure nonpolar covalent bond
4. ______ A polar covalent bond
5. ______ An ionic bond that would form between calcium and oxygen
6. ______ The bond in a diatomic molecule of an element
7. ______ A bond that is classified as nonpolar but that has a slight polarity
8. ______ The division between nonpolar covalent and polar covalent bonds
9. ______ A bond that would form between cesium and fluorine
10. ______ The division between ionic and polar covalent bonds
B. Illustrate the molecular shape of each of the following molecules. Identify each molecule as polar or nonpolar.
1) BFI2
2) NH2Cl
3) SCl2
4) CO2
5) CF4
6) NF3
REVIEW WORKSHEET
Bond Type
Representative
Unit
Metallic
Ionic
Polar Covalent
Nonpolar
Covalent
PRACTICE PROBLEMS
Bond
Formation
COMPARISON OF BONDS
Type of
Physical State
Elements
Melting Point
Solubility in
Water
Electrical
Conductivity
in Water
A. Predict the type of chemical bond (metallic, covalent, or ionic) you would expect for each of the following materials.
1. A material used in making electrical transmission wire.
_____________________________________
2. A material used to make the insulation wrapped around transmission lines that lie on the ocean floor.
______________________________________________
3. A material used as a lubricating oil.
______________________________________________
4. A material that is dissolved in large quantities in sea water.
_______________________________________
5. A material used to make high-temperature furnaces.
_______________________________________
6. A material used in the manufacture of wires in suspension bridges.
_________________________________
7. A material used to make cans.
__________________________________
8. A material used as a gaseous propellant in spray cans, such as deodorant or shaving cream dispensers.
_____________________________________________
9. A material that evaporates readily at room temperature.
_________________________________
10. A material that is a good conductor when melted but a poor conductor when solid._________________________
WORKSHEET H—EXTRA CREDIT
_____ 1. Which list of formulas represents compounds only?
A) CO2, H2O, NH3
B) H2, Ne, NaCl
C) H2, N2, O2
D) MgO, NaCl, O2
_____ 2. Which property could be used to identify a compound in the laboratory?
A) mass
B) temperature
C) melting point
D) volume
_____ 3. Given a formula for oxygen:
O=O
What is the total number of electrons shared between the atoms represented in this formula?
A) 1
B) 8
C) 2
D) 4
_____ 4. Which substance can not be decomposed by a chemical change?
A) AlCl3
B) HI
C) H2O
D) Cu
_____ 5. An atom in the ground state has seven valence electrons. This atom could be an atom of which
element?
A) calcium
B) oxygen
C) fluorine
_____ 6. As a bond between a hydrogen atom and a sulfur atom is formed, electrons are
D) sodium
A) shared to form an ionic bond
B) shared to form a covalent bond
C) transferred to form an ionic bond
D) transferred to form a covalent bond
_____ 7. A barium atom attains a stable electron configuration when it bonds with
A) one chlorine atom
B) two chlorine atoms
C) one sodium atom
D) two sodium atoms
_____ 8. Sodium atoms, potassium atoms, and cesium atoms have the same
A) atomic radius
B) first ionization energy
C) total number of protons
D) oxidation state
_____ 9. When sodium and fluorine combine to produce the compound NaF, the ions formed have the same electron configuration as
atoms of
A) argon, only
B) neon, only
C) both argon and neon
D) neither argon nor neon
_____ 10. Matter that is composed of two or more different elements chemically combined in a fixed
proportion is classified as
A) a compound
B) a mixture
C) an isotope
D) a solution
C) CH4
D) NH4Cl
_____ 11. Which formula represents an ionic compound?
A) H2
B) CH3OH
_____ 12. What is the total number of different elements present in NH4NO3?
A) 7
B) 3
C) 9
WORKSHEET I—EXTRA CREDIT
1. Define electronegativity:
2. Define polar covalent bond:
3. How does a metallic bond form?
4. What geometric shape do all diatomic molecules have?
D) 4
5. List 3 properties of ionic compounds.
6. Classify the following bonds as either Ionic (I), Nonpolar Covalent (NP), Polar Covalent (P) or Metallic (M).
______ Ni-Cl
_____ C-Br
_____ Fe
______ Fe-Fe
_____ Be-F
_____ Si-O
7. What does VSEPR Theory state?
8. Why are electrons sometimes shared unequally?
9. Why do polar molecules form puddles?