10 points HW assignment 6 Chem 1211 Dr.Stroeva
✓ Complete assignment in pen or pencil in clear, neat, readable manner.
✓ Scan and combine all pages in one PDF file. (Use GSU library facilities for printing
scanning works if required)
✓ Submit via iCollege before 11/07 at 11:59 PM.
✓ No late submissions are accepted.
Module 3: Covered concepts 3.6-3.8
Part 1. Covalent Bonding (Video presentations and PPt unit 9 parts 9.4-9.5 )
By completion of this assignment, you will be able:
• Define Covalent bonding vs. Ionic bonding.
• Know and understand lone pairs and bonding pairs.
• Know and understand Bonding pairs vs. bonding groups.
• Know and understand Bond polarity.
• Know and understand dipole moment and bond polarity.
The sharing of valence electrons is called covalent bonding or __________ ____________.
Electrons that are not shared by atoms but belong to a ___________ atom are called _______ pairs.
Designate all lone pairs and all bonding pairs for sulfur
dioxide.
Single bonding is when ____________ electron pair is shared.
Double bonding is when ____________ electron pairs are shared.
Triple bonding is when ____________ electron pairs are shared.
Single bonding is _______ bonding group. Double bonding is _______ bonding group. Triple
bonding is _______ bonding group.
The single bond is the longest and __________. The triple bond is the shortest and ___________.
The result of unequal sharing of electrons in between two atoms is a _________covalent bond.
The larger the difference in electronegativity, the _________ ____________ bond.
1
, 10 points HW assignment 6 Chem 1211 Dr.Stroeva
Dipole moment, μ, is a measure of bond _____________. The end with the larger electron density
gets a partial ____________ charge. The end that is electron deficient gets a partial _____________
charge.
➢ Complete the table below:
Note! The only pure covalent bond does not have clearly separated partial charges. Non-polar and polar covalent
bonds have partial charges on bonded atoms.
Bond Polarity Partial charge on the atom
H-N N
N-O O
O-H H
C-H H
H-F H
S-O S
C-O C
H-S S
O-F O
B-C C
Part 2. Covalent Compounds. Lewis Dot Structures. Formal Charge (Video presentations
and PPt unit 9 parts 9.6-9.7 )
By completion of this assignment, you will be able:
Know and understand the general approach in creating Lewis’s Dot structures.
Be able to find formal charge and prove correct Lewis’s dot structures.
Exceptions in octet rule
The algorithm in creating a Lewis’s dot structure:
1. Count total amount of ____________ ____________ of all atoms in the molecule (compound).
2. Choose ________ _____________. The central atom is the atom of an element with the
_____________electronegativity. Exception: ________ atom cannot be the central atom because
it needs only 2 electrons for the completed electron configuration.
3. Put ____________ atoms around the central atom and connect them to the central atom with
_______________ of electrons.
4. Add electrons to atoms of the most ________________ elements in order to satisfy the
_______________rule.
5. Add remaining electrons to the _____________ atom.
2
✓ Complete assignment in pen or pencil in clear, neat, readable manner.
✓ Scan and combine all pages in one PDF file. (Use GSU library facilities for printing
scanning works if required)
✓ Submit via iCollege before 11/07 at 11:59 PM.
✓ No late submissions are accepted.
Module 3: Covered concepts 3.6-3.8
Part 1. Covalent Bonding (Video presentations and PPt unit 9 parts 9.4-9.5 )
By completion of this assignment, you will be able:
• Define Covalent bonding vs. Ionic bonding.
• Know and understand lone pairs and bonding pairs.
• Know and understand Bonding pairs vs. bonding groups.
• Know and understand Bond polarity.
• Know and understand dipole moment and bond polarity.
The sharing of valence electrons is called covalent bonding or __________ ____________.
Electrons that are not shared by atoms but belong to a ___________ atom are called _______ pairs.
Designate all lone pairs and all bonding pairs for sulfur
dioxide.
Single bonding is when ____________ electron pair is shared.
Double bonding is when ____________ electron pairs are shared.
Triple bonding is when ____________ electron pairs are shared.
Single bonding is _______ bonding group. Double bonding is _______ bonding group. Triple
bonding is _______ bonding group.
The single bond is the longest and __________. The triple bond is the shortest and ___________.
The result of unequal sharing of electrons in between two atoms is a _________covalent bond.
The larger the difference in electronegativity, the _________ ____________ bond.
1
, 10 points HW assignment 6 Chem 1211 Dr.Stroeva
Dipole moment, μ, is a measure of bond _____________. The end with the larger electron density
gets a partial ____________ charge. The end that is electron deficient gets a partial _____________
charge.
➢ Complete the table below:
Note! The only pure covalent bond does not have clearly separated partial charges. Non-polar and polar covalent
bonds have partial charges on bonded atoms.
Bond Polarity Partial charge on the atom
H-N N
N-O O
O-H H
C-H H
H-F H
S-O S
C-O C
H-S S
O-F O
B-C C
Part 2. Covalent Compounds. Lewis Dot Structures. Formal Charge (Video presentations
and PPt unit 9 parts 9.6-9.7 )
By completion of this assignment, you will be able:
Know and understand the general approach in creating Lewis’s Dot structures.
Be able to find formal charge and prove correct Lewis’s dot structures.
Exceptions in octet rule
The algorithm in creating a Lewis’s dot structure:
1. Count total amount of ____________ ____________ of all atoms in the molecule (compound).
2. Choose ________ _____________. The central atom is the atom of an element with the
_____________electronegativity. Exception: ________ atom cannot be the central atom because
it needs only 2 electrons for the completed electron configuration.
3. Put ____________ atoms around the central atom and connect them to the central atom with
_______________ of electrons.
4. Add electrons to atoms of the most ________________ elements in order to satisfy the
_______________rule.
5. Add remaining electrons to the _____________ atom.
2
