Thursday Oct 8 Naming acids
Fri Oct 9 Naming Covalent compounds
Mon Oct 12 Ionic vs. covalent lab
Venn Ionic vs. Cov.
Tues Oct 13 Quiz over acids & covalent compounds / Dot diagrams
Wed Oct 14 PSAT for all 10th grade (11th grade report to Mrs Jones)
VSEPR theory minilab
Thurs Oct 15 continue Minilab – polar vs. nonpolar / Work time
Fri Oct 16 workday
Monday Oct 19 Review
Tuesday Oct 20 TEST – NB check
Georgia Performance Standard:
SC1 d – Name and write formulas for covalent compounds and acids.
SC3 e – Compare and contrast types of chemical bonds. (Ionic & covalent)
Why are valence electrons related to the nature of
the chemical bond?
KQ - How does an ionic bond compare to a covalent bond?
KQ - How do you use electronegativity values to determine
polarity?
Notebook check:
Vocabulary
Covalent / Acid handout
Venn diagram
Notes on VSEPR
Model Minilab (chart)
Virtual minilab
Answer Learning targets
Vocabulary you should know:
Chemical Bond
Valence electron (trend)
Ionic bond
Covalent bond
Nonpolar covalent bond
Polar covalent bond
VSEPR theory
electronegativity
single, double & triple bond
formula unit
molecule
Study Guide (Learning targets)
At the end of this unit, you should be able to…
BONDING
1) Explain what chemical bonds are and why they form.
2) Define electronegativity and use electronegativity values to determine bond types.
3) Compare and contrast ionic, polar covalent and nonpolar covalent bonds in terms of their electronegativity
differences, properties, behaviors, etc.
4) Identify the typical characteristics of substances containing ionic, covalent and metallic bonds (melting point,
structure, physical properties, etc.)
5) Identify the number of valence electrons in an atom based on its location on the periodic table. Draw a dot
diagram for an element to illustrate the number of valence electrons it has.
6) Create Lewis structures for molecules and polyatomic ions containing single, double, and triple bonds.
7) Predict the shapes of molecules and polyatomic ions using VSEPR theory.
Great video review for ionic bonding: (6 min)
http://www.nbclearn.com/chemistrynow/cuecard/56354
Tutorial on covalent bonding:
http://www.brightstorm.com/science/chemistry/chemical-bonds/covalent-bonds/
Naming acids tutorial:
http://www.brightstorm.com/science/chemistry/acids-and-bases/naming-acids/
Acid nomenclature:
Acids formulas begin with _________________ . Acids are usually covalent compounds but are treated
as cation/anion combinations. Name them as an ionic compound and then apply the acid rules.
Acid rules: ________________
________________
________________
Name
1) H2SO4 _____________________
2) HBr ________________________
3) HNO2 _______________________
4) HI __________________________
5) H2S _________________________
6) H2CO3 ______________________
7) HClO2 _______________________
8) HClO3 _______________________
9) H2Cr2O7 ____________________
10)
H3PO3 ______________________
11)
Hydrofluoric acid ______________
12)
Hydrochloric acid ______________
13)
Hydronitric acid _______________
14)
Sulfurous acid _________________
15)
Nitric acid ____________________
16)
Acetic acid ___________________
17)
Phosphoric acid _______________
18)
Hydrocyanic acid ______________
19)
Chromic acid __________________
20)
Perchloric acid _________________
Covalent compounds:
 Electrons are ________________ so no _________ result.
 Form between 2 __________________.
 Use _________________ to tell the number of _______ in the compound.
Greek Prefixes: _______, _________,________,_______, _________,
_______,_________,_________,_______,_________
Naming Covalent Compounds Practice
Write the formulas for the following covalent compounds:
1)
Nigrogen tribromide __________________________________
2)
hexaboron selenide __________________________________
3)
chlorine dioxide __________________________________
4)
hydrogen iodide __________________________________
5)
iodine pentafluoride __________________________________
6)
dinitrogen trioxide __________________________________
7)
Nitrogen trihydride__________________________________
8)
phosphorus triiodide __________________________________
9)
carbon monoxide ___________________________________
Write the names for the following covalent compounds:
10)
P4S5 __________________________________
11)
CO2 __________________________________
12)
SeF6 __________________________________
13)
Si2Br6 __________________________________
14)
SCl4 __________________________________
15)
CF4 __________________________________
16)
SiO2__________________________________
17)
NF3 __________________________________
Unit 6: Predicting Shapes of Covalent Compounds
Now that you know how to draw the Lewis dot structures of covalent compounds, you can now use
these structures to determine the three dimensional shapes of molecules.
VSEPR Theory: (Valence Shell Electron Pair Repulsion theory)
1. Electrons all have a ____________ charge and like charges _________________.
2. In molecules, bonding pairs and non-bonding pairs (called __________ pairs) repel
each other to the greatest possible extent.
3. The repulsion of the like charges gives the molecule a 3-D ________________ that
depends on the numbers of _______________ and ___________ pairs.
4. Even though double and triple bonds have more than 1 __________ of electrons in the
same region, they will respond to the repulsive effects as a ______________ unit (just like
a single bond).
5
Shapes obtained for molecules with:
1)
4 bonding regions:
2)
3 bonding regions + 1 lone pair:
3)
3 bonding regions, 0 lone pair:
4)
2 bonding regions, 2 lone pair:
5)
2 bonding regions, 2 lone pair:
Formula
Lewis Diagram
HCl
HBr
H2O
CH4
CO2
H2CO
NH3
Hard ones to try: HCOOH, CH3NH2, C2H4
Structural Formula
Shape
Polarity
Building and Naming Molecules
Learning Targets: I can name a covalent compound, given its formula. I can write the formula of a covalent
compound, given its name.






Open the http://phet.colorado.edu/
Click the “Play with Sims”.
Click the “Chemistry” link on the left hand side of the page, then “General Chemistry”.
Click the “Build a Molecule” simulation. Press “Download” hard disk or “Run” for on-line interaction.
Stay in the “Make Molecule” Tab
Explore how to make bonds by dragging the atoms and placing them together. Once the bond is formed,
you can break the bond by placing the cursor between the atoms. Once you build a structure, you can break
all bonds (atomize the particle) by clicking on the blue square, next to the green “3d” toggle.
Kit #1
Draw the Lewis (electron-dot) structure of the hydrogen atom ______ and the oxygen atom ___________.

Two possible molecules can be built with Kit #1. Build both molecules, and view the space-filling and
ball and stick models by clicking the green “3D” toggle .
The element ______________ , whose molecular formula is _______ and Lewis structure is _______; and,
the compound ____________, whose molecular formula is _______ and Lewis structure is ____________.

Once you have built both molecules, place one of the molecules on the right column by dragging it
into the black space and move to the next kit.

Click on “Reset Kit” to replace the original set of atoms in the bins, build the second molecule, and
drag it to the correct black space in the right column.

Go to Kit #2 by pressing on the Kit #1 “Next” yellow arrowhead.
Kit #2

Four molecules can be built with Kit #2. Two of the molecules are elements, while the other two are
compounds. Build the four molecules. Any molecule that is required in the right column may be
dragged there. You might need to “Reset Kit” if you make a required molecule to complete the
exercise. Make sure you view the space-filling and ball and stick models.
Fill the following table:
Name

Formula
Elements
Lewis Structure
Name
Compounds
Molecular
Lewis
Formula
Structure
Go to Kit #3 by pressing on the Kit #3 “Next” yellow, right-hand arrowhead.
Kit #3
Draw the Lewis (electron-dot) structure of the carbon atom __________ , the nitrogen atom __________,
and the oxygen atom ____________.

More than ten (10) molecules can be built with this kit: Two (2) elements and at least eight (8)
compounds. Two of the molecules are required in the right hand tray: carbon dioxide (CO 2) and
nitrogen (N2). You should do CO2 and N2 as your ninth and tenth molecules.

Build at least ten (10) different molecules, including CO2 and N2. List the names and formulas on the
following table. Don’t forget to view the space-filling and ball-and-stick models for each molecule. If
the molecule contains a double or a triple bond, check (√) the appropriate column.
Substance Name

Molecular
Formula
Double
Bond
Triple
Bond
Substance Name
Molecular
Formula
Double
Bond
Triple
Bond
Finish the exercise by building CO2 and N2 and viewing their “3D” models. Draw the Lewis
structure, below, and fill their data on the table. Once you finish your analysis, drag these molecules
to the right-hand column.
Lewis structures:
CO2
N2
Second, Third, and Fourth Collections

Complete the following collections, build the fifteen (15) required molecules, and fill the following
table with the compound name, formula, and the types of bonds found in the molecule
Name

Formula
Types of Bonds
Single Double Triple
Close the simulation.
Name
Formula
Types of Bonds
Single
Double Triple