Each student who wants to have the opportunity to take the RETAKE Test on Tuesday 0226-13. All work must be turn in the completed work before or on the date of the retake.
Identify the compound and write the name:
_____ 1.
Co(NO3)2
_______________________________
_____ 2.
H3(PO4)
_______________________________
_____ 3.
SO3
_______________________________
_____ 4.
SeF6
_______________________________
_____ 5.
H3(PO3)
_______________________________
_____ 6.
CaCO3
_______________________________
Thinking
Formula
___7. Phosphorous Pentachloride _______________
_______________
___8. Hydrosulfuric acid
_______________
_______________
___9. Iron (III) Acetate
_______________
_______________
___10. Silicon dioxide
_______________
_______________
___11. Oxalic Acid
_______________
_______________
_ 12. Magnesium perchlorate
_______________
_______________
Complete the rest of this worksheet on SEPARTE PAPER
.
13.
List at least three pieces of information about Ionic vs. Covalent Bonding:
14.
List the chemical characteristics (lab behaviors) of Ionic vs. Covalent Compounds
15.
16.
17.
18.
19.
20.
21.
22.
How is an acid identified?
What are the rules for naming acids?
How is polarity determined? Give an example of a polar molecule and a non-polar molecule.
What is meant by the term “Likes dissolve Likes”?
Explain the number of electrons in a single covalent bond, a double covalent bond, and a
triple covalent bond?
Explain what a sigma bond is:
Explain what a pi bond is:
How many sigma and pi bonds are found in a single covalent bond, a double covalent bond, and
a triple covalent bond?
Explain why the diatomic halogens exist as gases (F2 and Cl2), liquid (Br2), and solid (I2).
[Hint: Intermolecular forces and number of electrons]
Be able to draw a molecule and identify its shape and polarity (probably need to put
these on separate paper).
Formula
ClI
23.
24.
25.
electron-dot/ball
stick
SeF2
shape
CH4
polarity
PCl3
unshared
Intermolecular Angle
pairs of e- Force
Extra Credit
PCl5
CO2
SeF6 CH2O
Place the following molecules in order of lowest boiling point to highest boiling point:
C8H18
CH4
C3H8
C2H2
C5H12
Draw the following molecules and explain why each has the boiling point it has:
H2O [100oC]
C2H5OH (ethanol) [78oC]
o
C2H6 (ethane) [-89 C]
HOCH2CH2OH (ethane 1,2 diol) [197oC]
CH4 (methane) [-164oC]
(ethylene glycol (antifreeze))
If a student were given a liquid sample of a substance and wanted to determine if it was
ionic, covalent polar, covalent non-polar; explain three simple tests/experiments they could
perform to make their decision.