Chemistry Study Guide-Test 3-Chemical bonding
SPI 3221.3.1 Analyze ionic and covalent compounds in terms of their formation (electron transfer versus sharing),
names, chemical formulas (e.g., molecular: H2O, CO2, NH3; empirical: NaCl, CaBr2, Al(NO3)3), percent composition,
and molar masses.
Section 1: The Ionic Bond and Compound
1. What is an ionic bond?
2. Describe and draw the crystal lattice (ionic compound structure) and label with cation and anion.
3. List at least two physical properties of ionic compounds and be able to explain this property using the crystal
lattice as justification for the property.
Section 2: The Covalent bond and Molecules
4.
5.
6.
7.
8.
What is a covalent bond?
Describe the single, double and triple covalent bond?
List the bonds (single, double, triple) from strongest to weakest bond strength
List the bonds (single, double, triple) from longest to shortest bond length
List at least two general physical properties of covalent compounds and explain why.
Section 3: Metallic Bonding
9. Describe and draw the electron sea model of a metal and label with metal cation and delocalized electrons
10. List at least two physical properties of metals (one must be ductile/malleable) and be able to explain this
property using the metallic crystal as justification for the property.
Section 4: Nomenclature of compounds (ionic, covalent, acids) **NOTE: ON THE TEST, THEY WILL ALL BE MIXED
TOGETHER IN ONE SECTION, YOU SHOULD BE VERY FAMILIAR WITH HOW TO IDENTIFY AS IONIC, COVALENT OR AN ACID
AND NAME ACCORDINGLY
11. Name the following ionic componds:
a. FeO
b. NaBr
c. Na2SO4
12. Write the formulas for the following ionic compounds:
a. Iron (III) oxide
b. Calcium Chloride
c. Ammonium hydroxide
13. Name the following covalent compounds:
a. CO2
b. N2O5
c. N2O
14. Write the formulas for the following covalent compounds:
a. Carbon tetrabromide
b. Carbon monoxide
c. Silicon dioxide
15. Name the following acids:
a. HNO3 (aq)
b. H3P (aq)
c. H2SO3 (aq)
16. Write the formulas for the following acids:
a. Hydroiodic acid
b. Phosphoric acid
c. Hydrochloric acid
d. AgNO3
e. Ba(OH)2
f. Cu2S
d. Sodium phosphate
e. Cobalt (II) Nitride
f. Lead (IV) oxide
d. NO
e. H2O
f. SCl3
d. Sulfur trioxide
e. Xenon hexafluoride
f. Dinitrogen heptoxide
d. HCN (aq)
e. HClO4 (aq)
f. HBr (aq)
d. Acetic acid
e. Hydrofluoric acid
f. Hypochlorous acid
Section 5: Molecular Structures
17. For the following compounds draw the Lewis structure, identify the electron geometry, the molecular shape,
bond angles, and hybridization of the central atom
a. BeCl2
h. SCl2
b. AlCl3
i. SF4
c. CCl4
j. ClF3
d. PF5
k. XeF2
e. SF6
l. BrF5
f. NO2m. XeF4
g. NH3
Section 6: Polarity
18.
19.
20.
21.
What is a non-polar covalent bond?
What is a polar covalent bond?
What determines whether or not a molecule is polar or non-polar? *be able to explain this
Assuming that all atoms bound to the central atom are the same, you should know which molecular shapes
predict a polar molecule. You should also know which molecular shapes predict a non-polar molecule.
22. For EVERY compound (a.-m.) in question 17, identify the molecule as a polar or non-polar molecule.
23. Below are two Lewis structures for a compound with carbon as the central atom. Identify which one is polar and
which one is non-polar and EXPLAIN WHY.
Section 7: Intermolecular Forces
24. What is an intermolecular force and how is this different from an intramolecular force?
25. List and describe the 3 intermolecular forces that we discussed in class and order them by weakest to strongest
(generally)
26. How does an intermolecular force affect the boiling point of a substance?
27. List the following by increasing boiling point and explain why you listed them in this way: KBr, Ne, HF, BrCl
28. List the following by increasing boiling point and explain why you listed them in this way: He, Ar, Xe, Kr
ESSAY: The following essay question needs to be written prior to the test day and turned in with the test. It should be
typed, 12 font, Calibri/times new roman/arial, 1 complete page, double spaced, 1 in. margins, NO HEADINGS besides
your name, printed and turned in at test time this is not a separate assignment, it is a part of the test, not having it on
test day is equivalent of turning in a test with a missing question…it cannot be made up later. Do NOT wait until the
night before. DO NOT use excuses like “my printer didn’t work” “I don’t have a computer”…etc. You have received this in
plenty of time to complete it by the time you start the test. It must be complete by the test.
You will use this website as your 1st source. You will use their list to choose your properties. You must have 3 other
sources, total of 4. Use APA format (I will put up a guide on my page): http://water.usgs.gov/edu/waterproperties.html
Describe 2 physical properties and 1 chemical property of water and how polarity and intermolecular forces in water
explain these properties.