Pre AP Compound Practice Exam 2015
These are the objectives for the unit. Read over them and think of ways they could be tested.
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4.
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12.
Understand why atoms bond to form stable electron configurations
Differentiate between ionic and covalent bonds and predict the type of bond between elements using electronegativity values
Identify, write, and name ionic compounds given elements or polyatomic ions and a periodic table
Understand and use polyatomic ions in formulas; memorize common polyatomic ions
Identify, write, and name molecular compounds given elements and atomic or mass ratios
Write electron dot diagrams and use these to predict single, double, and triple bonds
Calculate molar mass of compounds and complete mole calculations.
Predict and list chemical and physical properties of ionic and molecular compounds
Compare the arrangement of atoms in molecular, ionic crystals, polymers, amorphous, and metallic substances
Predict molecular geometry using VESPER
Understand and describe metallic bonds and alloys
Conceptualize and calculate percent composition of elements in compounds as well as other macro examples
Complete the following free response questions.
1. List four properties of ionic compounds:
2. How can you identify a binary molecular compound from the name/formula?
3. Why is it important to use roman numerals like II or IV when naming an ionic compound with a transition metal?
4. Describe the actions of the valance electrons in metallic bonds.
5. In a covalent/molecular bond, electrons are ___________ while in an ionic bond electrons are ___________ or
_____________.
6. Non-metals tend to __________ electrons and become _____________ in ionic bonding.
7. Atoms want a full outer energy level. For most atoms, this is ___________ electrons which is why this is called
the __________ rule.
9. Give the molar mass for the following compounds.
a. H2SO4
b. C2H2
c. Ba(OH)2
10. Draw an electron dot diagram to predict the type of bonding and the number of
bonds between two atoms of nitrogen in the diatomic molecule N2.
11. Name the following compounds:
1. Li2S
6. N7S8
2. CO3
7. PbO
3. CuBr
8. FeBr3
4. Cu2O
9. Ba(CN)2
5. Na2SO4
12. Write the formulas for the following compounds:
6. lithium carbonate
5. cupric sulfate
7. potassium cyanide
6. dihydrogen monoxide
8. tin (IV) chlorite
7. Lead (II) iodide
9. beryllium oxide
8. ammonium sulfate
13. What is meant by the term polar? How can you tell if a bond it polar covalent, nonpolar covalent or ionic?
14. Calculate the mass of
1.25 moles of LiCl
2.57 x 1023 molecules of water
15. Find the % oxygen by mass in water.
16. If a compound consists of 38.7 % C, 16.1 % H and 45.2 % N, what is the empirical formula?
Complete the following multiple choice questions by choosing the best answer.
17. There are _____ paired and _____ unpaired electrons in the Lewis symbol for a phosphorus atom.
a. 4, 2
b. 2, 4
c. 2, 3
d. 4, 3
e. 0, 3
18.
a.
b.
c.
d.
e.
Based on the octet rule, magnesium most likely forms a _____ ion.
Mg2+
Mg2Mg6Mg6+
Mg-
20. Which of the following would have to gain two electrons in order to achieve a noble gas electron
configuration?
O Sr Na Se Br
a. Br
b. Sr
c. Na
d. O & Se
e. Sr, O, & Se
21.
a.
b.
c.
d.
e.
Elements from opposite sides of the periodic table tend to form ____________.
covalent compounds
ionic compounds
compounds that are gaseous at room temperature
homonuclear diatomic compounds
covalent compounds that are gaseous at room temperature
22.
a.
b.
c.
d.
e.
How many single covalent bonds must a silicon atom form to have a complete octet in its valence shell?
3
4
1
2
0
23.
a.
b.
c.
d.
e.
Compounds consisting entirely of nonmetals ____________.
are noble gases
are ionic
do not exist
are molecular
are always solid at room temperature
24. A double bond consists of _____ pairs of electrons shared between two atoms.
a. 1
b. 2
c. 3
d. 4
e. 6
25.
a. 0
26.
a.
b.
c.
d.
e.
What is the maximum number of double bonds that a hydrogen atom can form?
b. 1
c. 2
d. 3
e. 4
The central atom in _____ violates the octet rule.
ClF3
PCl3
SO3
CCl4
CO2
27. The Lewis structure of the CO2 molecule has ____ double bond(s).
a. 0
b.1
c. 2
d. 3
e. 4
28.
a.
b.
c.
d.
e.
The basis of the VSEPR model of molecular bonding is ____________.
regions of electron density on an atom will organize themselves so as to maximize s-character
regions of electron density in the valence shell of an atom will arrange themselves so as to maximize overlap
atomic orbitals of the bonding atoms must overlap for a bond to form
electron pairs in the valence shell of an atom will arrange themselves so as to minimize repulsions
hybrid orbitals will form as necessary to, as closely as possible, achieve spherical symmetry
29. The electron-domain geometry of _____ is tetrahedral.
a. CBr4
b. PH3
c. CCl2Br2
d. XeF4
e. all of these except XeF4
30.
a.
b.
c.
d.
e.
The molecular geometry of the SF2 molecule is __________.
linear
bent
trigonal planar
tetrahedral
octahedral
Fill in the missing name or formula:
Name
Formula
calcium chloride
______________________________
barium nitride
______________________________
silver oxide
______________________________
iron(II) oxide
______________________________
lithium sulfate
______________________________
barium nitrate
______________________________
dinitrogen pentoxide
______________________________
calcium acetate
______________________________
water
______________________________
ammonia
______________________________
magnesium sulfate
______________________________
______________________________
Ca3P2
______________________________
CBr4
______________________________
KCl
______________________________
Na2CO3
______________________________
Al2O3
______________________________
FeBr2
______________________________
Sn(ClO3)4
______________________________
NO2
______________________________
AgBr
______________________________
NaNO3
______________________________
CuCl2
Find the molar mass of the following compounds:
lithium sulfate
______________________________
barium hydroxide
_____________________________
magnesium acetate
______________________________