Download Part 1: Complete the chart below using a periodic table

Chemistry: Semester 1 Final Exam Review
Name: _________________________
The chemistry final exam is on Wednesday, January 21 (hours 1-3) and Thursday, January
22 (hours 4-6). It consists of 38 multiple choice questions and 8 short answer questions.
Clickers – What do I need to study in order to be ready for the final?
Clicker
Concept
1
models of the atom
2
3
protons, neutrons,
and electrons
protons, neutrons,
and electrons
Check if
INCORRECT
Review
Packet
Problems
Book Pages to Read
Book Practice
Problems
1-3
p. 102-108, p. 127-130
p. 108: 14; p. 132: 13
4-8
p. 110
p. 111: 15, 16
4-8
p. 111
p. 122: 50
4
isotopes
9
p. 112
p. 113: 20; p. 116: 21
5
nuclear reactions
10
p. 800-802
p. 808: 12
6
valence electrons
11-13
p. 187-188
p. 193: 7
7
ion charge
11-13
p. 188- 192
p. 193: 5, 6, 9
14-15
p.133-135
p. 135: 8; p. 151: 70
16
p. 261, 266
p. 282: 67
16
p. 268-269
p. 270: 22
17
p. 262-265, 270
p. 263: 11; p. 265: 13;
p. 270: 24
19
p. 330-336
p. 339: 24
20
p. 337-339
p. 339: 26
20
p. 337-339
p. 339: 26
8
9
10
11
12
13
14
electron
configuration
naming ionic
compounds
naming covalent
compounds
writing formulas of
compounds
types of reactions
predicting products
of reactions
predicting products
of reactions
15
balancing equations
21-22
p. 324-327
p. 327: 3; p. 328: 5
16
balancing equations
23
p. 324-327
p. 327: 3; p. 328: 5
17
molar mass
24
p. 293-296
p. 315: 53
18
mole conversions
25-26
p. 297-299
p. 315: 58a-c, 59a-c
19
stoichiometry
27-30
p. 359-362
p. 361: 13
20
rate of reactions
31-33
p. 545-547
p. 547: 2, 4, 5
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Unit 1: Atomic Structure and the Periodic Table
Models of the Atom
1. Complete the chart below about the five different models of the atom:
Model
Drawing
What does this model tell us about the structure of
the atom?
Dalton
Thomson
Rutherford
Bohr
Quantum
2. Explain one similarity and one difference between Thomson’s model of the atom and
Rutherford’s model of the atom.
3. Explain one similarity and one difference between Rutherford’s model of the atom and Bohr’s
model of the atom.
Protons, Neutrons, and Electrons
4. How do you determine the number of protons in an atom?
5. How do you determine the number of electrons in an atom?
6. How do you determine the number of neutrons in an atom?
7. Because atoms are electrically neutral, the number of _______________ must equal the number
of _______________.
2
8. Use a periodic table to complete the chart below:
Element
Atomic
Atomic
# of
Symbol
Number
Protons
a
Chlorine
# of
Electrons
# of
Neutrons
Mass
Number
18
b
Potassium
39
c
Magnesium
24
d
Fluorine
e
Aluminum
f
Sodium
g
Argon
10
27
11
40
Isotopes
9. Use a periodic table to complete the chart below:
Atomic
Number
Element
a
Lithium
b
Bromine
c
Copper
Atomic
Mass
(Atomic
Weight)
Number of
Protons
Number of
Electrons
Possible
Mass
Numbers
(2
numbers)
Possible
Number of
Neutrons
(2
numbers)
Mass of
More
Common
Isotope
Nuclear Reactions – Alpha and Beta Decay
10. Complete the following nuclear reactions and identify whether each is alpha or beta decay:
14
0
a. 6 C-1 e + _____
type: _______________
b.
32
14
32
c.
212
84
Po 2He + _____
d.
214
84
Po 82Pb + _____
Si 15P + _____
type: _______________
4
type: _______________
210
type: _______________
3
Valence Electrons
11. Use a periodic table to complete the chart below:
Element
a
Lithium
b
Oxygen
c
Potassium
d
Chlorine
e
Aluminum
Chemical
Symbol
Number
of
Valence
Electrons
Lewis Dot
Diagram
Will it lose
or gain
electrons to
become an
ion?
Number of
electrons
gained/lost
Charge on
the Ion
12. List two elements that have similar chemical and physical properties to barium.
13. Why do the elements you chose have similar chemical and physical properties to barium?
Electron Configurations
14. How many electrons can the following subshells hold?
s subshell: __________
p subshell: __________
d subshell: __________
f subshell: __________
15. Use a periodic table to complete the chart below:
Electron Configuration
a
1s22s22p63s23p64s23d2
b
1s22s22p63s23p64s1
Element
c
phosphorous
d
fluorine
e
calcium
# of Valence
Electrons
Shorthand Electron
Configuration
Unit 2: Ionic and Covalent Compounds
Naming Ionic and Covalent Compounds
16. Circle whether the following compounds are ionic or covalent and then name the compounds:
a) MgBr2
Ionic/Covalent ___________________________________
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b) SnF4
Ionic/Covalent ___________________________________
c) Ca(NO3)2
Ionic/Covalent ___________________________________
d) (NH4)2O
Ionic/Covalent ___________________________________
e) Fe3(PO4)2
Ionic/Covalent ___________________________________
f) SiF4
Ionic/Covalent ___________________________________
g) KCl
Ionic/Covalent ___________________________________
h) BaSO4
Ionic/Covalent ___________________________________
i) PbI2
Ionic/Covalent ___________________________________
j) N2S3
Ionic/Covalent ___________________________________
Writing Formulas for Ionic and Covalent Compounds
17. Fill in the chart below to show the transfer of electrons when calcium and phosphorous form an
ionic bond. Then write the resulting chemical formula.
# of valence
electrons
Lewis Dot Diagram
Will it lose or gain
electrons? How many?
Calcium (Ca)
Phosphorous (P)
Chemical Formula
18. Circle whether the following compounds are ionic or covalent and then write the formulas for the
compounds:
a) lead(IV) oxide
Ionic/Covalent _________________________
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b) aluminum bromide
Ionic/Covalent _________________________
c) nitrogen tribromide
Ionic/Covalent _________________________
d) ammonium sulfate
Ionic/Covalent _________________________
e) sodium phosphate
Ionic/Covalent _________________________
f) copper(II) nitride
Ionic/Covalent _________________________
g) lithium sulfide
Ionic/Covalent _________________________
h) diphosphorus pentoxide Ionic/Covalent _________________________
i) iron(II) carbonate
Ionic/Covalent _________________________
j) potassium chlorate
Ionic/Covalent _________________________
Unit 3: Chemical Reactions
Types of Reactions
19. Identify the following types of reactions (synthesis, decomposition, combustion, single
replacement, or double replacement):
a) C6H14 + O2 → CO2 + H2O
_________________________
b) AgNO3 + Ni → Ni(NO3)2 + Ag
_________________________
c) Ca(C2H3O2)2 + Na2CO3 → CaCO3 + NaC2H3O2
_________________________
d) NaClO3 → NaCl + O2
_________________________
e) Ca + HCl → CaCl2 + H2
_________________________
f) Cu + S8 → CuS
_________________________
g) C3H8 + O2 → CO2 + H2O
_________________________
h) BaCO3 → BaO + CO2
_________________________
i) AgNO3 + K3PO4 → Ag3PO4 + KNO3
_________________________
j) K + H2O → KOH + H2
_________________________
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Predicting Reaction Products
20. Identify the type of reaction, and then predict the products:
a) HNO3 + Ni →
Type of reaction:
Products:
HNO3 + Ni → _________________________
b) Ca(OH)2 + HCl → Type of reaction:
Products:
c) Li + Cl2 →
d) Zn + H2SO4 →
_________________________
Zn + H2SO4 → _________________________
e) LiNO3 + K3PO4 → Type of reaction:
Products:
_________________________
Li + Cl2 → _________________________
Type of reaction:
Products:
_________________________
Ca(OH)2 + HCl → _________________________
Type of reaction:
Products:
_________________________
_________________________
LiNO3 + K3PO4 → _________________________
Balancing Chemical Equations
21. What is the law of conservation of mass?
22. Why must equations be balanced?
23. Balance the following equations:
a) _____ Al(OH)3 + _____ H2CO3 → _____ Al2 (CO3)3 + _____ H2O
b) _____ Al + _____ S8 → _____ Al2S3
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c) _____ Cs +_____ N2 →_____ Cs3N
d) _____ Mg +_____ Cl2 → _____ MgCl2
e) _____ Rb +_____ RbNO3 →_____ Rb2O +_____ N2
Unit 4: Stoichiometry (or Calculating Chemical Quantities)
Molar Mass and Mole Conversions
24. Calculate the molar mass of the following:
a) CO2
__________
b) Na2SO4
__________
c) Cu(NO3)2 __________
25. Calculate the number of moles in the following:
a) 964 g Na2SO4
b) 23.7 g Cu(NO3)2
26. Calculate the number of grams in the following:
a) 5.15 moles Na2SO4
b) 0.97 moles Cu(NO3)2
8
Stoichiometry
27. In the reaction below, what is the ratio of moles of iron (Fe) used to moles of iron chloride (FeCl 3)
produced?
___Fe + ___Cl2
 ___FeCl3
28. How many moles of sodium carbonate (Na2CO3) are needed to react completely with 3.0 moles of
calcium hydroxide (Ca(OH)2)?
___Na2CO3 + ___Ca(OH)2  ___NaOH + ___CaCO3
29. When 13.5 g of calcium chloride react with an excess of silver nitrate, how many grams of silver
chloride are produced?
___CaCl2 + ___AgNO3  ___Ca(NO3)2 + ___AgCl
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30. Iron (III) oxide and hydrogen gas are heated to form metallic iron and water. How many grams of
iron are produced by heating 12.4 grams of iron (III) oxide?
Unit 5: Rates of Reactions
31. What effect does each of the following have on the rate of a reaction? Explain your reasoning.
a) Switching from a powder reactant to a solid block of the same reactant
b) Adding more of a reactant
c) Keeping the temperature constant using a water bath
32. A 6.0 g sample of Mg reacts with HCl in two different experiments. The reaction for both was:
Mg + 2HCl → MgCl2 + H2
In the first experiment, it took 6.2 minutes for all the Mg to react. In the second experiment, it took 10.8
minutes for all the Mg to react. What are some possible explanations for the change in rate in the second
experiment?
33. Using a drawing, explain why increasing the surface area increases the rate of a reaction.
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