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Ms. Mai
Chemistry
Name:
Period:
1st Semester Final Exam Review Sheet
YOU MUST COMPLETE THIS ENTIRE REVIEW SHEET BEFORE TAKING THE FINAL EXAM.
THERE WILL BE NO CALCULATORS ALLOWED DURING THE FINAL EXAM.
SHOW ALL WORK ON A SEPARATE SHEET OF PAPER.
Atomic Structure
1. What is the difference between mass number and atomic number?
2. Which elements have similar chemical properties?
3. What is an isotope?
4. What do all atoms of a given element have the same number?
5. Which particle plays the greatest role in determining the properties of an element?
6. Differentiate between period and group.
7. Where are metals, semi-metals, and nonmetals located on the periodic table?
8. Where are alkali metals, alkaline earth metals, halogens, noble gases, and transitions metals located?
9. Use your periodic table to complete the table below
ATOM
SYMBOL
ATOMIC
MASS
# OF
# OF
# OF
NUMBER NUMBER PROTONS ELECTRONS NEUTRONS
Fe
56
CHLORINE
ARGON
26
17
40
Al
HYDROGEN
TITANIUM
NITROGEN
KRYPTON
SULFUR
10. Fill in the following chart
Element
Chromium
Iodine
Potassium
Vanadium
Lithium
Neon
Californium
Barium
Strontium
Platinum
1
27
1
48
26
18
13
18
22
13
1
22
7
36
32
Group Name (ex. Noble Gas)
7
36
7
16
Metal/Nonmetal/Metalloid
Trends in the Periodic Table
11. Describe the following trend on the periodic table.
a. Atomic Number
b. Atomic Size
c. Ionization Energy
d. Electronegativy
12. Which atom is more electronegative, fluorine or lithium?
13. Which atom has a greater ionization energy, nitrogen or bismuth?
14. Which atom has a larger atomic radius, fluorine or barium?
15. Which element is more like lithium in terms of properties, sodium or beryllium?
16. Which element has more electrons in its valence shell, sodium or magnesium?
17. Which element is closer to achieving noble gas configuration, magnesium or lithium?
Bonding
18. Describe how a cation and an anion is formed.
19. What do metals typically do when they become ions? What about nonmetals?
20. What type of elements bond together in ionic bonds? covalent bonds? metallic bonds?
21. How do electrons in ionic bonding interact? Covalent bonding?
22. How does the relative size of an anion and cation compare to its neutral atom?
23. Which element would calcium more likely bond with, oxygen or fluorine?
24. Which element would nitrogen more likely bond with, magnesium or chlorine?
25. Which element will react more readily with chlorine, sodium or magnesium?
26. Draw Lewis Dot Structures for the following compounds
a. Cl2
d. CH2Cl2
a. H2
e. NH3
b. CH4
f. CH3OH
c. CH3I
g. H2O
h.
i.
j.
k.
27. Label each of the following compounds as ionic or covalent.
a. C6H12O6
c. NH2CH2
b. NaCl
d. SiO2
e. H2O
f. MgBr2
28. How many valence electrons do the following atoms have?
a. Magnesium
d. Helium
b. Carbon
e. Silicon
c. Argon
f. Potassium
g. Sulfur
h. Calcium
i. Hydrogen
Balancing Equations
29. In balancing equations, what must be the same on both sides of the equation?
30. What is the only thing you can change when you balance an equation?
O2
N2
HCN
C2H2
31. Balance the following equations
a. NaOH + H2SO4  Na2SO4 + H2O
b. Pb(C2H3O2)2 + H2S  PbS + HC2H3O2
c. KOH + Al2(SO4)3  K2SO4 + Al(OH)3
d. Ca(NO3)2 + K3PO4 Ca3(PO4)2 + KNO3
e. Na2CO3 + Al2(SO4)3 + H2O  Na2SO4 + Al(OH)3 + CO2
f. C2H5OH + O2  CO2 + H2O
32. Complete the following equations and identify which type of reaction it is.
a. Fe + Cl2 
b. Cu + Br2 
c. PCl5 
d. H2SO4 
e. Mg + PbSO4 
f. K + HgCl2 
g. Na3PO4 + MgSO4 
h. Pb(NO3)2 + H2SO4 
Mole Conversions
33. What does Avogadro’s number represent?
34. Calculate the molar mass of each of these substances.
a. AlCl3
d. TeF4
b. KF
e. ZnO
c. KMnO4
f. CaSO4
g. PbS
h. Ba(SCN)2
i. H2CO3
35. Calculate the mass of 1.000 mole of CaCl2
36. How many moles are in 4 grams of H2O?
37. Calculate number of moles in 32.0 g of CH4
38. Determine mass in grams of 40.0 moles of Na2CO3
39. Calculate moles in 168.0 g of HgS
40. How many moles are in 27.00 g of H2O
41. Calculate the number of molecules in the following:
a. 67.2 grams NaCl
b. 1 mole H2O
c. 33 grams of CH4
d. 3.00 mole AlCl3
42. Determine the number of atoms from moles. (In other words, convert from moles into atoms.)
a. 2.00 mole HC2H3O2
b. 5.00 mole Ag2O
c. 0.000300 mole AuCl3
d. 0.00550 mole CH4
43. Use the following equation to answer the questions below: N2 + 3H2  2NH3
a. How many moles of NH3 are in 1.75 moles of N2?
b. How many moles of N2 are in 5.23 moles of H2?
c. How many moles of H2 are in 3.02 moles of NH3?
44. Determine the mass of carbon dioxide produced when 0.85 grams of butane (C4H10) reacts with oxygen
according to the following unbalanced chemical equation: C4H10(l) + O2(g)  CO2(g) + H2O(g)
45. Determine the mass of sodium nitrate produced when 0.73 grams of nickel (II) nitrate reacts with
sodium hydroxide according to the following unbalanced chemical equation:
Ni(NO3)2(aq) + NaOH(aq)  Ni(OH)2(aq) + NaNO3(aq)
46. When iron (II) hydroxide is mixed with phosphoric acid, iron (II) phosphate precipitate results.
a. Balance the following equation: Fe(OH)2(aq) + H3PO4(aq) 
3(PO4)2(s) + H2O(l)
b. If 3.20g of Fe(OH)2 is treated with 2.50 g of H3PO4, what is the limiting reagent and what is the
excess reagent?
c. Using the previous information, how many grams of Fe3(PO4)2 precipitate can be formed?
47. Quicklime (CaO) can be prepared by roasting limestone (CaCO3). When 2.00 x 103g of CaCO3 are
heated, the actual yield of CaO is 1.50 x 103g. What is the percent yield? CaCO3  CaO + CO2
48. If 1.85g of Aluminum reacts with an excess of Copper (II) Sulfate (CuSO4), the percentage yield of Cu
is 56.6%. What mass of Cu is produced? 2Al + 3CuSO4  3Cu + Al2(SO4)3
49. Assume that 2.0mol of methane (CH4) is burned in the presence of excess oxygen. What is the
percentage yield if the reaction produces 87.0g of CO2? CH4 + 2O2  CO2 + 2H2O
50. Calculate the volume of 45.9 grams of C6H12O11 gas at STP.
Thermodynamics
Study the chart below. You will have 2-3 questions on your final exam.
Exothermic
Endothermic
Releases energy/heat
Absorbs energy/heat
Condensation and Freezing
Evaporation and Melting
Energy is on the right side of the equation
Energy is on the left side of the equation
Example: CH4 + 2O2  CO2 + 2H2O + energy
Example: N2 + O2 + energy  2NO
Graph goes from higher to lower
Graph goes from lower to higher