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Rogers’ Chemistry
Final Review Sheet
1. Define and give an example of a (an):
a. Compound
b. element
c. mixture
d. heterogeneous mixture
e. homogeneous mixture
f. qualitative observation
g. quantitative observation
h. chemical property
i. physical property
j. intensive property
k. extensive property
2. Are the following elements or compounds
a. Hydrogen
b. water
c. gold
d. sugar
3. Name the Si base unit for the following measurements
a. Length
b. Volume
c. Mass
d. Temperature
4. The density of ethanol is 0.798 g/mL. What is the mass of 17.4 mL of
ethanol?
5. Convert:
a. 46 grams  milligrams
b. 35 nanometers  picometers
c. 289 kilobytes  decibytes
6. Express the following numbers in scientific notation:
a. 0.000000027
b. 356
c. 47,764
d. 0.096
7. Express the following as decimals
a. 1.52 x 10-2
b. 7.78 x 10-8
c. 9.34 x 106
8. How many sig figs are in the following numbers?
a. 4867
b. 56
c. 60,104
d. 2900
e. 40.2
f. 8900.
g. 0.7
9. Carry out the following operations and express your answer in the correct
number of sig figs
a. 5.6792 + 0.6 + 4.33
b. 3.70 – 2.9133
c. 4.51 x 3.6666
d. (3000 + 6.827)/(0.043 – 0.021)
10. Name the three types of radiation and the symbol for each
11. Complete the following nuclear equations.
a.
28
Al  _____ + 
b. ______ 
c.
210
d.
35
234
Th
+

Bi  _______ +
S  _______
+


12. Fill in the following chart:
Substance
Carbon
Lead
Chlorine
Neon
Oxygen
Hydrogen
Atomic
Mass
Atomic
Number
Protons
Neutrons
Electrons
13. Complete the following isotope chart:
Symbol
# Neutrons
# protons
2
# electrons
Atomic mass
H
14
14
39
C
N
2
1
7
6
21
19
K
82
206
14. Strontium consists of four isotopes with masses of 84 (abundance 0.50%),
86 (abundance of 9.9%), 87 (abundance of 7.0%), and 88 (abundance of
82.6%). Calculate the atomic mass of strontium.
15. Naturally occurring europium (Eu) consists of two isotopes was a mass of
151 and 153. Europium-151 has an abundance of 48.03% and Europium153 has an abundance of 51.97%. What is the atomic mass of europium?
16. Write the formulas for the following:
a. Sodium oxide
b. iron (II) sulfide
c. barium fluoride
d. dihydrogen tetroxide
e. Cobalt (IV) Phosphate
17. Write the names of the following compounds
a. Li2CO3
b. C2H5
c. FeO
d. PF3
e. HF
f. H3PO4
18. On the periodic table below label the: metals, nonmetals, metalloids,
transition metals, halogens, alkali metals, noble gases, s block, p clock, d
block, f block.
19. Using the periodic table below show the trends of ionization energy,
electro negativity, and atomic radius.
20. How many moles of Fe are present in 24.6 grams of Fe2O3?
21. Write the empirical formulas for the following molecules
a. C2N2
b. C9H20
c. Al2Br6
d. Na2S4O6
e. TiCl4
22. What is the difference between an ionic compound and a covalent
compound? How do you tell the difference?
23. How many particles are in the following:
a. 5.10 moles of Sulfur
b. 17.5 moles of water
c. 87.5 grams of carbon dioxide
d. 12 grams of steam
e. 345.8 grams of H3PO4
24. Calculate the molar mass of the following:
a. SO3
b. CH4
c. K2SO4
d. Li2CO3
e. Al(OH)3
f. Co3(PO4)4
25. Calculate Percent composition of the following:
a. SnO2
b. CHCl3
c. NH3
d. NH4OH
26. Using the following percents, figure out the empirical formula of the
compound:
a. Allicin, which smells like garlic, is 44.4% Carbon, 6.21% H, 39.5 %
S, and 9.86 % Oxygen.
b. A compound with 2.1% H, 65.3 % O and 32.6% S
c. A compound that is 40.1% C, 6.6% H and 53.3% O
27. Determine the molecular formula for the following
a. Empirical formula: CH3 Molar Mass: 30.0 grams/mole
b. Empirical Formula C2H3O Molar Mass: 172.0 grams/mole
c. Emperical formual AlCl3
Moalr Mass: 667.5 grams/mole
28. Balance the following equations:
a. _____ K2O + _____ H2O  _____ KOH
b. _____ KClO3  _____ KCl + _____ O2
c. _____ C6H5OH + _____ O2  _____ CO2 + ______ H2O
d. _____ Fe + _____ S  _____Fe2S3
e. _____ Na + _____ HOH  _____NaOH + _____H2
f. _____ NaCl + _____ H2SO4  _____ Na2SO4 + _____HCl
g. _____KI + _____ Pb(NO3) 2  _____PbI2 + _____ KNO3
h. _____ Al + ______ H2SO4  _____ Al2(SO4) 3 + _____H2
i. _____ Cu + _____ H2O  _____ CuO + _____ H2
j. _____ Al(NO3) 3 + _____ NaOH 
____ Al(OH) 3 + ___ NaNO3
29. Write the word equation for the following reactions:
a. N2H4 + H2O2  N2 + H2O
b. Pb(NO3)2 + NaCl  PbCl2 + NaNO3
c. Mg + AgNO3  Mg(NO3)2 + Ag
d. K3PO4+ Ca(NO3)2  Ca3(PO4)2 + KNO3
30. Turn the following sentences in chemical equations. (And Balance)
a. Aluminum is a good choice for outdoor furniture because it reacts
with oxygen in air to form a thin protective coating of aluminum
oxide.
b. When barium chloride is allowed to react with silver nitrate, barium
nitrate and silver chloride are both produced.
31. Count and write down the number of atoms for each different element in
the following compounds.
e. LiOH
b. Ag(NO3)2
c. 3 BeCl2
d. (NH4)3P
e. 6 C3H6
f. 4 Al2(CO3)3
32. Identify which one of the five types of chemical reactions the following
reactions are: (They are not balanced, this is OK)
f. C5H7 + O2  CO2 + H2O
g. AgNO3 + Cu  Cu(NO3)2 + Ag
h. S + O2  SO3
i. NaCl + CaF2  NaF + CaCl2
j. C2H2O  C + H2 + O2
33. Ethylene (C2H4 ) reacts with oxygen gas to produce carbon dioxide and
water. If you start with 45 grams of ethylene, how many grams of carbon
dioxide will be produced?
34. Given the equation: HCl + Na2SO4  NaCl + H2SO4
If you start with 20 grams of hydrochloric acid, how many grams of sulfuric
acid will be produced?
35.Given the following equation: LiOH + KCl  LiCl + KOH
a. I began this reaction with 20 grams of lithium hydroxide. What is
my yield of lithium chloride?
b. I actually produced 6 grams of lithium chloride. What is my percent
yield?
36. 6 CO2 + 5 H2O  C6H10O5 + 6 O2
If 4.58 grams of carbon dioxide is reacted with 18.6 grams of water how
much oxygen gas is produced? What is the limiting reactant? How much
of the excess reactant is left?
37. NaCl + AgNO3 ---> NaNO3 + AgCl
How much silver chloride is produced if 18.8 grams of NaCl is reacted
with 25.9 grams of AgNO3? What is the limiting reactant? How much of
the excess reactant is left?
38. Write the net ionic equations for the following:
a. __Na2S(aq) + __ZnCl2 (aq) - __ZnCl2 (s) +
__NaCl(aq)
b. __NaCl (aq) + _ Ag(C2H3O2) (aq) → __Na(C2H3O2) (aq) + __AgCl (s)
c. __Ca(OH)2 (aq) + __H3PO4 (aq) → ___H2O (l) + _____ Ca3(PO4)2 (s)
d. _____ HNO3 (aq) + ____ Ni (s) → ____ Ni(NO3)2 (aq) + _____ H2 (g)
39. A gas takes up 36.7 L of space at STP. How many moles of gas are present?
40. At a pressure of 654 mm Hg a gas occupies 34.9 L. How much space will it
occupy at 4.1 atm?
41. A sample of argon gas is kept in a 2.3 L container and at 320C is exerts a
pressure of 4.7 atm. How many moles of gas are there?
42. A gas occupies 5.6 L at a temperature of 564 K, how much space will it
occupy at 340 K?
43. Nitrogen monoxide reacts with oxygen to produce nitrogen dioxide. If 9.0L of
NO are reacted with excess oxygen at STP, how many grams of nitrogen dioxide
is produced?
44. S + O2  SO2
If 2.54 grams of S are reacted with oxygen, how many liters of SO2 are
produced if the reaction takes place at 30.8 oC and 1.12 atm?
45. A mixture of gases contains three gasses. There pressure are 3.45 atm, 987
torr, and 345 mm Hg. What is the total pressure of the mixture in atm?
46. What is the difference between an ideal and a real gas?
47. What is the difference between an exothermic and an endothermic reaction?
Give an example of each.
48. What is the wavelength of light in nm that has a frequency of 8.6 x 1013 Hz?
49. Calculate the energy of a photon with wavelength 624 nm.
50. Electrons can be described as both ______________ and ________________.
51. What are the four quantum numbers and what do they represent?
52. Write the electron configuration of the following :
a. P
b. K+
c. Cu+4
53. Write the SHORT HAND configuration for the following:
a. Cl
b. Ni
c. Au
54. What is Hund’s rule?
55. Why isn’t the following an acceptable set of quantum numbers? ( 2,4,1,+1/2)
56. Draw the orbital diagram for Oxygen
57. List the three phases of matter and the major properties of each.
58. Draw the following molecules (lewis structures) and determine if they are
polar or nonpolar:
a. PCl3
b. CH4
c. CH3OH
d. SO2
e. SF6
59. Determine what INTERMOLECULAR force(s) are present in each of the
above.
60. What is resonance? Draw a compound that shows resonance.
61. A hydrate is a compound that contains ________________. Write the formula
for Magnesium Chloride pentahydrtae.
62. What is the molarity of a solution that conatins 45.8 grams of NaCl dissolved
in 450ml of water?
63. How many grams of magnesium oxide are present in 670 mL of a 5.4 M
solution?
64. Label the following diagram:
65. Indicate what each of the letters represents in the following diagram:
66. Use the solubility curve below to answer these questions:
a. what type of compounds decrease in solubility as temperature increase?
b. how many grams of NaCl can be dissolved in 50 grams of water at 50OC
c. At 95OC what two compounds have roughly the same solubility?
d. how many moles of NH3 should be added to 75 g of water at 25OC to
make a saturated solution?
67. What is the firrence between an acid and a base? What do all acids have? What
do all bases have?
68. What is the pOH, [H+] and [OH-] of acid rain with a pH of 4.82?
69. Calculate the pH of a 0.3 molar solution of hydrochloric acid.
70. Calculate the pOH of a 0.004 molar nitrous acid solution.
71. Explain the purpose of a titration and how they work.