Download Print out Reviews # 1 through # 17

EOC REVIEW #1
1. List the following in order from smallest to largest.
(A) 1 dm3
(B) 1 mL
(C) 1 cL
(D) 1 L
(E) 1 dL
2. Convert the following. Express your answer in standard scientific notation.
(A) 36 cm to m
(B) 68.9 m to dm
(C) 14.8 g to kg
(D) 3.72 x 10-3 kg to g
(E) 1.44 kL to L
(F) 66.3 L to cm3
3. What is the mass, in kg, of 14.0 L of gasoline given the density of gasoline is 0.680 g/cm 3?
4. What is the mass of a cube of aluminum that is 3.0 cm on each edge given the density of aluminum to be
2.7 g/cm3?
5. How many significant figures are in each of the following measurements?
(A) 0.1430 g
(B) 1.072 km
(C) 0.074 cm
(D) 10,800 mL
-2
3
(E) 8.750 x 10 dm
(F) 5.00 kg
6. Round off each of the following measurements to 3 significant figures.
(A) 98.473 L
(B) 12.17 oC
(C) 0.00076321 kg
(D) 7.485 x 104 mm
(E) 57.048 m
(F) 1764.9 mL
7. Distinguish between accuracy and precision of a measurement.
8. A technician experimentally determined the boiling point of octane as 124.1 oC. The accepted boiling point of
octane is 125.7oC. Calculate the percent error.
EOC REVIEW #2
1. Classify each of following as a physical or chemical change.
(A) bending a piece of cork
(B) burning coal
(C) cooking a steak
(D) cutting glass
2. Identify each of the following samples of matter as heterogeneous or homogeneous.
(A) spaghetti sauce
(B) glass
(C) table sugar
(D) river water (with mud)
(E) sand from the beach
(F) nitrogen
3. Classify the following properties of the element silicon as chemical or physical properties.
(A) blue-gray color
(B) melts at 1410oC
(C) brittle
(D) reacts vigorously with fluorine
(E) insoluble in water
4. Give the symbol for each element described below.
(A) nonmetal in Group 14
(B) a metal in Group 15
(C) the 2 elements that are liquids at room temperature
EOC REVIEW #3
1. What did Rutherford’s gold foil experiment tell us about the structure of the atom?
2. Find the molar mass of each of the following compounds.
(A) Ca3(PO4)2
(B) PCl3
(C) Pb(NO3)2
3. How many moles of magnesium are equal to 3.01 x 10 22 atoms of magnesium?
4. How many molecules are in 4.00 moles of glucose, C6H12O6?
5. How many grams are in 2.14 moles of CO?
6. How many grams are in 4.65 x 1024 molecules of NO2?
7. Complete the following table.
Symbol
Name
# of p+
Mass #
# of e-
Atomic #
# of no
hydrogen – 1
carbon – 14
19
39
17
18
zinc – 65
40
+2
Ca
4
92
2
235
-----------------------------------------------------------------------------------------------------------------------------------------EOC REVIEW #4
1. Write the electron configurations and draw the HOEL orbital notations for the elements that are identified by
these atomic numbers.
(A) 15
(B) 12
(C) 9
(D) 18
2. Give the symbol and name for the atom whose electron configuration corresponds to each of the following
electron configurations.
(A) 1s2 2s2 2p6 3s2 3p6
(B) 1s2 2s2 2p6 3s2 3p6 4s1
2
2
6
2
6
2
10
3
(C) 1s 2s 2p 3s 3p 4s 3d 4p
(D) 1s2 2s2 2p6 3s2 3p6 4s2 3d7
2
2
4
(E) 1s 2s 2p
(F) 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2
3. Identify the four quantum numbers for the last electron added to the element described in 2. (E).
4. Draw the electron dot diagrams for the following elements.
(A) argon
(B) phosphorus
(C) sodium
(D) silicon
(E) aluminum
(F) bromine
EOC REVIEW #5
1. How is an element’s outer electron configuration related to its position on the Periodic Table?
2. What are the symbols for all of the elements that have the following outer electron configuration?
(A) s1
(B) s2 p2
(C) s2 p5
3. Indicate which element in each of the following pairs has the larger atomic radius.
(A) sodium , lithium
(B) selenium , oxygen
(C) strontium , magnesium
(D) nitrogen , fluorine
(E) carbon , germanium
(F) zinc , bromine
4. Arrange each set of elements in order of increasing ionization energy.
(A) Be , Mg , Sr
(B) Bi , Cs , Ba
(C) Na , Al , S
5. In each of the following pairs, which element is more electronegative?
(A) Cl , F
(B) C , N
(C) Kr , Br
(D) As , Ca
6. How many valence electrons do each of the following atoms have?
(A) K
(B) C
(C) Mg
(D) O
7. State the number of electrons either lost or gained in forming each ion.
(A) Br-1
(B) Na+1
(C) As-3
+2
+1
(D) Ca
(E) Cu
(F) H-1
EOC REVIEW #6
1. Explain the difference between ionic and molecular (covalent) compounds, giving two examples of each.
2. Draw Lewis structures for the following compounds:
(A) OF2
(B) SiO2
(C) NI3
(D) NO3-1
(E) CCl4
(F) SO2
3. Tell polarity, class (A, B, E) and shape of each of the above molecules.
EOC REVIEW # 7
1. Write the formula and the name for the compounds formed from these pairs of substances.
(A) barium and sulfur
(B) calcium and nitrogen
(C) lithium and oxygen
(D) copper (II) and iodine
2. Write the formulas for these compounds.
(A) sodium bromide
(B) tin (II) fluoride
(C) potassium sulfide
(D) calcium phosphide
3. Name these binary compounds.
(A) ZnS
(B) BaO
(C) KCl
(D) CuBr2
4. Name the following compounds:
(A) MgCl2
(B) LiBr
(C) Al2S3
(D) CaCO3
(E) MnO2
(F) NaOH
(G) NO2
(H) Al2(SO4)3
(I) SO3
(J) K3PO4
(K) BaO
(L) CO
5. Calculate the percent by mass of carbon in propane, C3H8.
6. What is the percent of magnesium in magnesium bromide?
7. Calculate the empirical formula of each compound with the following percent composition.
(A) 67.6% Hg, 10.8% S, 21.6% O
(B) 69.94% iron, 30.06% oxygen
EOC REVIEW # 8
1. Match each type of reaction with the phrase that best describes it.
(A) double replacement
(1) a single reactant
(B) combustion
(2) two ionic compounds
(C) decomposition
(3) oxygen and a compound
(D) single replacement
(4) a single product
(E) synthesis
(5) an element & a compound
2.
After balancing the following equations, identify them as to type:
(A)
___ Ca + ___ N2  ___ Ca3N2
(B)
___ Mg + ___ H2SO4  ___ MgSO4 + ___ H2
(C)
___ C2H6 + ___ O2  ___ CO2 + ___ H2O
(D)
___ Pb(NO3)2 + ___ NaI  ___ PbI2 + ___ NaNO3
(E)
___ Fe3O4  ___ Fe + ___ O2
3. Use the Activity Series to determine if the following reactions will occur or not. Predict the products if the
reaction happens.
(A) fluorine + sodium bromide 
(B) iron (II) nitrate + potassium 
(C) calcium + zinc phosphate 
(D) iodine + potassium chloride 
(E) magnesium + chromium (III) acetate 
(F) strontium chlorate + manganese 
EOC REVIEW # 9
1. How many moles of ammonia are produced when 0.600 moles of nitrogen react with excess hydrogen?
___ N2 (g) + ___ H2 (g)  ___ NH3 (g)
2. Calculate the number of grams nitrogen that are required to make 7.24 moles of ammonia (NH 3).
___ N2 (g) + ___ H2 (g)  ___ NH3 (g)
3. How many grams of nitrogen are needed to produce 30.6 grams of NH 3?
___ N2 (g) + ___ H2 (g)  ___ NH3 (g)
4. What is the theoretical yield (in grams) of aluminum oxide when 13.5 grams of aluminum are reacted with
excess oxygen gas? If 21.2 grams of aluminum oxide were produced in an experiment, what is the percent
yield?
___ Al + ___ O2  ___ Al2O3
5. How many molecules of oxygen are produced when 29.9 grams of water are decomposed according to the
following equation?
___ H2O  ___ H2 + ___ O2
6. Sodium chloride can be prepared by the reaction of sodium metal with chlorine gas.
(A) Write the balanced equation for the reaction:
(B) 6.70 moles of Na reacts with 3.20 moles of Cl2
- What is the limiting reactant?
- How many moles of NaCl are produced?
EOC REVIEW # 10
1. What is the mass of nitrogen gas is contained in a 355 mL container at a pressure of 802 torr and a
temperature of 73oC?
2. At 54oC, a gas has a pressure of 1.25 atm and a volume of 625 mL. When the temperature is decreased to
25oC and the pressure is changed to 745 mm Hg, what is the new volume?
3. A mixture of gases contains helium, neon, and argon. The total pressure of the mixture of gases is 1510 mm
Hg. If the pressure of neon is 1.02 atm and the pressure of argon is 97.2 kPa, what is the partial pressure of
the helium (in mm Hg)?
4. What is the density of N2 gas at 35oC and 1.25 atm?
5. A gas effuses 4.7 times faster than PCl 3. What is the molar mass of the unknown gas?
6. At STP, 23.6 liters of acetylene are burned in excess oxygen gas. How many grams of carbon dioxide are
formed?
___ C2H2 + ___ O2  ___ CO2 + ___ H2O
7. AT STP, how many liters of oxygen are needed to produce 19.8 liters of SO 3 according to this equation?
___ SO2 (g) + ___ O2 (g)  ___ SO3 (g)
EOC REVIEW #11
Part 1 – Phase Diagram – Use the following phase diagram to answer questions 1 – 5.
1. What are the temperature and pressure at the triple point?
2. What is the critical temperature of this substance?
3. What is the normal melting point for this substance? The normal boiling point?
4. At 1.0 atm pressure (standard pressure), does this substance undergo sublimation?
5. Indicate the state(s) of matter present at:
(A) 102oC and 2.5 atm
(B) 40oC and 0.5 atm
(C) 45oC and 1.0 atm
(D) 0oC and 0.75 atm
o
(E) 75 C and 2.0 atm
(F) 70oC and 1.0 atm
Part 2 – Heat Calculations – Use the data given on the Reference Tables to solve the following problems.
6. How many Joules of heat are required to melt a 17.5 gram sample of ice at 0.0 oC?
7. How many Joules of heat are required to heat a 17.5 gram sample of water from 0.0oC to 24.3oC?
EOC REVIEW #12
Part 1 – Solubility Curves – Use the following graph to answer questions 1 – 4.
1. At what temperature does 50 grams of KCl dissolved in 100 grams of water form a saturated solution?
2. How many grams of NaNO3 will dissolve in 300 grams of water at 60 oC?
3. If 32 grams of NaCl are dissolved in 100 grams of water at 30 oC, is the solution saturated, unsaturated, or
supersaturated?
4. How many grams of solid precipitate will form if a saturated NH 4Cl solution is cooled from 80oC to 20oC?
Part 2 – Concentration of Solutions
5. How many grams of Al(C2H3O2)3 are needed to dissolve to make 500. mL of a 2.50 M solution?
6. What is the molarity of a solution made by diluting 25.0 mL of 12 M hydrochloric acid to 250. mL?
7. What is the molality of a solution made by adding 93.4 grams of Zn(ClO 3)2 to 1000. grams of water?
What is the boiling point of this solution? (Kb for water = 0.52oC/m)
Part 3 – Solubility – Write (s) or (aq) next to each product. Then, write the net ionic equation.
8. ___ Mg(NO3)2 (aq) + ___ Na2O (aq)  ___ NaNO3 ( ) + ___ MgO ( )
9. ___ Zn(ClO3)2 (aq) + ___ K2CO4 (aq)  ___ KClO3 ( ) + ___ ZnCO3 ( )
EOC REVIEW #13
1. Given the reaction at equilibrium:
2 N2 (g) + O2 (g)  2 N2O (g)
(A) What is the equilibrium constant expression (Keq)?
(B) What is the value of Keq if [N2] = 5.22 M, [O2] = 2.91 M, and [N2O] = 3.75 M?
Use the information given below to answer questions 2 - 4.
Given the reaction at equilibrium:
2 A (g) + 3 B (g) + heat  C (g) + 3 D (g)
2. If the [B] increases...
(A) Which direction would the equilibrium shift?
(B) What would happen to the [A]?
(C) What would happen to the [C]?
(D) What would happen to the [D]?
(E) What would happen to the value of Keq?
3. If the temperature decreases...
(A) Which direction would the equilibrium shift?
(B) What would happen to the [A]?
(C) What would happen to the [B]?
(D) What would happen to the [C]?
(E) What would happen to the [D]?
(F) What would happen to the value of Keq?
4. If pressure increases...
(A) Which direction would the equilibrium shift?
(B) What would happen to the [A]?
(C) What would happen to the [B]?
(D) What would happen to the [C]?
(E) What would happen to the [D]?
(F) What would happen to the value of Keq?
EOC REVIEW #14
1. A standardized (known) 1.03 M solution of KOH is used to determine the concentration of an unknown
H2SO4 solution.
(A) What type of lab procedure would you use to determine the concentration (molarity) of the acid?
(B) If 50.0 mL of KOH is needed to neutralize 200.0 mL of H2SO4, what is the concentration of the acid?
2. Identify the acid (A), base (B), conjugate acid (CA), and conjugate base (CB) in the following reactions:
(A) NH3 + HBr  NH4+1 + Br-1
(B) H2O + NH2-1  NH3 + OH-1
3. What is the conjugate base of…
(A) HF
(B) H2O
(C) H2PO4-1
(D) HSO4-1
4. What is the conjugate acid of…
(A) Br-1
(B) H2O
(C) S-2
(D) HPO4-2
5. Fill in the following chart:
[H+1]
pOH
[OH-1]
pH
A, B, or N
2.29 x 10-6 M
2.04
4.03 x 10-9 M
11.29
6. What is the pH of a solution containing 0.020 M benzoic acid (C6H5COOH)? Benzoic acid is monoprotic and
has a Ka value of 6.6 x 10-5?
EOC REVIEW #15
1. Does the diagram represent an exothermic or
an endothermic reaction?
2. Which letter represents H?
3. Which letter represents Ea?
4. If a catalyst were added to this reaction, what
letters would change?
Use the following equation to answer # 5 – 8.
H2O (l) + energy  H2O (g)
5. Is this reaction exothermic or endothermic?
6. Is the value of H for this reaction positive or negative?
7. Is the value of S for this reaction positive or negative?
8. This reaction is ( sometimes / always / never ) spontaneous.
EOC REVIEW #16
1. If you start with 75.0 grams of Cs-137, how much time will pass before the amount remaining is 4.6875
grams? The half-life of Cs-137 is 30.17 years.
2. The half-life of Zn-71 is 2.4 minutes. If one had 100.0 g at the beginning, how many grams would be left after
7.2 minutes has elapsed?
3. After 24.0 days, 2.00 milligrams of an original 128.0 milligram sample remain. What is the half-life of the
sample?
4.
214
84
Po + 2
5. ______ +
6.
27
13
1
0
4
2
He + 2
n 
142
56
Al + ______ 
24
0
-1
e  ______
Ba +
11
91
Na +
36
Kr + 3
4
He
2
1
0
n
7. Identify the type of nuclear reaction and fuel used in most nuclear reactors.
EOC REVIEW #17
Given the following equation:
2 Na+1 (aq) + Ca (s)  Ca+2 (aq) + 2 Na (s)
1. What is the oxidation half-reaction?
2. What is the reduction half-reaction?
3. Which substance is oxidized?
4. Which substance is reduced?
5. Which substance is the oxidizing agent?
6. Which substance is the reducing agent?
7. Which element is the anode?
8. Which element is the cathode?