Download Final Exam Review

Final Exam Review 2014
Ch.3 Scientific Measurement: pg. 96 (74, 79)
74. Make the following conversions:
A. 157 cs to seconds
B. 42.7 L to milliliters
C. 261 nm to millimeters
D. 0.065 km to decimeters
E. 642 cg to kilograms
F. 8.25 x 102 cg to nanograms
79. Rank these numbers from smallest to largest:
A. 5.3 x 104
B. 5.7 x 103
C. 4.9 x 10-2
D. 0.0057
E. 5.1 x 10-3
F. 0.0072 x 102
Ch.17 Thermochemistry: pg. 586 (61, 74)
61. Explain why ice melts in at 0 ͒C without an increase
of temperature, even though heat flows from the
surroundings to the system (the ice).
74. A 1.55-g piece of stainless steel absorbs 141 J of
heat when its temperature increase by 178 ͒C. What
is the specific heat of the stainless steel?
Ch.4 Atomic Structure: pg. 115 #21, pg. 119 #34, pg. 122 #51
21. Three Chromium isotopes are Chromium-50, Chromium-52, and
Chromium-53. How many neutrons are in each isotope, given that
Chromium has an atomic number of 24?
34. List the number of protons, neutrons, and electrons in each pair of
isotopes.
A. 63 Li, 73 Li
B. 4220Ca, 4410Ca
C. 7834 Se, 8034Se
51. Complete the following table:
# of Electrons
10
# of Protons
Mass #
B.______
A.______
15
25
14
F.______
H.______
25
Ch.5 Electrons in Atoms: pg. 153 #59, pg. 157 #1-14
59. An atom of an element has two electrons in the first
energy level and five electrons in the second energy
level. Write the electron configuration for this atom and
and name the element. How many unpaired electrons does
an atom of this element have?
1. Select the correct electron configuration for silicon, atomic number 14.
A. 1s2 2s2 2p2 3s2 3p2 3d2 4s2
B. 1s2 2s2 2p4 3s2 3p4
C. 1s2 2s6 2p6
D. 1s2 2s2 2p6 3s2 3p2
2. Which two orbitals have the same shape?
A. 2s and 2p
B. 2s and 3s
C. 3p and 3d
D. more than one is correct.
3. Which of these statements characterize the nucleus of every atom?
I. It has a positive charge.
II. It is very dense.
III. It is composed of protons, electrons, and neutrons.
A. I and II only
B. II and III only
C. I and III only
D. I, II, and III
4. As the wavelength of light increases...
A. the frequency increases
B. the speed of light increases
Atomic #
9
D.______
C.____
47
E.____
55
G.____
C. the energy decreases
D. the intensity increases
5. In the third energy level of an atom...
A. there are two energy sublevels
B. the f sublevel has 7 orbitals
C. there are 3 s orbitals
D. a maximum of 18 electrons are allowed
Letter choices for 6-10
A. s2 p6
B. s2 p2
C. s2
D. s4 p1
E. s2 p4
Which configuration is the configuration of the highest
occupied energy level for each of these elements?
6. sulfur
7. germanium
8. beryllium
9. krypton
10. strontium
Use the drawings to answer 11-14; each represents
an electromagnetic wave.
A.
B.
C.
11. Which wave has the longest wavelength?
12. which wave has the highest energy?
13. which wave has the lowest frequency?
14. which wave has the highest amplitude?
Ch.6 Organizing the Elements: pg. 187 #30,31,51, pg. 190 #88
30. Identify each property below as more characteristic of a metal or a nonmetal.
A. a gas at room temperature
B. brittle
C. malleable
D. poor conductor of electric current
E. shiny
31. In general, how are metalloids different from metals and nonmetals?
51. In which pair of elements are the chemical properties of the elements most
similar? Explain your reasoning.
A. sodium and chlorine
B. nitrogen and phosphorous
C. boron and oxygen
88. The volume of a liquid in a graduated cylinder is reported as 31.8 mL.
A. How many significant figures are there in this measurement?
B. In which digit is there uncertainty?
Ch.7 Ionic and Metallic Bonding: pg.214 #28,32,67
28. To which group on the periodic table does each of the following
elements belong? How many valence electrons do atoms of
each element have?
A. nitrogen
B. lithium
C. phosphorous
D. barium
E. bromine
F. carbon
32. write the symbol for the ion formed when each of the following elements
loses its valence electrons.
A. aluminum
B. lithium
C. barium
D. potassium
E. calcium
F. strontium
67. Which of the following compounds are most likely not ionic?
A. H2O
B. Na2O
C. CO2
D. CaS
E. SO2
F. NH3
Ch.8 Covalent Bonding: pg. 256 #39,43,77,110, pg.261 #6
39. The melting point of a compound is 1240 ͒C. Is this compound most likely an
ionic compound or a molecular compound?
43. Identify the phrases that generally apply to molecular compounds:
A. contain metals and nonmetals
B. are often gases or liquids
C. have low melting points
D. contain ionic bonds
E. use covalent bonding
77. What is the geometry around the central atom in each of these simple molecules?
A.
B.
C.
D.
110. Which of these statements about the periodic table is correct?
I. Elements are arranged in order of increasing mass
II. A period is a horizontal row
III. Nonmetals are located on the right side of the table
A. I only
B. I and II only
C. I, II, and III
D. I and III only
E. II and III only
6. Draw the electron dot structure for each example molecule.
example
molecular shape
arrangement of
electron pairs
non-bonding pairs
bonding pairs
CH4
tetrahedral
tetrahedral
0
4
NCl3
pyramidal
tetrahedral
1
3
H2S
bent
tetrahedral
2
2
HF
linear
tetrahedral
3
1
Ch.9 Chemical Names and Formulas: pg. 299 #80,81
80. Write formulas for these compounds:
A. potassium permanganate
B. calcium hydrogen carbonate
C. dichlorine heptoxide
D. trisilicon tetranitride
E. sodium dihydrogen phosphate
F. phosphorus pentabromide
81. Write formulas for these compounds:
A. magnesium sulfide
B. sodium phosphite
C. barium hydroxide
D. copper (II) nitrite
E. potassium sulfite
F. calcium carbonate
G. sodium bromide
H. ferric sulfate
Ch.10 Chemical Quantities: pg. 327 #35, pg. 338 #54, 65,111,116,122,pg. 343 #2,
35. calculate the percent by mass of nitrogen in these fertilizers:
A. NH3
B. NH4NO3
54. find the number of moles in each substance:
A. 2.41 x 1024 formula units of NACl
B. 9.03 x 1024 formula units of Hg
C. 4.65 x 1024 molecules of NO2
65. how many moles is each of the following:
A. 15.5 g SiO2
B. 0.0688 g AgCl
C. 79.3 g Cl2
D. 5.96 g KOH
E. 937 g Ca( C2H3O2)2
F. 0.800 g Ca
111. classify each of the following as a physical change or a chemical change:
A. an aspirin tablet is crushed to a powder
B. a red rose turns brown
C. grape juice turns to wine
D. fingernail polish remover evaporates
E. a bean seed sprouts
F. a piece of copper is beaten into a thin sheet
116. how many protons, electrons, and neutrons are in each isotope?
A. zirconium-90
B. palladium-108
C. bromine-81
D. antimony-123
122. draw electron dot structures and predict the shapes of the following molecules:
A. PH3
B. CO
C. CS2
D. CF4
2. calculate the molar mass of ammonium phosphate, (NH4)3 PO4
A. 113.0 g/mol
B. 121.0 g/mol
C. 149.0 g/mol
D. 242.0 g/mol
Ch.11 Chemical Reactions: pg. 377#41,43, pg.380 #75
41. write a balanced equation for each of the following double- replacement reactions:
A. H2C2O4(aq) + KOH (aq) →
B. CdBr2(aq) + Na2S(aq) →
43. balance each equation and identify its type:
A. Hf(s) + N2(g) → Hf3N4(s)
B. Mg(s) + H2SO4(aq) → MgSo4(aq) + H2(g)
C. C2H6(g) + O2(g) → CO2(g) + H2O(g)
D. Pb(NO3)2(aq) + NaI(aq) → PbI2(s) + NaNO3(aq)
75. calculate the number of moles in each substance:
A. 54.0 L of nitrogen dioxide (at STP)
B. 1.68 g of magnesium ions
C. 69.6 g of sodium hypochlorite
D. 4.27 x 1024 molecules of carbon monoxide
Ch. 12 Stoichiometry: pg. 411 #47c. pg. 416 #102, pg. 417 #1
47c. How many grams of N2F4 can be produced from 225 g F2?
102. how many moles is each of the following:
A. 47.8 g KNO3
B. 2.22 L SO2 (at STP)
C. 2.25 x 1022 molecules PCL3
1. nitric acid is formed by the reaction of nitrogen dioxide with water.
3NO2(g) + H2O(l) → NO(g) + 2HNO3(aq)
How many moles of water are needed to react with 8.4 mol NO2
A. 2.8 mol
B. 3.0 mol
C. 8.4 mol
D. 25 mol
Ch. 14 The Behavior of Gases: pg.480 #49, pg.484 #123
49. describe what happens to the volume of a balloon when it
is taken outside on a cold winter day. explain why the
observed change happens
123. use the drawings to explain how gas pressure is produced.
Ch. 19 Acids, Bases, and Salts: pg.652 #6, pg. 662 #18,19, pg.675 #39,42
6. how are the properties of acids and bases similar? how are they different?
18. how are the concentrations of hydrogen ions and hydroxide ions related
in an aqueous solution?
19. what is the range of pH values in the following solutions:
A. basic
B. acidic
C. neutral
39. what are the products of a reaction between an acid and a base?
42. write balanced equations for the following acid-base reactions:
A. H2SO4 (aq) + KOH (aq) →
B. H3PO4 (aq) + Ca(OH)2 (aq) →
C. HNO3 (aq) + Mg(OH)2 (aq) →