CHEMISTRY 1201, Lecture section 02 and
03
Problem supplement for the Final Exam
- SPRING 2002
I have included some of my new questions as well
as Dr. Chan's (Lecture section 1) E3 questions and Dr. Wright's (Lecture
section 4) E2 questions. I could not get my paws on their other tests. Sorry!
THIS IS NOT A
SAMPLE FINAL - too many questions!
Please review ALL of our lecture
exams (E1, E2, and E3) and all five HWs (esp. the last one since it did
not get tested on the last exam), and the recommended questions from the
textbook + the sample E1, E2 and E3 also available on the web. Also, please
read through Ch.13.1 - 13.5, and be familiar with the concepts.
TRY TO SOLVE THE PROBLEMS BEFORE ACCESSING THE
ANSWERS
!!!!!!!
Let me know if there are any problems, errors, too many correct answers
(there should be only one correct answer to each of the 75 questions).
You can email me at folga@lsu.edu
I am aware that on some platforms this test looks ugly - I cannot
correct formatting errors I do not see on my screen.
1. The temperature of 25oC is
in Kelvins.
a) 103 b)
138 c) 166
d) 248 e) 298
2. The freezing point of water at 1 atm pressure is .
a) 0oF
b) 0 K c) 0oC
d) -273oC
e) -32oF
4. You have to calculate the mass of a 30.0 mL liquid sample with density of 1.52 g/mL, but you have forgotten the formula. Which way of reasoning would help you in finding the correct mass?
a) if 1 mL of a liquid has the mass of 1.52g, then 30.0 mL has the mass of g.
b) if 1.52 mL of a liquid has the mass of 1 g, then 30.0 mL has the mass of g.
5. A wooden object has a mass of 10.782 g and occupies
a volume of 13.72 mL. What is the density of the object determined to
an appropriate number of significant figures?
a) 8 x 10-1 g/mL
b) 7.9 x 10-1 g/mL
c) 7.86 x 10-1 g/mL
d) 7.859 x 10-1 g/mL
e)
7.8586 x 10-1
g/mL
6. A strip of zinc metal weighing 2.00 g is placed in an aqueous solution containing 2.50 g of silver nitrate. Silver metal(s) and a solution of zinc nitrate is formed. How many grams of Ag(s) will form?
a) 2.00 b) 1.59 c) 0.98 d) 0.092 e) 0.0045
7. The atomic number indicates .
a) the number of neutrons in a nucleus
b) the total number of neutrons and protons in a nucleus
c) the number of protons or electrons in a neutral atom
d) the number of atoms in 1g of an element
e) the number of different isotopes of an element
8. Which atom has the smallest number of neutrons?
a) carbon-14
b) nitrogen-14
c) oxygen-16
d) fluorine-19
e) neon-20
9. Which atom has the largest number of neutrons?
a) phosphorous-30
b) chlorine-37
c) potassium-39
d) argon-40
e) calcium-40
10. Which compounds do not have the same empirical formula?
a) C2H 2 , C6H6
b) CO, CO2
c) C2H 4 , C3H6
d) C2H4 O 2 , C6H12O6
e) C2H 5 COOCH 3, CH3CHO
11. Which formula/name pair is incorrect?
| a) |
FeSO4 |
iron(II) sulfate |
| b) |
Fe2(SO3)3 |
iron(III)
sulfite |
| c) |
FeS |
iron(II)
sulfide |
| d) |
FeSO3 |
iron(II)
sulfite |
| e) |
Fe2(SO4)3 |
iron(III) sulfide |
12. Which formula/name pair is incorrect?
| a) |
NO |
nitrogen monoxide |
| b) |
N2O |
nitrogen
peroxide |
| c) |
NO2 |
nitrogen
dioxide |
| d) |
N2O5 |
dinitrogen
pentoxide |
| e) |
N2O3 | dinitrogen trioxide |
13. Which metal does not require to have its charge specified in the names of ionic compounds it forms?
a) Mn b) Fe
c) Cu d) Ca
e) Pb
14. Which metal does not form cations of differing charges?
a) Na b) Cu
c) Co d) Fe
e) Sn
15. In which reaction does the oxidation number of hydrogen change?
a) HCl(aq) + NaOH(aq) -->NaCl(aq) + H2O(l )
b) 2 Na(s) + 2 H2 O(l) --> 2 NaOH(aq) + H2(g)
c) CaO(s) + H2 O(l) --> Ca(OH) 2(s)
d) 2 HClO4(aq) + CaCO3(s) --> Ca(ClO4)2(aq) + H 2O( l ) + CO 2 (g)
e) SO2(g) + H2O(l) --> H2SO3(aq)
16. In which species does sulfur have the highest oxidation number?
a) S8 (elemental form of sulfur)
b) H2S
c) SO2
d) H2SO 3
e) K2SO 4
17. A tenfold dilution of a sample solution can be obtained
by taking
.
a)
1 part sample and
9 parts solvent
b) 1 part sample and 10 parts solvent
c) 9 parts sample and 1 part solvent
d) 10 parts sample and 1 part solvent
e) 99 parts sample and 1 part solvent
18. Which solution has the same number of moles of solute A as 50.00 mL of 0.100M solution of NaOH?
a) 20.00 mL of 0.200 M solution of A
b) 25.00 mL of 0.175M solution of A
c) 30.00 mL of 0.145 M solution of A
d) 50.00 mL of 0.125M solution of A
e) 100.00 mL of 0.0500 M solution of A
Consider the following electron configurations to answer the next
5 questions:
(i) 1s2 2s2 2p6 3s 2 3p6 4s2 3d10 4p6 5s 1
(ii) 1s2 2s2 2p6 3s2 3p 5
(iii) 1s2 2s2 2p6 3s2 3p 6 4s2 3d8
(iv) 1s2 2s2 2p6 3s2 3p 6 4s2 3d10 4p6
(v) 1s2 2s2 2p4 3s1
19. An example of an electron configuration of a transition metal is .
a) (i)
b) (ii)
c) (iii)
d) (iv)
e) (v)
20. An example of an excited state electron configuration for fluorine is .
a) (i)
b) (ii)
c) (iii)
d) (iv)
e) (v)
21. The ground state electron configuration of an element with the smallest number of valence electrons is .
a) (i)
b) (ii)
c) (iii)
d) (iv)
e) (v)
22. The ground state electron configuration of an element with the largest number of valence electrons is .
a) (i)
b) (ii)
c) (iii)
d) (iv)
e) (v)
23. An electron configuration of an element belonging to group VIIA (17) is .
a) (i)
b) (ii)
c) (iii)
d) (iv)
e) (v)
24. What is the wavelength of light with frequency of 3.22 x 1014 Hz?
a) 9.32 x 10-7 nm b) 932 nm c) 649 nm d) 1.07 x 10 6 nm e) 9.66 x 10 22 nm
25. How many different principal quantum numbers can be found in the ground state electron configuration of nickel?
a) 2
b) 3
c) 4
d) 5
e) 6
26. The three quantum numbers
for an electron in a hydrogen atom in a certain state are: n
=4, l=1, and m
l = 1. What type of
orbital is the electron located in?
a) 2s
b) 3s
c) 3d
d) 4p
e) 4d
27. In a many-electron
atom, which combination of quantum numbers n, l, ml
and m
s may correspond
to the thirty-seventh electron?
a) n = 3
l = 2
ml = 2
ms = 1
b) n = 4
l = 3
ml = 2
ms = 1/2
c) n = 4
l = 2
ml = -1
ms = -1/2
d) n = 5
l = 0
ml = 0
ms = 1/2
e) n = 5 l = 1 ml = 0 ms = -1/2
28. Which element would be expected to have chemical properties closest to those of fluorine?
a) S b) Fe c) Ne d) O e) Cl
29. Atomic radius generally increases as we move .
a) down the group and from right to left across a period.
b) Up a group and from left to right across a period.
c) Down a group and from left to right across a period.
d) Up a group and from right to left across a period.
e) Down a group. The period position has no effect.
30. Of the following elements, which has the largest first ionization energy?
a) B b) N c) P d) Si e) C
31. In general, as you go across a period in the periodic table from left to right: (1) the atomic radius ; (2) the electron affinity becomes negative; and (3) the first ionization energy .
a) decreases, decreasingly, increases
b) increases, increasingly, decreases
c) increases, increasingly, increases
d) decreases, increasingly, increases
e) decreases, decreasingly, decreases
32. Element M reacts with chlorine to form a compound with the formula Mc l 2. Element M is more reactive than magnesium and has a smaller radius than barium. This element is .
a) Sr b) K c) Na d) Ra e) Be
33. Of the following substances, is always produced when an active metal reacts with water.
a) NaOH b) H2O c) CO2 d) H2 e) O2
34. Oxides of most nonmetals combine with water to form .
a) an acid
b) a base
c) water and salt
d) water
e) hydrogen gas
35. The series that correctly lists from left to right a halogen, an alkaline earth metal, a transition metal, and an active metal is .
a) Cl, K, V, Mg
b) Br, Ba, Cr, Na
c) O, Ca, Ce, Al
d) F, Sr, Fe, Sn
e) S, Sr, Si, Sn
36. The halogens, alkali metals, and alkaline earth metals have valence electrons, respectively.
a) 2, 4, and 6
b) 1, 5, and 7
c) 8, 2, and 3
d) 7, 1, and 2
e) 2, 7, and 4
37. The only noble gas without 8 valence electrons is .
a) Ar
b) Ne
c) He
d) Kr
e) All noble gases have 8 valence electrons
38. Elements from opposite sides of the periodic table tend to form .
a) covalent compounds
b) ionic compounds
c) compounds that are gaseous at room temperature
d) homonuclear diatomic compounds
e) covalent compounds that are gaseous at room temperature
39. Which isoelectronic series is correctly arranged in order of increasing radius?
a) K+ < Ca 2+ < Ar < Cl-
b) Cl- < Ar < K + < Ca2+
c) Ca2+ < Ar < K+ < Cl-
d) Ca2+ < K + < Ar < Cl-
e) Ca2+ < K + < Cl- < Ar
40. A gaseous element reacts with Na to form a compound with the general formula NaX. This element is in group .
a) 4A b) 5A c) 6A d) 7A e) 1A
41. In the nitrite ion (NO2-), .
a) both bonds are single bonds
b) both bonds are double bonds
c) one bond is a double bond, and the other is a single bond
d) both bonds are the same, each being stronger and shorter than a single bond but weaker and longer than a double bond
e) there are 20 valence electrons
42. The central atom in violates the octet rule.
a) NH3
b) SeF2
c) BF3
d) AsF3
e) CF4
43. The central atom in must violate the octet rule or its Lewis structure could not be drawn at all.
a) ClF3
b) PCl3
c) SO3
d) CCl4
e) CO2
44. An electron domain is a .
1. lone pair
2. single bond
3. double bond
4. triple bond
5. central atom
a) 1 or 2
b) 1, 2, 3, or 4
c) 5 only
d) 2, 3, or 4
e) 1 or 5
45. Of the molecules below, only
is polar.
a) CCl4
b) CH4
c) SeF4
d) SiCl4
e) BF 3
46. When 3 atomic orbitals are mixed to form hybrid orbitals, how many hybrid orbitals are formed?
a) 1 b) 6 c) 3 d) 4 e) 5
Use the following list of covalent species
(i.e. molecules or ions) to answer the next FIVE
questions.
You may find it useful to draw the
best Lewis structures of the following species
first, i.e.: before attempting
to answer the questions. The central atom is shown in bold
.
a) H2O
b) CH4
c) H3O+
d) IF
5
e) ClF3
47. Which of the species with the sp3 hybridized central atom has the smallest bond angle?
48. Which species from the list above has the following properties?
- a square pyramidal shape
- an expanded octet on the central atom.
49. Which one species from the list above has the ideal tetrahedral angles?
50. From the table above, select a species with the following properties:
- molecular polarity
- two lone pairs of electrons on the central atom
51. Which species from the list above has a trigonal pyramidal shape?
* * *
52. The basis for the VSEPR model of molecular bonding is:
a) hybrid orbitals will form as closely as possible to achieve spherical symmetry
b) electron pairs (domains) will arrange themselves so as to minimize repulsions
c) atomic orbitals of the bonding atoms must overlap
d) regions of the electron density organize themselves as close as possible
53. The molecular geometry of XeCl4 is
a) tetrahedral
b) square pyramidal
c) octahedral
d) square planar
e) see-saw
54. The F-B-F bond angle in BF2- is .
a) 90o
b) somewhat less than 180o
c) 120o
d) somewhat less than 120o
e) 180o
55. Of the following, only is polar, and hence soluble in water.
a) CH3OH
b) SF6
c) BF3
d) CH4
e) CCl4
56. What is the hybridization of the central atom in a trigonal bipyramidal molecule?
a) sp3
b) sp4
c) sp5
d) sp3d
e) sp3d 2
57. Which statement about the chemical bonds is
false?
a) the shorter the X-X bond, the stronger the bond
b) the stronger the bond, the higher the bond enthalpy
c) double X=X bonds are longer than single X-X bonds
d) multiple bonds are stronger than single bonds
e) electrons is multiple bonds require more space than those in single bonds
58. The sp2 hybrid orbitals point towards the corners of a(n) .
a) equilateral triangle
b) tetrahedron
c) trigonal bipyramid
d) octahedron
e) pentagon
59. Which of the pairs of VSEPR electron domain arrangements (electronic geometries) and hybridizations is mismatched?
a) octahedral - sp
b) tetrahedral - sp3
c) trigonal bipyramidal - sp 3d
d) trigonal planar - sp 2
e) linear - sp
60. A gas originally at 300K and 1 atm pressure in a 3.9 L flask is cooled at constant pressure until the temperature is 11oC. The new volume of the gas is L.
a) 3.7
b) 0.27
c) 3.9
d) 4.1
e) 0.24
61. The density of N2O at 1.0 atm and 100K is g/L. (MM = 44.01 g/mol)
a) 1.0
b) 0.0227
c) 5.36
d) 0.187
e) 2.7 x 10-3
62. The volume of HCl(g), required to react with an excess of calcium metal to produce 44.8 L of hydrogen gas at 101325 Pa and 0oC is ............ L. Assume the same temperature and pressure conditions for HCl(g) as for the H2(g).
Ca(s) + 2 HCl(g) --> CaCl2(s) + H2(g)
a) 11.2 b) 22.4 c) 33.6 d) 44.8 e) 89.6
63. Standard temperature and pressure (STP), in the context of gases, refers to .
a) 298K and 1 atm
b) 273K and 1 atm
c) 298K and 1 torr
d) 273K and 1 Pa
e) 273K and 1 torr
64. Automobile air bags use the decomposition of NaN 3 as their sourse of gas for rapid inflation:
2 NaN3(s) --> 2 Na(s) + 3 N2(g)
What amount (moles) of NaN3 is required to provide 40.0L of N2 at 25oC and 760 torr?
a) 1.63
b) 1.08
c) 2.45
d) 1242.6
e) 827.4
65. Arrange the following gases in order of increasing average molecular speed (rms, u ) at 25oC.
He, F2, CO, NO
a) He < N2 < F2 < CO
b) He < F2 < NO < CO
c) CO < F2 < NO < He
d) F2 < NO < CO < He
e) CO < He < NO < F2
66. The root-mean square speed of CO at 113oC is
m/s.
a) 317
b) 58.2
c) 586
d) 993
e) 31.5
67. Crystalline solids .
a) have their particles arranged randomly
b) have highly ordered structures
c) are usually very soft
d) exist only at high temperatures
e) exist only at very low temperatures
68. Which of the following exhibits dipole-dipole interactions between molecules?
a) XeF4
b) AsH3
c) CO2
d) BCl3
e) Cl2
69. What intermolecular force is responsible for the fact that ice is less dense than water?
a) London dispersion forces
b) Ion-dipole interactions
c) Ionic bonding
d) Dipole-dipole interactions
e) Hydrogen bonding
70. CH4 molecules are attracted to one another by:
a) London dispersion forces
b) Ion-dipole interactions
c) Ionic bonding
d) Dipole-dipole interactions
e) Hydrogen bonding
71. Of the following,
has the highest
boiling point.
a) H2O
b) CO2
c) CH4
d) Kr
e) NH3
72. Of the following,
has the highest
boiling point.
a) KCl
b) H2O
c) H2S
d) H2Te
e) HBr