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Simulated Final Exam (SF15Gc1FF)
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1. What would be observed if the Thomson model was correct?
A. Alpha particles passing through foil with little to no deflection.
B. Electron capture, positron emitted
C. Alpha particles deflection with little to no pass through
D. Gamma radiation followed by photon release in the UV range
E. None of the above
2. Choose the correct answer for 56Fe2+
A. 26 protons, 30 neutrons, 26 electrons
B. 26 protons, 31 neutrons, 24 electrons
C. 26 protons, 30 neutrons, 24 electrons
D. 25 protons, 30 neutrons, 24 electrons
E. None of the above
3. Take the log of the energy (in joules) of a photon with a wavelength of 528 nm.
A. 3.76 x 10-19
B. -18.42
C. 18.42
D. 3.76 x 1019
E. None of the above
4. Calculate the wavelength in nm of hydrogen emitted photon from energy level (n) of 5 to an energy level (n) of 3.
A. 2813
B. 9611
C. 3.116 x 103
D. 1.283 x 103
E. None of the above
5. Nitrogen has how many electrons that are unpaired?
A. 2
B. 3
C. 4
D. 5
E. None of the above
6. Consider a hydrogen atom that has a principle quantum number of 2. What would be the total number of orbitals for
that shell?
A. 6
B. 5
C. 4
D. 3
E. None of the above
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7. Select the true statement
A. the magnetic quantum number is in reference to the spin of the electron
B. the magnetic quantum number depends on the orientation of the atom relative to the Earth’s magnetic poles NOT
its geographic poles.
C. the magnetic quantum number is in reference to the orbital’s orientation in space in comparison to the other
orbitals in the atom.
D. The identity of an atom is dictated by the number of electrons the atom possesses.
E. None of the above
8. Rank from largest to smallest atomic radius (Te, Sn, Sr).
A. Sn > Te > Sr
B. Sr > Sn > Te
C. Te > Sn > Sr
D. Te > Sr > Sn
E. None of the above
8. Rank from largest to smallest atomic radius (Sn, Te, Sr).
A. Sn > Te > Sr
B. Sr > Sn > Te
C. Te > Sn > Sr
D. Te > Sr > Sn
E. None of the above
9. Rank the given by ionization energy (smallest to largest)
O, Na, F, C, Li
A.
B.
C.
D.
E.
Li < O < Na < C < F
F < C < Li < O < Na
Na < Li < C < O < F
F < O < C < Li < Na
None of the above
10. Choose Calcium Permanganate
A. Ca(MnO4)2
B. Ca(C2H3O2)2
C. Ca(KMnO4)2
D. Ca(C8H10N4O2)
E. None of the above
11. 48.81 grams of HCl corresponds with how many moles?
A. 1.08
B. 1.34
C. 2.11
D. 1.43
E. None of the above
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12. Select the ion with 1s22s22p63s23p6 configuration
A. Ar
B. FC. Ca2+
D. Au
E. None of the above
13. Select the number of lone pairs on iodine in ICl4+
A. 3
B. 2
C. 1
D. 0
E. None of the above
14. What is the name for I2O7
A. Iodine perhepoxide
B. Diiodine heptoxide
C. Diiodine perheptoxide
D. Diiodine heptamonoxide
E. None of the above
15. Select the molecular geometry for NCl3
A. Trigonal Planar
B. Tetrahedral
C. Pyramidal
D. Linear
E. None of the above
16. Select the one with polar bonds but is nonpolar
A. PCl5
B. CH4
C. O2
D. NH3
E. None of the above
17. What is the hybridization of I in IF5
A. sp3d3
B. sp3d2
C. sp3d
D. None of the above
18. What is the hybridization of I in IF3
A. sp3d3
B. sp3d2
C. sp3d
D. None of the above
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19. Matter has only particle or only wave properties, true or false?
20. Given the data for the compound (MX2), calculate the lattice energy.
IE + IE (M) = 1,514 kJ/mol
M(s)  M(g) ΔH = 75.1 kJ/mol
ΔH (MX ) = -1,304 kJ/mol
X (g)  2X(g) ΔH = 229 kJ
EA (X) = -329 kJ/mol
IE (X) = 271 kJ/mol
1
2
o
o
f
2
2
1
21. Cl-37 and Cl-35 make up the atomic mass for Cl (35.5 amu) seen on the periodic table. Find the percentages of each.
A. 55, 45, respectively
B. 25, 75, respectively
C. 50, 50, respectively
D. 5, 100, respectively
E. None of the above
22. Find the empirical formula for a compound that is composed of hydrogen (12.5% by mass) and nitrogen (87.5% by
mass)
23. Given the reaction below, how many moles of NH3 is made with infinite N2 and 1.029 moles of hydrogen?
N2 (g) + 3H2 (g)  2NH3
24. Ionic compounds that are soluble and have OH- are called
A. Strong
B. Strong Bases
C. Strong Acids
D. Acids
E. None of the above
25. Calculate the concentration of Na2CO3 if 2.609 g is dissolved in water to make a 2.5 x 102 mL solution
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26. What is the oxidation number of S in Na2SO4?
A. 4
B. 6
C. 8
D. 10
E. None of the above
27. Find the specific heat capacity for a substance if it takes 42.6 J to heat 1.98 grams of it at an initial temperature of
30° C to 60 ° C
28. Find ΔH for the reaction and data given below if 2.659 g of H2O is produced
H2(g) + 1/2O2(g)  H2O(l)
ΔH = -285.9 kJ/mol
29. Hydrogen gas effuses in 2.419 minutes. Gas X of equal volume and conditions effuses in 11.098 mins. Find the mm of
the gas X.
30. True or false: Intramolecular bonds are weaker than intermolecular forces
31. Find the ratio of mass (grams) and volume (liters) of CFCl3 at 342 torr and 28.95 ° C.
32. Find the volume of gas if pressure is one-third of the original pressure. (original vol = 31.95 L, original pressure =
161.106 kPa)
33. Give the bond order of O2+
A. 0
B. 0.5
C. 1
D. 2.5
E. None of the above
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34. Give an estimated normal melting point from the phase diagram below.
F. 18 ° C
G. 291 K
H. 75 ° C
I. 303 K
J. None of the above
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