Miami Chemistry Electrons Configuration & Levels Multiple Choice Questions chemistry……………………………………………………………..

Miami Chemistry Electrons Configuration & Levels Multiple Choice Questions chemistry……………………………………………………………… 1. Which of the following is the correct electron configuration for Zn2+?
A. 1s22s22p63s23p64s03d10
B. 1s22s22p63s23p64s23d8
C. 1s22s22p63s23p64s23d10
D. 1s22s22p63s23p64s03d8
2. Which of the following quantum number sets is possible?
A. n = 2; l = 2; ml = 1;
B. n = 2; l = 1; ml = -1;
C. n = 2; l = 0; ml = -1;
D. n = 2; l = 0; ml = 1;
3. What is the maximum number of electrons allowed in a single atomic energy level
in terms of the principal quantum number n?
A. 2n
B. 2n + 2
C. 2n2
D. 2n2 + 2
4. Which of the following equations describes the maximum number of electrons
that can fill a subshell?
A. 2l + 2
B. 4l + 2
C. 2l2
D. 2l2 + 2
5. Which of the following atoms only has paired electrons in its ground state?
A. Sodium
B. Iron
C. Cobalt
D. Helium
6. An electron returns from an excited state to its ground state, emitting a photon
at ? = 500 nm. What would be the magnitude of the energy change if one mole of
these photons were emitted? (Note: h = 6.626 × 10-34 J·s)
A. 3.98 × 10-21 J
B. 3.98 × 10-19 J
C. 2.39 × 103 J
D. 2.39 × 105 J
7. Suppose an electron falls from n = 4 to its ground state, n = 1. Which of the
following effects is most likely?
A. A photon is absorbed.
B. A photon is emitted.
C. The electron moves into a p-orbital.
D. The electron moves into a d-orbital.
8. Which of the following isotopes of carbon is LEAST likely to be found in nature?
A. 6C
B. 12C
C. 13C
D. 14C
9. Which of the following best explains the inability to measure position and
momentum exactly and simultaneously according to the Heisenberg uncertainty
A. Imprecision in the definition of the meter and kilogram
B. Limits on accuracy of existing scientific instruments
C. Error in one variable is increased by attempts to measure the other
D. Discrepancies between the masses of nuclei and of their component particles
10. Which of the following electronic transitions would result in the greatest gain in
energy for a single hydrogen electron?
A. An electron moves from n = 6 to n = 2.
B. An electron moves from n = 2 to n = 6.
C. An electron moves from n = 3 to n = 4.
D. An electron moves from n = 4 to n = 3.
11. Suppose that an atom fills its orbitals as shown:
Such an electron configuration most clearly illustrates which of the following laws
of atomic physics?
A. Hund’s rule
B. Heisenberg uncertainty principle
C. Bohr model
D. Rutherford model
12. How many total electrons are in a
A. 54
B. 55
C. 78
D. 133
13. The atomic weight of hydrogen is 1.008 amu. What is the percent composition
of hydrogen by isotope, assuming that hydrogen’s only isotopes are 1H and 2D?
A. 92% H, 8% D
B. 99.2% H, 0.8% D
C. 99.92% H, 0.08% D
D. 99.992% H, 0.008% D
14. Consider the two sets of quantum numbers shown in the table, which describe
two different electrons in the same atom.
n l ml ms
2 1 1 +1/2
3 1 -1 +1/2
Which of the following terms best describes these two electrons?
A. Parallel
B. Opposite
C. Antiparallel
D. Paired
15. Which of the following species is represented by the electron configuration
I. Cr
II. Mn+
III. Fe2+
A. I only
B. I and II only
C. II and III only
D. I, II, and III
16. Which of the following best describes ionic compounds?
A. Ionic compounds are formed from molecules containing two or more atoms.
B. Ionic compounds are formed of charged particles and are measured by molecular
C. Ionic compounds are formed of charged particles that share electrons equally.
D. Ionic compounds are three-dimensional arrays of charged particles.
17. Which of the following compounds has a formula weight between 74 and 75
grams per mole?
A. KCl
B. C4H10O
C. MgCl2
D. BF3
18. Which of the following is the gram equivalent weight of H2SO4 with respect to
A. 49.1 g
B. 98.1 g
C. 147.1 g
D. 196.2 g
19. Which of the following molecules CANNOT be expressed by the empirical
formula CH?
A. Benzene
B. Ethyne
20. In which of the following compounds is the percent composition of carbon by
mass closest to 62 percent?
A. Acetone
B. Ethanol
C. C3H8
D. Methanol
21. What is the most specific characterization of the reaction shown?
Ca(OH)2 (aq) + H2SO4 (aq) ? CaSO4 (aq) + H2O (l)
A. Single-displacement
B. Neutralization
C. Double-displacement
D. Oxidation–reduction
22. In the reaction shown, if 39.05 g of Na2S are reacted with 113.3 g of AgNO3, how
much of the excess reagent will be left over once the reaction has gone to
Na2S + 2 AgNO3 ? Ag2S + 2 NaNO3
A. 13.0 g Na2S
B. 26.0 g Na2S
C. 41.4 g AgNO3
D. 74.3 g AgNO3
23. Using a given mass of KClO3, how would one calculate the mass of oxygen
produced in the following reaction, assuming it goes to completion?
2 KClO3 ? 2 KCl + 3 O2
24. Aluminum metal can be used to remove tarnish from silver when the two solid
metals are placed in water, according to the following reaction:
3 AgO + 2 Al ? 3 Ag + Al2O3
This reaction is a:
I. double-displacement reaction.
II. single-displacement reaction.
III. oxidation–reduction reaction.
IV. combination reaction.
A. II only
B. IV only
C. I and III only
D. II and III only
25. Which of the following types of reactions generally have the same number of
reactants and products?
I. Double-displacement reactions
II. Single-displacement reactions
III. Combination reactions
A. I only
B. II only
C. I and II only
D. II and III only
26. A reaction that utilizes oxygen and hydrocarbons as reactants and that produces
carbon dioxide and water as products is best characterized as:
A. single-displacement.
B. combustion.
C. metathesis.
D. decomposition.
27. In the process of photosynthesis, carbon dioxide and water combine with energy
to form glucose and oxygen, according to the following equation:
What is the theoretical yield of glucose if 30 grams of water are reacted with excess
carbon dioxide and energy, according to the equation above?
A. 30.0 g
B. 50.0 g
C. 300.1 g
D. 1801 g
28. In the following reaction:
Au2S3 (s) + H2 (g) ? Au (s) + H2S (g)
If 2 moles of Au2S3 (s) is reacted with 5 moles of hydrogen gas, what is the limiting
A. Au2S3 (s)
B. H2 (g)
C. Au (s)
D. H2S (g)
29. Which of the following would make the strongest electrolytic solution?
A. A nonpolar covalent compound with significant solubility.
B. A ionic compound composed of one cation with +3 charge and three anions with
-1 charge.
C. A polar covalent compound with a small dissociation constant.
D. An ionic compound composed of two cations with +1 charge and one anion with
-2 charge.
30. What is the molecular formula of a compound with an empirical formula of B2H5
and a molar mass of 53.2 g/mol?
A. B2H5
B. B3H7
C. B4H10
D. B6H15
31. Chlorine has two isotopic forms,
amu and is 75.53% abundant in nature.
and 37Cl.
has a relative mass of 34.97
has a relative mass of 36.97 amu and
is 24.47% abundant in nature. Calculate the atomic mass of chlorine.
32. Determine the molarity of the following samples.
a) 4.35 moles of KMnO4 are dissolved in enough water to give a 750 mL solution.
b) 20.0 g of NaOH are dissolved in enough water to give a 1.50 L solution
33. A sample of N2 gas occupies 1.62 L at 755 mm Hg and 0 oC. What volume, in
liters, will the gas occupy at 725 mm Hg and 50 oC?

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