Download Atomic Structure Practice Answers

AP Chem
Test 5
1-36: 2 points each
36-39: 8 each
1. The ground state of Fe2+ is
A. 1s22s22p63s23p63d54s1
B. 1s22s22p63s23p63d6
C. 1s22s22p63s23p63d64s2
D. 1s22s22p63s23p63d84s2
E. 1s22s22p63d44s2
2. Which of these only contains atoms that are diamagnetic in their ground state?
A. Kr, Ca, P
B. Cl, Mg, Cd
C. Ar, K, Ba
D. He, Sr, C
E. Ne, Be, Zn
3. A valence electron from an arsenic atom might have the following set of quantum numbers in the
ground state.
A. 4,1,0,1/2
B. 4,1,2,-1/2
C. 3,1,0,1/2
D. 5,1,-1,-1/2
E. 4,2,1,1/2
4-7 refer to the following:
A.
B.
C.
D.
E.
1s21p62s22p3
1s22s22p63s23p64s23d104p65s24d1
1s22s22p63s23p63d3
1s22s22p5
1s22s22p63s23p64s23d104p6
4. The electron configuration of a halogen is: D
5. This is a possible configuration for a transition metal atom. B
6. This electron configuration is not possible. A
7. This is a possible configuration for a transition metal ion. C
8-11 refer to the following:
A.
B.
C.
D.
E.
Pauli exclusion principle
Electron shielding
The wave properties of matter
Heisenberg’s uncertainty principle
Hund’s rule
8. The exact position of an electron is not known. D
9. Oxygen atoms, in their ground state, are paramagnetic E
10. An atomic orbital can hold no more than 2 electrons A
11. The reason the 4s orbitals fill before the 3d. B
12. In the ground state, the highest energy electron of a rubidium atom might have which of the following
sets of quantum numbers?
A. 5,0,1,1/2
B. 5,1,1,1/2
C. 4,0,0,1/2
D. 5,0,0,1/2
E. 6,0,0,1/2
13. Calcium reacts with element X to form an ionic compound. If the ground state electron configuration
of X is 1s22s22p4 what is the simplest formula of this compound?
A. CaX
B. CaX2
C. Ca4X2
D. Ca2X2
E. Ca2X3
14. The differentiating electrons for transition elements are
A. d
B. s
C. p
D. f
E. valence electrons
15. How many electrons can be held in n=3?
A. 2
B. 8
C. 10
D. 18
E. 32
16. In which of the following pairs is the element with the higher ionization energy listed first?
A. Na, Cs
B. Te, Se
C. P, N
D. Ba, Sr
E. I, Br
17. In which of the following pairs is the first element expected to have a higher electronegativity than the
second?
A. O, P
B. Cs, Rb
C. I, Br
D. Al, P
E. Sb, As
18. A solid element has two valence electrons. It must be
A. a halogen
B. a noble gas
C. a radioactive element
D. an alkali metal
E. an alkaline earth metal
19. The number of protons, electrons, and neutrons in argon-40 is
A. 18e, 18p, 40n
B. 40e, 40p, 18n
C. 18e, 22p, 18n
D. 18e, 18p, 22n
E. 40e, 18p, 22n
20. Which is the least likely to have allotropes?
A. S
B. P
C. H
D. Se
E. Sn
21. Which of the following is expected to have the largest third ionization energy?
A. Be
B. B
C. C
D. N
E. Al
22. Which pair will have the most similar properties?
A. K and Li
B. S and P
C. Si and C
D. Sr and Ba
E. F and I
23. Most elements in the periodic table are
A. nonmetals
B. liquids
C. gases
D. metals
E. metalloids
24. How many protons, neutrons, and electrons are in a form of bromine?
A. 35p, 45n, 35e
B. 35p, 80n, 35e
C. 45p, 35n, 45e
D. 80p, 35n, 80e
E. Neutrons can’t be determined unless an isotope is specified.
25. Chemical properties of the elements are determined by the
A. electrons
B. ionization energy
C. protons
D. neutrons
E. electronegativity
26. In which pair is the larger atom listed first?
A. K, Ca
B. Na, K
C. Cl, S
D. Mg, Na
E. O, N
27. Which of the following is least likely to be a metalloid?
A. As
B. Hg
C. Ge
D. Si
E. Sb
28. Which of the following does not have the same level of shielding as the others?
A. Na
B. F
C. O
D. N
E. C
29. Which orbital type shields higher energy orbitals the most?
A. s
B. p
C. d
D. f
E. All are the same
30. Which type of orbital has the greatest penetration?
A. s
B. p
C. d
D. f
E. All are the same
31. Which is the smallest?
A. F
B. O
C. B
D. Ne
E. Li
32. Why is the answer to #31 the smallest?
A. It has less shielding
B. It has more penetration by its highest occupied orbital
C. It has less shielding and more penetration
D. It has the same shielding but more protons
E. It has less shielding and more protons
33. Which is a closer approximation to reality?
A. Dalton’s model
B. The Bohr model
C. The quantum mechanical model
D. All are equal
E. None are correct
34. Which quantum number specifies the energy level?
A. n
B. l
C. m
D. s
E. None
35. How many g orbitals are there?
A. 1
B. 3
C. 5
D. 7
E. 9
36. An electron
A. is a particle
B. is a wave
C. is both
D. is neither
E. has properties of both particles and waves
37. What is the frequency of light emitted when an electron goes from the 3s orbital of H to the 1s orbital?
What is the energy when an electron falls from 3p to 1s?
38. The energy required to break a C-C bond is about 350 kJ/mole. A particular violet photon has a
wavelength of 420nm. Can it break the bond? What about an ultraviolet photon with wavelength 150nm?
Show work.
39. Consider the following 4 ionization energies for aluminum:
Al = Al+ + eAl+ = Al2+ + eAl2+ = Al3+ + eAl3+ = Al4+ + ea.
b.
c.
d.
580kJ/mole
1815kJ/mole
2740kJ/mole
11,600kJ/mole
Account for the trend.
Explain the large increase between 3 and 4
Which ion has the greatest electron affinity? Explain
List the 4 in order of decreasing size. Explain your ordering.
40. One of the emission spectral lines for Be3+ has a wavelength of 253.4nm. This transition begins with
the electron in n=5. What energy level did the electron fall to?