CCMS Inorganic Chemistry 2012 Inorganic Chemistry
Mid-term Exam
Student ID :
1.
Name:
Grade:
What is the name of the energy that results from the interaction of charged particles?(2’)
A) thermal energy. B) kinetic energy. C) chemical energy. D) electrostatic energy.
E) charged energy.
2. Visible light, radio waves, microwave radiation, infrared, ultraviolet radiation, X-rays, and
gamma rays all constitute the electromagnetic spectrum. What similar characteristic do all
of these spectrums share? (2’)
A) They all have the ability to generate heat in objects.
B) They all have the same frequencies.
C) They are all the transmission of energy in the form of waves.
D) They have equal energies.
E) They have the same electron spin state.
3. A _________ is a point at which a standing wave has zero amplitude. (2’)
A) Crevice
B) Node
C) Pit
D) Burrow
E) Orbital
4.
The FM station KDUL broadcasts music at 99.1 MHz. Find the wavelength of these waves (c
= 3.0 ×108m/s). (2’)
A) 1.88 ×10–2 m
B) 0.330 m
C) 3.03 m
D) 5.33 ×102 m
E) > 103 m
5.
Atomic orbitals developed using quantum mechanics
. (2’)
A) describe regions of space in which one is most likely to find an electron.
B) describe exact paths for electron motion.
C) give a description of the atomic structure which is essentially the same as the Bohr
model.
D) allow scientists to calculate an exact volume for the hydrogen atom.
E) are in conflict with the Heisenberg Uncertainty Principle.
6. In the quantum mechanical treatment of the hydrogen atom, which one of the following
combinations of quantum numbers is not allowed? (2’)
A)
a
B) b
C) c
D) d
E) e
1 CCMS Inorganic Chemistry 2012 7.
What is element of Period 3 with the following successive IEs?
IE1=738 IE2= 1450
IE3=7732 IE4= 10,539 IE5= 13,628
A) Mg
B) Al
C) Si
D) P
E) S
(2’)
8. What is the maximum number of electrons in an atom that can have the following set of
quantum numbers? n = 4
l=3
ml = –2
ms = +1/2
(2’)
A) 0
B) 1
C) 2
D) 6
E) 10
9. A possible set of quantum numbers for the last electron added to complete an atom of
germanium in its ground state is
(2’)
n
l
ml ms
A 4
0
0
+1/2
B 3
0
+1 –1/2
C 4
1
–1 +1/2
D 3
1
+1 –1/2
E 4
2
+2 –1/2
A) A
B) B
C) C
D) D
E) E
10.
Which ground-state atom has an electron configuration described by the following orbital
diagram?
(2’)
[Ne] ↑↓
3s
A)
11.
phosphorus
↑
B)
↑
3p
nitrogen
↑ C) arsenic
D)
vanadium
How many unpaired electrons does a ground-state atom of sulfur have?
A) 0
B) 1
C) 2
D) 3
E) 4
E)
sulfur
(2’)
12. Which two electron configurations represent elements that would have similar chemical
properties? (1) 1s22s22p4 (2) 1s22s22p5 (3) [Ar]4s23d104p3
(4) [Ar]4s23d104p4 (2’)
A) (1) and (2)
B) (1) and (3)
C) (1) and (4)
D) (2) and (4)
E) (2) and
(3)
13. Arrange these ions in order of increasing ionic radius: K+, P3–, S2– , Cl–. (2’) A ) K+ < Cl– < S2– < P3–
B) K+ < P3– < S2– < Cl–
C) P3– < S2– < Cl– < K+
D) Cl– < S2– < P3– < K+
E) Cl– < S2– < K+ < P3–
14. Which of the following elements has the largest second ionization energy (IE2)? (2’)
A) Li
B) B
C) O
D) F
E) Na
15.
Which of these pairs consists of isoelectronic species?
A) Mn2+ and Ar
B) Zn2+ and Cu2+ C) Na+ and K+
2 (2’)
D) Cl– and S
E) K+ and Cl–
CCMS Inorganic Chemistry 2012 16.
For each of the following pairs, predict which species would have the higher first
(5’)
ionization potential.
(a) Na or Al
(b) Ca or Ba
(c) Br or Kr
(d) Fe or Cl
(e) C or N
17. Explain why atoms such as Cr and Cu do not have “regular” electron configurations. (5’)
18. Write complete electron configurations for the following ions:
(a) S2−
(b) Mg2+
(c) I−
(d) Cu+
(e) Mo2+
(f) Ni
(12’)
19. Write all the possible sets of four quantum numbers for electrons in the 5d subshell. (7’)
20. Briefly explain the following on the basis of electron configurations: (9’)
a. The most common ion formed by silver has a 1+ charge.
b. Cm has the outer electron configuration 5f76d17s2frather than 5f87s2.
c. Sn often forms an ion having a charge of 2+ (thestannous ion).
21. Sketch the 3pz and 4dxz hydrogen-like atomic orbitals, label their phases. (10’)
22. Suggest explanations for the following. (6’)
(a) High values of ionization energies are associated with the noble gases.
(b) In an Li atom in its ground state, the outer electron occupies a 2s rather than a 2p
orbital.
23. Consider the process of shielding in atoms, using Be as an example. What is being
shielded? What is it shielded from? What is doing the shielding? (6’)
24. Give the name or formula of the following compound. (10’)
Na2S
Ca(OH)2
CuSO4.5H2O
Co2(CO3)3
Fe3(PO4)2
Manganese(II) chlorate
Barium acetate
hydrogen cyanide
Lithium nitride
Potassium permanganate
3 CCMS Inorganic Chemistry 2012 Answer
1-5 DCBCA 6-10 EABCA 11-15
16.
(a) Al
(b) Ca
(c) Kr
CCAAE
(d) Cl
(e) N
17. Hund’s rule
18. (a) 1s22s22p63s23p6
(b) 1s22s22p6
(c) 1s22s22p63s23p64s23d104p65s64d105p6
(d) 1s22s22p63s23p64s24p63d10
(e) 1s22s22p63s23p64s23d104p64d4
(f) 1s22s22p63s23p63d84s2
19. (5,2,-2,+1/2) (5,2,-2,-1/2) (5,2,-1,+1/2) (5,2,-1,-1/2) (5,2,0,+1/2) (5,2,0,-1/2)
(5,2, 2,+1/2) (5,2, 2,-1/2) (5,2, 1,+1/2) (5,2, 1,-1/2)
20. (a) Ag [Kr]4d105s1 Ag+ [Kr]4d10
state.
(b) Hund’s rule
(c) Inert electron effect
21.
easy to lose the 5s electron to reach a more stable
(方向和相位)
22. (a) full-fill electron configuration
(b) E2s < E2p for Li atom
23. Nuclear is being shielded. 2s electron is shielded from and 1s electron is doing the
shielding.
24. calcium hydroxide; sodium sulfide; cobalt(III) carbonate;
copper (II) sulfate pentahydrate;
Iron(II) phosphate
Mn(ClO3)2
Li3N
HCN
KMnO4
Ba(C2H3O2)2
4