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Bài tập Hóa học bằng Tiếng Anh môn Hóa học đại cương | Trường Đại học Nông Lâm thành phố Hồ Chí Minh

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Bài tập Hóa học bằng Tiếng Anh môn Hóa học đại cương | Trường Đại học Nông Lâm thành phố Hồ Chí Minh. Tài liệu giúp bạn tham khảo, ôn tập và đạt kết quả cao. Mời đọc đón xem!

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Home exercises
Part 1
1. The wavelength of the green light from a traffic signal is centered at 522 nm. What is the
frequency of this radiation?
2. Calculate the energy (in joules) of
a) a photon with a wavelength of 5.00x10
4
nm (Infrared region)
b) a photon with a wavelength of 5.00x10
-2
nm.
3. The energy of a photon is 5.87x10
-20
J. What is the wavelength (in nanometers)?
4. What is the wavelength of a photon emitted during a transition from the n
i
=5 state to the n
f
= 2
in the hydrogen atom?
5. Calculate the wavelength in the following two cases:
* The wavelength of an electron traveling at 1.24x10
7
m/s. m
e
= 9.1x10
-31
kg
* The wavelength of a baseball of mass 149g traveling at 41.3m/s.
6. Calculate the wavelength of the “particle” in the following two cases:
a) The fastest serve in tennis is about 62 m/s. Calculate the wavelength associated with a
6.0x10
-2
kg tennis ball traveling at this velocity
b) Calculate the wavelength associated with an electron moving at 62 m/s.
7. How many individual orbitals are there in the third shell? Write out n, l, m
l
quantum numbers
for each one and label each set by the s, p, d, f designations.
8. Describe the characteristics of an s orbital, a p orbital, and a d orbital. Which of the following
orbitals do not exist: 1p, 2s, 2d, 3p, 3d, 3f, 4g?
9. What is the maximum number of electrons in an atom that can have the
following quantum numbers? Specify the orbitals in which the electrons
would be found. (a) n = 2, m
s
= +1/2; (b) n=4, m
l
= +1; (c) n=3, l =2; (d) n=2, l=0, m
s
=
+1/2; (e) n=4, l =3, m
l
=-2
10. An electron in a certain atom is in the n=2 quantum level. List the possible values of l and m
l
that it can have.
11. List all the possible subshells and orbitals associated with the principle quantum number n, if
n=5.
12. Indicate which of the following sets of quantum numbers in an atom are unacceptable and
explain why:
(a) (1,0,1/2,1/2) (b) (3,0,0,+1/2) (c) (2,2,1,+1/2)
(d) (4,3,-2,+1/2) (e) (3,2,1,1,)
13. Indicate the number of unpaired electrons present in each of the following atoms: B (Z=5),
Ne (Z=10), P (Z=15), Sc (Z=21), Mn (Z=25), Se (Z=34), Kr (Z=36), Fe (Z=26), I (Z=53), Pb
(Z=82), Cd (Z=48).
14. Draw the shapes (boundary surfaces) of the following orbitals: a) 2p
y
; b) 3
d
Z
2
; c) 3d
x
2
− y
2
15. Draw orbital diagrams for atoms with the following configuration:
a) 1s
2
2s
2
2p
5
b) 1s
2
2s
2
2p
6
3s
2
3p
3
c) 1s
2
2s
2
2p
6
3s
2
3p
6
4s
2
3d
7
16. The ground-state electron configurations listed here are incorrect. Explain what mistakes
have been made in each and write the correct electron configurations
Al: 1s
2
2s
2
2p
4
3s
2
3p
3
B: 1s
2
2s
2
2p
5
F: 1s
2
2s
2
2p
6
17. Without referring to a periodic table, write the electron configuration of the elements with
the following atomic numbers: a) 9; b) 20; c) 26; d) 33. Classify the elements.
18. Specify the group of the periodic table in which each of the following elements is found: a)
[Ne] 3s
1
, b) [Ne]3s
2
3p
3
, c) [Ne]3s
2
3p
6
, d) [Ar]4s
2
3d
8
19. A M
2+
ion derived from a metal in the 1
st
transition metal series has four electrons in the 3d
subshell. What element might M be?
20. In general, ionization energy increases from left to right across a given period. Aluminum,
however, has a lower ionization energy than magnesium. Explain.
21. Two atoms has the electron configurations 1s
2
2s
2
2p
6
and 1s
2
2s
2
2p
6
3s
1
. The first ionization
energy of one is 2080 KJ/mol, and that of the other is 496 KJ/mol. Match each ionization
energy with one of the given electron configurations. Justify your choice ?
22. A hydrogenlike ion is an ion containing only one electron. The energies of the electron in a
hydrogenlike ion are given by
E
n
=−(2. 18 x 10
−18
J )Z
2
(
1
n
2
)
Where n is the principle quantum number and Z is the atomic number of the element.
Calculate the ionization energy of the He
+
ion.
23. From the following data, calculate the average bond energy for the N-H bond:
NH
3
(g) NH
2
(g) + H(g) H
o
= 435KJ
NH
2
(g) NH(g) + H(g) H
o
= 381 KJ
NH(g) N(g) + H(g) H
o
= 360 KJ
24. The energy needed for the following process is 1.96x10
4
KJ.mol
-1
:
Li(g) Li
3+
(g) + 3e
-
If the first ionization energy for lithium is 520 kJ/mol
-1
, calculate the second ionization
energy of lithium, that is, the energy required for the process
Li
+
(g) Li
2+
(g) + e
-
(Use the equation:
E
n
=−(2. 18 x 10
−18
J )Z
2
(
1
n
2
)
)
25. According to VB theory, explain, why the nitrogen atom cannot have pentavalence, while the
phosphorus has.
26. Determine and explain all possible valences of the following atoms: S, Cl, C.
27. Draw a Lewis formula for the following species: H
2
O, H
3
O
+
, NF
3
, OF
2
, BF
3
, [BF
4
]
-
, SF
4
, SF
6.
28. What is the hybridization of the central atom in each of the following: NCl
3
, CF
4
, SF
6
, NH
3
,
NH
4
+
.
29. What hybridizations are predicted for the central atoms in the following molecules:
H
2
O H
2
S H
2
Se H
2
Te
104.5
o
92.2
o
91
o
89.5
o
Why the bond angles decrease by the above order?
30. Predict geometry of the following molecules: H
2
O, H
3
O
+
, CH
4
, CO
2
, SO
2
, BF
3
.
31. Describe the hybridization of N in each of these species:
i) NH
3
; ii) NH
4
+
; iii) H
¨
N
=
¨
N
H; iv) ; v) H
2
¨
N
-
¨
N
H
2
32. What change in hybridization occurs in the following reaction?
NH
3
+ BF
3
→H
3
N: BF
3
31. Briefly discuss the bond angles in the hydroxylamine molecule in terms of the ideal geometry
and the small changes caused by electron-pair repulsions.
32. Use the appropriate milecular orbital energy diagram to write the electron configuration for
each of the following; calculate the bond order of each, and predict which would exist (a)
H
2
+
; (b) H
2
; (c) H
2
-
; (d) H
2
2-
.
33. Repeat exercise 32 for (a) He
2
+
; (b) He
2
; (c) He
2
2+
34. Repeat exercise 32 for (a) N
2
; (b) Ne
2
; (c)C
2
2-
35. Repeat exerice 32 for (a) Li
2
; (b) Li
2
+
; (c) O
2
2-
36. Use the appropriate molecular orbital energy diagram to write electron configurations of the
following molecules and ions: (a) Be
2
, Be
2
+
, Be
2
-
; (b) B
2
, B
2
+
, B
2
-
.
37. Use the preceding diagram to fill in an MO diagram for NO
-
, what is the bond order of NO
-
?
It is paramagnetic? How would you assess its stability?
38. Repeat exercise 37 for NO
+
39. Repeat exercise 37 for CN
+
. Refer to the preceding diagram but assume that the
2px
2py
MOs
are lower in energy than the 2σ
p
MO.
40. Explain why ionization energies of molecules H
2
, N
2
, C
2
, CO higher than those of the
corresponding atoms ?
H C N O F
I
1
(KJ.mol
-1
) 1308 1083 1396 1312 1675
H
2
C
2
N
2
O
2
F
2
I
1
(KJ.mol
-1
) 1488 1154 1507 1173 1526
41. Compare dipole moment of the following molecules: NH
3
and NF
3
and explain?
42. Do the following molecules have dipole moment ? Explain?
F
2
; BeF
2
; BF
3
; CF
4
; CO
2
; SO
2

Tài liệu khác của Trường Đại học Nông Lâm thành phố Hồ Chí Minh

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Home exercises

Part 1

  1. The wavelength of the green light from a traffic signal is centered at 522 nm. What is the frequency of this radiation?
  2. Calculate the energy (in joules) of
    1. a photon with a wavelength of 5.00x104 nm (Infrared region)
    2. a photon with a wavelength of 5.00x10-2 nm.
  3. The energy of a photon is 5.87x10-20 J. What is the wavelength (in nanometers)?
  4. What is the wavelength of a photon emitted during a transition from the ni=5 state to the nf = 2 in the hydrogen atom?
  5. Calculate the wavelength in the following two cases:

* The wavelength of an electron traveling at 1.24x107 m/s. me = 9.1x10-31 kg

* The wavelength of a baseball of mass 149g traveling at 41.3m/s.

6. Calculate the wavelength of the “particle” in the following two cases:

a) The fastest serve in tennis is about 62 m/s. Calculate the wavelength associated with a 6.0x10-2 kg tennis ball traveling at this velocity

b) Calculate the wavelength associated with an electron moving at 62 m/s.

  1. How many individual orbitals are there in the third shell? Write out n, l, ml quantum numbers for each one and label each set by the s, p, d, f designations.
  2. Describe the characteristics of an s orbital, a p orbital, and a d orbital. Which of the following orbitals do not exist: 1p, 2s, 2d, 3p, 3d, 3f, 4g?
  3. What is the maximum number of electrons in an atom that can have the following quantum numbers? Specify the orbitals in which the electrons would be found. (a) n = 2, ms = +1/2; (b) n=4, ml = +1; (c) n=3, l =2; (d) n=2, l=0, ms = +1/2; (e) n=4, l =3, ml =-2
  4. An electron in a certain atom is in the n=2 quantum level. List the possible values of l and ml that it can have.
  5. List all the possible subshells and orbitals associated with the principle quantum number n, if n=5.
  6. Indicate which of the following sets of quantum numbers in an atom are unacceptable and explain why:

(a) (1,0,1/2,1/2) (b) (3,0,0,+1/2) (c) (2,2,1,+1/2)

(d) (4,3,-2,+1/2) (e) (3,2,1,1,)

  1. Indicate the number of unpaired electrons present in each of the following atoms: B (Z=5), Ne (Z=10), P (Z=15), Sc (Z=21), Mn (Z=25), Se (Z=34), Kr (Z=36), Fe (Z=26), I (Z=53), Pb (Z=82), Cd (Z=48).
  2. Draw the shapes (boundary surfaces) of the following orbitals: a) 2py; b) 3; c) 3d

15. Draw orbital diagrams for atoms with the following configuration:

a) 1s22s22p5 b) 1s22s22p63s23p3 c) 1s22s22p63s23p64s23d7

16. The ground-state electron configurations listed here are incorrect. Explain what mistakes have been made in each and write the correct electron configurations

Al: 1s22s22p43s23p3

B: 1s22s22p5

F: 1s22s22p6

  1. Without referring to a periodic table, write the electron configuration of the elements with the following atomic numbers: a) 9; b) 20; c) 26; d) 33. Classify the elements.
  2. Specify the group of the periodic table in which each of the following elements is found: a) [Ne] 3s1, b) [Ne]3s23p3, c) [Ne]3s23p6, d) [Ar]4s23d8
  3. A M2+ ion derived from a metal in the 1st transition metal series has four electrons in the 3d subshell. What element might M be?
  4. In general, ionization energy increases from left to right across a given period. Aluminum, however, has a lower ionization energy than magnesium. Explain.
  5. Two atoms has the electron configurations 1s22s22p6 and 1s22s22p63s1. The first ionization energy of one is 2080 KJ/mol, and that of the other is 496 KJ/mol. Match each ionization energy with one of the given electron configurations. Justify your choice ?
  6. A hydrogenlike ion is an ion containing only one electron. The energies of the electron in a hydrogenlike ion are given by

Where n is the principle quantum number and Z is the atomic number of the element. Calculate the ionization energy of the He+ ion.

  1. From the following data, calculate the average bond energy for the N-H bond:

NH3(g)  NH2(g) + H(g) Ho = 435KJ

NH2(g)  NH(g) + H(g) Ho = 381 KJ

NH(g)  N(g) + H(g) Ho = 360 KJ

  1. The energy needed for the following process is 1.96x104KJ.mol-1:

Li(g)  Li3+ (g) + 3e-

If the first ionization energy for lithium is 520 kJ/mol-1, calculate the second ionization energy of lithium, that is, the energy required for the process

Li+(g)  Li2+(g) + e-

(Use the equation:)

  1. According to VB theory, explain, why the nitrogen atom cannot have pentavalence, while the phosphorus has.
  2. Determine and explain all possible valences of the following atoms: S, Cl, C.
  3. Draw a Lewis formula for the following species: H2O, H3O+, NF3, OF2, BF3, [BF4]-, SF4, SF6.
  4. What is the hybridization of the central atom in each of the following: NCl3, CF4, SF6, NH3, NH4+.
  5. What hybridizations are predicted for the central atoms in the following molecules:

H2O H2S H2Se H2Te

104.5o 92.2o 91o 89.5o

Why the bond angles decrease by the above order?

  1. Predict geometry of the following molecules: H2O, H3O+, CH4, CO2, SO2, BF3.
  2. Describe the hybridization of N in each of these species:
  3. NH3; ii) NH4+; iii) H = H; iv) ; v) H2 - H2
  4. What change in hybridization occurs in the following reaction?

NH3 + BF3 →H3N: BF3

31. Briefly discuss the bond angles in the hydroxylamine molecule in terms of the ideal geometry and the small changes caused by electron-pair repulsions.

32. Use the appropriate milecular orbital energy diagram to write the electron configuration for each of the following; calculate the bond order of each, and predict which would exist (a) H2+; (b) H2; (c) H2-; (d) H22-.

33. Repeat exercise 32 for (a) He2+; (b) He2; (c) He22+

34. Repeat exercise 32 for (a) N2; (b) Ne2; (c)C22-

35. Repeat exerice 32 for (a) Li2; (b) Li2+; (c) O22-

36. Use the appropriate molecular orbital energy diagram to write electron configurations of the following molecules and ions: (a) Be2, Be2+, Be2-; (b) B2, B2+, B2-.

37. Use the preceding diagram to fill in an MO diagram for NO-, what is the bond order of NO- ? It is paramagnetic? How would you assess its stability?

38. Repeat exercise 37 for NO+

39. Repeat exercise 37 for CN+. Refer to the preceding diagram but assume that the 2px2py MOs are lower in energy than the 2σp MO.

40. Explain why ionization energies of molecules H2, N2, C2, CO higher than those of the corresponding atoms ?

H C N O F

I1 (KJ.mol-1) 1308 1083 1396 1312 1675

H2 C2 N2 O2 F2

I1 (KJ.mol-1) 1488 1154 1507 1173 1526

41. Compare dipole moment of the following molecules: NH3 and NF3 and explain?

42. Do the following molecules have dipole moment ? Explain?

F2; BeF2; BF3; CF4; CO2; SO2

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