1. General Chemistry Chem 110 Revision
Chapter 7

2. E = h x n E= h c / l Energy nf ni Energy absorbed Energy emitted
General equation
Energy for e in level n
Energy for e when it move
from i level to f level
E = h x n
E= h c / l
Energy absorbed
Energy emitted ni nf
∆ E positive
∆ E negative

3. shape of various subshells
Quantum Numbers
Angular momentum
Quantum Number (ℓ)
shape of various subshells
spin Quantum
Number (ms)
ms = +1/2 and −1/2.
Magnetic Quantum
Number (mℓ)
−ℓ ≤ ml ≤ ℓ.
three-dimensional orientation
Principal Quantum
Number (n)
describes the energy level
n= 1,2,3,4,5,6,7
For certain value of (n):
- (n2) No. of orbitals
- (2n2) No. of electrons
Quantum No.
0 to (n − 1). ℓ=
n = 1, 2 , 3, 4 ………
ℓ = 0 to (n-1)
mℓ = - ℓ to 0 to + ℓ
ms = +½ or -½ ℓ 1 2 3
subshell Name s p d f

4. Shell Subshell Orbital 1s 2s 3s 2p 3p 3d s p d ℓ= n ℓ n=1 ℓ =0 n=2-1 +1 -2 +2 n ℓ mℓ
Shell
Subshell
Orbital 1s 2s 3s 2p 3p 3d
n=1
ℓ =0 s
n=2
ℓ =1 p
n=3
ℓ =2 d d
four-leaf clovers
Increasing of Energy p
dumbbell-shaped. s
spherical
0 to (n − 1). ℓ=
=(2 ℓ +1) mℓ

5. Aufbau principle Fill up” electrons in lowest energy orbitals
Pauli exclusion principle
Hund’s rule

6. [1] Calculate the energy, in joules, required to excite a hydrogen atom by causing an electronic transition
from the n = 1 to the n = 4 principal energy level.
2.04 J
2.19  105 J
2.04  J
3.27  J
[2] What is the wavelength of radiation that has a frequency of 7.5×1014s-1?
A ×106 nm
B ×10-7 nm
C ×1023 nm
D ×102 nm

7. [3] What is the four quantum numbers for the last electron in Aluminum(Al13) atom
n=2, ℓ= 1, mℓ=-1, ms=+1/2
n=3, ℓ=3, mℓ=-1, ms=+1/2
n=3, ℓ=1, mℓ=-1, ms=+1/2
n=2, ℓ= 1, mℓ=-1,ms=-1/2
[4] Which one of the following electrons has the same energy as an electron with
quantum numbers n = 5, l = 2, ml = -1 , ms = +1/2?
n = 5, l = 2, ml = 0, ms = +1/2
n = 4, l = 3, ml = -1, ms = +1/2
n = 4, l = 2, ml = 3, ms = -1/2
None of these
[5] What is the four quantum numbers for the last electron in Sodium (Na11) atom
n = 3, ℓ = 1, mℓ = 0, ms = -½
n = 3, ℓ = 0, mℓ = 0, ms =+ ½
n = 2, ℓ = 1, mℓ = -1, ms = +½
n = 2, ℓ = 0, mℓ = -1, ms =+ ½

8. [6] Which one of the following electrons have the same energy as an electron with quantum numbers n = 4, l = 3, ml = -1 , ms = +1/2?
n = 5, l = 1, ml = -1 , ms = ½
n = 4, l = 3, ml = -1 , ms = ½
n = 4, l = 2, ml = 2 , ms = -½
None of these
[7 ]Which one of the following electrons have the same energy as an electron with quantum
numbers n = 4, l = 2, ml = -1 , ms = +1/2?
n=5, l = 1, ml = -1, ms= +1/2
n=4, l = 3, ml = -1, ms= +1/2
n=4, l = 2, ml = 2, ms= -1/2
None of these
[8] What is the four quantum numbers for the last electron in Silicon (Si) atom
n= 3, l = 2, ml = 0, ms = - ½
n= 3, l = 1, ml = 0, ms = +½
n= 2, l = 1, ml = -1, ms = -½
n= 2, l = 0, ml = -1, ms = +½

9. [9] Which statement about the four quantum numbers which describe electrons in
atoms is incorrect?
n = principal quantum number, n = 1, 2, 3,
l = subsidiary quantum number, l = 1, 2, 3, ... , (n+1)
ml = magnetic quantum number, ml = (-l), .... , 0, .... , (+l)
ms = spin quantum number, ms = +1/2 or -1/2.
[10] What is the total number of orbitals in the n = 3 level?
(A) 2
(B) 8
(C) 9
(D) 3
[11] Which of the following statements about the quantum numbers is incorrect?
(A) n has integral values from 1 to ∞
(B) L has values from 1 to ∞
(C) mL has values of -L to +L, including zero
(D) ms has values of ,

10. gallium Ga in its ground state is n L mL ms (A) 4 0 0 -1/2
[12] A possible set of quantum numbers for the last electron added to complete an atom of
gallium Ga in its ground state is
n L mL ms
(A) /2
(B) /2
(C) /2
(D) /2
[13]The number of orbitals in a d subshell is?
A.1
B.3
C. 5
D.7
[14] The maximum number of electron for one orbital is?
A.2 electron
B.1 electron
C. 3 electron
D.6 electron

11. [15] Which one of the following sets of quantum number is not possible?
(3 , 0 , 0 , +1/2 )
(4 , 3 , -2 , -1/2 )
(1 , 0 , 0 , +1/2 )
(3 , 2 , 1 , 1 )
[16]The last two electrons in C6 atom should differ in the value of the quantum number: n l ml ms
[17] The representative elements are those with unfilled energy levels in which the
"last electron" was added to 
an s or p orbital..
an s orbital.
a p or d orbital.
an f orbital.

12. [18] Choose the incorrect quantum numbers for electron in an atom?
(1 , 0 , 0 , +1/2)
(4 , 3 , -2 , -1/2)
[19 The number of orbital in a p subshell is?
A. 1
B. 7
C. 5
D. 3
[20] The maximum number of electrons that can occupy an energy level described by
the principal quantum number,n,is?
A. n+1
B. 2n
C. n2
D. 2n2

13. [21] The maximum number of electron for one orbital is? 2 electron
[22] The electron configuration of a neutral atom is[Ne] 3s23p3. The four quantum
numbers of the last electron are:
A. (3 , 1 , +1 , +1/2 )
B. (2 , 0 , 0 , +1/2 )
C. (2 , 0 , -1 , +1/2 )
D. (3 , 2 , -1 , +1/2 )
[23] Atoms of which two elements have the same number of unpaired electrons?
Na and C
O and C
Mg and C
Al and C

14. [24] Atoms of which two elements have the same number of unpaired electrons?
Si and Cl
Al and Cl
Mg and Cl
N and Cl
[25] Which anion contains the most number of electrons?
P3-
Se2-
Si4-
S2-
[26] Atoms of which two elements have the same number of unpaired electrons?
Si and F
B and F
Ca and F
N and F

15. [27]The ground-state electron configuration for an atom of indium (In) is 
[Ar]4s23d104p1.
[Ar]4s24p63d5.
[Kr]5s25p64d5.
[Kr]5s24d105p1.
[28] The [Ar]4s24p5 element are found in _______ of the periodic table. 
Group 2A
Group 7A
Period 7
Group 8A
[29] How many electrons are found in the (Sn2+) ion? 48
119 22 69

16. [30] Atoms of which two elements have the same number of unpaired electrons?
Na and S
Si and S
Mg and S
Al and S
[31] Which ground-state atom has an electron configuration described by the following
orbital diagram?          
   
(A) phosphorus
(B) germanium
(C) selenium
(D) tellurium
[32] All the following electronic ground-state configurations are correct except
(A) 20Ca: [Ar] 4s2
(B) 25Mn: [Ar] 4s2 4d5
(C) 29Cu: [Ar] 4s13d10
(D) 54Xe: [Kr] 5s24d10 5p6

17. [33] Which of the following is paramagnetic?
(A) K+
(B) Sn+2
(C) Sc+3
(D) Cr+3
[34] The general electron configuration for atoms of all elements in Group 5A is 
(A) ns2np1
(B) ns2np5
(C) ns2np4
(D) ns2np3
[35] What is the electron configuration of the Cr24?
A. ( 1s2 2s2 2p6 3s2 3p5 4s2 3d5 )
B. ( 1s2 2s2 2p6 3s3 3p6 4s2 3d3 )
C. ( 1s2 2s2 2p6 3s2 3p6 4s1 3d5 )
D. ( 1s2 2s2 2p6 3s2 3p6 4s2 3d4 )

18. [36] A ground –state atom of Mn+2 has ---------unpaired electrons and is -----.
2,paramagnetic
4,diamagnetic
0,diamagnetic
5, paramagnetic
[37] The orbital diagram for a ground state O2- atom is:
A. ↓↑ ↓↑ ↓↑ ↓ ↑ ↑
1s 2s p
B ↓↑ ↓↑ ↓↑ ↑ ↑
1s 2s p
C ↓↑ ↓↑ ↑ ↑ ↑
1s 2s p
D. ↓↑ ↓↑ ↓↑ ↓↑ ↓↑
1s s p

19. [38] Which two electron configurations represent elements that would have similar
chemical properties? 1. 1s22s22p s22s22p5 3. [Ar]4s23d104p3 4. [Ar]4s23d104p4
A.(2) and (4)
B. (1) and (2)
C.(2) and (3)
D. (1) and (4)
[39] What is the electron configuration of the Mo42?
A. ( 1s2 2s2 2p6 3s2 3p6 4s2 3 d104p65s14d9 )
B. ( 1s2 2s2 2p6 3s2 3p6 4s2 3d104p6 5s1 4d5)
C. ( 1s2 2s2 2p6 3s2 3p6 4s2 3d104p64d9 5s2)
D. ( 1s2 2s2 2p6 3s2 3p6 4s2 3d104p6 5s2 4d4

20. [40] Which of the orbital diagrams is not follow the pauli exclusion principle?↑ ↑↑ ↑ ↑↓ ↑ ↑↓ ↑↓ ↑ ↑ ↓ ↑↓ ↑↓ ↓↓
A. (1) and(6)
B. (2) and(5)
C. (1) ,(2)and(6)
D. (3) ,(4)and(5)
[41] Which of the orbital diagrams is not follow Hand's rule? ↑ ↑↑ ↓ ↑↓ ↑ ↑↓ ↑↓ ↑ ↑↓ ↓↓ ↑ ↓ ↑↓
A. (1) and(4)
B. (1) and(5)
C. (2) and(3)
D. (2) ,(4)and(6)

21. [42]Choose the incorrect quantum numbers for electron in an atom?
(1 , 0 , 0 , +1/2)
(4 , 3 , -2 , -1/2)
[43] The number of orbital in a p subshell is?
A. 1
B. 7
C. 5
D. 3
[44] The maximum number of electrons that can occupy an energy level described by
the principal quantum number ,n, is?
A. n+1
B. 2n
C. n2
D. 2n2

22. numbers of the last electron are: A. (3 , 1 , +1 , +1/2 )
[45] The electron configuration of a neutral atom is[Ne] 3s23p3. The four quantum
numbers of the last electron are:
A. (3 , 1 , +1 , +1/2 )
B. (2 , 0 , 0 , +1/2 )
C. (2 , 0 , -1 , +1/2 )
D. (3 , 2 , -1 , +1/2 ) 46
What is the energy (in joules) a photon must have in order to excite an electron from E2 to E3? A)
5 ×10–10 J B)
10 × 10–19 J C)
5 × 10–19 J D)
15 × 10–19 J
47. The atomic number of an element is 73. Is this element diamagnetic or paramagnetic?
 (A)
Diamagnetic
 (B)
Paramagnetic

23. N, 3p electrons; Si, 6s electrons; S, 5d electrons B)
48.
Give the values of the quantum numbers associated with the 2p subshell. A)
n = 2, l = 2, ml = –2, –1, 0, 1, 2 B)
n = 2, l = 1, ml = 0 C)
n = 2, l = 1, ml = 1 D)
n = 2, l = 1, ml = –1, 0, 1
49.
State the total number of: p electrons in N (Z = 7); s electrons in Si (Z = 14); and 3d electrons in S (Z = 16). A)
N, 3p electrons; Si, 6s electrons; S, 5d electrons B)
N, 2p electrons; Si, 6s electrons; S, 5d electrons C)
N, 3p electrons; Si, 6s electrons; S, 0d electrons D)
N, 6p electrons; Si, 6s electrons; S, 0d electrons
50.
The electron configuration of a neutral atom is 1s22s22p63s2. Name the element. A) Si B) Na C) Mg D) Al

24. 51. Which of the following species has the most unpaired electrons
Which of the following species has the most unpaired electrons? S+, S, or S–?
 (A) S+
 (B) S
 (C) S–
 (D)
They all have the same number of unpaired electrons.
52.
Use the Aufbau principle to obtain the ground-state electron configuration of selenium. A)
Se: [Ar]4s23d104p3 B)
Se: [Ar]4s23d104p4 C)
Se: [Ar]4s23d104p5 D)
Se: [Ar]4s23d104p6
54. How many orbitals are allowed in a subshell if the angular momentum quantum number
for electrons in that subshell is 3? 
A. 1
B. 3
C. 5
D. 7
E. 9

25. 57. Transition metal elements have atoms or ions with partially filled
55. How many electrons in a ground-state cadmium atom are in orbitals labeled by ml = -1? 
A. 2
B. 10
C. 12
D. 18
E. 36
56. A ground-state atom of iron has ___ unpaired electrons and is _____. 
A. 0, diamagnetic
B. 6, diamagnetic
C. 3, paramagnetic
D. 5, paramagnetic
E. 4, paramagnetic
57. Transition metal elements have atoms or ions with partially filled 
A. s subshells.
B. p subshells.
C. d subshells.
D. f subshells.
E. g subshells.