ELECTRONIC STRUCTURE OF AN ATOM QUESTIONNAIRE
PREPARED BY YELLOW GROUP
1. Before 1925, quantum theory
a) faced little challenge to its credibility
b) lacked organization
c)had wide applications
d) was widely accepted
2 Generally, the mathematics of modern quantum mechanics is
a) perfunctory
b) unimportant
c)simplified
d) complex
3. Schrodinger's equation described the
a)procedure for splitting an atom
b)complement of the wave function
c)behavior of "matter" waves
d)motion of light
4. Solutions to Schrodinger's equation are labeled with
a) psi
b) phi
c) mu
d) pi
5. Which physicist proposed the uncertainty principle in 1927?
a) Niels Bohr
b)Albert Einstein
c)Arnold Schrodinger
d)Werner Heisenberg
6.What energy level is closest to the nucleus?
A.5th
C.2nd
B.3rd
D.1st
7.In the types of sublevels,what sublevels has a highest energy?
A.p
B.d
C.f
D.s
8.what is the shape of the p sublevel?
A.Spherical
B.Complex
C.Dumbbell
9.What is the total numbers of electrons in the 3rd energy level?
A.8
B.10
C.14
D.18
10.How many electrons holds in every orbital?
A.3
B.2
C.1
D.4
WRITE YOUR ANSWER IN A PROVIDED SPACE
___________ a LAPNICRIP – It is the quantum number that represents the energy level the electron is in.
___________ b LATOBRI – It is a representation of the wave function of a hydrogen-like atom.
___________ c ALGANUR MUTMENMO – It is a quantum number that represents the shape of orbitals.
___________ d NOTRECLE – It is the particle that can be described by four quantum numbers
___________ e MEGATINC – It represents the quantum number that describes the orientation of an
orbital.
___________ f NEREGY EVELL – It is being represented by n.
___________ g RHEPES – It is the shape of the s orbital.
2. Give the n and ℓ values for the following orbitals
a. 1s _______________________________
b. 3p _______________________________
c. 5f _______________________________
d. 4d _______________________________
3. What is the mℓ values for the following types of orbitals?
a. s _______________________________
b. p _______________________________
c. d _______________________________
d. f _______________________________
4. How many possible orbitals and how many electrons can inhabit the energy level n
a. 4 _______________________________
b. 5 _______________________________
5. State the number of possible electrons described by the following quantum numbers
a. n = 3, l = 0 _______________________________
b. n = 3, l = 1 _______________________________
c. n = 3, l = 2, ml = -1 ________________________
d. n = 5, l = 0, mℓ =-2, ms =-1/2 _________________
6. Which of the following is not a valid set of quantum numbers? Explain your answer.
a. n = 2, l = 2, ml = 0, and ms = -1/2
b. n = 2, l = 1, ml = -1, and ms = -1/2
c. n = 3, l = 0, ml = 0, and ms = 1
d. n = 3, l = 2, ml = 3, and ms = ½
7. What is the maximum electron pairs that can occupy an:
a. s orbital _______________________________
b. the subshell of p orbitals _______________________________
c. the subshell of d orbitals _______________________________
d. the subshell of f orbitals _______________________________
e. the subshell of g orbitals _______________________________
8. INDICATE THE ELECTRON CONFIGURATION, NOBLE GAS CONFIGURATION, AND NO. OF ELECTRONS.
MOREOVER, DRAW AN ORBITAL DIAGRAM AND INDICATE IF IT IS PARAMAGNETIC OR DIAMAGNETIC.
A. NE
B. O
ANSWER KEY
1. B
2. D
3. C
4. A
5. D
6. D
7. C
8. C
9. D
10. B
1. Rearrange the letters
a. Principal
b. Orbital
c. Angular momentum
d. Electron
e. Magnetic
f. Energy level
g. Sphere
2. Give the n and ℓ values
a. n=1, l = 0
b. n=3, l =1
c. n= 5, l= 3
d. n= 4, l=2 3.
3. mℓ values
a. ml= 0
b. ml= -1, 0,1
c. ml= -2, -1, 0, 1, 2
d. ml= -3, -2, -1, 0, 1, 2, 3
4. Possible Orbitals
a. 32 electrons
b. 50 electrons
5. Number of possible electrons
a. 2
b. 6
c. 2
d. not possible
6. Valid Set of Quantum Numbers
a. l =2 is not allowed, maximum is 1
b. possible
c. ms should only be ½ or -1/2
d. mℓ should only be within the values of 2l+1; mℓ should only be
within the values of 2l+1
7. Maximum electron pairs
a. 1
b. 3
c. 5
d. 7
e. 9
___________
