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WorksheetsRevision Chapter 2: Atomic Structure
Total questions: 22
Worksheet time: 6hrs 30mins
In a line spectrum of emission of hydrogen atom, how many lines can be observed if the electrons transit within n=4 and n=1
3
4
5
6
Line corresponding to the shortest wavelength is obtained in a hydrogen spectrum when the electron drops from
n=2 to n=1
n=3 to n=1
n=4 to n=2
n=4 to n=1
Choose the transition of electrons involving the greatest energy change.
n=4 to n=3
n=3 to n=1
n=4 to n=2
n=4 to n=1
The electronic configuration with the lowest energy for 7 electrons in a 3d subshell is obtained based on
Hund's rule
The Aufbau principle
The Pauli Exclusion Principle
The Heisenberg's uncertainty principle
What is the wavelength, λ of the fourth line in the Balmer series?
410 nm
432 nm
486 nm
654 nm
Calculate the energy required to excite an electron from n=2 to n=4
4.09 x10-19 J
5.45 x10-19 J
2.05 x106 J
2.74 x106 J
Pick the transition resulting the shortest wavelength
P
Q
R
S
The diagram shows lines of emission spectrum in Balmer Series. Select the transition of electron that gives rise to the line L.
n=1 to n=5
n=3 to n=2
n=4 to n=2
n=5 to n=2
An atom with principal quantum number, n=3 has a total number of orbitals of
13
14
16
18
What is the frequency, in s-1 of a radiation with energy of 3.37 x 10-19 J per photon?
5.08 x 10-54 s-1
5.08 x 1014 s-1
5.08 x 10-15 s-1
5.08 x 1015 s-1
What is the energy, in J, of one mole of photons emitted with a frequency of 6.336 x 1015 Hz?
4.20 x 10-18 J
3.96 x 106 J
2.53 x 106 J
3.88 x 1014 J
A possible set of quantum numbers for an electron in the 3d-orbital is
(n.l,m,s) = (3,1,+1,-1/2)
(n.l,m,s) = (3,2,0,-1/2)
(n.l,m,s) = (3,1,+3,+1/2)
(n.l,m,s) = (3,3,+2,-1/2)
Which of the following electronic configuration is for 7N3+ ?
1s2 2s2
1s2 2s2 2p3
1s2 2s2 2p6
1s2 2s2 2p6 3s1
The electronic configuration of oxygen atom in the ground state is represented by
What is the electronic configuration for Ni2+?
[Ar] 3d6
[Ar] 3d8
[Ar] 3d10
[Ar] 3d8 4s2
The maximum number of electrons occupying atomic orbitals of shell M (n=3) is
8
10
18
32
Orbital with quantum number, n=3, l =2 and m=+2 is
2p
3s
3p
3d
The electronic configuration of copper atom is 1s2 2s2 2p6 3s2 3p6 3d10 4s1.
Determine the number of electrons in the copper atom in ground state with the azimuthal quantum number l=0.
7
8
10
12
For 18Ar, calculate the total number of electrons with magnetic quantum number, m=0.
8
10
12
16
Which of the following represent an element that forms ion with a charge of -2?
1s2 2s2 2p6 3s2
1s2 2s2 2p6 3s2 3p2
1s2 2s2 2p6 3s2 3p4
1s2 2s2 2p6 3s2 3p5
After filling up the 3p orbital, which orbital must electrons next occupy?
3d
4s
4p
3s
Which of the following defines the Pauli exclusion principle?
When electrons are filled into orbitals with equivalent energy, the electrons occupy each orbital singly before they occupy the orbitals in pairs/
An orbital can hold maximum of 2 electrons with different quantum numbers
Electrons occupy the orbital with the lowest energy first before they occupy orbitals with higher energy
Half-filled orbitals contribute to the stability of an atom
