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Chemistry — Second Secondary

Chemistry — Second Secondary

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Chemistry — Second Secondary 2026/2027

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Question bank: Chapter 2 — Atomic Structure

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  • Questions count: 40
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1.
The atom according to Thomson's model is
a hollow sphere with a nucleus
a solid sphere of uniform positive charge with electrons embedded in it
a nucleus surrounded by orbits
a cloud of electrons only
2.
In Rutherford's experiment the beam used consisted of
electrons
neutrons
alpha particles
X-rays
3.
The screen used to detect alpha particles in Rutherford's experiment was coated with
silver chloride
zinc sulphide
lead oxide
calcium carbonate
4.
The observation that most alpha particles passed straight through the gold foil shows that
the atom is mostly empty space
the nucleus is negative
electrons are heavy
the foil is a solid sphere
5.
A very small number of alpha particles were reflected back. This shows the existence of
an electron cloud
a small, dense, positive nucleus
neutral particles
a negative nucleus
6.
The deflection of some alpha particles shows that the dense part of the atom is
negatively charged
neutral
positively charged
magnetic only
7.
Rutherford compared the atom to
a plum pudding
the solar system
a hollow ball
a layered onion
8.
The line spectrum of an element is
continuous
the same for all elements
a characteristic property of the element
visible only for hydrogen
9.
Bohr's model successfully explained the line spectrum of
helium
hydrogen
lithium
all elements
10.
The red line of the visible hydrogen spectrum is due to the electron falling from
n = 6 to n = 2
n = 5 to n = 2
n = 4 to n = 1
n = 3 to n = 2
11.
The lines of the hydrogen spectrum in the ultraviolet region result from electron transitions to
n = 1
n = 2
n = 3
n = 4
12.
A 'quantum' is
a particle in the nucleus
the amount of energy gained or lost when an electron changes level
a kind of orbital
the speed of an electron
13.
When an excited electron returns to a lower level it
absorbs a quantum
emits light of definite wavelength
becomes a positive ion
stops moving
14.
In Bohr's calculations the energy differences between successive levels
are equal
increase with distance from the nucleus
decrease with distance from the nucleus
are zero
15.
Which of the following is a shortcoming of Bohr's model?
it introduced the quantum idea
it failed to explain the spectrum of helium
it explained hydrogen's spectrum
it used the principal quantum number
16.
Bohr's equations depict the hydrogen atom as
spherical in three dimensions
planar (flat)
a cloud
a solid
17.
The dual nature of the electron means that it behaves as
a particle only
a wave only
a particle and a wave
neither
18.
The uncertainty principle was put forward by
Heisenberg
Schrödinger
Bohr
Thomson
19.
The wave equation of the atom was formulated by
Rutherford
Heisenberg
Schrödinger
Pauli
20.
The region of space with the highest probability of finding an electron is called
orbit
orbital
shell only
quantum
21.
Which value of the principal quantum number n is possible?
0
1/2
3
−2
22.
The maximum number of electrons in the M shell (n = 3) is
8
10
18
32
23.
The number of sublevels in the main level n = 4 is
1
3
4
16
24.
For n = 3 the possible values of ℓ are
1, 2, 3
0, 1, 2
0, 1, 2, 3
−2 … +2
25.
The sublevel with ℓ = 2 is designated
s
p
d
f
26.
The number of orbitals in the 4f sublevel is
3
5
7
14
27.
The number of orbitals in the third main energy level is
3
6
9
18
28.
The magnetic quantum number mℓ for a p sublevel can take the values
0 only
−1, 0, +1
−2 … +2
+1, +2, +3
29.
The maximum number of electrons that the d sublevel can hold is
5
6
10
14
30.
The spin quantum number can have the values
0 and 1
+1/2 and −1/2
+1 and −1
1, 2, 3
31.
The quantum number that describes the shape of the sublevel is
n
ℓ
mℓ
ms
32.
According to Pauli's exclusion principle, two electrons in one atom cannot have
the same spin
the same n
the same four quantum numbers
the same energy
33.
Which sublevel is filled immediately after 3p?
3d
4s
4p
4d
34.
Which is the correct order of increasing energy?
3d < 4s < 4p
4s < 3d < 4p
4p < 3d < 4s
3d < 4p < 4s
35.
The electron configuration of ₁₇Cl is
1s2 2s2 2p6 3s2 3p6
1s2 2s2 2p6 3s2 3p5
1s2 2s2 2p6 3s1 3p6
1s2 2s2 2p6 3s2 3p4
36.
The number of electrons in the 3d sublevel of ₂₆Fe is
2
4
6
8
37.
According to Hund's rule the 2p electrons of nitrogen are arranged as
2px2 2py1
2px1 2py1 2pz1
2px2 2py2 2pz0
2px3
38.
The number of unpaired electrons in an oxygen atom (₈O) is
0
1
2
4
39.
The total number of electrons in the fourth main level (N) of ₃₀Zn in its ground state is
2
10
12
18
40.
The atomic number of an atom whose configuration ends with 3p3 is
13
14
15
17
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