Curriculum
Login

Curriculum

Chemistry — Second Secondary

Chemistry — Second Secondary

0/75

Chemistry — Second Secondary 2026/2027

0/47
Quiz

Question bank: Chapter 3 — The Periodic Table and Classification of Elements

Submit quiz
Once you submit, you will no longer be able to change your answers. Are you sure you want to submit the quiz?
Cancel Submit
  • Questions count: 48
Start Quiz
1.
The modern periodic table arranges the elements in ascending order of
atomic mass
atomic number
atomic radius
number of neutrons
2.
The modern periodic table consists of
8 groups and 7 periods
18 groups and 7 periods
18 groups and 8 periods
7 groups and 18 periods
3.
The s-block contains the groups
1A and 2A
1A and 7A
2A and 3A
zero and 1A
4.
The number of vertical columns in the d-block is
5
7
10
14
5.
The lanthanide series is formed by successive filling of the
3d sublevel
4f sublevel
5f sublevel
6p sublevel
6.
All the actinides are
noble gases
radioactive elements
non-metals
liquid at room temperature
7.
The outer configuration of the elements of group 5A is
ns2 np2
ns2 np3
ns2 np5
ns1
8.
An element whose configuration ends with 4s2 3d6 is located in
period 3, s-block
period 4, d-block
period 4, p-block
period 3, d-block
9.
The noble gases (except He) end with the outer configuration
ns2 np4
ns2 np5
ns2 np6
ns1
10.
The representative elements include
only the s-block
the s and p blocks except group zero
the d-block
the f-block
11.
An element has the configuration [Ne] 3s2 3p4. It is in
period 3, group 4A
period 3, group 6A
period 2, group 6A
period 4, group 6A
12.
Atomic (covalent) radius is defined as
the distance between nucleus and farthest electron
half the distance between the nuclei of two identical bonded atoms
twice the distance between nuclei
the radius of the nucleus
13.
Going from left to right in a period, atomic radius decreases because
the number of shells increases
the effective nuclear charge increases
the shielding increases a lot
the number of neutrons decreases
14.
Which atom has the largest radius?
Cl
Al
Na
Mg
15.
Going down a group the atomic radius increases because
the number of energy levels increases
the nuclear charge decreases
the electrons become fewer
the ionization energy increases
16.
Which is correct?
Na+ is larger than Na
Cl− is larger than Cl
Fe3+ is larger than Fe2+
Mg2+ is larger than Mg
17.
Which has the smallest radius?
Fe
Fe2+
Fe3+
all equal
18.
Ionization energy is the energy required to remove
one electron from any atom
one mole of electrons from one mole of gaseous atoms
one electron from a molecule
all electrons from an atom
19.
The first ionization energy generally
decreases across a period
increases across a period
is constant across a period
is zero for metals
20.
Which element has the lowest first ionization energy?
Li
Na
K
Cs
21.
The third ionization energy of magnesium is very large because the electron is removed from
the 3s sublevel
a saturated inner level
a half-filled level
a d sublevel
22.
The highest (most negative) electron affinity values belong to
alkali metals
alkaline earths
halogens
noble gases
23.
The electron affinity of nitrogen is positive because
its 2p sublevel is half-filled
its radius is large
it is a metal
it has no electrons in 2s
24.
Electronegativity increases
down a group
across a period from left to right
with increasing radius
for noble gases
25.
The most electronegative element is
O
Cl
F
N
26.
Which of the following describes an atom bonded to another atom?
electron affinity
electronegativity
ionization energy
atomic radius
27.
Metals are described as electropositive because they
gain electrons
lose electrons to form positive ions
share electrons equally
have small radii
28.
Which of the following is a metalloid?
Na
Si
S
Cl
29.
The strongest metallic element is
Li
Na
Cs
Ba
30.
The oxide that reacts with both HCl and NaOH is
Na₂O
SO₃
ZnO
CO
31.
Carbon monoxide is classified as a(n)
acidic oxide
basic oxide
amphoteric oxide
neutral oxide
32.
Which of the following oxides gives an acid when dissolved in water?
MgO
SO₃
K₂O
Na₂O
33.
Across period 3 from Na to Cl, the oxides
become more basic
become more acidic
do not change
become neutral
34.
The hydrogen halide with the strongest acidic character is
HF
HCl
HBr
HI
35.
The oxidation number of manganese in KMnO₄ is
+2
+4
+6
+7
36.
The oxidation number of oxygen in sodium peroxide Na₂O₂ is
−2
−1
0
+1
37.
The oxidation number of hydrogen in CaH₂ is
+1
0
−1
+2
38.
The oxidation number of nitrogen in NH₄+ is
+3
+1
−3
−4
39.
The oxidation number of carbon in CH₃OH is
−4
−2
0
+2
40.
The oxidation number of sulphur in Na₂S₂O₃ is
+2
+4
+6
−2
41.
Oxidation is the process of
gaining electrons
losing electrons
gaining protons
decreasing the oxidation number
42.
The reducing agent is the reactant that
is reduced
gains electrons
loses electrons
does not change
43.
Which of the following is not a redox reaction?
Zn + 2HCl → ZnCl₂ + H₂
2Mg + O₂ → 2MgO
NaOH + HCl → NaCl + H₂O
Cl₂ + 2KI → 2KCl + I₂
44.
Which compound can act only as an oxidizing agent?
NH₃
H₂S
K₂Cr₂O₇
CH₄
45.
In Zn + CuSO₄ → ZnSO₄ + Cu the spectator ion is
Zn2+
Cu2+
SO₄2−
none
46.
The balanced net ionic equation of Zn and Fe3+ (forming Zn2+ and Fe2+) is
Zn + Fe3+ → Zn2+ + Fe2+
Zn + 2Fe3+ → Zn2+ + 2Fe2+
2Zn + Fe3+ → 2Zn2+ + Fe2+
Zn + 3Fe3+ → Zn2+ + 3Fe2+
47.
The reaction 2H₂O₂ → 2H₂O + O₂ is an example of
neutralisation
disproportionation
comproportionation
precipitation
48.
The reaction 2H₂S + SO₂ → 3S + 2H₂O is an example of
disproportionation
comproportionation
neutralisation
decomposition without redox
  • 1
  • 2
  • 3
  • 4
  • 5
  • 6
  • 7
  • 8
  • 9
  • 10
  • 11
  • 12
  • 13
  • 14
  • 15
  • 16
  • 17
  • 18
  • 19
  • 20
  • 21
  • 22
  • 23
  • 24
  • 25
  • 26
  • 27
  • 28
  • 29
  • 30
  • 31
  • 32
  • 33
  • 34
  • 35
  • 36
  • 37
  • 38
  • 39
  • 40
  • 41
  • 42
  • 43
  • 44
  • 45
  • 46
  • 47
  • 48