Periodic Classification of Elements Test

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Periodic Classification of Elements Test - 2

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Weekly Quiz Competition

Question 1
1 / -0

The numbers of groups in the s-block and p-block of the periodic table, respectively, are

A
10 and 6

B
6 and 2

C
2 and 6

D
2 and 10

Solution

There exists a correlation between the periodic table and the electronic configuration.
The s-block of the periodic table comprises elements in which the last electron enters the s-subshell. The s-subshell can accommodate 2 electrons and the s-block of the periodic table has 2 groups.

The p-block of the periodic table comprises elements in which the last electron enters the p-subshell. The p-subshell can accommodate 6 electrons and the p-block of the periodic table has 6 groups.
Question 2
1 / -0

The elements with atomic numbers 4, 12, 20, 38 and 56 belong to

A
alkali metals

B
alkaline earth metals

C
halogen group

D
noble gases

Solution

These are the atomic numbers of group 2 elements, known as the alkaline earth metals.

Element Atomic number

Beryllium 4

Magnesium 12

Calcium 20

Strontium 38

Barium 56
Question 3
1 / -0

The most metallic element in group 15 (nitrogen family) is

Group 15

N

P

As

Sb

Bi

A
P

B
N

C
Bi

D
Sb

Solution

The metallic character (electropositive character) in elements increases down the group on account of the increase in atomic radius and the decrease in ionisation energy.
Question 4
1 / -0

Observe the elements of period III and select the strongest reducing and oxidising agents, respectively.

Na, Mg, Al, Si, P, S, Cl, Ar

A
Na and Mg

B
S and Cl

C
Na and Cl

D
Al and Si

Solution

Among the options, Na is the most electropositive element and is the strongest reducing agent; and Cl is the most electronegative element and is the strongest oxidising agent.
Question 5
1 / -0

Select the pair of amphoteric oxides from the following:

A
Na₂O and CaO

B
ZnO and AI₂O₃

C
P₂O₅ and SO₂

D
SIO₂ and CI₂O

Solution

Metallic oxides are basic in nature. For example, Na₂O and CaO.

Non-metallic oxides are acidic in nature. For example, P₂O₅, SO₂, SiO₂ and CI₂O.
Oxides of some metals are amphoteric, and can neutralise both acids and bases.

Example:
ZnO + 2HCI → ZnCI₂ + H₂O
ZnO + 2NaOH → Na₂ZnO₂ + H₂O
AI₂O₃ + 6HCI → 2AICI₃ + 3H₂O
AI₂O₃ + 2NaOH → 2NaAIO₂ + H₂O
Question 6
1 / -0

Which among the following is the smallest in size?

A
N³⁻

B
O^2-

C
F^-

D
Na⁺

Solution

Na⁺ will have the smallest ionic radius because 10 electrons are held by 11 protons in the nucleus.
Question 7
1 / -0

Which of the following is not correct about the modern periodic table?

A
The elements in a period have the same number of shells.

B
The outermost electron of the elements in a period have the same Azimuthal quantum number.

C
The number of shells occupied increase regularly down a group.

D
The effective nuclear charge increases across a period.

Solution

The Azimuthal quantum number changes across a period.
e.g. Period III has portions of the s-block (groups 1 & 2), d-block (groups 3 to 12), p-block (groups 13 to 18)
l = 0 in the s-block, l = 2 in the d-block, and l = 1 in the p-block.
Question 8
1 / -0

Elements A, B and C have positions in the periodic table as shown below:

Group 16 Group 17

-------- --------

-------- A

-------- --------

B C

(i) A is a metal.
(ii) C is smaller in size as compared to B.
(iii) Element A forms a negatively charged ion.

Which of the above statements is/are correct?

A
All (i), (ii) and (iii)

B
Only (ii) and (iii)

C
Only (ii)

D
Only (i) and (iii)

Solution

A belongs to group 17, and is a non-metal; hence, statement (i) is incorrect.
C is smaller in size than B because the atomic radius decreases across the period.
A is electronegative and will form anions by gaining electrons.
Question 9
1 / -0

The bond in the compounds formed by the combination of group 14 and group 17 elements of the periodic table will be a/an

A
electrovalent bond

B
co-ordinate bond

C
Van der Waals bond

D
covalent bond

Solution

The elements of group 14 and group 17 are non-metallic and they bond by sharing electrons; hence, they are covalent compounds.
Question 10
1 / -0

An element A belongs to third period and second group of the periodic table. The number of valence electrons of element A is

A
one

B
two

C
three

D
four

Solution

The element is Mg.
Each element of group 2 (group of alkaline earth metals) has 2 valence electrons.

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Element	Atomic number
Beryllium	4
Magnesium	12
Calcium	20
Strontium	38
Barium	56

Group 16	Group 17
--------	--------
--------	A
--------	--------
B	C

Periodic Classification of Elements Test - 2

Result

Periodic Classification of Elements Test - 2

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Question 1

10 and 6

6 and 2

2 and 6

2 and 10

Solution

Question 2

alkali metals

alkaline earth metals

halogen group

noble gases

Solution

Question 3

P

N

Bi

Sb

Solution

Question 4

Na and Mg

S and Cl

Na and Cl

Al and Si

Solution

Question 5

Na2O and CaO

ZnO and AI2O3

P2O5 and SO2

SIO2 and CI2O

Solution

Question 6

N3−

O2-

F-

Na+

Solution

Question 7

The elements in a period have the same number of shells.

The outermost electron of the elements in a period have the same Azimuthal quantum number.

The number of shells occupied increase regularly down a group.

The effective nuclear charge increases across a period.

Solution

Question 8

All (i), (ii) and (iii)

Only (ii) and (iii)

Only (ii)

Only (i) and (iii)

Solution

Question 9

electrovalent bond

co-ordinate bond

Van der Waals bond

covalent bond

Solution

Question 10

one

two

three

four

Solution

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Na₂O and CaO

ZnO and AI₂O₃

P₂O₅ and SO₂

SIO₂ and CI₂O

N³⁻

O^2-

F^-

Na⁺