Periodic Classification of Elements Test

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Periodic Classification of Elements Test - 3

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Weekly Quiz Competition

Question 1
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Which of the following sets of elements has a strong tendency to form anions?

A
Ca, In, Te

B
Na, Mg, Al

C
N, O, F

D
V, Cr, Mn

Solution

Non-metals can have the tendency to form anions. Thus, from given options, (N, O and F) are non-metals and thus, can form anion easily.
Question 2
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Which of the following represents the correct order of electronegativities?

A
P > O > N

B
N > P > O

C
O > N > P

D
N > O > P

Solution

Electronegativity decreases as you go down a group within the periodic table. This is because of the longer distance between the nucleus and the outer valence electron shell within an atom. This decreases the attraction. Thus, the correct order of electronegativities is O > N > P.
Question 3
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Which of the following has the lowest electronegativity?

A
F

B
He

C
Hg

D
Cl

Solution

Helium has the lowest electronegativity because it is a noble gas and noble gases are chemically very stable as they have the maximum number of valence electrons that their outer shell can hold.

Thus, the noble gas atom, being electrically neutral, would not be able to exert much attractive force on free-ranging electrons, i.e. low electronegativity.
Question 4
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Why is Gallium more electronegative than aluminium even though electronegativity of the elements decreases down the group?

A
Due to increase in atomic size

B
Due to increase in ionization energy

C
Due to increase in effective nuclear charge

D
Due to increase in atomic radii

Solution

Gallium is more electronegative than aluminium due to increase in effective nuclear charge.
Question 5
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Which of the following is the correct order of arrangement of elements in a period according to their metallic character?

A
Na < Li < K < Cs < Rb

B
Rb < Li < K < Na < Cs

C
Li < Na < K < Rb < Cs

D
Na < Li < Rb < Cs < K

Solution

The correct order of arrangement of elements in a period according to their metallic character is Li < Na < K < Rb < Cs. As we go down a group, metallic character increases.
Question 6
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Which of the following is the correct order of arrangement of decreasing atomic radii of F, F^–, O and O^2–?

A
O^2– > O > F^– > F

B
F^– > O^2– > F > O

C
O^2– > F^– > F > O

D
O^2– > F^– > O > F

Solution

The correct decreasing order of arrangement of atomic radii of F, F^–, O and O^2– is O^2– > F^– > O > F because size of the anions is greater than the corresponding atoms and also across a period, the size of atom decreases.
Question 7
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Which of the following is of the smallest size?

A
Cl^–

B
S^2–

C
Na

D
Na⁺

Solution

The size of the anions is greater than the corresponding atoms. Also, the size of the cation is smaller than the parent atom due to increase in the effective nuclear charge.

Thus, among the given options, Na⁺ is the smallest in size. Moreover, the loss of one electron from the Na atom leads to the removal of the 3s subshell.
Question 8
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Arrange the following set of atoms in order of increasing atomic radius:

F, Br, Cl, I

A
I, F, Br, Cl

B
F, Cl, Br, I

C
F, I, Br, Cl

D
Cl, Br, I, F

Solution

The increasing order of atomic radii among the given halogens is F, Cl, Br, I because as we move down a group, the size of atom increases.
Question 9
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Why does the atomic radius increase down the group?

A
Due to an increase in the nuclear charge

B
Due to an increase in the distance between the outermost electrons and the nucleus

C
Due to an increase in the force of attraction between outermost electrons and the nucleus

D
Due to an increase in the number of valence electrons

Solution

On moving down the group in the periodic table, there is an addition of a new shell which increases the atomic radius.
Question 10
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Which of the following elements has the highest electropositive nature?

A
Na

B
Cs

C
K

D
Rb

Solution

The electropositive character increases down the group due to the decrease in the ionisation energy. Among the group 1 elements, caesium (Cs) has the least ionisation energy and is the most electronegative element.

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Periodic Classification of Elements Test - 3

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Periodic Classification of Elements Test - 3

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Question 1

Ca, In, Te

Na, Mg, Al

N, O, F

V, Cr, Mn

Solution

Question 2

P > O > N

N > P > O

O > N > P

N > O > P

Solution

Question 3

F

He

Hg

Cl

Solution

Question 4

Due to increase in atomic size

Due to increase in ionization energy

Due to increase in effective nuclear charge

Due to increase in atomic radii

Solution

Question 5

Na < Li < K < Cs < Rb

Rb < Li < K < Na < Cs

Li < Na < K < Rb < Cs

Na < Li < Rb < Cs < K

Solution

Question 6

O2– > O > F– > F

F– > O2– > F > O

O2– > F– > F > O

O2– > F– > O > F

Solution

Question 7

Cl–

S2–

Na

Na+

Solution

Question 8

I, F, Br, Cl

F, Cl, Br, I

F, I, Br, Cl

Cl, Br, I, F

Solution

Question 9

Due to an increase in the nuclear charge

Due to an increase in the distance between the outermost electrons and the nucleus

Due to an increase in the force of attraction between outermost electrons and the nucleus

Due to an increase in the number of valence electrons

Solution

Question 10

Na

Cs

K

Rb

Solution

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O^2– > O > F^– > F

F^– > O^2– > F > O

O^2– > F^– > F > O

O^2– > F^– > O > F

Cl^–

S^2–

Na⁺