Periodic Classification of Elements Test

Result

Periodic Classification of Elements Test - 8

Score
-
out of -
Rank
-
out of -

TIME Taken - -

SHARING IS CARING

If our Website helped you a little, then kindly spread our voice using Social Networks. Spread our word to your readers, friends, teachers, students & all those close ones who deserve to know what you know now.

Weekly Quiz Competition

Question 1
1 / -0

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
1 / -0

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
1 / -0

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
1 / -0

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
1 / -0

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
1 / -0

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
1 / -0

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
1 / -0

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
1 / -0

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
1 / -0

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.
Question 11
1 / -0

The element with the highest electron affinity is

A
N

B
H

C
He

D
F

Solution

Electron affinity is defined as the change in energy (in kJ/mole) of a neutral atom (in the gaseous phase) when an electron is added to the atom to form a negative ion. Halogens have the greatest electron affinity as by gaining one electron, they attain noble gas configuration. Thus, among the given elements, fluorine has the highest electron affinity.
Question 12
1 / -0

With respect to chlorine, hydrogen will be

A
electronegative

B
neutral

C
electropositive

D
None of the above

Solution

Chlorine is more electronegative and in an H-Cl bond, the shared pair of electrons are drifted more towards the Cl atom. Hydrogen is relatively electropositive.
Question 13
1 / -0

Electronegativity refers to the tendency of an atom to

A
lose electrons

B
repel electrons

C
share electrons with the other atoms

D
attract bonding electrons

Solution

Electronegativity refers to the tendency of an atom to attract bonding electrons.
Question 14
1 / -0

Which of the following oxides forms the strongest base?

A
MgO

B
Al₂O₃

C
Na₂O

D
CaO

Solution

From the given oxides, Na₂O forms the strongest base.
Question 15
1 / -0

Which of the following is a metalloid?

A
Magnesium

B
Gallium

C
Germanium

D
Vanadium

Solution

A metalloid is a chemical element with properties intermediate between those of typical metals and nonmetals. The elements boron, silicon, germanium, arsenic, antimony, tellurium and polonium are metalloids.
Question 16
1 / -0

Which of the following elements has 4 electrons in its outermost shell?

A
Beryllium

B
Silicon

C
Sulphur

D
Magnesium

Solution

Silicon belongs to carbon family. Thus, it has 4 electrons in its valence shell.
Question 17
1 / -0

Which of the following elements has zero electron affinity in the 3^rd period of the periodic table?

A
Argon

B
Phosphorus

C
Aluminium

D
Sulphur

Solution

The electron affinity value of noble gases are zero because of the stable electronic configuration of ns²np⁶ which has no tendency to take in additional electron. No energy is released and their electron affinities are zero.
Question 18
1 / -0

Which of the following factors is inversely related to the metallic character of an element?

A
Reducing power

B
Atomic size

C
Electronegativity

D
None of these

Solution

Electronegativity is a chemical property that describes the tendency of an atom or a functional group to attract electrons towards itself. Non-metallic elements have a strong tendency to gain electrons. Therefore, electronegativity is directly related to the non-metallic character of elements. We can also say that electronegativity is inversely related to the metallic character of elements. Thus, the increase in electronegativity across a period is accompanied by an increase in non-metallic character (or a decrease in metallic character) of elements. Similarly, the decrease in electronegativity down a group is accompanied by a decrease in non-metallic character (or an increase in metallic character) of elements.
Question 19
1 / -0

The element which accepts electrons rarely to form anion belongs to

A
0 group and 3^rd period

B
VI A group and 3^rd period

C
VII A group and 2^nd period

D
VIII A group and 3^rd period

Solution

The element which accepts electrons rarely to form anion belongs to VIII A group and 3^rd period.
Question 20
1 / -0

The electronic configuration of chromium (Z = 24) is

A
1s², 2s², 2p⁶, 3s², 3p⁶, 3d⁴, 4s²

B
1s², 2s², 2p⁶, 3s², 3p⁶, 3d⁵, 4s¹

C
1s², 2s², 2p⁶, 3s², 3p⁶, 3d⁶, 4s⁰

D
1s², 2s², 2p⁶, 3s², 3p⁶, 3d³, 4s³

Solution

The electronic configuration of chromium (Z = 24) is 1s², 2s², 2p⁶, 3s², 3p⁶, 3d⁵, 4s¹.

User

Question Analysis

Correct -
Wrong -
Skipped -

My Perfomance

Score
-
out of -
Rank
-
out of -

Re-Attempt Weekly Quiz Competition

Periodic Classification of Elements Test - 8

Result

Periodic Classification of Elements Test - 8

Score

-

Rank

-

SHARING IS CARING

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

Question 11

N

H

He

F

Solution

Question 12

electronegative

neutral

electropositive

None of the above

Solution

O^2– > O > F^– > F

F^– > O^2– > F > O

O^2– > F^– > F > O

O^2– > F^– > O > F

Cl^–

S^2–

Na⁺

Al₂O₃

Na₂O

0 group and 3^rd period

VI A group and 3^rd period

VII A group and 2^nd period

VIII A group and 3^rd period

1s², 2s², 2p⁶, 3s², 3p⁶, 3d⁴, 4s²

1s², 2s², 2p⁶, 3s², 3p⁶, 3d⁵, 4s¹

1s², 2s², 2p⁶, 3s², 3p⁶, 3d⁶, 4s⁰

1s², 2s², 2p⁶, 3s², 3p⁶, 3d³, 4s³