Periodic Properties Test

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Periodic Properties Test - 8

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Weekly Quiz Competition

Question 1
1 / -0

The elements with atomic numbers 9, 17, 35, 53 and 85 are all

A
noble gases

B
halogens

C
heavy metals

D
light metals

Solution

The elements with atomic numbers 9, 17, 35, 53 and 85 are all halogens.
Z = 9 for Fluorine
Z = 17 for Chlorine
Z = 35 for Bromine
Z = 53 for Iodine
Question 2
1 / -0

Amongst the following elements (whose electronic configurations are given below), the one having the highest ionization enthalpy is

A
[Ne] 3s²3p¹

B
[Ne]3s²3p³

C
[Ne]3s²3p²

D
[Ne]3d¹⁰4s²4p²

Solution

The first ionization energy will be the highest for [Ne]3s²3p³ as it has half filled electronic configuration.
Question 3
1 / -0

The polarizing power of the anions N^3-, O^2- and F^-, follows the order

A
N^3- > O^2- > F^-

B
O^2-> N^3- > F^-

C
N^3- > F^-> O^2-

D
O^2- > F^- > N^3-

Solution

Polarizability of anion: Tendency of anion to get distorted because of the polarizing power of cation is called polarizability of anion.
Polarizability of anion is directly proportional to both charge of anion and size of anion.
Question 4
1 / -0

Which of the following is a set of isoelectronic species (At. No. of Cs = 55, Br = 35)?

A
N^3-, F^-, Na⁺

B
Be, Al³⁺, Cl^-

C
Ca²⁺, Cs^₊, Br

D
Na⁺, Ca²⁺, Mg²⁺

Solution

Isoelectronic species are elements or ions that have the same number of electrons. The ions present in option (1) have equal number of electrons.
Question 5
1 / -0

The formation of oxide ion O^2- (g) requires first an exothermic and then an endothermic step as shown below:

O (g) + e^- → O^- (g) ΔH_o = - 142 kJ/mol
O^- + e^- → O^2- (g) ΔH_o = + 844 kJ/mol

This is because

A
oxygen is more electronegative

B
oxygen has high electron affinity

C
O^- will tend to resist the addition of another electron

D
O^- ion has comparatively larger size than oxygen atom

Solution

This is because O^- will tend to resist the addition of another electron.
Question 6
1 / -0

For P^3-, S^2- and Cl^- ions, the increasing order of size is

A
Cl^-, S^2-, P^3-

B
P^3-, S^2-, Cl^-

C
S^2-, Cl^-, P^3-

D
S^2-, P^3-, Cl^-

Solution

In isoelectronic species, the size of ion decreases as nuclear charge increases.
Question 7
1 / -0

The correct order of increasing radii of the elements Na, Rb, K and Mg is

A
Mg, Na, K, Rb

B
Mg, K, Na, Rb

C
Na, K, Rb, Mg

D
Na, Rb, K, Mg

Solution

The correct order of increasing radii of the elements Na, Rb, K and Mg is Mg, Na, K and Rb.
Question 8
1 / -0

The correct order of increasing radii of the elements Na, Si, Al and P is

A
Si, Al, P, Na

B
Al, Si, P, Na

C
P, Si, Al, Na

D
Al, P, Si, Na

Solution

The correct order of increasing radii of the given elements is P, Si, Al, Na because radii decreases as we move from left to right across a period.
Question 9
1 / -0

In which of the following pairs is the first atom or ion not larger than the second?

A
K, K⁺

B
S, O

C
Br, Br^-

D
N, O

Solution

The correct answer is (3) as the size of the atom is always less than that of its anion.
Question 10
1 / -0

The ionisation enthalpy of nitrogen is more than that of oxygen because of

A
greater attraction of nucleus for the electron

B
extra stability of half filled p-orbitals

C
smaller size of nitrogen atom

D
more penetrating effect

Solution

The ionisation enthalpy of nitrogen is more than that of oxygen because of extra stability of half filled p-orbitals.

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Periodic Properties Test - 8

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Periodic Properties Test - 8

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Question 1

noble gases

halogens

heavy metals

light metals

Solution

Question 2

[Ne] 3s23p1

[Ne]3s23p3

[Ne]3s23p2

[Ne]3d104s24p2

Solution

Question 3

N3- > O2- > F-

O2- > N3- > F-

N3- > F- > O2-

O2- > F- > N3-

Solution

Question 4

N3-, F-, Na+

Be, Al3+, Cl-

Ca2+, Cs+, Br

Na+, Ca2+, Mg2+

Solution

Question 5

oxygen is more electronegative

oxygen has high electron affinity

O- will tend to resist the addition of another electron

O- ion has comparatively larger size than oxygen atom

Solution

Question 6

Cl-, S2-, P3-

P3-, S2-, Cl-

S2-, Cl-, P3-

S2-, P3-, Cl-

Solution

Question 7

Mg, Na, K, Rb

Mg, K, Na, Rb

Na, K, Rb, Mg

Na, Rb, K, Mg

Solution

Question 8

Si, Al, P, Na

Al, Si, P, Na

P, Si, Al, Na

Al, P, Si, Na

Solution

Question 9

K, K+

S, O

Br, Br-

N, O

Solution

Question 10

greater attraction of nucleus for the electron

extra stability of half filled p-orbitals

smaller size of nitrogen atom

more penetrating effect

Solution

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[Ne] 3s²3p¹

[Ne]3s²3p³

[Ne]3s²3p²

[Ne]3d¹⁰4s²4p²

N^3- > O^2- > F^-

O^2-> N^3- > F^-

N^3- > F^-> O^2-

O^2- > F^- > N^3-

N^3-, F^-, Na⁺

Be, Al³⁺, Cl^-

Ca²⁺, Cs^₊, Br

Na⁺, Ca²⁺, Mg²⁺

O^- will tend to resist the addition of another electron

O^- ion has comparatively larger size than oxygen atom

Cl^-, S^2-, P^3-

P^3-, S^2-, Cl^-

S^2-, Cl^-, P^3-

S^2-, P^3-, Cl^-

K, K⁺

Br, Br^-