Chemical Periodicity Test

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Chemical Periodicity Test - 3

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Weekly Quiz Competition

Question 1
4 / -1

Which of these dose not reflect the periodicity of the elements

A
Bonding behaviour

B
Electronegativity

C
Ionization energy

D
Neutron/proton ratio

Solution

n/p ratio is a cause of radioactivity.
Question 2
4 / -1

Elements of atomic number 6 is placed in

A
IV group

B
IV period

C
VI group

D
III group

Solution

1s²2s²2p² here are 4e⁻ in valence shell therefore it goes to IV- group.
Question 3
4 / -1

An element has electronic configuration 1s²2s²2p⁶3s²3p⁴. Predict their period, group and block

A
Period = 3rd, block = p, group = 16

B
Period = 5th, block = s, group = 1

C
Period = 3rd, block = p, group = 10

D
Period = 4th, block = d, group = 12

Solution

By obserbing principal quantum number (n), Orbital (s,p,d,f) and equating no. of e⁻s we are able to find the period, block and group of element in periodic table.
Question 4
4 / -1

The element having the electronic configuration 1s²,2s²2p⁶,3s²3p¹ is

A
A transition element

B
A representative element

C
An inert gas

D
An inner-transition element

Solution

A representative element as last e⁻enters p-orbital.
Question 5
4 / -1

The element with atomic number 55 belongs to

A
s−block

B
p−block

C
d−block

D
f−block

Solution

Electronic configuration for an element with atomic number 55 is [Xe]6s¹ . So it belongs to s-block since it has last electron in s-orbital.
Question 6
4 / -1

In which of the following groups all the three members are of the alkaline earth metals family

A
Al,Sr,Ti

B
Li,Na,K

C
Mg,Ba,Ca

D
Rb,Cs,Fr

Solution

Mg,Ba and Ca belongs to alkaline earth metals family.
Question 7
4 / -1

Which of the following remains unchanged on descending a group in the Periodic Table?

A
Valence electrons

B
Atomic size

C
Density

D
Metallic character
Solution
- Valence electrons: Each group is characterized by its valence electrons, i.e., the number of electrons in the outermost shell of the elements are the same within a group. Thus, the common oxidation states for the elements of the same group are fixed.
  Due to the same number of valence electrons, elements of the same group show similar chemical properties.
- Atomic size: Moving down the group, a new shell is added with each period. The electron in the new shell also increases shielding. Therefore, the Z_eff decreases along with which the attractive force of the nucleus decreases, and thus the size increases.
- Density: Density = Mass/Volume . Moving down the group, mass as well as volume increases. Therefore, density depends on the dominating factor. Usually, down the group, density increases, i.e., the effect of mass dominates.
- Metallic character: Moving down the group, the nuclear attractive force on outer electrons decreases due to a decrease in Z_eff which is due to an increase in shielding by outer valence electrons. As a result, the oxidation potential decreases down the group, and therefore, metallic character increases.
Question 8
4 / -1

Which of the following has the smallest size

A
Na⁺

B
Mg⁺²

C
Cl^-

D
F^-

Solution

As the nuclear charge per e⁻ is maximum in Mg⁺², it has smallest size among Na⁺Mg⁺²Cl⁻ and F⁻.
Question 9
4 / -1

The lanthanide contraction is responsible for the fact that

A
Zr and Y have about the same Ionization energy.

B
Zr and Nb have similar oxidations state.

C
Zr and Hf have about the same radius.

D
Zr and Ce have the same oxidation state.

Solution

Due to poor schielding of (n – 2)f – electrons, the size of Zr and Hf are same. Hence the actual radii is different. Due to the contraction the radius turns same.
Question 10
4 / -1

Radius of the isoelectronic species:

A
increases with the increase of nuclear charge

B
decreases with the increase of nuclear charge

C
is the same for all

D
first increases and then decreases

Solution

An isoelectronic series is a series of elements and ions that have equal numbers of electrons. Since they each have the same of electrons, their periodic trend in atomic radius and ionic radius predicts that the isoelectronic species with the greatest number of protons will have the smallest radius.

Thus Radius of the isoelectronic species decreases with increasing charge.

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Chemical Periodicity Test - 3

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Chemical Periodicity Test - 3

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Question 1

Bonding behaviour

Electronegativity

Ionization energy

Neutron/proton ratio

Solution

Question 2

IV group

IV period

VI group

III group

Solution

Question 3

Period = 3rd, block = p, group = 16

Period = 5th, block = s, group = 1

Period = 3rd, block = p, group = 10

Period = 4th, block = d, group = 12

Solution

Question 4

A transition element

A representative element

An inert gas

An inner-transition element

Solution

Question 5

s−block

p−block

d−block

f−block

Solution

Question 6

Al,Sr,Ti

Li,Na,K

Mg,Ba,Ca

Rb,Cs,Fr

Solution

Question 7

Valence electrons

Atomic size

Density

Metallic character

Solution

Question 8

Na+

Mg+2

Cl-

F-

Solution

Question 9

Zr and Y have about the same Ionization energy.

Zr and Nb have similar oxidations state.

Zr and Hf have about the same radius.

Zr and Ce have the same oxidation state.

Solution

Question 10

increases with the increase of nuclear charge

decreases with the increase of nuclear charge

is the same for all

first increases and then decreases

Solution

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Na⁺

Mg⁺²

Cl^-

F^-