Classification of Elements and Periodicity in Properties Test

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Classification of Elements and Periodicity in Properties Test - 21

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Weekly Quiz Competition

Question 1
1 / -0

The electron affinity of sulphur is -200 kJ/mol. Then the electron affinity of oxygen is :

A
-142 kJ/mol

B
-702 kJ/mol

C
-332 kJ/mol

D
-348 kJ/mol

Solution

Due to small size and high electron density of oxygen compared to sulphur, interelectronic repulsion is higher in oxygen, resulting in less energy being released when an electron is added to oxygen, due to lesser stability after an electron is added, which is due to the interelectronic repulsion in the small oxygen atom. Hence, the electron affinity value of oxygen is lower than that of sulphur.

It is an exception to the normal trend of electron affinity in the periodic table.

Hence, the correct option is $$\text{A}$$
Question 2
1 / -0

The element having highest electron affinity is :

A
fluorine

B
nitrogen

C
chlorine

D
oxygen

Solution

Halogens has higher electron affinity and it is supposed to be for fluorine, but chlorine has higher electron affinity than fluorine due to fluorine's smaller size. Hence, among given options chlorine has highest electron affinity.
Question 3
1 / -0

The energy released when an electron is added to a neutral gaseous atom would be highest if the element belongs to:

A
VII A group

B
V A group

C
VI A group

D
II A group

Solution

Halogens have high E.A. Hence, if an element belongs to group VIIA of periodic table, its E.A. will be high.
Question 4
1 / -0

The element with high electron affinity is :

A
nitrogen

B
oxygen

C
sulphur

D
phosphorous

Solution

Among nitrogen, oxygen, sulphur and phosphorous, sulphur has the maximum electron affinity.
Nitrogen has a lower electron affinity than oxygen and oxygen has a lower electron affinity than sulphur.
Nitrogen has a lower electron affinity than phosphorous.
Question 5
1 / -0

Boron and silicon resemble chemically. This is due to the equal value of their:

A
electron affinity

B
atomic volume

C
ions polarizing power

D
nuclear charge

Solution

Boron and silicon resemble chemically. This is due to the equal value of their ion's polarizing power.
This chemical resemblance is called diagonal relationship. It is due to similarity in ionic sizes and charge/radius ratio of elements.
Question 6
1 / -0

Among the following electronic configurations which one will have low electron affinity value?

A
$$1s^{2}$$

B
$$1s^{2} 2s^{2}$$

C
$$1s^{2} 2s^{2} 2p^{4}$$

D
$$1s^{2} 2s^{2} 2p^{5}$$

Solution

Among the given electronic configurations $$1s^2$$ belongs to helium. As it is a noble gas, it will have low electron affinity value.
Question 7
1 / -0

Among the following electronic configurations which one will have highest electron affinity value?

A
$$1s^{2}$$

B
$$1s^{2} 2s^{2}$$

C
$$ 1s^{2} 2s^{2} 2p^{4}$$

D
$$ 1s^{2} 2s^{2} 2p^{5}$$

Solution

Halogens, belonging to VII A group have the highest electron affinity value among the period.
Question 8
1 / -0

Diagonal relationship is quite pronounced in the elements of:

A
$$ 2^{nd}$$ and $$3^{rd}$$ periods

B
$$ 1^{st}$$ and $$2^{nd}$$ periods

C
II and III groups

D
$$3^{rd}$$ and $$4^{th}$$ periods

Solution

A diagonal relationship exists between certain pairs of diagonally adjacent elements in the second and third periods of the periodic table.
Question 9
1 / -0

The correct order of electron affinity is:

A
$$Se< S< O$$

B
$$O < Se < S$$

C
$$ S< O< Se$$

D
$$ S< Se< O$$

Solution

Electron affinity increases from the first element to the second element in a group. It is applicable to all p-block element groups. Hence, oxygen has lesser electron affinity than that of sulphur and however in a group, it decreases from top to bottom as size increases.

Electron affinity of S is more than oxygen due to small size of oxygen. The addition of extra electron to oxygen causes more inter-electronic repulsion which decreases the electron affinity.

Hence, correct order is S > Se > O.

Option B is correct.
Question 10
1 / -0

Boron is diagonally related to:

A
boron

B
aluminium

C
magnesium

D
silicon

Solution

Boron and silicon are both semiconductors, form halides that are hydrolysed in water and form acidic oxides. Boron and silicon have diagonal relationship.

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Re-Attempt Weekly Quiz Competition

Classification of Elements and Periodicity in Properties Test - 21

Result

Classification of Elements and Periodicity in Properties Test - 21

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SHARING IS CARING

Question 1

-142 kJ/mol

-702 kJ/mol

-332 kJ/mol

-348 kJ/mol

Solution

Question 2

fluorine

nitrogen

chlorine

oxygen

Solution

Question 3

VII A group

V A group

VI A group

II A group

Solution

Question 4

nitrogen

oxygen

sulphur

phosphorous

Solution

Question 5

electron affinity

atomic volume

ions polarizing power

nuclear charge

Solution

Question 6

$$1s^{2}$$

$$1s^{2} 2s^{2}$$

$$1s^{2} 2s^{2} 2p^{4}$$

$$1s^{2} 2s^{2} 2p^{5}$$

Solution

Question 7

$$1s^{2}$$

$$1s^{2} 2s^{2}$$

$$ 1s^{2} 2s^{2} 2p^{4}$$

$$ 1s^{2} 2s^{2} 2p^{5}$$

Solution

Question 8

$$ 2^{nd}$$ and $$3^{rd}$$ periods

$$ 1^{st}$$ and $$2^{nd}$$ periods

II and III groups

$$3^{rd}$$ and $$4^{th}$$ periods

Solution

Question 9

$$Se< S< O$$

$$O < Se < S$$

$$ S< O< Se$$

$$ S< Se< O$$

Solution

Question 10

boron

aluminium

magnesium

silicon

Solution

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