p-Block Elements Test

Result

p-Block Elements Test - 39

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Weekly Quiz Competition

Question 1
1 / -0

Group 16 elements have a lower value of first ionization enthalpy as compared to group 15 elements because:

A
Half filled p-orbitals in group 15 elements are more stable

B
Group 16 elements have smaller size than group 15 elements

C
Group 16 elements contain double bond while group 15 elements have triple bond

D
Group 16 elements have more number of electrons in p-orbitals

Solution

Group 16 elements have a lower value of first ionization enthalpy as compared to group 15 elements. As group 15 elements have half filled p-orbital due to which group 15 have got extra stability.
Question 2
1 / -0

Covalency of oxygen cannot exceed 2 unlike sulphur which can show +4 or +6 because

A
Oxygen atom does not have d-orbitals

B
Oxygen atom has two unpaired electrons in its valence shell

C
Oxygen can form a double bond with another oxygen atom

D
Dectrons of oxygen atom cannot be promoted to d-orbitals due to its small size

Solution

Oxygen does not have a d-orbital thereby not exceeding its covalency beyond 2. Whereas sulphur has vacant d-orbitals hence can exceed its covalency to +4 or +6.
Question 3
1 / -0

Bond angle in H₂O(104.5^∘) is higher than the bond angle of H₂S (92.1^∘). The difference is due to:

A
O is diatomic and S is tetra-atomic

B
Difference in electronegativity of S and O

C
Difference in oxidation states of S and O

D
Difference in shapes of hybrid orbitals of S and O

Solution

The difference in the bond angles is linked with the electronegativities of oxygen and sulphur atoms. As we move down the group from O to Te, the size of the central atom goes on increasing and its electronegativity goes on decreasing.
As a result, the position of the two bond pairs shifts away and away from the central atom as we move from H₂O to H₂Te. Consequently, the repulsion between the bond pairs decreases as we move from H₂O to H₂Te and therefore, the bond angle decreases in the order.
Question 4
1 / -0

Arrange the following hydrides of group 16 elements in order of increasing stability:

A
H₂S < H₂O < H₂Te > H₂Se

B
H₂O < H₂Te < H₂Se < H₂S

C
H₂O < H₂S < H₂Se < H₂Te

D
H₂Te < H₂Se < H₂S < H₂O

Solution

There is a decrease in bond enthalpy (H- E) the size of the element increases on moving down the group hence, the stability decreases on moving down group.
Question 5
1 / -0

The hybridisation of sulphur in sulphur tetrafluoride is:

A
sp³ d

B
sp³ d²

C
sp³ d³

D
sp³