Chemistry Test 29

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Chemistry Test 29

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Weekly Quiz Competition

Question 1
4 / -1

Which dioxide of group 16 element is not solid at room temperature?

A
SeO₂

B
TeO₂

C
SO₂

D
Both SO₂ and SeO₂

Solution

Among the given species SO₂ is gas while SeO₂ and TeO₂ are solids.
Question 2
4 / -1

The decreasing values of bond angles from NH₃ (106^o) to SbH₃ (101^o) down group-15 of the periodic table is due to

A
Increasing bp-bp repulsion

B
Increasing p-orbital character in sp³

C
Decreasing lp-bp repulsion

D
Decreasing electronegativity

Solution

Because of having same group decreasing electronegativity is the answer
Question 3
4 / -1

In XeF₂, the three lone pairs occupy:

A
Three equatorial position

B
Two axial and one equatorial position

C
Two equatorial and one axial position

D
Three axial positions

Solution

XeF₂ has sp³d hybridisation with two bond pairs and three lone pairs. To minimise the repulsion between the lone pairs and bond pairs, all the lone pairs occupy the equatorial positions. The bond pairs occupy the axial positions.
Question 4
4 / -1

Boron compounds behave as Lewis acid because of their

A
acidic nature

B
covalent nature

C
electron deficient behaviour

D
ionization property

Solution

A Lewis acid is therefore any substance, such as the H+ ion, that can accept a pair of nonbonding electrons. In other words, a Lewis acid is an electron-pair acceptor. In boron compound, boron has generally six electrons in its valence shell and hence can accept two more electrons.
Question 5
4 / -1

Graphite is a good conductor of electricity because:

A
It has sp ²- hybridized carbon atoms

B
It has free electrons and layers of carbon atoms

C
It is crystalline in nature

D
It has free atoms

Solution

Graphite contains layers of carbon atoms. The layers slide over each other easily because there are only weak forces between them, making graphite slippery. These electrons can move through the graphite, carrying charge from place to place and allowing graphite to conduct electricity.
Question 6
4 / -1

Among hypohalous acids, the acids with higher Ka value is:

A
HIO

B
HFO

C
HClO

D
BrOH

Solution

Greater the electronegativity of the halogen atoms in the oxyacid, greater is the acidic character of the oxoacid of halogen. HFO does not exist because F doesn’t form oxyacid due to the absence of d- orbitals in its valence shell. Hence, HClO has the highest Ka.

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Chemistry Test 29

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Chemistry Test 29

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Question 1

SeO2

TeO2

SO2

Both SO2 and SeO2

Solution

Question 2

Increasing bp-bp repulsion

Increasing p-orbital character in sp3

Decreasing lp-bp repulsion

Decreasing electronegativity

Solution

Question 3

Three equatorial position

Two axial and one equatorial position

Two equatorial and one axial position

Three axial positions

Solution

Question 4

acidic nature

covalent nature

electron deficient behaviour

ionization property

Solution

Question 5

It has sp ­2- hybridized carbon atoms

It has free electrons and layers of carbon atoms

It is crystalline in nature

It has free atoms

Solution

Question 6

HIO

HFO

HClO

BrOH

Solution

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SeO₂

TeO₂

SO₂

Both SO₂ and SeO₂

Increasing p-orbital character in sp³

It has sp ²- hybridized carbon atoms