Chemical Bonding and Molecular Structure Test 14

Result

Chemical Bonding and Molecular Structure Test 14

Score
-
out of -
Rank
-
out of -

TIME Taken - -

SHARING IS CARING

If our Website helped you a little, then kindly spread our voice using Social Networks. Spread our word to your readers, friends, teachers, students & all those close ones who deserve to know what you know now.

Weekly Quiz Competition

Question 1
1 / -0

Which of the following has the maximum value of dipole moment?

A

B

C

D

Solution

Here, Chlorine is more electronegative than $$NO_2$$.
Therefore, for chlorine the dipole moment will be greater than that for $$NO_2$$.
Also, $$\mu=e\times d$$
The greater the distance between the atoms, the higher will be the dipole moment.
Therefore, the distance is greater in IMAGE $$01$$ and IMAGE $$02$$.
Therefore, IMAGE $$01$$ has the maximum value of dipole moment.
Question 2
1 / -0

The molecular that will have dipole moment IS ZERO

A
2,2-Dimethylpropane

B
Cis-2-butane

C
Trans-2-pentene

D
2,2,3,3-Tereathylpentane

Solution
Question 3
1 / -0

In which of the following dimer empty atomic orbital of central atom of monomer does not involve in hybridisation?

A
$$Ga_2H_6$$

B
$$Al_2Br_6$$

C
$$Be_2H_4$$

D
$$Cl_2O_6$$

Solution

Dichlorine hexoxide is the chemical compound with the molecular formula $$Cl_2O_6$$, which is correct for its gaseous state. However, in liquid or solid form, this chlorine oxide ionizes into the dark red ionic compound chloryl perchlorate $$[ClO_2]^+[ClO_4]^−$$, which may be thought of as the mixed anhydride of chloric and perchloric acids.

$$Ga_2H_6,Al_2Br_6,Be_2H_4$$ have no empty orbital only in $$Cl_2O_6 $$ $$Cl$$has empty orbital and $$Cl_2O_6$$ dimer empty atomic orbital of central atom of monomer does not involve in hybridisation.
Question 4
1 / -0

Peroxide linkage is present in :

A
$$H_2O$$

B
$$BaO_2$$

C
$$OF_2$$

D
$$H_2SO_4$$

Solution

Peroxide linkage
means (0-0) linkage
this linkage is present in $$BaO_2$$ which is barium oxidation .
refer to image
B is the correct answer.
Question 5
1 / -0

The dipole moment of a bond $$AB$$ is $$5\ D$$ and its bond distance is $$150\ pm$$. The percentage ionic charactor of this bond is?

A
$$78.5\%$$

B
$$83\%$$

C
$$24\%$$

D
$$69.5\%$$

Solution

Dipole moment= charge $$\times$$ distance between the dipoles
$$=1.6 \times 10^{-19}\times 150 \times 10^{-12}$$ ($$1$$ pm= $$10^{-12}$$m)
$$=\cfrac {240 \times 10^{-31}}{3.336}=7.190$$ ($$10=3.336 \times 10^{-30}$$cm)
% of ionic character= $$\cfrac {5}{7.19}\times 100=69.54$$%
Question 6
1 / -0

A diatomic molecule has a dipole moment of 1.2D. If the bond distance is $$1.0 \mathring{A}$$, fraction of an electronic charge on each atom is:

A
$$10\%$$

B
$$20\%$$

C
$$25\%$$

D
$$50\%$$

Solution

Electronic charge $$'e'=\dfrac { Dipole\quad moment }{ Bond\quad length } =\dfrac { 1.2\times { 10 }^{ -18 }esucm }{ 1\times { 10 }^{ -18 }cm } =1.2\times { 10 }^{ -10 }esu$$
Now fraction of electronic charge $$=\dfrac { 1.2\times { 10 }^{ -10 } }{ 4.8\times { 10 }^{ -10 } } =0.25$$
$$\because$$ charge of electron $$=4.8\times { 10 }^{ -10 }esu=25$$% of $${ e }^{ - }$$
Ans :- Option C.
Question 7
1 / -0

The dipole moment of is $$1.5\ D$$. The dipole moment of?

A
$$0\ D$$

B
$$1.5\ D$$

C
$$2.86\ D$$

D
$$2.25\ D$$

Solution
Question 8
1 / -0

Which of the following pair of molecules will have permanent dipole moments for both members?

A
$$SiF_{4}$$and $$NO_{2}$$

B
$$ CO_{2}$$ and $$NO_{2}$$

C
$$ CO_{2}$$ and $$O_{3}$$

D
$$SiF_{4}$$ and $$CO_{2}$$

Solution

As $$CO_2$$ is a linear molecule, thus its net dipole moment is zero.
(Refer to Image 1)
$$SiF_4 \longrightarrow$$ tetrahedral geometry (Refer to Image 2)
Net dipole moment is not zero.
$$NO_2 \longrightarrow$$ bent structure, because of lone pair of Nitrogen
(Refer to Image 3)
Thus net dipole moment is not zero.
Thus $$SiF_4$$ & $$NO_2$$ both contain permanent dipole moment.
Question 9
1 / -0

If dipole moment of HI is $$0.38$$D and bond length of HI is $$1.6 AA$$, then percentage covalent characted in HI bond is?

A
$$4.95 \%$$

B
$$5.9 \%$$

C
$$95.05 \%$$

D
$$47.5 %$$

Solution
Question 10
1 / -0

Which of the following has zero dipole moment?

A
$$BF_3$$

B
$$BeClBr$$

C
$$CH_2Cl_2$$

D
COS

Solution

In $$BF_3$$ the shape of the molecule is trigonal planar. The three $$F$$ are so attached to $$B$$ that the resultant dipole due to two $$B-F$$ bonds cancels the third dipole. Hence the overall dipole moment of the molecule is $$0$$. Hence the correct option is $$A$$.