Chemical Bonding and Molecular Structure Test 18

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Chemical Bonding and Molecular Structure Test 18

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Weekly Quiz Competition

Question 1
1 / -0

Which of the following molecules(s) have dipole moment?
I)$$Trans-pent-2-ene$$
II)$$cis-hex-3-ene$$
III)$$2,2-Dimethyl propane$$
IV)$$2,2,3,3-tertramethyl butane$$

A
I,II

B
II,III

C
I,III

D
I,IV
Question 2
1 / -0

Hydrogen combines with other element by

A
Losing an electron

B
Gaining an electron

C
Sharing an electron

D
Losing, gaining or sharing elecrtron

Solution

Hydrogen can combine with other elements by losing, gaining and sharing of electrons.

(i) Losing of electron $$:H_2+F_2\rightarrow 2H^++F^−$$

(ii) Gaining of electrons $$:2Na+H_2\rightarrow 2Na^++2H^−$$

(iii) Sharing of electrons$$:N_2+3H_2\xrightarrow[500^oC\ \\ \\ \\ \ \\ High \ pressure]{Fe+Mo}2NH_3$$

$$C+2H_2\xrightarrow[]{1200^oC}\ CH_4$$

$$\mathbf{Hence\ the\ correct\ answer\ is\ option\ (D).}$$
Question 3
1 / -0

Molecule AB has a bond length of 1.617 A and a dipole moment of 0.38 D. The fractional charge on each atom (absolute magnitude) is :
($${ e }_{ 0 }=\quad 4.802\quad \times \quad { 10 }^{ -10 }$$ esu)

A
$$0$$

B
$$0.05$$

C
$$0.5$$

D
$$1.0$$

Solution

Dipole moment $$(\mu )= q\times d$$
$$\mu = 0.38D$$ (given) = $$0.38\times 10^{-18}$$ esu cm
$$q=\frac{\mu }{d}=\frac{0.38\times 10^{-18}}{1.617\times 10^{-8}}$$
fractional charge = $$\frac{particle\, charge}{Total\, charge}$$
$$=\frac{0.38\times 10^{-18}}{1.617\times 10^{-8}\times 4.802\times 10^{-10}}$$
$$= 0.048$$
Question 4
1 / -0

Which of the following has the highest dipole moment?

A
$$AsH_3$$

B
$$SbH_3$$

C
$$PH_3$$

D
$$NH_3$$

Solution

As we go down a group, Electronegativity of elements decreases.
So, the difference between electronegativities of elements of a group and Hydogen decreases.
So, the dipole moment of trihydrides of a group decreases as we go down a group.
So, $$\mathrm{NH_3}$$ has the highest dipole moment among trihydrides of Nitrogen Family.

Hence, Option "D" is the correct answer.
Question 5
1 / -0

Which one of the following has the strongest $$O-O$$ bond?

A
$$O_{2}^{+}$$

B
$$O_{2}$$

C
$$O_{2}^{-}$$

D
$$O_{2}^{2-}$$

Solution

$$O^+_2$$ has $$15$$ electrons whose bond order is $$2.5$$
(Refer to Image) Stronger bond has higher bond order.
Hence, $$O^+_2$$ has strongest $$O-O$$ bond.
Question 6
1 / -0

One of the resonating structure of $$SO_{4}^{-2}$$ is as shown.
Which set formal charge on oxygen and bond order is correct?

A
$$-0.5$$ and $$1.5$$

B
$$1.5$$ and $$3$$

C
$$2$$ and $$3$$

D
$$1.5$$ and $$1.5$$

Solution

All resonating structures of $$SO_4^{2-}$$ are
(Refer to Image)
Formal charge on (1)= $$\cfrac {-1+0-1+0-1+0}{6}=-0.5$$
Bond order= $$\cfrac {1+2+1+2+1+2}{6}= \cfrac {3}{2}=1.5$$
Question 7
1 / -0

If the dipole moment of $$C-Cl$$ bond is $$1.2$$ $$D$$, then the resulting value of dipole moment in:

A
$$1.2$$ and $$0.6$$ respectively

B
$$0.6$$ and $$1.2$$ respectively

C
Less than $$1.2$$ $$D$$ and more than $$1.2$$ $$D$$ respectively

D
More than $$1.2$$ $$D$$ in both

Solution

net dipole moment's magnitude $$=\sqrt{ (1.2)^{2} + (1.2)^{2} +2 (1.2)^{2} \cos \theta }$$
$$=1.2\ D$$
net dipole moment's magnitude $$=\sqrt{(1.2)^{2} + (1.2)^{2} +2 (1.2)^{2} \cos \theta }$$
$$= (\sqrt{3})(1.2)\ D$$
Question 8
1 / -0

Hybridization of sulphur in $$SF$$$$_{4}$$ molecules are :

A
$$sp$$$$^{3}d^{3}$$

B
$$sp$$$$^{3}$$d

C
$$sp$$$$^{3}d^{2}$$

D
$$dsp$$$$^{2}$$

Solution
Question 9
1 / -0

Which of the following has least dipole moment:

A
$$NF_3$$

B
$$CO_2$$

C
$$SO_2$$

D
$$NH_3$$

Solution

$$CO_2$$ is a linear molecule, so our dipoles are symmetrical; the dipoles are equal in magnitude but point in opposite directions.

$$CO_2$$ has linear shape like shown in the image.

Due to this shape the dipoles of two oxygen atoms cancel each other and that is why $$CO_2$$ has

$$0$$ dipole moment.
Question 10
1 / -0

The bond angle and hybridization in ether $$(CH_3OCH_3)$$ is ______.

A
$$106.51^0 , sp^{2}$$

B
$$110^0$$ , $$sp^3$$

C
$$109.28^0, sp^3$$

D
None of these.

Solution