Chemical Bonding and Molecular Structure Test 35

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Chemical Bonding and Molecular Structure Test 35

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Weekly Quiz Competition

Question 1
1 / -0

Which of the following molecules does not have a dipole moment?

A
$$IBr$$

B
$$CHCl_3$$

C
$$CH_2Cl_2$$

D
$$BF_3$$

Solution

Due to symmetrical strucure it has zero dipole moment.
Question 2
1 / -0

Which of the following combination of orbitals does not form any type of covalent bond (if z-axis is molecular axis)?

A
$$p_z+p_z$$

B
$$p_y+p_y$$

C
$$s+p_y$$

D
$$s+s$$

Solution

$$s+p_y$$ doesnt form covalent bond. as $$p_y$$ is oriented along $$y$$ axis and $$s$$ is non-directional. So according to $$VBT$$ they will not form a covalent bond.
Question 3
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$$Cl - Cl$$ distance in structure $$(A)$$ is:

A
$$2.32 A^{\circ}$$

B
$$4.64 A^{\circ}$$

C
$$1.16 A^{\circ}$$

D
$$9.28 A^{\circ}$$

Solution

In structure (A), $$Cl - Cl$$ bond length is twice the distance between $$Pt $$ and $$Cl$$.
Hence, the $$Cl-Cl$$ bond length is $$2\times 2.32 = 4.64 A^o$$.
Question 4
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Which plot best represents the potential energy $$(E)$$ of two hydrogen atoms as they approach one another to form a hydrogen molecule?

A

B

C

D

Solution

At large distances, the energy is zero, meaning that there is no interaction. This agrees with our understanding that two atoms placed infinitely far apart do not interact with each other in any meaningful way, or at the very least we can say that they are not bonded to each other. As the atoms start approaching one another, the force of attraction between the nucleus of one and electron of the other, and vice versa comes into play. Similarly repulsive forces between the two nuclei and between the two atom's electrons also exists. The distance at which the repulsive forces are exactly balanced by attractive forces is bond length. Here, the energy is minimum. If the two atoms are further brought closer to each other, repulsive forces become more dominant and energy increases.
Question 5
1 / -0

Directions For Questions

A paper published in the research journal Science in 2007 (S. Vallina and K. Simo, Science, 305, 506 Jan 26, 2007) reported studies of dimethyl sulphide (DMS, an important green house gas that is released by marine phytoplankton. This gas represents the largest natural source of atmospheric sulphur and a major precursor of hygroscopic (i.e., cloud forming) particles in the clean air over the remote oceans, thereby acting to reduce the amount of solar radiation that crosses the atmosphere and is absorbed by the ocean.

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Steric number of sulphur is DMS is:

A
$$2$$

B
$$3$$

C
$$4$$

D
$$5$$

Solution

In DMS, $$S$$ is bonded to $${ CH }_{ 3 }$$ by $$2$$ single bond, the $$S$$ atom also has $$2$$ lone pairs.The steric number will be $$2+2=4$$.
Question 6
1 / -0

Correct order of dipole moment is:

A
$$I = II = III$$

B
$$I < II < III$$

C
$$I > II > III$$

D
$$II < III < I$$

Solution

As in I compound both groups have strong -I effect so it has the highest dipole moment, then III have both groups with +I effect so it has a second-highest dipole moment.
so order is $$III < II < I$$.

Hence, the correct option is $$C$$
Question 7
1 / -0

Directions For Questions

The space model which is obtained by joining the points representing various bonded atoms gives the shape of the molecule. The geometry of the molecule is definite relative arrangement of the bonded atoms in a molecule. The shape and geometry of a molecule is explained by valence shell electron pair repulsion theory given by Gillespie and Nyholm.

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Select the correct code for the following repulsion orders, according to VSEPR theory
(I) lone pair-lone pair $$>$$ lone pair-bond pair
(II) lone pair-bond pair $$>$$ bond pair-bond pair
(III) lone pair-lone pair $$>$$ bond pair-bond pair
(IV) lone pair-bond pair $$>$$ lone pair-lone pair

A
$$I, II$$ and $$III$$

B
$$II$$ and $$IV$$

C
$$I, II$$ and $$IV$$

D
All
Solution
According to the $$VSEPR$$ theory, lone pairs of electrons occupy more space than bonding pairs. As a consequence, this is an order of the magnitude of repulsion.

$$lp-lp>lp-bp>bp-bp$$
Greatest repulsion is between 2 lone pairs.
Followed by repulsion between one lone pair and one bonding pair.
The weakest repulsion is between 2 bonding pairs, the magnitude of repulsion between bonding pairs of electrons depends on the $$EN$$ difference between a central atom and the other atoms.
Question 8
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Which species has the maximum number of lone pair of electron on the central atom?

A
$${ \left( Cl{ O }_{ 3 } \right) }^{ - }$$

B
$$Xe{F}_{4}$$

C
$$Sn{F}_{4}$$

D
$${ \left( { I }_{ 3 } \right) }^{ - }$$

Solution

$${ I }_{ 3 }^{ - }$$ has the maximum number of lone pair of electron on the central atom.
$${ I }_{ 3 }^{ - },Xe{F}_{4},S{F}_{4}$$ and $$Cl{ O }_{ 3 }^{ - }$$ have $$3,2,1,1$$ lone pair of electron respectively.
Question 9
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Among the following, the molecule with the highest dipole moment is:

A
$$C{ H }_{ 3 }Cl$$

B
$$C{ H }_{ 2 }{ Cl }_{ 2 }$$

C
$$CH{ Cl }_{ 3 }$$

D
$$C{ Cl }_{ 4 }$$

Solution

$$C{ H }_{ 3 }Cl$$ has a greater dipole moment because of the $$C{H }_{ 3 }-$$ is a strong electron donor. The atoms are in a tetrahedron with the carbon in the centre. The electronegativity of the chlorine creates the dipole and three of them create a greater net force.
$${ \mu }_{ C{

Cl }_{ 4 } }=0,{ \mu }_{ CH{ Cl }_{ 3 } }=1.0D,{ \mu }_{ C{ H }_{ 2

}{ Cl }_{ 2 } }=1.6D,{ \mu }_{ C{ H }_{ 3 }Cl }=1.86D$$
$$C{ H }_{ 3 }Cl$$ has the highest dipole moment.
Question 10
1 / -0

What is the formal charge on the chlorine atom in the oxyacid $$HOClO_2$$ if it contains single bonds ?

A
$$-2$$

B
$$-1$$

C
$$+1$$

D
$$+2$$

Solution

formal charge= valence electrons-(lone electrons+bonds)
$$=7-(2+3)=+2$$