Chemical Bonding and Molecular Structure Test 19

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Chemical Bonding and Molecular Structure Test 19

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Weekly Quiz Competition

Question 1
1 / -0

Which of the following posses two lone pairs of electrons on the cebtral atom and square planar in shape?
(i) $$SF _ 4$$ (ii) $$ XeO _ 4$$ (iii) $$XeF _ 4$$ (iv) $${ ICl }_{ 4 }^{ - }$$

A
I, III

B
III, IV

C
II, IV

D
All

Solution
Question 2
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Choose the correct options:

A
In $$O_2F_2$$, the $$O-F$$ bond length is lesser than expected value.

B
In trislyl amine $$(SiH_3)_3$$N, the bond length is lesser than expected value

C
The bond angle in $$OF_2$$ is lesser than in $$Cl_2O$$

D
The Be atom in $$BeCl_2(s)$$ is $$sp^3$$ hybridised.

Solution
Question 3
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The dipole moment of chlorobenzene is $$1.73 D$$. The dipole moment of $$p-dichlorobenzene$$ is excepted to be:

A
$$3.46 D$$

B
$$0.00 D$$

C
$$1.73 D$$

D
$$1.00 D$$

Solution

Dipole - moment of chlorobenzene is $$1.73$$D. The dipole moment of a molecule is determined by the electronegativity of elements in the molecule and the symmetry of the molecule. Because, p-dichlorobenzene i.e, $$1,4-$$dichlorobenzene is symmetrical, the molecule will have a zero dipole moment.
Question 4
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Covalancy of nitrogen in molecule is:

A
$$1$$

B
$$3$$

C
$$6$$

D
$$4$$

Solution

$$N=1s^22s^22p^3=3$$
Nitrogen has two $$2s$$ and three $$2p$$ valence electrons. By sharing the three $$2p$$ electrons,nitrogen can form three covalent bonds.So the co valency of nitrogen atom is 3.
Question 5
1 / -0

In $${ PO }_{ 4 }^{ 3- }$$ ion the formal charge on the oxygen atom of P-O bond is:

A
+1

B
-1

C
-0.75

D
+0.75

Solution

Formal charge on an atom $$=$$ total no. of values electron no. of lone pair $$+\dfrac{1}{2}$$ ( bonding electrons )
Formal charge on oxygen $$=6- \left[ 6+ \dfrac{1(2)}{2 \times 2} \right]$$
$$=6-7$$
$$=-1$$
We know that there are $$3$$ oxygen having charge than formal charge will be $$-1 \times 3 =-3$$
Now the formal charge on oxygen $$= -3/4 =-0.75$$
Question 6
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Which of the following involves transfer of five electrons?

A
$$MnO_4^ - \to M{n^{2 + }}$$

B
$$CrO_4^{2 - } \to C{r^{3 + }}$$

C
$$MnO_4^{2 - } \to Mn{O_2}$$

D
$$C{r_2}O_7^{2 - } \to 2C{r^{3 + }}$$

Solution

$$x + 4( - 2) = - 1$$
$$x - 8 = - 1$$
$$x = + 7$$
Question 7
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The main factor responsible for weak acidic nature of $$B-F$$ bonds in $$BF_3$$ is:

A
large electronegativity of F

B
three centred two electron bonds in $$BF_3$$

C
$$p \pi$$ - $$d \pi$$ back bonding

D
$$p \pi$$ - $$p \pi$$ back bonding

Solution

As refer to the above image, in $$BF_3$$ boron atom accepts the lone pairs of fluorine to form $$p^{\pi}-p^{\pi}$$ back bonding. Hence, its Lewis acidic character is decreased.
Question 8
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The strength of sigma bonds formed by axial overlap of $$s-$$ or $$p-$$ orbitals of $$2nd$$ shell of participating atom decreases as:

A
$$s-s>p-s>p-p$$

B
$$s-s>p-p>s-p$$

C
$$p-s>s-s>p-p$$

D
$$p-p>s-p>s-s$$

Solution
Question 9
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Which statement is correct :-

A
All the compounds having polar bonds, have dipole moment

B
$$SO_{2}$$ is non-polar

C
$$H_{2}O$$ molecule is non polar, having polar bonds

D
$$PH_{3}$$ is polar molecule having non polar bonds

Solution
Question 10
1 / -0

The number of anti-bonding electron pairs in $${O}_2^-$$ molecular ion on the basis of molecular orbital theory is (atomic no. of $$O$$ is $$8$$) :

A
$$5$$

B
$$2$$

C
$$7$$

D
$$6$$

Solution