CBSE Questions for Class 11 Medical Chemistry Chemical Bonding And Molecular Structure Quiz 11 - MCQExams.com

Which of the following contains maximum number of lone pairs on the central atom?
  • $$\mathrm{C}\mathrm{l}\mathrm{O}_{4}^{-}$$
  • $$\mathrm{X}\mathrm{e}\mathrm{F}_{4}$$
  • $$\mathrm{S}\mathrm{F}_{4}$$
  • $$\mathrm{I}_{3}^{-}$$
Which of the following orbitals can not undergo hybridisation amongst themselves?
$$(I)\ 3d, 4s$$ 
$$(II)\ 3d, 4d$$ 
$$(III)\ 3d, 4s$$ & $$4p $$ 
$$(IV) \ 3s, 3p$$ & $$4s$$
  • $$II$$
  • $$II$$ and $$III$$
  • $$I, II$$ and $$IV$$
  • $$II$$ and $$IV$$
Which of the following statements is incorrect?
  • Out of trimethylamine and trimethylphosphine, trimethylamine has higher dipole moment.
  • Out of $$(SiH_3)_2O$$ and $$(CH_3)_2O$$, $$(SiH_3)_2O$$ is more basic.
  • The critical temperature of the water is higher than that of $$O_2$$ because of $$H_2O$$ molecule has the dipole moment.
  • Intermolecular hydrogen bonding increases the enthalpy of vaporization of a liquid due to the increase in the attraction between molecules.
Which of the following types of bonds are present in $$CuSO_4\cdot 5H_2O$$?
I: Electrovalent II: Covalent III: Coordinate
  • I, II
  • II, III
  • I, III
  • I, II, III
Maximum covalency shown by $$Be$$ and $$B$$ is:
  • 2 and 3
  • 2 and 4
  • 4 and 3
  • 4 and 4
In $$XeF_2, XeF_4$$ and $$XeF_6$$, the number of lone pairs of $$Xe$$ is respectively:
  • $$2, 3, 1$$
  • $$1, 2, 3$$
  • $$4, 1, 2$$
  • $$3, 2, 1$$
In which of the following pairs, indicated bond is of greater strength?
118283.jpg
  • I
  • II
  • Both are equal
  • None of the above
Which among the following have two lone pair of electrons on center atom?
  • $$CO_2$$
  • $${ClF}_3$$
  • $$SO_3^{2-}$$
  • $$XeF_4$$
The ratio of lone pairs in $$\displaystyle XeF_{2}$$ molecule and the lone pairs on its central atom is:
  • $$3$$
  • $$4$$
  • $$5$$
  • $$6$$
In a molecule of phosphorus (V) oxide, there are:
  • $$4P-P, 10P-O$$ and $$4P = O$$ bonds
  • $$12P-O$$ and $$4P = O$$ bonds
  • $$2P-O$$ and $$4P = P$$ bonds
  • $$6P-P, 12P-O$$ and $$4P= P$$ bonds
Rotation around the bond (between the underlined atoms) is restricted in:
  • $$\displaystyle\:\underline{C}_{2}H_{4}$$
  • $$\displaystyle\:\underline{C}_{2}O_{2}$$
  • $$\displaystyle\:\underline{C}_{2}H_{2}$$
  • $$\displaystyle\:\underline{C}_{2}H_{6}$$
The total number of valence electrons in $$4.2\ gm$$ of $${N}_{3}^{-}$$ ion are :
  • $$2.2\ N_A$$
  • $$4.2\ N_A$$
  • $$1.6\ N_A$$
  • $$3.2\ N_A$$
The correct statement regarding $$SO_2$$ molecule is:
  • two $$p\pi-d\pi$$ bonds
  • molecule has 2 lone pair, $$2\sigma$$ bonds and $$2\pi$$ bonds
  • two $$p\pi-p\pi$$ bonds
  • one $$p\pi-p\pi$$ bond and one $$p\pi-d\pi$$ bond
Out of given reaction which show change in hybridization of central atom__________.
  • $${ H }_{ 2 }{ BO }_{ 3 }$$ dissolve in water
  • $${ H }_{ 2 }{ SO }_{ 4 }$$ dissolve in water
  • $${ N }_{ 2 }{ O }_{ 5(g) }\longrightarrow { N }_{ 2 }{ O }_{ 5(s) }$$
  • $$P{ Br }_{ 5(g) }\longrightarrow P{ Br }_{ 5(s) }$$
  • $${ C }_{ 2 }{ H }_{ 6 }\xrightarrow [ bond\ cleavage\ of\ C-C\ bond ]{ Homolytic } $$
Assuming the bond direction to the z-axis, which of the overlapping of atomic orbitals of two atoms ($$A$$) and ($$B$$) will result in bonding?
(I) $$s$$-orbital of $$A$$ and $$p_x$$ orbital of $$B$$
(II) $$s$$-orbital of $$A$$ and $$p_z$$ orbital of $$B$$
(III) $$p_y$$ orbital of $$A$$ and $$p_z$$ orbital of $$B$$
(IV) $$s$$-orbital of both ($$A$$) and ($$B$$)
  • I and IV
  • I and II
  • III and IV
  • II and IV
The distance between two neutral atoms in equilibrium is :
  • $$\displaystyle \sqrt\frac{2A}{B}$$
  • $$\displaystyle \left(\frac{2A}{B}\right)^\dfrac{1}{6}$$
  • $$\displaystyle \frac{2A}{B}$$
  • $$\displaystyle \left(\frac{2A}{B}\right)^\dfrac{1}{2}$$
Dipole moment of $$\displaystyle NH_{3}$$ is ________ than $$\displaystyle NF_{3}.$$
  • medium
  • less
  • more
  • none of the above
Match list I (Complex ions) with list II (number of unpaired electrons) and select the correct answers:
List IList II
A$$[CrF_6]^{4-}$$1One 
B$$[MnF_6]^{4-}$$2two
C$$[Fe(CN)_6]^{4-}$$3zero
D$$[Mn(CN)_6]^{4-}$$4four
5five
  • $$A-4, B-1, C-2, D-5$$
  • $$A-2, B-5, C-3, D-1$$
  • $$A-4, B-5, C-3, D-1$$
  • $$A-2, B-1, C-3, D-5$$
An ionic compound is expected to have tetrahedral structure if r+ / r- lies in the range of:
  • 0.414 to 0.732
  • 0.225 to 0.414
  • 0.115 to 0.225
  • 0.732 to 1
Which of the following combination of orbitals does not form any type of covalent bond (if z-axis is molecular axis)?
  • $$p_z+p_z$$
  • $$p_y+p_y$$
  • $$s+p_y$$
  • $$s+s$$
Consider the given lewis dot structure:
The formal charges on $$B$$ and $$F$$ are respectively.
189900.png
  • $$-1 , 0$$
  • $$-1 , -1$$
  • $$0 , -1$$
  • $$-1 , +1$$
Which plot best represents the potential energy $$(E)$$ of two hydrogen atoms as they approach one another to form a hydrogen molecule?
Which of the following orbital combination does not form $$\pi$$-bond?
  • $$p_x+p_x$$ sideways overlapping
  • $$d_{\displaystyle x^2-y^2}+p_y$$ sideways overlapping
  • $$d_{xy}+d_{xy}$$ sideways overlapping
  • $$d_{yz}+p_y$$ sideways overlapping
Which species has the maximum number of lone pair of electron on the central atom?
  • $${ \left( Cl{ O }_{ 3 } \right) }^{ - }$$
  • $$Xe{F}_{4}$$
  • $$Sn{F}_{4}$$
  • $${ \left( { I }_{ 3 } \right) }^{ - }$$
What is the formal charge on the chlorine atom in the oxyacid $$HOClO_2$$ if it contains single bonds ?
  • $$-2$$
  • $$-1$$
  • $$+1$$
  • $$+2$$
Assertion: In dilute benzene solutions, equimolar addition of $$R_3N$$ and $$HCl$$ produce a substance with a dipole moment. In the same solvent, equimolar addition of $$R_3N$$ and $$SO_3$$ produce a substance having an almost identical dipole moment.
Reason:($$ N-S$$) bond is a more polar bond.
  • Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
  • Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
  • Assertion is correct but Reason is incorrect
  • Assertion is incorrect but Reason is correct
  • Both Assertion and Reason are incorrect
The correct order of dipole moment is :
  • $$C{ H }_{ 4 }< N{ F }_{ 3 }< N{ H }_{ 3 }< { H }_{ 2 }O$$
  • $$N{ F }_{ 3 }< C{ H }_{ 4 }< N{ H }_{ 3 }< { H }_{ 2 }O$$
  • $$N{ H }_{ 3 }< N{ F }_{ 3 }< C{ H }_{ 4 }< { H }_{ 2 }O$$
  • $${ H }_{ 2 }O< N{ H }_{ 3 }< N{ F }_{ 3 }< C{ H }_{ 4 }$$
Assuming the additivity of covalent radii in the $$C - I$$ bond, what would be the iodine-iodine distance in each of the diiodobenzene? Assume that the ring is regular hexagon and that each $$C - I$$ bond lies on a line through the centre of the hexagon. (Take $$C- C$$ bond-length $$= 1.40\mathring{A}$$ radius of iodine atom $$=1.33\mathring{A}$$, radius of carbon atom $$= 0.77\mathring{A}$$) 
In $$o -, m -$$ and $$p -$$ isomers, bond angles are respectively $$60^o, 120^o$$ and $$180^o$$. Hence, the distance between two-atoms is:
  • $$3.5\mathring{A}$$
  • $$4.0\mathring{A}$$
  • $$7.0\mathring{A}$$
  • $$8.0\mathring{A}$$
In $$XeF_2$$, $$XeF_4$$ and $$XeF_6$$ the number of lone pairs on Xe is respectively__________.
  • 2, 3, 1
  • 1, 2, 3
  • 4, 1, 2
  • 3, 2, 1
For the type of interactions:$$(I)$$ Covalent bond, $$(II)$$ van der waal's forces, $$(III)$$ Hydrogen bonding, $$(IV)$$ Dipole-dipole interaction, which represents the correct order of increasing stability?
  • $$(I)< (III)< (II)< (IV)$$
  • $$(II)< (III)< (IV)< (I)$$
  • $$(II)< (IV)< (III)< (I)$$
  • $$(IV)< (II)< (III)< (I)$$
The $$C- C$$ single-bond distance is $$1.54\mathring {A}$$. What is the distance between the terminal carbons in propane? Assume that the Four bonds of any carbons atom are pointed towards the corners of a regular tetrahedron.
Plan structure of propane is assumed to be tetrahedral with bond angle of $$\theta = 109^o28'$$,. thus, form the value of $$\left(\frac{\theta}{2}\right)$$ and sin values, distance between terminal C-atoms can be determind. 
  • $$6.52\mathring{A}$$
  • $$4.52\mathring{A}$$
  • $$2.52\mathring{A}$$
  • None of these
The hybridizations of atomic orbitals of nitrogen in $$NO_2^+ ,\ N{ O }_3^-$$ and $$NH_4^+$$ respectively are :
  • $$sp,\ sp^2 $$ and $$sp^3$$
  • $$sp^2,\ sp$$ and $$sp^3$$
  • $$sp,\ sp^3$$ and $$sp^2$$
  • $$sp^2,\ sp^3$$ and $$sp$$
What is hybridization?
  •  The mixing of two or more atomic orbitals to form new orbitals that describe the covalent bonding in molecules.
  • The mixing of electrons in the electron sea model to account for the number of bonds in a molecule.
  • The mixing of two or more atomic orbitals to form new orbitals that describe the location of electrons in atoms.
  • The mixing of two or more molecules
  • The mixing of two or more atoms to make a new compound or molecule.
The formal charges of $$N_{(1)}, N_{(2)}$$ and $$O$$ atoms in $$: \overset {. .}{N_{(1)}} = N_{(2)} = \overset {. .}{O}:$$ are respectively
  • $$+1, -1, 0$$
  • $$-1, +1, 0$$
  • $$+1, +1, 0$$
  • $$-1, -1, 0$$
What is a non-bonding electron domain?
  • A lone pair of electrons
  • An area of electron density
  • A double bond
  • The area of electron density in an anion
What is the first thing you need to know to use the hybridization theory?
  • The number of valence electrons in the participating atoms.
  • The number of total electrons in the participating atoms.
  • Where the element lies on the periodic table.
  • How many of each molecule are being made.
  • The valence bond theory.
Which of the following best describes the term dipole moment?
  • When electrons are unevenly distributed within a molecule
  • When several atoms in a compound are electronegative
  • A non polar molecule
  • Having more than four dipoles

Calculate the formal charges on oxygen atoms 1, 2, 3 respectively.
475123_7b171b45fafe4614b1a7b483d7696b5c.png
  • 0, -1, +1
  • 0, +1, -1
  • 1, 0, -1
  • 1, 0, +1
The figure above represents any of the four trihalides of nitrogen, $$NF_{3}, NCl_{3}, NBr_{3}$$, and $$NI_{3}$$, where the X represents the halogen atoms. Here is some additional information regarding the elements involved.
ElementElectronegativityAtomic Radius
$$N$$$$3.0$$$$70 pm$$
$$F$$$$4.0$$$$64 pm$$
$$Cl$$$$3.0$$$$99 pm$$
$$Br$$$$2.8$$$$114 pm$$
$$I$$$$2.5$$$$133 pm$$
Of the four nitrogen trihalides, only one is not a molecular dipole. Which one is the nonpolar molecule, and why is it nonpolar?
531636_9bc4450eadb04def8d83ffa96c75227c.png
  • $$NI_{3}$$. The bond polarities off-set effect of the lone pair.
  • $$NBr_{3}$$. The bonds are virtually nonpolar, and the size of the bromine atoms cause the bond angles to be larger than the normal $$109.5^{\circ}$$ for tetrahedral orbital geometry.
  • $$NCl_{3}$$. Nitrogen and chlorine each have electronegativities of $$3.0$$, so the bonds are nonpolar, which means the molecule will be nonploar
  • $$NF_{3}$$. The electron density in the three N-F bonds is drawn toward the base of the trigonal pyramidal structure, while the lone pair place electron density at the top of the pyramid. The effects off-set.
Dipole moment of $$CH_2 X_2 > CH_3 X, $$ then $$X$$ is :
  • $$F$$
  • $$Cl$$
  • $$Br$$
  • $$I$$
The number of $$\sigma-bond$$ and $$\pi-bond$$ in $$HCP$$ are respectively:
  • $$2$$ and $$2$$
  • $$1$$ and $$3$$
  • $$2$$ and $$1$$
  • none of these
The $$H-F$$ bond and the $$H-I$$ bond have different values of their bond polarity. Which of the following statements correctly identifies the bond that is more polar and gives the correct reason for this difference?
  • The $$H-I$$ bond is more polar than the $$H-F$$ bond because iodine is more electronegative than fluorine.
  • The $$H-F$$ bond is more polar than the $$H-I$$ bond because fluorine is more electronegative than iodine.
  • Depends on the temperature.
  • None of these.
You have three solids. One is a metal; one is an ionic compound; one is a molecular/covalent compound. You test all three solid samples to identify their bonding.

SampleAppearanceMelting Point $$(
^{\circ}C)$$		Conductivity
AShiny$$962$$conductive
BCrystalline$$801$$conductive in aqueous solution
CPowdery$$186$$not conductive

Based on this data, identify the type of bonds present in each sample.
  • Sample A is a metal.

    Sample B is a salt.

    Sample C is a molecule.
  • Sample A is a molecule

    Sample B is a metal.

    Sample C is a salt.
  • Sample A is a salt.

    Sample B is a metal.

    Sample C is a molecule.
  • Sample A is a molecule.

    Sample B is a salt.

    Sample C is a metal.
In addition reactions of aldehydes, the carbonyl carbon atom changes from:
  • $$sp^3$$ to $$sp^2$$
  • $$sp^2$$ to $$sp^3$$
  • $$sp$$ to $$sp^3$$
  • $$sp^3$$ to $$sp$$
Among the following, the molecule of highest dipole moment is:
  • $$C{ Cl }_{ 4 }$$
  • $$N{ H }_{ 3 }$$
  • $${ H }_{ 2 }O$$
  • $$CH{ Cl }_{ 3 }$$
  • $$B{ F }_{ 3 }$$

Find the incorrect option with respect to the relevant characteristic.
  • $$NH_3> NF_3$$ (Dipole moment)
  • $$CO_2< CO_3^-2$$ (CO bond length)
  • $$NH_2^- < NH_4^+ $$ (Bond Angle)
  • $$I^->I^+$$ (Ionization energy)
If element $$Mn^{y+}$$ has spin only magnetic moment 1.732 BM, then:
  • Number of unpaired electron in $$ Mn^{+y}=1$$
  • $$y=4$$
  • $$y=6$$
  • Both $$(A) \& (C)$$
Hybridisation of carbon in $${ CH }_{ 2 }=CH-\overset { \oplus  }{ { CH }_{ 2 } }$$ is:
  • $${ sp }^{ 2 }$$
  • $$sp$$
  • $${ sp }^{ 3 }$$
  • all of these
Methanoic acid, $$HCOOH$$ has two different  $$C-O$$ bond lengths.
  • True
  • False
Complete the balanced and following reaction:


$$Na_2HPO_4 + X \rightarrow  Y + NaH_2PO_4$$
  • X = $$NaHCO_3$$

    Y = NaCl
  • X = $$HCO_{3}^-$$

    Y = $$NaHCO_3$$
  • X = $$NaHCO_3$$

    Y = $$H_2CO_3$$
  • X = $$H_2CO_3$$

    Y = $$NaHCO_3$$
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