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Chemical Bonding and Molecular Structure

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Q 1. Element {tex} \mathrm { X } {/tex} is strongly electropositive and element {tex} \mathrm { Y } {/tex} is strongly electronegative. Both are univalent. The compound formed would be

{tex} \mathrm { X } ^ { + }\ \mathrm { Y } ^ { - } {/tex}

{tex} \mathrm X ^ { - } \ \mathrm X ^ { + } {/tex}

{tex} \mathrm X - \mathrm Y {/tex}

{tex} \mathrm X \rightarrow \mathrm Y {/tex}

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Q 2. The species having bond order different from that in {tex} \mathrm { CO } {/tex} is

{tex} \mathrm { NO } ^ { - } {/tex}

{tex} \mathrm { NO } ^ { + } {/tex}

{tex} \mathrm { CN } ^ { - } {/tex}

{tex} N _ { 2} {/tex}

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Q 3. What hybride orbitals are employed by carbon atoms {tex} 1,2 {/tex} and {tex} 3 , {/tex} respectively as labelled in the compound shown?

{tex} s p ^ { 3 } , s p , s p {/tex}

{tex} s p ^ { 3 } , s p ^ { 2 } , s p {/tex}

{tex} s p ^ { 3 } , s p , s p ^ { 2 } {/tex}

{tex} s p ^ { 3 } , s p ^ { 2 } , s p ^ { 2 } {/tex}

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Q 4. Which are non-polar molecules?

{tex} \mathrm { I }: \mathrm { NCl } _ { 3 } ; \quad \mathrm { II }: \mathrm { SO } _ { 3 } ; \quad \mathrm { III }: \mathrm { PCl } _ { 5 } {/tex}

{tex} \mathrm {I} {/tex} only

{tex} \mathrm {II} {/tex} only

{tex} \mathrm {I} {/tex} and {tex} \mathrm {II} {/tex} only

{tex} \mathrm {II} {/tex} and {tex} \mathrm {III} {/tex} only

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Q 5. {tex} \mathrm { C } - \mathrm { H } {/tex} bond distance is the longest in

{tex} \mathrm { C } _ { 2 } \mathrm { H } _ { 2 } {/tex}

{tex} \mathrm { C } _ { 2 } \mathrm { H } _ { 4 } {/tex}

{tex} \mathrm { C } _ { 2 } \mathrm { H } _ { 6 } {/tex}

{tex} \mathrm { C } _ { 2 } \mathrm { H } _ { 2 } \mathrm { Br } _ { 2 } {/tex}

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Q 6. An ionic compound {tex} A ^ { + } B ^ { - } {/tex} is most likely to be formed from {tex} A {/tex} and {tex} B {/tex} when

Ionization energy of {tex} A {/tex} is low

Electron affinity of {tex} B {/tex} is low

Electronegativity of {tex} B {/tex} is low

Ionization energy of {tex} B {/tex} is low

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Q 7. Compound {tex} X {/tex} is highly volatile and insoluble in water. Bonding in {tex} X {/tex} is

Ionic

Covalent

Polar covalent

Coordinate

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Q 8. The structure of {tex} 1,3 {/tex} -butadiene is {tex} \mathrm { CH } _ { 2 } = \mathrm { CH } - \mathrm { CH } = \mathrm { CH } _ { 2 } {/tex} and the distance between the central carbon atom is {tex} 1.46 \mathrm { {\text{Å}}} \text { (instead of } 1.54 {\text{Å}} ) {/tex}. This is due to

Existence of on-octet resonance structures involving double bonding between the central carbon atoms

Decrease in bond length when terminal double bonds exist

{tex} s p ^ { 2 } - s p ^ { 2 } {/tex} overlapping

{tex} p - p {/tex} overlaping

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Q 9. In {tex} \mathrm { I } _ { 3 } ^ { - } , {/tex} Lewis base is

{tex} \mathrm { I } _ { 2 } {/tex}

{tex}\mathrm I ^ { - } {/tex}

{tex}\mathrm { I }_ { 2 } ^ { + } {/tex}

{tex} \mathrm { I }_{ 2 }^{-} {/tex}

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Q 10. Which among the following sulphates is insoluble in water?

{tex} \mathrm { CuSO } _ { 4 } {/tex}

{tex} \mathrm { CdSO } _ { 4 } {/tex}

{tex} \mathrm { PbSO } _ { 4 } {/tex}

{tex} \mathrm { Bi } _ { 2 } \left( \mathrm { SO } _ { 4 } \right) _ { 3 } {/tex}

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Q 11.

Which represents metallic character in an element?

None of these

Partially filled bonds or overlapping bonds represent metal

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Q 12.

The enolic form of acetone contain

bonds, bond and 1 lone pair

Two lone pairs on O-atom

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Q 13.

The common features among the species

Bond order three and isoelectronic

Bond order three and weak field ligands

Bond order two and

Isoelectronic and weak field ligands

| | | |

| 14 14 14 | 3 3 3 | Strong Strong weak |

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Q 14.

The high density of water compared to ice is due to

Hydrogen bonding interactions

Dipole-dipole interactions

Dipole-induced dipole interactions

Induced dipole induced dipole interactions

Due to H-bonding in water molecules, water has high density

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Q 15.

Among the following species, identify the isostructural pairs

Thus,

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Q 16.

Which combination will give the strongest ionic bond?

Force of attraction between cation and anion is

Where,

**Size of**

**Charge on**

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Q 17.

Ratio of

Naphthalene

Tetracyano methane

Enolic form of urea

equal

C

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Q 18.

In which pair or pairs is the strongest bond found in the first species?

I:

I only

II only

I and III only

II and III only

**Bond order**

I.

II.

III.

Larger the bond order, greater the bond energy

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Q 19.

Benzyl chloride

Benzoyl chloride

Chlorobenzene

Allyl chloride

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Q 20.

Select the correct statement about resonance

The larger the number of the contributing structures, the greater the stability of the molecule

Greater number of the covalent bonds add to the stability of the molecule

The positive charge should reside, as far as possible, on the less electronegative element

All the above are correct statements

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Q 21.

Which of the following have identical bond order?

I.

III.

I, III

II, IV

I, II, III

I, IV

| | |

I. | 14 | 3.0 |

II. | 17 | 1.5 |

III. | 14 | 3.0 |

IV. | 12 | 2.0 |

I and II have same bond-order

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Q 22.

The geometry of the atoms in the species

Tetrahedral

Square

Trigonalbipyramidal

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Q 23.

In a Lewis dot structure, the electrons which complete an octet but are not located between two atoms are referred to as

Bonding pairs

Delta minus electrons

Excess electrons

Lone pairs

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Q 24.

Which one of the following compounds has the electron-pair geometry as the trigonalbipyramidal with three equatorial positions occupied by lone pairs of electrons?

(a)

(b)

(c)

(d)

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Q 25.

Correct Lewis structure is

In (c), octet of

In (a), (b) and (d), octets of C, N and O as expected are not complete

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