Question # 1

Which of the following statements is not correct regarding bonding molecular orbitals?

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Bonding molecular orbitals possess less energy than atomic orbitals from which they are formed

Bonding molecular orbitals have low electron density between the two nuclei

Every electron in the bonding molecular orbitals contributes to the attraction between atoms

Bonding molecular orbitals are formed when the electron waves undergo constructive interference

The Electro-negatively difference for ionic bond must be greater than

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1.6

1.7

1.8

1.0

XeF₄has shape of

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Sphere

Trigonal bipyramidal

Tetrahedral

Square planar

Molecular orbital picture of N₂indicates

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One unpaired electron

Two unpaired electron

No unpaired electron

None of these

Which for the following has no dipole moment

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HCI

H₂S

H₂O

CO₂

The force which holds the atoms together to form a compound is called

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A chemical bond

Van der waal's force

Dispersion force

London force

Generally the bond formed by metals with non-metals is

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Ionic

Covalent

Polar

Non- polar

Which of the following phenomena will occur when two atoms of the elements having same spin of electron approach for bonding?

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Orbital overlap will not occur

Bonding will not occur

Both (A) and (B) are correct

None of the above are correct

Generally ionization energy of atoms decreases by

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Decreases in atomic size

Increase in atomic size

Increase in nuclear charge

None of these

Hydrogen chloride molecule contains

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Covalent bond

Double bond

Co-ordinate bond

Electrovalent bond

Maximum hydrogen bonds in water are

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4

3

2

8

H-bonding is not present in

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Glycerine

Water

Hydrogen sulphide

Hydrogen fluride

According to MO Theory, the species O₂+ possesses

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bond order of 2.5

three unpaired

diamagnetic character

stability lower then O₂

N-atom forms three covalent bonds, its electronic configuration is

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Three sp²hybrid are co-planar at an angle of

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104.5°

109.5°

107°

120°

Noble gases have the electronic configuration with their valance shell ns²np⁶except one

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He

Ne

Kr

Xe

The covalent bonds are

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Unidirectional

Bi-directional

Non-directional

Multi-directional

Among the alkaline earth metals the element forming predominantly covalent compounds is

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Be

Mg

Sr

calcium

B-atom in BF₃has

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sp³hybridization

sp²hybridization

sp hybridization

no hybridization

The three N - Hσ-bonds are made by

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sp³- s overlap

sp²- s overlap

P - p overlap

sp - overlap

From the difference between expected bond energies for the normal covalent bond and experimentally determined values Pauling calculated the values of

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Ionization potential of elements

Electron affinity of elements

Electronegativity of elements

Bond length

Atomic number of Al is 13. When it forms ionic bond with oxygen the number of electrons lost by 1 Al atom is

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1

2

3

4

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The ionization energy of A is high and electron affinity of B is low

The ionization energy of A is low and electron affinity of B is high

Both the ionization energy of A and electron off affinity of B are high

Both the ionization energy of A and electron affinity of B are low

Nitrogen in NH₃is sp³hybridized but the bond angle in NH₃is 107° and not 109.5° due to

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sp³orbital planar

sp³orbital trigonal

Repulsion between lone pair and bonded pairs

None of them

The bond order of individual C - C bond is benzene is

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One

Two

Between one and two

One and two alternately

Which is made by coordinate covalent bond

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H₃O⁺

H₂O

CH₄

HCl

Electronegativity values of the elements F, CI and Br vary

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F > CI > Br

Br > CI > F

Cl > Br > F

CI > F > Br

In OF₂, number of bond pairs and Ione paris of electrons are respectively

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2,6

2,8

2,10

2,9

The electron affinity of chlorine may be represented by the equation

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The boiling point of heavy water is

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108°C

101.4°C

99°C

110°C

On the basis of VSEPR theory SO₂is a

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Liner molecule

A bent molecule

A strong molecule

A gaseous molecule

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