Question # 1

The overlapping of two partially filled atomic orbital is in such a way that the probability of finding the electron pair is maximum along the axis joining the two nuclei, the bond is

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Sigma bond

Pi bond

Ionic bond

Non-polar bond

Coordinate covalent bond is present in the molecules

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H₂O

BF₃

SiO₂

SO₂

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

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

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The driving force for making a bond is

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To attain noble gas electronic configuration

To make soled compounds

To make different compounds

To make gaseous substances

Shape of CIO₃is

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Triangular pyramidal

Tetrahedral

Triangular planar

Triangular bipyramidal

Which of the following has polar bond

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O₂

N₂

HCl

Cl₂

Generally electron affinities for elements in a period from left to right

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Decreases

Increases

Remain same

Increases alternatively

Size of an anion is increased as compared to its atom because of the

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Addition of new shell

Repulsion of electrons in the valence shell

Decrease in nuclear charge

Increase in the unclear charge

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

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Be

Mg

Sr

calcium

Which of the following geometry is associated with the compound in which the central atom assumes sp³d hybridization?

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Planar

Pyramidal

Angular

Trigonal bipyramidal

All covalent bonds formed between the two atoms are non-polar when

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Covalent bond between two non-metal atoms

Covalent bond between metal and non-metal

Covalent bond between two atoms of same element

Covalent bond between metal atoms

Which of the following species is paramagnetic?

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CO₂

NO

O^2-

CN

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

A molecule in which sp²hybrid orbitals are used by the central atom in forming covalent bonds in

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He₂

SO₂

PCl₅

N₂

Which is made by coordinate covalent bond

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H₃O⁺

H₂O

CH₄

HCl

The boiling point of heavy water is

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108°C

101.4°C

99°C

110°C

The geometry of 4 sp³hybrid orbitals on an atom is

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Square planar

Tetrahedral

Trigonal planar

Linear

Atoms obey octet rule by sharing-electrons making covalent bonds according to

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Lewis and Kossal theory

Valance bond theory

VSEPR theory

Molecular orbital theory

In which of the following theories the hybridizationis considered

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Vsepr

Lewis

Molecule orbital

Valence bond

Two H-atom combine to form a strong H₂molecule due to

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Increase in potential energy

Decrease in potential energy

Energy remains unchanged

Distance is increased

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

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

Which of the following molecules have multiple bonds

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CH₄

C₂H₄

C₂H₆

CCI₄

The number of antibonding electron pairs in O^2-molecular ion on the basis of MOT is

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4

3

2

5

Covalent compounds are soluble in

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Polar solvents

Non-polar solvents

Concentrated acids

All solvents

Hydrogen chloride molecule contains

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Covalent bond

Double bond

Co-ordinate bond

Electrovalent bond

The degree of polarity of molecule is known as its

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Dipole moment

Moment arm

Bond energy

Ionic character

Which of the following molecules has unpaired electrons in anti-bonding molecular orbitals?

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O₂

N₂

Br₂

F₂

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Excitantion of an electron from 2s to 2p-orbital

Transfer of three electrons from B to the other atoms

Excitation of two electrons form 2s orbital to 2p orbital

Formation of molecular ion

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