Question # 1

Which of the following molecules has a net dipole moments

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CO₂

CS₂

SO₂

CCI₄

Outer shells of two elements X and Y have two and six electrons respectively. If they combine, the expected formula of compound will be

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XY

X₂Y

X₂Y₃

XY₂

The electronegativity of elements in a period from left to right

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Decreases

Increases

First decreases then increases

First increases then decreases

Hydrogen chloride molecule contains

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Covalent bond

Double bond

Co-ordinate bond

Electrovalent bond

According to VSEPR theory, the shape of the water molecule is

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Octahedral

Distorted tetrahedral

Planar triangle

Linear

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

Shape of CIO₃is

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Triangular pyramidal

Tetrahedral

Triangular planar

Triangular bipyramidal

The tendency of an atom to attract shared electron pair towards itself is called

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Covelent bond

Electronegativity

Ionization potential

Electronic affinity

Planar geometry of molecules is due to

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sp³hybridization

sp²hybridization

sp hybridization

P - p overlap

Water H₂O is liquid while hydrogen sulphide H₂S is a gas beause

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Water has higher molecular weight

Hydrogen sulphide is a weak acid

Sulphure has high electronegativity than oxyhe

Water molecules associate through hydrogen bonding

SnCI₂have ______ shape

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Planner

Tetrahedral

Angular

None

Which of the following charge

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Li

Be

H

He

In sp²hybridization bond angle is _____

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120°

180°

109.5°

None

If two lone pairs are present then bond angle of tetrahedral compound reduces to ______ degrees

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109.5°

107.5°

104.5°

None

On the basis of VSEPR theory SO₂is a

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Liner molecule

A bent molecule

A strong molecule

A gaseous molecule

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

Covalent compounds are soluble in

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Polar solvents

Non-polar solvents

Concentrated acids

All solvents

The boiling point of heavy water is

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108°C

101.4°C

99°C

110°C

Inter molecular forces in solid hydrogen are

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Covalent forces

Van der Waal forces or London dispersion forces

Hydrogen bonds

All of these

When two hydrogen atoms approach to form a chemical bond

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The repulsive forces dominate the attractive forces

The attractive forces, dominate the repulsive forces

The energy of atoms increases

The two atoms start ionization

The shape of the molecule SF₂Cl₂is

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Trigonal bipyradmidal

Cubic

Octahedral

Tetrahedral

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

The electronegativeities of F,Cl,Br and I are 4.0,3.0,2.8,2.5 respectively.Hydrogen halide with a high percentage of ionic character is

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HF

HCL

HBr

HI

The shape of CIO^-₃according to valence shell electron pair repulsion theory will be

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Planar triangle

Pyramidal

Tetrahedral

Square planar

When of the following is isolelectronic with krypton

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Ca⁺⁺

Al⁺⁺⁺

Br^-1

I^-1

One of the following bonds is polar but compound is non-polar

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H₂O

NH₃

HCl

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

Which of the following molecules have multiple bonds

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CH₄

C₂H₄

C₂H₆

CCI₄

The three N - Hσ-bonds are made by

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sp³- s overlap

sp²- s overlap

P - p overlap

sp - overlap

B-atom in BF₃has

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sp³hybridization

sp²hybridization

sp hybridization

no hybridization

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