Chemistry Chapter 4 Mock Test

Arrange the given compounds in the order of increasing dipole moment.

(I)Toluene (II) m- dichlorobenzene

(III) o-dichlorobenzene (IV) p- dichlorobenzene

IV<II<I<III
IV<I<III<II
IV<I<II<III
I<IV<II<III

Find the number of bonding electron pairs in white phosphorous.

12
8
6
4

The molecule that has the highest bond order is:

\(O_{2}\)
\(He_{2}\)
\(Li_{2}\)
\({N}_2\)

A bond is formed_______ with maximum covalent character between non-metallic elements.

between identical atoms
between atoms of the same size
between chemically similar atoms
between atoms of widely different electronegativities

What is the shape of IF₇ molecule?

Tetrahedral
Trigonal bi-pyramidal
Pentagonal bi-pyramidal
Octahedral

Find the number of nodal planes that ‘ d’ orbital possess.

Three
Two
One
Four

What is the bond angle in sp\(^{2} \)hybridization?

90°
109°2'
120°
180°

Which is the mode of hybridization of carbon in CO₂?

\(sp^{3}\)
\(sp^{2}\)
sp
None of these

Find the electron pair which forms a bond between two similar non-metallic atoms.

Equally shared in between the two
In a similar spin condition
By complete transfer from one atom to other
Dissimilar shared between the two

Molecule that has trigonal planar geometry is:

\(BF_{3}\)
\(NH_{3}\)
\(PCl_{3}\)
\(IF_{3}\)

What is the shape of a molecule of NH₃ in which central atoms contains lone pair of electron?

Pyramidal
Square planar
Planar trigonal
Tetrahedral

The halides that has maximum melting point is:

NaF
Nal
NaBr
NaCl

If the electron pair forming a bond between two atoms A and B is not in the center then which is the bond?

\(\pi\) bond
non-polar bond
polar bond
single bond

What is H₂O?

A bent (angular) triatomic molecule
A linear triatomic molecule
Both of these
None of these

The paramagnetism of O₂ molecule is because of the presence of_______ according to molecular orbital theory.

unpaired electrons in the anti-bonding\(\Pi \) molecular orbital
unpaired electron in the bonding \(\Pi \) molecular orbital
unpaired electrons in the anti-bonding\( \sigma\) molecular orbital
unpaired electrons in the bonding\( \sigma\) molecular orbital

Formula that does not correctly represent the bonding capacity of the atom involved is:

The ionization of hydrogen atom would give rise to ______.

hydroxyl ion
proton
hydronium ion
hybrid ion

Compounds that is ionic is________.

\(CH_{4}\)
KI
\(H_{2}\)
Diamond

Statement 1 :\( \sigma \) is strong whereas \( {\pi} \) is a weak bond

Statement 2 : Atoms rotate freely about \( \pi \) bond

Both statement 1 and statement 2 are true and the statement 2 is the correct explanation of the statement 1.
Both statement 1 and statement 2 are true but statement 2 is not the correct explanation of the statement 1.
statement 1 is true but statement 2 is false.
The statement 1 and statement 2 both are false.

Liquids that is not deflected by a non-uniform electrostatic field is:

Hexane
Nitrobenzene
Chloroform
Water

Which is the correct statement about electrovalent compound’s?

Are insoluble in polar solvent
Conduct current in fused state
Boiling points are low
Belting points are low

Which of the following molecules which contains unpaired electrons?

Hydrogen peroxide
Molecular oxygen
Molecular nitrogen
Carbon monoxide

Electrovalent compounds generally have_______ as compared to covalent compounds.

high melting points and high boiling points
high melting points and low boiling points
low melting points and high boiling points
low melting points and low boiling points

_____shows least dipole character.

Ether
Ethane
Ethanol
Water

The bond energies of H – H and cl – cl are 430 kJ mol^-1 and 242 kJ mol^-1 respectively, \(\Delta H_{t}\) for HCI is given as 91 kJ mol^–¹. What will be the bond energy of HCI?

245 kJ
285 kJ
427 kJ
766 kJ

Which of the following does NOT contain isoelectronic species?

\({BO}^{3-}_{3}\) , \( {CO}^{2-}_{3}\) , \({NO}_{3}^{-}\)
\({SO}^{2-}_{3}\) , \({CO}^{2-}_{3}\), \({NO}_{3}^{-}\)
\({CN}^{-}\) , \({N}_{2}\), \({C}_{2}^{2-}\)
\({PO}^{3-}_{4} , {SO}^{2-}_{4}, {ClO}_{4}^{-} \)

______is non-linear molecule.

\(BeCl_{2}\)
\(CS_{2}\)
\(CO_{2}\)
\( CO_{3}\)

What is the bond order in \({C}_{2}\) molecule according to the molecular orbital theory?

3
2
1
0

What will be the structure of the compound formed by sp³d hybridization?

Trigonal bipyramidal
Angular
Pyramidal
Planar

Find the percentage of s-character of the hybrid orbitals in methane, ethene and ethyne respectively.

10,20,40
25, 33, 50
25, 50, 75
50, 75, 100

What is the bond order of \(He^{+}_{2}\) molecule ion?

\(\frac{1}{4}\)
\(\frac{1}{2}\)
2
1

The atoms are bonded by _____ in\( N_{2}\) molecule

three \(\sigma \)bonds
two \( \alpha\) One \( \sigma\)
one \( \alpha\) One \(\sigma\)
one \( \alpha \)Two \( \sigma\)

What is the structure of \(XeF_{2} \) molecule?

Square planar
Linear
Pyramidal
Triangular planar

Which one has lowest probable inter atomic forces in the following metals?

Mercury
Zinc
Silver
Copper

______shows \(dsp^{2}\) hybridization.

\({ PtCl }^{2-}_{4}\)
\({ NH }^{+}_{4}\)
\(SCl _{4}\)
\({ NiCl }^{2-}_{4}\)

______ does not show hydrogen

Ethyl ether
Acetic acid
Ethyl alcohol
Chloroform

Find the force that holds atoms together in an electrovalent bond.

electrostatic force of attraction
Vander Waal's force
dipole attraction force
all the above

105° is the bond angle between two hybrid orbitals. Find the % s-orbital character of hybrid orbital.

Between 22-23%
Between 21-22%
Between 19-20%
Between 20-21%

Find the increasing order for polarisability of halide ions.

\(F ^{-}, Cl^{-}, Br^{-}, I^{-}\)
\(I^{-}, Br^{-}, Cl^{-}, F^{-}\)
\(Cl^{-}, Br^{-}, I^{-}, F^{-}\)
\(F^{-}, I^{-}, Br^{-}, Cl^{-}\)

Find the correct order of bond length.

None of these

Find the maximum possible number of hydrogen bonds in which an \(H_{2} O\) molecule can participate

4
3
5
2

Find the incorrect statement from the following statements.

\(dsp^{3 }\)hybrid orbitals are all at 90° to one another
.\(d^{2}sp^{3 }\) hybrid orbitals are directed towards the corners of a regular octahedron
\(Sp^{2}\)sp2 hybrid orbitals are formed from two p atomic orbitals and one s atomic orbital
Hybridization is the mixing of atomic orbitals prior to their combining into molecular orbitals

Resonating structures possess different_______

electronic arrangements
atomic arrangements
functional groups
alkyl groups

Non-polar from the following compounds is:

\(H_{2}SO_{4}\)
\(Cl_{2}\)
NaCl
\(H_{2}S\)

_____molecule does not exist on the basis of molecular orbital theory.

\(Li_{2}\)
\(He_{2}\)
\(He^{+}_{2}\)
\(H^{+}_{2}\)

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