ECAT Pre Engineering Chemistry Chapter 6 MCQ Test With Answer

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

• 4 A
• 3 B
• 2 C
• 5 D

The degree of polarity of molecule is known as its

• Dipole moment A
• Moment arm B
• Bond energy C
• Ionic character D

Ca, Mg, Be, Ba, belong to the same group, the order of their ionization energy values is

• Be > Mg> Ca > Ba A
• Ba > Ca > Mg > Be B
• Ca > Mg > Be > Ba C
• Ba > Mg > Ca > Be D

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

• HF A
• HCL B
• HBr C
• HI D

XeF₄has shape of

• Sphere A
• Trigonal bipyramidal B
• Tetrahedral C
• Square planar D

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

• Addition of new shell A
• Repulsion of electrons in the valence shell B
• Decrease in nuclear charge C
• Increase in the unclear charge D

Three sp²hybrid are co-planar at an angle of

• 104.5° A
• 109.5° B
• 107° C
• 120° D

Tripple bond is present in

• O₂ A
• H₂ B
• N₂ C
• Cl₂ D

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

• He₂ A
• SO₂ B
• PCl₅ C
• N₂ D

The number of bonds in nitrogen molecule is

• 
  A
• 
  B
• 
  C
• 
  D

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

• Increase in potential energy A
• Decrease in potential energy B
• Energy remains unchanged C
• Distance is increased D

When elements of group I react with the elements of group VIA theory form

• Ionic bond A
• Covalent bond B
• Polar bond C
• None D

The nature of interparticle forces in benzene is

• Dipole-dipole interaction A
• Dispersion force B
• Ion-dipole interaction C
• H-bonding D

On the basis of VSEPR theory SO₂is a

• Liner molecule A
• A bent molecule B
• A strong molecule C
• A gaseous molecule D

Elements have the tendency to attain 8 electrons in their valence shell. This is known as

• Octer rule A
• Hunds rule B
• Pauli exclusion principle C
• Auf ban principle D

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

• Ionization potential of elements A
• Electron affinity of elements B
• Electronegativity of elements C
• Bond length D

Which of the following molecules have its central atom sp²hybridized

• CH₄ A
• C₂H₂ B
• C₂H₄ C
• CCl₄ D

The covalent bonds are

• Unidirectional A
• Bi-directional B
• Non-directional C
• Multi-directional D

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

• 2,6 A
• 2,8 B
• 2,10 C
• 2,9 D

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

• Planar triangle A
• Pyramidal B
• Tetrahedral C
• Square planar D

The bond order in No is 2.5 while that in NO⁺is 3.Which of the following statements is true for these two species?

• Bond length in NO⁺is greater than in NO A
• Bond length in unpredictable B
• Bond length in NO⁺is equal to that in NO C
• Bond length in NO is greater than in NO⁺ D

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

• Sigma bond A
• Pi bond B
• Ionic bond C
• Non-polar bond D

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

• O₂ A
• N₂ B
• Br₂ C
• F₂ D

Which of the following species has unpaired electrons in antibonding molecular orbitals

• 
  A
• 
  B
• 
  C
• 
  D

Which carbon is more electronegative?

• sp³- hybridized carbon A
• sp-hybridized carbon B
• sp²-hybridized carbon C
• always same irrespective of its hybrid state D

Antibonding MO is formed by

• Addition of atomic orbitals A
• Substraction of atomic orbitals B
• Multiplication of atomic orbitals C
• None of these D

• The ionization energy of A is high and electron affinity of B is low A
• The ionization energy of A is low and electron affinity of B is high B
• Both the ionization energy of A and electron off affinity of B are high C
• Both the ionization energy of A and electron affinity of B are low D

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

• Covalent bond between two non-metal atoms A
• Covalent bond between metal and non-metal B
• Covalent bond between two atoms of same element C
• Covalent bond between metal atoms D

Electronegativity values of the elements F, CI and Br vary

• F > CI > Br A
• Br > CI > F B
• Cl > Br > F C
• CI > F > Br D

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

• Covelent bond A
• Electronegativity B
• Ionization potential C
• Electronic affinity D