ECAT Pre Engineering Chemistry Chapter 6 MCQ Test With Answer

The shape of methanol, ammonia and water molecule can be explained by assuming

• Sp³ hybridization A
• Sp²hybridization B
• Sp hybridization C
• All of these D

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

• 109.5° A
• 107.5° B
• 104.5° C
• None D

Which for the following has no dipole moment

• HCI A
• H₂S B
• H₂O C
• CO₂ D

Three sp²hybrid are co-planar at an angle of

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

The bond angle depends upon the

• Types of bonds A
• Number of bonds B
• Non-bonding electron pairs C
• All of the above D

The formation of compounds like PF₅, BCI₃, SF₆indicates that

• These halides are ionic A
• These halides are covalent B
• They are Lewis acids C
• Octet rule not obeyed so the rule is not universal 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

In which of the following theories the hybridizationis considered

• Vsepr A
• Lewis B
• Molecule orbital C
• Valence bond D

The covalent bonds are

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

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

XeF₄has shape of

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

Mg becomes isoelectronic with neon when it

• Loses two electrons A
• Gains two electrons B
• Loses 1 electron C
• Gains 1 electron D

On the basis of VSEPR theory SO₂is a

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

Which of the following hydrides has the lowest boiling point?

• H₂O A
• H₂S B
• H₂S3 C
• H₂Te 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

In H₂O molecule the bond angle is

• 90° A
• 109.5° B
• 107° C
• 104.5° D

H-bonding is not present in

• Glycerine A
• Water B
• Hydrogen sulphide C
• Hydrogen fluride 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 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

A bond between two atoms may be obtained by sharing of electrons such a bond is called

• An ionic bond A
• A coordinate bond B
• A dative bond C
• A covalent bond D

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

• He A
• Ne B
• Kr C
• Xe D

When of the following is isolelectronic with krypton

• Ca⁺⁺ A
• Al⁺⁺⁺ B
• Br^-1 C
• I^-1 D

The electron affinity of chlorine may be represented by the equation

• 
  A
• 
  B
• 
  C
• 
  D

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

• Planar A
• Pyramidal B
• Angular C
• Trigonal bipyramidal D

The bond angle H - O - H in ice ins closest to

• 120° , 28^' A
• 60° B
• 90° C
• 109° D

The equation for the first ionization energy of hydrogen is

• 
  A
• 
  B
• 
  C
• 
  D

Ionization energies increase from left to right along the period due to

• Increase in nuclear charge A
• Repulsion of electron increases B
• Repulsion of protons increase C
• Atomic size increase along the period D