ECAT Pre Engineering Chemistry Chapter 6 MCQ Test With Answer

The bond order of individual C - C bond is benzene is

• One A
• Two B
• Between one and two C
• One and two alternately 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

In H₂O molecule the bond angle is

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

Ionic radius, in a period from left to right

• Increases A
• Decreases B
• Decreases then increases C
• Increases and decreases D

Which of the following has unchanged valency?

• H A
• Na B
• Fe C
• Oxygen D

The nature of interparticle forces in benzene is

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

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

• Be A
• Mg B
• Sr C
• calcium 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

The number of bonds in nitrogen molecule is

• 
  A
• 
  B
• 
  C
• 
  D

During the formation of a chemical bond the potential energy of the system

• Decreases A
• Increases B
• Does not change C
• None of these 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

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

• 
  A
• 
  B
• 
  C
• 
  D

Atomic number of Al is 13. When it forms ionic bond with oxygen the number of electrons lost by 1 Al atom is

• 1 A
• 2 B
• 3 C
• 4 D

The structure of ICI₂is

• Trigonal A
• Trigonal bipyramidal B
• Octahedral C
• Square planar D

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

• 
  A
• 
  B
• 
  C
• 
  D

When of the following is isolelectronic with krypton

• Ca⁺⁺ A
• Al⁺⁺⁺ B
• Br^-1 C
• I^-1 D

Which of the following molecules have sp³hybridized carbon

• CH₄ A
• C₂H₄ B
• C₂H₂ C
• CO₂ D

On the basis of VSEPR theory SO₂is a

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

Which of the following has zero depole-moment?

• CIF A
• PCl₃ B
• SiF₄ C
• CFCl₄ D

The force which holds the atoms together to form a compound is called

• A chemical bond A
• Van der waal's force B
• Dispersion force C
• London force 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

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

Which of the following charge

• Li A
• Be B
• H C
• He D

Which of the following molecules have multiple bonds

• CH₄ A
• C₂H₄ B
• C₂H₆ C
• CCI₄ D

Tripple bond is present in

• O₂ A
• H₂ B
• N₂ C
• Cl₂ D

The boiling point of heavy water is

• 108°C A
• 101.4°C B
• 99°C C
• 110°C D

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

• Water has higher molecular weight A
• Hydrogen sulphide is a weak acid B
• Sulphure has high electronegativity than oxyhe C
• Water molecules associate through hydrogen bonding D

The degree of polarity of molecule is known as its

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

Molecular orbital picture of N₂ indicates

• One unpaired electron A
• Two unpaired electron B
• No unpaired electron C
• None of these D