Chemical Bonding and Molecular Structure Chapter-Wise Test 2

Correct answer Carries: 4.

Wrong Answer Carries: -1.

The strongest type of bond in terms of bond dissociation energy is:

A triple bond, as in \( \ce{N2} \) (bond enthalpy ~946 kJ/mol), is the strongest due to three shared electron pairs.

Triple bond
Double bond
Single bond
Hydrogen bond
1

Which of the following has a triple bond?

In \( \ce{C2H2} \) (ethyne), the carbon atoms share three electron pairs, forming a triple bond (1 sigma + 2 pi).

\( \ce{C2H4} \)
\( \ce{CH4} \)
\( \ce{C2H2} \)
\( \ce{H2O} \)
3

Which molecule violates the octet rule by having more than 8 electrons around the central atom and involves d-orbital hybridization?

In \( \ce{SF6} \), sulfur has 6 bonds (12 electrons) with \( sp^3d^2 \) hybridization, exceeding the octet using d-orbitals.

\( \ce{SF6} \)
\( \ce{BF3} \)
\( \ce{NH3} \)
\( \ce{CH4} \)
1

The bond order of \( \ce{H2} \) molecule according to molecular orbital theory is:

For \( \ce{H2} \), electronic configuration is \( (\sigma 1s)^2 \). Bond order = \( \frac{2 - 0}{2} = 1 \).

1
2
3
0
1

Which molecule has the shortest bond length among those with a double bond?

Among molecules with a double bond, \(\ce{O2}\) has a bond length of ~121 pm, shorter than \(\ce{C2H4}\) (~134 pm), \(\ce{SO2}\) (~143 pm), or \(\ce{NO2}\) (~124 pm), due to higher bond strength and smaller atomic radii.

\(\ce{C2H4}\)
\(\ce{SO2}\)
\(\ce{NO2}\)
\(\ce{O2}\)
4

Which molecule contains a single bond with a bond length of approximately 154 pm?

In \( \ce{C2H6} \) (ethane), the \( \ce{C-C} \) single bond has a bond length of ~154 pm, typical for carbon-carbon single bonds.

\( \ce{N2} \)
\( \ce{C2H6} \)
\( \ce{CO} \)
\( \ce{HF} \)
2

The shape of \( \ce{XeF4} \) molecule is:

In \( \ce{XeF4} \), xenon is \( sp^3d^2 \) hybridized with 6 electron pairs (4 bonding, 2 lone), resulting in a square planar shape.

Tetrahedral
Octahedral
Trigonal bipyramidal
Square planar
4

Which molecule has a square planar shape?

In \( \ce{XeF4} \), xenon is \( sp^3d^2 \) hybridized with 6 electron pairs (4 bonding, 2 lone), resulting in a square planar molecular shape.

\( \ce{SF6} \)
\( \ce{PF5} \)
\( \ce{XeF4} \)
\( \ce{ClF3} \)
3

Which molecule exhibits \( sp^3 \) hybridization at its central atom?

In \( \ce{CH4} \), carbon uses one s and three p orbitals to form four \( sp^3 \) hybrid orbitals, resulting in a tetrahedral shape.

\( \ce{CH4} \)
\( \ce{C2H4} \)
\( \ce{BeCl2} \)
\( \ce{BCl3} \)
1

Which molecule has a trigonal planar electron pair geometry but a bent molecular shape?

In \( \ce{SO2} \), sulfur has 3 electron domains (2 bonding, 1 lone pair), giving a trigonal planar electron geometry (\( sp^2 \)), but a bent molecular shape.

\( \ce{SO2} \)
\( \ce{BF3} \)
\( \ce{CH4} \)
\( \ce{NH3} \)
1

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