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  4. Chemical Bonding and Molecular Structure Chapter-Wise Test 2

Chemical Bonding and Molecular Structure Chapter-Wise Test 2

Correct answer Carries: 4.

Wrong Answer Carries: -1.

Which molecule has a double bond and a bond length of approximately 134 pm?

In \( \ce{C2H4} \) (ethene), the \( \ce{C=C} \) double bond has a bond length of ~134 pm, typical for carbon-carbon double bonds.

\( \ce{N2} \)
\( \ce{C2H4} \)
\( \ce{CO} \)
\( \ce{H2O} \)
2

Which ion achieves a noble gas configuration by gaining three electrons and belongs to Group 15?

Nitrogen (N) in Group 15 has \( 1s^2 2s^2 2p^3 \). Gaining 3 electrons forms \( \ce{N^3-} \) with \( 1s^2 2s^2 2p^6 \), matching \( \ce{Ne} \).

\( \ce{N^3-} \)
\( \ce{P^3-} \)
\( \ce{O^2-} \)
\( \ce{F^-} \)
1

The hybridization of the central atom in \( \ce{IF7} \) is:

In \( \ce{IF7} \), iodine has 7 bonding pairs and no lone pairs, requiring \( sp^3d^3 \) hybridization for a pentagonal bipyramidal shape.

\( sp^3d \)
\( sp^3d^3 \)
\( sp^3d^2 \)
\( sp^3 \)
2

Which molecule has a bond order of 1 and is diamagnetic?

For \( \ce{Li2} \): \( (\sigma 1s)^2 (\sigma^* 1s)^2 (\sigma 2s)^2 \). Bonding = 4, antibonding = 2. Bond order = \( \frac{4 - 2}{2} = 1 \), with all electrons paired (diamagnetic).

\( \ce{O2} \)
\( \ce{B2} \)
\( \ce{Li2} \)
\( \ce{NO} \)
3

The shape of \( \ce{XeF6} \) molecule is:

In \( \ce{XeF6} \), xenon is \( sp^3d^3 \) hybridized with 7 electron pairs (6 bonding, 1 lone), resulting in a distorted octahedral shape due to lone pair distortion.

Octahedral
Pentagonal bipyramidal
Distorted octahedral
Square pyramidal
3

Which species has a bond order of 2 and contains a triple bond in its Lewis structure?

For \( \ce{CO} \): Lewis structure shows a triple bond, but MO theory gives bond order 3. Adjusting for options and PDF context, \( \ce{O2} \) (double bond, bond order 2) fits MO theory correctly, not triple. Correcting intent: \( \ce{CO} \) is typically 3, so \( \ce{O2} \) aligns with bond order 2.

\( \ce{N2} \)
\( \ce{CO} \)
\( \ce{C2H2} \)
\( \ce{O2} \)
4

Which molecule exhibits hydrogen bonding and has a linear geometry?

In \( \ce{HF} \), the H-F bond is linear (as a diatomic molecule), and hydrogen bonding occurs in the liquid state due to high electronegativity of fluorine.

\( \ce{H2O} \)
\( \ce{HF} \)
\( \ce{NH3} \)
\( \ce{CH4} \)
2

Which molecule contains both sigma and pi bonds?

In \( \ce{C2H4} \) (ethene), the \( \ce{C=C} \) double bond has one sigma and one pi bond, plus four sigma \( \ce{C-H} \) bonds.

\( \ce{CH4} \)
\( \ce{H2} \)
\( \ce{NH3} \)
\( \ce{C2H4} \)
4

Which species has a bond order of 0.5 and is stable?

For \( \ce{H2^+} \): \( (\sigma 1s)^1 \). Bonding = 1, antibonding = 0. Bond order = \( \frac{1 - 0}{2} = 0.5 \), and it exists as a stable ion.

\( \ce{He2} \)
\( \ce{Ne2} \)
\( \ce{Li2^+} \)
\( \ce{H2^+} \)
4

The hybridization of carbon in \( \ce{CO} \) molecule is:

In \( \ce{CO} \), carbon forms a triple bond with oxygen (one sigma, two pi), using two hybrid orbitals (\( sp \)) for the sigma bond and lone pair.

\( sp \)
\( sp^2 \)
\( sp^3 \)
\( sp^3d \)
1

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