How does an increase in the percentage of s-character in a carbon atom's hybrid orbital affect the carbon's effective electronegativity and the length of the resulting $\text{C}-\text{H}$ bond?

A) It decreases the carbon's electronegativity and increases the $\text{C}-\text{H}$ bond length.

B) It increases the carbon's electronegativity and decreases the $\text{C}-\text{H}$ bond length.

C) It decreases the carbon's electronegativity and decreases the $\text{C}-\text{H}$ bond length.

D) It increases the carbon's electronegativity and increases the $\text{C}-\text{H}$ bond length.

In a propadiene ($\text{CH}_2=\text{C}=\text{CH}_2$) molecule, what is the hybridization of the central carbon atom and the relative geometric orientation of the two terminal $\text{CH}_2$ planes?

A) The central carbon atom is $sp^2$-hybridized, and the two terminal $\text{CH}_2$ planes are coplanar.

B) The central carbon atom is $sp$-hybridized, and the two terminal $\text{CH}_2$ planes are mutually perpendicular.

C) The central carbon atom is $sp$-hybridized, and the two terminal $\text{CH}_2$ planes are coplanar.

D) The central carbon atom is $sp^3$-hybridized, and the two terminal $\text{CH}_2$ planes are oriented at an angle of $109.5^\circ$.

Which statement correctly compares the carbon–carbon bonds in ethane ($\text{C}_2\text{H}_6$), ethene ($\text{C}_2\text{H}_4$), and ethyne ($\text{C}_2\text{H}_2$)?

A) Ethane exhibits the shortest carbon–carbon bond length and the highest bond dissociation energy because single $\sigma$ bonds provide the strongest axial orbital overlap.

B) Ethene has a shorter carbon–carbon bond length and higher bond dissociation energy than ethyne because $sp^2$ hybrid orbitals have a greater percentage of s-character than $sp$ hybrid orbitals.

C) Ethyne exhibits the shortest carbon–carbon bond length and the highest bond dissociation energy because of its higher bond order and the greater s-character of its $sp$ hybrid orbitals.

D) Ethane has a shorter carbon–carbon bond length than ethene because the absence of $\pi$ electron repulsion allows the two carbon nuclei to approach each other more closely.

Which statement correctly describes the orbital overlaps that form the bonds in an ethene ($\text{C}_2\text{H}_4$) molecule?

A) One $sp^2\text{--}sp^2$ $\sigma$ bond and one $p\text{--}p$ $\pi$ bond between the carbon atoms, and $sp^2\text{--}s$ $\sigma$ bonds between carbon and hydrogen atoms.

B) One $sp^3\text{--}sp^3$ $\sigma$ bond and one $p\text{--}p$ $\pi$ bond between the carbon atoms, and $sp^3\text{--}s$ $\sigma$ bonds between carbon and hydrogen atoms.

C) Two $sp^2\text{--}sp^2$ $\sigma$ bonds between the carbon atoms, and $p\text{--}s$ $\sigma$ bonds between carbon and hydrogen atoms.

D) One $sp\text{--}sp$ $\sigma$ bond and one $p\text{--}p$ $\pi$ bond between the carbon atoms, and $sp\text{--}s$ $\sigma$ bonds between carbon and hydrogen atoms.

Which option correctly gives the hybridization states of the carbon atoms from left to right and the total number of pi (π) bonds in a propyne molecule (CH₃–C≡CH)?

A) sp³, sp², sp and one π bond

B) sp³, sp, sp and two π bonds

C) sp², sp, sp and two π bonds

D) sp³, sp², sp² and one π bond

Bonding in carbon compounds Knowledge-Based Practice

Chemistry · Organic Chemistry · Chemistry · Hydrocarbons

5 Chemistry practice questions on Bonding in carbon compounds. Questions that assess core concepts and understanding.

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1.
How does an increase in the percentage of s-character in a carbon atom's hybrid orbital affect the carbon's effective electronegativity and the length of the resulting $\text{C}-\text{H}$ bond?
- A) It decreases the carbon's electronegativity and increases the $\text{C}-\text{H}$ bond length.
- B) It increases the carbon's electronegativity and decreases the $\text{C}-\text{H}$ bond length.
- C) It decreases the carbon's electronegativity and decreases the $\text{C}-\text{H}$ bond length.
- D) It increases the carbon's electronegativity and increases the $\text{C}-\text{H}$ bond length.
2.
In a propadiene ( $\text{CH}_2=\text{C}=\text{CH}_2$ ) molecule, what is the hybridization of the central carbon atom and the relative geometric orientation of the two terminal $\text{CH}_2$ planes?
- A) The central carbon atom is $sp^2$ -hybridized, and the two terminal $\text{CH}_2$ planes are coplanar.
- B) The central carbon atom is $sp$ -hybridized, and the two terminal $\text{CH}_2$ planes are mutually perpendicular.
- C) The central carbon atom is $sp$ -hybridized, and the two terminal $\text{CH}_2$ planes are coplanar.
- D) The central carbon atom is $sp^3$ -hybridized, and the two terminal $\text{CH}_2$ planes are oriented at an angle of $109.5^\circ$ .
3.
Which statement correctly compares the carbon–carbon bonds in ethane ( $\text{C}_2\text{H}_6$ ), ethene ( $\text{C}_2\text{H}_4$ ), and ethyne ( $\text{C}_2\text{H}_2$ )?
- A) Ethane exhibits the shortest carbon–carbon bond length and the highest bond dissociation energy because single $\sigma$ bonds provide the strongest axial orbital overlap.
- B) Ethene has a shorter carbon–carbon bond length and higher bond dissociation energy than ethyne because $sp^2$ hybrid orbitals have a greater percentage of s-character than $sp$ hybrid orbitals.
- C) Ethyne exhibits the shortest carbon–carbon bond length and the highest bond dissociation energy because of its higher bond order and the greater s-character of its $sp$ hybrid orbitals.
- D) Ethane has a shorter carbon–carbon bond length than ethene because the absence of $\pi$ electron repulsion allows the two carbon nuclei to approach each other more closely.
4.
Which statement correctly describes the orbital overlaps that form the bonds in an ethene ( $\text{C}_2\text{H}_4$ ) molecule?
- A) One $sp^2\text{--}sp^2$ $\sigma$ bond and one $p\text{--}p$ $\pi$ bond between the carbon atoms, and $sp^2\text{--}s$ $\sigma$ bonds between carbon and hydrogen atoms.
- B) One $sp^3\text{--}sp^3$ $\sigma$ bond and one $p\text{--}p$ $\pi$ bond between the carbon atoms, and $sp^3\text{--}s$ $\sigma$ bonds between carbon and hydrogen atoms.
- C) Two $sp^2\text{--}sp^2$ $\sigma$ bonds between the carbon atoms, and $p\text{--}s$ $\sigma$ bonds between carbon and hydrogen atoms.
- D) One $sp\text{--}sp$ $\sigma$ bond and one $p\text{--}p$ $\pi$ bond between the carbon atoms, and $sp\text{--}s$ $\sigma$ bonds between carbon and hydrogen atoms.
5.
Which option correctly gives the hybridization states of the carbon atoms from left to right and the total number of pi (π) bonds in a propyne molecule (CH₃–C≡CH)?
- A) sp³, sp², sp and one π bond
- B) sp³, sp, sp and two π bonds
- C) sp², sp, sp and two π bonds
- D) sp³, sp², sp² and one π bond

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Organic Chemistry · Chemistry

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