Grade 11 : Chemistry - Chemical Bonding (Set 3)

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Grade 11 : Chemistry - Chemical Bonding (Set 3)— Questions & Detailed Solutions

Structure of Ozone ($O_3$): Central Oxygen atom ($O_B$) forms a double bond with one terminal oxygen ($O_A$) and a single coordinate bond with the other terminal oxygen ($O_C$).
What is the formal charge on the central oxygen atom ($O_B$) in the ozone ($O_3$) molecule?

(A)

(B)

(C)

-1

(D)

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✓ Correct Option: (B)

Explanation: Formal charge is calculated as $FC = V - N - \frac{B}{2}$, where $V = 6$ (valence electrons), $N = 2$ (non-bonding electrons), and $B = 6$ (bonding electrons from 3 bonds). $FC = 6 - 2 - \frac{6}{2} = +1$.

According to VSEPR theory, what is the molecular geometry of sulfur tetrafluoride ($SF_4$)?

(A)

Tetrahedral

(B)

Square planar

(C)

See-saw

(D)

Trigonal bipyramidal

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✓ Correct Option: (C)

Explanation: Sulfur has 6 valence electrons. In $SF_4$, it forms 4 single bonds with fluorine and has 1 lone pair (steric number = 5). The electron geometry is trigonal bipyramidal, but due to 1 equatorial lone pair, the molecular shape is See-saw.

Compound Cation Radii (pm) Cation Charge
LiCl 76 +1
NaCl 102 +1
KCl 138 +1
RbCl 152 +1
Based on Fajan's rules and the data above, which alkali metal chloride possesses the highest covalent character?

Compound	Cation Radii (pm)	Cation Charge
LiCl	76	+1
NaCl	102	+1
KCl	138	+1
RbCl	152	+1

(A)

RbCl

(B)

KCl

(C)

NaCl

(D)

LiCl

View Correct Answer & Detailed Solution

✓ Correct Option: (D)

Explanation: According to Fajan's rules, smaller cation size leads to higher polarizing power and higher covalent character. Since $Li^+$ has the smallest ionic radius (76 pm), LiCl exhibits the maximum covalent character.

What is the hybridization of the central atom and the shape of the xenon tetrafluoride ($XeF_4$) molecule?

(A)

$sp^3d$, Trigonal bipyramidal

(B)

$sp^3d^2$, Square planar

(C)

$sp^3d^2$, Octahedral

(D)

$sp^3$, Tetrahedral

View Correct Answer & Detailed Solution

✓ Correct Option: (B)

Explanation: Xenon has 8 valence electrons. In $XeF_4$, 4 electrons form bonds with fluorine and 4 remain as 2 lone pairs. Steric number = $4 + 2 = 6$, giving $sp^3d^2$ hybridization. The 2 lone pairs occupy axial positions to minimize repulsion, resulting in a Square planar geometry.

Using Molecular Orbital Theory, determine the bond order of the dioxygen cation ($O_2^+$).

(A)

1.5

(B)

2.0

(C)

2.5

(D)

3.0

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✓ Correct Option: (C)

Explanation: $O_2^+$ has 15 electrons. Bonding electrons $N_b = 10$, Antibonding electrons $N_a = 5$. Bond order = $\frac{N_b - N_a}{2} = \frac{10 - 5}{2} = 2.5$.

Statement I: Ammonia ($NH_3$) has a net dipole moment of 1.47 D.
Statement II: Nitrogen trifluoride ($NF_3$) has a net dipole moment of 0.23 D.
Which statement correctly explains why the dipole moment of $NH_3$ is significantly greater than that of $NF_3$?

(A)

In $NH_3$, the lone pair dipole opposes the N-H bond dipoles.

(B)

In $NF_3$, the lone pair dipole opposes the resultant vector of N-F bond dipoles.

(C)

Nitrogen is more electronegative than fluorine.

(D)

$NF_3$ has a planar structure while $NH_3$ is pyramidal.

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✓ Correct Option: (B)

Explanation: In $NH_3$, N is more electronegative than H, so N-H bond dipoles point toward N in the same direction as the lone pair dipole. In $NF_3$, F is more electronegative than N, so N-F dipoles point away from N, opposing the lone pair dipole.

Consider the molecule vinylacetylene: $HC \equiv C - CH = CH_2$.
Calculate the total number of sigma ($\sigma$) and pi ($\pi$) bonds present in one molecule of vinylacetylene.

(A)

$6\sigma, 3\pi$

(B)

$7\sigma, 3\pi$

(C)

$7\sigma, 2\pi$

(D)

$8\sigma, 3\pi$

View Correct Answer & Detailed Solution

✓ Correct Option: (B)

Explanation: Single bonds contain $1\sigma$; double bonds contain $1\sigma + 1\pi$; triple bonds contain $1\sigma + 2\pi$. Counting: 4 C-H $\sigma$ bonds + 3 C-C $\sigma$ bonds = $7\sigma$ bonds. $\pi$ bonds: 2 from $C\equiv C$ + 1 from $C=C$ = $3\pi$ bonds.

Ionic Compound	Cation Charge	Anion Charge
NaCl	+1	-1
NaF	+1	-1
MgO	+2	-2
AlN	+3	-3

(A)

NaCl

(B)

MgO

(C)

AlN

(D)

NaF

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✓ Correct Option: (C)

Explanation: Lattice energy is proportional to $|z_+ z_-|$. AlN has charges of +3 and -3, giving a charge product of 9, which is larger than MgO (4) or NaCl (1). Thus, AlN has the highest lattice energy.

Q14

Approaching orbitals along the x-axis: A spherical $s$ orbital approaches a dumbbell $p_y$ orbital oriented perpendicular to the x-axis.
Which pair of atomic orbitals results in ZERO net overlap (non-bonding) when approaching along the x-axis?

(A)

$s$ and $p_x$

(B)

$p_y$ and $p_y$

(C)

$s$ and $p_y$

(D)

$p_x$ and $p_x$

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✓ Correct Option: (C)

Explanation: An $s$ orbital approaching a $p_y$ orbital along the x-axis overlaps equally with the positive and negative lobes of $p_y$. The positive and negative overlap regions cancel out, yielding zero net overlap.

Q15

Which pair among the following consists of ISOSTRUCTURAL species (same molecular geometry)?

(A)

$CO_2$ and $SO_2$

(B)

$NH_3$ and $H_3O^+$

(C)

$ClF_3$ and $BF_3$

(D)

$XeF_4$ and $SF_4$

View Correct Answer & Detailed Solution

✓ Correct Option: (B)

Explanation: Both $NH_3$ and $H_3O^+$ have 3 bond pairs and 1 lone pair on the central atom (steric number = 4, $sp^3$ hybridization), giving both species a trigonal pyramidal geometry.

Q16

Comparing $N_2^+$ and $N_2^-$, which species is MORE stable and why?

(A)

$N_2^-$ because it has more total electrons.

(B)

$N_2^+$ because it has fewer electrons in antibonding orbitals.

(C)

Both have identical stability because both have a bond order of 2.5.

(D)

$N_2^-$ because it has a higher bond order.

View Correct Answer & Detailed Solution

✓ Correct Option: (B)

Explanation: Both $N_2^+$ and $N_2^-$ have a bond order of 2.5. However, $N_2^-$ has 3 electrons in antibonding MOs (specifically $\pi^* 2p$), whereas $N_2^+$ has only 2 antibonding electrons. Antibonding electrons exert a net destabilizing effect, making $N_2^+$ more stable.

Q17

The experimental dipole moment of HCl is 1.03 D. The internuclear distance between $H$ and Cl is 1.275 \AA ($1\text{ D} = 3.336 \times 10^{-30}\text{ C m}$, $e = 1.602 \times 10^{-19}\text{ C}$).
What is the percentage ionic character of the $H-Cl$ bond?

(A)

16.8%

(B)

33.5%

(C)

50.0%

(D)

83.2%

View Correct Answer & Detailed Solution

✓ Correct Option: (A)

Explanation: $\mu_{\text{ionic}} = q \times d = (1.602 \times 10^{-19}) \times (1.275 \times 10^{-10}) = 2.0425 \times 10^{-29}\text{ C m} = 6.12\text{ D}$. Percentage ionic character = $\frac{\mu_{\text{exp}}}{\mu_{\text{ionic}}} \times 100 = \frac{1.03}{6.12} \times 100 \approx 16.8%$.

Q18

What is the molecular shape and the number of lone pairs on the central Xe atom in xenon difluoride ($XeF_2$)?

(A)

Bent, 2 lone pairs

(B)

Linear, 3 lone pairs

(C)

Linear, 2 lone pairs

(D)

Trigonal planar, 3 lone pairs

View Correct Answer & Detailed Solution

✓ Correct Option: (B)

Explanation: Central Xe has 8 valence electrons. In $XeF_2$, 2 electrons form bonds with fluorine, leaving 6 non-bonding electrons (3 lone pairs). Steric number = $2 + 3 = 5$ ($sp^3d$). The 3 lone pairs occupy equatorial positions, resulting in a Linear molecular shape.

Q19

Structure of propadiene (allene): $H_2C^{(1)} = C^{(2)} = C^{(3)}H_2$.
What are the hybridization states of carbon atoms 1, 2, and 3 from left to right in propadiene?

(A)

$sp^2, sp^2, sp^2$

(B)

$sp^3, sp, sp^3$

(C)

$sp^2, sp, sp^2$

(D)

$sp, sp^2, sp$

View Correct Answer & Detailed Solution

✓ Correct Option: (C)

Explanation: $C^{(1)}$ forms 3 $\sigma$ bonds ($sp^2$). Central $C^{(2)}$ forms 2 $\sigma$ bonds (sp). $C^{(3)}$ forms 3 $\sigma$ bonds ($sp^2$). Thus, the hybridization states are $sp^2, sp, sp^2$.

Q20

Molecule Hybridization Lone Pairs Bond Angle
$CH_4$ $sp^3$ 0 $109.5^\circ$
$NH_3$ $sp^3$ 1 $107.0^\circ$
$H_2O$ $sp^3$ 2 $104.5^\circ$
Based on VSEPR theory and the table above, why does $H_2O$ have a smaller bond angle than $NH_3$?

Molecule	Hybridization	Lone Pairs	Bond Angle
$CH_4$	$sp^3$	0	$109.5^\circ$
$NH_3$	$sp^3$	1	$107.0^\circ$
$H_2O$	$sp^3$	2	$104.5^\circ$

(A)

$H_2O$ experiences lone pair-lone pair repulsion which is stronger than lone pair-bond pair repulsion in $NH_3$.

(B)

Oxygen is less electronegative than nitrogen.

(C)

$NH_3$ has more lone pairs than $H_2O$.

(D)

$H_2O$ is non-polar whereas $NH_3$ is polar.

View Correct Answer & Detailed Solution

✓ Correct Option: (A)

Explanation: Repulsion strength follows the order: lone pair-lone pair (lp-lp) > lone pair-bond pair (lp-bp) > bond pair-bond pair (bp-bp). $H_2O$ has 2 lone pairs leading to strong lp-lp repulsion, compressing the H-O-H bond angle to $104.5^\circ$ compared to $107^\circ$ in $NH_3$.

Grade 11 : Chemistry - Chemical Bonding (Set 3)

Grade 11 : Chemistry - Chemical Bonding (Set 3)— Questions & Detailed Solutions

Structure of Ozone ($O_3$): Central Oxygen atom ($O_B$) forms a double bond with one terminal oxygen ($O_A$) and a single coordinate bond with the other terminal oxygen ($O_C$).
What is the formal charge on the central oxygen atom ($O_B$) in the ozone ($O_3$) molecule?

According to VSEPR theory, what is the molecular geometry of sulfur tetrafluoride ($SF_4$)?

Compound Cation Radii (pm) Cation Charge
LiCl 76 +1
NaCl 102 +1
KCl 138 +1
RbCl 152 +1
Based on Fajan's rules and the data above, which alkali metal chloride possesses the highest covalent character?

What is the hybridization of the central atom and the shape of the xenon tetrafluoride ($XeF_4$) molecule?

Using Molecular Orbital Theory, determine the bond order of the dioxygen cation ($O_2^+$).

Statement I: Ammonia ($NH_3$) has a net dipole moment of 1.47 D.
Statement II: Nitrogen trifluoride ($NF_3$) has a net dipole moment of 0.23 D.
Which statement correctly explains why the dipole moment of $NH_3$ is significantly greater than that of $NF_3$?

Consider the molecule vinylacetylene: $HC \equiv C - CH = CH_2$.
Calculate the total number of sigma ($\sigma$) and pi ($\pi$) bonds present in one molecule of vinylacetylene.

Which of the following compounds exhibits intramolecular hydrogen bonding, making it steam-volatile with a lower boiling point?

Which of the following choices correctly represents the decreasing order of H-M-H bond angle among Group 15 hydrides?

According to Molecular Orbital Theory, which of the following homonuclear diatomic molecules contains TWO unpaired electrons in its ground state?

What is the formal C-O bond order in the carbonate ion ($CO_3^{2-}$)?

In solid state, phosphorus pentachloride exists as $[PCl_4]^+[PCl_6]^-$. What is the hybridization of the phosphorus atom in the cationic species $[PCl_4]^+$?

Ionic Compound Cation Charge Anion Charge
NaCl +1 -1
NaF +1 -1
MgO +2 -2
AlN +3 -3
Based on charge product and ion size principles, which compound possesses the HIGHEST lattice energy?

Approaching orbitals along the x-axis: A spherical $s$ orbital approaches a dumbbell $p_y$ orbital oriented perpendicular to the x-axis.
Which pair of atomic orbitals results in ZERO net overlap (non-bonding) when approaching along the x-axis?

Which pair among the following consists of ISOSTRUCTURAL species (same molecular geometry)?

Comparing $N_2^+$ and $N_2^-$, which species is MORE stable and why?

The experimental dipole moment of HCl is 1.03 D. The internuclear distance between $H$ and Cl is 1.275 \AA ($1\text{ D} = 3.336 \times 10^{-30}\text{ C m}$, $e = 1.602 \times 10^{-19}\text{ C}$).
What is the percentage ionic character of the $H-Cl$ bond?

What is the molecular shape and the number of lone pairs on the central Xe atom in xenon difluoride ($XeF_2$)?

Structure of propadiene (allene): $H_2C^{(1)} = C^{(2)} = C^{(3)}H_2$.
What are the hybridization states of carbon atoms 1, 2, and 3 from left to right in propadiene?

Molecule Hybridization Lone Pairs Bond Angle
$CH_4$ $sp^3$ 0 $109.5^\circ$
$NH_3$ $sp^3$ 1 $107.0^\circ$
$H_2O$ $sp^3$ 2 $104.5^\circ$
Based on VSEPR theory and the table above, why does $H_2O$ have a smaller bond angle than $NH_3$?

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Grade 11 : Chemistry - Chemical Bonding (Set 3)

Grade 11 : Chemistry - Chemical Bonding (Set 3)— Questions & Detailed Solutions

Structure of Ozone ($O_3$): Central Oxygen atom ($O_B$) forms a double bond with one terminal oxygen ($O_A$) and a single coordinate bond with the other terminal oxygen ($O_C$).What is the formal charge on the central oxygen atom ($O_B$) in the ozone ($O_3$) molecule?

According to VSEPR theory, what is the molecular geometry of sulfur tetrafluoride ($SF_4$)?

CompoundCation Radii (pm)Cation ChargeLiCl76+1NaCl102+1KCl138+1RbCl152+1Based on Fajan's rules and the data above, which alkali metal chloride possesses the highest covalent character?

What is the hybridization of the central atom and the shape of the xenon tetrafluoride ($XeF_4$) molecule?

Using Molecular Orbital Theory, determine the bond order of the dioxygen cation ($O_2^+$).

Statement I: Ammonia ($NH_3$) has a net dipole moment of 1.47 D.Statement II: Nitrogen trifluoride ($NF_3$) has a net dipole moment of 0.23 D.Which statement correctly explains why the dipole moment of $NH_3$ is significantly greater than that of $NF_3$?

Consider the molecule vinylacetylene: $HC \equiv C - CH = CH_2$.Calculate the total number of sigma ($\sigma$) and pi ($\pi$) bonds present in one molecule of vinylacetylene.

Which of the following compounds exhibits intramolecular hydrogen bonding, making it steam-volatile with a lower boiling point?

Which of the following choices correctly represents the decreasing order of H-M-H bond angle among Group 15 hydrides?

According to Molecular Orbital Theory, which of the following homonuclear diatomic molecules contains TWO unpaired electrons in its ground state?

What is the formal C-O bond order in the carbonate ion ($CO_3^{2-}$)?

In solid state, phosphorus pentachloride exists as $[PCl_4]^+[PCl_6]^-$. What is the hybridization of the phosphorus atom in the cationic species $[PCl_4]^+$?

Ionic CompoundCation ChargeAnion ChargeNaCl+1-1NaF+1-1MgO+2-2AlN+3-3Based on charge product and ion size principles, which compound possesses the HIGHEST lattice energy?

Approaching orbitals along the x-axis: A spherical $s$ orbital approaches a dumbbell $p_y$ orbital oriented perpendicular to the x-axis.Which pair of atomic orbitals results in ZERO net overlap (non-bonding) when approaching along the x-axis?

Which pair among the following consists of ISOSTRUCTURAL species (same molecular geometry)?

Comparing $N_2^+$ and $N_2^-$, which species is MORE stable and why?

The experimental dipole moment of HCl is 1.03 D. The internuclear distance between $H$ and Cl is 1.275 \AA ($1\text{ D} = 3.336 \times 10^{-30}\text{ C m}$, $e = 1.602 \times 10^{-19}\text{ C}$).What is the percentage ionic character of the $H-Cl$ bond?

What is the molecular shape and the number of lone pairs on the central Xe atom in xenon difluoride ($XeF_2$)?

Structure of propadiene (allene): $H_2C^{(1)} = C^{(2)} = C^{(3)}H_2$.What are the hybridization states of carbon atoms 1, 2, and 3 from left to right in propadiene?

MoleculeHybridizationLone PairsBond Angle$CH_4$$sp^3$0$109.5^\circ$$NH_3$$sp^3$1$107.0^\circ$$H_2O$$sp^3$2$104.5^\circ$Based on VSEPR theory and the table above, why does $H_2O$ have a smaller bond angle than $NH_3$?

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Structure of Ozone ($O_3$): Central Oxygen atom ($O_B$) forms a double bond with one terminal oxygen ($O_A$) and a single coordinate bond with the other terminal oxygen ($O_C$).
What is the formal charge on the central oxygen atom ($O_B$) in the ozone ($O_3$) molecule?

Compound Cation Radii (pm) Cation Charge
LiCl 76 +1
NaCl 102 +1
KCl 138 +1
RbCl 152 +1
Based on Fajan's rules and the data above, which alkali metal chloride possesses the highest covalent character?

Statement I: Ammonia ($NH_3$) has a net dipole moment of 1.47 D.
Statement II: Nitrogen trifluoride ($NF_3$) has a net dipole moment of 0.23 D.
Which statement correctly explains why the dipole moment of $NH_3$ is significantly greater than that of $NF_3$?

Consider the molecule vinylacetylene: $HC \equiv C - CH = CH_2$.
Calculate the total number of sigma ($\sigma$) and pi ($\pi$) bonds present in one molecule of vinylacetylene.

Ionic Compound Cation Charge Anion Charge
NaCl +1 -1
NaF +1 -1
MgO +2 -2
AlN +3 -3
Based on charge product and ion size principles, which compound possesses the HIGHEST lattice energy?

Approaching orbitals along the x-axis: A spherical $s$ orbital approaches a dumbbell $p_y$ orbital oriented perpendicular to the x-axis.
Which pair of atomic orbitals results in ZERO net overlap (non-bonding) when approaching along the x-axis?

The experimental dipole moment of HCl is 1.03 D. The internuclear distance between $H$ and Cl is 1.275 \AA ($1\text{ D} = 3.336 \times 10^{-30}\text{ C m}$, $e = 1.602 \times 10^{-19}\text{ C}$).
What is the percentage ionic character of the $H-Cl$ bond?

Structure of propadiene (allene): $H_2C^{(1)} = C^{(2)} = C^{(3)}H_2$.
What are the hybridization states of carbon atoms 1, 2, and 3 from left to right in propadiene?

Molecule Hybridization Lone Pairs Bond Angle
$CH_4$ $sp^3$ 0 $109.5^\circ$
$NH_3$ $sp^3$ 1 $107.0^\circ$
$H_2O$ $sp^3$ 2 $104.5^\circ$
Based on VSEPR theory and the table above, why does $H_2O$ have a smaller bond angle than $NH_3$?