Grade 11 : Chemistry - Chemical Bonding (Set 2)

Back to Quizzes

Complete Syllabus Question Paper

Grade 11 : Chemistry - Chemical Bonding (Set 2)— Questions & Detailed Solutions

A sodium atom (Na) transfers its single valence electron to a chlorine atom (Cl) to form a stable crystal lattice of sodium chloride (NaCl).
Which type of chemical bond is formed during this process?

(A)

Ionic bond

(B)

Polar covalent bond

(C)

Nonpolar covalent bond

(D)

Metallic bond

View Correct Answer & Detailed Solution

✓ Correct Option: (A)

Explanation: Ionic bonding occurs when one or more valence electrons are completely transferred from a metal atom to a non-metal atom, resulting in electrostatic attraction between oppositely charged ions ($Na^+$ and $Cl^-$).

In a molecule of hydrogen gas ($H_2$), two hydrogen atoms each contribute one electron to achieve a stable electronic configuration.
What type of bond holds the two hydrogen atoms together?

(A)

Ionic bond

(B)

Nonpolar covalent bond

(C)

Coordinate covalent bond

(D)

Hydrogen bond

View Correct Answer & Detailed Solution

✓ Correct Option: (B)

Explanation: A covalent bond involves equal sharing of electron pairs between two atoms of the same electronegativity, forming a nonpolar covalent bond.

According to the octet rule, main-group elements generally tend to bond in such a way that each atom has how many electrons in its valence shell?

(A)

(B)

(C)

(D)

View Correct Answer & Detailed Solution

✓ Correct Option: (C)

Explanation: The octet rule states that atoms tend to gain, lose, or share electrons to achieve a noble gas configuration containing 8 valence electrons.

In a water molecule ($H_2O$), oxygen has an electronegativity of 3.44 while hydrogen has an electronegativity of 2.20.
How should the $O-H$ bonds in water be classified based on this electronegativity difference?

(A)

Nonpolar covalent

(B)

Polar covalent

(C)

Purely ionic

(D)

Metallic

View Correct Answer & Detailed Solution

✓ Correct Option: (B)

Explanation: An electronegativity difference between approximately 0.4 and 1.7 leads to unequal sharing of bonding electrons, creating a polar covalent bond.

What is the total number of valence electrons present in a methane ($CH_4$) molecule?

(A)

(B)

(C)

(D)

View Correct Answer & Detailed Solution

✓ Correct Option: (A)

Explanation: Carbon contributes 4 valence electrons and each of the 4 hydrogen atoms contributes 1 valence electron: $4 + 4(1) = 8$ valence electrons.

Consider beryllium chloride ($BeCl_2$) in the gas phase, where beryllium has two bonding electron pairs and no lone pairs around the central atom.
What molecular geometry is predicted by VSEPR theory for $BeCl_2$?

(A)

Bent

(B)

Trigonal planar

(C)

Tetrahedral

(D)

Linear

View Correct Answer & Detailed Solution

✓ Correct Option: (D)

Explanation: With 2 electron domains and zero lone pairs around the central atom, VSEPR theory predicts a linear shape with a bond angle of $180^ op$.

An ammonium ion ($NH_4^+$) is formed when an ammonia molecule ($NH_3$) reacts with a hydrogen ion ($H^+$).
What type of bond is formed when the lone pair on nitrogen is donated to the vacant orbital of $H^+$?

(A)

Ionic bond

(B)

Coordinate covalent (dative) bond

(C)

Hydrogen bond

(D)

Metallic bond

View Correct Answer & Detailed Solution

✓ Correct Option: (B)

Explanation: A coordinate covalent (or dative) bond occurs when both shared electrons in a bond are provided by a single donor atom.

Which set of elements can form strong hydrogen bonds when directly bonded to hydrogen?

(A)

C, N, O

(B)

Na, K, Cl

(C)

N, O, F

(D)

F, Cl, Br

View Correct Answer & Detailed Solution

✓ Correct Option: (C)

Explanation: Hydrogen bonding requires hydrogen to be covalently attached to highly electronegative, small atoms: Nitrogen ($N$), Oxygen ($O$), or Fluorine ($F$).

Comparing carbon-carbon single ($C-C$), double ($C=C$), and triple ($C≡C$) bonds in organic compounds.
Which bond type has the shortest bond length and highest bond dissociation energy?

(A)

Triple bond ($C≡C$)

(B)

Double bond ($C=C$)

(C)

Single bond ($C-C$)

(D)

All have equal bond length

View Correct Answer & Detailed Solution

✓ Correct Option: (A)

Explanation: As bond order increases (single to double to triple), more shared electrons draw the nuclei closer together, shortening the bond and increasing bond strength.

Q10

How many sigma ($σ$) and pi ($π$) bonds are present in a single covalent double bond between two atoms?

(A)

2 sigma bonds, 0 pi bonds

(B)

1 sigma bond, 1 pi bond

(C)

0 sigma bonds, 2 pi bonds

(D)

1 sigma bond, 2 pi bonds

View Correct Answer & Detailed Solution

✓ Correct Option: (B)

Explanation: A single double bond consists of 1 head-on overlapping sigma ($σ$) bond and 1 sideways overlapping pi ($π$) bond.

Q11

In methane ($CH_4$), the central carbon atom forms four equivalent $C-H$ single bonds directed toward the corners of a regular tetrahedron.
What is the hybridization state of the central carbon atom in $CH_4$?

(A)

(B)

$sp^2$

(C)

$sp^3$

(D)

$sp^3d$

View Correct Answer & Detailed Solution

✓ Correct Option: (C)

Explanation: Mixing one $s$ orbital and three $p$ orbitals yields four equivalent $sp^3$ hybrid orbitals directed tetrahedrally with bond angles of $109.5^ op$.

Q12

Carbon dioxide ($CO_2$) contains two polar $C=O$ double bonds arranged linearly ($O=C=O$).
Why is the net dipole moment of carbon dioxide equal to zero ($μ = 0$ D)?

(A)

The individual bond dipole moments cancel out due to symmetrical linear geometry

(B)

The $C=O$ bonds are completely nonpolar

(C)

Carbon and oxygen have identical electronegativity

(D)

Lone pairs on carbon cancel the bond dipoles

View Correct Answer & Detailed Solution

✓ Correct Option: (A)

Explanation: $CO_2$ is a linear molecule ($180^ op$). The two equal bond dipoles point in opposite directions and cancel vectorially, resulting in a nonpolar molecule.

Q13

Metals exhibit high electrical conductivity, malleability, and metallic luster.
Which model best describes the bonding in solid metallic copper?

(A)

Rigid network of shared electron pairs

(B)

Alternating cations and anions held by electrostatic forces

(C)

Discrete molecules held together by dispersion forces

(D)

Positive metal ions immersed in a sea of delocalized valence electrons

View Correct Answer & Detailed Solution

✓ Correct Option: (D)

Explanation: Metallic bonding is described as an array of positive atomic cores (cations) suspended within a mobile, delocalized 'sea of electrons'.

Q14

What is the formal charge of the central oxygen atom in the ozone molecule ($O_3$) with the resonance structure $O=Äö^+-O^-$?

(A)

(B)

(C)

-1

(D)

View Correct Answer & Detailed Solution

✓ Correct Option: (B)

Explanation: Formal charge = Valence $e^-$ - Lone pair $e^-$ - $½$(Bonding $e^-$). For central oxygen: $6 - 2 - ½(6) = 6 - 2 - 3 = +1$.

Q15

Carbonate ion ($CO_3^{2-}$) cannot be accurately represented by a single Lewis structure, as all three $C-O$ bonds are experimentally found to be identical in length and strength.
Which phenomenon accounts for this equivalency of bonds?

(A)

Resonance

(B)

Hydrogen bonding

(C)

Van der Waals attraction

(D)

Electronegativity reversal

View Correct Answer & Detailed Solution

✓ Correct Option: (A)

Explanation: Resonance occurs when two or more valid Lewis structures describe a molecule; the actual structure is a hybrid with intermediate bond character.

Q16

According to Molecular Orbital (MO) Theory, why is molecular oxygen ($O_2$) paramagnetic?

(A)

All of its electrons are paired

(B)

It contains a triple bond

(C)

It contains two unpaired electrons in antibonding $π^*$ orbitals

(D)

Its bond order is zero

View Correct Answer & Detailed Solution

✓ Correct Option: (C)

Explanation: The MO configuration of $O_2$ places one unpaired electron in each of the degenerate $π^*2p_x$ and $π^*2p_y$ antibonding orbitals, making it paramagnetic.

Q17

Lattice enthalpy measures the strength of ionic bonds in a crystal lattice.
Which combination of ionic properties leads to the highest lattice enthalpy?

(A)

High ionic charges and small ionic radii

(B)

Low ionic charges and large ionic radii

(C)

Low ionic charges and small ionic radii

(D)

High ionic charges and large ionic radii

View Correct Answer & Detailed Solution

✓ Correct Option: (A)

Explanation: Lattice enthalpy is directly proportional to the product of ionic charges ($q_1 q_2$) and inversely proportional to internuclear distance ($r$).

Q18

Consider methane ($CH_4$), ammonia ($NH_3$), and water ($H_2O$). Each central atom has 4 electron pairs (tetrahedral electron geometry).
What is the approximate $H-N-H$ bond angle in ammonia ($NH_3$)?

(A)

$109.5^ op$

(B)

$107^ op$

(C)

$104.5^ op$

(D)

$120^ op$

View Correct Answer & Detailed Solution

✓ Correct Option: (B)

Explanation: Ammonia has 3 bonding pairs and 1 lone pair. Lone pair-bonding pair repulsion compresses the ideal tetrahedral angle ($109.5^ op$) to about $107^ op$.

Q19

Which type of weak intermolecular force exists between all atoms and molecules, including nonpolar noble gas atoms like Argon (Ar)?

(A)

Ionic force

(B)

Dipole-dipole force

(C)

Covalent bonding

(D)

London dispersion forces

View Correct Answer & Detailed Solution

✓ Correct Option: (D)

Explanation: London dispersion forces arise from temporary, instantaneous dipole fluctuations and exist between all atoms and molecules.

Q20

Two $p$ orbitals on adjacent atoms overlap laterally (sideways), perpendicular to the internuclear axis.
What type of covalent bond is produced by this lateral overlap?

(A)

Sigma ($σ$) bond

(B)

Ionic bond

(C)

Pi ($π$) bond

(D)

Metallic bond

View Correct Answer & Detailed Solution

✓ Correct Option: (C)

Explanation: Sideways (parallel) overlap of atomic $p$ orbitals produces a pi ($π$) bond with electron density above and below the internuclear axis.

Grade 11 : Chemistry - Chemical Bonding (Set 2)

Grade 11 : Chemistry - Chemical Bonding (Set 2)— Questions & Detailed Solutions

A sodium atom (Na) transfers its single valence electron to a chlorine atom (Cl) to form a stable crystal lattice of sodium chloride (NaCl).
Which type of chemical bond is formed during this process?

In a molecule of hydrogen gas ($H_2$), two hydrogen atoms each contribute one electron to achieve a stable electronic configuration.
What type of bond holds the two hydrogen atoms together?

According to the octet rule, main-group elements generally tend to bond in such a way that each atom has how many electrons in its valence shell?

In a water molecule ($H_2O$), oxygen has an electronegativity of 3.44 while hydrogen has an electronegativity of 2.20.
How should the $O-H$ bonds in water be classified based on this electronegativity difference?

What is the total number of valence electrons present in a methane ($CH_4$) molecule?

Consider beryllium chloride ($BeCl_2$) in the gas phase, where beryllium has two bonding electron pairs and no lone pairs around the central atom.
What molecular geometry is predicted by VSEPR theory for $BeCl_2$?

An ammonium ion ($NH_4^+$) is formed when an ammonia molecule ($NH_3$) reacts with a hydrogen ion ($H^+$).
What type of bond is formed when the lone pair on nitrogen is donated to the vacant orbital of $H^+$?

Which set of elements can form strong hydrogen bonds when directly bonded to hydrogen?

Comparing carbon-carbon single ($C-C$), double ($C=C$), and triple ($C≡C$) bonds in organic compounds.
Which bond type has the shortest bond length and highest bond dissociation energy?

How many sigma ($σ$) and pi ($π$) bonds are present in a single covalent double bond between two atoms?

In methane ($CH_4$), the central carbon atom forms four equivalent $C-H$ single bonds directed toward the corners of a regular tetrahedron.
What is the hybridization state of the central carbon atom in $CH_4$?

Carbon dioxide ($CO_2$) contains two polar $C=O$ double bonds arranged linearly ($O=C=O$).
Why is the net dipole moment of carbon dioxide equal to zero ($μ = 0$ D)?

Metals exhibit high electrical conductivity, malleability, and metallic luster.
Which model best describes the bonding in solid metallic copper?

What is the formal charge of the central oxygen atom in the ozone molecule ($O_3$) with the resonance structure $O=Äö^+-O^-$?

Carbonate ion ($CO_3^{2-}$) cannot be accurately represented by a single Lewis structure, as all three $C-O$ bonds are experimentally found to be identical in length and strength.
Which phenomenon accounts for this equivalency of bonds?

According to Molecular Orbital (MO) Theory, why is molecular oxygen ($O_2$) paramagnetic?

Lattice enthalpy measures the strength of ionic bonds in a crystal lattice.
Which combination of ionic properties leads to the highest lattice enthalpy?

Consider methane ($CH_4$), ammonia ($NH_3$), and water ($H_2O$). Each central atom has 4 electron pairs (tetrahedral electron geometry).
What is the approximate $H-N-H$ bond angle in ammonia ($NH_3$)?

Which type of weak intermolecular force exists between all atoms and molecules, including nonpolar noble gas atoms like Argon (Ar)?

Two $p$ orbitals on adjacent atoms overlap laterally (sideways), perpendicular to the internuclear axis.
What type of covalent bond is produced by this lateral overlap?

Discussion 0

Enjoyed this content?

Grade 11 : Chemistry - Chemical Bonding (Set 2)

Grade 11 : Chemistry - Chemical Bonding (Set 2)— Questions & Detailed Solutions

A sodium atom (Na) transfers its single valence electron to a chlorine atom (Cl) to form a stable crystal lattice of sodium chloride (NaCl).Which type of chemical bond is formed during this process?

In a molecule of hydrogen gas ($H_2$), two hydrogen atoms each contribute one electron to achieve a stable electronic configuration.What type of bond holds the two hydrogen atoms together?

According to the octet rule, main-group elements generally tend to bond in such a way that each atom has how many electrons in its valence shell?

In a water molecule ($H_2O$), oxygen has an electronegativity of 3.44 while hydrogen has an electronegativity of 2.20.How should the $O-H$ bonds in water be classified based on this electronegativity difference?

What is the total number of valence electrons present in a methane ($CH_4$) molecule?

Consider beryllium chloride ($BeCl_2$) in the gas phase, where beryllium has two bonding electron pairs and no lone pairs around the central atom.What molecular geometry is predicted by VSEPR theory for $BeCl_2$?

An ammonium ion ($NH_4^+$) is formed when an ammonia molecule ($NH_3$) reacts with a hydrogen ion ($H^+$).What type of bond is formed when the lone pair on nitrogen is donated to the vacant orbital of $H^+$?

Which set of elements can form strong hydrogen bonds when directly bonded to hydrogen?

Comparing carbon-carbon single ($C-C$), double ($C=C$), and triple ($C≡C$) bonds in organic compounds.Which bond type has the shortest bond length and highest bond dissociation energy?

How many sigma ($σ$) and pi ($π$) bonds are present in a single covalent double bond between two atoms?

In methane ($CH_4$), the central carbon atom forms four equivalent $C-H$ single bonds directed toward the corners of a regular tetrahedron.What is the hybridization state of the central carbon atom in $CH_4$?

Carbon dioxide ($CO_2$) contains two polar $C=O$ double bonds arranged linearly ($O=C=O$).Why is the net dipole moment of carbon dioxide equal to zero ($μ = 0$ D)?

Metals exhibit high electrical conductivity, malleability, and metallic luster.Which model best describes the bonding in solid metallic copper?

What is the formal charge of the central oxygen atom in the ozone molecule ($O_3$) with the resonance structure $O=Äö^+-O^-$?

Carbonate ion ($CO_3^{2-}$) cannot be accurately represented by a single Lewis structure, as all three $C-O$ bonds are experimentally found to be identical in length and strength.Which phenomenon accounts for this equivalency of bonds?

According to Molecular Orbital (MO) Theory, why is molecular oxygen ($O_2$) paramagnetic?

Lattice enthalpy measures the strength of ionic bonds in a crystal lattice.Which combination of ionic properties leads to the highest lattice enthalpy?

Consider methane ($CH_4$), ammonia ($NH_3$), and water ($H_2O$). Each central atom has 4 electron pairs (tetrahedral electron geometry).What is the approximate $H-N-H$ bond angle in ammonia ($NH_3$)?

Which type of weak intermolecular force exists between all atoms and molecules, including nonpolar noble gas atoms like Argon (Ar)?

Two $p$ orbitals on adjacent atoms overlap laterally (sideways), perpendicular to the internuclear axis.What type of covalent bond is produced by this lateral overlap?

Share This Quiz

Discussion 0

Enjoyed this content?

More Quizzes for Grade 11

Grade 11 : Mathematics - Sets (Set 2) | Concept of Maths

Grade 11 : Chemistry - Basic Concepts (Set 7) | Concept of Maths

Grade 11 : Biology - Morphology of Plants (Set 3)

Grade 11 : Biology - Morphology of Plants (Set 4)

Grade 11 : Mathematics - Sets (Set 2) | Concept of Maths

Grade 11 : Mathematics - Relations (Set 2) | Concept of Maths

A sodium atom (Na) transfers its single valence electron to a chlorine atom (Cl) to form a stable crystal lattice of sodium chloride (NaCl).
Which type of chemical bond is formed during this process?

In a molecule of hydrogen gas ($H_2$), two hydrogen atoms each contribute one electron to achieve a stable electronic configuration.
What type of bond holds the two hydrogen atoms together?

In a water molecule ($H_2O$), oxygen has an electronegativity of 3.44 while hydrogen has an electronegativity of 2.20.
How should the $O-H$ bonds in water be classified based on this electronegativity difference?

Consider beryllium chloride ($BeCl_2$) in the gas phase, where beryllium has two bonding electron pairs and no lone pairs around the central atom.
What molecular geometry is predicted by VSEPR theory for $BeCl_2$?

An ammonium ion ($NH_4^+$) is formed when an ammonia molecule ($NH_3$) reacts with a hydrogen ion ($H^+$).
What type of bond is formed when the lone pair on nitrogen is donated to the vacant orbital of $H^+$?

Comparing carbon-carbon single ($C-C$), double ($C=C$), and triple ($C≡C$) bonds in organic compounds.
Which bond type has the shortest bond length and highest bond dissociation energy?

In methane ($CH_4$), the central carbon atom forms four equivalent $C-H$ single bonds directed toward the corners of a regular tetrahedron.
What is the hybridization state of the central carbon atom in $CH_4$?

Carbon dioxide ($CO_2$) contains two polar $C=O$ double bonds arranged linearly ($O=C=O$).
Why is the net dipole moment of carbon dioxide equal to zero ($μ = 0$ D)?

Metals exhibit high electrical conductivity, malleability, and metallic luster.
Which model best describes the bonding in solid metallic copper?

Carbonate ion ($CO_3^{2-}$) cannot be accurately represented by a single Lewis structure, as all three $C-O$ bonds are experimentally found to be identical in length and strength.
Which phenomenon accounts for this equivalency of bonds?

Lattice enthalpy measures the strength of ionic bonds in a crystal lattice.
Which combination of ionic properties leads to the highest lattice enthalpy?

Consider methane ($CH_4$), ammonia ($NH_3$), and water ($H_2O$). Each central atom has 4 electron pairs (tetrahedral electron geometry).
What is the approximate $H-N-H$ bond angle in ammonia ($NH_3$)?

Two $p$ orbitals on adjacent atoms overlap laterally (sideways), perpendicular to the internuclear axis.
What type of covalent bond is produced by this lateral overlap?