Welcome to Inamjazbi Learn Chemistry! 🎉 This ultimate Class 11 Chemistry MCQs test covers ChemicalBonding. Test your knowledge with interactive questions, get instant feedback on each answer, and see your final score at the end! 🧠Keep track of your score and challenge yourself!
Whether you are preparing for exams or just love Chemistry, this quiz is perfect for sharpening your concepts. Ready, set, answer! ⚡
#Class11Chemistry #ChemistryMCQs #InamjazbiLearnChemistry #InteractiveQuiz #ChemistryTest #AtomicStructure #PeriodicTable #ChemicalBonding #StudyChemistry #ExamPrep
🔥🌟 Grand Chemistry Interactive MCQs Quiz Test on Chemical Bonding for Class FSC/MDCAT/ECAT Set I 🧪💡 | Learn & Practice!
1. If the bond angle is AB₂ type molecule is 104.5°, it geometry should be;
a) Linear
b) Pyramidal
c) Bent
d) Planar Trigonal
✅ Correct Answer: (c)
The bond angle of 104.5° is the characteristic of AB₂ type of molecules with bent or V-shaped or angular geometry.
The bond angle of 104.5° is the characteristic of AB₂ type of molecules with bent or V-shaped or angular geometry.
2. The highest bond energy in the following is:
a) Cl–Cl
b) H–F
c) H–O
d) H–N
✅ Correct Answer: (b)
Bond energy is directly proportional to the bond polarity or partial ionic character which in turn is proportional to the difference in electronegativity of the bonded atoms. Greater the ΔEN, greater is the bond energy. H–F bond has the greatest ΔEN (1.9) and hence it has the highest bond energy (in fact highest among all diatomic molecules containing single bond; 570 kJmol⁻¹). The second highest bond energy is for H – O bond with second highest ΔEN (1.4). The next highest bond energy is for H–N bond with third highest ΔEN (0.9). Cl–Cl being non-polar has the least bond energy.
Bond energy is directly proportional to the bond polarity or partial ionic character which in turn is proportional to the difference in electronegativity of the bonded atoms. Greater the ΔEN, greater is the bond energy. H–F bond has the greatest ΔEN (1.9) and hence it has the highest bond energy (in fact highest among all diatomic molecules containing single bond; 570 kJmol⁻¹). The second highest bond energy is for H – O bond with second highest ΔEN (1.4). The next highest bond energy is for H–N bond with third highest ΔEN (0.9). Cl–Cl being non-polar has the least bond energy.
3. The molecule which has zero dipole moment is:
a) NH₃
b) HCl
c) H₂O
d) CCl₄
✅ Correct Answer: (d)
Symmetrical molecules with linear, trigonal or tetrahedral geometry show zero dipole moment. CCl₄ has symmetrical tetrahedral structure in which all four bond moments for C–Cl bonds being directed in opposite directions are cancel out giving net zero dipole moment.
Symmetrical molecules with linear, trigonal or tetrahedral geometry show zero dipole moment. CCl₄ has symmetrical tetrahedral structure in which all four bond moments for C–Cl bonds being directed in opposite directions are cancel out giving net zero dipole moment.
4. The molecule which has maximum bond angle
a) CS₂
b) H₂O
c) NH₃
d) BF₃
✅ Correct Answer: (a)
Linear molecules like CS₂, CO₂, BeCl₂, C₂H₂, HgCl₂, ZnCl₂ etc. with AB₂ formula has the largest bond angle of 180°.
Linear molecules like CS₂, CO₂, BeCl₂, C₂H₂, HgCl₂, ZnCl₂ etc. with AB₂ formula has the largest bond angle of 180°.
5. The shape and hybridization of BCl₃ molecule is:
a) Tetrahedral & sp³
b) Linear & sp
c) Planar trigonal & sp²
d) Angular & sp³
✅ Correct Answer: (c)
Being AB₃ molecule with no non-bonding orbital, BCl₃ has sp² hybridization with planar trigonal shape.
Being AB₃ molecule with no non-bonding orbital, BCl₃ has sp² hybridization with planar trigonal shape.
6. Amongst the following molecules which one has trigonal pyramidal shape?
a) SO₂
b) CO₂
c) NH₃
d) C₂H₄
✅ Correct Answer: (c)
The ÄB₃ molecules like :NH₃, :PH₃, :PCl₃, :NCl₃ etc. with one lone pair & 3 bond pairs has trigonal pyramidal shape
The ÄB₃ molecules like :NH₃, :PH₃, :PCl₃, :NCl₃ etc. with one lone pair & 3 bond pairs has trigonal pyramidal shape
7. A simple covalent molecule possesses two bond pairs and two lone pairs around the central atom, its shape should be:
a) Linear
b) Planar trigonal
c) Angular
d) Tetrahedral
✅ Correct Answer: (c)
The presence of two bond pairs and two lone pairs around the central atom gives rise to angular shape to the molecules. Such molecules have :ÄB₂ type general formula.
The presence of two bond pairs and two lone pairs around the central atom gives rise to angular shape to the molecules. Such molecules have :ÄB₂ type general formula.
8. The correct relation between Debye and coulomb meter is:
a) 1D=3.33 ×10⁻³⁰Cm
b) 1D = 1.6 × 10⁻¹⁹Cm
c) 1D = 1.88 × 10⁻¹²Cm
d) 1D =1.23 × 10⁻⁸Cm
✅ Correct Answer: (a)
The SI unit of dipole moment C-M and cgs unit debye is inter related as 1D = 3.33 × 10⁻³⁰Cm.
The SI unit of dipole moment C-M and cgs unit debye is inter related as 1D = 3.33 × 10⁻³⁰Cm.
9. The bond order of N₂ molecule is:
a) 0
b) 1
c) 2
d) 3
✅ Correct Answer: (d)
The bond order of N₂ molecule is 3 showing that it has triple bond between two nitrogen atoms.
The bond order of N₂ molecule is 3 showing that it has triple bond between two nitrogen atoms.
10. The number of sigma and pi bonds in C₂H₄ molecules are respectively:
a) 3 and 1
b) 2 and 2
c) 5 and 1
d) 4 and 2
✅ Correct Answer: (c)
There are total 5 sigma and one pi bond in in C₂H₄ molecule.
There are total 5 sigma and one pi bond in in C₂H₄ molecule.
11. In which of the following molecules octet rule is NOT followed?
a) CH₄
b) NH₃
c) NO
d) CO₂
✅ Correct Answer: (c)
NO is an odd electron molecules containing N with 7 valence electrons (because NO has an odd number of electrons: 11 total). This means nitrogen cannot complete an octet — it has only 7 electrons around it.Hence, NO is an odd electron molecule and does not follow the octet rule. ✨ Key Point: Odd electron molecules (like NO, NO₂, ClO₂) are exceptions to the octet rule. They can’t have 8 electrons around the central atom because the total number of valence electrons is odd.
NO is an odd electron molecules containing N with 7 valence electrons (because NO has an odd number of electrons: 11 total). This means nitrogen cannot complete an octet — it has only 7 electrons around it.Hence, NO is an odd electron molecule and does not follow the octet rule. ✨ Key Point: Odd electron molecules (like NO, NO₂, ClO₂) are exceptions to the octet rule. They can’t have 8 electrons around the central atom because the total number of valence electrons is odd.
12. Neutral atoms of Neon have the same number of electrons as each of the following EXCEPT:
a) F⁻
b) Na⁺
c) Mg²⁺
d) O⁻
✅ Correct Answer: (d)
Neon has 10 electrons. All the ions given have 10 electrons except O⁻ which has 9 electrons.
Neon has 10 electrons. All the ions given have 10 electrons except O⁻ which has 9 electrons.
13. Which of the following compounds exhibits the highest ionic character due to large electronegativity difference and strong lattice energy?
a) NaCl
b) KCl
c) MgO
d) All of them equally
✅ Correct Answer: (c) MgO
🔎 NaCl & KCl: Both are classic ionic salts (metal + non metal). They have strong ionic bonds, but their lattice energies are lower compared to MgO. In MgO, Magnesium is a +2 cation, oxygen is a –2 anion. The charges are higher (+2/–2 vs +1/–1 in NaCl/KCl). This gives much stronger electrostatic attraction and higher lattice energy. Hence, MgO has the highest ionic character. All of them: Incorrect, because ionic character varies with charge and electronegativity difference.✨ Key Concept for MDCAT: Ionic bond strength ∝ (charge on ions × electronegativity difference) / distance between ions. Higher charges (like Mg²⁺ and O²⁻) → stronger ionic bond. Therefore, MgO is the most ionic among the given compounds.
🔎 NaCl & KCl: Both are classic ionic salts (metal + non metal). They have strong ionic bonds, but their lattice energies are lower compared to MgO. In MgO, Magnesium is a +2 cation, oxygen is a –2 anion. The charges are higher (+2/–2 vs +1/–1 in NaCl/KCl). This gives much stronger electrostatic attraction and higher lattice energy. Hence, MgO has the highest ionic character. All of them: Incorrect, because ionic character varies with charge and electronegativity difference.✨ Key Concept for MDCAT: Ionic bond strength ∝ (charge on ions × electronegativity difference) / distance between ions. Higher charges (like Mg²⁺ and O²⁻) → stronger ionic bond. Therefore, MgO is the most ionic among the given compounds.
14. Which of the following compounds contains a predominantly covalent bond, considering electronegativity differences and the nature of the elements involved?
a) NaCl
b) CaCO₃
c) MgO
d) HCl
✅ Correct Answer: (d)
Non-metallic elements with electronegativity difference less than 1.7 form covalent bond. Both H and Cl are non-metals with ΔEN ≈ 0.9 (< 1.7 threshold), so bond is polar covalent (not purely ionic). 👉 Therefore, HCl is the correct answer because it is formed between two non metals with ΔEN < 1.7. In NaCl: Na (metal) + Cl (non metal) with ΔEN ≈ 2.1 → strongly ionic. In CaCO₃, Ca²⁺ bonded ionically to CO₃²⁻.Inside carbonate, C–O bonds are covalent, but overall compound is ionic. In MgO, ΔEN ≈ 2.3 → highly ionic with strong lattice energy.
Non-metallic elements with electronegativity difference less than 1.7 form covalent bond. Both H and Cl are non-metals with ΔEN ≈ 0.9 (< 1.7 threshold), so bond is polar covalent (not purely ionic). 👉 Therefore, HCl is the correct answer because it is formed between two non metals with ΔEN < 1.7. In NaCl: Na (metal) + Cl (non metal) with ΔEN ≈ 2.1 → strongly ionic. In CaCO₃, Ca²⁺ bonded ionically to CO₃²⁻.Inside carbonate, C–O bonds are covalent, but overall compound is ionic. In MgO, ΔEN ≈ 2.3 → highly ionic with strong lattice energy.
15. Which of the following molecules contains only single covalent bonds formed by orbital overlap, with no double or triple bonds present?
a) O₂
b) N₂
c) CO₂
d) CH₄
✅ Correct Answer: (d) CH₄
🔎 O₂ (Oxygen): Bond order = 2 → contains a double bond. Not purely single bonds.🔎 N₂ (Nitrogen):Bond order = 3 → contains a triple bond. Not purely single bonds.🔎 CO₂ (Carbon dioxide): Each C–O bond is a double bond. No single bonds present.🔎 CH₄ (Methane):Carbon undergoes sp³ hybridization.Forms four equivalent single covalent bonds with hydrogen atoms. Each bond is formed by overlap of C–H orbitals. Therefore, CH₄ is the only molecule here with only single covalent bonds.✨ Advanced Concept for MDCATBond order determines whether a bond is single, double, or triple. Molecules like O₂, N₂, CO₂ have higher bond orders → multiple bonds. CH₄ is unique because it has only single bonds and is a classic example of tetrahedral geometry with bond angle 109.5°.
🔎 O₂ (Oxygen): Bond order = 2 → contains a double bond. Not purely single bonds.🔎 N₂ (Nitrogen):Bond order = 3 → contains a triple bond. Not purely single bonds.🔎 CO₂ (Carbon dioxide): Each C–O bond is a double bond. No single bonds present.🔎 CH₄ (Methane):Carbon undergoes sp³ hybridization.Forms four equivalent single covalent bonds with hydrogen atoms. Each bond is formed by overlap of C–H orbitals. Therefore, CH₄ is the only molecule here with only single covalent bonds.✨ Advanced Concept for MDCATBond order determines whether a bond is single, double, or triple. Molecules like O₂, N₂, CO₂ have higher bond orders → multiple bonds. CH₄ is unique because it has only single bonds and is a classic example of tetrahedral geometry with bond angle 109.5°.
16. Which of the following correctly describes the bond angle and hybridization in methane (CH₄)?
a) Bond angle = 120°, Hybridization = sp²
b) Bond angle = 109.5°, Hybridization = sp³
c) Bond angle = 180°, Hybridization = sp
d) Bond angle = 104.5°, Hybridization = sp³
✅ (b) Bond angle = 109.5°, Hybridization = sp³
🔎 In CH₄, carbon forms 4 single covalent bonds with hydrogen. To minimize electron pair repulsion, carbon undergoes sp³ hybridization. This produces a tetrahedral geometry.The ideal bond angle in a tetrahedron is 109.5°. 🔎 Options (a), (c), and (d) are incorrect because they correspond to trigonal planar (120°), linear (180°), and bent/angular (104.5°) geometries, respectively.✨ Key Concept for MDCAT: 💡 sp³ hybridization → tetrahedral → 109.5° bond angle. 💡 sp² hybridization → trigonal planar → 120° bond angle. 💡 sp hybridization → linear → 180° bond angle. 💡 Bent/angular molecules (like H₂O) → ~104.5° bond angle
🔎 In CH₄, carbon forms 4 single covalent bonds with hydrogen. To minimize electron pair repulsion, carbon undergoes sp³ hybridization. This produces a tetrahedral geometry.The ideal bond angle in a tetrahedron is 109.5°. 🔎 Options (a), (c), and (d) are incorrect because they correspond to trigonal planar (120°), linear (180°), and bent/angular (104.5°) geometries, respectively.✨ Key Concept for MDCAT: 💡 sp³ hybridization → tetrahedral → 109.5° bond angle. 💡 sp² hybridization → trigonal planar → 120° bond angle. 💡 sp hybridization → linear → 180° bond angle. 💡 Bent/angular molecules (like H₂O) → ~104.5° bond angle
17. Which of the following elements, when acting as the central atom, can accommodate more than eight valence electrons due to the availability of vacant d orbitals?
a) N
b) Te
c) F
d) O
✅ Correct Answer: (b)
🔎 Nitrogen (N), Oxygen (O), Fluorine (F):All are Period 2 elements.Their valence shell has only s and p orbitals (no d orbitals).Therefore, they cannot expand their octet beyond 8 electrons. Tellurium (Te):A Period 5 element.Has vacant 5d orbitals available in its valence shell.Can expand its octet and form compounds like TeCl₆²⁻, where Te accommodates 12 valence electrons. 👉 Thus, Te is capable of having more than eight valence electrons.✨ Advanced Concept for MDCAT: Octet rule exceptions:💡 Odd electron molecules (e.g., NO, ClO₂).💡 Incomplete octet (e.g., BeCl₂, BF₃).💡 Expanded octet (elements in Period ≥ 3, e.g., PCl₅, SF₆, TeCl₆²⁻).💡 Expansion is possible only when vacant d orbitals are available in the valence shell.
🔎 Nitrogen (N), Oxygen (O), Fluorine (F):All are Period 2 elements.Their valence shell has only s and p orbitals (no d orbitals).Therefore, they cannot expand their octet beyond 8 electrons. Tellurium (Te):A Period 5 element.Has vacant 5d orbitals available in its valence shell.Can expand its octet and form compounds like TeCl₆²⁻, where Te accommodates 12 valence electrons. 👉 Thus, Te is capable of having more than eight valence electrons.✨ Advanced Concept for MDCAT: Octet rule exceptions:💡 Odd electron molecules (e.g., NO, ClO₂).💡 Incomplete octet (e.g., BeCl₂, BF₃).💡 Expanded octet (elements in Period ≥ 3, e.g., PCl₅, SF₆, TeCl₆²⁻).💡 Expansion is possible only when vacant d orbitals are available in the valence shell.
18. The electronic structure of SO₂ is best represented as a resonance hybrid. Which statement correctly explains the nature of its bonding?
a) SO₂ is a resonance hybrid of two equivalent structures with identical S–O bond lengths.
b) SO₂ contains one S=O double bond and one S–O single bond, giving unequal bond lengths.
c) SO₂ is a resonance hybrid of three structures, each with different bond orders.
d) SO₂ has no resonance and contains only localized bonds.
✅ Correct Answer: (a)
🔎 Resonance in SO₂:Two equivalent resonance structures can be drawn: one with double bond to the left oxygen, one with double bond to the right oxygen. 👉 In reality, the molecule is a resonance hybrid of these two. Both S–O bonds are identical in length and strength. Bond order is intermediate (~1.5) for each S–O bond due to delocalization. Resonance involves pπ–pπ overlap and pπ–dπ overlap. This delocalization stabilizes the molecule.✨ Advanced Concept for MDCAT:Resonance explains why bond lengths are equal even if Lewis structures suggest otherwise. In SO₂, resonance hybridization gives delocalized π electrons.
🔎 Resonance in SO₂:Two equivalent resonance structures can be drawn: one with double bond to the left oxygen, one with double bond to the right oxygen. 👉 In reality, the molecule is a resonance hybrid of these two. Both S–O bonds are identical in length and strength. Bond order is intermediate (~1.5) for each S–O bond due to delocalization. Resonance involves pπ–pπ overlap and pπ–dπ overlap. This delocalization stabilizes the molecule.✨ Advanced Concept for MDCAT:Resonance explains why bond lengths are equal even if Lewis structures suggest otherwise. In SO₂, resonance hybridization gives delocalized π electrons.
19. Which of the following compounds is expected to have the lowest melting point, considering lattice energy, ionic charges, and polarization effects?
a) Al₂O₃
b) MgO
c) NaCl
d) Fe₂O₃
✅ Correct Answer: (c) NaCl
🔎 ⚡Al₂O₃ (Al³⁺ / O²⁻): Very high charges (+3/–2). Strong electrostatic attraction → very high lattice energy → very high melting point.⚡MgO (Mg²⁺ / O²⁻):Charges +2/–2.Stronger attraction than NaCl → higher melting point.⚡Fe₂O₃ (Fe³⁺ / O²⁻):Charges +3/–2.Strong ionic bonds → high melting point.⚡NaCl (Na⁺ / Cl⁻):Charges only +1/–1.Lowest electrostatic attraction. Lowest lattice energy. 👉 Therefore, lowest melting point among the given compounds.✨ Advanced Concept for MDCAT:⚡Lattice energy ∝ (charge on ions × charge on ions) / distance between ions⚡Higher charges → stronger attraction → higher melting point.⚡Smaller ions → stronger attraction → higher melting point.⚡NaCl has the lowest melting point because it involves monovalent ions (+1/–1) with relatively large ionic radii compared to Mg²⁺, Al³⁺, Fe³⁺.
🔎 ⚡Al₂O₃ (Al³⁺ / O²⁻): Very high charges (+3/–2). Strong electrostatic attraction → very high lattice energy → very high melting point.⚡MgO (Mg²⁺ / O²⁻):Charges +2/–2.Stronger attraction than NaCl → higher melting point.⚡Fe₂O₃ (Fe³⁺ / O²⁻):Charges +3/–2.Strong ionic bonds → high melting point.⚡NaCl (Na⁺ / Cl⁻):Charges only +1/–1.Lowest electrostatic attraction. Lowest lattice energy. 👉 Therefore, lowest melting point among the given compounds.✨ Advanced Concept for MDCAT:⚡Lattice energy ∝ (charge on ions × charge on ions) / distance between ions⚡Higher charges → stronger attraction → higher melting point.⚡Smaller ions → stronger attraction → higher melting point.⚡NaCl has the lowest melting point because it involves monovalent ions (+1/–1) with relatively large ionic radii compared to Mg²⁺, Al³⁺, Fe³⁺.
20. Which of the following bonds exhibits the least polar character, considering electronegativity differences and resulting partial charges?
a) C–H
b) C–Cl
c) C–O
d) C–N
✅ Correct Answer: (a) C–H)
🔎 Polarity depends on ΔEN (electronegativity difference): Greater ΔEN → more polar bond. Smaller ΔEN → less polar bond.⚡C–H: ΔEN = 0.4 → 👉 least polar or almost non polar.⚡C–N: ΔEN = 0.5 → slightly polar and more polar than C–H.⚡C–Cl: ΔEN = 0.5 → polar, with partial negative charge on Cl.⚡C–O: ΔEN = 1.0 → highly polar. ✨ Advanced Concept for MDCAT: ⚡Polarity trend: C–O > C–Cl ≈ C–N > C–H. ⚡C–H bonds are often treated as non polar in organic chemistry because ΔEN is very small. This explains why hydrocarbons are generally non polar molecules despite having covalent bonds.
🔎 Polarity depends on ΔEN (electronegativity difference): Greater ΔEN → more polar bond. Smaller ΔEN → less polar bond.⚡C–H: ΔEN = 0.4 → 👉 least polar or almost non polar.⚡C–N: ΔEN = 0.5 → slightly polar and more polar than C–H.⚡C–Cl: ΔEN = 0.5 → polar, with partial negative charge on Cl.⚡C–O: ΔEN = 1.0 → highly polar. ✨ Advanced Concept for MDCAT: ⚡Polarity trend: C–O > C–Cl ≈ C–N > C–H. ⚡C–H bonds are often treated as non polar in organic chemistry because ΔEN is very small. This explains why hydrocarbons are generally non polar molecules despite having covalent bonds.
21. Two elements, X and Y, have outermost shells containing two and six electrons respectively. When they combine:
a) The expected formula is XY, with purely covalent bonding.
b) The expected formula is XY₂, with X forming sp hybridization.
c) The expected formula is XY, with ionic bonding between X²⁺ and Y²⁻.
d) The expected formula is X₂Y₃, with mixed ionic and covalent character.
✅ Correct Answer: (c)
Since element X has only two valence electrons, it likely to be a metallic element of group IIA (alkaline earth metals) which are divalent and tend lose two electrons to form divalent cation(X²⁺) and element Y has six valence electrons, it must be a non-metallic element of group VIA (chalcogens) which is bivalent and needs two electrons to complete its octet forming bivalent anion (Y²⁻). Hence the compound formed between X and Y must have formula of the type AB i.e. XY (X²⁺ and Y²⁻ balance charges in a 1:1 ratio). The bond is predominantly ionic because of the large electronegativity difference between a Group 2 metal and a Group 16 non metal.
Since element X has only two valence electrons, it likely to be a metallic element of group IIA (alkaline earth metals) which are divalent and tend lose two electrons to form divalent cation(X²⁺) and element Y has six valence electrons, it must be a non-metallic element of group VIA (chalcogens) which is bivalent and needs two electrons to complete its octet forming bivalent anion (Y²⁻). Hence the compound formed between X and Y must have formula of the type AB i.e. XY (X²⁺ and Y²⁻ balance charges in a 1:1 ratio). The bond is predominantly ionic because of the large electronegativity difference between a Group 2 metal and a Group 16 non metal.
22. In the N₂ molecule, the two nitrogen atoms are linked through a triple bond. Which of the following statements correctly describes the bonding electrons and bond characteristics?
a) N₂ has a bond order of 2, with 4 electrons shared in covalent bonding.
b) N₂ has a bond order of 3, with 6 electrons shared in covalent bonding, and sp hybridization of orbitals.
c) N₂ has a bond order of 3, with 10 electrons shared in covalent bonding, including lone pairs.
d) N₂ has a bond order of 4, with 8 electrons shared in covalent bonding, indicating a quadruple bond.
✅ Correct Answer: (b)
N₂ has a triple bond → bond order = 3.Triple bond = 1 sigma + 2 pi bonds. Each bond involves 2 electrons → total 6 electrons used in covalent bonding. Each nitrogen atom undergoes sp hybridization to form the sigma bond. Lone pairs are not counted in covalent bonding electrons → option (c) is a trap.Quadruple bonds (option d) do not exist in N₂ → incorrect.
N₂ has a triple bond → bond order = 3.Triple bond = 1 sigma + 2 pi bonds. Each bond involves 2 electrons → total 6 electrons used in covalent bonding. Each nitrogen atom undergoes sp hybridization to form the sigma bond. Lone pairs are not counted in covalent bonding electrons → option (c) is a trap.Quadruple bonds (option d) do not exist in N₂ → incorrect.
23. Which of the following has maximum ionic character?
a) LiCl
b) KCl
c) CsCl
d) NaCl
✅ Correct Answer: (c)
According to the Fajan's rule, smaller the cation, bigger the anion, more is the covalent character. On the other hand, bigger cation, in the given case Cs⁺, will favor ionic character, as the anion is same for all. Here, Cs⁺ is the biggest cation. Hence, CsCl will have maximum ionic character.
According to the Fajan's rule, smaller the cation, bigger the anion, more is the covalent character. On the other hand, bigger cation, in the given case Cs⁺, will favor ionic character, as the anion is same for all. Here, Cs⁺ is the biggest cation. Hence, CsCl will have maximum ionic character.
24. Which of the following have same number of electrons in the outermost orbit?
a) Pb, Sb
b) As, Bi
c) N, O
d) P, Ca
✅ Correct Answer: (b)
Elements of same group have same number of electrons in their outermost shell. As and Bi are the members of group VA and both have 5 valence electrons.
Elements of same group have same number of electrons in their outermost shell. As and Bi are the members of group VA and both have 5 valence electrons.
25. Which of the following pairs of elements and valence electrons is INCORRECT?
a) Al = 3
b) Br = 7
c) S = 4
d) Sr = 2
✅ Correct Answer: (c)
Group number of an element represent its valence electrons. Sulphur being a member of group VIA should contain 6 valence electrons not 4.
Group number of an element represent its valence electrons. Sulphur being a member of group VIA should contain 6 valence electrons not 4.
26. Which of the following does not have a noble gas electron configuration? (or Which of the following is NOT isoelectronic with a noble gas?)
a) S²⁻
b) Ba⁺
c) Sb³⁻
d) Sc³⁺
✅ Correct Answer: (b)
Ba⁺ contains only 55 electrons (not 54) and it does not have a noble gas electronic configuration.
Ba⁺ contains only 55 electrons (not 54) and it does not have a noble gas electronic configuration.
27. In the Lewis structure for the OF₂ molecule, the number of lone pairs of electrons around the central oxygen atom is
a) 0
b) 3
c) 1
d) 2
✅ Correct Answer: (d)
The number of lone pairs of electrons around the central atom of group VA (N, P, etc.) = 1. The number of lone pairs of electrons around the central atom of group VIA (O, S, etc.) = 2. The number of lone pairs of electrons around the central atom of group VIIA (F, Cl, etc.) = 3
The number of lone pairs of electrons around the central atom of group VA (N, P, etc.) = 1. The number of lone pairs of electrons around the central atom of group VIA (O, S, etc.) = 2. The number of lone pairs of electrons around the central atom of group VIIA (F, Cl, etc.) = 3
28. Which one of the following violates the octet rule?
a) PCl₃
b) NF₃
c) AsF₅
d) OF₂
✅ Correct Answer: (c)
Elements of group VA like N, P, As etc. violate the octet rule when they show their highest oxidation state of +5 forming AB₅ type like compounds. AsF₅ violates the octet rule having 10 electrons around central As atom.
Elements of group VA like N, P, As etc. violate the octet rule when they show their highest oxidation state of +5 forming AB₅ type like compounds. AsF₅ violates the octet rule having 10 electrons around central As atom.
29. Which one of the following species contains a polar covalent bond?
a) Carbon dioxide
b) Magnesium fluoride
c) Sodium chloride
d) Oxygen
✅ Correct Answer: (a)
(a) Carbon dioxide (CO₂): Each C=O bond is polar covalent (due to electronegativity difference between C and O). However, the molecule overall is nonpolar because of its linear symmetry. But the question asks about bond, not whole molecule → so polar covalent bond exists. Thus, only CO₂ contains polar covalent bonds (even though the overall molecule is non-polar due to symmetry).(b) Magnesium fluoride (MgF₂): This is an ionic compound, not covalent. (c) Sodium chloride (NaCl): Also ionic, not covalent. (d) Oxygen (O₂): Both atoms same → nonpolar covalent bond.
(a) Carbon dioxide (CO₂): Each C=O bond is polar covalent (due to electronegativity difference between C and O). However, the molecule overall is nonpolar because of its linear symmetry. But the question asks about bond, not whole molecule → so polar covalent bond exists. Thus, only CO₂ contains polar covalent bonds (even though the overall molecule is non-polar due to symmetry).(b) Magnesium fluoride (MgF₂): This is an ionic compound, not covalent. (c) Sodium chloride (NaCl): Also ionic, not covalent. (d) Oxygen (O₂): Both atoms same → nonpolar covalent bond.
30. Which of the following ions has a pseudo-noble-gas electron configuration?
a) Fe²⁺
b) Cu⁺
c) Mn²⁺
d) Ni⁺
✅ Correct Answer: (b)
An element with pseudo noble gas configuration has 18 electrons in the outermost shell instead of 8. EC of Cu⁺ = [Ar], 3d¹⁰ (pseudo inert gas configuration).
An element with pseudo noble gas configuration has 18 electrons in the outermost shell instead of 8. EC of Cu⁺ = [Ar], 3d¹⁰ (pseudo inert gas configuration).
Your Score: 0 / 0
💥 غزل جونؔ ایلیا 💥
🌌 نہ ہوا نصیب قرار جاں ہوسِ قرار بھی اب نہیں
💔 تیرا انتظار بہت کیا تیرا انتظار بھی اب نہیں
💔 تیرا انتظار بہت کیا تیرا انتظار بھی اب نہیں
📜 تجھے کیا خبر مہ و سال نے ہمیں کیسے زخم دئیے یہاں
🖋️ تیری یادگار تھی اک خلش تیری یادگار بھی اب نہیں
🖋️ تیری یادگار تھی اک خلش تیری یادگار بھی اب نہیں
🗣️ نہ گلے رہے نہ گماں رہے گزارشیں ہیں نہ گفتگو
⚡ وہ نشاطِ وعدہ وصل کیا ہمیں اعتبار بھی اب نہیں
⚡ وہ نشاطِ وعدہ وصل کیا ہمیں اعتبار بھی اب نہیں
❤️ کسے نذر دیں دل و جاں بہم کہ وہ نہیں کا کلِ خم بہ خم
🌹 کسے ہر نفس کا حساب دیں کہ شمیمِ یار بھی اب نہیں
🌹 کسے ہر نفس کا حساب دیں کہ شمیمِ یار بھی اب نہیں
🌙 وہ جو اپنی جاں سے گزر گئے انہیں کیا خبر ہے کہ شہر میں
🕊️ کسی جاں نثار کا ذکر کیا کوئی سوگوار بھی اب نہیں
🕊️ کسی جاں نثار کا ذکر کیا کوئی سوگوار بھی اب نہیں
🌪️ وہ ہجومِ دل زدگاں کہ تھا، تجھے مژدہ ہو کہ بکھر گیا
🏠 ترے آستانے کی خیر ہو، سرِ رہ غبار بھی اب نہیں
🏠 ترے آستانے کی خیر ہو، سرِ رہ غبار بھی اب نہیں
🔥 نہیں اب تو اہل جنوں میں بھی وہ جو شوق شہر میں عام تھا
🌈 وہ جو رنگ تھا کبھی کو بہ کو سر کوئے یار بھی اب نہیں
🌈 وہ جو رنگ تھا کبھی کو بہ کو سر کوئے یار بھی اب نہیں
💭 رہے نام رشتئہ رفتگاں نہ شکایتیں ہیں نہ شوخیاں
🤝 کوئی عذر خواہ تو اب کہاں کوئی عذر دار بھی اب نہیں
🤝 کوئی عذر خواہ تو اب کہاں کوئی عذر دار بھی اب نہیں
Tags
Aptitude test (MDCAT/ECAT)
First year
High-Yield Chemical Bonding MCQs
MDCAT ECAT Chemical Bonding
MDCAT ECAT FSC Chemistry Chemical Bonding Quiz