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🔷🔥Chemical Bonding MCQs for MDCAT, ECAT & FSC: Your Ultimate Practice Guide! Quiz # 1🧪✨
1️⃣ The highest bond energy in the following is:
🟨 A Cl–Cl
🟩 B H–O
🟦 C H–F
🟪 D H–N
2️⃣ The molecule which has zero dipole moment is:
🟨 A NH₃
🟩 B HCl
🟦 C CCl₄
🟪 D H₂O
3️⃣ The correct relation between Debye and coulomb meter is:
🟨 A 1 D = 3.33 × 10⁻³⁰ C·m
🟩 B 1 D = 1.6 × 10⁻¹⁹ C·m
🟦 C 1 D = 1.88 × 10⁻¹² C·m
🟪 D 1 D = 1.23 × 10⁻⁸ C·m
4️⃣ Octet rule is not followed in the formation of:
🟨 A CH₄
🟩 B BCl₃
🟦 C NF₃
🟪 D CO₂
5️⃣ Which factor is not responsible for the formation of ionic bond?
🟨 A Crystal lattice energy
🟩 B Ionization enthalpy
🟦 C Electron affinity
🟪 D Density
6️⃣ Which of the following compound possesses covalent bond?
🟨 A MgCl₂
🟩 B BF₃
🟦 C NaH
🟪 D CsCl
7️⃣ Which of the following molecule has not zero dipole moment?
🟨 A SO₂
🟩 B CO₂
🟦 C BF₃
🟪 D BeF₂
8️⃣ Maximum how many numbers of hydrogen bond can be formed by H₂O molecule?
🟨 A 2
🟩 B 3
🟦 C 4
🟪 D 1
9️⃣ Which of the following has co-ordinate covalent bond?
🟨 A NH₄⁺
🟩 B H₂O
🟦 C H₃O⁺
🟪 D Both A and C
1️⃣0️⃣ Which of the following has the highest bond energy?
🟨 A C₂H₂
🟩 B C₂H₄
🟦 C C₂H₆
🟪 D C₂H₅OH
1️⃣1️⃣ Which one of the following bond has the most polar character?
🟨 A C–O
🟩 B C–Br
🟦 C C–F
🟪 D C–S
1️⃣2️⃣ Generally an ionic bond is formed between elements of group:
🟨 A IA and VIIA
🟩 B IIIA and VIIA
🟦 C VA and VIIA
🟪 D None of them
1️⃣3️⃣ Chemical bond formation takes place due to interaction of ……… electrons.
🟨 A Valence
🟩 B Inner
🟦 C Free
🟪 D Paired
1️⃣4️⃣Which molecule does not have single covalent bond?
🟨 A O₂
🟩 B N₂
🟦 C CCl₄
🟪 D HF
1️⃣5️⃣ Which molecule has single covalent bond?
🟨 A O₂
🟩 B N₂
🟦 C C₂H₂
🟪 D None of them
1️⃣6️⃣ Which one is incorrect regarding the examples of Non-Polar bond?
🟨 A S=C=S
🟩 B PH₃
🟦 C CH₄
🟪 D CH₃Cl
1️⃣7️⃣ Which molecule contains three shared pairs of electrons between two of its atoms?
🟨 A N₂
🟩 B C₂H₄
🟦 C CO₂
🟪 D H₂O
1️⃣8️⃣ Which of the following is ionic?
🟨 A HCl
🟩 B CHCl₃
🟦 C KI
🟪 D IF₅
1️⃣9️⃣ In which molecule intra molecular hydrogen bond can be formed?
🟨 A o-nitro phenol
🟩 B Aniline
🟦 C Ethylene glycol
🟪 D All of these
2️⃣0️⃣ How many core electrons does a fluorine (F) atom contain?
🟨 A 2
🟩 B 5
🟦 C 7
🟪 D 10
2️⃣1️⃣ The degree or extent of polarity of a molecule is called:
🟨 A Bond energy
🟩 B Moment arm
🟦 C Dipole moment
🟪 D Ionic character
2️⃣2️⃣The one sided sharing of electrons b/w two atoms produces which type of bond?
🟨 A Covalent bond
🟩 B Hydrogen bond
🟦 C Dative bond
🟪 D Ionic bond
2️⃣3️⃣ Which of the following has the shortest C–C bond length?
🟨 A C₂H₂
🟩 B C₂H₄
🟦 C C₂H₆
🟪 D C₂H₅OH
2️⃣4️⃣ Which molecule has single covalent bond?
🟨 A O₂
🟩 B CH₄
🟦 C CO₂
🟪 D N₂
2️⃣5️⃣ Which molecule has double covalent bond?
🟨 A HF
🟩 B N₂
🟦 C CCl₄
🟪 D O₂
2️⃣6️⃣ Bond making is always:
🟨 A Endothermic
🟩 B Exothermic
🟦 C Both A and B
🟪 D None of them
2️⃣7️⃣ A covalent bond in which the shared electron pair is attracted equally by the two atoms is called:
🟨 A Polar bond
🟩 B Non-Polar bond
🟦 C Dative bond
🟪 D Hydrogen bond
2️⃣8️⃣ Which molecule has greater bond energy?
🟨 A Polar molecule
🟩 B Non-Polar molecule
🟦 C None of them
🟪 D All of them
2️⃣9️⃣ A bond is said to be 100% covalent, if it exists between atoms of:
🟨 A Same elements
🟩 B Different elements
🟦 C Same group
🟪 D Different group
3️⃣0️⃣ Which one of the following bond has the least polar character?
🟨 A C–H
🟩 B C–Cl
🟦 C C–O
🟪 D C–N
3️⃣1️⃣ Which one of the following has zero dipole moments?
🟨 A Diatomic polar molecules
🟩 B Non-linear (bent) polyatomic molecules
🟦 C Polyatomic polar symmetrical molecules
🟪 D Polyatomic polar unsymmetrical molecules
3️⃣2️⃣ The b.p of water is higher than H₂S because:
🟨 A It has ionic bonding
🟩 B Water can form 3D hydrogen bonding of varying length
🟦 C Water is non-polar
🟪 D None of the above
3️⃣3️⃣ In which one of the following does ionic bonding occur between the named atoms?
🟨 A Silicon and chlorine in silicon tetrachloride
🟩 B Hydrogen and aluminium in aluminum hydride
🟦 C Cesium and fluorine in cesium fluoride
🟪 D Iron and chlorine in tetrachloroferrate ion
3️⃣4️⃣ Which equation defines the lattice energy of the ionic compound XY?
🟨 A X(s) + Y(s) → XY(s)
🟩 B X⁺(s) + Y⁻(s) → XY(s)
🟦 C X(g) + Y(g) → XY(s)
🟪 D X⁺(g) + Y⁻(g) → XY(s)
3️⃣5️⃣ In order to form a compound with oxygen, an atom of a Group II element must:
🟨 A Transfer two electrons to an atom of oxygen
🟩 B Receive two electrons from an atom of oxygen
🟦 C Share two electrons with an atom of oxygen
🟪 D Bond with two atoms of oxygen
3️⃣6️⃣ Which of the following relation is correct?
🟨 A Bond order ∝ bond energy ∝ bond length ∝ stability
🟩 B Bond order ∝ bond energy ∝ 1/bond length ∝ stability
🟦 C Bond order ∝ 1/bond length ∝ 1/bond energy ∝ stability
🟪 D Bond order ∝ bond energy ∝ bond length ∝ 1/stability
3️⃣7️⃣ What is formed when an element X of atomic number 19 reacts with an element Y of atomic number 17?
🟨 A A covalent compound of formula XY₂
🟩 B A covalent compound of formula XY
🟦 C An ionic compound of formula XY
🟪 D An ionic compound of formula X₂Y
3️⃣8️⃣ Which one has zero dipole moment?
🟨 A Linear polyatomic polar molecule
🟩 B Diatomic polar molecule
🟦 C Non-linear (angular) polyatomic polar molecule
🟪 D None of the above
3️⃣9️⃣ Element X and Y combine to form the gas XY₂. What are X and Y?
🟨 A Calcium & Chlorine
🟩 B Carbon & Hydrogen
🟦 C Carbon & Oxygen
🟪 D Hydrogen & Oxygen
✅Answers of Chemical Bonding MCQs for MDCAT, ECAT & FSC: Your Ultimate Practice Guide! Quiz # 1🧪✨
🟦1️⃣C 🟦 H–F
🟦2️⃣C 🟦 CCl₄
🟦3️⃣A 🟨 1 D = 3.33 × 10⁻³⁰ C·m
🟦4️⃣B 🟩 BCl₃
🟦5️⃣D 🟪 Density
🟦6️⃣B 🟩 BF₃
🟦7️⃣A 🟨 SO₂
🟦8️⃣C 🟦 4
🟦9️⃣D 🟪 Both A and C
1️⃣0️⃣A 🟨 C₂H₂
1️⃣1️⃣C 🟦 C–F
1️⃣2️⃣A 🟨 IA and VIIA
1️⃣3️⃣A 🟨 Valence
1️⃣4️⃣B 🟩 N₂
1️⃣5️⃣D 🟪 None of them
1️⃣6️⃣D 🟪 CH₃Cl
1️⃣7️⃣A 🟨 N₂
1️⃣8️⃣C 🟦 KI
1️⃣9️⃣D 🟪 All of these
2️⃣0️⃣A 🟨 2
2️⃣1️⃣C 🟦 Dipole moment
2️⃣2️⃣C 🟦 Dative bond
2️⃣3️⃣A 🟨 C₂H₂
2️⃣4️⃣B 🟩 CH₄
2️⃣5️⃣B 🟩 N₂
2️⃣6️⃣B 🟩 Exothermic
2️⃣7️⃣B 🟩 Non-Polar bond
2️⃣8️⃣B 🟩 Non-Polar molecule
2️⃣9️⃣A 🟨 Same elements
3️⃣0️⃣ A🟨 C–H
3️⃣1️⃣ C🟦 Polyatomic polar symmetrical molecules
3️⃣2️⃣B🟩Water can form 3D hydrogen bonding of varying length
3️⃣3️⃣ C🟦 Cesium and fluorine
3️⃣4️⃣ D🟪 X⁺(g) + Y⁻(g) → XY(s)
3️⃣5️⃣ A🟨 Transfer two electrons to an atom of oxygen
3️⃣6️⃣B 🟨Bond order ∝ bond energy ∝ 1/bond length ∝ stability
3️⃣7️⃣ C🟦 An ionic compound of formula XY
3️⃣8️⃣ A🟪 Linear polyatomic polar molecule
3️⃣9️⃣D 🟨 Hydrogen & Oxygen
🔷🔥Chemical Bonding MCQs for MDCAT, ECAT & FSC: Your Ultimate Practice Guide! Quiz # 2🧪
1️⃣ If the bond angle in AB₂ type molecule is 104.5°, its geometry should be:
🟨 A Linear
🟩 B Pyramidal
🟦 C Bent
🟪 D Planar Trigonal
2️⃣ The molecule which has maximum bond angle:
🟨 A CS₂
🟩 B H₂O
🟦 C NH₃
🟪 D BF₃
3️⃣ The shape and hybridization of BCl₃ molecule is:
🟨 A Tetrahedral & sp³
🟩 B Linear & sp
🟦 C Planar trigonal & sp²
🟪 D Angular & sp³
4️⃣ Among the following molecules which has trigonal pyramidal shape?
🟨 A SO₂
🟩 B CO₂
🟦 C NH₃
🟪 D C₂H₄
5️⃣ A simple covalent molecule with 2 bond pairs and 2 lone pairs around central atom, its shape is:
🟨 A Linear
🟩 B Planar trigonal
🟦 C Angular
🟪 D Tetrahedral
6️⃣ The bond order of N₂ molecule is:
🟨 A 3
🟩 B 1
🟦 C 2
🟪 D 0
7️⃣ The number of sigma and pi bonds in C₂H₄ molecules are respectively:
🟨 A 5 & 1
🟩 B 2 & 2
🟦 C 3 & 1
🟪 D 4 & 2
8️⃣ The molecular orbitals which have higher energy than parent atomic orbitals are called:
🟨 A BMO
🟩 B Hybrid orbital
🟦 C AMO
🟪 D All of them
9️⃣ Sigma bond has ……….. electron density:
🟨 A Highest
🟩 B Lowest
🟦 C Intermediate
🟪 D All of them
🔟 A molecule of acetylene (C₂H₂) contains total:
🟨 A 2 σ & 2 π bonds
🟩 B 4 σ & 1 π bond
🟦 C 3 σ & 3 π bonds
🟪 D 5 σ & no π bond
1️⃣1️⃣ Inter-electronic repulsion forces decrease sharply with increasing:
🟨 A Bond angle
🟩 B Bond length
🟦 C Bond energy
🟪 D All of them
1️⃣2️⃣ Benzene has bond angles same as:
🟨 A Tetrahedral geometry
🟩 B Linear geometry
🟦 C Triangular geometry
🟪 D None of these
1️⃣3️⃣ Which one pair has same type of hybridization of central atom?
🟨 A BF₃, SO₃
🟩 B BF₃, NH₃
🟦 C CH₃⁺, BF₃
🟪 D H₂S, SO₂
1️⃣4️⃣ How many sigma bonds can be predicted between two atoms?
🟨 A 3
🟩 B 1
🟦 C 2
🟪 D 4
1️⃣5️⃣ The presence of lone pair on the central atom ………… bond angle:
🟨 A Contract
🟩 B Expand
🟦 C Has no effect
🟪 D All of them
1️⃣6️⃣ Which of the following has pyramidal shape?
🟨 A NH₃
🟩 B PH₃
🟦 C PCl₃
🟪 D All of them
1️⃣7️⃣ The shape of NHCl₂ molecule is:
🟨 A Tetrahedral
🟩 B Angular
🟦 C Planar Trigonal
🟪 D Linear
1️⃣8️⃣ Bond length is largest in case of ………. overlapping:
🟨 A sp²-s
🟩 B sp²-sp²
🟦 C sp³-sp³
🟪 D sp-sp
1️⃣9️⃣ In CH₄ molecule, a sigma bond is formed by axial overlapping of half-filled:
🟨 A s-s orbitals
🟩 B s-sp³ orbitals
🟦 C d-d orbitals
🟪 D p-p orbitals
2️⃣0️⃣ Strongest bond is formed by the overlap of:
🟨 A s-s orbitals
🟩 B p-p orbitals
🟦 C s and p orbitals
🟪 D None of them
2️⃣1️⃣ In which molecule carbon atom is sp³ hybridized?
🟨 A C₂H₂
🟩 B C₂H₆
🟦 C C₃H₆
🟪 D C₂H₄
2️⃣2️⃣ A molecule of ethylene (C₂H₄) contains total:
🟨 A 2 σ & 1 π bond
🟩 B 5 σ & 1 π bond
🟦 C 4 σ & 2 π bond
🟪 D 3 σ & 1 π bond
2️⃣3️⃣ In which of the following strong H-bond is present?
🟨 A F-H…F
🟩 B O-H…O
🟦 C O-H…N
🟪 D O-H…F
2️⃣4️⃣ What is bond energy of H-bond?
🟨 A 40 J mol⁻¹
🟩 B 40 kJ mol⁻¹
🟦 C 40 kg J mol⁻¹
🟪 D 40 cal mol⁻¹
2️⃣5️⃣ In OF₂, number of bond pairs and lone pairs of electrons are respectively:
🟨 A 2, 8
🟩 B 2, 9
🟦 C 2, 8
🟪 D 2, 10
2️⃣6️⃣ The shape of CO₂ molecule is similar to:
🟨 A H₂S
🟩 B SnCl₂
🟦 C SO₂
🟪 D BeF₂
2️⃣7️⃣ How many core electrons does a Sulfur (S) atom contain?
🟨 A 4
🟩 B 6
🟦 C 8
🟪 D 10
2️⃣8️⃣ Which one of the following ions has more electrons than protons and more protons than neutrons?
🟨 A D⁻
🟩 B D₃O⁺
🟦 C OD⁻
🟪 D OH⁻
2️⃣9️⃣ Which one has the same number of electrons as an alpha particle?
🟨 A H
🟩 B H⁺
🟦 C He
🟪 D Li⁺
3️⃣0️⃣ Which one does not contain delocalized electrons?
🟨 A Copper
🟩 B Benzene
🟦 C Diamond
🟪 D Graphite
3️⃣1️⃣ Which one conducts electricity by movement of ions?
🟨 A Copper metal
🟩 B Mercury
🟦 C Molten sodium chloride
🟪 D Graphite
3️⃣2️⃣ The molecular orbitals which have higher energy than parent atomic orbital are called:
🟨 A BMO
🟩 B Hybrid orbital
🟦 C AMO
🟪 D All of them
3️⃣3️⃣ Sigma bond has ……….. electron density:
🟨 A Highest
🟩 B Lowest
🟦 C Intermediate
🟪 D All of them
3️⃣4️⃣ A molecule of acetylene (C₂H₂) contains total:
🟨 A 2 σ & 2 π bonds
🟩 B 4 σ & 1 π bond
🟦 C 3 σ & 3 π bonds
🟪 D 5 σ & no π bond
3️⃣5️⃣ Inter-electronic repulsion forces decrease sharply with increasing:
🟨 A Bond angle
🟩 B Bond length
🟦 C Bond energy
🟪 D All of them
3️⃣6️⃣ Benzene has bond angles same as:
🟨 A Tetrahedral geometry
🟩 B Linear geometry
🟦 C Triangular geometry
🟪 D None of these
3️⃣7️⃣ Which one pair has same type of hybridization of central atom?
🟨 A BF₃, SO₃
🟩 B BF₃, NH₃
🟦 C CH₃⁺, BF₃
🟪 D H₂S, SO₂
3️⃣8️⃣ In O₂, each oxygen atom is …………. Hybridized.
🟨 A sp²
🟩 B sp³
🟦 C sp
🟪 D None of them
3️⃣9️⃣ How many sigma bonds can be predicted between two atoms?
🟨 A 3
🟩 B 1
🟦 C 2
🟪 D 4
4️⃣0️⃣ The presence of lone pair on the central atom ………… bond angle:
🟨 A Contract
🟩 B Expand
🟦 C Has no effect
🟪 D All of them
4️⃣1️⃣ Which of the following has pyramidal shape?
🟨 A NH₃
🟩 B PH₃
🟦 C PCl₃
🟪 D All of them
4️⃣2️⃣ The shape of NHCl₂ molecule is:
🟨 A Tetrahedral
🟩 B Angular
🟦 C Planar Trigonal
🟪 D Linear
4️⃣3️⃣ Bond length is largest in case of ………. overlapping:
🟨 A sp²-s
🟩 B sp²-sp²
🟦 C sp³-sp³
🟪 D sp-sp
4️⃣4️⃣ In CH₄ molecule a sigma bond is formed by axial overlapping of half filled:
🟨 A s-s orbitals
🟩 B s-sp³ orbitals
🟦 C d-d orbitals
🟪 D p-p orbitals
4️⃣5️⃣ Strongest bond is formed by the overlap of:
🟨 A s-s orbitals
🟩 B p-p orbitals
🟦 C s and p orbitals
🟪 D None of them
4️⃣6️⃣ In which molecule carbon atom is sp³ hybridized?
🟨 A C₂H₂
🟩 B C₂H₆
🟦 C C₃H₆
🟪 D C₂H₄
4️⃣7️⃣ A molecule of ethylene (C₂H₄) contains total:
🟨 A 2 σ & 1 π bond
🟩 B 5 σ & 1 π bond
🟦 C 4 σ & 2 π bond
🟪 D 3 σ & 1 π bond
4️⃣8️⃣ In OF₂, number of bond pairs and lone pairs of electrons are respectively:
🟨 A 2, 8
🟩 B 2, 9
🟦 C 2, 8
🟪 D 2, 10
4️⃣9️⃣ The shape of CO₂ molecule is similar to:
🟨 A H₂S
🟩 B SnCl₂
🟦 C SO₂
🟪 D BeF₂
✅Answers of Chemical Bonding MCQs for MDCAT, ECAT & FSC: Your Ultimate Practice Guide! Quiz # 2🧪✨
🟦1️⃣ 🟦 C Bent
🟦2️⃣ 🟪 D BF₃
🟦3️⃣ 🟦 C Planar trigonal & sp²
🟦4️⃣ 🟦 C NH₃
🟦5️⃣ 🟦 C Angular
🟦6️⃣ 🟨 A 3
🟦7️⃣ 🟨 A 5 & 1
🟦8️⃣ 🟩 B Hybrid orbital
🟦9️⃣ 🟨 A Highest
1️⃣0️⃣ 🟨 A 2 σ & 2 Ï€ bonds
1️⃣1️⃣ 🟩 B Bond length
1️⃣2️⃣ 🟨 C Triangular geometry
1️⃣3️⃣ 🟨 A BF₃, SO₃
1️⃣4️⃣ 🟩 B 1
1️⃣5️⃣ 🟨 A Contract
1️⃣6️⃣ 🟪 D All of them
1️⃣7️⃣ 🟩 B Angular
1️⃣8️⃣ 🟦 C sp³-sp³
1️⃣9️⃣ 🟩 B s-sp³ orbitals
2️⃣0️⃣ 🟩 B p-p orbitals
2️⃣1️⃣ 🟩 B C₂H₆
2️⃣2️⃣ 🟦 C 4 σ & 2 Ï€ bond
2️⃣3️⃣ 🟩 B O-H…O
2️⃣4️⃣ 🟩 B 40 kJ mol⁻¹
2️⃣5️⃣ 🟪 D 2, 10
2️⃣6️⃣ 🟪 D BeF₂
2️⃣7️⃣ 🟦 C 8
2️⃣8️⃣ 🟨 A D⁻
2️⃣9️⃣ 🟦 C He
3️⃣0️⃣ 🟨 A Copper
3️⃣1️⃣ 🟦 C Molten sodium chloride
3️⃣2️⃣ 🟩 B Hybrid orbital
3️⃣3️⃣ 🟨 A Highest
3️⃣4️⃣ 🟨 A 2 σ & 2 Ï€ bonds
3️⃣5️⃣ 🟩 B Bond length
3️⃣6️⃣ 🟨 A Tetrahedral geometry
3️⃣7️⃣ 🟨 A BF₃, SO₃
3️⃣8️⃣ 🟦 A sp²
3️⃣9️⃣ 🟩 B 1
4️⃣0️⃣ 🟨 A Contract
4️⃣1️⃣ 🟪 D All of them
4️⃣2️⃣ 🟩 B Angular
4️⃣3️⃣ 🟦 C sp³-sp³
4️⃣4️⃣ 🟩 B s-sp³ orbitals
4️⃣5️⃣ 🟩 B p-p orbitals
4️⃣6️⃣ 🟩 B C₂H₆
4️⃣7️⃣ 🟦 C 4 σ & 2 Ï€ bond
4️⃣8️⃣ 🟪 D 2, 10
4️⃣9️⃣ 🟪 D BeF₂
🔷🔥Chemical Bonding VSEPR Theory MCQs for MDCAT, ECAT & FSC: Your Ultimate Practice Guide! Quiz # 3🧪
1️⃣ Electron-pair geometry of CO₂ is:
🟥 A. Bent
🟦 B. Linear
🟩 C. Trigonal planar
🟨 D. Tetrahedral
2️⃣ Shape of SO₂ according to VSEPR:
🟥 A. Linear
🟦 B. Bent
🟩 C. Trigonal planar
🟨 D. Pyramidal
3️⃣ H₂O has bond angle less than 109.5° because:
🟥 A. Double bonds
🟦 B. Two lone pairs
🟩 C. More electronegativity
🟨 D. Four bonding pairs
4️⃣ NH₃ has which shape?
🟥 A. Bent
🟦 B. Trigonal planar
🟩 C. Trigonal pyramidal
🟨 D. Linear
5️⃣ Electron domains in BF₃:
🟥 A. Two
🟦 B. Three
🟩 C. Four
🟨 D. Five
6️⃣ Shape of PCl₅ according to VSEPR:
🟥 A. Tetrahedral
🟦 B. Trigonal bipyramidal
🟩 C. Octahedral
🟨 D. Square pyramidal
7️⃣ SF₆ has geometry:
🟥 A. Square planar
🟦 B. Trigonal bipyramidal
🟩 C. Octahedral
🟨 D. T-shaped
8️⃣ Lone pairs always prefer which position in 5-electron pair geometry?
🟥 A. Axial
🟦 B. Equatorial
🟩 C. Random
🟨 D. Peripheral
9️⃣ Shape of XeF₂ is:
🟥 A. Linear
🟦 B. Bent
🟩 C. See-saw
🟨 D. T-shaped
🔟 Electron-pair geometry of NH₄⁺:
🟥 A. Tetrahedral
🟦 B. Trigonal planar
🟩 C. Linear
🟨 D. Octahedral
1️⃣1️⃣ Shape of CH₄ is:
🟥 A. Trigonal pyramidal
🟦 B. Tetrahedral
🟩 C. Trigonal planar
🟨 D. Bent
1️⃣2️⃣ Which has maximum bond angle?
🟥 A. H₂O
🟦 B. NH₃
🟩 C. BF₃
🟨 D. CH₄
1️⃣3️⃣ NO₂⁻ has shape:
🟥 A. Bent
🟦 B. Linear
🟩 C. T-shaped
🟨 D. Pyramidal
1️⃣4️⃣ A molecule with 4 bonding pairs and 0 lone pairs is:
🟥 A. Linear
🟦 B. Tetrahedral
🟩 C. Bent
🟨 D. Square planar
1️⃣5️⃣ Regions of electron density in CO₃²⁻ are:
🟥 A. Four
🟦 B. Two
🟩 C. Three
🟨 D. Five
1️⃣6️⃣ Which molecule is see-saw shaped?
🟥 A. SF₄
🟦 B. SF₆
🟩 C. CO₂
🟨 D. NH₃
1️⃣7️⃣ Which has T-shaped geometry?
🟥 A. BrF₃
🟦 B. BF₃
🟩 C. NH₄⁺
🟨 D. CO₂
1️⃣8️⃣ A molecule with one lone pair and three bonding pairs is:
🟥 A. Linear
🟦 B. Bent
🟩 C. Trigonal pyramidal
🟨 D. Tetrahedral
1️⃣9️⃣ Central atom of XeF₄ is:
🟥 A. Trigonal planar
🟦 B. Octahedral
🟩 C. Square planar
🟨 D. Bent
2️⃣0️⃣ In VSEPR, double and triple bonds are counted as:
🟥 A. Two regions
🟦 B. Three regions
🟩 C. One region
🟨 D. Zero region
✅Answers of Chemical Bonding VSEPR Theory MCQs for MDCAT, ECAT & FSC: Your Ultimate Practice Guide! Quiz # 3🧪✨
🟦1️⃣🟦 B CO₂ → Linear Reason: Central C has 2 regions of electron density (2 double bonds), giving linear geometry.
🟦2️⃣🟦 B SO₂ → Bent Reason: Central S has 2 bonding pairs + 1 lone pair → bent shape.
🟦3️⃣🟦 BH₂O → Two lone pairs Reason: Lone pairs repel more strongly, reducing bond angle below 109.5°.
🟦4️⃣ 🟩 C NH₃ → Trigonal pyramidal Reason: 3 bonding pairs + 1 lone pair → pyramidal shape.
5️⃣ 🟦 B BF₃ → Three domains Reason: Central B has 3 bonding regions → trigonal planar electron geometry.
🟦6️⃣🟦 B PCl₅ → Trigonal bipyramidal Reason: 5 bonding pairs around P → trigonal bipyramidal geometry.
🟦7️⃣🟩 C Octahedral Reason: 6 bonding pairs around S → octahedral geometry.
🟦8️⃣🟦 B Lone pairs → Equatorial Reason: Lone pairs prefer equatorial positions in trigonal bipyramidal to minimize repulsion.
🟦9️⃣🟥 A XeF₂ → Linear Reason: 5 electron pairs (3 lone + 2 bonds) → linear arrangement.
1️⃣0️⃣🟥 A NH₄⁺ → Tetrahedral Reason: 4 bonding pairs, no lone pairs → tetrahedral geometry.
1️⃣1️⃣ 🟦 B CH₄ → Tetrahedral Reason: 4 bonding pairs around C → tetrahedral shape.
1️⃣2️⃣ 🟩 C BF₃ → Maximum bond angle Reason: Trigonal planar has 120°, larger than tetrahedral (109.5°) or bent/pyramidal (<109.5°).
1️⃣3️⃣ 🟥 A NO₂⁻ → Bent Reason: Central N has 2 bonds + 1 lone pair → bent geometry.
1️⃣4️⃣ 🟦 B 4 bonding pairs → Tetrahedral Reason: No lone pairs, 4 bonds → tetrahedral geometry.
1️⃣5️⃣ 🟩 C CO₃²⁻ → Three regions Reason: Resonance gives 3 equivalent bonds → trigonal planar electron geometry.
1️⃣6️⃣ 🟥 A SF₄ → See-saw Reason: 4 bonds + 1 lone pair in trigonal bipyramidal → see-saw shape.
1️⃣7️⃣ 🟥 A BrF₃ → T-shaped Reason: 3 bonds + 2 lone pairs in trigonal bipyramidal → T-shape.
1️⃣8️⃣ 🟩 C One lone + three bonds → Trigonal pyramidal Reason: Lone pair pushes bonds down → pyramidal geometry.
1️⃣9️⃣ 🟩 C XeF₄ → Square planar Reason: 4 bonds + 2 lone pairs in octahedral → square planar.
2️⃣0️⃣ 🟩 C Double/triple bonds → One region Reason: In VSEPR, multiple bonds count as a single electron domain.
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