Q. What is the hybridization of the central atom in NH4+?
A.
sp
B.
sp2
C.
sp3
D.
dsp3
Show solution
Solution
The central atom nitrogen in NH4+ undergoes sp3 hybridization to form four equivalent bonds with hydrogen.
Correct Answer:
C
— sp3
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Q. What is the hybridization of the central atom in O3 (ozone)?
A.
sp
B.
sp2
C.
sp3
D.
dsp2
Show solution
Solution
The central oxygen atom in O3 is sp2 hybridized, leading to a bent molecular shape.
Correct Answer:
B
— sp2
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Q. What is the hybridization of the central atom in ozone (O3)?
A.
sp
B.
sp2
C.
sp3
D.
dsp2
Show solution
Solution
In ozone (O3), the central oxygen atom is sp2 hybridized, resulting in a bent molecular shape.
Correct Answer:
B
— sp2
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Q. What is the hybridization of the central atom in PCl5?
A.
sp
B.
sp2
C.
sp3
D.
sp3d
Show solution
Solution
In PCl5, phosphorus is sp3d hybridized, allowing for five bonding pairs.
Correct Answer:
D
— sp3d
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Q. What is the hybridization of the central atom in SO2?
A.
sp
B.
sp2
C.
sp3
D.
dsp3
Show solution
Solution
The sulfur atom in SO2 is sp2 hybridized, forming one double bond and one single bond.
Correct Answer:
B
— sp2
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Q. What is the hybridization of the central atom in XeF4?
A.
sp
B.
sp2
C.
sp3
D.
dsp3
Show solution
Solution
The xenon atom in XeF4 is dsp3 hybridized, resulting in a square planar geometry.
Correct Answer:
D
— dsp3
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Q. What is the hybridization of the nitrogen atom in NH3?
A.
sp
B.
sp2
C.
sp3
D.
dsp3
Show solution
Solution
In NH3, nitrogen has three bonds and one lone pair, leading to sp3 hybridization.
Correct Answer:
C
— sp3
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Q. What is the hybridization of the phosphorus atom in PCl5?
A.
sp
B.
sp2
C.
sp3
D.
d2sp3
Show solution
Solution
In PCl5, phosphorus is surrounded by five chlorine atoms, indicating d2sp3 hybridization.
Correct Answer:
D
— d2sp3
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Q. What is the molecular geometry of ammonia (NH3)?
A.
Linear
B.
Trigonal planar
C.
Tetrahedral
D.
Trigonal pyramidal
Show solution
Solution
Ammonia has a trigonal pyramidal geometry due to the presence of a lone pair on nitrogen.
Correct Answer:
D
— Trigonal pyramidal
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Q. What is the molecular geometry of BF3 according to VSEPR theory?
A.
Trigonal planar
B.
Tetrahedral
C.
Octahedral
D.
Linear
Show solution
Solution
BF3 has three bonding pairs and no lone pairs, resulting in a trigonal planar geometry.
Correct Answer:
A
— Trigonal planar
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Q. What is the molecular geometry of BF3?
A.
Linear
B.
Trigonal planar
C.
Tetrahedral
D.
Bent
Show solution
Solution
BF3 has a trigonal planar geometry due to the three bonding pairs and no lone pairs on the central atom.
Correct Answer:
B
— Trigonal planar
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Q. What is the molecular geometry of CH4 according to VSEPR theory?
A.
Linear
B.
Trigonal planar
C.
Tetrahedral
D.
Octahedral
Show solution
Solution
According to VSEPR theory, CH4 has four bonding pairs and no lone pairs, resulting in a tetrahedral geometry.
Correct Answer:
C
— Tetrahedral
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Q. What is the molecular geometry of CH4?
A.
Linear
B.
Trigonal planar
C.
Tetrahedral
D.
Octahedral
Show solution
Solution
CH4 has a tetrahedral geometry due to four bonding pairs around the central carbon atom.
Correct Answer:
C
— Tetrahedral
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Q. What is the molecular geometry of NH3 according to VSEPR theory?
A.
Trigonal planar
B.
Tetrahedral
C.
Bent
D.
Trigonal pyramidal
Show solution
Solution
NH3 has three bonding pairs and one lone pair, resulting in a trigonal pyramidal geometry.
Correct Answer:
D
— Trigonal pyramidal
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Q. What is the molecular geometry of SF4?
A.
Tetrahedral
B.
Trigonal bipyramidal
C.
Seesaw
D.
Square planar
Show solution
Solution
SF4 has four bonding pairs and one lone pair, resulting in a seesaw molecular geometry.
Correct Answer:
C
— Seesaw
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Q. What is the molecular geometry of SO2?
A.
Linear
B.
Trigonal planar
C.
Bent
D.
Tetrahedral
Show solution
Solution
SO2 has two bonding pairs and one lone pair, resulting in a bent molecular geometry.
Correct Answer:
C
— Bent
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Q. What is the molecular geometry of the molecule with the electronic configuration of 1s2 2s2 2p2?
A.
Linear
B.
Trigonal Planar
C.
Tetrahedral
D.
Octahedral
Show solution
Solution
The electronic configuration corresponds to C2, which has a tetrahedral geometry due to sp3 hybridization.
Correct Answer:
C
— Tetrahedral
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Q. What is the molecular orbital configuration of F2?
A.
(σ1s)²(σ*1s)²(σ2s)²(σ*2s)²(σ2p)²(π2p)⁴(π*2p)²
B.
(σ1s)²(σ*1s)²(σ2s)²(σ*2s)²(σ2p)²(π2p)⁴
C.
(σ1s)²(σ*1s)²(σ2s)²(σ*2s)²(π2p)⁴(π*2p)²
D.
(σ1s)²(σ*1s)²(σ2s)²(σ*2s)²(σ2p)²(π2p)³(π*2p)²
Show solution
Solution
The correct configuration for F2 is (σ1s)²(σ*1s)²(σ2s)²(σ*2s)²(σ2p)²(π2p)⁴(π*2p)².
Correct Answer:
A
— (σ1s)²(σ*1s)²(σ2s)²(σ*2s)²(σ2p)²(π2p)⁴(π*2p)²
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Q. What is the molecular orbital configuration of O2?
A.
(σ1s)²(σ*1s)²(σ2s)²(σ*2s)²(σ2p)²(π2p)²(π*2p)¹
B.
(σ1s)²(σ*1s)²(σ2s)²(σ*2s)²(σ2p)²(π2p)²(π*2p)²
C.
(σ1s)²(σ*1s)²(σ2s)²(σ*2s)²(σ2p)²(π2p)³
D.
(σ1s)²(σ*1s)²(σ2s)²(σ*2s)²(σ2p)²(π2p)²(π*2p)⁴
Show solution
Solution
The correct configuration for O2 is (σ1s)²(σ*1s)²(σ2s)²(σ*2s)²(σ2p)²(π2p)²(π*2p)¹.
Correct Answer:
A
— (σ1s)²(σ*1s)²(σ2s)²(σ*2s)²(σ2p)²(π2p)²(π*2p)¹
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Q. What is the molecular orbital configuration of the F2 molecule?
A.
(σ1s)²(σ*1s)²(σ2s)²(σ*2s)²(σ2p)²(π2p)⁴(π*2p)²
B.
(σ1s)²(σ*1s)²(σ2s)²(σ*2s)²(σ2p)²(π2p)⁴(π*2p)⁴
C.
(σ1s)²(σ*1s)²(σ2s)²(σ*2s)²(σ2p)²(π2p)⁴(π*2p)¹
D.
(σ1s)²(σ*1s)²(σ2s)²(σ*2s)²(σ2p)²(π2p)³(π*2p)²
Show solution
Solution
The correct configuration for F2 is (σ1s)²(σ*1s)²(σ2s)²(σ*2s)²(σ2p)²(π2p)⁴(π*2p)².
Correct Answer:
A
— (σ1s)²(σ*1s)²(σ2s)²(σ*2s)²(σ2p)²(π2p)⁴(π*2p)²
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Q. What is the molecular orbital configuration of the O2 molecule?
A.
(σ1s)²(σ*1s)²(σ2s)²(σ*2s)²(σ2p)²(π2p)²(π*2p)¹
B.
(σ1s)²(σ*1s)²(σ2s)²(σ*2s)²(σ2p)²(π2p)²(π*2p)²
C.
(σ1s)²(σ*1s)²(σ2s)²(σ*2s)²(σ2p)²(π2p)¹(π*2p)¹
D.
(σ1s)²(σ*1s)²(σ2s)²(σ*2s)²(σ2p)²(π2p)¹(π*2p)²
Show solution
Solution
The correct configuration for O2 is (σ1s)²(σ*1s)²(σ2s)²(σ*2s)²(σ2p)²(π2p)²(π*2p)¹.
Correct Answer:
A
— (σ1s)²(σ*1s)²(σ2s)²(σ*2s)²(σ2p)²(π2p)²(π*2p)¹
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Q. What is the molecular shape of a molecule with the formula AX3E?
A.
Trigonal planar
B.
Tetrahedral
C.
Trigonal pyramidal
D.
Bent
Show solution
Solution
AX3E indicates three bonding pairs and one lone pair, resulting in a trigonal pyramidal shape.
Correct Answer:
C
— Trigonal pyramidal
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Q. What is the molecular shape of BF3 according to VSEPR theory?
A.
Bent
B.
Trigonal planar
C.
Tetrahedral
D.
Octahedral
Show solution
Solution
BF3 has three bonding pairs and no lone pairs, resulting in a trigonal planar shape.
Correct Answer:
B
— Trigonal planar
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Q. What is the molecular shape of NH3 according to VSEPR theory?
A.
Linear
B.
Trigonal planar
C.
Tetrahedral
D.
Trigonal pyramidal
Show solution
Solution
NH3 has three bonding pairs and one lone pair, resulting in a trigonal pyramidal shape.
Correct Answer:
D
— Trigonal pyramidal
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Q. What is the primary type of bonding in sodium chloride (NaCl)?
A.
Covalent
B.
Ionic
C.
Metallic
D.
Hydrogen
Show solution
Solution
Sodium chloride is primarily held together by ionic bonds formed between Na+ and Cl- ions.
Correct Answer:
B
— Ionic
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Q. What is the shape of a molecule with the formula AX3E?
A.
Trigonal planar
B.
Tetrahedral
C.
Trigonal pyramidal
D.
Bent
Show solution
Solution
AX3E indicates three bonding pairs and one lone pair, resulting in a trigonal pyramidal shape.
Correct Answer:
C
— Trigonal pyramidal
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Q. What is the shape of the ammonia (NH3) molecule?
A.
Linear
B.
Trigonal planar
C.
Tetrahedral
D.
Trigonal pyramidal
Show solution
Solution
Ammonia has a trigonal pyramidal shape due to the presence of a lone pair on the nitrogen atom.
Correct Answer:
D
— Trigonal pyramidal
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Q. What is the shape of the molecular orbital in the case of a π bond?
A.
Spherical
B.
Dumbbell
C.
Linear
D.
Planar
Show solution
Solution
π bonds are formed by the side-to-side overlap of p orbitals, resulting in a planar shape.
Correct Answer:
D
— Planar
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Q. What is the shape of the molecular orbital in the highest occupied molecular orbital (HOMO) of benzene?
A.
Linear
B.
Trigonal planar
C.
Tetrahedral
D.
Cyclic
Show solution
Solution
The HOMO of benzene is cyclic due to the delocalization of π electrons in the ring structure.
Correct Answer:
D
— Cyclic
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Q. What is the shape of the molecular orbital of the highest energy in O2?
A.
spherical
B.
dumbbell
C.
double dumbbell
D.
linear
Show solution
Solution
The highest energy molecular orbital in O2 is a π* orbital, which has a dumbbell shape.
Correct Answer:
B
— dumbbell
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Showing 61 to 90 of 195 (7 Pages)
Chemical Bonding MCQ & Objective Questions
Chemical bonding is a fundamental concept in chemistry that plays a crucial role in understanding the behavior of substances. Mastering this topic is essential for students preparing for school exams and competitive tests. Practicing MCQs and objective questions on chemical bonding not only enhances your knowledge but also boosts your confidence, helping you score better in exams. Engaging with practice questions allows you to identify important questions and solidify your understanding of key concepts.
What You Will Practise Here
Types of chemical bonds: ionic, covalent, and metallic
Bonding theories: VSEPR theory, hybridization, and molecular orbital theory
Key concepts: electronegativity, bond polarity, and bond length
Important formulas related to bond energy and lattice energy
Diagrams illustrating molecular shapes and bond angles
Definitions of key terms: bond order, resonance, and dipole moment
Real-life applications of chemical bonding in everyday materials
Exam Relevance
The topic of chemical bonding is frequently tested in various examinations, including CBSE, State Boards, NEET, and JEE. Students can expect questions that assess their understanding of bonding types, molecular shapes, and energy concepts. Common question patterns include multiple-choice questions that require students to identify bond types or predict molecular geometry based on given data. Familiarity with these patterns will enhance your exam preparation and performance.
Common Mistakes Students Make
Confusing ionic and covalent bonds due to overlapping characteristics
Misunderstanding hybridization and its implications for molecular geometry
Neglecting to consider electronegativity differences when predicting bond types
Overlooking the significance of resonance structures in molecular stability
Failing to apply the VSEPR theory correctly to determine molecular shapes
FAQs
Question: What are the main types of chemical bonds?Answer: The main types of chemical bonds are ionic bonds, covalent bonds, and metallic bonds.
Question: How does electronegativity affect bond formation?Answer: Electronegativity determines how strongly an atom attracts electrons, influencing whether a bond will be ionic or covalent.
Question: Why is understanding chemical bonding important for exams?Answer: Understanding chemical bonding is crucial as it forms the basis for many topics in chemistry, and is frequently tested in exams.
Now is the time to take your understanding of chemical bonding to the next level! Dive into our practice MCQs and test your knowledge to ensure you are well-prepared for your upcoming exams. Every question you solve brings you one step closer to mastering this essential topic!
