NEET Chemistry Chemical Bonding and Molecular Structure Class 11 Questions

The formation of the oxide ion, O₂−(g), from oxygen atom requires first an exothermic and then an endothermic step as shown below : O(g) + e− → O−(g); ΔH° = −141 kJ mol−1 Ω−(g) + e− → O₂−(g); ΔH° = +780 kJ mol−1 Thus, process of formation of O₂− in gas phase is unfavourable even though O₂− is isoelectronic with neon. It is due to the fact that,

Which of the following statements is not correct from the view point of molecular orbital theory?

What is the geometry of the BCl3 molecule?

What is the average bond enthalpy of the O-H bonds in water based on the provided data?

What is the concept that describes the stability of ionic compounds due to the attraction between positive and negative ions?

What type of overlap forms a sigma (σ) bond?

What is the dipole moment of ammonia (NH3)?

What type of bond is formed between sodium and chlorine in the formation of NaCl?

What is the primary reason for the shape of a molecule according to VSEPR theory?

What is the lattice enthalpy of NaCl in kJ mol⁻¹?

What is the primary factor that determines the shape of a molecule according to VSEPR theory?

What type of bond is formed between the carbon atoms in ethyne?

Which type of molecular orbital is formed by the linear combination of 2p z orbitals from two atoms?

What is the predicted geometry of PCl5 according to VSEPR Theory?

What is the bond length of the C–C bond in ethane (C2H6)?

What is the enthalpy change associated with the process of a gas phase atom in its ground state gaining an electron called?

Which of the following statements about molecular orbitals is correct?

Which of the following statements about molecular orbitals and their properties is correct?

Which of the following statements about covalent bonds and molecular orbitals is correct?

Which of the following statements about the octet rule and hybridization are correct?

Which combination of statements about the bonding in C2H2 and C2H4 is correct?

Which of the following statements about bond angles and molecular stability is correct?

Which of the following combinations correctly describes bond angles and molecular shapes based on lone pair and bond pair interactions?

Which of the following statements about covalent bonding and molecular structure is correct?

Which of the following statements about covalent bonds and molecular structure is correct?

Which combination of statements about molecular geometry and dipole moments is correct?

Assertion (A): Hybrid orbitals are more effective in forming stable bonds than pure atomic orbitals.

Reason (R): Hybrid orbitals are directed in space to minimize repulsion between electron pairs.

Assertion (A): The VSEPR theory can predict the geometry of p-block element compounds accurately.

Reason (R): The theoretical basis of VSEPR theory regarding electron pair repulsions is well-established and undisputed.

Assertion (A): In the formation of a covalent bond, the potential energy of the system decreases.

Reason (R): Attractive forces between atoms are stronger than repulsive forces at the bond formation point.

Assertion (A): The ammonium ion, NH4+, is an exception to the general rule of cations being derived from metallic elements.

Reason (R): Ammonium ion is made up of two non-metallic elements.

Assertion (A): The Lewis dot structures are useful in understanding the formation and properties of a molecule.

Reason (R): Lewis structures always provide accurate representations of the molecular geometry.

Assertion (A): Li2 molecule is stable.

Reason (R): The bond order of Li2 is 0.

Assertion (A): The dipole moment of NH3 is greater than that of NF3.

Reason (R): In NH3, the orbital dipole due to the lone pair is in the same direction as the resultant dipole moment of the N-H bonds.

Assertion (A): In a PCl5 molecule, the axial P-Cl bonds are longer than the equatorial P-Cl bonds.

Reason (R): The axial bonds in a trigonal bipyramidal geometry experience more repulsion than the equatorial bonds.

Assertion (A): NH3 has a higher dipole moment than NF3.

Reason (R): In NH3, the lone pair dipole is aligned with the N-H bond dipoles, while in NF3, it opposes the N-F bond dipoles.

Assertion (A): In ethyne, the C–C bond consists of one sigma bond and two pi bonds.

Reason (R): In sp hybridisation, each carbon atom in ethyne has two unhybridised p orbitals that overlap to form pi bonds.

Assertion (A): Hybrid orbitals are directed in space to minimize repulsion between electron pairs.

Reason (R): Promotion of an electron is an essential condition for hybridization.

Assertion (A): In the molecular orbital theory, the π* antibonding molecular orbital has a node between the nuclei.

Reason (R): The π bonding molecular orbital has larger electron density above and below the inter-nuclear axis.

Assertion (A): In ethane (C2H6), each carbon atom forms three sp3-s sigma bonds with hydrogen atoms.

Reason (R): The C–H bond length in ethane is 154 pm.

Match Column-I with Column-II.

Match Column-I with Column-II.

Match Column-I with Column-II.

Which of the following statements regarding the dipole moment of NH3 and NF3 is correct?

Calculate the average bond enthalpy of the O-H bond in a water molecule given the following bond dissociation enthalpies: H2O(g) → H(g) + OH(g); ΔaH1V = 502 kJ mol–1, OH(g) → H(g) + O(g); ΔaH2V = 427 kJ mol–1.

In the molecule BF3, what is the angle between any two B-F bonds?

In the context of molecular orbital theory, how many molecular orbitals are formed when two p orbitals overlap?

Consider a diagram showing molecular orbitals formed by the combination of two 1s atomic orbitals. Which of the following describes the nature of the resulting molecular orbitals?

Consider a diagram representing the Lewis structure of the ozone (O3) molecule, with atoms labeled as 1, 2, and 3. If the formal charges of these atoms are calculated, which configuration of formal charges is correct?

Which type of molecular orbital is characterized by having electron density located between the nuclei of the bonded atoms?

In molecular orbital theory, which molecular orbital is lower in energy than the σ2p z molecular orbital?