Practice free Chemical Bonding and Atomic Structure (Chemistry) NEET multiple-choice questions online with instant answers and detailed explanations. No login required.
The formation of an $H_2$ molecule, according to Valence Bond Theory, involves the overlap of which types of orbitals?
The context mentions: 'For example the formation of the $H_2$ molecule from two hydrogen atoms involves the overlap of the 1s orbitals of the two H atoms which are singly occupied.'
What is the primary consequence of orbital overlap in bond formation, as described by Valence Bond Theory?
The text states: 'Because of orbital overlap the electron density between the nuclei increases which helps in bringing them closer.'
Who introduced the concept of hybridization of atomic orbitals to explain the characteristic shapes of polyatomic molecules?
The context states: 'For explaining the characteristic shapes of polyatomic molecules Pauling introduced the concept of hybridisation of atomic orbitals.'
Valence Bond Theory was initially introduced by which scientists?
The text explicitly mentions: 'Valence bond theory was introduced by Heitler and London (1927) and developed further by Pauling and others.'
Which of the following concepts is NOT explicitly mentioned as a basis for the discussion of Valence Bond Theory in the provided text?
The passage lists: 'A discussion of the valence bond theory is based on the knowledge of atomic orbitals, electronic configurations of elements (Units 2), the overlap criteria of atomic orbitals, the hybridization of atomic orbitals and the principles of variation and superposition.' Lattice energy is related to ionic compounds, not explicitly the basis for VB theory presented here.
At the equilibrium inter-nuclear distance in the $H_2$ molecule, what happens to the potential energy of the system?
The text details the formation of $H_2$: 'At the equilibrium inter-nuclear distance (bond distance) the energy touches a minimum. Any attempt to bring the nuclei still closer results in a sudden increase in energy and consequent destabilization of the molecule.'
Valence Bond Theory is used to explain the formation and geometrical shapes of molecules like:
The text states: 'sp, $sp^2$, $sp^3$ hybridizations of atomic orbitals of Be, B, C, N and O are used to explain the formation and geometrical shapes of molecules like $BeCl_2$, $BCl_3$, $CH_4$, $NH_3$ and $H_2O$.'
What is a limitation of the Lewis approach that Valence Bond Theory addresses?
The text mentions: 'As we know that Lewis approach helps in writing the structure of molecules but it fails to explain the formation of chemical bond. It also does not give any reason for the difference in bond dissociation enthalpies and bond lengths...'
Which of the following is crucial for describing bonding in terms of Valence Bond Theory, but not directly explained by VSEPR theory?
The text states: 'Similarly the VSEPR theory gives the geometry of simple molecules but theoretically, it does not explain them and also it has limited applications. To overcome these limitations the two important theories based on quantum mechanical principles are introduced. These are valence bond (VB) theory and molecular orbital (MO) theory.' VB theory discusses bond formation 'in terms of overlap of orbitals.'
Match List-I with List-II:
| List-I | List-II |
|---|---|
| A. Coke | I. Carbon atoms are sp³ hybridised. |
| B. Diamond | II. Used as a dry lubricant. |
| C. Fullerene | III. Used as a reducing agent. |
| D. Graphite | IV. Cage-like molecules. |
Choose the correct answer from the options below:
Coke: reducing agent. Diamond: sp³. Fullerene: cage. Graphite: dry lubricant.
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