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Solved Practice Questions on Hybridisation and Shapes of Molecules | Inorganic Chemistry PDF Download
Q.1. Which one of the following properties is not shown by NO?
(a) it is diamagnetic in the gaseous state
(b) it is a neutral oxide
(c) it combines with oxygen to form nitrogen dioxide
(d) its bond order is 2.5
Correct Answer is Option (a)
Q.2. The compound which contains both ionic and covalent bond:
(a) KCl
(b) KCN
(c) CH4
(d) H2
Correct Answer is Option (b)
Q.3. Which of the following compounds has the smallest bond angle in its molecule?
(a) H2O
(b) H2S
(c) NH3
(d) SO2
Correct Answer is Option (b)
Q.4. The maximum number of 90° angles between bond pair-bond pair of electrons is observed in
(a) dsp2 hybridisation
(b) sp3d hybridisation
(c) dsp3 hybridisation
(d) sp3d2 hybridisation
Correct Answer is Option (d)
Q.5. Which one of the following pairs of molecules will have permanent dipole moments for both members?
(a) NO2 and CO2
(b) NO2 and O3
(c) SiF4 and CO2
(d) SiF4 and NO2
Correct Answer is Option (b)
Q.6. Ether is more volatile than alcohol having the same molecular formula. This is due to
(a) alcohols having resonance structures
(b) intermolecular hydrogen bonding in ethers
(c) intermolecular hydrogen bonding in alcohols
(d) the dipolar character of ethers
Correct Answer is Option (c)
Q.7. In which solvent NaCl has maximum solubility?
(a) H2O
(b) C2H5OH
(c) CH3COCH3
(d) C2H5OC2H5
Correct Answer is Option (a)
Q.8. The main axis of a diatomic molecule is z, molecular orbital px and py overlap to form which of the following orbital?
(a) pi molecular orbital
(b) sigma molecular orbital
(c) gamma molecular orbital
(d) No bond will be formed
Correct Answer is Option (a)
Q.9. BCl3 is a planar molecule whereas NCl3 is pyramidal because
(a) B-Cl bond is more polar than NaCl bond
(b) N-Cl bond is more covalent than B-Cl bond
(c) the nitrogen atom is smaller than boron atom
(d) BCl3 has no pair but NCl3 has a lone pair of electrons
Correct Answer is Option (d)
Q.10. Total number of lone pair of electrons in I3- ion is
(a) 3
(b) 6
(c) 9
(d) 12
Correct Answer is Option (c)
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FAQs on Solved Practice Questions on Hybridisation and Shapes of Molecules - Inorganic Chemistry
| 1. What is hybridization and why is it important in the study of molecules? |  |
Ans. Hybridization is the process by which atomic orbitals combine to form new hybrid orbitals, which influences the shape and bonding properties of molecules. It is important in the study of molecules as it helps explain the observed molecular geometries and the types of bonds formed between atoms.
| 2. How can we determine the hybridization of an atom in a molecule? | |
Ans. The hybridization of an atom in a molecule can be determined by following a few steps. Firstly, count the number of sigma bonds and lone pairs around the atom. Then, use the following guidelines:
- If the atom has 2 sigma bonds or 0 lone pairs, it is sp hybridized.
- If the atom has 3 sigma bonds or 1 lone pair, it is sp2 hybridized.
- If the atom has 4 sigma bonds or 2 lone pairs, it is sp3 hybridized.
- If the atom has 5 sigma bonds or 3 lone pairs, it is sp3d hybridized.
- If the atom has 6 sigma bonds or 4 lone pairs, it is sp3d2 hybridized.
| 3. What are the different shapes of molecules based on hybridization? | |
Ans. The shapes of molecules are determined by the hybridization of the central atom. Some common shapes based on hybridization are:
- Linear: sp hybridization, such as in carbon dioxide (CO2).
- Trigonal planar: sp2 hybridization, such as in boron trifluoride (BF3).
- Tetrahedral: sp3 hybridization, such as in methane (CH4).
- Trigonal bipyramidal: sp3d hybridization, such as in phosphorus pentachloride (PCl5).
- Octahedral: sp3d2 hybridization, such as in sulfur hexafluoride (SF6).
| 4. How does hybridization affect the bond angles in a molecule? | |
Ans. Hybridization affects the bond angles in a molecule because the hybrid orbitals determine the spatial arrangement of the atoms. The types of hybrid orbitals involved in bonding determine the angles between the bonded atoms. For example, in molecules with sp3 hybridization, the bond angles are approximately 109.5 degrees, resulting in a tetrahedral shape. In molecules with sp2 hybridization, the bond angles are approximately 120 degrees, resulting in a trigonal planar shape.
| 5. Can hybridization explain the shapes of all molecules? | |
Ans. No, hybridization can't explain the shapes of all molecules. While hybridization is a useful concept for understanding the shapes of many molecules, there are cases where other factors such as lone pairs and molecular symmetry play a significant role in determining the shape. In such cases, a more detailed analysis is required, taking into account the specific electron distribution and molecular geometry.
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