Hybridization of Orbitals
Chemistry ⇒ Chemical Bonding and Structure
Hybridization of Orbitals starts at 11 and continues till grade 12.
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Describe the difference between sigma and pi bonds in terms of orbital overlap and hybridization.
Describe the process of hybridization in methane (CH4).
Describe the role of hybridization in determining the shape of molecules.
Explain why the bond angle in water (H2O) is less than the ideal tetrahedral angle.
Explain why the bond angles in ammonia (NH3) are less than the ideal tetrahedral angle.
Explain why the carbon atom in ethene (C2H4) is sp2 hybridized.
Explain why the central atom in PCl5 is sp3d hybridized.
State the hybridization and geometry of the central atom in BF3.
Which of the following is NOT a possible hybridization for carbon?
(1) sp
(2) sp2
(3) sp3
(4) sp3d2
Which of the following is the correct order of bond angles for sp, sp2, and sp3 hybridizations?
(1) sp > sp2 > sp3
(2) sp3 > sp2 > sp
(3) sp2 > sp > sp3
(4) sp3 > sp > sp2
Which of the following molecules exhibits sp3 hybridization at the central atom?
(1) BeCl2
(2) BF3
(3) CH4
(4) CO2
Which of the following molecules has a bent geometry due to hybridization?
(1) CO2
(2) H2O
(3) BF3
(4) CH4
Fill in the blank: In sp hybridization, the bond angle between the hybrid orbitals is ______ degrees.
In the molecule C2H2 (ethyne), the carbon atoms are ______ hybridized.
In the molecule NH4+, the nitrogen atom is ______ hybridized.
In the molecule PF5, the phosphorus atom forms ______ sigma bonds.
State True or False: All sigma bonds are formed by hybridized orbitals.
State True or False: d orbitals are involved in the hybridization of elements in the second period.
True or False: In sp2 hybridization, one s orbital and two p orbitals mix to form three equivalent hybrid orbitals.
True or False: Lone pairs occupy more space than bonding pairs in hybridized orbitals.
