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Shapes of Orbitals Video Lecture - JEE
FAQs on Shapes of Orbitals Video Lecture - JEE
| 1. What are the different shapes of orbitals? |  |
Ans. The different shapes of orbitals are s, p, d, and f orbitals. The s orbital is spherical in shape, the p orbital is dumbbell-shaped, the d orbital is cloverleaf-shaped, and the f orbital is complex and has multiple lobes.
| 2. How many orbitals are present in each subshell? | |
Ans. The s subshell has only one orbital, the p subshell has three orbitals, the d subshell has five orbitals, and the f subshell has seven orbitals. Each orbital can hold a maximum of two electrons.
| 3. What is the significance of the shape of orbitals? | |
Ans. The shape of orbitals determines the spatial distribution of electron density around the nucleus. It helps in understanding the behavior and properties of atoms and molecules. The different shapes of orbitals influence the bonding and molecular geometry of compounds.
| 4. Can orbitals of different shapes overlap? | |
Ans. Yes, orbitals of different shapes can overlap. Overlapping of orbitals is essential for the formation of chemical bonds between atoms. The overlap of orbitals allows the sharing of electrons, leading to the formation of covalent bonds.
| 5. How do the shapes of orbitals affect electron configuration? | |
Ans. The shapes of orbitals determine the arrangement of electrons in an atom. Each orbital can hold a specific number of electrons, and the arrangement of electrons in different orbitals follows a specific pattern determined by the shape of the orbitals. The electron configuration of an atom or ion is determined by the filling of orbitals according to the Aufbau principle, Pauli exclusion principle, and Hund's rule.
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Nov 25, 2024 Last updated |
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